b.sc chemistry model i

MAHATMA GANDHI UNIVERSITY

PRIYADARSHINI HILLS, KOTTAYAM-686560

CHOICE BASED CREDIT

SYSTEM

SCHEME, SYLLABI AND

MODEL QUESTION PAPERS

FOR

UNDERGRADUATE PROGRAMMES IN

CHEMISTRY

2016

2

CONTENTS

Page No

Acknowledgement 3

List of BOS Members 4

Introduction 5

Programme Structure

Bsc Chemistry Programme – (Model - I) 22

B.Sc. Chemistry (Vocational) – Model -II 25

Bsc Chemistry– Model -IIIPetrochemicals 28

Syllabus

Core (Chemistry) Courses 32

Complementary Courses In Chemistry 84

Bsc Chemistry (Vocational) – Model -II 103

Model III. Bsc Petrochemicals 114

Model Question Papers

Chemistry Core 124

Complementary Physical Sciences 161

Complementary Life Sciences 169

Model II 177

Model III 188

3

2. Acknowledgement.

The Board of Studies in Chemistry (U G) puts on record our sincere thanks to the

honourble Vice Chancellor of Mahatma Gandhi University, Dr. Babu Sebastian, for the

guidance and help extended to us during the restructuring of B. Sc. Chemistry syllabus.

We thank the Pro Vice Chancellor of the University Dr. Sheena Shukoor, for the for her

valuable suggestions.

The Board of Studies thank the members of M. G. University syndicate for all the help

extended to us.

We thank the Registrar of the University, Academic Section and the Finance Section for

extending their service for the smooth completion of syllabus restructuring.

Special thanks are due to the representatives of the colleges affiliated to M. G.

University, who have actively participated and contributed in the two-day workshop. The

enthusiasm and sincerity shown by the teachers from various colleges in the context of

syllabus restructuring is highly appreciated.

For the Board of Studies in Chemistry,

Kottayam Dr V T Thomas

07-05-2016 Chairman

4

3 List of BOS Members.

1. Dr V T Thomas (Chairman) Ho D and Associate Professor(Retired), St

Thomas College, Pala.

2. Dr Shaji Joseph, HoD and Associate Professor, S B College, Changanassery.

3. Dr Thomas Mathew, Associate Professor, Mar Thoma College, Thiruvalla.

4. Dr Sunil Jacob, Associate Professor, Catholicate College, Pathanamthitta.

5. Dr Paulson Mathew, Associate Professor, St Thomas College, Trichur.

6. Prof Bejoy Mathew, Associate Professor, St Thomas College, Pala.

7.Dr Sheelakumari Isacc, Associate Professor, UC College, Aluva.

8 Prof P K Rajappan Nair, Associate Professor, NSS College, Changanassery.

9. Dr James C Joseph, Associate Professor (Retired), K E College, Mannanam.

10. Dr M K Muraleedharan Nair, Associate Professor, Maharaja’ s College,

Ernakualam.

5

4 Introduction.

Mahatma Gandhi University introduced choice based credit and semester and Grading

System in colleges affiliated to the University from the Academic year 2009-2010, under

Direct Grading System. Subsequently, the Kerala State Higher Education Council

constituted a committee of experts headed by Prof. B. Hridayakumari, to study and make

recommendations for the improvement of the working of the Choice Based Credit and

Semester System in Colleges affiliated to the Universities in the State. The State Government

accepted the recommendations of the Committee and the Syndicate and the Academic

Council of the Mahatma Gandhi University have resolved to reform the existing CBCSS

regulations. Accordingly, REGULATIONS FOR UNDER GRADUATE PROGRAMMES

UNDER CHOICE BASED COURSE-CREDIT-SEMESTER SYSTEM AND GRADING,

2013 was introduced in the University from the Academic year 2013-14 onwards, under

Indirect Grading System. The University Grants Commission, in order to facilitate student

mobility across institutions within and across countries and also to enable potential

employers to assess the performance of students, insisted to introduce uniform grading

system in the Universities. The Academic Council of the Mahatma Gandhi University at its

meeting held on 23rd May 2015 resolved to introduce the UGC Guidelines for Choice Based

Credit Semester System from the Academic year 2016-17 onwards and the syndicate of the

University at its meeting held on 1st August 2015 approved the resolution of the Academic

Council. Hence it becomes necessary to modify the existing CBCSS regulation as follows.

5.TITLE

B. Sc. CHEMISTRY PROGRAMME - Graduate Programmes under Choice Based

Credit System, 2016” (UGCBCS 2016).

6. SCOPE

6.1 Applicable to all regular Under Graduate Programmes conducted by the University with

effect from 2016 admissions, except for Professional and B.Voc programmes. Also

applicable to Distance/Private Undergraduate Programmes with suitable modifications.

Under Graduate Programmes in Management Studies are included as non-professional

programmes. Provided that the existing CBCSS Regulations 2013 shall be applicable to

students who were admitted prior to the commencement of these Regulations and who are

continuing their studies.

6

6.2 Examinations of the courses being run under the Distance/Private registration scheme

shall be conducted annually.

6.3 The provisions herein supersede all the existing regulations for the

Regular/Distance/Private Undergraduate programmes to the extent herein prescribed.

7. AIMS AND OBJECTIVES OF THE PROGRAMME

7.1 Aims:

The Board of Studies in Chemistry (UG) recognizes that curriculum, course content

and assessment of scholastic achievement play complementary roles in shaping education.

The committee is of the view that assessment should support and encourage the broad

instructional goals such as basic knowledge of the discipline of Chemistry including theories

and techniques, concepts and general principles. This should also support the ability to ask

physical questions and to obtain solutions to physical questions by use of qualitative and

quantitative reasoning and by experimental investigation. The important student attributes

including keen observation, curiosity, creativity and reasoned skepticism and understanding

links of Chemistry to other disciplines and to societal issues should be given encouragement.

With this in mind, we aim to provide a firm foundation in every aspect of Chemistry and to

explain a broad spectrum of modern trends in chemistry and to develop experimental,

computational and mathematics skills of students.

1. The programme also aims to develop the following abilities:

2. Read, understand and interpret chemical information – verbal, mathematical and

graphical.

3. Impart skills required to gather information from resources and use them.

4. To give need based education in chemistry of the highest quality at the undergraduate

level.

5. Offer courses to the choice of the students.

6. Perform experiments and interpret the results of observation.

7. Provide an intellectually stimulating environment to develop skills and enthusiasms of

students to the best of their potential.

8. Use Information Communication Technology to gather knowledge at will.

9. Attract outstanding students from all backgrounds.

7

7.2 Objectives:

The syllabi are framed in such a way that it bridges the gap between the plus two and

post graduate levels of Chemistry by providing a more complete and logical framework in

almost all areas of basic Chemistry.

8. Course Design:

The U.G.programme in Chemistry must include (a) Common courses, (b) Core

courses, (c) Complementary Courses, (d) Choice based courses(e) Generic elective and (f)

Project. No course shall carry more than 4 credits. The student shall select any one Generic

Elective course in Sem V offered by the Departments which offers the core courses or

physical education department, depending on the availability of infrastructure facilities, in the

institution. The number of Courses for the restructured programme should contain 12

compulsory core courses ,1 generic elective ,1 choice based course from the frontier area of

the core courses, 6 core practicals,1 project in the area of core, 8 complementary courses, 2

complementary practicals otherwise specified, from the relevant subjects for complementing

the core of study. There should be 10 common courses, or otherwise specified, which

includes the first and second language of study.

8

9.B. Sc. Programme in Chemistry

9.1. PROGRAMME STRUCTURE

Model I BSc

a Programme Duration 6 Semesters

b Total Credits required for successful completion of the

Programme 120

c Credits required from Common Course I 22

d Credits required from Common Course II 16

e Credits required from Core course and Complementary

courses including Project 79

f Generic Elective (GE) 3

g Minimum attendance required 75%

Model II BSc

A Programme Duration 6 Semesters

B Total Credits required for successful completion of the

Programme 120

C Credits required from Common Course I 16

D Credits required from Common Course II 8

E Credits required from Core + Complementary +

Vocational Courses including Project 93

F Generic Elective (GE) 3

G Minimum attendance required 75%

9

Model III BSc

a Programme Duration 6 Semesters

b Total Credits required for successful completion of the

Programme 120

c Credits required from Common Course I 8

d Credits required from Core + Complementary + Vocational

Courses including Project 109

e Generic Elective (GE) 3

f Minimum attendance required 75%

9.2. Courses:

There shall be three different types (models) of courses in Chemistry programme. The

programme (Model I) consists of common courses with 38 credits, core, Choice based

course, Generic elective & complementary courses with 82 credits. The programme

(Vocational -Model II) consists of common courses with 24 credits, core, Choice based

courses, Generic elective & complementary courses with 96 credits. The programme (Model

III) consists of common courses with 8 credits, core, Choice based course, Generic elective &

complementary courses with 112 credits.

10

9.3 Scheme of Courses:

The different types of courses and its number are as the following:

Model- I Model- II Model- III

Courses No. Courses No. Courses No

.

Common Courses 10 Common Courses 6 Common Courses 2

Core Courses 12 Core Courses 12 First Core Courses 12

Project 1 Project 1 Project 1

Core practical 6 Core Practical 6 First Core practical 6

Generic Elective 1 Generic Elective 1 Generic Elective 1

Choice based Course 1 Choice based Course 1 Choice based Course 1

Vocational courses 6 Second core Courses 6

Vocational practical 3 Second Core practical 2

OJT 1 OJT 1

Complementary Courses 8 Complementary Courses 4 Complementary Courses 8

Complementary practical 2 Complementary practical 2

Total 41 Total 41 Total 42

9.4. Course Code:

Every course in the programme should be coded with an eight digit alphaneumeric code

according to the following criteria. The first two letters of the code indicates the name of

programme ie. CH for Chemistry. One digit to indicate the semester. ie., CH1 (Chemistry, 1st

semester). Two letters form the type of courses such as, CC for common courses, CR for core

course, VO for vocational course, CM for Complementary courses, GE for Generic elective,

CB for Choice based core, OJ for On the Job Training, OC for Optional Core, PR for project

ie.., CH1CR (Chemistry,1st semester Core course). The letter T may be used to denote theory

paper and the letter P may be used to denote practical papers. Two digits to indicate the

paper’s relative position in the programme, ie., CH5CRT06 (Chemistry, 5th semester, Core

course, Theory, sixth paper).

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9.5. Courses with Credits:

Courses with Credits of different courses and scheme of examinations of the programme is

the following

Courses Model I Model II Model III

Credits Total Credits Total Credits Total

Core Courses 46 46 46

Generic Elective 3 3 3

Choice Based Core 3 3 3

Project 2 2 2

Vocational Courses Nil 24 Nil

OJT - 2 2

2nd Core Courses Nil Nil 24

Total 54 80 80

Complementary Courses I 14 16 16

Complementary Courses II 14 Nil 16

Total 28 16 32

Common Courses 38 24 8

Total 38 24 8

Grand Total 120 120 120

9.6. Scheme of Distribution of Instructional hours for Core courses:

Semester Model I Model II Model III

Theory Practical Theory Practical Theory Practical

First semester 2 2 6 4 6 4

Second semester 2 2 6 4 6 4

Third semester 3 2 9 6 10 4

Fourth semester 3 2 9 6 10 4

Fifth semester 15 10 15 10 15 10

Sixth Semester 15 10 15 10 15 10

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10.DEFINITIONS

10.1 ‘Academic Week’ is a unit of five working days in which the distribution of work is

organized from day one to day five, with five contact hours of one hour duration

on each day.

10.2 ‘Choice Based Course’ means a course that enables the students to familiarize the

advanced areas of core course.

10.3 ‘Common Course I’ means a course that comes under the category of courses for

English and Environmental Studies & Human Rights and ‘Common Course II’

means additional language.

10.4 ‘Complementary Course’ means a course which would enrich the study of core

courses.

10.5 ‘Core course’ means a course in the subject of specialization within a degree

programme.

10.6 ‘Course’ comprises ‘Paper(s)’ which will be taught and evaluated within a

programme.

10.7 ‘Credit’ is the numerical value assigned to a paper according to the relative

importance of the syllabus of the programme.

10.8 ‘Generic Elective (GE)’ means an elective paper chosen from any discipline/

subject, in an advanced area.

10.9 ‘Grade’ means a letter symbol (A, B, C, etc.), which indicates the broad level of

performance of a student in a Paper/Course/ Semester/Programme.

10.10 ‘Grade Point’ (GP) is the numerical indicator of the percentage of marks

awarded to a student in a paper.

10.11 ‘Paper’ means a complete unit of learning which will be taught and evaluated

within a semester.

10.12 ‘Parent Department’ means the department which offers core course/courses

within an undergraduate programme.

10.13 ‘Programme’ means a three year programme of study and examinations

spread over six semesters, the successful completion of which would lead to the

award of a degree.

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10.14 ‘Semester’ means a term consisting of 90 working days, inclusive of tutorials,

examination days and other academic activities within a period of six months.

10.15 ‘Vocational Course’ (Skill Enhancement Course) means a course that

enables the students to enhance their practical skills and ability to pursue a vocation

in their subject of specialization.

11. ELIGIBILITY FOR ADMISSION AND RESERVATION OF SEATS

11.1 Eligibility for admission, norms for admission and reservation of seats for various

Undergraduate Programmes shall be according to the regulations framed/orders issued

by the University in this regard, from time to time.

11.2 Students can opt for any one of the Generic Elective Papers offered by different

departments of the college in fifth semester (subject to the availability of vacancy in

the concerned discipline). If the number of applications exceeds the number of

vacancies for a particular Generic elective paper, priority will be given to the students

from the parent department (core subject). Selection of students in the generic elective

paper will be done in the college based on merit and interest of the students.

12. DURATION OF COURSE

12.1 The duration of U.G. Programmes shall be 6 semesters.

12.2 A student may be permitted to complete the programme, on valid reasons, within a

period of 12 continuous semesters from the date of commencement of the first semester

of the programme.

13. Attendance: Students having a minimum of 75% average attendance for all the courses

only can register for the examination.

Attendance Evaluation

For all papers

% of attendance Marks

90 and above 5

85 – 89 4

80-84 3

76-79 2

75 1

(Decimals are to be rounded to the next higher whole number)

14

14. Medium Instruction

Medium of instructions can be either English or Malayalam.

15. EXAMINATIONS.

15.1 The evaluation of each paper shall contain two parts:

(i) Internal or In-Semester Assessment (ISA)

(ii) External or End-Semester Assessment (ESA)

The internal to external assessment ratio shall be 1:4. There shall be a maximum of 80 marks

for external evaluation and maximum of 20 marks for internal evaluation. Both internal

and external marks are to be mathematically rounded to the nearest integer.

For all papers (theory & practical), grades are given on a 10-point scale based on the

total percentage of marks, (ISA+ESA) as given below: -

Percentage of Marks Grade Grade Point

95 and above S Outstanding 10

85 to below 95 A+ Excellent 9

75 to below 85 A Very Good 8

65 to below 75 B+ Good 7

55 to below 65 B Above Average 6

45 to below 55 C Satisfactory 5

40 to below 45 D Pass 4

Below 40 F failure 0

Ab Absent 0

15.2CREDIT POINT AND CREDIT POINT AVERAGE

Credit Point (CP) of a paper is calculated using the formula

CP=C x GP, where C is the Credit; GP is the Grade Point

Semester Grade Point Average (SGPA) of a Semester is calculated using the formula.

SGPA =TCP/TC, where

TCP is the Total Credit Point of that semester i.e.,

TC is the Total Credit of that semester i.e., Where n is the number of papers in

that semester

Cumulative Grade Point Average (CGPA) of a programme is calculated using the formula.

15

CGPA = TCP/TC, where

TCP is the Total Credit Point of that programme ie,

TC is the Total Credit of that programme ie,

Where n is the number of papers in that programme

Grade Point Average (GPA) of a Course (Common Course 1, Common Course 11,

Complementary Course 1, Complementary Course 11, Vocational Course, Core Course) is

calculated using the formula.

GPA = TCP/TC, Where

TCP is the Total Credit Point of course ie,

TC is the Total Credit of that course, ie, where n is the number of papers in that

course

Grades for the different courses, semesters and overall programme are given based on

the corresponding CPA as shown below:

GPA Grade

9.5 and above S Outstanding

8.5 to below 9.5 A+ Excellent

7.5 to below 8.5 A Very Good

6.5 to below 7.5 B+ Good

5.5 to below 6.5 B Above Average

4.5 to below 5.5 C Satisfactory

4.0 to below 4.5 D Pass

Below 4.0 F Failure

Note: A separate minimum of 30% marks each for internal and external (for both theory and

practical) and aggregate minimum of 40% are required for a pass for each paper. For a pass

in a candidate secures F Grade for any one of the papers offered in a semester/programme

only F grade will be awarded for that Semester/Programme until he/she improves this to D

grade or above within the permitted period.

15.3 MARKS DISTRIBUTION FOR EXTERNAL EXAMINATION AND

INTERNAL EVALUATION

16

The external theory examination of all semesters shall be conducted by the University

at the end of each semester. Internal evaluation is to be done by continuous assessment. For

all papers (theory and practical) total marks of external examination is 80 and total marks of

internal evaluation is 20.

Marks distribution for external and internal assessments and the components for

internal evaluation with their marks are shown below:

Components of the internal evaluation and their marks are as below.

15. 4. For all theory papers

a) Marks of external Examination : 80

b) Marks of internal evaluation : 20

All the three components of the internal assessment are mandatory.

Components of theory Internal

Evaluation

MARKS

Attendance 5

Assignment/Seminar/Viva 5

Test Paper(s) (1 or2)

(1x10=10; 2x5=10)

10

Total 20

15.5 For all practical papers (conducted only at the end of even semesters)



17


Components of Practical-internal

evaluation

Marks

Attendance 5

Record* 10

Lab involvement 5

Total 20

*Marks awarded for Record should be related to number of experiments recorded.

15.6 For projects



Components of Project – Evaluation

External

Marks

Dissertation (External) 50

Viva-Voce(External) 30

Total 80

All the four components of the internal assessment are mandatory.

Components of Project Internal

Evaluation

Marks

Punctuality 5

Experimentation/Data Collection 5

Knowledge 5

Report 5

Total 20

15.6 OJT Evaluation

For On the J ob Training there is only internal evaluation.

18

15.7 . ASSIGNMENTS

Assignments are to be done from 1st to 4th Semesters. At least one assignment should

be done in each semester for all papers.

15.8 SEMINAR/ VIVA

A student shall present a seminar in the Vth semester and appear for Viva- voice in

the 6th semester for all papers.

15.9 . INTERNAL ASSESSMENT TEST PAPERS

At least one internal test- paper is to be attended in each semester for each paper. The

evaluations of all components are to be published and are to be acknowledged by the

candidates. All documents of internal assessments are to be kept in the college for two years

and shall be made available for verification by the University. The responsibility of

evaluating the internal assessment is vested on the teacher(s) who teach the paper.

15.10 MARKS DISTRIBUTION FOR EXTERNAL EXAMINATION AND

INTERNAL EVALUATION

The external theory examination of all semesters shall be conducted by the University at

the end of each semester. Internal evaluation is to be done by continuous assessment.

For all papers (theory and practical) total marks of external examination is 80 and total

marks of internal evaluation is 20.

Marks distribution for external and internal assessments and the components for

internal evaluation with their marks are shown below:

15.10.1 For all theory papers




19

Components of Internal

Evaluation of theory Marks

Attendance 5

Assignment /Seminar/Viva 5

Test paper(s) (1 or 2)

(1x10=10; 2x5=10) 10

Total 20

15.10.2 For all practical papers




Components Internal

evaluation of Practical

Marks

Attendance 5

Test paper 5

Record* 5

Lab involvement 5

Total 20

*Marks awarded for Record should be related to number of experiments recorded and

duly signed by the concerned teacher in charge.

15.10.3 For projects

15.10.3.1 All students are to do a project in the area of core course. This project can be

done individually or in groups (not more than five students) for all subjects which

may be carried out in or outside the campus. The projects are to be identified during

the II semester of the programme with the help of the supervising teacher. The report

of the project in duplicate is to be submitted to the department at the sixth semester

and are to be produced before the examiners appointed by the University. External

Project evaluation and Viva / Presentation is compulsory for all subjects and will be

conducted at the end of the programme.

20



Components of External Evaluation of

Project

Marks

Dissertation (External) 50

Viva-Voce (External) 30

Total 80


Components Internal

Evaluation of project Marks

Punctuality 5

Experimentation/Data collection 5

Knowledge 5

Report 5

Total 20

15.10.4 . External examination

The external theory examination of all semesters shall be conducted by the University of the

end of each semester.

15.10.4.1 Students having a minimum of 75% average attendance for all the course only

can register for the examination,

15.10.4.2 There will be no supplementary exams. For reappearance/ improvement, the

students can appear along with the next batch.

15.10.4.3 A candidate who has not secured minimum marks/credits in internal examinations

can re-do the same registering along with the University examination for the same

semester, subsequently.

16. Conduct of Practical examinations

16.1 Practical examinations will be conducted only at the end of even semesters for all

programmes.

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16.2 Pattern of questions for external examination of practical papers will decided by the

concerned Board of practical examination.

17 PATTERN OF QUESTIONS (Theory papers)

Questions shall be set to assess, knowledge acquired, standard application of

knowledge, application of knowledge in new situations, critical evaluation of knowledge and

the ability to synthesize knowledge. The question setter shall ensure that questions covering

all skills are set. He/ She shall also submit a detailed scheme of evaluation along with the

question paper.

A question paper shall be a judicious mix of very short type, short answer type, short essay

type/ problem solving type and long essay type questions

Total no. of

questions

No of questions

to be answered

Marks for

each Question

Total

mark

s

Short Answer 12 9 2 18

Answer 9 6 4 24

Problem/Short Essay 5 3 6 18

Essay 4 2 10 20

Total 30 20 80

22

18. Consolidated Scheme for I to VI semesters

PROGRAMME STRUCTURE

1. BSc Chemistry Programme – (Model - I)

Sem

este

r

Title of the Course

No. of

hou

rs

per

wee

k

No. of

Cre

dit

s

Tota

l

hrs

/sem

este

r Un

iver

sity

Exam

du

rati

on

Marks

IA EA

1

English I 5 4 90 3 20 80

English/ Common Course I 4 3 72 3 20 80

Second Language I 4 4 72 3 20 80

CHICRT01 – General Inorganic Chemistry 2 2 36 3 20 80

CH2CRP01 Qualitative Inorganic Analysis 2 36 No Exam

Complementary Mathematics

4

3

72 3 20 80

Complementary Physics 2 2 36 3 20 80

Complementary Physics Practical 2 36 No Exam 20 80

2

English II 5 4 90 3 20 80

English/ Common Course II 4 3 72 3 20 80

Second Language II 4 4 72 3 20 80

CH2CRT02 – Chemical Bonding and Nuclear

Chemistry 2 2 36 3 20 80

CH2CRP01 Qualitative Inorganic Analysis 2 2 36 3 20 80


4

3

72 3 20 80


Complementary Physics Practical 2 2 36 3 20 80

23

3

English III 5 4 90 3 20 80

II Lang/Common Course I 5 4 90 3 20 80

CH3CRT03 –Basic Organic Chemistry-I

3

3

54

3

20

80

CH4CRP02 Qualitative Organic Analysis

2 36 No exam


5

4

90

3

20

80

Complementary Physics

3

3

54

3

20

80

Complementary Physical Practical 2 36 No exam

4

English IV 5 4 90 3 20 80

II Lang/ Common Course II 5 4 90 3 20 80

CH4CRT04 Basic Organic Chemistry-II

3

3

54

3

20

80


2 2 36 3 20 80


5

4

90

3

20

80


Complementary Physical Practical 2

2

36

3

20

80

5

CH5CRT05 – Analytical and Environmental

Chemistry 3 3 54 3 20 80

CH5CRT06 – Advanced Organic Chemistry-I 3 3 54 3 20 80

CH5CRT07 – States of Matter, Colloids and

General Informatics 3 3 54 3 20 80

CH5CRT08 – Quantum Mechanics,

Spectroscopy and Photochemistry 3 3 54 3 20 80

CH5GET Generic Elective 3 3 54 3 20 80

CH6CRP03 Volumetric Analysis 3 54 No exam 20 80

CH6CRP04

Organic Preparations and Chromatography 2 36 No exam 20 80

24

CH6CRP05

Physical Chemistry Practical 3 54 No exam 20 80

CH6PRP01Project 2 36 No

evaluation

6

CH6CRT09 Coordination Chemistry and

Organometallics 3 3 54 3 20 80

CH6CRT10 Advanced Organic Chemistry-II 3 3 54 3 20 80

CH6CRT11 Thermodynamics and Chemical

Kinetics 3 3 54 3 20 80

CH6CRT12 Solution Chemistry 3 3 54 3 20 80

CH6CBT Choice Based Course 3 3 54 3 20 80

CH6CRP03Volumetric Analysis 3 2 54 3 20 80

CH6CRP04

Organic Preparations and Chromatography 2 2 36 3 20 80

CH6CRP05

Physical Chemistry Practical 3 2 54 3 20 80

CH6CRP06

Gravimetric Analysis 2 2 36 3 20 80

CH6PRP01 Project 2 20 80

Generic Elective

Sl.

No.

Semester Course Title

1 V CH5GET01Novel

Inorganic Solids

2 V

CH5GET02

Industrial

Chemistry

3 V CH5GET03Green

Chemistry

Choice Based Course

Sl.

No.


1 VI CH6CBT01Polymer

Chemistry

2 VI

CH6CBT02Instrumental

Methods of Chemical

Analysis

3 VI

CH6CBT03Computer

Applications in

Chemistry

25

2. B.Sc. Chemistry (Vocational) – Model -II

Sem

este

r Title of the Course

No. of

hou

rs p

er

wee

k

No. of

Cred

its

Tota

l h

rs/s

emes

ter

Un

iver

sity

Exam

du

rati

on

Marks

IA EA

1

English I 5 4 90 3 20 80

Second Language I 5 4 90 3 20 80


CH2CRP01- Qualitative Inorganic Analysis 2 36 No exam

Complementary Mathematics 5

4

90 3 20 80

CH1VOT01 Industrial Aspects of Inorganic and

Organic Chemistry 4 3 72 3 20 80

CH2VOP01 Vocational Practical

Organ

2 36 No exam 20 80

2

English II 5 4 90 3 20 80

Second language II 5 4 90 3 20 80

CH2CRT02 –– Chemical Bonding and Nuclear Chemistry

Chemistry

2 2 36 3 20 80

CH2CRP01- Qualitative Inorganic Analysis 2 2 36 3 20 80

Complementary Mathematics 5 4 90 3 20 80

CH2VOT02 Industrial Applications of Physical

Chemistry

App

4 3 72 3 20 80

CH2VOP01 Vocational Practical 2 2 36 3 20 80

3

English III 5 4 90 3 20 80

CH3CRT03 – Basic Organic Chemistry-I

3 3

54 3 20 80


2 36 No exam


5

4

90 3 20 80

CH3VOT03 Unit Operations in Chemical Industry 3 3 54 3 20 80

CH3VOT04 Unit Processes in Organic Chemicals

Manufacture 3 3 54 3 20 80

CH2VOP02 Vocational Practical 2 36 No exam

CH2VOP03 Vocational Practical 2 36 No exam

4

English IV 5 4 90 3 20 80


3 3 54 3 20 80


2 2 36 3 20 80

26

On the Job Training All the students have to undergo on the job training in a chemical

industry for a minimum period of 15 days and submit a project report. The period of 15 days

need be at a single stretch. The vacation days may be utilized for this purpose. A report of the


CH4VOT05 Instrumental Methods of Chemical

Analysis-I

3

3

54 3 20 80

CH4VOT06 Instrumental Methods of Chemical

Analysis-II 3 3 54 3 20 80



5

CH5CRT05 – Analytical and Environmental Chemistry 3 3 54 3 20 80

CH5CRT06– Advanced Organic Chemistry-I 3 3 54 3 20 88

CH5CRT07 – States of Matter, Colloids and General

Informatics 3 3 54 3 20 80

CH5CRT08– Quantum Mechanics, Spectroscopy and

Photochemistry

Photochemistry

3 3 54 3 20 80


CH6CRP03 Volumetric Analysis 3 54 No exam

CH6CRP04 Organic Preparations and Chromatography

2 36 No exam

CH6CRP05 Physical Chemistry Practical

3 54 No exam

CH6PRP01Project 2 36 No evaluation

6

CH6CRT09 Coordination Chemistry and Organometallics

Organometallics

3 3 54 3 20 80


CH6CRT11 –Thermodynamics and Chemical Kinetics 3 3 54 3 20 80



CH6CRP03 Volumetric Analysis 3 2 54 3 20 80


2 2 36 3 20 80

CH6CRP05 Physical Chemistry Practical

3 2 54 3 20 80

CH6CRP06 Gravimetric Analysis 2 2 36 3 20 80

CH6PRP01Project 2 Evaluation 20 80

CH6OJP01 OJT 2 Evaluation 100

27

training should be submitted to the department during the sixth semester for internal

evaluation.

Generic Elective

Choice Based Course

Sl.

No.


1 V CH5GET01Novel

Inorganic Solids

2 V

CH5GET02

Industrial

Chemistry

3 V CH5GET03 Green

Chemistry

Sl.

No.

Semester Paper Title

1 VI CH6CBT01 Polymer Chemistry

2 VI CH6CBT02 Instrumental Methods of Chemical Analysis

3 VI CH6CBT03 Computer Applications in Chemistry

28

3. BSc Chemistry– Model -III Petrochemicals

(2 Core Courses, Common Course with 8 Credits)

Sem

este

r

Title of the Course

No. of

hou

rs

per

wee

k

No. of

Cred

its

Tota

l

hrs

/sem

este

r

Un

iver

sity

Exam

du

rati

on

Marks

IA EA

1

English - I 5 4 90 3 20 80


CH2CRP01- Qualitative Inorganic Analysis 2 36 No exam

CH1OCT01 Petroleum Geology 4 3 72 3 20 80

CH2OCP01 Practical I 2 36 No exam


Complementary Computer Science 3 3 54 3 20 80

Complementary Practical –I 2 36 No exam

2

English II 5 4 90 3 20 80

CH2CRT02 –– Chemical Bonding and

Nuclear Chemistry 2 2 36 3 20 80

CH2CRP01- Qualitative Inorganic Analysis 2 2 36 3 20 80

CH2OCT02 Test Methods and Petrolem

Processes 4 3 72 3 20 80

CH2OCP01 Practical I 2 2 36 3 20 80



Complementary Practical –I 2 2 36 3 20 80

3

CH3CRT03 – Basic Organic Chemistry-I

3 3 54 3 20 80

CH4CRP02 Qualitative Organic Analysis 2 36 No exam

CH3OCT03 Production and Application of

Compounds from Petroleum 4 4 72 3 20 80

CH3OCT04 Manufacture of Petrochemicals-I 3 3 54 3 20 80

CH4OCP02 Practical –II 2 36 No exam

29



Complementary Practical –II 2 36 No exam

4


3 3 54 3 20 80

CH4CRP02 Qualitative Organic Analysis 2 2 36 3 20 80

CH4OCT05 Manufacture of Petrochemicals-II 4 4 72 3 20 80

CH4OCT06 Petroleum Industries in India 3 3 54 3 20 80

CH4OCP02 Practical –II 2 2 36 3 20 80



Complementary Practical –II 2 2 36 3 20 80

5

CH5CRT05 – Analytical and Environmental

Chemistry 3 3 54 3 20 80

CH5CRT06 – Advanced Organic Chemistry-I 3 3 54 3 20 80

CH5CRT07 – States of Matter, Colloids and

General Informatics 3 3 54 3 20 80

CH5CRT08– Quantum Mechanics, Spectroscopy

and Photochemistry

3 3 54 3 20 80


CH6CRP03 Volumetric Analysis 3 36 No exam

CH6CRP04 Organic Preparations and

Chromatography 2 36 No exam

CH6CRP05 Physical Chemistry Practical 3 54 No exam

CH6PRP01Project 2 36 No evaluation

6

CH6CRT09 Coordination Chemistry and

Organometallics 3 3 54 3 20 80


CH6CRT11 –Thermodynamics and 3 3 54 3 20 80

30

Chemical Kinetics



CH6CRP03 Volumetric Analysis 3 2 54 3 20 80

CH6CRP04 Organic Preparations and

Chromatography 2 2 36 3 20 80

CH6CRP05 Physical Chemistry Practical 3 2 54 3 20 80

CH6CRP06 Gravimetric Analysis 2 2 36 3 20 80

CH6PRP01Project 2 Evaluation 20 80

CH6OJP01 OJT 2 Evaluation 100

On the Job Training All the students have to undergo on the job training in a chemical

industry for a minimum period of 15 days and submit a project report. The period of 15 days

need be at a single stretch. The vacation days may be utilized for this purpose. A report of the

training should be submitted to the department during the sixth semester for internal

evaluation.

Generic Elective

Sl. No. Semester Paper Title

1 V CH5GET01 Novel

Inorganic Solids

2 V CH5GET02 Industrial

Chemistry

3 V CH5GET03 Green

Chemistry

31

Choice Based Course

Sl.

No.

Semester Paper Title

1 VI CH6CBT01 Polymer Chemistry

2 VI CH6CBT02 Instrumental Methods of Chemical Analysis

3 VI CH6CBT03 Computer Applications in Chemistry

32

SYLLABUS FOR CORE (CHEMISTRY) COURSES

SEMESTER I

CH1CRT01 GENERAL INORGANIC CHEMISTRY

Credits – 2 (36 Hrs )

Module 1: Some Basic Chemical Concepts (6 hrs)

Symbol of elements – IUPAC Nomenclature. Atomic number and mass number - Atomic

mass – Isotopes, isobars and isotones. Molecular mass - Mole concept – Molar volume.

Oxidation and reduction – Oxidation number and valency – Variable valency - Equivalent

mass.

Qualitative Analysis: Applications of solubility product and common ion effect in the

precipitation of cations. Principle of intergroup separation of cations. Interfering acid radicals

and their elimination (oxalate, fluoride, borate and phosphate).

Module 2: Atomic Structure (9 hrs)

Introduction based on historical development – John Dalton's atomic theory – Thomson’s

atom model and its limitations – Rutherford’s atom model and its limitations - Failure of

classical physics – Black body radiation - Planck’s quantum hypothesis - Photoelectric effect

- Generalization of quantum theory - Atomic spectra of hydrogen and hydrogen like atoms–

Bohr theory of atom – Calculation of Bohr radius, velocity and energy of an electron -

Explanation of atomic spectra - Limitations of Bohr theory - Sommerfeld modification. Louis

de Broglie's matter waves – Wave-particle duality - Electron diffraction - Heisenberg's

uncertainty principle.

Schrödinger wave equation (derivation not expected), wave functions – significance of ψ and

ψ2 – Atomic orbitals and concept of Quantum numbers - Shapes of orbitals (s, p and d) -

Pauli’s Exclusion principle - Hund’s rule of maximum multiplicity - Aufbau principle –

Electronic configuration of atoms.

Module 3: Periodic Table and Periodic Properties (6 hrs)

Modern periodic law – Long form periodic table. Periodicity in properties: Atomic and ionic

radii - Ionization enthalpy - Electron affinity (electron gain enthalpy) – Electronegativity.

Electronegativity scales: Pauling and Mullikan scales. Effective nuclear charge – Slater rule

33

and its applications – Polarising power. Diagonal relationship and anomalous behavior of

first element in a group.

Module 4: Chemistry of s and p block elements (6 hrs)

Periodicity in s-and p- block elements with respect to electronic configuration, atomic and

ionic size, ionization energy and electro negativity. Allotropy in C, S and P. Oxidation states

with reference to elements in unusual and rare oxidation states like carbides and nitrides.

Inert pair effect.

Module 5: Chemistry of d and f block elements (9 hrs)

Transition Metals: General characteristics: Metallic character, oxidation states, size, density,

melting points, boiling points, ionization energy, colour, magnetic properties, reducing

properties, catalytic properties, complex formation and alloy formation. Difference between

first row and other two rows. Preparation, properties, structure and uses of KMnO4 and

K2Cr2O7.

Lanthanides: Electronic configuration and general characteristics – Occurrence of

lanthanides - Importance of beach sands of Kerala – Isolation of lanthanides from monazite

sand - Separation by ion exchange method. Lanthanide contraction: Causes and

consequences. Industrial importance of lanthanides.

Actinides: Electronic configuration and general characteristics – Comparison with

lanthanides.

.References

1. D.A. Skoog, D.M. West, F.J. Holler and S.R. Crouch, Fundamentals of Analytical

Chemistry, 8th Edition, Brooks/Cole, Thomson Learning, Inc., USA, 2004.

2. J. D. Lee, Concise Inorganic Chemistry, 5th edn., Blackwell Science, London, 2010.

3. B.R. Puri, L.R. Sharma and K.C. Kalia, Principles of Inorganic Chemistry, 31st

Edition, Milestone Publishers and Distributors, New Delhi, 2013.

4. Satya Prakash, Advanced Inorganic Chemistry, Volume 1, 5th Edition, S. Chand and

Sons, New Delhi, 2012.

5. J. Mendham, R.C. Denney, J. D. Barnes and M. Thomas, Vogel’s Text Book of

Quantitative Chemical Analysis, 6th Edition, Pearson Education, Noida, 2013.

6. R. Gopalan, Inorganic Chemistry for Undergraduates, Universities Press, Hyderabad,

2009.

34

SEMESTER II

CH2CRT02 CHEMICAL BONDING AND NUCLEAR CHEMISTRY

Credits-2 (36 hrs)

Module 1: Chemical Bonding – I (12hrs)

Introduction – Octet rule and its limitations. Types of bonds:

Ionic Bond: Factors favouring the formation of ionic bonds - Lattice energy of ionic

compounds - Born- Lande equation (derivation not expected) – Solvation enthalpy and

solubility of ionic compounds – Born-Haber cycle and its applications – Properties of ionic

compounds - Polarisation of ions – Fajan's rule and its applications.

Covalent Bond: Lewis theory. VSEPR theory: Postulates - Applications - Shapes of

molecules - BeF2, BCl3, SnCl2, CCl4, NH3, H2O, PF5, SF4, ClF3, XeF2, SF6, IF5, XeF4, IF7

and XeF6.

Hybridization: Definition and characteristics - sp (BeCl2, C2H2), sp2 (BF3, C2H4), sp3 (CH4,

NH3, H2O, NH4+, H3O

+ and SO42-), sp3d (PCl5), sp3d2 (SF6) and sp3d3 (IF7) hybridizations.

Valence Bond Theory- Limitations of VBT. Properties of covalent compounds. Polarity of

bonds – Percentage of ionic character –Dipole moment and molecular structure.

Module 2: Chemical Bonding – II (9 hrs)

Covalent Bond: Molecular Orbital Theory – LCAO - Bonding and anti bonding molecular

orbitals – Bond order and its significance. MO diagrams of homonuclear and heteronuclear

diatomic molecules: H2, He2, Li2, Be2, B2, C2, N2, O2, F2, CO and NO – Comparison of bond

length, magnetic behavior and bond energy of O2, O2+, O2

2+, O2- and O2

2-. Resonance

structures of borate, carbonate and nitrate ions – Comparison of bond energy. Comparison of

VB and MO theories. Metallic Bond: Free electron theory, valence bond theory and band

theory (qualitative treatment only) - Explanation of metallic properties based on these

theories.

Intermolecular Forces: Introduction. Hydrogen bond: Intra and inter molecular hydrogen

bonds – Effect on physical properties. Induction forces and dispersion forces: Van der Waals

forces, ion-dipole, dipole-dipole, ion-induced dipole, dipole-induced dipole and induced

dipole-induced dipole interactions

Module 3: Nuclear Chemistry (9 hrs)

Nuclear particles, size of the nucleus - Nuclear forces - Nuclear stability – N/P ratio –

Packing fraction – Mass defect – Binding energy. Nuclear models –Shell model and liquid

drop model.

35

Natural radioactivity – Modes of decay – Group displacement law – Theories of

disintegration – Rate of decay – Decay constant – Half-life period – Gieger-Nuttall rule –

Radioactive equilibrium –Disintegration series – Transmutation reactions using protons,

deutrons, α-particles and neutrons – Artificial radioactivity – Positron emission and K

electron capture – Synthetic elements.

Module 4: Applications of radioactivity (6 hrs)

Radio carbon dating – Rock dating – Isotopes as tracers – Study of reaction mechanism

(ester hydrolysis). Application of radioactive isotopes in medicine - Radio diagnosis and

radiotherapy. Nuclear fission - Atom bomb - Nuclear reactors - Nuclear reactors in India –

Nuclear fusion and Hydrogen bomb.

References

1. J. D. Lee, Concise Inorganic Chemistry, 5th edn., Blackwell Science, London.

2. B. R. Puri, L. R. Sharma, Kalia, Principles of Inorganic Chemistry, Milestone Publishers,

New Delhi.

3. C. N. R. Rao, University General Chemistry, Macmillan India.

4. F. A. Cotton, G. Wilkinson and P. L. Gaus, Basic Inorganic Chemistry, 3rd edn., John Wiley.

5. B. Douglas, D. Mc Daniel, J. Alexander, Concepts and models in Inorganic Chemistry.

6. H.J. Arnikar, Essentials of Nuclear Chemistry, 4th Edition, New Age International (P) Ltd.,

New Delhi, 1995 (Reprint 2005).

7. S. Glasstone, Source Book on Atomic Energy, 3rd Edition, East-West Press Pvt. Ltd.,

New Delhi, 1967.

36

Semester I and Semester II

Inorganic Chemistry Practical: Credit-2 72 hours

CH2CRP01 : Qualitative Inorganic Analysis

1. Study of the reactions of the following radicals with a view to their identification and

confirmation. Ag+ , Hg2+, Pb2+, Cu2+, Bi2+, Cd2+, As3+, Sn2+, Sb3+, Fe2+, Fe3+, Al3+, Cr3+, Zn2+

, Mn2+, Co2+, Ni2+, Ca2+, Sr2+, Ba2+, Mg2+, Li+ , Na+ , K+ , NH4+ . CO3

2- , S2- , SO4

2-, NO3,, F-,

Cl-, Br- , BO2- , C2O4

2- , C4H4O62- , CH3COO- , PO4

3- , AsO33- , AsO4

3- and CrO42-

2. Systematic qualitative analysis of mixtures containing two acid and two basic radicals

from the above list without interfering radical and with one interfering radical by Semi-micro

method only. (Minimum of 10 mixtures to be analysed)

References:

1. A. I. Vogel ‘A Text Book of Quantitative Inorganic Analysis Including Elementary

Instrumental Analysis’: (Third Ed.) (ELBS)

2. G. Svehla, Text Book of Vogel's Macro and Semi-micro Inorganic Analysis, revised,

Orient Longman.

3. V. V. Ramanujam, ‘Inorganic Semi micro Qualitative Analysis’, The National Publishing

Co., Chennai,

4. W. G. Palmer ‘Experimental Inorganic Chemistry’, Cambridge.

37

Semester III

CH3CRT03 Basic Organic Chemistry – I

Credit-3 54 hours

Module 1: Fundamentals of Organic Chemistry (8 hours)

Classification and IUPAC system of nomenclature of common organic compounds. Line

diagram drawing.

Meaning of reaction mechanism. Polarity of bonds.

Electronic displacements: Inductive effect, Electromeric Effect, Mesomeric effect,

Resonance and Hyperconjugation. Steric effects.

Cleavage of bonds: Homolysis and Heterolysis with suitable examples. Curly arrow rules,

formal charges.

Types of reagents: Nucleophiles and electrophiles.

Reactive intermediates: Carbocations, Carbanions, Free radicals and Carbenes – types, shape

and relative stability.

Types of organic reactions: Addition, Elimination, Substitution, Rearrangement and Redox

reactions (definition and one example each).

Module 2: Stereochemistry (12 hours)

Stereoisomerism – definition, classification.

Optical isomerism: Optical Activity, Specific Rotation, Concept of chirality (upto two

carbon atoms). Configuration. Enantiomerism, Diastereomerism and Meso compounds.

Racemic mixture and methods of resolution. Asymmetric synthesis (partial and absolute).

Threo and erythro; D and L designations; Cahn-Ingold-Prelog Rules: R/ S notation (for up to

2 chiral carbon atoms).

Geometrical isomerism:cis–trans, syn-anti and E/Z nomenclature (for upto two C=C

systems) with C.I.P rules. Methods of distinguishing geometrical isomers.

Conformational analysis: Conformational analysis with respect to ethane, butane and

cyclohexane. Relative stability and energy diagrams. Interconversion of Wedge formula,

Newman, Sawhorse and Fischer projection formulae. Chair, Boat and Twist boat forms of

cyclohexane with energy diagrams. Conformation of methyl cyclohexane.

Origin of ring strain in cyclic systems. Baeyer’s strain theory.

Module 3: Aliphatic Hydrocarbons (12 hours)

38

Alkanes:

Preparation: Catalytic hydrogenation, Wurtz reaction, Wurtz-Fittig reaction, Kolbe’s

synthesis, from Grignard reagent.

Reactions: Free radical substitution: Halogenation.

Alkenes:

Preparation: Elimination reactions: Mechanism of E1, E2, E1cb reactions. Dehydration of

alkenes and dehydrohalogenation of alkyl halides (Saytzeff’s and Hofmann’s rule);

Conversion of alkynes into cis alkenes (Partial catalytic hydrogenation) and trans alkenes

(Birch reduction).

Reactions: cis-addition (alk. KMnO4) and trans-addition (bromine). Addition of HX

(Markownikoff’s and anti-Markownikoff’s addition with mechanism), Hydration,

Ozonolysis, Oxymecuration-demercuration, Hydroboration-oxidation. 1,2- and 1,4-addition

reactions in conjugated dienes. Allylic and benzylic bromination using NBS.

Alkynes:

Preparation: Acetylene from CaC2 and conversion into higher alkynes; by dehalogenation of

tetra halides and dehydrohalogenation of vicinal dihalides.

Reactions: Acidity of alkynes, formation of metal acetylides, alkylation of terminal alkynes

and conversion into higher alkynes, addition of bromine and alkaline KMnO4, ozonolysis and

oxidation with hot alk. KMnO4.

Module 4: Aromatic Hydrocarbons (6 hours)

Aromaticity: Hückel’s rule - Application to benzenoid and non-benzenoid compounds.

Preparation (of benzene): from phenol, by decarboxylation, from acetylene, from benzene

sulphonic acid.

Reactions (of benzene): Electrophilic aromatic substitution: nitration, halogenation,

sulphonation and Friedel-Craft’s reaction (alkylation and acylation) with their mechanism.

Orientation of aromatic substitution. ortho, para and meta directing effects of groups.

Module 5: Alkyl and Aryl Halides (12 hours)

Alkyl Halides:

Preparation: from alkenes andalcohols.

Reactions: Hydrolysis, nitrite & nitro formation, nitrile & isonitrile formation. Williamson’s

ether synthesis: Types of nucleophilic substitution reactions - SN1, SN2 and SNi mechanisms

with stereochemical aspects and effects of solvent etc. Nucleophilic substitution vs.

elimination.

Aryl Halides:

Preparation: (Chloro, bromo and iodo-benzene case): from phenol, Sandmeyer

& Gattermann reactions.

Reactions (Chlorobenzene): Aromatic nucleophilic substitution (replacement by –OH group)

39

and effect of nitro substituent. Benzyne mechanism: KNH2/NH3 (or NaNH2/NH3).

Reactivity and relative strength of C-Halogen bond in alkyl, allyl, benzyl, vinyl and aryl

halides.

Organometallic compounds of Mg (Grignard reagents) – Formation, structure and synthetic

applications.

Module 6: Pericyclic Reactions (4 hours)

Classification – Electrocyclic reactions, Cycloadditions - Diels-Alder reaction and

Sigmatropic rearrangements - Claisen rearrangemen. Stereochemical aspects.

Reference Books:

1. Morrison, R.T., Boyd, R.N. & Bhattacharjee, S.K. Organic Chemistry, 7th ed.,

Dorling Kindersley (India) Pvt. Ltd (Pearson Education), 2011.

2. Graham Solomon, T.W., Fryhle, C.B. & Snyder, S.A. Organic Chemistry, John

Wiley & Sons, 2014.

3. McMurry, J. Organic Chemistry, 7th ed. Cengage Learning, 2013.

4. Sykes, P. A Guidebook to Mechanism in Organic Chemistry, Orient Longman, 1988.

5. Eliel, E.L. & Wilen, S.H. Stereochemistry of Organic Compounds, Wiley, 1994.

6. Finar, I.L. Organic Chemistry (Vol. 1 & 2), Dorling Kindersley (India) Pvt. Ltd

(Pearson Education).

7. Jain, M.K. & Sharma, S.C. Modern Organic Chemistry, Vishal Publishing Co. 2010.

8. Bahl, A. & Bahl, B.S. Advanced Organic Chemistry, S. Chand, 2010.

9. Kalsi, P. S. Stereochemistry - Conformation and Mechanism; New Age International,

2005.

10. Pillai, C.N. Organic Chemistry, Universities Press, 2008.

11. Gupta, S.S. Organic Chemistry, Oxford University Press, 2014.

40

Semester IV

CH4CRT04 Basic Organic Chemistry –II

Credit-3 54 hours

Module 1: Alcohols, Phenols and Ethers (14 hours)

Alcohols:

Preparation: Preparation of 1о, 2о and 3о alcohols: using Grignard reagent, Ester hydrolysis,

Reduction of aldehydes, ketones, carboxylic acid and esters.

Reactions: With sodium, HX (Lucas test), esterification, oxidation (with PCC, alk. KMnO4,

OsO4, acidic dichromate, conc. HNO3). Oppenauer oxidation. Ascent and descent of alcohol

series.

Diols: Oxidative cleavage of diols using Lead tetraacetate and Periodic acid. Pinacol-

Pinacolone rearrangement (with mechanism).

Phenols:

(Phenol case) Preparation: Cumene hydroperoxide method, from diazonium salts.

Reactions: Electrophilic substitution: Nitration, halogenation and sulphonation. Reimer-

Tiemann reaction and Fries rearrangement with mechanism. Preparation and uses of

nitrophenols, picric acid, resorcinol and quinol.

Ethers and Epoxides (aliphatic and aromatic):

Synthesis of ethers and epoxides.

Cleavage of ethers with HI. Zeisel’s method of estimation of alkoxy groups. Reactions of

epoxides with alcohols, ammonia derivatives and LiAlH4.

Module 2: Aldehydes and Ketones (aliphatic and aromatic): (14 hours)

Formaldehye, acetaldehyde, acetone, benzaldehyde and benzophenone.

Preparation: from acid chlorides and from nitriles.

Reactions – Reaction with HCN, ROH, NaHSO3, NH2-G derivatives. Iodoform test. Aldol,

Claisen-Schmidt, Knoevenagel and Benzoin condensations (with mechanism). Cannizzaro

reaction, Wittig reaction and Mannich reaction (with mechanism). Beckmann, Benzil-

Benzilic acid and Baeyer-Villiger rearrangements (with mechanism). Oxidations and

reductions (Clemmensen, Wolff-Kishner, LiAlH4, NaBH4, MPV, PDC).

Addition reactions of α, β- unsaturated carbonyl compounds - Michael addition.

Module 3: Carboxylic Acids, Sulphonic Acids and their Derivatives (18 hours)

Carboxylic acids (aliphatic and aromatic):

Preparation: Hydrolysis of nitrile, side chain oxidation and carboxylation of Grignard reagent.

Acidic and alkaline hydrolysis of esters.

Reactions: Structure of carboxylate ion, effect of substituents on acid strength.

Hell – Volhard - Zelinsky reaction and decarboxylation reaction.

41

Carboxylic acid derivatives (aliphatic):

Preparation: Acid chlorides, Anhydrides, Esters and Amides from acids and their

interconversion.

Reactions: Comparative study of nucleophilicity of acyl derivatives. Perkin condensation and

Claisen condensation (with mechanism). Dieckmann and Reformatsky reactions.

Methods of formation and reactions of dicarboxylic acids, hydroxy acids and unsaturated

acids like anthranilic acid, cinnamic acid, acrylic acid, oxalic acid, malonic acid, citric acid,

adipic acid, maleic acid and fumaric acid.

Sulphonic acids and their derivatives:

Preparation and reactions of benzene sulphonic acid, benzene sulphonyl chloride and ortho

and para toluene sulphonyl chlorides - uses.

Module 4: Active Methylene Compounds (4 hours)

Preparation: Ethyl acetoacetate by Claisen ester condensation. Keto-enol tautomerism.

Reactions: Synthetic uses of ethylacetoacetate, diethyl malonate and ethyl cyanoacetate

(preparation of non-heteromolecules only).

Alkylation of carbonyl compounds via enamines.

Module 5: Polynuclear Aromatic Compounds (4 hours)

Classification. Structure and properties of the following compounds with reference to

electrophilic and nucleophilic substitution: Naphthalene, Anthracene and Phenanthrene.

Elementary idea of naphthyl amines, naphthols, naphthaquinone and anthraquinone.

Reference Books:



2. Graham Solomon, T.W., Fryhle, C.B. & Snyder, S.A. Organic Chemistry, Wiley,

2014.


4. Finar, I.L. Organic Chemistry (Vol. 1), Dorling Kindersley (India) Pvt. Ltd (Pearson

Education).

5. Carey, F.A., Giuliano, R.M. Organic Chemistry, 8th ed., Tata McGraw Hill,.2012



8. Tewari, K.S. & Vishnoi, N.K. Organic Chemistry, Vikas Publishing House, 2012.



42

Semester III and IV

ORGANIC CHEMISTRY PRACTICALS- I

Cridit-2 72 hours


1. Determination of physical constants of solids and liquids.

2. Tests for elements: Nitrogen, Halogens and Sulphur

3. Tests for unsaturation.

4. Tests for aromatic character.

5. Study of the reactions of the following functional groups:

carboxylic acid, 1,2-dicarboxylic acid, phenol, aldehyde, ketone, ester, reducing and

nonreducing sugars, polynuclear hydrocarbon, primary, secondary and tertiary amines,

amides, diamide, nitro and halogen compounds.

6. Systematic analysis of the following organic compounds containing one functional group

and characterization with a derivative:

carboxylic acid, 1,2-dicarboxylic acid, phenol, aldehyde, ketone, ester, reducing and

nonreducing sugars, polynuclear hydrocarbon, primary, secondary and tertiary amines,

amide, diamide, nitro and halogen compounds.

(Minimum twelve compounds to be analysed)

Reference Books:

1. Furniss, B.S.; Hannaford, A.J.; Rogers, V. Smith, P.W.G.; Tatchell, A.R. Vogel’s Textbook

of Practical Organic Chemistry, 5th ed., Pearson Education, 2005.

2. Mann,F.G.; Saunders, B.C. Practical Organic Chemistry, 4th ed., Pearson Education, 2009.

3. Ahluwalia, V.K.; Dhingra, S. Comprehensive Practical Organic Chemistry – Qualitative

Analysis, Universities Press, 2000.

4. Vishnoi, N.K. Advanced Practical Organic Chemistry, 3rd ed., Vikas Publishing House,

New Delhi, 2010.

43

SEMESTER V

Credit-3 (54 hrs)

CH5CRT05 ANALYTICAL AND ENVIRONMENTAL CHEMISTRY

Module 1: Analytical methods in Chemistry (9 hours)

Titrimetric analysis - fundamental concepts. Methods of expressing concentration: Weight

percentage, molality, molarity, normality, mole fraction, ppm. and ppb. Primary standard-

secondary standard, quantitative dilution – problems. Acid base titrations- titration curves –

pH indicators. Redox titrations – titration curve –titrations involving MnO4- and Cr2O7

2- -

redox indicators. Complexometric titrations – EDTA titrations - titration curves – metal ion

indicators- Gravimetric analysis: Unit operations in gravimetric analysis Illustrations using

iron and barium estimation. Separation and purification techniques – Filtration,

Crystallization and precipitation – Fractional distillation, Solvent extraction.

Module 2: Evaluation of Analytical Data (9 hours)

Units, significant digits, rounding, scientific and prefix notation, graphing of data - Precision

and accuracy – Types of errors – Ways of expressing precision – Ways to reduce systematic

errors - reporting analytical data. Statistical treatment of analytical data – population and

samples –Mean and standard deviation – distribution of random errors– confidence limits –

tests of significance – Correlation and regression –Curve fitting and the method of least

squares.

Module 3: Chromatographic and Thermal Methods (12 hrs):

Column Chromatography - Principle, types of adsorbents, preparation of the column, elution,

recovery of substances and applications. Thin Layer Chromatography - Principle, choice of

adsorbent and solvent, Preparation of Chromatoplates, Rf-Values, significance of Rf values.

Paper Chromatography - Principle, Solvents used, Development of Chromatogram,

ascending, descending and radial paper chromatography. Ion - Exchange Chromatography –

Principle - Experimental techniques. Gas Chromatography - Principle - Experimental

techniques - Instrumentation and applications. High Performance Liquid Chromatography

(HPLC) - Principle- Experimental techniques, instrumentation and advantages.

Thermal Methods: Principle and applications of thermo gravimetry(TGA), differential

thermal analysis(DTA) and differential scanning calorimetry(DSC). Applications - TGA and

DTA of calcium oxalate monohydrate. Applications in the study of polymers.

Module 5: Inorganic Polymers (6 hrs)

44

Inorganic polymers – general properties, comparison with organic polymers, glass transition

temperature. Sulphur based polymers – polymeric sulphur nitride and chalcogenic glasses

(preparation, properties and uses). Phosphorus based polymers – polyphosphazenes and

polyphosphates. Silicon based polymers – silicones and silicone rubber (preparation,

properties and uses).

Module 6: Non aqueous solvents (6 hrs)

Classification of solvents, characteristics of solvents, reactions in liquid ammonia, liquid

sulphur dioxide and liquid HF (acid base, amphoteric, solvation, oxidation – reduction,

complex formation). Solutions of alkali metals in liquid ammonia.

Module 7: Environmental Chemistry (12 hrs)

Environmental segments- Biogeochemical cycles- Structure of the atmosphere - Air

pollution. Major air pollutants - Oxides of carbon, nitrogen and sulphur - Particulates –

London smog and photochemical smog. Effects of air pollution- Acid rain, greenhouse effect

and depletion of ozone layer. Bhopal Tragedy (a brief study). Control of air pollution -

Alternate refrigerants.

Water pollution: Water pollution due to sewage and domestic wastes – Industrial effluents –

Agricultural discharge – Eutrophication. Quality of drinking water - Indian standard and

WHO standard. Water quality parameters: pH, DO, BOD and COD – Determination of DO,

BOD and COD. Trace metal pollutants in water (Pb, Cd and Hg) - Minamata disease. Control

of water pollution. Soil pollution- Pollution due to pesticides and plastics (Sources, effects

and consequences).

References

1. J. Mendham. R.C. Denney, J.D. Barnes and M. Thomas, Vogel’s Textbook of Quantitative

Chemical Analysis, 6th Edition, Pearson Education, Noida, 2013.


Chemistry, 8th Edition, Brooks/Cole, Thomson Learning, Inc., USA, 2004.

3. J.E. Huheey, E.A. Keitler and R.L. Keitler, Inorganic Chemistry – Principles of Structure

and Reactivity, 4th Edition, Pearson Education, New Delhi, 2013.

4. D.F. Shriver and P. Atkins, Inorganic Chemistry, 5th Edition, Oxford University Press,

New York, 2010.

5. Gary L. Miessler, Paul J. Fischer and Donald A. Tarr, Inorganic Chemistry, 5th Edition,

Prentice Hall, New Jersey, 2013.

45

6. Wahid U. Malik, G.D. Tuli and R.D. Madan, Selected Topics in Inorganic Chemistry, S.

Chand and Co., New Delhi, 2010 (Reprint).

7. Gurudeep Raj, Advanced Inorganic Chemistry Vol-I, 33rd Edition, Krishna Prakashan

Media (P)Ltd., Meerut, 2014.

8. A.G. Sharpe and H.J. Emeleus, Modern Aspects of Inorganic Chemistry, 4th Edition, UBs

Publisher’s Distributors Ltd., New Delhi, 2000.

9. James E. Girard., Principles of Environmental Chemistry, 1st Indian Edition, Johns &

Bartlett India Pvt. Ltd., New Delhi, 2011.

10. A.K. De., Environmental Chemistry, 6th Edition, New Age International (P) Ltd., New

Delhi, 2006.

46

Semester V

CH5CRT06 Advanced Organic Chemistry – I

Credit-3 54 hours

Module 1: Nitrogen Containing Compounds (16 hours)

Nitro compounds (aliphatic and aromatic):

Preparation: Methods of preparation of nitroalkanes and aromatic nitro compounds.

Reactions: Tautomerism of nitromethane. Reduction products of nitrobenzene in acidic,

neutral and alkaline media. Electrolytic reduction and selective reduction of polynitro

compounds. Formation of charge transfer complexes.

Amines (aliphatic and aromatic):

Preparation: From alkyl halides, Gabriel’s phthalimide synthesis, Hofmann bromamide

reaction.

Reactions: Hofmann vs. Saytzeff elimination, Carbylamine test, Hinsberg test, with HNO2,

Schotten – Baumann Reaction (with mechanism). Electrophilic substitution reactions of

aniline: Halogenation, nitration and sulphonation. Stereochemistry of amines. Structural

features affecting basicity of aliphatic and aromatic amines. Comparative study of aliphatic

and aromatic amines. Distinction between 1°, 2° and 3° amines with Hinsberg reagent and

nitrous acid. Quaternary amine salts as phase-transfer catalysts.

Diazonium salts:

Preparation: From aromatic amines. Structure and stability of benzenediazonium salts.

Reactions: Structure and stability of benzene diazonium salts. Conversion to benzene,

phenol, chloro, bromo, iodo and fluoro benzenes, nitro benzene, dyes. Mechanisms of

Sandmeyer and Gatterman reactions. Schiemann and Gomberg reactions.

Preparation, structure and uses of Phenyl hydrazine, Diazomethane and Diazoacetic ester.

Arndt –Eistert synthesis – Mechanism of Wolff rearrangement.

Module 2: Heterocyclic Compounds (6 hours)

Classification and nomenclature. Structure and aromaticity of 5-numbered and 6-membered

rings containing one heteroatom.

Synthesis and reactions of:

Furan, Pyrrole, Thiophene (Paal-Knorr synthesis, Knorr pyrrole synthesis and Hantzsch

synthesis), Pyridine (Hantzsch synthesis), Indole (Fischer’s indole synthesis and Madelung

synthesis), Quinoline (Skraup synthesis, Friedlander’s synthesis, and Doebner- Miller

synthesis) and Isoquinoline (Bischler-Napieralski reaction, Pictet-Spengler reaction and

Pomeranz-Fritsch reaction).

Module 3: Drugs (6 hours)

Classification of drugs. Structure and therapeutic uses of antipyretics: Paracetamol (with

synthesis), Antibiotics: Chloramphenicol (with synthesis), Analgesics: Ibuprofen (with

synthesis), Antimalarials: Chloroquine (with synthesis), Antacids: Ranitidine, Anti-cancer

47

drugs: Chlorambucil. Psychotropic drugs: Tranquilizers, antidepressants and stimulants with

examples. Drug addiction and abuse. Prevention and treatment.

Drug action - Receptor theory. Structure –activity relationships of drug molecules.

Module 4: Dyes (4 hours)

Theories of colour and chemical constitution.

Classification of dyes. Natural and synthetic dyes.

Synthesis and applications of: Azo dyes – Methyl orange; Triphenyl methane dyes -

Malachite green and Rosaniline; Phthalein dyes – Phenolphthalein and Fluorescein; Indigoid

dyes - Indigotin; Anthraquinoid dyes – Alizarin. Edible Dyes (Food colours) with examples.

Module 5: Organic Photochemistry (4 hours)

Introduction. Photochemical versus Thermal reactions. Electronic excitation and fate of

excited molecules. Jablonski diagram. Fluorescence and phosphorescence. Photosensitisation.

Photochemical reactions: Norrish type I and II reactions of acyclic ketones, Paterno-Buchi

and Photo-Fries reactions.

Module 6: Organic Spectroscopy (18 hours)

General principles. Introduction to absorption and emission spectroscopy.

UV Spectroscopy: Types of electronic transitions, λmax, Chromophores and Auxochromes,

Bathochromic and Hypsochromic shifts, Intensity of absorption; Application of Woodward

Rules for calculation of λmax for the following systems: α,β-unsaturated aldehydes, ketones,

carboxylic acids and esters; Conjugated dienes: alicyclic, homoannular and heteroannular;

Extended conjugated systems (aldehydes, ketones and dienes); distinction between cis and

trans isomers.

IR Spectroscopy: Fundamental and non-fundamental molecular vibrations; IR absorption

positions of O and N containing functional groups; Effect of H-bonding, conjugation,

resonance and ring size on IR absorptions; Fingerprint region and its significance; application

in functional group analysis.

NMR Spectroscopy: Basic principles of Proton Magnetic Resonance, chemical shift and

factors influencing it; Spin – Spin coupling and coupling constant; Anisotropic effects in

alkene, alkyne, aldehydes and aromatics, Interpretation of NMR spectra of simple

compounds.

Applications of IR, UV and NMR for identification of simple organic molecules.

48

Mass Spectrometry: Introduction. EI ionisation. Determination of molecular mass by MS

(elementary idea only – fragmentation study not required).

Reference Books:



2. Graham Solomon, T.W., Fryhle, C.B. & Snyder, S.A. Organic Chemistry, Wiley,

2014.


4. Finar, I.L. Organic Chemistry (Vol. 1 & 2), Dorling Kindersley (India) Pvt. Ltd




7. John R. Dyer: Applications of Absorption Spectroscopy of Organic Compounds,

Prentice Hall.

8. R.M. Silverstein, G.C. Bassler & T.C. Morrill: Spectroscopic Identification of

Organic Compounds, Wiley.



49

CH5CRT07 States of matter, Colloids and General Informatics

Credits - 3 (54 Hours)

Aim

To study the general characteristics of different states of matter, colloids and role of

informatics in understanding Chemistry.

Objectives

To study the intermolecular forces in gases and liquids

To understand the dynamics of the molecules in the gases and liquids

To study liquefaction of gases

To learn the structure of solids

To study defects in crystals

To study the adsorption phenomena.

To understand colloidal state and its applications

To learn computer based applications in analysis and presentation of experimental data.

Module 1: Gaseous State (12 Hours)

Postulates of Kinetic Theory of Gases and derivation of the kinetic gas equation. Deviation of

real gases from ideal behaviour, compressibility factor, causes of deviation. van der Waals equation

of state for real gases. Boyle temperature (derivation not required). Critical phenomena and Andrews

isotherms of CO2, critical constants and their calculation from van der Waals equation. Virial equation

of state, van der Waals equation expressed in virial form.

Maxwell Boltzmann distribution laws of molecular velocities and molecular energies

(graphical representation – derivation not required) and their importance. Temperature dependence of

these distributions. Most probable, average and root mean square velocities (no derivation).

Collision properties: Collision cross section, collision number, collision frequency, collision

diameter and mean free path of molecules. Relation between mean free path and coefficient of

viscosity. Viscosity of gases and effect of temperature and pressure on coefficient of viscosity

(qualitative treatment only). Chapman Equation.

Barometric distribution law, Law of equipartition of energy, degrees of freedom and

molecular basis of heat capacities. Liquefaction of gases (based on Joule-Thomson effect)

Module 2: Liquid state (3 Hours)

Intermolecular forces in liquids (qualitative idea only). Surface tension and its measurement

by stalagmometer method, factors affecting Surface tension, Viscosity, Poisuelle’s equation,

Determination of viscosity by Ostwald’s viscometer, Effect of temperature on surface tension and

coefficient of viscosity of a liquid (qualitative treatment only).

.

50

Module 3: Group theory (6 Hours)

Elements of symmetry – Proper and improper axis of symmetry, plane of symmetry, centre of

symmetry and identity element. Combination of symmetry elements, Schoenflies symbol, Point

groups, C2V, C3V and D3h, Group multiplication table of C2V, Determination of point groups of

simple molecules like H2O, NH3 and BF3.

Module 4: Solid state (12 Hours)

The nature of the solid state – anisotropy – Forms of solids. Unit cells, crystal systems,

Bravais lattice types and identification of lattice planes. Laws of Crystallography – Law of

constancy of interfacial angles, Law of rational indices. Miller indices. X–Ray diffraction by

crystals, Bragg’s law. Bragg’s x-ray diffractometer method and powder pattern method. Analysis

of powder diffraction patterns of NaCl and KCl, density of cubic crystals.

Structure of ionic compounds of the type AX (NaCl, CsCl, ZnS) and AX2 (CaF2, Na2O)

Defects in crystals – stoichiometric and non-stoichiometric defects, extrinsic and intrinsic defects.

Electrical conductivity, semiconductors, n-type, p-type, Superconductivity – An introduction.

Liquid crystals and its thermographic behaviour. Classification, structure of nematic and

cholestric phases.

Module 5: Surface chemistry and Colloidal state (9 Hours)

Adsorption – types, adsorption of gases by solids – factors influencing adsorption – Freundlich

adsorption isotherm – Langmuir adsorption isotherm - derivation of Langmuir adsorption

isotherm. The BET theory (no derivation) – use of BET equation for the determination of surface

area.

Types of solutions – true, colloid and suspensions, Purification of colloids – Ultra filtration

and electrodialysis, optical and electrical properties of colloids. Ultra microscope, Electrical double

layer and zeta potential. Coagulation of colloids, Hardy-Schulz rule. Micelles and critical micelle

concentration, sedimentation and streaming potential, Application of colloids – Cottrell precipitator,

purification of water and delta formation.

Module 5: Overview of Information Technology (6 Hours)

Features of the modern personal computer and peripherals – computer network and internet –

overview of operating system and major application of softwares. Data information and knowledge –

knowledge management – internet as a knowledge repository – academic search techniques – creating

your cyber presence – open access initiation – open active publishing models – Basic concepts of IPR,

copy right and patents – plagiarism. Introduction to use of IT in teaching and learning –educational

softwares – INFLIBNET, NICNET, BRNET, NPTEL, VIRTUAL LABS OF MHRD – academic

services.

51

Module 6: Introduction to Chemo informatics (6 Hours)

History and evolution of chemo informatics, Use of chemo informatics, Prospects of

chemo informatics, Molecular Modelling and Structure elucidation.

Storage & retrieval, file formats – MOL, SDF, CML, PDB formats, SYBYL Line Notation,

SMILES of simple molecules like methane, ethyl alcohol, benzene cyclohexane.

Structure drawing, spread sheet and chemistry related soft wares.

Molecular visualization tools. Chemical Databases, Chemical Safety - Toxicology

Information - material safety data sheets .

References

1. P W Atkins, “Physical Chemistry”, Oxford University Press

2. R J Silby and R A Alberty, “Physical Chemistry”, John Wiley & Sons

3. F Daniels and R A Alberty, “Physical Chemistry”, Wiley Eastern

4. Puri, Sharma and Pathania, “Principles of Physical Chemistry”, Millennium Edition, Vishal

Publishing Co

5. R. Stephen Berry, Stuart A. Rice, John Ross, “Physical Chemistry”, 2nd edition, Oxford”.

6. Barrow, G.M. “Physical Chemistry”, Tata McGraw‐Hill (2007).

7. Castellan, G.W. “Physical Chemistry”,4th Ed. Narosa (2004).

8. K. L. Kapoor, “A Textbook of Physical chemistry”, Volumes 1, Macmillan India Ltd.,

9. B. R. Puri, L. R. Sharma, M. S. Pathania, “Elements of Physical chemistry”, Vishal Pub. Co.,

10. L V Azaroff, “Introduction to Solids”, McGraw Hill.

11. N B Hannay, “Solid State Chemistry”, Prentice Hall.

12. A. McQuarrie, J. D. Simon, “Physical Chemistry – A molecular Approach”, Viva Books Pvt.

Ltd.

13. Anthony R. West, “Solid State Chemistry and its Applications”, Wiley Eastern.

14. V Ramakrishnan and M S Gopinathan, “Group Theory in Chemistry”, Vishal Publishing.

15. Salahuddin Kunju and G. Krishnan “Group Theory and its Applications in Chemistry”

16. Rodgers, G.E. “Inorganic & Solid State Chemistry”, Cengage Learning India Ltd.,

17. Gurdeep Raj, “Advanced Physical Chemistry”, Goel Publishing House..

18. M Ravikumar ,Information Technology for Higher Education, Sonali Publications (2004)

19. V. Rajaram, Introduction to Information Technology, Prentice Hall.

20. Andrew R. Leach and V.J. Gillet An Introduction to Chemoinformatics

21. Asteiger, J. & Engel, T. (2003) Chemoinformatics: A text-book. Wiley-VCH.

22. Gupta, S. P. (2011) QSAR & Molecular Modeling. Anamaya Pub.: New Delhi.

23. Alexis Leon & Mathews Leon, Computers Today, Leon Vikas

24. Alexis & Mathews Leon, Fundamentals and Information Technology. Leon Vikas ISBN

08125907890.

52

25. Ramesh Bangia, ‘Learning Computer Fundamentals, Khanna Book Publishers, ISBN

818752252b.

26. Barbara Wilson, Information Technology, The Basics, Thomas Learning.

27. http://www.vlab.co.in

28. http://nptel.iitm.ac.in/

53

CH5CRT08 Quantum Mechanics, Spectroscopy and Photochemistry

Credits - 3 (54 Hours)

Aim

To understand the fundamentals of quantum mechanics and its applications in the study

of structure of atoms, bonding in molecules and molecular spectroscopy

Objectives

To differentiate between classical and quantum mechanics

To study the postulates of quantum mechanics and the quantum mechanical model of

hydrogen atom

To study molecular orbital theory

To study the principle and applications of microwave, infra-red, Raman, electronic

magnetic resonance and ESR spectroscopy.

To study the fundamentals of photochemistry

Module 1: Quantum mechanics (18 Hours)

Classical mechanics: Concepts, Radiation phenomena – Blackbody radiation, Photoelectric

effect, Compton effect and Atomic spectra. Plank’s quantum theory and explanation of the radiation

phenomena. de Broglie hypothesis, dual nature of electrons – Davisson and Germer’s experiment.

Heisensberg’s uncertainty principle and its significance.

Schrodinger wave equation – significance of Ψ, well behaved wave functions, Concept of operators-

Operator algebra – Linear and Hermitian operators - Laplacian and Hamiltonian operators – Eigen

functions and Eigen values of an operator.

Postulates of quantum mechanics, Application of quantum mechanics to simple systems –

Particle in 1-D box, normalization of wave function, application to linear conjugated polyene

(butadiene).

Introductory treatment of Schrödinger equation for hydrogen atom. – Conversion of Cartesian

coordinates to polar coordinates - The wave equation in spherical polar coordinates (derivation not

required) - Separation of wave equation - Radial and angular functions (derivation not required) –

Orbitals. Quantum numbers and their importance, hydrogen like wave functions – radial and angular

wave functions, radial distribution curves.

Molecular orbital theory: basic ideas – criteria for forming MO from AOs. Construction of

molecular orbital by LCAO method for H2+ ion (elementary idea only), physical picture of bonding

and anti bonding wave functions, concept of σ, σ*, π, π* orbitals and their characteristics. MO

diagrams of homonuclear and heteronuclear diatomic molecules – C2, N2, O2, F2, CO and NO.

Module 2: Molecular Spectroscopy-I (15 Hours)

Introduction: electromagnetic radiation, regions of the spectrum, interaction of

electromagnetic radiation with molecules, various types of molecular spectroscopic techniques, Born-

Oppenheimer approximation.

54

Rotation spectroscopy: Introduction to rotational spectroscopy, Rotational energy levels,

Selection rules, determination of bond lengths of diatomic molecules, isotopic substitution.

Vibrational spectroscopy: Introduction, Selection Rules, Classical equation of vibration,

calculation of force constant, concept of anharmonicity, Morse potential, dissociation energies,

fundamental frequencies, overtones, hot bands. Degrees of freedom for polyatomic molecules, modes

of vibration (H2O and CO2 as examples), concept of group frequencies, finger print region, Fermi

resonance.

Vibration-rotation spectroscopy: diatomic vibrating rotator, P, Q, R branches.

Raman spectroscopy: Introduction, Classical and quantum treatment of Raman effect,

Qualitative treatment of Rotational Raman effect; Vibrational Raman spectra, Stokes and anti-Stokes

lines: their intensity difference, rule of mutual exclusion.

Module 3: Molecular Spectroscopy-II (12 Hours)

Electronic spectroscopy: Introduction, selection rule, Franck-Condon principle, electronic

transitions, singlet and triplet states, fluorescence and phosphorescence, dissociation and

predissociation. Polyatomic molecules – qualitative description of σ, π and n- molecular orbitals,

their energy levels and the respective transitions.

Nuclear Magnetic Resonance (NMR) spectroscopy: Principles of NMR spectroscopy,

Larmor precession, chemical shift and low resolution spectra, different scales, spin-spin coupling

and high resolution spectra, interpretation of PMR spectra of organic molecules (Ethanol,

Acetaldehyde & Toluene).

Electron Spin Resonance (ESR) spectroscopy: Principle, hyperfine structure, ESR of

simple radicals (methyl radical, benzene radical and naphthalene radical).

Module 4: Photochemistry (9 Hours)

Characteristics of electromagnetic radiation, Laws of photochemistry- Grothus-Draper law,

Stark-Einstein law. Jablonsky diagram-qualitative description of fluorescence, phosphorescence,

non-radiative processes (internal conversion, intersystem crossing).Quenching of fluorescence.

Quantum yield, examples of low and high quantum yields, photochemical

reactions(decomposition of HBr, isomerisation of Maleic acid to Fumaric acid), photosensitised

reactions(photosynthesis, isomerization of 2-butene), chemiluminescence ,bioluminescence.

Quantitative analysis- Lambert-Beer’s law, physical significance of absorption coefficients.

References

1. R.K. Prasad, Quantum Chemistry, New Age International, 2001

2. Mc Quarrie, J. D. Simon, Physical Chemistry – A molecular Approach, Viva Books.

3. I. N. Levine, Physical Chemistry, Tata Mc Graw Hill,

4. A. Bahl, B. S. Bahl, G. D. Tuli, Essentials of Physical Chemistry, S. Chand and Company,

5. K. J. Laidler, John H.Meiser, Physical Chemistry, 2nd edn.

6. Banwell, C. N. & Mc Cash, E. M. Fundamentals of Molecular Spectroscopy,4th Ed. Tata

McGraw-Hill: New Delhi (2006).

55

7. Kakkar, R. Atomic & Molecular Spectroscopy: Concepts & Applications, Cambridge

University Press (2015).

8. Manas Chanda, Atomic structure and Chemical bonding in Molecular Spectroscopy” Tata

McGraw Hill.

9. D. L. Pavia, G. M. Lampman, G. S. Kriz, Introduction to spectroscopy, 3rd edn, Thomson

Brooks/Cole, 2001.

10. D. N. Satyanarayana, Electronic absorption spectroscopy and related techniques, Universities

Press.

11. D.N. Sathyanarayana, Introduction To Magnetic Resonance Spectroscopy

ESR,NMR,NQR, IK International, 2009.

12. House, J. E. Fundamentals of Quantum Chemistry,2ndEd. Elsevier: USA (2004).

13. Lowe, J. P. & Peterson, K. Quantum Chemistry, Academic Press (2005).

14. Gurdeep Raj, Photochemistry, 6th Edn, Goel Publishing House, 2014

15. Rohatgi-Mukherjee, Fundamentals of Photochemistry, New Age International (P) Ltd.

16. Puri, Sharma & Pathania, Priniciples of Physical Chemistry, Vishal Publishing Co.

17. N. J. Turro, Modern Molecular Photochemistry, 4th Edition University Science Books,

Sausalito, 1991.

18. Physical Chemistry, G.M .Barrow, 6th edn, The Mc GRAW-HILL Companies, INC

56

Semester V

Generic Elective Courses

(Chose any one of the following three)

Credit-3 54 hours

CH5GET01 NOVEL INORGANIC SOLIDS

Module 1: Synthesis and Modification of Inorganic Solids (8hours)

Conventional heat and beat methods, Co-precipitation method, Sol-gel methods,

Hydrothermal method, Ion-exchange and Intercalation methods.

Module 2 : Inorganic Solids of Technological Importance (8hours)

Solid electrolytes – Cationic, anionic, mixed. Inorganic pigments – coloured solids, white and

black pigments.

Molecular material and fullerides, molecular materials & chemistry – one-dimensional

metals, molecular magnets, inorganic liquid crystals.

Module 3: Nanomaterials (12 hours)

Overview of nanostructures and nanomaterials: classification.

Preparation of gold and silver metallic nanoparticles, self-assembled nanostructures-control

of Nano architecture-one dimensional control. Carbon nanotubes and inorganic nanowires.

Bio-inorganic nanomaterials, DNA and nanomaterials, natural and artificial nanomaterials,

bionano composites.

Module 4: Introduction to Engineering Materials for Mechanical Construction

(12hours)

Composition, mechanical and fabricating characteristics and applications of various types of

cast irons, plain carbon and alloy steels, copper, aluminium and their alloys like duralumin,

brasses and bronzes, cutting tool materials, super alloys, thermoplastics, thermosets and

composite materials.

Module 5: Composite Materials (10 hours)

Introduction, limitations of conventional engineering materials, role of matrix in composites,

classification, matrix materials, reinforcements, metal-matrix composites, polymer-matrix

composites, fibre-reinforced composites, environmental effects on composites, applications

of composites.

Module 6: Ceramics & Refractory Materials (4 hours)

Introduction, classification, raw materials, manufacture, properties and applications.

57

Reference Books:

Shriver; Atkins, Inorganic Chemistry, 5th ed., Oxford University Press, 2012.

Adam, D.M. Inorganic Solids: An Introduction to Concepts in Solid State Structural

Chemistry, John Wiley & Sons, 1974.

Poole, C.P.; Owens, F.J. Introduction to Nanotechnology, John Wiley & Sons, 2003.

Rodger, G.E. Inorganic and Solid State Chemistry, Cengage Learning India Edition,

2002.

Chakrabarty, D.K. Solid State Chemistry, New Age, 2010.

Kingery, W. D., Bowen H. K.; Uhlmann, D. R. Introduction to Ceramics, Wiley

Publishers, New Delhi, 1976.

58

CH5GET02 INDUSTRIAL CHEMISTRY

Module 1: Industrial Gases and Inorganic Chemicals (12 hours)

Industrial Gases: Large scale production, uses, storage and hazards in handling of the

following gases: oxygen, nitrogen, argon, neon, helium, hydrogen, acetylene, carbon

monoxide, chlorine, fluorine, sulphur dioxide and phosgene.

Inorganic Chemicals: Manufacture, applications, analysis and hazards in handling the

following chemicals: hydrochloric acid, nitric acid, sulphuric acid, caustic soda, common

salt,

borax, bleaching powder, sodium thiosulphate, hydrogen peroxide, potash alum, chrome

alum, potassium dichromate and potassium permanganate.

Module 2: Industrial Metallurgy - General Principles of Metallurgy (8 hours)

Chief modes of occurrence of metals based on standard electrode potentials. Ellingham

diagrams for reduction of metal oxides using carbon as reducing agent.

Hydrometallurgy, Methods of purification of metals (Al, Pb, Ti, Fe, Cu, Ni, Zn): electrolytic,

oxidative refining, Kroll process, Parting process, van Arkel-de Boer process and Mond’s

process.

Preparation of metals (ferrous and nonferrous) and ultrapure metals for semiconductor

technology.

Module 3: Silicate Industries (10 hours)

Glass: Glassy state and its properties, classification (silicate and non-silicate glasses).

Manufacture and processing of glass. Composition and properties of the following types of

glasses: Soda lime glass, lead glass, armoured glass, safety glass, borosilicate glass,

fluorosilicate, coloured glass, photosensitive glass.

Ceramics: Brief introduction to types of ceramics. Superconducting and semiconducting

oxides, fullerenes, carbon nanotubes and carbon fibre.

Cements: Manufacture of cement and the setting process, quick setting cements.

Module 4: Fertilizers (6 hours)

Different types of fertilizers (N, P and K). Manufacture of the following fertilizers: Urea,

ammonium nitrate, calcium ammonium nitrate, ammonium phosphates, superphosphate of

lime.

Module 5: Surface Coatings (8

hours)

Brief introduction to and classification of surface coatings. Paints and pigments -

formulation,

composition and related properties. Fillers, Thinners, Enamels, emulsifying agents. Special

59

paints (Heat retardant, Fire retardant, Eco-friendly paint, Plastic paint), Dyes, Wax polishing,

Water and Oil paints, Metallic coatings (electrolytic and electrodeless), metal spraying and

anodizing.

Module 6: Batteries (4 hours)

Working of the following batteries: Pb acid, Li-Battery, Solid state electrolyte battery. Fuel

cells, Solar cell and polymer cell.

Module 7: Catalysis (6hours)

General principles and properties of catalysts, homogenous catalysis (catalytic steps and

examples) and heterogenous catalysis (catalytic steps and examples) and their industrial

applications. Deactivation or regeneration of catalysts.

Application of zeolites as catalysts.

Reference Books:

Stocchi,E. Industrial Chemistry, Vol-I, Ellis Horwood Ltd., 1990.

Felder,R.M.; Rousseau,R.W.; Bullard L.G. Elementary Principles of Chemical Processes,

4th ed.,Wiley, New York, 2015.

Dara,S. S. A Textbook of Engineering Chemistry, S. Chand & Company Ltd. New

Delhi.

• Kingery, W. D., Bowen H. K.; Uhlmann, D. R. Introduction to Ceramics, 2nd ed., Wiley

New York, 1976.

• Kent, J. A. (ed) Riegel’s Handbook of Industrial Chemistry, 9th Ed., CBS Publishers, New

Delhi, 1997

• Jain, P. C.; Jain, M. Engineering Chemistry, Dhanpat Rai & Sons, Delhi 2005

• Gopalan, R., Venkappayya, D.; Nagarajan, S. Engineering Chemistry, Vikas

Publications, New Delhi, 2004.

• Sharma, B. K. Engineering Chemistry, Goel Publishing House, Meerut, 2006

60

CH5GET03 GREEN CHEMISTRY

Module 1: Introduction to Green Chemistry (4 hours)

What is Green Chemistry? Need for Green Chemistry. Goals of Green Chemistry.

Limitations/ Obstacles in the pursuit of the goals of Green Chemistry.

Module 2: Principles of Green Chemistry and Designing a Chemical Synthesis (24

hours)

Twelve principles of Green Chemistry with their explanations and examples and special

emphasis on the following:

Designing a Green Synthesis using these principles; Prevention of Waste/ byproducts;

maximum incorporation of the materials used in the process into the final products, Atom

Economy, calculation of atom economy of the rearrangement, addition, substitution and

elimination reactions.

Prevention/ minimization of hazardous/ toxic products reducing toxicity.

risk = (function) hazard × exposure; waste or pollution prevention hierarchy.

Green solvents– supercritical fluids, water as a solvent for organic reactions, ionic

liquids, fluorous biphasic solvent, PEG, solventless processes, immobilized solvents

and how to compare greenness of solvents.

Energy requirements for reactions – alternative sources of energy: use of microwaves

and ultrasonic energy.

Selection of starting materials; avoidance of unnecessary derivatization – careful use

of blocking/protecting groups.

Use of catalytic reagents (wherever possible) in preference to stoichiometric reagents;

catalysis and green chemistry, comparison of heterogeneous and homogeneous catalysis,

biocatalysis, asymmetric catalysis and photocatalysis.

Prevention of chemical accidents designing greener processes, inherent safer design,

principle of ISD “What you don’t have cannot harm you”, greener alternative to Bhopal Gas

Tragedy (safer route to carbaryl) and Flixiborough accident (saferroute to cyclohexanol)

subdivision of ISD, minimization, simplification, substitution, moderation and limitation.

Strengthening/ development of analytical techniques to prevent and minimize the

generation of hazardous substances in chemical processes.

Module 3: Examples of Green Synthesis/ Reactions and Some Real World Cases

(16 hours)

1. Green Synthesis of the following compounds: adipic acid, catechol, disodium

iminodiacetate (alternative to Strecker synthesis)

2. Microwave assisted reactions in water: Hofmann Elimination, methyl benzoate to benzoic

61

acid, oxidation of toluene and alcohols; microwave assisted reactions in organic solvents

Diels-Alder reaction and Decarboxylation reaction

3. Ultrasound assisted reactions: sonochemical Simmons-Smith Reaction (Ultrasonic

alternative to Iodine)

4. Surfactants for carbon dioxide – replacing smog producing and ozone depleting

solvents with CO2 for precision cleaning and dry cleaning of garments.

5. Designing of Environmentally safe marine antifoulant.

6. Rightfit pigment: synthetic azopigments to replace toxic organic and inorganic

pigments.

7. An efficient, green synthesis of a compostable and widely applicable plastic (poly

lactic acid) made from corn.

8. Healthier fats and oil by Green Chemistry: Enzymatic interesterification for

production of no Trans-Fats and Oils

9. Development of Fully Recyclable Carpet: Cradle to Cradle Carpeting

Module 4: Future Trends in Green Chemistry 10 hours)

Oxidation reagents and catalysts; Biomimetic, multifunctional reagents; Combinatorial green

chemistry; Proliferation of solventless reactions; co crystal controlled solid state synthesis

(C2S3); Green chemistry in sustainable development.

Reference Books:

Anastas, P.T.; Warner, J.C.: Green Chemistry - Theory and Practical, Oxford

University Press, New York, 1998.

Matlack, A.S. Introduction to Green Chemistry, Marcel Dekker, 2001.

Cann, M.C.; Connely, M.E. Real-World Cases in Green Chemistry, American

Chemical Society, Washington DC, 2000.

Ryan, M.A.;Tinnesand, M. Introduction to Green Chemistry, American Chemical

Society, Washington DC, 2002.

Lancaster, M. Green Chemistry: An Introductory Text, RSC Publishing, 2nd Edition,

2010.

Ahluwalia, V.K. Kidwai, M.R. New Trends in Green Chemistry, Ananmaya Publishers,

New Delhi, 2005.

Ahluwalia,V.K. Green Chemistry - Environmentally Benign Reaction, Ane Books, New

Delhi, 2006.

Ahluwalia,V.K. Green Chemistry - Greener Alternatives to Synthetic Organic

Transformations, Narosa Publishing, New Delhi, 2011.

Kumar, V. An Introduction to Green Chemistry, Vishal Publishing Co. Jalandhar, 2007.

62

SEMESTER VI

CH6CRT09 COORDINATION CHEMISTRY AND ORGANOMETALLICS

Credit-3 54 hours

Module 1: Coordination Chemistry (18 hrs)

Introduction - Types of ligands – Anionic, cationic and neutral – IUPAC Nomenclature -

Structural and stereo isomerism in coordination compounds. Chelates and chelate effect-

Stability of complexes: Inert and labile complexes - Factors influencing stability. Stepwise

stability constant and overall stability constant. Review of Werner’s theory and Sidgwick’s

concept of coordination – EAN rule. Bonding theories: Valence bond theory - Geometries of

coordination numbers 4 and 6 – Inner orbital and outer orbital complexes- Limitations of

VBT. Crystal filed theory - Splitting of d-orbitals in octahedral, tetrahedral, tetragonal and

square planar complexes - Jahn Teller Effect– Factors affecting crystal field splitting - CFSE

of low spin and high spin octahedral complexes. Spectrochemical series - Explanation of

geometry, magnetism and spectral properties - Merits and demerits of Crystal field theory.

Molecular orbital theory – evidence for metal ligand covalency- MO diagram for octahedral

complexes (with sigma bonds only). Spectral and magnetic properties of complexes –

electronic absorption spectrum of [Ti(H2O)6]2+. Calculation of magnetic moments – spin only

formula. Application of coordination chemistry in qualitative and quantitative analysis of

metal ions such as Cu2+, Zn2+, Ni2+ and Mg2+.

Module 2: Organometallic Compounds (6 hrs)

Definition – Classification based on the nature of metal-carbon bond and on the basis of

hapticity. Naming of organometallic compounds. The 18- electron rule and stability –

Ferrocene: Preparation, properties and bonding (VBT only). Metal-alkene complexes- –

Zeise’s salt. Catalytic properties of organometallic compounds - Zeigler Natta catalyst in the

polymerization of alkene and Wilkinson catalyst in the hydrogenation of alkene (mechanism

not expected).

Module 3: Metal Carbonyls and Metal clusters (6 hrs)

Preparation and properties of mononuclear carbonyls - Structures of Mo(CO)6, Fe(CO)5 and

Ni(CO)4. Polynuclear carbonyls, bridged carbonyls and bonding in carbonyls – Mn2(CO)10

and Fe2(CO)9. EAN of metals in metal carbonys – indication of metal-metal bonding. Metal

clusters - carbonyl and halide clusters - Quadruple bond – structure of Re2CI82-.

63

Module 4: Bioinorganic Chemistry (9 hrs)

Essential and trace elements in biological systems – Structure and functions of Haemoglobin

and myoglobin - Mechanism of oxygen transport, cooperativity, Bohr effect. Vitamin B12

(structure not expected). Electron carriers – cytochromes. Chlorophyll and photosynthesis.

Role of alkali and alkaline earth metals in biological systems, Na/K pump. Importance of Ca and

Mg. Biological functions and toxicity of metals – Fe, Cu, Zn, Cr, Mn, Ni, Co, Cd, Hg and Pb.

Metalloenzymes of zinc, manganese and copper, nitrogenase. Treatment of metal toxicity by

chelation therapy. Anti cancer drugs – cisplatin and carboplatin.

Module 5: Metallurgy (6hrs)

Occurrence of metals based on standard electrode potential – methods of concentration of

ores- reduction to free metal – electrometallurgy and hydrometallurgy. Refining of metals-

electrolytic, vapour phase, oxidative and zone refining. Thermodynamics of the oxidation of

metals to metal oxide – Ellingham diagram.

Module 6: Industrially important materials (9 hrs)

Refractory materials - carbides, nitrides, borides. Graphite and graphite oxide, intercalation

compounds of alkali metals, carbon monofluoride, intercalation compounds of graphite with

metal halides, glass, silicates, zeolites, ultramarines and ceramics.

Nanomaterials – synthesis – chemical precipitation, mechano-chemical method, micro

emulsion method, reduction technique, chemical vapour deposition and sol-gel method (brief

study). Properties and applications of fullerenes, carbon nanotubes and graphenes.

References

1. F.A. Cotton and G. Wilkinson, Advanced Inorganic Chemistry, 6th Edition, Wiley

India Pvt. Ltd., New Delhi, 2009 (Reprint).

2. J.E. Huheey, E.A. Keitler and R.L. Keitler, Inorganic Chemistry – Principles of

Structure and Reactivity, 4th Edition, Pearson Education, New Delhi, 2013.

3. D.F. Shriver and P. Atkins, Inorganic Chemistry, 5th Edition, Oxford University

Press, New York, 2010.

4. B.R. Puri, L.R. Sharma and K.C. Kalia, Principles of Inorganic Chemistry, 31st

Edition,

Milestone Publishers and Distributors, New Delhi, 2013.

5. P.L. Soni and Mohan Katyal, Textbook of Inorganic Chemistry, 20th Edition, S.

Chand and Sons, New Delhi, 2013.

6. Satya Prakash, Advanced Inorganic Chemistry, Volume 2, S. Chand and Sons, New

Delhi, 2005.

7. J.D. Lee, Concise Inorganic Chemistry, 5th Edition, Oxford University Press, New

Delhi 2008.

8. R. Gopalan and V. Ramalingam, Concise Coordination Chemistry, 1st Edition, Vikas

Publishing House, New Delhi, 2001.

64

9. Wahid U. Malik, G D. Tuli and R.D. Madan, Selected Topics in Inorganic Chemistry,

S. Chand and Co., New Delhi, 2010 (Reprint).

10. V. S. Muraleedharan and A. Subramania, Nanosciece and nanotechnology, Ane

Books Pvt. Ltd. New Delhi, 2009

11. T. Pradeep, Nano; The Essentials, Mc Graw-Hill education, New Delhi, 2006.

65

Semester VI

CH6CRT10 Advanced Organic Chemistry – II

Credit-3 54 hours

Module 1: Natural Products (6 hours)

Terpenoids

Terpenoids – Classification. Isoprene rule. Structure elucidation and uses of citral and

geraniol. Natural rubber - structure, latex processing methods, vulcanisation, rubber

compounding, mastication and uses.

Alkaloids

Alkaloids - General methods of isolation. Classification. Physiological action and medicinal

importance. Structure elucidation of coniine, nicotine and piperine.

Module 2: Vitamins, Steroids and Hormones (6 hours)

Vitamins

Vitamins – Classification. Structure, biological functions and deficiency diseases of vitamins

A, B1, B2, B3, B5, B6 and C.

Steroids

Steroids – Introduction. Diels’ hydrocarbon. Structure and functions of cholesterol.

Elementary idea of HDL and LDL. Vitamin D - structure, biological functions and deficiency

diseases.

Hormones

Hormones – Introduction. Steroid hormones, peptide hormones and amine hormones

(example, endocrine gland and biological functions; structure not required). Artificial

hormones.

Module 3: Carbohydrates (12 hours)

Classification of carbohydrates. Reducing and non-reducing sugars.

General Properties of Glucose and Fructose, their open chain structure. Epimers,

mutarotation and anomers. Determination of configuration of Glucose (Fischer proof). Cyclic

structure of glucose. Haworth projections. Cyclic structure of fructose. Chain lengthening and

chain shortening of aldoses - Kiliani-Fischer synthesis and Wohl degradation.

Interconversion of aldoses and ketoses.

Linkage between monosaccharides. Structure of disaccharides (sucrose, maltose, cellobiose).

Reactions and uses of sucrose. Artificial sugars (sweeteners) – sucralose.

66

Structure of the polysaccharides starch and cellulose (excluding their structure elucidation).

Industrial applications of cellulose.

Module 4: Amino Acids, Peptides and Proteins (8 hours)

Classification of amino acids. Synthesis, ionic properties and reactions of α-amino acids.

Zwitterion structure and Isoelectric point.

Polypeptides. Synthesis of simple peptides (upto tripeptides) by N-protecting

(benzyloxycarbonyl and t-butyloxycarbonyl) & C-activating groups. DCC method.

Merrifield’s solid phase peptide synthesis.

Classification of proteins. Overview of Primary, Secondary, Tertiary and Quaternary

structure of proteins. Determination of primary structure of proteins. Determination of N-

terminal amino acid (by FDNB and Edman method) and C–terminal amino acid (by

hydrazinolysis and with carboxypeptidase enzyme). Helical and sheet structures.

Denaturation of proteins.

Module 5: Nucleic Acids (4 hours)

Components of Nucleic acids: Adenine, guanine, cytosine, thymine and uracil (structure

only), other components of nucleic acids. Nucleosides and nucleotides (nomenclature),

Structure of polynucleotides; Structure of DNA (Watson - Crick Model) and RNA.

Biological functions of DNA and RNA - Replication and protein biosynthesis. Transcription

and Translation. Genetic code.

Module 6: Enzymes (4 hours)

Introduction, classification and characteristics of enzymes. Salient features of active site of

enzymes.

Mechanism of enzyme action, factors affecting enzyme action, Coenzymes and cofactors and

their role in biological reactions, Specificity of enzyme action (including stereospecificity),

Enzyme inhibitors and their importance, phenomenon of inhibition (Competitive and

Noncompetitive inhibition including allosteric inhibition).

Module 7: Lipids (4 hours)

Introduction to lipids. Classification.

Oils and fats: Extraction and refining. Common fatty acids present in oils and fats. Omega

fatty acids. Trans fats and their effect. Hydrogenation, Rancidity. Acid value, Saponification

value, Iodine value and RM value.

Biological importance of waxes, phospholipids and glycolipids.

67

Soaps. Cleaning action of soaps. Synthetic detergents. Environmental aspects. ABS and LAS

detergents.

Module 8: Polymers (6 hours)

Introduction and classification.

Polymerisation reactions - Addition and condensation - Mechanism of cationic, anionic and

free radical addition polymerization; Metallocene-based Ziegler-Natta polymerisation of

alkenes.

Preparation and applications of plastics – thermosetting (Phenol-formaldehyde,

Polyurethanes) and thermosoftening (Polythene, PVC); Fibres – natural and synthetic

(acrylic, polyamide, polyester); Synthetic rubbers – SBR, Nitrile rubber and Neoprene.

Introduction to conducting polymers with examples.

Environmental hazards and biodegradability of polymers. Recycling of plastics.

Module 9 : Supramolecular Chemistry (4 hours)

Introduction. Molecular recognition. Host-guest interactions. Types of non-covalent

interactions and molecular receptors. Role of molecular recognition in biopolymer (DNA and

protein) structure organisation.

Reference Books:

1. Finar, I. L. Organic Chemistry (Volume 2), Dorling Kindersley (India) Pvt. Ltd.




3. Nelson, D. L. & Cox, M. M. Lehninger’s Principles of Biochemistry, 7th ed.,W. H.

Freeman.

4. Berg, J.M., Tymoczko, J.L. & Stryer, L. Biochemistry, W.H. Freeman, 2002.

5. Bhat S.V., Nagasampagi, B.A. & Sivakumar M. Chemistry of Natural Products,

Narosa, 2005.



8. Tewari, K.S. & Vishnoi, N.K. Organic Chemistry, Vikas Publishing House, 2012.

9. Billmeyer, F.W. Textbook of Polymer Science, Wiley.

10. Gowariker, V.R., Viswanathan, N.V. & Sreedhar J. Polymer Science, 2nd ed., New

Age, 2015

11. Steed, J. W. & Atwood, J.L. Supramolecular Chemistry, 2nd ed., Wiley, 2009.

12. Dodziuk, H. Introduction to Supramolecular Chemistry, Springer, 2002.

68

CH6CRT11 Thermodynamics and Chemical Kinetics

Credits – 3 (54 hours)

Aim

To provide an insight into the thermodynamic and kinetic aspects of chemical reactions

and phase equilibria.

Objectives

To study the laws of thermodynamics

To derive Gibbs-Helmholtz, Clausius-Clapeyron, Gibbs-Duhem equations

To derive the relation between Kp, Kc and Kx

To derive the phase rule

To derive the rate equations for zero, first and second order reactions

To study the phase diagrams of one and two component systems

To understand the theories of chemical kinetics

To get an elementary idea of catalysis including enzyme catalysis.

Module 1: Thermodynamics-I (15 Hours)

Basic concepts- system, surroundings, types of systems. Extensive and intensive properties,

macroscopic properties. State functions and path functions. Types of Processes, Zeroth law of

thermodynamics. Definition of internal energy and enthalpy. Heat capacities at constant volume (Cv)

and at constant pressure (Cp), relationship between Cp and Cv.

First law of thermodynamics –Mathematical statement of first law. Reversible process and

maximum work. Calculation of work, heat, internal energy change and enthalpy change for the

expansion of an ideal gas under reversible isothermal and adiabatic condition.

The Joule-Thomson effect – derivation of the expression for Joule-Thomson coefficient. Sign

and magnitude of Joule-Thomson coefficient, inversion temperature.

Thermochemistry – standard states. Enthalpies of formation, combustion and neutralization.

Integral and differential enthalpies of solution. Hess’s law and its applications. Kirchoff’s equation.

Module 2: Thermodynamics-II (12 Hours)

Second law: Limitations of first law –Different statements of IInd law, Thermodynamic scale

of temperature. Carnot cycle and its efficiency, Carnot theorem.

Concept of entropy – Definition and physical significance. Entropy as a function of volume

and temperature, Entropy as a function of pressure and temperature. Entropy as a criteria of

spontaneity and equilibrium.

Gibbs and Helmholtz free energies and their significances- criteria of equilibrium and

spontaneity. Gibbs-Helmholtz equation, dependence of Gibbs free energy change on temperature,

69

volume and pressure. Partial molar quantities – Chemical potential – Gibbs–Duhem

equation. Concept of fugacity.

Module 3: Chemical Equilibria (6 Hours)

Law of mass action-equilibrium constant – Relation between Kp, Kc and Kx –

Thermodynamic treatment of the law of mass action – Vant Hoff reaction isotherm –Temperature

dependence of the equilibrium constant – The Van'tHoffs equation –Pressure dependence of the

equilibrium constant Kp.

Module 4: Phase equilibria (9 Hours)

The phase rule, equilibrium between phases – conditions. One component system – water

system, sulphur system. Two component systems – solid-liquid equilibrium – Simple Eutectic, Lead-

Silver system, Formation of compounds with Congruent Melting Point; Ferric chloride–Water system,

Formation of compounds with Incongruent Melting Point Sodium sulphate–Water system. Three

component systems having one partially miscible pair – Acetic acid–Water–Chloroform system.

.

Moduel 5:Chemical Kinetics (12 Hours)

Rate of reaction, rate equation, order and molecularity of reactions, Integrated rate

expressions for first and second order reactions. Zero order reactions, pseudo order reactions, half life.

Theories of chemical kinetics: Effect of temperature on the rate of reaction: Arrhenius

equation, concept of activation energy, Collision theory, Transition state theory. Thermodynamic

parameters for activation – Eyring equation (no derivation needed), enthalpy and entropy of

activation. Theory of unimolecular reactions – Lindemann Theory.

Kinetics of complex (composite) reactions: Opposing reactions, consecutive reactions, and

parallel (simultaneous) reactions. Chain reactions – steady state treatment, Hydrogen– Bromine

reaction.

Catalysis: Homogeneous catalysis, enzyme catalysis – Michaelis–Menten equation (no

derivation needed). Heterogeneous catalysis – Surface catalysis, Elementary idea about Autocatalysis.

References

1. R. P. Rastogi, R. R. Misra, An Introduction to Chemical Thermodynamics, 6th edn., Vikas

Pub. Pvt. Ltd. (2003).

2. P. Atkins and J Paula, The elements of Physical chemistry, 7th edn., Oxford University Press.

3. K.K. Sharma, L.K. Sharma, A Textbook of Physical Chemistry, 4th edn, Vikas publishing

House.

4. B. R. Puri, L. R. Sharma, M. S. Pathania, Elements of Physical chemistry, Vishal Pub. Co.

Jalandhar

5. J. Rajaram and J. C. Kuriakose, Thermodynamics, Shoban Lal Nagin Chand & Co (1986).

6. D. A. McQuarrie, J. D. Simon, Physical Chemistry – A molecular Approach, Viva Books Pvt.

Ltd.

7. F. A. Alberty and R. J .Silby, Physical Chemistry, John Wiley.

8. G. M. Barrow, Physical Chemistry, 5th edn., Tata McGraw Hill.

9. G. K. Vemulapalli, Physical Chemistry, Prentice-Hall of India Pvt. Ltd.

10. G. W. Castellan, Physical Chemistry, 3rd edn.,Narosa Publishing House, New Delhi,(2004).

70

11. F Daniels and R A Alberty, Physical Chemistry, Wiley Eastern.

12. R. Stephen Berry, Stuart A. Rice, John Ross, Physical Chemistry, 2nd edition, Oxford.

13. Gurdeep Raj, Advanced Physical Chemistry, Goel Publishing House.

14. S. Glasstone, Thermodynamics for Chemists, Affiliated East West Publishers.

15. G.S. Rush Brooke, Statistical Mechanics, Oxford University Press.

16. T.L. Hill, Introduction to Statistical Thermodynamics, Addison Wesley.

17. K. L. Kapoor, A Textbook of Physical chemistry, Volumes 3, Macmillan India Ltd.

18. B. R. Puri, L. R. Sharma, M. S. Pathania, Elements of Physical chemistry, Vishal Pub.

19. Gurdeep Raj, Chemical Kinetics, Krishna’s Educational Publishers (2014).

20. K. J. Laidler, Chemical kinetics, 3rd edn, Pearson education, 2004.

21. J Rajaram and J C Kuriakose, Kinetics and Mechanisms of Chemical Transformations,

Macmillan, 2006.

71

CH6CRT12 SOLUTION CHEMISTRY

Credits - 3 (54 hours)

Aim

To provide an insight into the characteristics of different types of solutions and

electrochemical phenomena.

Objectives

To study the behaviour of binary liquid mixtures, CST, azeotropes, colligative properties

To study solubility of gases in liquids,

To study ionic equilibria and electrical properties of ions in solution.

To study the concepts of acids and bases, pH and buffer solutions

Module 1:Solutions (12 Hours)

Introduction – Binary liquid solutions – Raoult’s law- ideal and non-ideal solutions – ∆Gmix,

∆Vmix, and ∆Smix for ideal solutions. Vapour pressure – composition and temperature –composition

curves of ideal and non-ideal binary liquid solutions. Fractional distillation of binary liquid-liquid

solutions – distillation of immiscible liquids, partially miscible liquid-liquid systems. Critical solution

temperature (CST).

Solubility of gases in liquids – Henry’s law. Distribution of a solute between two solvents–

Nernst distribution law.

Colligative properties of dilute solutions – vapour pressure lowering, Boiling point elevation

and freezing point depression (thermodynamic derivation). Molar mass determination-related

problems – Osmotic pressure –laws of osmotic pressure – Reverse osmosis – purification of sea

water. Abnormal molecular masses – van’t Hoff factor – Degree of association and Degree of

dissociation.

Module 2:Ionic Equilibria (9 hours)

Introduction – Concepts of acids and bases, relative strength of acid-base pairs, influence of

solvents, Dissociation constants – acids, bases, and polyprotic acids. Ostwald’s dilution law.

Degree of ionization, factors affecting degree of ionization, ionization constant and ionic

product of water- pH. Effects of solvents on ionic strength, Levelling effect.

Buffer solutions – Mechanism of buffer action, Henderson equation. Hydrolysis of salts –

degree of hydrolysis and hydrolysis constant, determination of degree of hydrolysis, pH of salt

solutions.

Solubility and solubility product of sparingly soluble salts – Applications of solubility product

principle.

72

Module 3: Electrical Conductance (15 Hours)

Introduction- Faraday’s laws of electrolysis, electrochemical equivalent & chemical

equivalent. Electrolytic conductivity, molar conductivity – Variation of molar conductivity with

concentration. Kohlrausch’s law – Applications.

Ionic mobility – relation with ion conductivity, influence of temperature on ion conductivity,

ion conductivity and viscosity – Walden’s rule. Abnormal ion conductivity of hydrogen and hydroxyl

ions.

Transference number and its experimental determination using Hittorf and Moving boundary

methods.

Debye-Hückel theory of strong electrolytes – the concept of ionic atmosphere, Asymmetry

and electrophoretic effect, Debye- Hückel-Onsager equation (no derivation). Activity, mean ionic

activity and mean ionic activity coefficients of electrolytes. Ionic strength of a solution, Debye-

Hückel limiting law (no derivation).

Applications of conductance measurements – Determinations of degree of dissociation of

weak electrolytes, conductometric titrations involving strong acid- strong base, strong acid-weak base,

weak acid- strong base, weak acid–weak base and precipitation titrations.

Module 4: Electromotive force (18 Hours)

Introduction – Electrochemical cells and electrolytic cells, Galvanic cells, characteristics of

reversible cells. Reversible electrodes – Different types, Reference electrodes – Standard Hydrogen

Electrode, Calomel electrode, Electrode potential – Electrochemical series. Representation of cells,

Electrode reactions and cell reactions Derivation of Nernst equation for electrode potential and cell

potential, Gibb’s Helmholtz equation and EMF of a cell, calculation of ∆G, ∆H and ∆S from EMF

data. Calculation of equilibrium constant from EMF data.

Concentration cells – Electrode concentration cell and electrolyte concentration cells. Types

of electrolyte concentration cells – with transference and without transference, liquid junction

potential and salt bridge. Fuel cells – the hydrogen-oxygen fuel cell.

Applications of emf measurements – determination of solubility product, determination of pH

using hydrogen electrode, quinhydrone electrode and glass electrode.

Potentiometric titrations of acid-base and redox reaction, oxidation reduction indicators.

Irreversible electrode processes – overvoltage and electrode polarisation- Hydrogen and Oxygen

overvoltage (Theories not required). Principle of polarography.

Corrosion of metals – forms of corrosion, corrosion monitoring and prevention methods.

References

1. B. R. Puri, L. R. Sharma, M. S. Pathania, Elements of Physical chemistry, VishalPub. Co.

Jalandhar.

2. K. L. Kapoor, A Textbook of Physical chemistry, Volume 4, Macmillan India Ltd.

3. Barrow, G.M. Physical Chemistry, Tata McGraw‐Hill (2007).

4. Castellan, G.W. Physical Chemistry,4th Ed. Narosa (2004).

5. Kotz, J.C., Treichel, P.M. & Townsend, J.R., General Chemistry, Cengage Learning India

Pvt. Ltd. New Delhi (2009).

6. Mahan, B.H. University Chemistry, 3rd Ed. Narosa (1998).

73

7. K. L. Kapoor, A Textbook of Physical chemistry, Volumes 1, Macmillan India Ltd,

8. Glasstone S, An Introduction to Electrochemistry, East-West Press (Pvt.) Ltd. (2006).

9. Gurdeep Raj, Advanced Physical Chemistry, Goel publishing house.

10. Glasstone and Lewis, Elements of Physical Chemistry, Macmillan

11. K. L. Kapoor, A Textbook of Physical chemistry, Volumes 3, Macmillan India Ltd.

12. I.N. Levine, Physical Chemistry, Tata Mc Graw Hill

13. F A Alberty and R J Silby, Physical Chemistry, John Wiley.

14. P. W. Atkins, The elements of Physical chemistry, 8th edn, Oxford University Press.

15. D. A. McQuarrie, J. D. Simon, Physical Chemistry – A molecular Approach, Viva Books Pvt.

Ltd.

16. S. H. Marron and J. B. Lando, Fundamentals of Physical Chemistry, Macmillan Ltd.

17. G. K. Vemulapalli, Physical Chemistry, Prentice-Hall of India Pvt. Ltd. (1997)

74

Semester VI

Choice Based Courses

(Chose any one of the following three)

Credits-3 54 hours

CH6CBT01 POLYMER CHEMISTRY

Module 1: Introduction and History of Polymeric Materials (4 hours)

History of Polymers - Terminology. Different schemes of classification of polymers, Polymer

nomenclature, Molecular forces and chemical bonding in polymers. Texture of polymers.

Module 2: Functionality and Its Importance (4 hours)

Classification of polymerization processes. Criteria for polymer formation. Relationships

between functionality, extent of reaction and degree of polymerization. Bifunctional systems,

Poly-functional systems.

Module 3: Mechanism and Kinetics of Polymerization (6 hours)

Mechanism and kinetics of step growth, radical chain growth, ionic chain (both cationic and

anionic) and coordination polymerizations. Mechanism and kinetics of copolymerization.

Mechanism of ring opening and group transfer polymerisations.

Module 4: Polymerisation Techniques (4 hours)

Polymerisation techniques: Bulk, solution, suspension and emulsion polymerisations. Melt,

solution and interfacial polycondensation techniques.

Module 5: Physical Properties of Polymers (12 hours)

Structure-Property relationships of polymers.

Crystallization and Crystallinity :Determination of crystalline melting point and degree of

crystallinity, Morphology of crystalline polymers, Factors affecting crystalline melting point.

Molecular weight of polymers :Determination of Molecular Weight of Polymers(Mn, Mw,

etc) by end group analysis, viscometry, light scattering and osmotic pressure methods.

Molecular weight distribution and its significance. Polydispersity index.

75

Glass Transition Temperature (Tg): Definition. Factors influencing glass transition

temperature (Tg). Tg and molecular weight. Tg and melting point. Importance of

Tg.Determination of Tg-Dialatometric method.

Module 6: Reactions of Polymers (4 hours)

Hydrolysis, hydrogenation, addition, substitution, crosslinking, vulcanisation and cyclisation

reactions.

Module 7: Polymer Degradation (4 hours)

Types of degradation. Thermal, mechanical, photo and oxidative degradations of polymers.

Module 8 : Polymer Processing (4 hours)

Polymer processing techniques: Compression moulding, Injection moulding, Blow moulding,

Extrusion moulding, Thermoforming, Die casting, Film casting, Rotational casting,

Calendering and Spinning.

Module 9: Chemistry of Commercial Polymers (8 hours)

Brief introduction to preparation, structure, properties and applications of the following

polymers: polyolefins, poly(vinyl chloride) and related polymers, polystyrene and styrene

copolymers, poly(vinyl acetate) and related polymers, acrylic polymers, fluoro polymers,

polyamides (aliphatic and aromatic) and related polymers. Formaldehyde resins (PF, UF and

MF), polyurethanes, polycarbonates, epoxy resins.

Module 10 : Specialty Polymers (4 hours)

High temperature resistant and flame retardant polymers. Biomedical applications of

polymers. Controlled drug delivery systems.

Conducting polymers [polyacetylene, polyaniline, poly(p-phenylene sulphide), polypyrrole,

polythiophene]. Conduction mechanism and applications.

Reference Books:

Carraher, C.E. Seymour/Carraher’sPolymer Chemistry, 6th ed.,Marcel Dekker,

New York, 2003.

Odian, G. Principles of Polymerization, 4th ed. Wiley, 2004.

Billmeyer, F.W. Textbook of Polymer Science, 3rd ed. Wiley-Blackwell,1984.

Gowariker, V.R., Viswanathan, N.V.; Sreedhar J. Polymer Science, 2nd ed., New Age,

2015.

Ghosh, P. Polymer Science & Technology, 2nd ed., Tata McGraw-Hill, New Delhi, 2002.

Lenz, R.W. Organic Chemistry of Synthetic High Polymers. Interscience Publishers, New

York, 1967.

76

CH6CBT02 INSTRUMENTAL METHODS OF

CHEMICAL ANALYSIS

Module 1 : Introduction to Spectroscopic Methods of Analysis (4 hours)

Recap of the spectroscopic methods covered in detail in the core chemistry syllabus:

Treatment of analytical data, including error analysis. Classification of analytical methods

and the types of instrumental methods. Consideration of electromagnetic radiation.

Module 2 : Molecular Spectroscopy ( 18 hours)

Infrared spectroscopy:

Interactions with molecules: absorption and scattering. Means of excitation (light sources),

interpretation of spectrum (qualitative, mixtures, resolution), Advantages of Fourier

Transform (FTIR). Samples and results expected. Applications: Issues of quality assurance

and quality control. Special problems for portable instrumentation and rapid detection.

UV-Visible/ Near IR spectroscopy: Emission, absorption, fluorescence and photoacoustic.

Excitation sources (lasers, time resolution), wavelength dispersion (gratings, prisms,

interference filters, laser, placement of sample relative to dispersion, resolution). Detection of

signal (photocells, photomultipliers, diode arrays, sensitivity and S/N). Single and Double

Beam instruments. Interpretation (quantification, mixtures, absorption vs. fluorescence and

the use of time, photoacoustic, fluorescent tags).

NMR spectroscopy: Principle, Instrumentation, Factors affecting chemical shift, Spin coupling.

Applications.

Module 3 : Separation Techniques (16 hours)

Chromatography: Gas chromatography, liquid chromatography, supercritical fluids.

Importance of column technology (packing, capillaries). Separation based on increasing

number of factors (volatility, solubility, interactions with stationary phase, size, electrical

field). Detection: simple vs. specific (gas and liquid). Detection as a means of further analysis

(use of tags and coupling to IR and MS). Electrophoresis (plates and capillary) and use with

DNA analysis.

Immunoassays and DNA techniques

Mass spectrometry: Making the gaseous molecule into an ion (electron impact, chemical

ionization). Making liquids and solids into ions (electrospray, electrical discharge, laser

desorption, fast atom bombardment). Separation of ions on basis of mass to charge ratio,

Magnetic, Time of flight, Electric quadrupole. Resolution, time and multiple separations.

Detection and interpretation (how this is linked to excitation).

77

Module 4 : Elemental Analysis (8 hours)

Atomic spectroscopy: Atomic absorption, Atomic emission, and Atomic fluorescence.

Excitation and getting sample into gas phase (flames, electrical discharges, plasmas).

Wavelength separation and resolution (dependence on technique). Detection of radiation

(simultaneous scanning, signal noise). Interpretation (errors due to molecular and ionic

species, matrix effects, other interferences).

Module 5: Electroanalytical Methods (4 hours)

Principles and applications of potentiometry, voltammetry and polarography.

Module 6: X-ray Analysis and Electron Spectroscopy (Surface Analysis) (4 hours)

Principles of XRD, SEM, TEM and STM.

Reference Books:

Skoog,D. A.; Holler,F. J.; Crouch, S.R. Principles of Instrumental Analysis - 6th ed.,

Saunders College Publishers, 2007.

Willard, H.H.; Merritt, L.L.; Dean, J.A.; Settle, F.A. Instrumental Methods of Analysis, 7th

ed., Van Nostrand, 1974.

Christian, G.D.; O’Reilly, J.E. Instrumental Analysis, 2nd ed., Allyn and Bacon, 1986.

Atkins,P.W.; de Paula, J. Physical Chemistry, 8th ed., Oxford University Press, 2006.

Castellan,G.W.: Physical Chemistry, 3rd. ed., Narosa, New Delhi, 2004.

Banwell,C.N.; McCash, E.M.: Fundamentals of Molecular Spectroscopy,4th ed., Tata

McGraw Hill, 1994.

Moore,W.J.: Physical Chemistry, 5th ed., Orient Longman, 1998.

78

CH6CBT03 COMPUTER APPLICATIONS IN CHEMISTRY

Module 1: Basic Computer System (in brief) (4 hours)

Hardware and Software; Input devices, Storage devices, Output devices, Central Processing

Unit (Control Unit and Arithmetic Logic Unit); Number system (Binary, Octal and

Hexadecimal Operating System); Computer Codes (BCD and ASCII); Numeric/String

constants and variables. Operating Systems (DOS, WINDOWS, and Linux); Software

languages: Low level and High Level languages (Machine language, Assembly language;

QBASIC, FORTRAN and C++); Software Products (Office, Chemsketch, Scilab, Matlab,

Hyperchem, etc.), internet applications.

Module 2 :Use of Programming Language for Solving Problems in Chemistry (36

hours)

Computer Programming Language- QBASIC, (for solving some of the basic and in turn

complicated chemistry problems). QB4 version of QBASIC can be used.

Programming Language – QBASIC; Commands: INPUT and PRINT Commands;

GOTO, If, ELSEIF, THEN and END IF Commands; FOR and NEXT Commands;

Library Functions ( ABS, ASC, CHR$, EXP,INT, LOG, RND, SQR, TAB and

trigonometric Functions), DIM, READ, DATA, REM, RESTORE, DEF FNR,

GOSUB, RETURN, SCREEN, VIEW, WINDOW, LINE, CIRCLE. LOCATE, PSET

Commands.

Simple programs using above mentioned commands.

QBASIC programs for Chemistry problems - Example: plotting van der Waal

Isotherms (Simple Problem, available in general text books) and observe whether van

der Waal gas equation is valid at temperatures lower than critical temperature where

we require to solve a cubic equation and calculation of area under the curves

(Complicated Problem, not available in general text books).

Solution of quadratic equation, polynomial equations (formula, iteration and

Newton – Raphson methods, binary bisection and Regula Falsi); Numerical

differential, Numerical integration (Trapezoidal rule), Simultaneous equations,

Matrix addition and multiplication, Statistical analysis.

Module 3 : Use of Software Products (14 hours)

Computer software like Scilab, Excel, etc to solve some of the plotting or calculation

problems.

Basic idea of Molecular Modelling using software like Chemsketch, Arguslab andAccelerys

JDraw etc for geometry optimization and potential energy surface (localand global minima).

79

Reference Books:

• McQuarrie, D. A. Mathematics for Physical Chemistry, University Science Books, 2008.

• Mortimer, R. Mathematics for Physical Chemistry, 3rd ed. Elsevier, 2005.

• Steiner, E. The Chemical Maths Book, Oxford University Press, 1996.

• Yates, P. Chemical Calculations, 2nd Ed. CRC Press, 2007.

• Harris, D. C. Quantitative Chemical Analysis, 6th ed., Freeman, 2007 (Chapters 3-5).

• Levie, R. de, How to Use Excel in Analytical Chemistry and in General Scientific Data

Analysis, Cambridge Univ. Press, 2001.

• Noggle, J. H. Physical Chemistry on a Microcomputer, Little Brown & Co., 1985.

• Venit, S.M. Programming in BASIC: Problem Solving with Structure and Style. Jaico

Publishing House, Delhi, 1996.

80

Semester V and VI:

CH6CRP03 Volumetric Analysis

Credits-2 108 hours

A. Acidimetry and alkalimetry

1. Strong acid – Weak base

2. Strong base – Weak acid

3. Estimation of Na2CO3 and NaHCO3 in a mixture

4. Estimation of NaOH and Na2CO3 in a mixture

5. Estimation of ammonia in ammonium salts by direct and indirect methods

B. Complexometric Titrations using EDTA

1. Estimation of Zn

2. Estimation of Mg

3. Estimation of Mg and Ca in a mixture

4. Estimation of Ni

5. Determination of hardness of water

C. Oxidation – reduction Titrations

Permanganometry

1. Estimation of ferrous iron

2. Estimation of oxalic acid

3. Estimation of sodium oxalate

4. Estimation of calcium

Dichrometry

5. Estimation of ferrous iron using internal indicator

6. Estimation of ferrous iron using external indicator

7. Estimation of ferric iron using internal indicator

8. Estimation of ferric iron using external indicator

Iodimetry and Iodometry

9. Estimation of copper

10. Estimation of arsenious oxide

81

ORGANIC CHEMISTRY PRACTICALS – II

Crdits-2 72hours


A. Basic Laboratory Skills

1. Crystallisation – Any four compounds using ethyl acetate, ethanol, and water - Record

the yield of recovery.

2. Distillation - Purification of water and ethyl acetate-Record the yield of recovery.

3. Solvent extraction – aniline from water - methyl benzoate from water - using ether-

Record the yield of recovery. (Any two experiments shall be done).

B. Organic Preparations

I. Organic preparations involving:

1. Oxidation (benzaldehyde to benzoic acid).

2. Hydrolysis (methyl salicylate or ethyl benzoate to the acid).

3. Nitration (m-dinitrobenzene and picric acid).

4. Halogenation (p-bromoacetanilide from acetanilide).

5. Acylation (Benzoylation of aniline, phenol, β-naphthol).

6. Esterification (benzoic acid ester).

7. Iodoform from acetone or ethyl methyl ketone.

8. Side chain oxidation (benzyl chloride to benzoic acid).

9. Claisen – Schmidt reaction: Dibenzal acetone from benzaldyde.

C. Chromatography

1. TLC - Separation and identification- Determination of Rf value of o-and p- nitroanilines,

o- and p-chloroanilines, p-chlorophenol and p-nitrophenol, p-chloroaniline and p–nitroaniline,

benzil and o-nitroaniline or any two amino acids.

2. Column Chromatography – Purification of o-nitro aniline, o-nitrophenol, benzil, m- dinitro

benzene, benzene azo –β-naphthol (non–evaluative).

Reference Books:

1. Furniss, B.S.; Hannaford, A.J.; Rogers, V. Smith, P.W.G.; Tatchell, A.R. Vogel’s Textbook

of Practical Organic Chemistry, 5th ed., Pearson Education, 2005.

2. Mann,F.G.; Saunders, B.C. Practical Organic Chemistry, 4th ed., Pearson Education, 2009.

3. Ahluwalia, V.K.; Aggarwal, R. Comprehensive Practical Organic Chemistry –

Preparation and Quantitative Analysis, Universities Press, 2000.

4. Vishnoi, N.K. Advanced Practical Organic Chemistry, 3rd ed., Vikas Publishing House,

New Delhi, 2010.

82

CH6CRP05-Physical Chemistry Practical

Credits 2 (108 hrs)

1. Viscosity – percentage composition of a mixture.

2. Heat of solution – KNO3, NH4Cl

3. Heat of neutralization

4. Determination of equivalent conductance of an electrolyte

5. Conductometric titration – strong acid vs. strong base, weak acid-strong base

6. Determination of partition coefficient of non-volatile solute between two immiscible solvents.

E.g. I2 between CCl4 and water.

7. Transition temperature of salt hydrates. (Sodium thiosulphate, sodium acetate)

8. Determination of the surface tension of a liquid (Drop number method or Drop weight method)

Semester VI

1. A study of two component system simple eutectic only.

2.Critical solution temperature of phenol-water system.

3. Effect of electrolytes on the CST of phenol-water system.

4. Molecular weight determination by Rast's method. (using naphthalene, camphor or biphenyl

as solvent and acetanilide, p-dichlorobenzene etc. as solute.)

5. Kinetics of simple reactions eg. Acid hydrolysis of methyl acetate.

6. Potentiometric titration – Fe2+vs. Cr2O72–, I- vs. MnO4–

7. Data analysis of kinetic experiments using spreadsheet program (determination of rate

constant)

8. Determination of equivalence point of potentiometric and conductometric titrations using

spreadsheet program.

References

1. W. G. Palmer: ‘Experimental physical chemistry’, Cambridge University Press.

2. J.B. Yadav: Advanced Practical Physical Chemistry Goel Publishing House.

3. R.C. Das and B. Behra; ‘Experiments in Physical Chemistry’ , Tata McGraw hill.

83

4. K.K. Sharma : ‘An Introduction of Practical Chemistry’: Vikas Publishing House,

New Delhi

5. Khosla, B. D.; Garg, V. C. & Gulati, A. Senior Practical Physical Chemistry,R. Chand &

Co.: New Delhi (2011).

COMPUTER LABORATORY -Non evaluative (A report of the work done should be included

in the physical chemistry record)

Computer Lab based instruction on the use of computer and internet in learning. Use of educational

softwares, information mining from internet and using INFLIBNET/NICNET, NPTEL and

VIRTUAL LABS OF MHRD. Word processing and document preparation. Introduction to chemical

structure drawing, visualization of molecules using chemistry softwares.

References: R T Mishra, Teaching of information Technology

SEMESTER VI

CH6CRP06 GRAVIMETRIC ANALYSIS

(2 Credits) 36 hours

1. Estimation of Barium as barium sulphate

2. Estimation of iron as Fe2O3

3. Estimation of sulphate as barium sulphate

4. Estimation of copper as cuprous thiocynate

5. Estimation of nickel as nickel dimethyl glyoxime.

References

1. J. Mendham. R.C. Denney, J.D. Barnes and M. Thomas, Vogel’s Textbook of

Quantitative Chemical Analysis, 6th Edition, Pearson Education, Noida, 2013.


Chemistry, 8th Edition, Brooks/Cole, Thomson Learning, Inc., USA, 2004. 3. G. D. Christian, Analytical Chemistry, JohnWiley and Sons.

R. D. Day, A. L. Uderwood, Quantitative analysis,6

84

COMPLEMENTARY COURSES IN CHEMISTRY

I-SEMESTER

CH1CMT01 : Basic Theoretical and Analytical Chemistry

(Common to physical sciences and geology)

Credits-2 (36 Hrs)

Aim: The aim of the course is to provide an insight into some of the fundamental concepts

and principles that are very essential in the study of chemistry

Module 1: Fundamental Concepts in Chemistry (6 hrs)

Modern periodic law – Long form periodic table. Periodicity in properties: Atomic radii,

ionic radii, ionization enthalpy, electron affinity (electron gain enthalpy) and

electronegativity (Pauling scale). Atomic mass - Molecular mass - Mole concept – Molar

volume - Oxidation and reduction – Oxidation number and valency - Equivalent mass.

Theory of acids and bases: Arrhenius theory, Bronsted-Lowry theory and Lewis theory. pH,

pOH, pK and buffers. Preparation of buffer solution having a known pH.

References 1. B. R. Puri, L. R. Sharma, M.S. Pathania, Elements of Physical Chemistry, 3rd edn. Vishal

Pub. CO., 2008 (Chapter 16)

2. C. N. R. Rao, University General Chemistry, Macmillan.

Module 2 : Laws of Thermodynamics (6 Hrs)

System and Surrounding. First law of Thermodynamics: Internal energy, Significance of

internal energy change, enthalpy, Second law of Thermodynamics: free energy, Entropy and

Spontaneity, Statement of second law based on entropy, Entropy change in Phase transitions

(No derivation required)-entropy of fusion, entropy of vaporization, entropy of sublimation.

The concept of Gibbs's free energy- Physical significance of free energy, conditions for

equilibrium & spontaneity based on ΔG values. Effect of temperature on spontaneity of

Reaction. Third law of Thermodynamics.

References: 1. K.K. Sharma and L.K. Sharma, A Textbook of Physical Chemistry, 5th Edition, Vikas


2. J. Rajaram and J.C. Kuriacose, Chemical Thermodynamics, Pearson Education, New

Delhi, 2013.

3. R. P. Rastogi, R. R. Misra, An Introduction to Chemical Thermodynamics, 6th edn.,

Vikas Pub. Pvt. Ltd. (2003 ),

Module 3: Chemical Bonding (6 Hrs)

Chemical Bonding: Introduction – Type of bonds. Ionic bond: Factors favouring the

formation of ionic bonds - Lattice energy of ionic compounds and its applications. Covalent

bond: Lewis theory - Valence bond theory – Coordinate bond. VSEPR theory and examples.

Hybridisation: sp(BeF2),sp2(BF3),sp3(CH4),sp3d (PCl5), sp3d2 (SF6) and sp3d3 (IF7). Molecular

orbital theory (elementary ideas): LCAO – Electronic configuration of H2,C2, N2, O2 and CO

– Calculation of bond order – Explanation of bond length and bond strength. Intermolecular

forces - Hydrogen bonding in H2O - Dipole-dipole interactions.

References:

1. Manas Chanda, Atomic Structure and Molecular Spectroscopy

2. P. L. Soni Inorganic Chemistry

85

3. B. R. Puri, L. R. Sharma, M.S. Pathania, Elements of Physical Chemistry, 3rd edn. Vishal

Pub. CO., 2008 (Chapter 19)

4. C. N. R. Rao, University General Chemistry, Macmillan.

Module 4: Nuclear Chemistry (9 Hrs)

Nuclear stability - Mass Defect, Binding energy, nuclear forces, magic number, packing

fraction, n/p ratio. Natural and induced radioactivity, radioactivity – detection, units of

radioactivity. Modes of decay – Group displacement law. Isotopes, isobars and isotones with

examples. Nuclear fission - Atom bomb – Nuclear fusion – Hydrogen bomb - Nuclear

reactors - Nuclear reactors in India. Application of radioactive isotopes – 14C dating – Rock

dating – Isotopes as tracers – Radio diagnosis and radiotherapy.

References

1. H.J. Arnikar, Essentials of Nuclear Chemistry (Revised IV edn.) ,New Age, 1995.

2. B. R. Puri, L. R. Sharma, M.S. Pathania, Elements of Physical Chemistry, 3rd edn. Vishal

Pub. Co., 2008.

Module 5 : Analytical Principles (9 Hrs)

Methods of expressing concentration: Weight percentage, molality, molarity, normality, mole

fraction, ppm and millimoles.

Theory of volumetric analysis – Primary and secondary standards, criteria for primary

standards, preparation of standard solutions, standardization of solutions, end point. Acid

base, redox and complexometric titrations and corresponding indicators. Principles in the

separation of cations in qualitative analysis - Applications of common ion effect and

solubility product - Microanalysis and its advantages. Reporting analytical data: Units,

significant digits, rounding, scientific and prefix notation, graphing of data - Precision and

accuracy – Types of errors – Ways of expressing precision – Methods to reduce systematic

errors.

References 1. R. A. Day Junior, A.L. Underwood, Quantitative Analysis, 5th edn. Prentice Hall of India

Pvt. Ltd. New Delhi, 1988(Chapters 2,3,4,6,8,11)

2. Vogel’s Text Book of Quantitative Chemical Analysis, J. Mendham, R. C. Denney, J.D.

Barnes, M. Thomas, 6th edn. Pearson Education (2003)(Chapters 3,4,10)

3. R. Gopalan, Analytical Chemistry, S. Chand and Co., New Delhi.

86

II –SEMESTER

CH2CM02: Basic Organic and Inorganic Chemistry

(Common to physical sciences and geology )

Credits-2 (36Hrs)

Aim The aim of the course is to understand some fundamental aspects of organic and inorganic

chemistry

Module 1: Organic Chemistry – Some Basic Concepts (9 hrs)

Introduction: Origin of organic chemistry – Uniqueness of carbon – Homologous series –

Nomenclature of alkyl halides, alcohols, aldehydes, ketones, carboxylic acids and amines.

Structural isomerism: Chain isomerism, position isomerism, functional isomerism and

metamerism. Arrow formalism in organic chemistry - Homolysis and heterolysis of bonds –

Electrophiles and nucleophiles. Polarity of bonds. Reaction Intermediates: Carbocations,

carbanions and free radicals (preparation, structure, hybridization and stability).

Types of organic reactions – addition, substitution and elimination reactions (elementary

ideas only)

References 1. I. L. Finar, Organic Chemistry Vol. I , 6th edn. Pearson.

2. S. M. Mukherji, S. P Singh, R. P Kapoor, Organic Chemistry Vol.1,NewAge

International(P) Ltd,2006(Chapter 2)

Module 2: Natural and Synthetic Polymers (9 Hrs)

Classification of polymers: Natural, synthetic; linear, cross-linked and network; plastics,

elastomers, fibres; homopolymers and copolymers. Polymerization reactions, typical

examples- polyethene, polypropylene, PVC, phenol-formaldehyde and melamine-

formaldehyde resins, polyamides (nylons) and polyester. Natural rubber: structure,

vulcanization. Synthetic rubbers- SBR, nitrile rubber, neoprene. Glass transition temperature

of polymers (Tg)- Definition- Factors affecting Tg. Importance of Tg. Biodegradability of

polymers, environmental hazards.

Reference 1. V.R. Gowarikar, Polymer Chemistry, New Age International Pvt. Ltd., New Delhi,

2010.

Module 3:Transition Elements, Lanthanoids and Actinoids: (9 Hrs)

Transition Elements-General group trends with special reference to electronic configuration,

variable valency, colour, magnetic properties, ability to form complexes, alloy formation,

interstitial compounds and stability of various oxidation states (Latimer diagrams) for Mn, Fe

and Cu.

Lanthanoids: Electronic configurations, Oxidation states, colour, magnetic properties,

lanthanide contraction, separation of lanthanides (ion exchange method only). Uses or

applications of lanthanides and their compounds

Actinoids: electronic configuration, oxidation states, actinide contraction, position of

actinides in the periodic table.

References

1. J. D. Lee, Concise Inorganic Chemistry 5th edn., Blackwell Science, London

2. B. R. Puri, L. R. Sharma, K. C. Kalia, Principles of Inorganic Chemistry, Milestone

Publishers, New Delhi

87

Module 4: General Principles of Metallurgy (6 Hours)

Occurrence of metals based on standard electrode potential, concentration of ores

(Gravity separation, magnetic separation, electrostatic separation, froth floatation & leaching)

Calcination, roasting and smelting. Reduction to free metal – reduction using carbon and

other reducing agents, Electrolytic reduction. Refining of metals – electrolytic refining,

oxidative refining, zone refining, Van Arkel-de-Boer method. Thermodynamics of the

oxidation of metals to metal oxides - Ellingham diagrams.

1. B. R. Puri, L. R. Sharma, K. C. Kalia, Principles of Inorganic Chemistry, Milestone

Publishers, New Delhi (Chapter 10)

2. S. Prakash, G. D. Tuli, S. K. Basu and R. D. Madan, Advanced Inorganic Chemistry,

Volume I, S Chand,( Chapter 20)

3. A. Cottrel, An introduction to metallurgy, 2nd edn., University press.

4. J.D.Lee, Concise Inorganic Chemistry, 5th edition , Oxford University Press, New Delhi

2008.

Module 5: Non aqueous solvents (3 hours) Classification of solvents, solvation, characteristics of solvents, reactions in liquid ammonia,

liquid sulphur dioxide and liquid HF (acid base, amphoteric, solvation, oxidation – reduction,

complex formation)

References 1. B. R. Puri, L. R. Sharma, K. C. Kalia, Principles of Inorganic Chemistry, Milestone

Publishers, New Delhi(Chapter 7)

2. J. E. Huheey, E. A. Keiter, R. L. Keiter, O K Medhi, Inorganic Chemistry, 4th edn.,

Pearson 2006 ( Chapter 9)

88

COMPLEMENTARY COURSES

PRACTICAL-I

(Semester I and II)

( Common to physical sciences, Life sciences, Geology and Family & community

sciences)

CH2CMP01: Volumetric Analysis

Credits 2 72 hours Standard solution must be prepared by the student

1. Acidimetry and Alkalimetry

1. Standardization of HCl with standard Na2CO3 solution

2. Standardization of NaOH with standard oxalic acid solution

3. Estimation of any acid using standard NaOH

4. Estimation of any alkali using standard HCl.

2. Permanganometry 1. Standardization of KMnO4 using (i) oxalic acid (ii) Mohr’s salt

2. Estimation of Fe2+ in Mohr’s salt and crystalline Ferrous Sulphate using standard KMnO4.

3. Dichrometry

1. Estimation of Ferrous ions (external indicator)

2. Estimation of Ferrous ions (internal indicator)

3. Estimation of FeSO4. 7 H2O (external indicator)

4. Iodimetry and Iodometry

1. Standardization of Iodine solution

2. Standardization of Sodium thiosulphate

3. Estimation of KMnO4

4. Estimation of Copper

References 1. D. A. Skoog, D. M. West, and S. R. Crouch, Fundamentals of Analytical Chemistry 8th

edn, Brooks/Cole Nelson

2. Vogel’s Textbook of Quantitative Chemical Analysis 6th edn, Pearsons Education. Ltd.

3. G. D. Christian, Analytical Chemistry, John Wiley and Sons

4. R.D Day, A.L. Uderwood, Quantitative analysis,6th Edn., Prentice Hall of India Pvt. Ltd.

89

SEMESTER-III

CH3CMT03 : Advanced Physical Chemistry – I

(For students who have opted Physical Sciences and Geology as Main)

Credits-3 (54 Hrs) Aim: To give the students a thorough knowledge about molecular structure and its electrical

and nuclear properties and to develop proper aptitude towards the study of molecular

structure

Objectives:

To enable the students to get a clear idea about the molecular structure

To make students capable of understanding and studying electrical and nuclear

properties of molecules.

Module 1: Solids and Crystalline State (18 Hrs)

Classification of solids: amorphous, crystalline – differences. Lattice, lattice energy (general

idea), unit cell, examples of simple cubic, bcc and fcc lattices, calculation of number of atoms

in a unit cell, calculation of lattice parameters of cubic unit cell. Theories of Solid: band

theory, conductors, semiconductors and insulators, mention of super conductors. Magnetic

Properties: classification - diamagnetic, paramagnetic, antiferromagnetic, ferro and

ferrimagnetic, permanent and temporary magnets.

Symmetry of molecules-symmetry elements and symmetry operations – centre of symmetry,

plane of symmetry, proper and improper axes of symmetry, crystallographic point groups,

Schoenflies symbol. Symmetry elements in crystals - The seven crystal systems – Weiss and

Miller indices - Bravais lattices – Bragg’s equation (derivation required) and its applications

(mention only), structure determination of NaCl by X-ray diffraction.

Module 2: Liquid State and solutions (12 Hrs) Liquids: Intermolecular forces, liquids compared with gases and solids (qualitative idea

only), viscosity, surface tension (method of determination not expected), structure of liquids

(a qualitative description). Liquid crystals – the intermediate phase between solid and normal

liquid phases, thermographic behaviour, classification, structure of nematic and cholesteric

phases.

Solutions: Kinds of solutions - Solubility of gases in liquids – Henry's law and its

applications - Colligative properties - Osmotic pressure - Reverse osmosis and its

applications - Determination of molecular mass using colligative properties.

Module 3: Gaseous State (9hrs)

Gaseous State: Introduction - Kinetic molecular model of gases – Maxwell distribution of

velocities and its use in calculating molecular velocities – Average velocity, RMS velocity

and most probable velocity (derivations not required) – Boyle’s law – Charles’s law – Ideal

gas equation – Behaviour of real gases – Deviation from ideal behaviour - Van der Waals

equation (derivation not required).

Module 4: Surface Chemistry and Colloids (9 Hrs) Adsorption – types of adsorption of gases by solids, factors influencing adsorption,

Freundlich adsorption isotherm – Langmuir adsorption isotherm (derivation not required).

True solution, colloidal solution and suspension. Classification of colloids: Lyophilic,

lyophobic, macromolecular, multimolecular and associated colloids with examples.

Purification of colloids by electrodialysis and ultrafiltration. Properties of colloids: Brownian

90

movement – Tyndall effect – Electrophoresis. Origin of charge and stability of colloids –

Zeta potential – Coagulation - Hardy Schulze rule – Protective colloids - Gold number.

Emulsions. Applications of colloids: Delta formation, medicines, emulsification, cleaning

action of detergents and soaps.

Module 5: Phase Equilibrium (6Hrs) The phase rule, definition, equilibrium between phases, one component system – water

system, two component systems: solid- liquid equilibrium – simple eutectic, lead-silver

system, solid solution. Distribution law, partition coefficient, applications.

References: 1. B.R. Puri, L.R. Sharma, M.S. Pathania, Elements of Physical Chemistry, 40thedn.

Vishal Pub. Co. Jalandhar (2013)

2. B. R. Puri, L.R. Sharma and K.C. kalia, Principles of Inorganic Chemistry, Milestone

Publishers New Delhi. 2013.

3. J.A. K. Tareen and T.R. N. Kutty, A basic course in Crystallography, University

Press, 2000.

4. Anthony R West, Solid State Chemistry and its Applications”, Wiley Eastern

5. V.Ramakrishnan and M.S.Gopinathan, “Group Theory in Chemistry”, Vishal

Publishing Co.

6. Gurdeep Raj, “Advanced Physical Chemistry”, Goel Publishing House.

7. Walter J. Moore, Physical Chemistry, 4thEdn. Longmans Green and Co. Ltd.

8. P. W Atkins, “Physical Chemistry”, Oxford University Press.

9. R. J Silby and R.A Alberty, “Physical Chemistry”, John Wiley & Sons.

91

SEMESTER-IV

CH4CMT04: Advanced Physical Chemistry – II

(For students who have opted Physical Sciences and

Geology as Main)

Credits-3 (54 Hrs) Aim :To promote understanding of the basic facts and concepts in spectroscopy and to

develop interest in students to study the structure and properties of matter.

Objectives :

To help the students to get a basic idea about spectroscopy

To enable the students to study the rules governing chemical reactions and factors

influencing them.

Module 1: Introduction to Spectroscopy (9 Hrs) Interaction of electromagnetic radiation with matter, electromagnetic spectrum, quantization

of energy, electronic, vibrational and rotational energy levels, Boltzmann distribution of

energy (formula only), population of levels.

UV- Visible Spectroscopy: Beer Lambert’s law, molar extinction coefficient and its

importance, UV spectrum, max, chromophore, auxochrome, red shift, blue shift, types of

transition.

Infra-red spectroscopy: vibrational degrees of freedom, types of vibrations – symmetric and

asymmetric stretching and bending, calculation of force constant, concept of group

frequencies-frequencies of common functional groups in organic compounds, Fingerprint

region in IR spectra.

Rotational Spectroscopy: diatomic molecules, determination of bond length.

Module 2: Nano Chemistry (9hrs) Terminology- scales of nanosystems- nanoparticles. Nanomaterials – synthesis – chemical

precipitation, mechano-chemical method, micro emulsion method, reduction technique,

chemical vapour deposition and sol-gel method (brief study).Properties and applications of

fullerenes and carbon nanotubes. Nanochemical devices- optoelectronic devices-

photodetectors- LEDs and lasers.

Module 3: Kinetics, Catalysis & Photochemistry: (18 hrs)

Kinetics: Rates of reactions - Factors influencing rate of reactions - Order and molecularity -

Zero, first, second and third order reactions - Derivation of integrated rate equations for first

order and second order reactions (single reactant only) - Half-life period for first order

reaction - Units of rate constants - Influence of temperature on reaction rates - Arrhenius

equation - Calculation of Arrhenius parameters - Collision theory of reaction rate, Activated

complex theory-basic concepts-no derivation required.

Catalysis: Types of catalysis – Homogeneous and heterogeneous catalysis. Theories of

catalysis: Outline of intermediate compound formation theory and adsorption theory.

Laws of photochemistry, Grothus Draper law, Stark-Einsten’s Law, Beer Lambert’s Law.

Photochemical equivalence and quantum explanation for low and high quantum yields.

Photosensitization, Jablonski diagram- Fluorescence and phosphorescence, flash photolysis

and chemiluminescence.

Module 4: Electrochemistry (18hrs)

Introduction- Faraday’s laws of electrolysis, electrochemical equivalent and chemical

equivalent, Specific conductance, equivalent conductance and molar conductance - Variation

92

of conductance with dilution - Kohlrausch's law - Degree of ionization of weak electrolytes -

Application of conductance measurements –Determination of degree of dissociation of weak

electrolytes, conductometric titrations involving strong acid- strong base, strong acid-weak

base, weak acid- strong base, and precipitation titration.

Galvanic cells - Cell and electrode potentials - IUPAC sign convention, Types of electrodes:

Reference electrodes – Standard hydrogen electrode and calomel electrode, Indicator

electrodes-metal-metal ion electrodes, Quinhydron electrode and Redox electrodes. Standard

electrode potential - Nernst equation, electro chemical series. Gibb’s Helmholtz equation and

EMF of a cell.

Fuel cells- H2-O2 fuel cell. Potentiometric titrations of acid-base and redox reactions-

precipitation reactions.

References:

4. Banwell, C. N. &Mc Cash, E. M. Fundamentals of Molecular Spectroscopy 4th Ed.

Tata McGraw-Hill: New Delhi (2006).

5. D. L. Pavia, G. M. Lampman, G. S. Kriz, Introduction to spectroscopy 3rd edn,

Thomson Brooks/Cole, 2001.

6. V. S. Muraleedharan and A. Subramania, Nanosciece and nanotechnology, Ane

Books Pvt. Ltd. New Delhi, 2009

7. T. Pradeep, Nano: The Essentials, McGraw-Hill education, New Delhi,2006.

8. K.K. Sharma and L.K. Sharma, A Textbook of Physical Chemistry, 5th Edition, Vikas


9. B. R. Puri, L.R. Sharma, M. S. Pathania, Elements of Physical Chemistry, 40th edn.

Vishal Pub. Co. Jalandhar (2003).

10. G. M. Barrow, Physical Chemistry, 5th Edition, Tata McGraw Hill Education, New

Delhi, 2006.

11. G. K. Vemulapalli, Physical Chemistry, Prentice-Hall of India Pvt. Ltd. (1997)

12. GurdeepRaj, Photochemistry, 6th Edn, Goel Publishing House, 2014.

93

(Semesters III and IV)

PRACTICAL-II

Credits-2 (72Hrs)

CH4CMP02 :Physical Chemistry Practical

(For students who have opted Physical Sciences and Geology as Main)

1. Viscosity-percentage composition of sucrose solution.

2. Determination of Partition coefficient of a non-volatile solute

3. Transition temperature of salt hydrates, eg. Sodium thiosulphate Sodium acetate etc.

4. Critical solution temperature of phenol water system

5. Phase diagram of two component systems

6. .Heat of Solution KNO3, NH4Cl

7. Heat of neutralization

8 Determination of equivalent conductance of an electrolyte

9 . Conductometric titration of strong acid Vs. strong base

10. Potentiometric titrations : Fe2+ Vs. Cr2O72- and Fe2+ Vs. KMnO4

11. Determination of molecular weight by Rast’s method. (Using naphthalene, or biphenyl as

solvent and acetanilide, p–dichlorobenzene etc.as solute)

12. Kinetics of simple reactions, e.g. Acid hydrolysis of methyl acetate

References

1. W. G. Palmer: ‘Experimental physical chemistry’, Cambridge University Press.

2. J. B. Yadav: Advanced Practical Physical Chemistry Goel Publishing House.

3. R. C. Das and B. Behra; ‘Experiments in Physical Chemistry’ , Tata McGraw hill.

4. K. K. Sharma : ‘An Introduction of Practical Chemistry’: Vikas Publishing House, New

Delhi

94

Syllabus for B.Sc. Chemistry (Complementary)

for Life Sciences and Family & Community Science core

Semester I

Course CH1CM05: BASIC THEORETICAL AND ANALYTICAL CHEMISTRY

(For students who have opted Life Sciences and Family & Community Science as core)

Credits-2 (36 Hrs)

Aim:

The aim of the course is to provide an insight into some of the fundamental concepts and

principles that are very essential in the study of Chemistry.

Objectives:

1. To study the concepts of atomic structure, chemical bonding, periodic properties, acids and

bases and solution chemistry.

2. To understand the basic principles of analytical techniques and chromatographic

techniques.

Module 1: Atomic Structure and Chemical Bonding (9 Hrs)

Atomic Structure: Bohr atom model and its limitations, Dual nature of matter and radiation.

Photoelectric effect, de Broglie equation, Heisenberg’s uncertainty principle, Concept of

orbital, Quantum numbers, shapes of orbitals (s, p, d), Electronic configuration of atoms -

Aufbau principle, Hund’s rule of maximum multiplicity, Pauli’s exclusion principle.

Chemical Bonding: Introduction – Type of bonds. Ionic bond: Factors favouring the

formation of ionic bonds - Lattice energy of ionic compounds and its applications. Covalent

bond: Lewis theory - Valence bond theory – Coordinate bond. VSEPR theory and examples.

Hybridisation: - sp3, sp2 and sp (ethane, ethene, ethyne). Molecular orbital theory: LCAO –

Electronic configuration of H2, B2, C2, N2, O2 and CO – Calculation of bond order –

Explanation of bond length and bond strength. Intermolecular forces - Hydrogen bonding in

H2O - Dipole-dipole interactions.

Module 2: Fundamental Concepts in Chemistry (9 hrs)

Modern periodic law – Long form of periodic table. Periodicity in properties: Atomic radii,

ionic radii, ionization enthalpy, electron affinity (electron gain enthalpy) and

electronegativity (Pauling scale). Atomic mass - Molecular mass - Mole concept – Molar

volume - Oxidation and reduction – Oxidation number and valency - Equivalent mass.

Methods of expressing concentration: Weight percentage, molality, molarity, normality, mole

fraction, ppm and millimoles.

Acids and bases: Arrhenius, Lowry-Bronsted and Lewis theories. Ionic product of water - pH

and pOH, Strengths of acids and bases - Ka and Kb, pKa and pKb. Buffer solution.

Preparation of buffer solution having a known pH. Solvation, solubility, solubility product,

common ion effect and their applications.

95

Module 3: Basic Principles of Analytical Chemistry (9 Hrs)

Laboratory operations (Non-evaluative): Laboratory safety and first aid. Use of different

glassware like pipette, burette, standard measuring flask, distillation apparatus; heating

methods, filtration techniques, weighing principle in chemical balance, weighing in electronic

balance.

Volumetric method of analysis: General principles. Primary and secondary standards, criteria

for primary standards, preparation of standard solutions, standardization of solutions, end

point. Acid base, redox and complexometric titrations and corresponding indicators.

Gravimetric method of analysis: General principles. Double burette method of titration:

Principle and advantages. Microanalysis and its advantages. Reporting of analytical data:

Units, significant digits, rounding, scientific and prefix notation, graphing of data - Precision

and accuracy – Types of errors – Ways of expressing precision – Methods to reduce

systematic errors.

Separation and purification techniques: Recrystallisation, use of drying agents, sublimation.

General principles of distillation, fractional distillation, distillation under reduced pressure.

Solvent extraction.

Module 4: Chromatographic Techniques (9 Hrs)

Chromatography - Principle of differential migration. Classification of chromatographic

methods. Basic principle and uses of Thin layer chromatography (TLC), Paper

chromatography (PC), Rf value, Column chromatography, Gas chromatography(GC), High

performance Liquid chromatography (HPLC), Ion Exchange chromatography (IEC).

References

1. B. R. Puri, L. R. Sharma, M.S. Pathania, Elements of Physical Chemistry, 3rd edn.

Vishal Pub. Co., 2008.

2. C. N. R. Rao, University General Chemistry, Macmillan, 2009.

3. Manas Chanda, Atomic Structure and Molecular Spectroscopy.

4. P. L. Soni, Inorganic Chemistry .

5. R. A. Day Junior, A.L. Underwood, Quantitative Analysis, 5th edn. Prentice Hall of

India Pvt. Ltd. New Delhi, 1988.

6. J. Mendham, R. C. Denney, J.D. Barnes, M. Thomas, Vogel’s Text Book of

Quantitative Chemical Analysis, 6th edn. Pearson Education (2003).

7. R. Gopalan, Analytical Chemistry, S. Chand and Co., New Delhi.

96

Semester II

CH2CMT06: BASIC ORGANIC CHEMISTRY


Credits-2 (36Hrs)

Aim:

The aim of the course is to understand some fundamental aspects of organic chemistry.

Objectives:

1. To study the fundamental concepts of organic chemistry and organic reaction mechanisms.

2. To study the stereochemistry of organic compounds.

3. To study about natural and synthetic polymers.

Module 1: Fundamental Concepts of Organic Chemistry (9 hrs)

Introduction: Origin of organic chemistry – Uniqueness of carbon – Homologous series.

IUPAC Nomenclature of alkyl halides, alcohols, aldehydes, ketones, carboxylic acids and

amines. Structural isomerism: Chain isomerism, position isomerism, functional isomerism

and metamerism. Arrow formalism in organic chemistry. Bond fission - homolytic and

heterolytic fission. Types of reagents - Electrophiles and nucleophiles. Polarity of bonds. Reaction

Intermediates: Carbocations, carbanions and free radicals (preparation, structure, hybridization and

stability). Types of organic reactions: Addition, Elimination, Substitution, Rearrangement and Redox

reactions (definition and one example each).

Module 2: Stereochemistry of Organic Compounds (9 Hrs)

Stereosiomerism – definition, classification

Optical Isomerism: Optical activity – Chirality – Enantiomers - Meso compounds -

Diastereoisomers – Optical isomerism in lactic acid and tartaric acid - Racemisation and

resolution (elementary idea).

Geometrical Isomerism: Definition – Condition – Geometrical isomerism in but-2-ene and

but-2-ene-1,4-dioic acid. cis and trans, E and Z configurations. Methods of distinguishing

geometrical isomers using melting point and dipole moment.

Conformations: Newman projection, Saw-horse projection, Conformations of ethane, n-

butane, cyclohexane and methyl cyclohexane - Relative stability and energy diagrams.

Conformation of methyl cyclohexane.

Module 3: Mechanisms of Organic Reactions (9 Hrs)

Meaning of reaction mechanism. Polarity of bonds. Electron Displacement Effects: Inductive

effect - Definition - Characteristics - +I and -I groups. Applications: Explanation of

97

substituent effect on the acidity of aliphatic carboxylic acids. Mesomeric effect: Definition –

Characteristics - +M and -M groups. Applications: Comparison of electron density in

benzene, nitrobenzene and aniline. Hyperconjugation: Definition – Characteristics. Example:

Propene. Applications: Comparison of stability of 1-butene & 2-butene. Electromeric effect:

Definition -Characteristics - +E effect (addition of H+ to ethene) and -E effect (addition of

CN- to acetaldehyde). Steric effect (causes and simple examples).

Substitution reactions: nucleophilic substitution of alkyl halides- SN1 and SN2 mechanisms.

Electrophilic substitutions in benzene-reaction mechanism. Addition reactions: electrophilic

addition to alkenes, the Markwonikoff’s rule, Peroxide effect. Elimination reactions: E1 and

E2 mechanisms.

Module 4: Natural and Synthetic Polymers (9 Hrs)

Introduction. Classification of polymers: Natural, synthetic; linear, cross-linked and network;

plastics, elastomers, fibres; homopolymers and copolymers. Polymerization reactions, typical

examples- polyethene, polypropylene, PVC, phenol-formaldehyde and melamine-

formaldehyde resins, polyamides (nylons) and polyester. Natural rubber: structure,

vulcanization. Synthetic rubbers- SBR, nitrile rubber, neoprene. Biodegradability of

polymers, environmental hazards. Recycling of plastics.

References

1. I. L. Finar, Organic Chemistry Vol. I , 6th edn. Pearson.

2. M.K. Jain, S.C. Sharma, Modern Organic Chemistry, Vishal Publishing Co. 2010.

3. S. M. Mukherji, S. P Singh, R. P Kapoor, Organic Chemistry Vol.1, New Age

International Pvt. Ltd, 2006.

4. S. Sengupta, Basic Stereochemisty of Organic Molecules, 2014.

5. E. L. Eliel, S.H. Wilen, Sterechemistry of Organic Compounds, Wiley, 1994.

6. Peter Sykes, A Guide Book to Mechanism in Organic Chemistry, 6th edn. Orient

Longman, 1988.

7. S. M. Mukherji, S.P Singh, Reaction Mechanism in Organic Chemistry, Macmillan,

3rd edn., 2003.

8. V.R. Gowarikar, N.V. Viswanathan, J. Sreedhar, Polymer Science, 2nd edn., New Age

International Pvt. Ltd., 2015.

98

SEMESTER III

CH3CMT07: ADVANCED INORGANIC AND ORGANIC CHEMISTRY (For students who have opted Life Sciences and Family & Community Science as Core)

Credits-3 (54 Hrs)

Aim:

The aim of the course is to promote understanding of facts and concepts and modern trends in

inorganic and organic chemistry.

Objectives:

1. To obtain a basic understanding of environmental chemistry, bioorganic chemistry and

heterocyclic compounds.

2. To learn about various types of fertilizers and pesticides.

3. To learn about various types of food additives and cosmetics.

Module 1: Introduction to Environmental Chemistry (18 Hrs)

Environment and its segments. Ecosystems - Biogeochemical cycles of Carbon, Nitrogen,

Phosphorus and Sulphur.

. Hydrosphere and Water Pollution: Water quality parameters, Dissolved oxygen-B.O.D and

C.O.D. Methods of determination of alkalinity and acidity of water. Pollutants of water -

sewage, industrial effluents, soap and detergents, pesticides, fertilizers, heavy metals. The

metabolic fate and toxic effect of pollutants. Water purification methods -sedimentation,

coagulation filtration, disinfection, ion exchange - desalination of sea water.

Air Pollution: Major regions of atmosphere. Pollution by oxides of nitrogen, sulphur,

carbon, hydrocarbon and other organic chemicals. Automobile exhausts - physiological

effects on vegetation and living organisms, Controlling of pollution. Ozone layer -

formation and its importance. Depletion of ozone layer – causes - effect on living things.

Chlorofluorocarbon substitutes. Greenhouse effect, Global warming, Acid rain. Green

chemistry – general idea, importance.

.

Module 2: Bioinorganic Chemistry (9 hrs)

Thermodynamics of Living cell- Exergonic and endergonic reactions, coupled reactions.

Metal ions in biological systems - Biochemistry of iron – Metalloporphyrins - Haemoglobin

and myoglobin, pH of blood, cytochromes, Ferredoxine - Mechanism of O2 and CO2

transportation - Chlorophyll and photosynthesis (mechanism not expected) elementary idea

of photophosphorylation. Photosynthesis and respiration – comparison. – Elementary idea of

structure and mechanism of action of sodium potassium pump. Biochemistry of zinc and

cobalt.

99

Module 3: Heterocyclic Compounds (9 Hrs)

Aromaticity – Huckel rule, preparation (any one method), properties, structure and

aromaticity of furan, pyrrole, pyridine and indole. Pyrimidines & purines - adenine, guanine,

thymine, cytosine and uracil.

Moduele 4: Chemistry and Agriculture (9 Hrs)

Fertilizers: NPK, superphosphates, triple super phosphate, uses of mixed fertilizers,

micronutrients and their role, bio-fertilizers, plant growth hormones.

Pesticides: Classifications with simple examples, Biopesticides. Insecticides – stomach

poisons, contact insecticides, fumigants. Method of preparation and use of DDT, BHC,

pyrethrin. Herbicides - structure and function of 2, 4,-D and 2,4,5 –T, Fungicides- inorganic

and organic- Bordeaux mixture. Excessive use of pesticides – environmental hazards.

Module 5: Food Additives and Cosmetics (9 Hrs)

Food Additives: Food preservatives, artificial sweeteners, flavours, emulsifying agents,

antioxidants, leavening agents and flavour enhancers (definition and examples, structures not

required) – Structure of BHT, BHA and MSG - Commonly used permitted and non-permitted

food colours (structures not required) - Fast foods and junk foods & their health effects – Soft

drinks and their health effects.

Cosmetics: Introduction, classification. Dental cosmetics, Shampoos, Hair dyes, Skin

products, Shaving cream, Talcum powder, perfumes and deodorants (composition and health

effects).

References 1. A.K. De, Environmental Chemistry, 6th edn., New Age International Pvt. Ltd. 2006.

2. I. L. Finar, Organic Chemistry Vol. 1 & 2, 6th edn., Pearson, 2002.

3. C.N. R. Rao, University General Chemistry, Macmillan 2009.

4. B. R. Puri, L.R. Sharma and K.C. Kalia, Principles of Inorganic Chemistry, Milestone

Publishers New Delhi. 2013.

5. G. T. Austin, Shreve’s Chemical Process, 5th edn., McGraw Hill, 1984.

6. Rastogi, Biochemistry, Tata Mc Graw Hill Publication, 1996.

7. B. Sreelakshmi, Food Science, New Age International Pvt. Ltd, New Delhi, 2015.

8. J.W. Hill, T.W. McCreary, D.K. Kolb, Chemistry for Changing Times, Prentice Hall, 12th

edn., 2010.

100

SEMESTER IV

CH4CMT08: ADVANCED BIO-ORGANIC CHEMISTRY

(For students who have opted Life Sciences and Family & Community Science as Core)

Credits-3 (54 Hrs)

Aim:

The aim of this course is to promote understanding of facts and concepts in bioorganic

chemistry and to develop interest in the study of biomolecules.

Objectives:

1. To study about natural products like terpenoids, alkaloids and lipids.

2. To study about biopolymers like proteins and nucleic acids.

3. To study about biomolecules like carbohydrates, vitamins, steroids and hormones.

4. To learn about the important topic of medicinal chemistry.

Module 1: Natural Products (9 hrs)

Terpenoids: Classification with examples – Isoprene rule – Isolation of essential oils by

steam distillation – Uses of lemongrass oil, eucalyptus oil and sandalwood oil - Source,

structure and uses of citral and geraniol.

Alkaloids: Classification – Isolation, general properties. Source, structure and physiological

activity of nicotine, coniine and piperine.

Lipids: Classification – Oils, fats and waxes (definition, structure and examples) – Acid

value, Saponification number and Iodine number – Hydrogenation and Rancidity. Soaps,

cleaning action of soaps. Synthetic detergents, environmental aspects.

Module 2 : Amino Acids and Proteins (9 hrs)

Amino acids: Classification – Zwitter ion formation and isoelectric point- Synthesis of

glycine, alanine, and phenyl alanine (any one method). Peptides: Peptide bond. Synthesis of

peptides (up to dipeptides). Proteins: Classification of proteins – Primary, secondary and

tertiary structure of proteins -– Denaturation of proteins – tests for proteins.

Module 3 : Enzymes and Nucleic Acids (9 hrs)

Enzymes: General nature, classification, cofactors, Characteristics, catalytic action – Theory

of enzyme catalysis – Michaelis-Menten theory.

Nucleic acids: Structure of pentose sugar, nitrogenous base, nucleoside and nucleotide –

Double-helical structure of DNA – Differences between DNA and RNA. Biological

Functions – Replication and protein biosynthesis. Transcription and Translation. Genetic

code.

Energy rich molecules: elementary structure of ATP, ADP and AMP.

101

Module 4 : Carbohydrates (9 hrs)

Carbohydrates: Classification with examples. Preparation and properties of glucose, fructose

and sucrose. Cyclic structures and Haworth projections of glucose, fructose, maltose and

sucrose (ring size determination not expected). – Mutarotation. Conversion of glucose to

fructose and vice versa. – Structure of Starch and cellulose (structure elucidation not

expected). Industrial applications of cellulose.

Module 5 : Vitamins, Steroids and Hormones (9 hrs)

Vitamins: Classification. Biological functions and deficiency diseases of vitamins A, B1, B2,

B3, B5, B6, B12, C, D, E and K.

Steroids: Introduction. Structure and functions of cholesterol. Elementary idea of HDL and

LDL. Bile acids.

Hormones: Introduction. Steroid hormones, peptide hormones and amine hormones

(example, endocrine gland and biological functions, structure not required). Artificial

hormones (only elementary study).

Module 6 : Drugs (9 hrs)

Classification of drugs. Structure, therapeutic uses and mode of action of antibiotics:

Ampicillin and Chloramphenicol, antipyretics: Paracetamol, analgesics: Aspirin, sulpha

drugs: Sulphanilamide, antacids: Ranitidine, antimalarials: Chloroquine, anti-cancer drugs:

Chlorambucil (synthesis not required). Psychotropic drugs: Tranquilizers, antidepressants and

stimulants with examples. Drug addiction and abuse. Prevention and treatment.

References

1. Maya Shankar Singh, L.G.Wade, Organic Chemistry, 6th Edition, Pearson Education,

New Delhi, 2013.

2. P.Y. Bruice, Essential Organic Chemistry, 1st Edition, Pearson Education, New

Delhi, 2013.

3. I.L. Finar, Organic Chemistry Vol. I & II, 5th Edition, Pearson Education, New Delhi,

2013.

4. M.K. Jain, S.C. Sharma, Modern Organic Chemistry, Vishal Publishing Co. 2010.

5. K.S. Tewari, N.K. Vishnoi and S.N. Mehrotra, A Textbook of Organic Chemistry, 2nd

Edition, Vikas Publishing House (P) Ltd., New Delhi, 2004.

6. A. Bahl and B.S. Bahl, Advanced Organic Chemistry, 1st Multicolour Edition, S.

Chand & Company, New Delhi, 2010.

7. A.C. Deb, Fundamentals of Biochemistry,9th Edn. New Central Book Agency,2001.

8. G. R. Chatwal, Synthetic Drugs, Himalaya Publishing House, Bombay, 1995.

9. J.Ghosh, A Textbook of Pharmaceutical Chemistry, S. Chand & Co Ltd., 1997.

10. Rastogi, Biochemistry, Tata Mc Graw –Hill Publication ,1996

102

(Semesters III and IV)

PRACTICAL – II

Credit – 2 (72 hrs)

CH4CMP03 : Organic Chemistry Practical

(For students who have opted Life Sciences and Family & Community Science as Core)

1. Tests for elements: Nitrogen, Halogen and Sulphur

2. Determination of physical constants

3. Study of reactions of common functional groups.

4. Qualitative analysis with a view to characterization of functional groups and identification

of the following compounds: Naphthalene, anthracene, chlorobenzene, benzyl chloride, p-

dichlorobenzene, benzyl alcohol, phenol, o-, m- and p- cresols, α-naphthol, β-naphthol,

resorcinol, benzaldehyde, acetophenone, benzophenone: benzoic acid, phthalic acid,

cinnamic acid, salicylic acid, ethyl benzoate, methyl salicylate, benzamide, urea, aniline, o-,

m- and p- toluidines, dimethyl aniline, nitrobenzene, o-nitrotoluene, m-dinitrobenzene and

glucose. (minimum of ten compounds to be analysed).

5. Organic preparation involving halogenation, nitration, oxidation, reduction, acetylation,

benozylation, hydrolysis, diazotization.

6. Isolation of an organic compound from a natural source.

References: 1. A. I Vogel, A Text Book of Practical Organic Chemistry, Longman.

2. F. G. Mann and B.C. Saunders, Practical Organic Chemistry, 4th Edn., Pearson

Education.

3. V. K. Ahluwalia and S. Dhingra, Comprehensive Practical Organic Chemistry,

Universities Press.

103

2. BSc Chemistry (Vocational) – Model -II

SYLLABUS FOR VOCATIONAL COURSES

(INDUSTRIALCHEMISTRY)

Semester I

CH1VOT01 Industrial Aspects of Inorganic and Organic Chemistry

Credits-3 (72 Hrs)

Aim: The aim of this course is to provide an exposure to the industrial aspects of different branches of

chemistry and some aspects of chemical engineering.

Objectives:

To study:

About coal, petroleum and non-petroleum fuels

The basic concepts of metallurgical operations

The basic concepts of food science

Industrial Aspects of Organic chemistry

Module 1

Petroleum-Natural gas-fraction of crude oil-fractional distillation -cracking-reforming-hydro forming-

isomerisation. Octane number and Cetane number, Knocking and antiknock compounds.

Non-petroleum fuels (CNG, LNG, Biodiesel, bio-gas, fuels derived from bio-mass), fuel from waste;

Gaseous fuels.

Basic idea about Synthetic fuels- Fischer-Tropsch synthesis and Bergius process.

(15Hrs)

Module 2

Coal: types -distillation of coal- carbonization- types of carbonization. Distillation of coal tar-

chemicals derived from them. Analysis of coal –ultimate analysis and proximate analysis.

(12 Hrs)

Renewable natural resources: Cellulose-starch-properties- modification -important

Industrial chemicals derived from them-Manufacture of oxalic acid and furfural

(12Hrs)

Industrial Aspects of Inorganic Chemistry

Module 3

Basic metallurgical operations: Pulverisation-calcination–roasting-refining-

104

Physicochemical principle of extraction of iron, classification of steel, heat treatment of steel,

passivity-copper -silver-sodium-aluminium-magnesium and zinc.

(12Hrs)

Module 4

Inorganic materials of industrial importance: Their availability-forms-structure and modification.

Alumina-silica –silicates-clays-mica-carbon-zeolites (9Hrs)

Food Science

Module 5

Food additives: structure and properties of artificial sweeteners-saccharin, cyclamate and aspartame.

Natural and artificial Food flavours- esters, aldehydes and heterocyclic compounds.

Properties and examples of food colours; restricted use; spurious colours; emulsifying agents –

preservatives, leavening agents- baking powder, yeast; taste makers –MSG and vinegar.

(12Hrs)

References:

1. E.J.Hoffmann, Coal conversion-the Energon Co. Lavamic, Wyoming USA

2. L.F.Hath, S.Matarm, From Agro Carbons to petrochemicals, Gulf publishing Co., Houston

3. Steiner, Introduction to petroleum chemicals, Pergamon press

4. T. Satheesh Babu, Textbook for Engineering Chemistry Aspirants; Saradhi Publishers, Kerala.

5. A. G. Hall,Cotton, Cellulose, its Chemistry and Technology Cellulose

6. E. Heuser, Chemistry of cellulose

7. R. L. Whistle, Methods in Carbohydrate Chemistry Vol.3

8. R.W. Kerr, Chemistry and industry of starch

9. O. B. Wurzburg, Modified starches- properties and uses

10. Herbash, Principles of extractive metallurgy Vol.1 and 2

11. A. Volskky, E. Sergievskaya, Theory of metallurgical process

12. A. R. Baiky, Clays,H .Ries,Text book of Metallurgy, John Wiley and sons

13. Fillipoy, Theory of metallurgical process, MIR Publications

14. Pchlke, Unit processes of extractive metallurgy, Elsevier publication

15. R.Gopalan, D. Venkappaya, S. Nagarajan; Engineering Chemistry; Vikas Publications, New

Delhi.

16. Jayashree Ghosh, Fundamental Concepts of Applied Chemistry, S. Chand and Co.

17. B. Sreelakshmi, Food Science, New Age.

105

Semester II

CH2VOT02 Industrial Aspects of Physical Chemistry

Credits-3 (72Hrs)

Aim: Familiarization of the industrial applications of some aspects of physical chemistry.

Objectives:

To understand:

Surface phenomena, catalysis and hydrochemistry.

General aspects of pesticides, lubricants and batteries.

Module 1

Surface and interfacial phenomena: Preparation and properties of colloids- colloidal dispersions,

sols and their preparation, properties of suspensions, optical properties of sols, kinetic properties of

sols, electrical properties of sols, electrophoresis and electro osmosis, stability of colloids,

precipitation of sols, associated colloids, macromolecular properties in solutions and molecular

weight determinations.

(9Hrs)

Module 2

Adsorption isotherm, sols-gels-emulsions-micro emulsions-micelles-aerosols-effect of

Surfactants-hydrotropes

(12Hrs)

Module 3

Catalysis: Introduction-types-homogeneous and heterogeneous –basic principles –mechanism-

factors affecting the performance. Introduction to phase transfer catalysis.

(9Hrs)

Enzyme Catalyzed reactions –rate –model – examples of industrially important enzyme catalyzed

reactions

(6Hrs)

Module 4

Pesticides-General introduction to pesticides (natural and synthetic), benefits and adverse effects,

synthesis, technical manufacture and uses of representative pesticides in following classes:

organochlorines (DDT and Gammexane), Organophosphates (Malathion, parathion), Quinones

(Chloranil)

(9Hrs)

Module 5

Lubricants: Classification of lubricants, lubricating oils (conducting and non-conducting), solid and

semisolid lubricants, synthetic lubricants. Properties of lubricants (viscosity index, cloud point, pour

point, aniline point, flash point).

(9Hrs)

Module 6

Hydrochemistry: Characteristics and uses of water, hardness of water – unit of hardness; water

softening methods- Clark’s process, lime soda process, modified lime soda process, permutit or

zeolite process and ion exchange process. Water purification- potability of water, clarification,

coagulation, contact and electrochemical coagulation, sterilization and disinfections of water,

percipitation – aeration –ozonisation- chlorination.

(9Hrs)

Module 7

Batteries: Primary and secondary batteries, Characteristics of battery.

Working of: Lead acid battery, Lithium ion battery, Nickel-cadmium cell, solar cell

106

(9Hrs)

References:

1. Shepherd, Aerosol science and technology

2. B. Delmon, G. Janner, Catalysis- Heterogeneous and homogeneous.

3. J .Anderson, Catalysis science and technology

4. J. Fendler, E. Fendler Catalysis in micellar and macro molecular systems

5. E. K. Rideal, H. S. Taylor, Catalysis in theory and practice

6. C. Starles, Phase transfer catalysis, Principles and techniques

7. J. J. Bikermann, Surface chemistry, Academic press

8. A.W. Adamson,Physical chemistry of surfaces

9. Delmon, Catalysis: Heterogeneous and homogeneous, Elseiver science publisher

10. R.Gopalan, D.Venkappayya, S.Nagarajan: Engineering Chemistry, Vikas Publications, New Delhi

11. T. Satheesh Babu, A Textbook for Engineering Chemistry Aspirants, Saradhi Publishers, Kerala.

12. B.K.Sharma: Engineering Chemistry, Goel Publishing House, Meerut.

Semester I & II

CH2VOP01 Practical-I

Credits-2 (72 hrs)

1. Simple Laboratory techniques: Crystallisation and distillation

2. Preparation of standard solution: Primary and secondary solution-determination of H2SO4, H3PO4

in a mixture

3. Determination of dissolved oxygen present in the given water sample

4. Determination of chemical oxygen demand (COD) present in the given water sample

5. Determination of total permanent and temporary hardness of water using EDTA

6. Ore analysis-dolomite, lime stone, calcite, Epsom salt.

References:

1. D. A. Skoog, D. M. West, and S. R. Crouch, Fundamentals of Analytical Chemistry 8th edn,

Brooks/Cole Nelson

2. Vogel’s Textbook of Quantitative Chemical Analysis 6th edn, Pearsons Education Ltd.

3. G. D. Christian, Analytical Chemistry, John Wiley and Sons

4. R. D Day, A.L. Uderwood, Quantitative analysis,6th Edn.,Prentice Hall of India Pvt. Ltd.

5. G.L.David Krupadanam, D. Vijaya Prasad, K. Varaprasad Rao, K.L.N. Reddy, C. Sudhakar,

Analytical Chemistry, University Press

6. Vogel’s Qualitative Inorganic Analysis, 7th edn., Pearson Education Ltd.

107

SEMESTER-III

CH3VOT03: Unit Operations in Chemical Industry

Credits-3 (54 Hrs)

Aim

To give an exposure to the various unit operations and processes in industry

Objectives

To study unit operations and processes such as:

Distillation

Absorption

Evaporation

Filtration

Crystallisation

Solvent Extraction

Module 1

Distillation: Introduction: Batch and continuous distillation, separation of azeotropes,

Plate columns and packed columns

(9Hrs)

Module 2

Absorption: Introduction: Equipment- packed columns, spray columns, bubble columns,

packed bubble columns, mechanical agitator.

(9Hrs)

Module 3

Evaporation: Introduction: Equipment- short tube (standard) evaporator, forced circulation

evaporators. Falling film evaporators. Climbing film(upward flow)evaporators, wiped(agitated)film

evaporators.

(12Hrs)

Module 4

Filtration: Introduction: Filter media and filter aids, Equipment- plate and frame filter press, nutch

filter, rotary drum filter, sparkler filter, candle filter, bag filter, centrifuge

Drying: Introduction: free moisture, bound moisture, drying curve, Equipment- traydryer, rotary

dryer, flash dryer, fluid bed dryer, drum dryer, spray dryer.

(12Hrs)

Module 5

Crystallization: Introduction: solubility, super saturation, nucleation, crystal growth,

Equipment- tank crystallizer, agitated crystallizer, evaporator crystallizer, draft tube crystalliser.

(12Hrs)

References:

1. W.L.Badger and J.T.Bachero, Introduction to Chemical Engineering, Tata

McGraw Hill, U.S.A

2. W.L.McCabe and J.C.Smith,Unit operations in Chemical Engineering, Tata

McGraw Hill N.Y

3. J.H.Perry, Chemical Engineering Hand Book, McGraw Hill, N.Y

4. D.D.Kale, Unit Operations – 1 and 2, Pune Vidyarthi Griha Prakashan, Pune

108

CH3VOT04: Unit Processes in Organic Chemicals Manufacture

Credits-3 (54 Hrs)

Aim

To provide an understanding of some important unit processes in organic chemicals manufacture

Objectives

To study unit processes such as:

Nitration

Halogenation

Sulphonation

Oxidation

Hydrogenation

Esterification

Amination

Module 1

Nitration: Introduction: Nitrating agents, mechanism of nitration processes such as nitration of (a)

Paraffinic hydrocarbons(b)Benzene to nitro benzene and meta di nitro benzene (c) Chlorobenzene to

o- and p- nitrochlorobenzene. (8Hrs)

Module 2

Halogenation: Introduction: mechanism of halogenation reactions, reagents for halogenation,

Halogenation of aromatics- side chain and nuclear halogenations. Chloral, mono chloroacetic acid and

dichlorofluoromethane. (8Hrs)

Sulphonation: Introduction: Sulphonating agents, chemical and physical factors in sulphonation.

Mechanism of sulphonation reaction. Commercial sulphonation of benzene and naphthalene.

(8Hrs)

Module 3

Oxidation: Introduction – types of oxidation reactions. Oxidizing agents. Mechanism of oxidation of

Organic compounds, Liquid phase oxidation, Vapour phase oxidation. Commercial manufacture of

benzoic acid and acetic acid. (6Hrs)

Hydrogenation: Introduction, Catalysts for hydrogenation reactions, Hydrogenation of vegetable oil,

Manufacture of methanol from carbon monoxide and hydrogen, hydrogenation of acids and esters to

alcohols, catalytic reforming. (9Hrs)

Module 4

Esterification: Introduction, esterification by organic acids, by addition of unsaturated compounds,

esterification of carboxylic acid derivatives, commercial manufacture of ethyl acetate, dioctyl

phthalate, vinyl acetate, cellulose acetate.

(7Hrs)

Module 5

Amination By reduction: Introduction, Methods of reduction- metal and acid, catalytic, sulphide,

electrolytic, metal hydrides, sodium metal, concentrated caustic oxidation, reduction. Commercial

manufacture of aniline and meta nitro aniline. (8Hrs)

Reference:

1. P.H. Groggins, Unit Process in Organic Synthesis, McGraw Hill, N.Y

109

SEMESTER IV

CH4VOT05:Instrumental Methods of Chemical Analysis-I

Credits-3

(54 Hrs)

Aim

To give an understanding of the principle and instrumentation of different instrumental methods of

chemical analysis

Objectives

To study the principle and instrumentation of UV-Visible and IR spectrophotometry.

Spectrofluorimetry, Atomic Absorption Spectrophotometry, Different Electroanalytical techniques

Module 1

Principles of Instrumentation

Characteristics of measurement system: Introduction- Functional units –

Classification(automatic/manual type, self operated/power operated, analogue/digital)-Performance

characteristics (Static/dynamic characteristics) –Zero order instrument and first order instrument

Signal and noise- types of noises- chemical noise- instrumental noise -thermal-shot –flicker and

environmental noise-S/N ratio and its significance- techniques for S/N enhancement – hardware and

software methods.

Transducers – characteristics of transducers, sensitivity and transfer function- some typical examples.

Photo emissive- photo conductive and photovoltaic systems- photomultiplier and photo diode.

(14 Hrs)

Module 2

Typical Analytical Instruments -1

Spectrophotometry : Interaction of electromagnetic radiation with matter- classification of methods-

Beer Lambert law- Deviation from Beer Lambert law.

UV- Visible spectrometry: Origin of absorption spectra, components of typical instrument – Source-

Tungsten filament lamp, Hydrogen and Deuterium discharge lamps.

Wavelength selectors- filters, prisms and grating -Sample cell - Detectors

Single and double beam spectrophotometers

I.R spectrophotometry: classification of the types-Sources – Nernst glower, globar, Nichrome wire-

Wavelength selectors-Sample cell – characteristics- sample preparation-solvent selection-Detectors –

thermal, pneumatic and pyroelectric-NDIR instruments

(16Hrs)

Module 3

Typical Analytical Instruments -2

Molecular fluorescence: spectrofluorimetry – factors affecting fluorescence –typical instrumentation

Atomic spectroscopy: (1) AAS – Principle- typical instrumentation –Flames, Nebulisers-burner

system- Non flame techniques-Resonant line source –HCL and EDL- source modulation- sample

preparation- Interference in measurements

(2) AES: Excitation techniques- arc, spark and ICP

Sampling: Basis of sampling- sampling procedure- Importance of representative sampling- sample

preparations of solid, liquid and gaseous analytes- Hazards in sampling.

(12Hrs)

Module 4

Electro Analytical Instrumentation

(1)Potentiometric methods: Principle- technique and detection limit

(2)Non Potentiometric methods:(a) Conductometry (b) Polarography (c) Amperometry

110

(d)Anodic stripping analysis (e) coulometry (primary and secondary)

(12Hrs)

References:

1. Jeffry,Basset, Mendhem,R.C Denwy,Vogel’s Text Book of Quantitative Inorganic

Analysis, 4th&5thEdition

2. Skoog and Leary, Principles of Instrumental analysis,4 th Edition, Sanders College Publishing

3. D.Patranabis, Principles of Industrial Instrumentation, 2nd Edition , Tata McGraw-Hill

Company, Delhi.

111

Semester IV

CH4VOT06: Instrumental Methods of Chemical Analysis-II

Credits-3 (54 Hrs)

Aim

To give an exposure to process instrumentation

Objectives

To study:

The principle, construction and working of devices for the measurement of temperature and pressure

The principle and instrumentation of Column, Paper, Thin- layer and Gas Chromatography

The working of microprocessor based instruments. The use of computers in chemistry

Module 1

Process Instrumentation

Difference between Process Instrumentation and Laboratory Instrumentation- concept of

measurement and accuracy

Principle, construction and working of following measurements

(1)Temperature: Glass thermometers- bimetallic thermometers- pressure spring thermometers- vapour

filled thermometers- resistance thermometers- radiation pyrometers

(2)Pressure: Manometers- barometers -Bourdon pressure gauge- bellow and diaphragmtype gauges-

Mc Cleod gauge - Pirani gauge, Electrical pressure transducer (Linear Variable Differential

Transformer type)

(12Hrs)

Module 2

Chromatography: General aspects of chromatography- Classification: Adsorption, Partition, Ion

exchange, Gel permeation and molecular sieving

Column chromatography: Construction and operation of column- choice of adsorbents and eluents,

methods of detection. Derivatisation- HPLC equipment-

Thin layer and paper chromatography: Different techniques- typical examples- Ion exchange

chromatography and Ion chromatography.

Gas chromatography: principle- types of carrier gases- stationary phases- different types of columns-

capillary columns- temperature programming- Typical detectors- TCD, FID and ECD

(12 Hrs)

Module 3

Microprocessor Based Instruments

Telemetry: Pneumatic- electrical (voltage telemetering)- frequency telemetering, multiplexing-

Modulation of digital data- transmission channels- fibre optics.

(15Hrs)

Module 4

Use of Computers in Chemistry

Introductory concepts of Hardware and Software- ALU- CPU- Algorithm- Flow chart etc

Fundamentals of C programming-

Data types- int, float ,char ..

Functions in C (main (),Input/Output functions, getchar(), putchar(), getch()….)

Standard library functions in C

Looping

Conditional operators like – if else, do while, switch break

File handling concept

Simple programs (Use of arrays and pointers not expected)

112

To calculate rate constant of first order reactions (Kinetics)

To calculate interplanar distance in crystals (crystallography)

To classify atoms into Fermions and bosons (Atomic structure)

(15Hrs)

References:

1. Byron Gottfried, Programming with C, 2ndEdition,Tata McGraw Hill

2. P. Balaguruswami, Programming with ANSI C, Tata McGraw Hill

3. K. V. Raman, Computers in Chemistry

4. D. P. Eckman, Industrial Instrumentation, John Wiley &Sons

5. D. Patranabis, Principles of Industrial Instrumentation, 2ndEdition , Tata McGraw-Hill

Company, Delhi.

6. Skoog and Leary, Principles of Instrumental analysis,4thEdition, Sanders College Publishing

Further Reading

1. Willard, Merrit, Dean &Settle- Instrumental Methods of Analysis,C.B.S Publishers, 4thEdition

2. J.G.Dick, Analytical Chemistry, McGraw Hill

Semester (III&IV)

CH4VOP02:Practical-II

Credits-2 (72 Hrs)

1 .Unit Process: ( 12 experiments )

One or two examples for each of the following unit process: Nitration, sulphonation, esterification,

hydrolysis, oxidation, halogenations, reduction, polymerisation

2. Determination of acid value, saponification value, and iodine value of oil.

3. Depression and elevation in boiling /melting point of solids and liquids

4. Chromatography-Column, paper and thin layer

113

CH4VOP03:Practical-III

Credits-2 (72 Hrs)

1.Instrumental methods of analysis: use of colorimeter, pH meter, potentiometer, conductometer,

refractometer, polarimeter.

2. Determine the amount of base NH4OH conductometrically by using strong acid.

3. Determination of neutralizing capacity of any antacid tablet- alkali content using HCl.

4. Determination of flash point and ignition point of liquids

5. Titrimetry – Estimation of acetic acid contents in vinegar sample

6. Determination of viscosity of oils – Ostwald viscometer.

7. Critical solution temperature – Phenol-water system.

References:

1. D. A. Skoog, D. M. West, and S. R. Crouch, Fundamentals of Analytical Chemistry 8th edn,

Brooks/Cole Nelson .

2. Vogel’s Textbook of Quantitative Chemical Analysis 6th edn, Pearsons Education Ltd.

3. G. D. Christian, Analytical Chemistry, John Wiley and Sons.

4. R. D Day, A.L. Uderwood, Quantitative analysis,6th Edn.,Prentice Hall of India Pvt. Ltd

5. D.D Despande, Physical Chemistry of macromolecules, Vishal Publication, New Delhi.

6. J.B.Yadav, Advanced Practical Physical Chemistry, Goel Publishing House.

114

Model III. BSc PETROCHEMICALS

Semester- 1 CH1OCT01: PETROLEUM GEOLOGY

Credits- 3 (72 hrs)

Aim: The aim of the course is to give an insight into the origin and exploration of petroleum.

Objectives :-

To study: Theories regarding the origin of petroleum.

Methods of exploration, drilling, storage and transportation of crude oil.

Module 1.

Theories of origin of petroleum-biogenic (organic) and abiogenic (inorganic) theory.

Differences between biogenic and abiogenic theory. Berthelot’s view, Mendeleeff’s view,

Engler’s theory and modern theory.

Establishment of Source Beds- nature of source material- transformation of organic matter

into petroleum- accumulation in Reservoir sediments- in situ transformation of petroleum-

thermal alteration-deasphalting - biodegradation and water washing. (16 hrs)

References

1. Speight G James, Marcel Dekker, The Chemistry and Technology of Petroleum , Inc 1991

2. A. I. Levorsen, Geology of Petroleum, second edition, CBS publishers.

3. Hunt J M, Petroleum Geochemistry and Geology,1996,2nd Edn WH Freeman, San

Francisco..

4. Richard C Selly, Elements of Petroleum Geology, Academic press, London.

5. Dr.KochuBaby Manjooran, Modern Petroleum Chemistry –An Overview

Module 2

Resource and reserves—proved, unproved, probable, possible and undiscovered reserves.

Geological framework of migration and accumulation. Concept of hydrocarbon migration

from source bed to the carrier beds—carrier beds to reservoir. Mechanics of entrapment of

hydrocarbon—traps in the path of migration-entrapment and accumulation of hydrocarbon.

Classification and types of traps-structural, statigraphic and combination type of traps.

Genesis of various types of Traps—Anticlinal theory-traps caused by faulting- traps caused

by fracturing.

(18 hrs)

References


2. A. I. Levorsen, Geology of Petroleum, second edition, CBS publishers.

3. Hunt J M, Petroleum Geochemistry and Geology,1996,2nd Edn WH Freeman, San

Francisco..


5. Dr.KochuBaby Manjooran, Modern Petroleum Chemistry –An Overview

Module 3

Oil Exploration methods- geophysical exploration---magnetic method, gravimetric method ,

seismic survey Borehole logging-electrical method---radio active method, density- Core

115

sampling. Drilling operations. Recovery of oil - natural method (primary oil recovery)—

dissolved gas drive— gas cap drive, water drive, gravity drive- secondary methods. Other

source of petroleum. Petroleum from coal, natural gas and its constitution.

Elemental analysis of crude oil, hydrocarbon compounds, non -hydrocarbon compounds in

crude oil, metallic constituents.

(18hrs)

References

1. Wiley Critical Content, Petroleum Technology volume 1, John Wiley and sons, New

Jersey.

2. Dr KochuBaby Manjooran, Modern Petroleum Chemistry –An Overview

Module 4

Transportation and storage of crude oil: Crude transportation and product transferring. Type

of storage tanks - Cone roof and floating roof, nitrogen blanketing, truck and tankers, LPG

bullets. Pipe line transfer, Rail way. Crude Reservoirs .Indian resources of petroleum

Function of refineries: simple refinery, complex refinery, integrated refinery- sweetening

process , stripping, distillation procedures, heat exchangers-separation of products from crude

oil, reduced crude oil ,vacuum distillation- Composition of different distillates. (20hrs)

References


2. Tripathi G.N ,Indian Petroleum Directory , Indian Petroleum Publishers

3. Asphalt hand book, Manual series , Asphalt institute 1989

4. W.L.Nelson ,Petroleum refining engineering, Mc.Graw Hill

5. R.A.Meyers ,Handbook of petroleum refining process

6. B.K Sharma ,Industrial Chemistry, Goyal Publication

7. Sukumar Maiti ,Introduction to Petrochemicals

8. D.S.J Jones ,Elements of Petroleum Processing

9. Dr.KochuBaby Manjooran ,Modern Petroleum Chemistry –An Overview

10. R.A.Meyers ,Handbook of petroleum refining process

11. B.K Sharma ,Industrial Chemistry, Goyal Publication

12. D.S.J Jones ,Elements of Petroleum Processing

13.Hunt J M, Petroleum Geochemistry and Geology,1996,2nd Edn WH Freeman, San

Francisco..


116

Semester- 2

CH2OCT02: Test Methods and Petroleum Processes Credits- 3 (72 hrs) Aim: the aim of the course is to provide an account of some important quality parameters of

crude oil fractions and also some important chemical modifications of petroleum fractions

Objectives :-

. To study: Important quality parameters of crude oil fractions

Cracking and reforming of petroleum

Characteristics of aviation fuel

Physical properties of bitumen

Module 1

Type of hydrocarbon fuels and its characteristics. ASTM methods of product testing.

Specifications for various fuels. Detailed study of

Naphtha, LPG ,Gasoline, Kerosene, Diesel, Fuel oils , Bitumen ,Rubberized bitumen and

bitumen emulsion (15 hrs)

Module 2

Introduction – Significance –effect of blending and illustration of the following: Pour point,

Cloud point , Cetane number ,Pour point Depressants

Octane number and octane boosters, Distillation, viscosity and its reducers

Flash point ,copper corrosion, calorific value, Reid vapour pressure, Aniline point, Diesel

index. Detailed study of Abel and PMC method.

Doctor solution and its uses. API gravity, existent gum and potential gum. (20 hrs)

Module 3

Evaluation of Bitumen: Elastic recovery, ductility, softening point, penetration test.

Aviation fuels: Different types of Aviation fuels .and analysis; silver corrosion , WSIM,

JEFTOT ,anti oxidants, static electricity reducers, final boiling point, total sulphur,

mercaptans, lubricity, smoke point freezing point, calorific value

Manufacture of gasoline by cracking, antiknock performance, research octane number, motor

octane number, road octane number (15 hrs)

Module 4

Cracking operations :Different types of cracking. Thermal cracking of petroleum products,

thermal cracking of vacuum gas oil. Types of thermal cracking: mixed phase cracking ,

vapour phase cracking, selective cracking, visbreaking. Catalytic cracking-Commercial

processes. Feed stocks of catalytic cracking, process variables of cracking. Catalysts for

cracking. Hydro cracking, hyro processing. Comparison of hydro cracking and hydro

treating. Hydro forming , plat forming, uniforming, ultra-forming, auto forming. Catalysts for

hydro cracking. Reforming: Thermal reforming, catalytic reforming , fixed bed reforming,

hyperforming. Isomerism . Hysomer process. Penex process-Alkylation.

(22hrs)

References

1. ASTM Methods, Indian standards(Methods of test for petroleum and its Products,)

2. Speight G James, Marcel Dekker ,The chemistry and technology of Petroleum ,Inc 1991

3. Tripathi G.N, Indian Petroleum Directory , Indian Petroleum Publishers

4. Asphalt hand book, Manual series , Asphalt institute 1989,

117

5. W.l. Nelson, Petroleum engineering .

6. B.K. Sharma ,Industrial Chemistry

7. Navid Nader Pow ,Petrochemical Production Process, S.B.S Publishers

8. Dr.KochuBaby Manjooran, Modern Petroleum Chemistry

(Semester I and II)

CH2OCP01: Practical -I Credits- 2 (72 hrs)

1.Determination of softening point

2.Determination of penetration of bitumen

3.Determination of Ductility of Bitumen

4.Determination of Aniline point of diesel fuel

5.Determination of Diesel Index

6.Distillation of Petrol

7.Distillation of Kerosene

8.Distillation of Diesel

9.Determination of water content in diesel –Dean Stark Method

10.Determination of water content in furnace oil- Dean Stark Method

Reference:

ASTM Methods, Indian standards(Methods of test for petroleum and its Products,)

118

Semester 3

CH3OCT03:Production and Application of Compounds from Petroleum Credits-4 (72 hrs)

Aim: The aim of this course is to give an account of the methods of preparation and

applications of some important petrochemicals

Objectives:

To study:

Manufacture of sulphur, hydrogen, petroleum coke and nitrogen compounds

Ammoxidation, hdroformylation and hydration reactions.

Manufacturing processes of ethylene, acetylene ,propylene and higher olefin.

Manufacture and processing of plastics

Module 1

Manufacture of sulphur from underground --Freush process--From hydrogen sulphide

Partial oxidation method and Engineering problems-- Hydrogen --Properties--hydrogen as a

fuel--- manufacture of hydrogen from naphtha cracking,--From hydrocarbons by partial

oxidation.-- Petroleum coke--Uses-manufacture by Hot oven method---thermal cracking---

fluidized coking--- Delayed coking--- and Nitrogen compounds in petroleum. Nitroparaffins-

-Nitro ethane---I nitro propane---2nitropropane.--manufacture of nitrogen compounds from

petroleum (24 Hrs)

Module 2

.Study of following reactions and applications :

Ammoxidation-- Applications of ammoxidation --.preparation of acrylonitrile-- Terephthalic

acid by ammoxidation -Lummns process—Hydroformylation ---oxo process--Modifications

of oxo process --Uses of oxo process—Hydrogenation-- Aldex process--Aldol condensation--

-oxidation-- Hydration – categories of hydration--Clathrates-Applications of hydration---

preparation of ethyl alcohol--Isopropyl alcohol—acrylamide( Dow chemical process)--

Acetaldehyde--Oxidation-type of oxides--Classification of oxides--application of oxidation in

petroleum compounds.---union carbide process --weaker process

(24 Hrs)

Module 3

Steam naphtha cracking of Hydrocarbons:

Manufacture of Ethylene--- Acetylene—Propylene-- Higher olefins from naphtha-- Process--

economics .(present day procedures and its economics) (12 hrs)

Module 4

Polymers: Classification- Addition and Condensation polymerisation – Examples.

Plastics: Properties—uses-thermoplastics- thermosetting plastics - moulding constituents of a

plastic-moulding of plastics into articles- compression moulding-injection moulding-transfer

moulding—extrusion moulding—engineering plastics. (12 Hrs)

References:-

1. W.L. Faith, Donald B Keyes, Ronald L Clark, Industrial Chemicals.

2. Speight G James, Marcel Dekker Inc 1991,The chemistry and technology of Petroleum

3. Tripathi G.N, Indian Petroleum Directory

4. B.K Sharma , Industrial Chemistry and Chemical Engineering ,Spits Petrochemicals-Wiley

5. A.L Waddan , Chemicals from petroleum

6. l.F Hatels and S. Mater Gulf, From Hydrocarbons to Petrochemicals

7. Jain an d Jain, Engineering chemistry

8. Navid Nadar Pow , Petrochemical production process

119

9. H Steiner ,Introduction to petrochemicals

10. Rakesh Rati, Petrochemical refining process

CH3OCT04: Manufacture of Petrochemicals-I Credits-3 (54 hrs)

Aim: To make the students aware of the methods of manufacture and uses of some of the

important petrochemicals.

Objectives: To study the manufacturing methods and uses of: Methanol, carbon black,

chlorinated methane, and hydrogen cyanide from methane and natural gas Ethyl chloride,

ethanol, ethanolamines, ethylene oxide, acrylonitrile, vinyl acetate, styrene, ethylene

glycol,acetaldehyde and acetic acid from ethylene.

Module 1

Manufacture from Natural gas

Methanol-properties and uses- manufacturing methods –catalytic hydration method.-side

reactions, Carbon black-uses and properties-Channel black-Furnace black(gas and oil)-

thermal black-Acetylene black-manufacture, Hydrogen cyanide-uses and properties-

manufacture by Andrew sons process-By Degusser process, Shawnigan process

(14hrs.)

Module 2

Manufacture from Methane

Chlorinated methane-uses ,Manufacture of methyl chloride-methyl dichloride-Chloroform-

carbon tetra chloride, carbon disulphide –uses- manufacture by Thacker process –Acetylene-

uses-manufacture by sachse process-wulf process (13 Hrs)

Module 3

Manufacture from Ethylene

Ethyl chloride-uses-manufacture by hydrochlorination ,Ethanol-Different process of

manufacture-uses-manufacture by catalytic hydration-, Ethylene oxide –uses and properties-

Manufacture by oxidation ,Ethanolamines- monoethanol amine - diethanol amine-triethanol

amines--uses- manufacture- Engineering problems

Ethylene glycol-uses-Different methods of preparation-Manufacture through chlorohydrin-

Manufacture by oxidation. (13hrs)

Module 4

Manufacture from Ethylene

Acetaldehyde-Process of manufacture- recent advances-uses-., Acetic acid-Uses and

manufacture by oxidation, styrene-uses-manufacture-by benzene-Purification--

Vinyl acetate-uses and manufacture by acetic acid and oxygen-- Vinyl chloride-uses-

manufacture by thermal pyrolysis- Acrylonitrile- uses and Manufacture by ethylene oxide

and hydrogen cyanide (14Hrs)

References:-





5. ASTM Methods, Indian standards

6. Sukumar Maiti ,Introduction to Petrochemicals

120

Semester 4

CH4OCT05: Manufacture of Petrochemicals -II Credits -4 (72 hrs)

Aim: To make the students aware of the methods of manufacture and uses of some

industrially important chemicals from petroleum.

Objectives: To study the methods of manufacture and uses of of the following petrochemicals

Isopropanol, cumene, glycerine and acrylonitrile from propylene Vinyl chloride

acetaldehyde, chloroprene, and acrylonitrile from acetylene Butadiene and benzene from C- 4

hydrocarbons Benzene, toluene, xylenes, naphthalene, linear alkyl benzene, detergents and

synthetic fibres.

Module 1

Manufacture from propylene

Isopropanol---uses-properties-manufacture by hydration method-- Cumene-uses-

manufacturing methods- Propylene-alkylation method,---Glycerin uses-natural glycerin

synthetic glycerin--manufacture by allyl chloride-- manufacture via acrolein--- Acrylonitrile -

- uses-- manufacture by amoxidation method (16 Hrs)

Module 2

Manufacture from Acetylene

Vinyl chloride-uses-manufacture-engineering problems-economics-- Acetaldehyde-uses-

properties-hydration of acetylene-hydration solutions-process of manufacture--- Chloroprene

–uses- Neoprene- manufacture,---Acrylonitrile –uses-properties-manufacture by hydrogen

cyanide process---disadvantages.

Acrylic acid- Reppe’s synthesis. Vinylacetate, acetone, Trichloroethylene, Perchloro

ethylene, vinyl ether and acetonitrile (method of production only)

(18Hrs)

Module 3

Manufacture from C-4 hydrocarbons and BTX aromatics

Butadiene-uses-occurrence-methods of preparation-manufacture by Houdry Process---

Benzene-uses –manufacture by hydrodealkylation--- C-4 oligomers.

BTX aromatics –Principal sources-Benzene-Toluene-Xylenes-uses -manufacture

Naphthalene-uses-sources-manufacture by hydrodealkylation, Linear alkyl benzene-General

reactions-side reactions-manufacture. (20hrs)

Module 4

Synthetic Fibres and Detergents-Production techniques of synthetic fibres-melt spinning, dry

spinning and solution (wet) spinning. Polyesters, Polyethylene terephthalate (PET) from p-

Xylene ,Poly carbonates, poly amides-Nylon6,Nylon6,6-Acrylic fibres (Orlon)- manufacture.

Synthetic paper-advantages over conventional paper- method of preparation.

Classification of detergents-uses of detergents-surfactants-additives-manufacture-cleaning

action of detergents. Difference between soap and detergents. LAS and ABS detergents.

(18hrs)

References:-






6. Sukumar Maiti, Introduction to Petrochemicals

7. Dr. BK Baskara Rao- A text book on petrochemicals, Khanna publishers, Delhi.

121

CH4OCT06: Petroleum Industries in India Credits-3 (54hrs)

Aim:. To create awareness among students about the petroleum industries in India

Objectives: To study:

Catalysts in petroleum industry

Petroleum and petrochemical industries in India.

Energy crisis and petrochemical industries.

Module 1 Energy crisis ---coal as an alternative to oil-Hydrogen- fuel of tomorrow-

advantages –non-conventional sources of energy—solar energy—bio gas-advantages-tidal

energy –geothermal energy-wind energy—nuclear fuels (general study only)

(8hrs) (8 Hrs)

Module 2

Importance of Petroleum and petrochemical industry in the contest of Indian economy –

general cost-capital cost-production cost-R&D economics-

Major govt oil companies engaged in refining and marketing petroleum, Function of ONGC.

Indian petrochemical industry –Difficulties encountered in Indian petro chemical industries.-

Public sector and private sector –Petroleum conception pattern

Indian reserves, Developments in petrochemical industry -developments in quality of

petroleum fuels and future –Future of petrochemical industry.

(16hrs)

Module 3

Catalysts in petroleum industry –General properties-classification—catalytic activity-

catalysts in refining process-Reforming catalysts-hydro treating catalysts-catalysts in petro

chemical industry-Ziegler catalyst-preparation-properties-disadvantages-miscellaneous

polymerization catalysts- recent advances in catalysts-Role of polymers in catalysts-enzyme

catalysts- preparation, structure, selectivity and application.

(18hrs)

Module 4

Pollution from petroleum industry—refinery pollution-water pollution—air pollution-sea

water pollution-effect of oil pollution- physical and chemical—control methods--

environmental protection-- National standards of air and water pollution

(12 Hrs)

References:-


2. Trimn , Catalysts in petrochemical refining

3. Jain and Jain, Engineering Chemistry



6. Sukumar Maiti, Introduction to Petrochemicals

122

CH4OCP02:Practical -II (Semester III and IV)

Credits-2 72 Hours

1. Determination of density of light oils

2. Determination of density of medium type oils

3. Determination of surface tension of kerosene

4. Determination of Viscosity of Diesel

5. Determination of Ried vapour pressure of petrol

6. Determination of Pour point.

7. Determination of Cloud point.

8. Determination of Flash point-PMC method.

9. Determination of Flash point-Abel’s method.

10. Determination of Smoke point of kerosene.

Reference: ASTM methods, Indian standards

123

MODEL QUESTION PAPERS

124

B.Sc. DEGREE (CBCS) EXAMINATION

Chemistry Core

SEMESTER I

CH1CRT01 GENERAL INORGANIC CHEMISTRY

(Common for the Programmes B.Sc. Chemistry Model I, Model II and B.Sc. Model III

Petrochemicals )

Time: 3 hrs Total marks-80

Section A

Answer any 9 questions. Each question carries 2 marks )

1. What is Photoelectric effect?

2. Distinguish between isotopes & isobars.

3. State the modern periodic law.

4. Write down the electronic configurations of nitrogen and sodium.

5. What is inert pair effect?

6. Draw the radial probability distribution curve of 1s orbital.

7. What is Heisenberg’s uncertainty principle?

8. Write Schrodinger wave equation and explain the terms involved.

9. Define ionic radius.

10. What are alloys? Give two examples.

11. Define common ion effect.

12. What are the possible values of l and m for n=3?

Section B

(Answer any six questions ,each question carries 4 marks)

13. Discuss the application of solubility product principle in inorganic qualitative

analysis.

14. Explain lanthanide contraction.

15. Give the preparation, properties& uses of potassium dichromate.

16. Discuss on the properties of the allotropes of carbon.

17. Which of the following species will have the largest &smallest size: Mg, Mg 2+, Al,

Al3+?

18. Explain the principle involved in the intergroup separation of cations.

19. Draw the shapes of 1s & 2p orbitals.

20. Calculate the effective nuclear charge of 4s &3d electrons in Zn atom?

21. Discuss the different electronegativity scales.

Section C

(Answer any three questions. Each question carries 6 marks.)

22. Explain the following statements with valid data: (a) Ionisation potential of nitrogen

is greater than that of oxygen, (b) Electron affinity of chlorine is more than fluorine.

125

23. What is meant by ‘interfering radicals’ ? Explain the principle and procedure for the

elimination of oxalate and phosphate.

24. Explain the catalytic properties of transition metals.

25. (a )Differentiate between molecular mass and equivalent mass, giving suitable

examples.

(b) Calculate the molality of a solution obtained by dissolving 2.5g of acetic acid in

75g benzene.

26. (a) Find the mass of the particle having a wavelength of 6.6 x10-4 cm and moving

with a velocity of 106cm/sec.

b) Calculate the product of uncertainties in position and velocity for an electron

of mass 9.1*10-31kg,

Section D

(Answer any Two questions. Each question carries 10 marks)

27. What are quantum numbers? Explain its significance.

28. Compare the properties of lanthanides and actinides.

29. (a)Give the postulates of Bohr’s atom model. What are its limitations?

b) How will you calculate the energy of an electron in hydrogen atom?

30. Describe the main features of long form of the periodic table.

126


Chemistry Core

SEMESTER II

CH2CRT02 CHEMICAL BONDING AND NUCLEAR CHEMISTRY


Petrochemicals )

Time: 3 Hrs Max. Marks: 80

Section A

(Answer any nine questions. Each question carries 2 marks)

1. Define octet rule.

2. Write Born-Lande equation and explain the terms.

3. State Fajan’s rule.

4. Write the resonance structure of carbonate ion.

5. Which is more stable O2 or O2+? Why?

6. What is the hybridization and shape of BeF2 molecule?

7. What are London dispersion forces?

8. Define percentage ionic character in a molecule.

9. What is spallation reaction? Explain.

10. Write the nuclear equation for the emission of alpha particle from Th-232.

11. The half life of Na-24 is 14.8 hours. Calculate its decay constant.

12. Name any two radioactive isotopes used in medicine.

(2x9=18)

Section B

(Answer any 6 questions. Each question carries 4 marks)

13. Define hybridisation. What are the characteristics of it?

14. Define dipole moment. Explain why the dipole moment of hydrogen halides

decreases from HF to HI.

15. Explain the terms polarisation, polaristability and polarising power.

127

16. Distinguish between Bonding molecular orbital and Antibonding molecular

orbital.

17. Discuss the structure, shape and hybridization in the molecule of ClF3.

18. State Group displacement laws. Explain the band theory of metals.

19. Define bond order. Calculate the bond order of N2 and O2 molecule.

20. Explain Geiger-Nuttal rule and the terms involved.

(6 x 4 =24)

Section C (Answer any 3 questions. Each question carries 6 marks)

21. Compare VB and MO theories

22. Explain the hybridisation and geometry of PCl3, PCl5 and SF6 molecules

23. Differentiate between Intermolecular and Intra molecular hydrogen bonding

with suitable examples. Also explain the effects of hydrogen bonding.

24. What is meant by artificial radioactivity? Give one example each for artificial

transmutation with proton, neutron and deuteron.

25. What are (a) synthetic elements (b) Radio carbon dating

26. Define binding energy. How is binding energy and mass defect related to

nuclear stability?

(3 x 6 =18)

Section D (Answer any 2 questions. Each question carries 10 marks)

27. Explain Born- Haber cycle with an example. What are the applications of

Born-Haber cycle?

28. (a)Discuss VSEPR theory. Using the theory assign the shapes of (i) XeF2 (ii)

XeF4 and (iii) XeF6 offering approximate explanation in each case.

29. (a) Draw the MO energy level diagram of CO molecule and explain its

properties. (b) He2 molecule does not exist. Why?

30. Write notes on: (a) preparation of transuranic elements. (b) Spallation reactions

and (c) Nuclear fission and fusion reactions and their applications.

128


Chemistry Core

Third Semester

CH3CRT03 BASIC ORGANIC CHEMISTRY – I


Petrochemicals )

Time: 3 Hours Maximum marks: 80

Section A


1. Differentiate between homolytic and heterolytic fission with suitable examples.

2. What is mesomeric effect?

3. Are SN2 reactions stereospecific or stereoselective? Justify.

4. Which is the order of stability of the following carbocations?

(CH3)3C+ ; + ; (CH3)2CH+

5. How is Grignard reagent prepared?

6. What is meant by conformation of a molecule? Represent the fully eclipsed conformation of

ethane.

7. What is Walden inversion? Explain.

8. What are reaction intermediates? Illustrate.

9. What is the role of light (or heat) in the halogenation of alkanes?

10. How do you explain the acidic nature of the C-H bond in acetylene?

11. Why do alkyl halides undergo nucleophilic substitution rather than electrophilic substitution?

12. What is Diels-Alder reaction?

(9 x 2 = 18 marks)

Section B

(Answer any six questions. Each question carries 4 marks)

13. What is hyperconjugation effect? How does it affect the properties and reactivity of a compound?

14. Tertiary butyl carbocation is more stable than isopropyl carbocation. Give reasons.

129

15. Discuss the optical activity of tartaric acid. Represent the meso-form of tartaric acid and explain

why it is optically inactive.

16. On which factors does the stability of conformations depend? Explain.

17. Differentiate between enantiomers and diastereomers with suitable examples.

18. What is 1,3-diaxial interaction? Explain with reference to methyl cyclohexane.

19. State and explain Huckel’s rule of aromaticity.

20. -CHO group in benzene is meta directing. Give reasons.

21. Acylation is always preferred to alkylation in Friedel-Crafts reaction. Explain.

(6 x 4 = 24 marks)

Section C

(Answer any three questions. Each question carries 6 marks)

22. What are the rules for assigning E or Z conformation to geometrical isomers? Assign the

configuration to trans-2-butene.

23. What is asymmetric synthesis? Discuss the different methods used for it.

24. State and explain Saytzeff’s and Hofmann’ rules with example for each.

25. Write briefly on non-benzenoid aromatic compounds.

26. Discuss the benzyne mechanism for nucleophilic aromatic substitution in aryl halides.

(3 x 6 = 18 marks)

Section D

(Answer any two questions. Each question carries 10 marks)

27. (a) Give the IUPAC names of: (i) Allyl alcohol (ii) Acrolein.

(b) How does inductive effective influence the acid and base strengths of organic

compounds?

(c) What are carbenes? How are they generated? Give a brief account of the structure

and shape of singlet and triplet carbenes.

28. Explain the Cahn-Ingold-Prelog rules for assigning R-S notations for optical isomers with suitable

examples.

29. Discuss the mechanism of addition of HBr to propene in the presence and in the absence of

peroxide. Also explain the rules involved in it.

30. Discuss the mechanisms of SN1 and SN2 reactions. Enumerate the differences between SN1 and

SN2 mechanisms. (2 x 10 = 20 marks)

130


Chemistry Core

Fourth Semester

CH4CRT04 BASIC ORGANIC CHEMISTRY - II


Petrochemicals )


Section A


1. Which is more acidic – Phenol or Alcohol. Why?

2. Suggest one method for the preparation of t-butyl alcohol.

3. What happens when ethylene glycol reacts with HIO4? Write the equation.

4. What is Fries rearrangement? Explain.

5. How will you prepare resorcinol?

6. What is iodoform reaction? Explain.

7. What is Hell-Volhard-Zelinsky reaction?

8. What is Claisen-Schmidt reaction?

9. Outline the method to estimate the number of methoxyl groups present in a compound.

10. Which is more reactive towards nucleophiles and why? Formaldehyde or Acetaldehyde.

11. How is phthalaldehyde obtained from naphthalene? Write the equation.

12. How will you convert methanol into ethanol?

(9 x 2 = 18 marks)

Section B


13. Give an example for Baeyer-Villiger oxidation with mechanism.

14. Draw the possible resonance forms of phenanthrene.

15. Explain the reactions of oxalic acid with glycerol. Also write the equations involved.

16. Convert acetic acid to:

(i) Ethyl ethanoate (ii) Ethanoic anhydride

(iii) Ethanamide (iv) Ethanoyl chloride.

17. How is citric acid formed by Reformatsky reaction? Write the products formed when citric acid is

heated.

18. What is Lucas test? Explain.

131

19. Carboxylic acid is acidic. Why? Discuss the effect of substituents on the acidity of aromatic

acids.

CH3

CO

SO2

NH . Give one property of the product.

Saccharin

20. Convert

21. Naphthalene on sulphonation gives 1-sulphonic acid at 400C; while 2-sulphonic acid at 1600C.

Explain.

(6 x 4 = 24 marks)

Section C


22. Phenol is acidic. Give reasons. Discuss the directive influence of –OH group in phenol towards

electrophilic substitution reaction.

23. What are Clemmensen and Wolff-Kishner reductions? Give their mechanism and one application

each in the case of aldehydes and ketones.

24. How is acetoacetic ester synthesised? Explain the keto-enol tautomerism of acetoacetic ester.

25. Write the mechanism of the following reactions:

(a) Perkin reaction (b) Dieckmann reaction.

26. Discuss the aromaticity of anthracene based on the structure.

(3 x 6 = 18 marks)

Section D


27. (a) Write the mechanism of Reimer-Tiemann reaction and Pinacol-Pinacolone rearrangement.

(b) Give one example for the preparation and reactions of epoxides.

28. Give one method of preparation with equations of the following compounds:

(a) Fumaric acid (b) Cinnamic acid (c) Malonic acid

(d) Adipic acid (e) Anthranilic acid.

29. Give three synthetic applications each of: (a) Malonic ester (b) Cyanoacetic ester.

30. Write the mechanism of the following reactions:

(i) Benzoin condensation (ii) Cannizzaro reaction

(iii) Wittig reaction (iv) Mannich reaction.

(2 x 10 = 20 marks)

132


Chemistry Core

SEMESTER V

CH5CRT05 ANALYTYCAL AND ENVIRONMENTAL CHEMISTRY

(Common for the Programmes B.Sc. Chemistry Model I, Model II and

B.Sc. Model III Petrochemicals )

Time: 3 Hrs Max.: 80 marks

Section A

Answer any nine questions

Each question carries 2 marks

1. Distinguish between molarity and molality.

2. What is meant by a primary standard? Give an example of a primary standard in volumetric

analysis.

3. Define solubility product.

4. What are redox indicators? Give an example.

5. Write down the expression for calculating standard deviation of a set of data.

6. Define Rf value.

7. What is the fundamental difference between DTA and DSC?

8. What is Green House Effect?

9. Explain the term ‘eutrophication’.

10. What is Minamata disease?

11. What are the constituents of photochemical smog?

12. Explain ‘glass transition temperature’.

(9×2=18)

Section B

Answer any six questions.

Each question carries 4 marks.

13. Differentiate between accuracy and precision.

14. Explain the causes and consequences of ozone layer depletion?

15. What are the advantages and disadvantages of liq. SO2 as a solvent?

16. Explain why solutions alkali metals in liquid ammonia are intensely coloured?

17. Discuss in details the various types of phosphorous based chain polymers.

18. Differentiate between COD and BOD.

19. Discuss the principle and method of complexometric titration by taking any one example.

20. What are chalcogenide glasses?

21. What are pH indicators? Give two examples and mention their applications.

(6×4=24)

Section C

Answer any 3 questions.

Each question carries 6 marks.

133

22. Discuss the structure, properties and uses of various types of silicone based polymers.

23. How COD of water samples determined? Explain the chemical reactions involved in the

procedure.

24. What is curve fitting? Using the principle of least squares, derive the equation for fitting a

straight line.

25. Briefly explain the principles of acid-base titration with the help of different titration curves.

26. Discuss the principle and applications of thermogravimetry.

(3×6=18)

Section D

Answer any 2 question.


27. Explain the unit operations in gravimetric analysis. Discuss the procedure for the gravimetric

estimation of iron in a solution of ferric alum.

28. Describe briefly the sources and environmental effects of air pollution due to oxides of carbon,

nitrogen and sulphur.

29. Discuss the merits and demerits of anhydrous HF as a non-aqueous solvent. Discuss briefly the

chemical reactions which take place in this solvent.

30. Explain the principle, experimental techniques and advantages of HPLC.

(2×10=20)

134


Fifth Semester

Chemistry Core

CH5CRT06 ADVANCED ORGANIC CHEMISTRY – I


Petrochemicals)


Section A


1. Write a chemical equation for electrolytic reduction of aromatic nitro compounds.

2. How would you distinguish between the following compounds using IR spectroscopy?

a) CH3OH and CH3OCH3 b) CH3COOCH3 and CH3CH2COOH

3. What is the use of nujol in IR spectroscopy?

4. Why are amines more basic than alcohols?

5. What is spin-spin splitting?

6. Write the resonance structures of diazomethane.

7. What are food colours? Name one permitted food colour.

8. Which one of the following decays of excited states takes place in fluorescence?

a) T2-T1 b) T1-S0 c) S1-S0 d) S2-S1

9. State the differences between photochemical reactions and thermal reactions.

10. What are antibiotics?

11. How many hertz does 1ppm corresponds to for a spectrophotometer operating at a

frequency of 60 MHz?

12. What is photosensitisation?

(9 x 2 = 18 marks)

Section B


13. What are singlet and triplet states?

14. Describe the action of phase transfer catalysts.

15. Why is TMS used as an internal standard in 1HNMR spectroscopy?

16. Write a short note on charge transfer complexes.

17. Explain Arndt –Eistert synthesis.

18. Is thiophene aromatic? Justify your answer.

19. Define the following terms with examples

a) Bathochromic shift b) Hypsochromic shift c) Chromophore

20. What is an azo dye? Give an example with structure.

21. What is the main use of Hinsberg test? Explain.

(6 x 4 = 24 marks)

135

Section C


22. Calculate the λmax of the following compounds:

23. Two isomeric compounds A and B have the molecular formulae C2H4Cl2. Compound

A gives one NMR signal as a singlet at δ=3.7, whereas B gives 2 signals, a doublet at

δ=2.1 and a quartet at δ=5.8. Assign the structure of compounds A and B.

24. Name the compounds A, B, C and D in the following reactions.

25. Explain structure-activity relationship of drug molecules with suitable examples.

26. Does N-methylbutylamine show optical activity? Validate your answer.

(3 x 6 = 18 marks)

Section D


27. (i) An organic compound C6H12O gave the following spectral information:

IR 1715cm-1; 1HNMR δ = 2 (3H singlet) and δ = 1 (9H singlet).

Suggest the structure of the compound.

(ii) Outline the synthesis of:

a) Alizarin b) Rosaniline c) Phenolphthalein d) Indigotin

28. Explain the reactions and uses of diazonium salts.

29. Write notes on:

a) Norrish Type-1 reaction b) Paterno-Buchi reaction

c) Photo-Fries reaction d) Jablonski diagram

30. Outline one synthesis each of Pyrrole, Pyridine, Indole, Quinoline and Isoquinoline

with equations.

(2 x 10 = 20 marks)

A Br2, NaOHB

H2OC

-CO2D

HClH3C NH3 Cl

136


Fifth Semester

Chemistry Core

CH5CRT07 States of Matter, Colloids and General Informatics


Petrochemicals )

Time: 3 Hours Max: 80 marks

Part A


1. Explain mean free path. How is it varies with pressure?

2. Define SMILES? Give an example.

3. Explain peptisation with one example.

4. Derive the Bragg equation for X-ray crystallography.

5. What are semiconductors? Explain what is meant by n- type and p- type conduction.

6. Give a short note on smectic and nematic liquid crystals.

7. Define Miller Indices. Sketch the (222) plane in a unit cell.

8. Give the Cp/Cv ratios of CO2 and SO2.

9. What is a point group? To which point group does the XeF4 molecule belong?

10. What is Meissener effect?

11. At what temperature will the root mean square velocity of O2 be same as that of SO2 at 27 oC?

12. Give a note on plagiarism.

(9x 2 = 18)

Part B


13. Write a note on liquefaction of gases? Give one method for Liquefaction of gases.

14. What are liquid crystals? How are they classified? Describe the applications of liquid crystals.

15. Give the purification techniques of colloids.

16. Give the viscosity determination by Ostwald’s viscometer and explain using the Poisuelle’s

equation.

17. Discuss Maxwell’s distribution of molecular velocities with equation. Illustrate the effect of

temperature on this distribution.

18. Explain the different types of defects in crystals.

19. Describe the elements of symmetry.

20. Differentiate between hexagonal close packing and cubic close packing in detail.

137

21. What are the basic concepts of IPR?

(6 x 4 = 24)

Part C


22. Explain critical phenomenon on the basis of isotherm of CO2 gas and give the continuity of

state.

23. Discuss the BET theory of multilayer adsorption. How is it used to determine the surface area

of the adsorbent?

24. Give the group multiplication table of C2V. Determine the point group of NH3 and BF3

molecules .

25. HgCl2 crystallizes in orthorhombic system. Using radiation with λ = 154pm, the (100), (010)

and (001) reflections (first order) from HgCl2 in an X-ray diffractometer occur at 7o25’, 3o28’

and 10o23’, respectively. If the density of the crystal is 5.42 g cm-3, calculate the dimensions

of the unit cell and the number of HgCl2 molecules in the unit cell. M(HgCl2 = 271.5 g mol-1)

26. At 27oC and 1 atm pressure, the coefficient of viscosity of nitrogen gas is 178µP. Calculate

(a) the mean free path λ and (b) the collision diameter d of nitrogen molecule using the

Chapman equation.

(3 x 6 = 18)

Part D


27. Derive van der Waal’s equation for n moles of a gas. Deduce van der Waal’s equation in

virial form and how can this used to determine the Boyle temperature.

28. (a) Describe the powder method for the study of crystal structure.

(b) Discuss the powder diffraction pattern of NaCl and correlate it with its crystal structure.

29. What are colloidal solutions? Explain its properties and applications.

30. What are the postulates of the kinetic molecular theory of gases? How would you justify these

postulates? Based on the postulates, derive the kinetic gas equation?

(2 x 10 = 20)

138

B.Sc DEGREE CBCS EXAMINATION

Fifth Semester

Chemistry Core

CH5CRT08 Quantum Mechanics and Spectroscopy


Petrochemicals )

Time: Three hours Total marks: 80

Section A

(Answer all the questions. Each question carries 2 marks)

1. What is the significance of Born-Oppenheimer approximation?

2. Sketch the normal modes of vibration of H2O molecule.

3. Which are more intense spectral lines: - stokes lines or antistokes lines? Why?

4. What is Born’s interpretation of wave function?

5. Explain photoelectric effect.

6. Draw the MO diagram of C2 molecule.

7. What is Beer- Lamberts law?

8. What is meant by quantum yield of a photochemical reaction?

9. Calculate the de Broglie wave length of electron that has been accelerated through a

potential difference of 100 V.

10. Define overtones and hot bands in IR spectra.

11. Explain chemiluminescence with an example.

12. What do you mean by hyperfine splitting in esr?

(9x2=

18)

Section B


13. What is meant by selection rules in spectroscopy? Give the selection rules for Raman

spectra.

14. Explain the concepts of group frequencies and finger print region in IR spectroscopy.

15. Elaborate the rule of mutual exclusion of IR and Raman spectra.

16. Describe the effect of conjugation on the electronic spectra of conjugated molecules.

17. Explain the term shielding of protons in NMR spectroscopy with a suitable example.

18. Show that eikx is an eigen function of the operator d/dx. Also show that 𝑒𝑘𝑥2 is not an

eigenfunction of the operator d/dx.

19. What is (i) a well behaved wave function (ii) a normalized wave function?

20. Define Compton Effect? How it provides evidence for the corpuscular nature of

radiation.

21. What are quantum numbers? Give the significance of magnetic quantum number.

139

(6x4=24)

Section C


22. The microwave spectrum of HCl consists of a series of equally spaced lines separated

by 20.86 cm-1. Calculate the bond length of HCl.

23. Draw the Jablonski diagram and explain fluorescence, phosphorescence and non-

radiative processes.

24. Draw and discuss the high resolution proton NMR spectrum of acidified ethanol.

25. Calculate the frequency of light emitted when an electron jumps from the first excited

state of butadiene to its ground state using particle in a box approximation. Given that

the length of the carbon chain in butadiene is 578 pm.

26. Explain the terms radial distribution function and radial distribution curves. Draw the

radial distribution curves for 1s, 2s and 2p orbitals of hydrogen atom.

(3x6=18)

Section D


27. State and explain the postulates of quantum mechanics.

28. Discuss the rotational spectra of diatomic molecules and show that the spectral lines

are equally spaced.

29. (a)Elaborate the construction of molecular orbital by LCAO method for H2+ ion.

(b) Compare and contrast σ ,σ *,π , π* molecular orbitals.

30. a) Explain the quantum mechanical treatment of Raman Effect.

b) Discuss Frank Condon principle.

(2x10=20)

140


Fifth Semester

Chemistry-Generic Elective

CH5GET01 NOVEL INORGANIC SOLIDS

Time: 3 Hours Max: 80 Marks

Section A


1. Distinguish between solid-solution co-precipitation and adsorption-occlusion co-

precipitation.

2. Differentiate between cationic and anionic solid electrolytes with suitable example.

3. Name one white pigment and black pigment of titanium.

4. Give any two applications of hydroxyapatite.

5. What you meant by natural nano crystals. Give one example.

6. What are the important structural methods for characterizing nano materials?

7. Give the different phases in Ni- based super alloy.

8. ‘Duralumin alloy is widely used for stressed structures in aircraft’. Why?

9. Give one similarity and one difference between Brass and Bronze.

10. What are the important allotropic forms of TiO2 composite

11. With suitable example briefly explain what you meant by intermetallics

12. Classify the following materials in to Neutral, Acidic and Basic refractory:

(A) - Graphite, (B) - Silica, (C) - China clay, (D) - Zirconia

(9x2=18)

Section B


13. Distinguish between Nematic and Smectic phases of liquid crystals.

14. Discuss briefly the important methods for the fabrication of nano wires.

15. What are the important characteristics of cutting-tool materials?

16. Differentiate between thermoplastics and thermosetting plastics with suitable example.

17. What you meant by primary and secondary phases in a composite?

141

18. Give the important applications of Whisker reinforced metal matrix composites (MMCs).

19. List out major metallurgical enhancement of MMCs compared to unreinforced materials.

20. Certain borides and nitrides are widely used as ceramics. Explain this with suitable

examples

21. Write a note on Refractory carbides.

(6x4=24)

Section C


22. Discuss the structure and properties of Buckminster fullerenes.

23. Write briefly on mild steel, medium steel and high carbon steel.

24. Describe the distinctive features of a self assembled nano structures.

25. With suitable chemical equation briefly describe the preparation of gold nano particles.

26. Explain briefly the important properties and applications of ceramics.

(3x6=18)

Section D


27. Explain the various methods employed for the synthesis of inorganic solids.

28. Discuss briefly the fabrication method, structure and applications of carbon nano tubes

(CNTs).

29. Explain the major steps involved in the fabrication of cast iron; also mention its important

applications.

30. Discuss briefly on metal matrix composite (MMCs), polymer matrix composites (PMCs)

and fibre - reinforced composites (FRCs); also mention their important applications.

(2x10=20)

142


Fifth Semester


CH5GET02 Industrial Chemistry

Time: 3 Hours Maximum: 80 Marks

Section A


1. What is the use of Borax bead test?

2. What are alums? Mention its important use.

3. Distinguish between carbon nanotubes and carbon fibre.

4. What is meant by anode mud?

5. Why CO is used in Mond’s process?

6. What is the use of ZSM-5?

7. Define the term turnover number.

8. What do you mean by selectivity of catalysts?

9. Define the term Plastic Paint and give one example.

10. Write any two uses of anodizing.

11. What are the raw materials used for the preparation of calcium ammonium nitrate?

12. What is the principle of solar cells?

(9x 2 = 18)

Section B

(Answer any sixquestions. Each question carries 4 marks)

13. How is bleaching powder manufactured? Mention its important use.

14. Describe a method for the preparation of ultrapure metal.

15. What is soda lime glass? Give its composition.

16. What are semiconducting oxides? Give an example.

17. What is meant by NPK value?

18. Write a note on heat retardant paints.

19. Briefly explain the working principle of lead- Acid batteries.

143

20. Explain the principle of fuel cells. Give an example.

21. Explain how zeolites can be used as catalysts?

(6 x 4 = 24)

Section C


22. Write a note on the storage and production of phosgene

23. Explain the theory of setting process of cement.

24. Discuss the steps Involved In the manufacture of Superphosphate of lime.

25. Discuss homogeneous and heterogeneous catalysis with suitable examples.

26. Explain the electrometallurgy of aluminium.

(3 x 6 = 18)

Section D


27. Discuss in detail the uses, storage and hazards in handling of the industrial gases: (a)

Acetylene and (b) Chlorine.

28. Explain the composition and Properties of: (a) Armoured glass, (b) Safety glass, (c)

Borosilicate glass, and (d) Photo Sensitive glass.

29. Discuss the general methods used for the refining of metals.

30. Explain the processes involved in electrolytic and electrode less metallic coating with

examples.

(2 x 10 = 20)

144

B.Sc. DEGREE (CBCS) EXAMINATION Fifth Semester


CH5GET03 GREEN CHEMISTRY


Section A


1. Define Green Chemistry.

2. Give any two examples for renewable starting materials.

3. Name the pesticide that was being manufactured at the Bhopal plant of Union

Carbide Corporation and the gas which caused the Bhopal Tragedy.

4. Give two examples for reactions having 100% atom economy.

5. Name the two chemists who postulated the Twelve Principles of Green

Chemistry.

6. What are the advantages of microwave assisted reactions?

7. Give two examples for green solvents.

8. What is sonochemical Simmons-Smith reaction?

9. Give two techniques for minimizing hazardous waste.

10. What type of reaction vessels are used in microwave reactions?

11. Why derivatization should be avoided in chemical processes?

12. Write a reaction for the “saponification of esters” under microwave irradiation.

(9 x 2 = 18 marks)

Section B


13. What is sonication? Which effect is responsible for supply of energy in

sonication?

14. What is the need for environmentally safe marine antifouling?

15. What is co-crystal controlled solid state synthesis?

16. Explain the green route for the dry cleaning of garments.

17. What are the milestones in Green Chemistry?

18. What is super critical CO2? What are its advantages?

19. Define ionic liquids. What are the characteristic of ionic liquids?

145

20. Explain why catalytic reagents are superior to stoichiometric reagents.

21. What are the goals and needs of Green Chemistry?

(6 x 4 = 24 marks)

Section C


22. Define atom economy. Calculate the atom economy for the reaction

C + 2H2O → CO2 + 2H2 if the desired product is hydrogen.

23. Give any two methods for the synthesis of azo pigments.

24. Explain the term ‘Cradle to Cradle Carpeting’.

25. Explain with suitable examples: Proliferation of solventless reactions.

26. Give two examples for microwave assisted reactions in organic solvents.

(3 x 6 = 18 marks)

Section D


27. Explain the twelve principles of Green Chemistry.

28. Explain the green route for the synthesis of the following:

i) Adipic Acid (ii) Catechol

(iii) Disodium iminodiacetate

29. Write a note on the following microwave assisted reactions in water:

(i) Hofmann elimination (ii) Methyl benzoate to benzoic acid

(iii) Oxidation of toluene

30. Write notes on the following topics:

(i) Combinatorial Green Chemistry

(ii) Green Chemistry in sustainable development.

(2 x 10 = 20 marks)

146


SEMESTER VI

Chemistry Core

CH6CRT09 Coordination Chemistry and Organometalics


Petrochemicals )

Time: 3 Hrs Max.: 80 marks

Section A

(Answer any nine questions. Each carries 2 marks)

1. What are ambidentate ligands. Give one example?

2. What are chelates. Give one example?

3. Square planar complexes do not exhibit optical isomerism. Why?

4. What is Wilkinson’s catalyst? Give one application.

5. What is Zeigler Natta catalyst? Explain with an example.

6. Give the industrial applications of metal clusters.

7. What are metalloenzymes? Give two examples.

8. Tetrahedral complexes generally have high spin. Explain.

9. What is zone refining?

10. Give the essential role of Na+ and K+ in biological systems.

11. What are refractories? How are they classified?

12. What is carborundum? Mention its use.

Section B


13. Explain the factors affecting the stability of complexes .

14. What is EAN rule? Calculate the effective atomic number of the central metal ion in the

following complexes: (i) (Co(en)2Cl2)Cl (ii) Pt ( NH3)4 Cl2)Cl2

15. What are low spin and high spin complexes? Give examples.

16. Explain the structure of Re2Cl82-

17. What is Ellingham diagram? Explain its application.

18. Discuss the methods used in the refining of metals.

19. Explain with example the use of chelation therapy for the treatment of metal toxicity.

20. Discuss the importance of any two complexes as anti-cancer drugs.

21. Explain with details of any four methods of synthesis of nano materials.

Section C


22. Explain the properties and applications of fullerenes and carbon nanotubes.

147

23. Give a detailed account of intercalation compounds of alkali metals, carbon

monofluoride and graphite.

24. Discuss the structure and bonding in metal carbonyls.

25. Give a detailed note on the biological functions and toxicity of metals such as Fe, Cu ,Cr,

and Pb.

26. What are the basic postulates of valence bond theory? Differentiate between inner orbital

complex and outer orbital complex with examples.

Section D

(Answer any two. Each question carries 10 marks)

27. Discuss the different kinds of isomerism possible in coordination complexes with

suitable examples.

28. Give an account of the properties of ferrocene. Explain its structure and bonding.

29. Distinguish between haemoglobin and myoglobin on the basis of their structure and

functions.

30. Discuss the splitting of d-orbitals in (a) tetrahedral (b) octahedral (c) square planar fields.

148


Sixth Semester

Chemistry Core

CH6CRT10 ADVANCED ORGANIC CHEMISTRY – II

(Common for the Programmes B.Sc. Chemistry Model I and Model II and B.Sc. Model III

Petrochemicals)


Section A


1. What is epimerization?

2. Draw the structure of sucrose. Sucrose is a non-reducing sugar. Give reason.

3. Write a note on osazone formation of glucose.

4. Explain isoprene rule by taking an example.

5. Write the structure and biological functions of vitamin C.

6. Write the structure of cholesterol.

7. Explain zwitter ion character of amino acids.

8. What is meant by denaturation of proteins.

9. What are hormones? Name two examples.

10. What are waxes? Explain their biological functions.

11. State the differences between DNA and RNA.

12. What are cofactors ?

(9 x 2 = 18 marks)

Section B


13. Elucidate the structure of coniine.

14. How are vitamins classified? Draw the structure of vitamins B1and B6.

15. Write briefly on the secondary structure of proteins.

16. Write a short note on enzyme action.

17. Write a note on formaldehyde resins.

18. Write a note on non-biodegradable polymers and related environmental hazards.

19. Write down the structure of vitamins D2 and D3 and explain their biological

functions.

20. What are synthetic rubbers? Explain with examples.

21. Explain the cleansing action of soaps.

149

(6 x 4 = 24 marks)

Section C


22. Write briefly on HDL and LDL cholesterols and their functions.

23. Explain the biosynthesis of proteins

24. Write briefly on the industrial application of cellulose.

25. Convert glucose to fructose and vice versa.

26. Describe any two end group analysis methods for the primary structure determination

of proteins.

(3 x 6 = 18 marks)

Section D


27. Explain the different mechanisms involved in polymerisation reactions by taking

suitable examples.

28. (i) Discuss briefly on the cyclic structure of glucose.

(ii) How will you convert glucose to arabinose and vice versa.

29. Write an account of various noncovalent interactions that form the basis of molecular

recognition.

30. What are lipids? How are they classified? Explain the different chemical constants

used in the analysis of oils and fats

(2 x 10 = 20 marks)

150

BSc DEGREE CBCS EXAMINATION

Sixth Semester

Chemistry Core

CH6CRT11 Thermodynamics and Chemical Kinetics

(Common for the Programmes B.Sc. Chemistry Model I and Model II and B.Sc. Model III

Petrochemicals)

Time: Three hours Max. Marks : 80

Section A


1. Explain the term enthalpy.

2. Describe the efficiency of a heat engine.

3. Define the term entropy. How entropy change is related to the quantity of heat?

4. Give the mathematical form of first law of thermodynamics.

5. State the phase rule and explain the terms involved.

6. Define and explain order of a reaction.

7. What do you mean by heat capacity of a system?

8. What are the limitations of the first law of thermodynamics?

9. Define fugacity.

10. Distinguish between isothermal and adiabatic changes.

11. Derive the relation between Kp and Kc.

12. Explain the law of mass action.

(9× 2 = 18 Marks)

Section B


13. Distinguish between open, closed and isolated systems.

14. Write a note on Joule – Thomson effect.

15. Distinguish between isothermal and adiabatic changes.

16. How entropy changes with volume and temperature?

17. What is meant by metastable equilibrium?

18. Derive phase rule thermodynamically.

19. Define and explain activation energy.

151

20. Distinguish between opposing, consecutive and parallel reactions.

21. Describe about enzyme catalysis.

(6× 4 = 24 Marks)

Section C

((Answer any three questions. Each question carries 6 marks)

22. How the nature of the reactant affect the rate of a reaction

23. The activation energy of a reaction is 12 kcal/mole over the temperature range 300 –

400 K. How many times will the rate of the reaction increase if the temperature is raised

from 300 K to 400 K?

24. Calculate the change in entropy accompanying the heating of one mole of helium gas,

assumed ideal, from a temperature of 298 K to a temperature of 1000 K at constant

pressure. Assume that Cv = 3/2R.

25. Derive Gibb’s Helmholtz equation.

26. Four moles of an ideal gas expand isothermally from 1 litre to 10 litres at 300 K.

Calculate the change in free energy of the gas (R = 8.314 J K-1 mol-1)

(3× 6 = 18 Marks)

Part D


27. (a) Explain Pb – Ag phase diagram and how desilverisation is done.

(b) Discuss three component liquid systems using acetic acid-water-chloroform system as

an example

28. (a) Show that Cp – Cv = R for one mole of an ideal gas

(b) Derive the adiabatic equation of state PVγ = a constant

29. (a) Derive Clausius – Clapeyron equation for liquid – vapor equilibria

(b) Derive Gibbs – Duhem equation

30. (a) Derive an expression for the rate constant of a second order reaction where the

initial concentrations of the reactants are different

(b) Discuss the Lindemann theory of unimolecular reactions

(2× 10 = 20 Marks)

152


Sixth Semester

Chemistry Core

CH6CRT12: Solution Chemistry (Common for the Programmes B.Sc. Chemistry Model I and Model II and B.Sc. Model III

Petrochemicals)

Time: Three Hours Max. Marks: 80

Part A


1. State Raoult’s Law? Write its mathematical expression.

2. Ammonia is a base. Illustrate using Bronsted-Lowery concept.

3. What is hydrogen and oxygen over voltage?

4. Define CST? Give one example.

5. What are the advantages of conductometric titrations?

6. What is quinhydrone electrode?

7. Define ionic product of water. What is its value at 298 K?

8. Calculate the osmotic pressure of an aqueous solution of sucrose containing 0.01 kg

per dm3 at 298 K.

9. What are asymmetry and electrophoretic effects?

10. What is salt bridge? Why is KCl commonly used in a salt bridge?

11. What is cell constant? Give an expression and what is its unit?

12. Calculate the pH of 10-8 M HCl.

(9x 2 = 18)

Part B


13. Explain the principle of washing using Distribution law.

14. The F- concentration of a saturated solution of calcium fluoride in water at 25 0C is

4.0 X 10-4 mol dm-3. Calculate its solubility product?

15. What is ionic strength? Calculate the ionic strength of (a) 0.2 molal Na2SO4 and (b)

0.01 M CuSO4.

16. How will you determine pH of a solution using glass electrode?

17. How does H+ and OH- ions show abnormal conductance?

18. State and Explain Henry’s Law with suitable example?

153

19. Calculate the emf at 25 0C of the cell Zn(s)/Zn2+(0.1 M)//Ag+ (0.1 M)/Ag(s). Given

E0Zn

2+/Zn = -0.76 V; E0

Ag+

/Ag = 0.80 V

20. State and explain HSAB principle with suitable examples.

21. The vapour pressure of a 5 % aqueous solution of a non-volatile organic substance at

373 K is 745 mm of Hg. Calculate the molar mass of the solute.

(6 x 4 = 24)

Part C


22. Explain Van’t Hoff factor? Give mathematical explanation for the effect of molecular

association and dissociation on it?

23. Derive the expression for the Kh and pH of a salt of strong acid and weak base in

aqueous solution?

24. State Kohlrausch’s law. Explain the applications of Kohlrausch’s law.

25. What is Ksp? Explain its application in analytical chemistry.

26. How do we distill out binary liquid solutions?

(3 x 6 = 18)

Part D


27. Write a brief note on buffer solutions. Derive Henderson’s equation and mention its

important applications

28. What is meant by the term transport numbers? Explain the Hittorf’s method of

determining transport numbers.

29. What is corrosion? Discuss the electrochemical theory of corrosion. Discuss briefly

how does it can be prevented?

30. Explain the electrolyte concentration cells with transference and without transference.

(2 x 10 = 20)

154

B.Sc. DEGREE (CBCS) EXAMINATION Sixth Semester

Chemistry- Choice Based Core

CH6CBT01 POLYMER CHEMISTRY


Section A


1. What is Bakelite? What are the monomers of it?

2. Give two examples for initiators which can be used in free radical polymerization.

3. What is Ziegler-Natta catalyst?

4. What is PMMA?

5. Give two examples of addition polymers.

6. What is meant by calendering?

7. What is polydispersity index?

8. Define degree of polymerization.

9. What is cure reaction?

10. Distinguish between homo and hetero polymers.

11. Mention two applications of Teflon.

12. What is die casting?

(9 x 2 = 18 marks)

Section B


13. Explain the melt polycondensation polymerization.

14. Explain the chemistry of free radical polymerization with suitable examples.

15. What are conducting polymers? Give one example.

16. Explain the important applications of epoxy resins.

17. Distinguish between addition and condensation polymers.

18. Distinguish between thermoplastic and thermosetting polymers with examples.

19. What is Tg? What are the factors influencing Tg?

20. Suggest a suitable method to calculate the relative amounts of crystalline and

amorphous material in a polymer sample.

21. What are high temperature resistant and flame retardant polymers?

(6 x 4 = 24 marks)

155

Section C


22. Give a brief account of the mechanism of ring opening polymerisation.

23. Discuss any two methods for the determination of molecular weight of polymers.

24. Explain the mechanism and kinetics of step growth polymerization.

25. Write a note on polymer degradation.

26. Explain controlled drug release phenomena. Discuss the biomedical applications of

polymers.

(3 x 6 = 18 marks)

Section D


27. Explain polymer reactions and their applications.

28. Describe bulk polymerization and solution polymerization and give their

advantages and disadvantages.

29. Describe the following polymer processing techniques:

(a) Compression moulding

(b) Injection moulding

(c) Rotational casting

30. Explain the properties and applications of polyvinyl chloride and Kevlar.

(2 x 10 = 20 marks)

156


Sixth Semester

Chemistry-Choice Based Core

CH6CBT02 Instrumental Methods of Chemical Analysis

Time: 3 Hours Maximum: 80marks

Section A


1. Give an application of XRD.

2. Define electrophoresis.

3. What are the components of a mass spectrometer?

4. What are photons?

5. Give two advantages of instrumental analysis.

6. What is the basic principle of IR spectroscopy?

7. Give the definition of resolution in mass spectrometry.

8. What is S/N stands for?

9. Give any two oxidants used in atomic absorption spectroscopy.

10. What is DME?

11. What is a supercritical fluid?

12. Give the use of gas chromatography.

(9x 2 = 18)

Section B

(Answer any sixquestions. Each question carries 4 marks)

13. What do you understand the term time of flight in mass spectrometry?

14. What is meant by electromagnetic radiations? How do the wavelengths and the frequencies of

different types of electromagnetic radiations vary?

15. What are the different factors affecting the chemical shift?

16. Give the principles of TEM and STM.

17. What do you understand by the term electric quadrupole?

18. What are the advantages of FTIR spectroscopy?

19. Explain the essential components of a mass spectrometer.

20. Discuss the application of IR spectroscopy in quality assurance and control.

21. Give the principle and applications of voltammetry.

(6 x 4 = 24)

Section C


157

22. What is Beer-Lambert law? Express it mathematically and give the significance of each term.

23. Explain the principle and applications of potentiometry.

24. Write a note on the methods used for the detection of signals in UV-Visible spectroscopy.

25. Give the excitation sources and getting sample into gas phase in atomic spectroscopic

methods. Explain.

26. Discuss about the single and double beam spectrophotometers used in UV-visible

spectroscopy.

(3 x 6 = 18)

Section D


27. Explain the principle, instrumentation and applications of NMR spectroscopy.

28. What are the different methods used for making solid, liquid and gaseous molecules into ions

in mass spectroscopy?

29. Explain the separation technique using column chromatography.

30. (a)What is an Immunoassay? Explain.

(b) What are the different techniques for DNA analysis?

(2 x 10 = 20)

158


Sixth Semester

Chemistry-Choice Based Core

CH6CBT03 COMPUTER APPLICATIONS IN CHEMISTRY

Max: Mark: 80 Time : 3 hours

Section A

Answer any 9 questions. Each question carries 2 marks

1. What is a sting variable?. Give one example.

2. Change 11010010102 to an octal digit number.

3. Name different number systems in computer.

4. What is mean by ASCII code?

5. What does BCD stands for in computing.

6. What is mean by debugging?

7. Identify the valid and invalid numeric and string variables from the following: a) $B9 b)

20G c) Y$ d) SUM X e) NUMBER

8. Write the following formula in QBASIC N = (2J +1)e-BJ (J+1)hc

kT

9. Give an example each for a low level and high-level language.

10. Write the expanded form of QBASIC

11. When do you get a ‘out of DATA’ error message?

12. What is a Linux kernel

Part B


13. Explain with an example, the purpose of following library functions a) ABS b) SQR 14.

Explain the following library function with an example a) MOD b) INT

15. What are logical and relationship operators? Explain with examples.

16. Explain the function of following commands in QBASIC a) DIM b) READ c) DATA d)

REM d) RESTORE e) DEF f) FNR

17. How can we investigate the reactivity of a molecule using hyperchem?.

159

18. What is matlab?. Why is it called a fourth-generation programming language?

19. Explain Newton-Raphson method in numerical analysis.

20. Explain the function of following keywords with suitable examples a) LINE b)

WINDOW c) SCREE d) VIEW

21. What are the advantages of C++ over Fortran in numerical computing?

Part C


22. Write a program in QBASIC to calculate sin x , which is given by

sin x = x -x3

3!+x5

5!-x7

7!

23. Write a program in QBASIC to calculate the pressure (in pascal) for volume varying from

1 liters to 25 liters in a step size of 0.5 liter of van der Waals gas. Your program should print

both volume and corresponding pressure.

P +an2

V 2

æ

èçö

ø÷V - nb( ) = nRT

24. What is trapezoidal rule? a) Explain the different steps involved in the integration of

y = 4x3

0

4

ò dx using trapezoid rule. b) Write a program in QBASIC for the above integration

25. What is the difference between GOSUB and DEF commands? Explain all necessary

conditions and statements.

26. Write a program in QBASIC to multiply following matrices X and Y to print the resultant

matrix Z

X =43 36

14 19

æ

èç

ö

ø÷ and Y =

41 22

31 53

æ

èç

ö

ø÷

Part D


160

27. Following data was obtained in the distribution of Iodine between CCl4 and water.

Corg 0.0085 0.012 0.0175 0.020 0.025

Caq 0.0001 0.00015 0.00024 0.0003

Write a program in QBASIC to fit this data to a straight line using linear least square fit. The

program should a) Read and Print above data and b) Calculate the equation which best fits

the it using the linear least square fit and print the value of the distribution coefficient. The

equation for slope is given by slope =xiyiåxi

2å

28. Explain Newton-Raphson technique. Write a program in QBASIC to find the pH of a

0.01 M solution of acetic acid using Newton-Raphson iteration. It is given that

Ka = 0.0000185 and use a tolerance of 0.000001

29. a) Write a program in QBASIC to generate the area under the normal curve over the

interval [0, 4] at intervals of 0.01z. b) This program in Part a gives final values for the

integral under the normal curve that are obviously too large. The last entry is 0.5002,

whereas, from the nature of the problem, we know that the integral cannot exceed 0.5000.

Suggest a reason for this.

30. Write short notes on Molecular Modeling and the different Software packages available

for doing molecular modeling.

161


First Semester

Complementary Chemistry

CH1CMT01 Basic Theoretical and Analytical Chemistry (For students who have opted Physical Science and Geology as main)


Part A


1. What are buffer solutions? Write an example of buffer solution.

2. Illustrate Group Displacement law with an example.

3. Define radioactivity .Name any two units used to express radioactivity.

4. Differentiate between Normality and Molarity.

5. Define the term end point.

6. What is coordinate bond? Does H3O+ contain a coordinate bond?

7. How many significant digits are there in 2.0 Х 10–3 mL?

8. State and explain third law of thermodynamics.

9. What is the significance of magic numbers?

10. Suggest an indicator for a redox and complexometric titrations.

11. Compare isobars and isotones with examples.

12. Calculate electronegativity of Carbon from the following data: EH–H = 104.2 kcal mol–1,

EC–C = 83.1 kcalmol–1 and EC–H = 98.8 kcal mol–1.

(9 ×2 =18)

Part B


13. Expalin the terms (a) Packing Fraction (b) Mass defect.

14. What is internal energy? Give its significance

15. Define the term ‘Acid’ based on Lewis theory as well as Bronsted-Lowry theory.

16. How does stability of nucleus depend on the N/P ratio? Describe.

17. What are primary and secondary standards? Why does Na2CO3 consider as a primary

standard?

18. What are the factors favoring the formation of ionic bond?

19. Define the terms (a) ppm & (b) Mole fraction.

20. Explain the different modes of radioactive decay.

21. Exothermic reactions favors spontaneity at low temperatures while Endothermic reactions

at high temperatures. Justify. (6 ×4 =24)

162

Part C


22. Give the structure of following molecules based on VSEPR theory: (a) PCl5, (b) IF7 (c)

BeF2.

23. (a) Compare and contrast precision and accuracy. (b) Describe the terms pH, pOH & pK.

24. Define nuclear fission and nuclear fusion. Briefly explain the working principle of

Nuclear Reactor.

25. (a) What is lattice energy of ionic compounds? What are its applications? (b) Explain the

Hydrogen bonding in H2O.

26. Explain the physical significance of entropy.

(3 ×6 =18)

Part D


27. (a) Explain different types of errors. How do you overcome systematic errors?

(b) What is common ion effect? Describe its applications.

28. (a) Explain the applications of radioactive isotopes. (b) How does Gieger Muller counter

used for the detection and measurement of radioactivity.

29. (a) Give a brief outline of Molecular Orbital Theory based on LCAO. (b) Calculate the

bond order of N2 and CO molecules using MOT.

30. What is Gibb’s free energy? Explain its physical significance and conditions for

equilibrium and spontaneity.

(2 ×10 =20)

163


Second Semester


CH2CMT02 Basic Organic and Inorganic Chemistry

(For students who have opted Physical Science and Geology as main)


Part A


1. What is glass transition temperature of polymers?

2. Write the general electronic configuration of transition metals and actinides.

3. Differentiate between plastics and elastomers.

4. What are protic and aprotic solvents? Give examples.

5. What are the products of homolytic and heterolytic bond fission?

6. Define oxidation state. What is the oxidation state of Mn in KMnO4& MnO2?

7. How is Nylon 6,6 prepared?

8. What is roasting in metallurgical process?

9. What is homologous series?

10. Explain any two applications of lanthanides.

11. Define biodegradable polymers. Give any two examples.

12. What is the IUPAC name of CH3CH2CH2CHO?

(9 ×2 =18)

Part B


13. What is vulcanization of rubber? What is its significance?

14. Which one is colored TiCl3 or TiCl4? Justify.

15. What is Ellingham diagram? What is its significance?

16. Explain the acid-base reactions in liquid NH3.

17. Explain the synthesis of Buna S and Neoprene.

18. Compare lanthanide and actinide contractions.

19. Discuss Van Arkel-de-Boer process?

20. What is Latimer diagram? How is it used to determine the stability of various oxidation

states of Fe in acidic solution?

21. Illustrate different types of structural isomerism in organic compounds with examples.

164

(6 ×4 =24)

Part C


22. What are the different types of polyethylene? Give its applications.

23. Describe various reactions in liquid sulphur dioxide?

24. Discuss addition and substitution reactions with examples.

25. Describe electrolytic refining and zone refining.

26. How do you separate lanthanides using ion exchange method?

(3 ×6 =18)

Part D


27. Discuss the general characteristics of transition elements?

28. Explain the various steps involved in the concentration of ores.

29. Explain the preparation, structure and uses of (a) Phenol–formaldehyde resin

(b) Melamine–formaldehyde resin.

30 Describe the formation, structure and stability of carbocations, carbanions and carbon free

radicals.

(2 ×10 =20)

165


SEMESTER – III


CH3CMT03 Advanced Physical Chemistry- I


Time: 3 hours Maximum: 80 marks

Section A


1. Explain the term degrees of freedom with regards to phase rule.

2. State and explain Charles law.

3. Give Vanderwall’s equation and explain the terms.

4. Define zeta potential.

5. Write the mathematical form of Langmuir Adsorption Isotherm and specify the terms.

6. Define Gold number.

7. Calculate the miller indices of crystal planes which cut through the crystal axes at

(2a,3b,c).

8. Define viscosity. How does viscosity vary with temperature?

9. What is plane of symmetry? Explain using an example.

10. State and explain Nernst distribution law.

11. What is Tyndall effect?

12. State and explain Henry’s law.

(9 ×2 =18)

Section B


13. Write a note on band theory of solids.

14. Give Maxwell distribution of molecular velocities. Explain its significance.

15. Explain the cleaning action of soap.

16. What is Triple point? Explain using water system.

17. What do you mean by unit cell? Represent diagrammatically the unit cells for

a)simple primitive b)B.C.C and c)F.C.C

18. Discuss on kinetic molecular theory of gases.

19. Discuss briefly on a)Electrodialysis b)Ultra filtration method.

20. Discuss the optical properties of colloids.

21. Discuss the structure of sodium chloride.

(6 ×4

=24)

Section C

(Answer any three questions. Each question carries 6marks)

166

22. 1.20g of a non-volatile organic substance was dissolved in 100g of acetone at 20oc

.The vapour pressureof the solution was found to be 182.5 torr. Calculate the molar

mass of substance.(Vapour pressure of acetone at 20oc is 185 torr). 23. Calculate the angle at which first order reflection will occur in X-ray spectrometer

,when x-ray’s of wavelength 1.54 Ao are diffracted by atoms of a crystal. Given that

d=4.04Ao.

24. For H2 gas calculate a)RMS Velocity b)Average velocity and c)Most probable

velocity at 0oc.

25. Derive Bragg Equation. What are its applications?

26. What are liquid crystals? How they are classified? Explain.

(3 ×6

=18)

Section D


27. Discuss different types of magnetism with suitable examples.

28. Explain colligative properties. How can we determine the molecular mass of a solute

by elevation in boiling point?

29. Discuss on two component system. Explain the phase diagram of Pb-Ag system.

30. What are colloids? How are they classified? Discuss its applications.

(2 ×10 =20)

167


SEMESTER – IV


Advanced Physical Chemistry- II


Time: 3 hours Maximum: 80 marks

Section A


1. What is the advantage of using SHE as the reference electrode?

2. Define activation energy of a reaction.

3. State and explain Beer- Lambert law.

4. What are lasers?

5. What do you mean by fingerprint region of an IR spectrum?

6. What are the differences between order and molecularity of a reaction?

7. Write Arrhenius equation and explain the terms.

8. Explain the phenomenon chemiluminescence.

9. Explain pseudo order reaction with an example.

10. Explain the terms Bathochromic shift and Hypsochromic shift with example.

11. Write down the Nernst equation and explain the terms.

12. Define Faraday. How does it related to electrochemical equivalent?

(9 ×2 =18)

Section B

(Answer any six questions. Each question carries 4marks)

13. Discuss the variation of molar conductance with concentration of strong and weak

electrolytes.

14. Explain any two methods for the synthesis of nanomaterials.

15. Explain the collision theory of reaction rate.

16. Sketch the Jablonski diagram and explain the various radiative and non radiative

transitions involved.

17. Discuss briefly the general characteristics of catalytic reactions.

18. Discuss the different types of vibrations in a polyatomic molecule using water

molecule as an example.

19. Describe the construction and function of a calomel electrode.

20. State Kohlrausch’s law.Explain any two applications of the law.

21. Discuss briefly the effect of temperature on reaction rates.

(6 ×4

=24)

Section C

(Answer any three questions. Each question carries 6marks)

168

22. The fundamental vibrational frequency of HCl is 2890cm-1.Calculate the force

constant of this molecule.The atomic masses are 1H = 1.673×10-27 kg; 35Cl =

58.06×10-27Kg.

23. (a) Define Einstein’s law of photochemical equivalence.

(b) A sample of acetone absorbs monochromatic radiation at the rate of 4.5 x

1020quanta sec-1. The number of moles of acetone decomposed in one second is 1.35 x

10-4. Calculate the quantum yield of photolysis of acetone.

24. Discuss the applications of fullerene and carbon nanotubes.

25. a)The half-life of the homogeneous gaseous reaction SO2Cl2 SO2+Cl2,which

obeys first order kinetics is 8 min. How long will it take for the concentration of

SO2Cl2 to be reduced to 1% of its initial value?

b) The rate constant of a second order reaction is 5.70×10-5 dm3 mol-1 s-1 at 25oc

and1.64×10-4 dm3 mol-1 s-1 at 40 oC. Calculate the activation energy.

26. What are fuel cells? Explain Hydrogen-Oxygen fuel cell.

(3 ×6 =18)

Section D


27. Discuss the different types of catalysis and theory of catalysis.

28. What are the various applications of conductance measurements?

29. (a) How can we calculate the bond length of a diatomic molecule by using its

rotational spectrum?

(b) Explain briefly the theory of UV visible spectroscopy.

30. (a) Explain the principles of potentiometric titrations. What are its advantages over

ordinary titrations?

(b) Discuss briefly on electrochemical series and its applications.

(2 ×10 =20)

169


First Semester


CH1CMT05 BASIC THEORETICAL AND ANALYTICAL CHEMISTRY



Section A


1. What is Hund’s rule of maximum multiplicity?

2. What is a buffer solution? How does a mixture of acetic acid and sodium acetate act as a

buffer?

3. Distinguish between orbit and orbital.

4. Calculate the molarity of sodium carbonate solution prepared by dissolving 0.53 g pure

anhydrous Na2CO3 in 500 ml of distilled water.

5. Explain absolute and relative errors.

6. State Aufbau principle.

7. What is redox titration? Explain the principle involved in it using chemical equations.

8. What is Heisenberg’s uncertainty principle?

9. Calculate the concentration of OH- ions in a 0.10 M solution of ammonium hydroxide. (Kb of

NH4OH = 1.81 x 10-5).

10. State and explain Lowry-Bronsted concept of acids and bases.

11. Differentiate between accuracy and precision.

12. What are the criteria for a primary standard?

(9 x 2 = 18 marks)

Section B


13. Discuss ion exchange chromatography.

14. Explain photoelectric effect.

15. The solubility product of Mg(OH)2 at 250C is 1.2 x 10-11. Calculate the solubility of

magnesium hydroxide in grams per litre. (Mg = 24, O = 16, H = 1)

16. Discuss the principles of gravimetric analysis.

17. Explain the Arrhenius concept of acids and bases.

18. What is de Broglie wavelength? Calculate the wavelength associated with a bullet of mass 1g

travelling with a velocity of 3 x 102 ms-1. (h = 6.62 x 10-34 Js)

19. Calculate the concentration of sodium formate (HCOONa) that must be present in a solution

of 0.10 M solution of formic acid to produce a buffer solution of pH 3.80. (Ka for formic acid

is 1.8 x 10-4).

20. State Pauli’s exclusion principle. Based on this principle show that the maximum number of

electrons that can be accommodated in an orbital is 8 when n =2.

170

21. A buffer solution contains 0.20 mole of NH4OH and 0.25 mole of NH4Cl per litre. Calculate

the pH of the solution. (Dissociation constant of NH4OH at room temperature is 1.81 x 10-5).

(6 x 4 = 24 marks)

Section C


22. Explain the hybridization and geometry of acetylene molecule.

23. Discuss briefly on valence bond theory of chemical bonding. What are its main limitations?

24. How does ionization energy vary along a period? Explain.

25. What are the postulates of VSEPR theory?

26. Briefly explain solvent extraction.

(3 x 6 = 18 marks)

Section D


27. What are quantum numbers? Explain the significance of each.

28. Describe the principles and uses of high performance liquid chromatography.

29. Explain the terms common ion effect and solubility product. Discuss their applications in

qualitative cation analysis.

30. Give an account of molecular orbital theory of homonuclear molecules.

(2 x 10 = 20 marks)

171


Second Semester


CH2CMT06 BASIC ORGANIC CHEMISTRY

(For students who have opted Life Sciences and Family & Community Sciences as core)


Section A


1. Distinguish between homolytic and heterolytic fission with an example each.

2. What are electrophiles? Give an example of neutral electrophile.

3. Discuss the shape of ethane molecule.

4. What are free radicals? Give one method for its formation.

5. What do you mean by conformational isomers? Explain.

6. Explain geometrical isomerism by taking the example of maleic and fumaric acids.

7. What do you mean by Walden inversion?

8. Alkyl halides are easily hydrolysed while aryl halides are not. Why?

9. Among formic acid and acetic acid which is more acidic and why?

10. What is vulcanization of rubber? What are the advantages of vulcanization?

11. What are thermoplastics and thermosetting plastics? Give one example each.

12. What is chirality? Explain with an example.

(9 x 2 = 18 marks)

Section B


13. What is Markownikoff’s rule? Explain with an example.

14. Represent the conformations of n-butane. Which is the most stable conformation of n-butane?

Give the reason for your answer.

15. Explain mesomeric effect.

16. How are Nylon 6 and Nylon 6,6 prepared?

17. Differentiate between elastomers and fibres with one example each.

18. How will you account for the greater stability of tertiary carbocations?

19. What is hyperconjugation? How does it differ from resonance?

20. Draw the chair and boat conformations of cyclohexane and discuss their stability.

21. What is inductive effect? How does it influence the acid strength of organic acids?

(6 x 4 = 24 marks)

Section C


172

22. What are carbanions? Discuss the factors affecting stability of carbanions.

23. Write a note on synthetic rubbers.

24. Discuss the mechanism of E1 elimination with a suitable example.

25. Describe the E and Z nomenclature of geometrical isomers.

26. What do you mean by linear, crosslinked and network polymers? Explain with examples.

(3 x 6 = 18 marks)

Section D


27. Illustrate the following with examples:

a) Enantiomers b) Diastereomers c) Racemic modification d) Meso form.

28. (i) Differentiate between addition polymerization and condensation polymerization.

(ii) Write a note on non-biodegradable polymers and discuss how they cause environmental

hazards.

29. Explain SN1 and SN2 mechanisms using suitable examples and discuss their stereochemistry.

30. Discuss the synthesis and applications of:

a) Phenol-formaldehyde resin

b) Melamine-formaldehyde resin.

(2 x 10 = 20 marks)

173


Third Semester


CH3CMT07 ADVANCED INORGANIC AND ORGANIC CHEMISTRY



Section A


1. Which are the important regions of the atmosphere?

2. Define the term atom economy.

3. Name two green solvents.

4. What is a coupled reaction? Explain.

5. What are cytochromes? Explain.

6. State Huckel’s rule for aromaticity.

7. Give one method for the synthesis of indole.

8. The NPK value of a fertilizer is 10-10-10. What do you understand from this?

9. Give one method of preparation of DDT.

10. What is an emulsifying agent? What is its role in food chemistry?

11. What are food preservatives? Give two examples.

12. What are the main ingredients in toothpaste?

(9 x 2 = 18 marks)

Section B


13. Draw the temperature profile of the atmosphere.

14. Explain greenhouse effect.

15. Name the important pollutants in acid rain. What are its effects on the ecosystem?

16. Give two examples of metalloporphyrins and their functions.

17. How will you prepare furan? Discuss its aromaticity. Furan is less aromatic than benzene. Explain

this by giving one reaction of it.

18. Discuss on micronutrients and their role in plant growth.

19. Write briefly on environmental hazards due to excessive use of pesticides.

20. Write briefly on food colours and discuss the need of restricted use of food colours.

21. Write a note on the toxicology of cosmetics.

(6 x 4 = 24 marks)

174

Section C


22. What are the causes and consequences of ozone layer depletion?

23. How is pyridine isolated from coal tar? Why pyridine is basic in nature? Give one reaction to

show its basic character.

24. Explain one method each for the preparation of BHC and pyrethrin.

25. Discuss plant growth hormones and biofertilizers.

26. Write a note on the health effects of junk foods and soft drinks.

(3 x 6 = 18 marks)

Section D


27. Describe the ways in which air gets polluted. How does air pollution affect human health and

welfare?

28. Discuss the biochemical functions of haemoglobin and myoglobin.

29. How is furan prepared? Furan is aromatic but less aromatic than pyrrole. Explain why.

Explain the properties of furan as a diene and as an aromatic compound.

30. Write briefly on organic and inorganic fungicides and their uses.

(2 x 10 = 20 marks)

.

175


Fourth Semester


CH4CMT08 ADVANCED BIO-ORGANIC CHEMISTRY



Section A


1. What are fibrous proteins? Give two examples.

2. What is meant by isoelectric point of amino acids?

3. What are the structural components present in ATP?

4. Draw the Haworth configuration of β-D-glucose and β-D-fructose.

5. In what respect do vitamins differ from hormones?

6. What are the common methods used for the extraction of essential oils?

7. Distinguish between nucleosides and nucleotides.

8. What are the characteristic features of enzymes?

9. What is meant by saponification? Explain.

10. Draw the structure of cholesterol and mention its physiological importance.

11. Name two steroid hormones.

12. What are antibiotics? Give two examples.

(9 x 2 = 18 marks)

Section B


13. How is alanine synthesized in the laboratory?

14. What are waxes? Explain their biological functions.

15. Write a note on peptide hormones.

15. Discuss the application of isoprene rule with an example.

16. Draw the structure of vitamin C and explain its biological activities.

176

17. How is nicotine isolated? Give its physiological action on human beings.

18. Discuss in short the structure and biological functions of RNA.

19. Discuss the mechanism of enzyme action.

20. What is denaturation of proteins? What changes takes place during denaturation?

21. What are the essential differences between tranquilizers and antidepressants? Give two

examples of each.

(6 x 4 = 24 marks)

Section C


22. Explain the structure of DNA.

23. How is fructose converted to glucose? Give details.

24. Discuss the structure and reactions of citral.

25. Explain the cleansing action of soap.

26. Write a short note on mutarotation. Explain using glucose as an example.

(3 x 6 = 18 marks)

Section D


27. (i) Explain the different chemical constants used for the analysis of oils and fats.

(ii) What are synthetic detergents? Give examples. List a few advantages of

syndets over soaps.

28. Give an account of the primary, secondary and tertiary structures of proteins.

29. (i) Write a note on the structure of starch and cellulose.

(ii) Explain the industrial applications of cellulose.

30. Describe the following with suitable examples:

(a) Antipyretics (b) Antimalarials

(c) Antacids (d) Anticancer drugs.

(2 x 10 = 20 marks)

177

B.Sc DEGREE CBCS EXAMINATION

First semester

CH1VOT01 Industrial Aspects of organic and Inorganic Chemistry

(For B.Sc. Chemistry Model II- Industrial Chemistry)

Time: 3 Hrs Max :80 marks

Section A


1. What is meant by zone refining? Name two metals purified by zone refining.

2. Give a note on chain silicate.

3. Define octane number and cetane number.

4. Write about doctor solution and leaded petrol?

5. Explain the terms- gangue and flux.

6. Define calorific value of a fuel.

7. What are artificial sweeteners? Give examples for low calorific sweeteners.

8. What is colorant present in turmeric?

9. What is the monomer of cellulose?

10. What are the components of starch and Draw the structure of starch.

11. Distinguish between calcination and roasting with suitable examples

12. What is meant by froth flotation process?

(9 x 2 = 18)

Section B

Answer any six questions. Each question carries 4 marks

13. How is the anti- knocking property of a fuel improved?

14. Explain (a) cupellation and (b) poling.

15. How Lead is extracted from its ore by auto reduction method

16. What are zeolites? Give its importance.

17. What are the products of starch hydrolysis?

18. What do you mean by refining of petroleum?

19. Write a note on food preservatives

20. What is MSG? What are adverse effects of using MSG?

21. What are viscosity reducers?

(6 x 4 = 24)

Section C

Answer any three questions. Each question carries 6 marks

22. Explain purification of bauxite by Baeyer’s process.

178

23. How is magnesium extracted from sea water?

24. Explain the mechanism and application of reforming

25. Write a note on hydrocarbon fuels.

26. What are the different methods of adulteration?.

(3 x 6 = 18)

Section D

Answer any two questions. Each question carries 10 marks

27. Describe the metallurgical process for the extraction of iron

28. Write briefly on types of cracking, mechanism and chemical changes occurring

during cracking.

29. Explain the fractional distillation of petroleum.

30. What are food additives? Explain the various food additives.

(2 x 10 = 20 )

179

B. Sc. DEGREE (CBCS) EXAMINATION

Second Semester

CH2VOT02 Industrial Aspects of Physical Chemistry

(For B.Sc. Chemistry Model II- Industrial Chemistry)

Time : Three Hours Maximum : 80

marks

Part A

Answer any 9 Questions

Each question carries 2 mark

1. Explain electrophoresis and gold number.

2. Define surfactants.

3. What is zeta potential?

4. What are pesticides? Give any two examples of organochlorine pesticides.

5. Define cloud point and pour point.

6. How is hardness of water expressed?

7. Distinguish primary and secondary batteries? Provide examples.

8. What is emulsion? Give one example.

9. Explain hydrotropes with an example.

10. How solid, semisolid and synthetic lubricant differ from each other.

11. What is an adsorption isotherm. Give the expression for Langmuir adsorption isotherm.

12. Differentiate homogeneous and heterogeneous catalysis with an example.

(9 x 2 = 18)

Part B

Answer any six Questions


13. What are the factors affecting catalysis. Explain phase transfer catalysis.

14. Differentiate between Lyophilic and Lyophobic Sol. Give one example for each.

15. How is Gammaxane manufactured?

16. What is zeolite process?

17. Explain solar cell.

18. Give a note on the classification of pesticides.

180

19. Differentiate between conducting and non-conducting lubricating oils.

20. Explain Clark’s process for water softening.

21. (i) What are aerosols? Give two examples.

(ii) How physisorption differs from chemisorption.

(6 x 4 = 24)

Part C

Answer any three Questions


22. Discuss briefly any three methods for preparation of colloids.

23. Explain the manufacture and uses of malathion and quinones.

24. (a) What are conducting and nonconducting lubricants.

(b) Explain any two properties of lubricants.

25. (i)What is Ion exchange process? Explain.

(ii) Write a note on waste water treatment.

26. Explain the working of Nickel-Cadmium cell and lead acid battery.

( 3 x 6 = 18)

Part D

Answer any two Questions


27. (a) Explain briefly on industrially important enzyme catalyzed reactions.

(b) What are micelles? Explain their formation.

28. What do you mean by disinfection of water? Briefly explain the various methods used for it.

29. Write a note on kinetic, optical and electrical properties of colloids.

30. Briefly explain

a) Viscosity index of lubricants

b) Lime soda process

c) Lead acid Battery (2 x10 = 20)

181

B. Sc. DEGREE CBCS EXAMINATION Third Semester

Model II-Vocational Chemistry

CH3VOT03 Unit Operations in Chemical Industry

Time: Three hours Total marks:80

Section A

(Answer 9 questions. Each question carries 2 marks)

1. How will you separate a mixture of acetone and methyl alcohol? Justify your answer?

2. What is meant by the term packing efficiency?

3. Why is coke considered as a good adsorbent for gases

4. What is the difference in the action of water on silica gel and fused CaCl2?

5. Differentiate between physisorption and chemisorption?

6. Define boiling point. How is it related to pressure? Explain.

7. What are the advantages of candle filter over other filters?

8. What is the principle of centrifuge?

9. What do you mean by free moisture and bound moisture?

10. What is critical humidity?

11. Define solubility?

12. Differentiate between saturation and super-saturation?

Section B


13. Explain the principle of distillation with the help of boiling point diagram?

14. What is the principle of fractional distillation? Mention one of its industrial applications?

15. Discuss the principle of agitated film evaporator?

16. What are the desirable conditions for a satisfactory tower packing for gas adsorption?

17. Explain: a) packed column b) spray column c) bubble column

18. Write a note on column packings.

19. Why do some substances shrink during drying? What are the effects of shrinking?

20. What is nucleation? How are super-saturation and nucleation related to crystal growth?

21. Differentiate: (i) batch and continuous distillation

(ii) plate columns and packed columns

Section C


22. Narrate the specific uses and working of plate columns used in distillation.

23. What are azeotropes? How are they separated?

24. Give a brief account of working and application of forced circulation evaporators

25. Discuss the working of Rotary drier and Flash drier and mention their uses?

26. Write notes on: Drum Drier and Spray Drier?

Section D


27. Explain batch and continuous distillation. Discuss the industrial applications?

28. Discuss the principle, construction and working of a) standard evaporator b) long tube vertical

evaporators.

29. Write an essay on various filtration equipments?

30. What is crystallization? Discuss Agitated and Tank Crystallizers and explain the industrial

applications?

182

B. Sc. DEGREE CBCS EXAMINATION

Third Semester

Model II Vocational Chemistry

CH3VOT04 Unit Processes in Organic Chemicals Manufacture

Time: Three hours Total marks: 80

Section A


31. Represent the mechanism of nitration of benzene.

32. Illustrate the specific use of NBS in halogenation process.

33. Give a brief account on freons.

34. What are the precautions to be taken during fluorination process?

35. Sulphonation of naphthalene is a temperature dependent reaction. Justify?

36. Represent the equation for the manufacture of acrolein.

37. Give an example of a liquid phase oxidation reaction?

38. Illustrate the use of sodium metal as reducing agent for organic compounds.

39. How is methanol manufactured from CO and H2? Write the equation.

40. What is the mechanism of direct esterification process.

41. Give an example of esterification by addition to unsaturated compounds.

42. Illustrate the use of concentrated caustic oxidation-reduction method for the preparation of amino

compounds with one example.

Section B


43. What is Van’t Hoff factor? Determine the Van’t Hoff factor of nitric acid in sulphuric acid

mixture.

44. Discuss briefly the vapour phase nitration of paraffins.

45. What are the products of chlorination of toluene under different conditions? Explain with

equations.

46. Give the products of sulphonation and compare the rates of reaction of C6H5 – NMeI and

C6H5OH?

47. Illustrate the use of the following catalysts in synthesis: a) V2O5 b) Copper-Chromium oxide c)

FeCl3 and d) H2O2/FeSO4

48. What is meant by hardening of oils? Explain with suitable examples and equations.

49. What is trans-esterification? Give the example of one industrially important trans-esterification

process.

50. Briefly outline the esterification process by organic acid and by derivatives of carboxylic acid?

51. Cite the details of reduction of m-dinitrobenzene to m-nitro aniline.

Section C


52. How is monochloroacetic acid prepared?

53. What are the products formed when phenol is brominated in: a) water and b) CS2? Justify your

answer.

54. Explain commercial manufacture of benzoic acid.

55. Discuss briefly the hydrogenation catalysts. What are the merits of hydride reducing agents over

metal and acid reduction?

56. What is catalytic reforming? Give details.

183

Section D

(Answer any 2 questions. Each question carries 10marks)

57. Discuss briefly the commonly used nitrating agents. Give an account of conversion of benzene to

nitrobenzene and m-dinitrobenzene.

58. What are the specific conditions required for the use of different sulphonating agents? Examine

the relative merits of batch and continuous sulphonation.

59. Briefly outline the manufacture of: i) di-octyl phthalate ii) ethyl acetate iii) vinylacetate and iv)

cellulose acetate.

60. What is amination reaction? Explain how is it effected using metal-acid/alkali reagents taking

nitrobenzene as example? Explain the commercial preparation of aniline.

184

BSc DEGREE (CBCS) EXAMINATION

FOURTH SEMESTER


CH4VOT05 INSTRUMENTAL METHODS OF CHEMICAL ANALYSIS – I

TIME:3 Hrs MAX.:80 Marks

SECTION A


1. What are zero order instruments?

2. Explain the significance of S/N ratio?

3. What are transducers?

4. State Beer Lamberts law.

5. What is pneumatic detector?

6. What is meant by sampling?

7. Name any two non potentiometric analytical method.

8. Differentiate digital and analogue instruments

9. Explain the principle of conductometry

10. What is ICP?

11. What is fluorescence?

12. What is NDIR instrument? 9X2=18

SECTION B


13. Write a note on photomultiplier tube.

14. Discuss the performance characteristics of an instrument.

15. Explain the different types of detectors used in IR Spectroscopy.

16. What are factors effecting fluorescence.

17. Write a note on Wavelength selectors.

18. Discuss the principle of coloumetry.

19. Explain the instrumentation of spectroflourimetry.

20. Describe the different causes of deviation from Beers law.

21. What are the characteristics of a transducer. 6X4=24

SECTION C


22. Briefly discuss different types of noises..

23. Explain the instrumentation in IR spectroscopy.

24. Discuss the importance of sampling procedures in analysis. Explain the sampling procedures

employed in analysis of gases and liquids.

25. Explain the excitation techniques used in AES

26. Explain the principle and working of potentiometric analysis.

3X6=18

185

SECTION D


27. Discuss the techniques to enhance S/N ratio.

28. Briefly explain the principle and instrumentation of AAS.

29. Write a note on polarography and amperometry.

30. Explain the components of a typical of UV Visible spectrometry instrument. 2X10=20

186

B Sc DEGREE CBCS EXAMINATION

Fourth Semester


CH4VOT06 INSTRUMENTAL METHODS OF CHEMICAL ANALYSIS -II

Time: 3hrs Max. Marks 80

Section A


1. What are the different scales for measurement of temperature?. How are they

inter related?

2. What are the limitations of mercury thermometer?. Mention the range of temperature

that can be measured with mercury thermometers

3. What is a Maximum thermometer?.

4. At which temperature is the value in the centigrade scale identical to that in the

Fahrenheit scale.

5. Out line the operation of Bellow type element for pressure measurement.

6. Compare Hardware and Software of a Computer.

7. Explain the principle behind paper chromatography.

8. How is Rf value useful in the characterisation of compounds?

9. What is isocratic elution and gradient elution?.

10. What is the principle of adsorption column chromatography?.

11. Explain RAM and ROM

12. Out line the principle and operation of bimetallic thermometer.

(2×9 = 18)

Section B

Answer any 6 questions . Each question carries 4 marks

13. What are barometers?. What are their applications?

14. What is the principle and working of Bourden pressure Gauge?.

15. Explain gel Chromatography.

16. Discuss about various types of manometers used for pressure measurement.

17. What is the principle of HPLC?.

18. Discuss the working of thermal conductivity gauge used for pressure measurement.

19. Explain the Library functions in C Programming.

20. Write a note on Looping in C.

21. Explain the principle and working of Radiation Pyrometers used to measure the

temperature of furnace.

(4×6 = 24)

Section C

187


22. Write down the principle and working of resistance thermometer.

23. Discuss briefly about TLC.

24. Explain the construction of mercury in glass thermometer.

25. Write a note on Data input and output in C Programming.

26. Define Telemetry. Discuss about voltage telemetry and pneumatic telemetry.

(3×6= 18)

Section D

Answer any two question. Each question carries 10 marks

27. Describe briefly the principle, working, and application of Ion exchange

chromatography.

28. Write the principle, working and application of McLeod gauge.

29. A)What is Multiplexing.? Discuss about frequency division multiplexing and time

division multiplexing . B) Write a note on transmission channels.

30. (a)Discuss on the various Data types in C Programming.

(b) Write a C Programme to calculate the rate constant for First order reaction.

(2× 10 = 20)

188

BSc Degree (CBCS) Examination

First Semester

Model III Petrochemicals

CH1OCT01 PETROLEUM GEOLOGY

Time : 3 Hours Max. Marks : 80

Section A

Answer any 9 Questions (Each question carries 2 marks)

1. What are the criteria of good gasoline?

2. Explain sweetening process. .

3. What is Naphtha?

4. Give the composition and uses of Natural gas.

5. What are the advantages of spiral heat exchangers?

6. Discuss any one method for the production of petroleum from coal.

7. Distinguish between resource and reserves.

8. What are the non hydrocarbon compounds in crude oil?

9. Briefly explain metallic constituents in crude oil.

10. Explain in situ transformation of petroleum in reservoirs.

11. What is bitumen? What are its uses?

12. Explain magnetic method of oil exploration.

(2 x 9 = 18)

Section B

Answer any 6 questions (Each question carries 4 marks)

13. Write a note on Indian resources of petroleum.

14. Give a short account on different steps involved in mining of petroleum.

15. Discuss briefly on the main fractions obtained by fractional distillation of crude oil.

Give its composition.

189

16. Explain the term deasphalting.

17. Discuss briefly cone roof storage tank. What are its advantages?

18. What is Nitrogen blanketing? Explain.

19. Differentiate biogenic and abiogenic theories of origin of petroleum.

20. Explain natural methods of oil recovery.

21. Write a note on establishment of source beds. (4 x 6 = 24)

PART-C


22. Explain transformations of petroleum occurring in reservoir sediments.

23. Explain the classification of reserves.

24. Briefly explain anticlinal theory.

25. Briefly explain recovery of oil by primary and secondary methods.

26. Explain the functions of simple, complex and integrated refineries.

(3 x 6 = 18)

PART-D

Answer any Two Questions (Each question carries 10 marks)

27. Discuss briefly the different oil exploration methods and drilling operations.

28. Write a note on transportation and storage of crude oil.

29. Explain the theories of origin of petroleum.

30. a) Write a note on Geological framework of migration and accumulation of

petroleum.

b) Explain the classification of traps.

(10 x 2 = 20)

190

BSc Degree (CBCS)Examination

Second Semester


CH2OCT02 TEST METHODS AND PETROLEUM PROCESSES

Time: 3 Hours Max. Marks: 80

Section A

Answer Any 9 Questions (Each question carries 2 marks)

1. What is catalytic cracking? Name two catalyst used in catalytic cracking..

2. What are the different types of aviation fuels?

3. What are pour point depressants? Give examples.

4. Define diesel index?

5. Explain potential gum test?

6. Give the composition and uses of Natural gas.

7. Give the composition and uses of fuel oil?

8. Discuss visbreaking.

9. What are the criteria of good gasoline?

10. Explain ductility of Bitumen.

11. Briefly explain plat forming.

12. Explain Aniline point. What is its significance?

(2x9=18)

Section B


13. Explain hydro cracking. How does it differ from hydro treating?

14. Distinguish between cloud point and pour point.

15. What is Isomerisation? Explain Penex process of isomerisation.

16. What is copper corrosion test? Explain in detail.

17. What is Doctor solution .Explain its use.

18. What are the criteria of good kerosene?

19. Give a short note on ASTM method f product testing.

20. What is silver corrosion test? What is its significance?

21. Briefly explain the composition and specification of LPG. (4 x 6= 24)

191

Section C


22. Write a note on Abels and PMC methods of analysis.

23. Differentiate between road octane number and motor octane number.

24. Discuss briefly on some physical properties which are important to evaluate

Bitumen.

25. Explain rubberised bitumen and bitumen emulsion.

26. What is reforming? Write briefly on different types of reforming techniques .

(3 x 6 = 18)

PART-D

Answer any two questions (Each question carries 10 marks)

27. Discuss briefly on different types of thermal cracking.

28. Write briefly on catalytic cracking. What are its advantages over thermal

cracking?

29. a) Discuss in detail analysis of Aviation fuel.

b )Explain the various methods for measuring viscosity of oil?

30. Discuss any five techniques used for the evaluation of quality parameters of

diesel and petrol.

(10x 2= 20)

192


Third Semester

BSc Model III Petrochemicals

CH3OCT03 Production and Applications of Compounds from

Petroleum


Section A


30. What are the advantages of hydrogen as fuel?

31. Explain Aldol condensation.

32. What is Lumnus process?

33. Give one method for the preparation of isopropyl alcohol and its two uses.

34. What are the properties of thermosetting polymers?

35. Discuss Freush process.

36. Distinguish between hydrogenation and hydration.

37. What are the major products in steam naphtha cracking of hydrocarbon?

38. Briefly explain Petroleum coke.

39. Explain addition polymerisation with an example.

40. What are clatharates?

41. Write down the structure of acrylonitrile and mention its uses.

(2 x 9 = 18)

Section B


193

42. Write a note on nitro compounds in petroleum. Give preparation of any one of it.

43. Give a short account on the preparation of hydrogen.

44. Discuss briefly on the preparation and structure of Terephthalic acid.

45. What is Ammoxidation? Discuss the applications in detail.

46. Discuss briefly on application of oxidation in petroleum compounds?

47. What is Hydroformylation? Discuss Oxo process.

48. Differentiate between fluidized coking and delayed coking.

49. Explain union carbide process.

50. Write a note on the steam naphtha cracking of hydrocarbons..

(4 x 6 = 24)

Section C


51. Give an account of classification of oxides.

52. Explain the classification of polymers with examples.

53. Briefly explain Dow chemical process.

54. Briefly explain manufacture of sulphur.

55. Discuss in detail on the manufacture of higher olefins from Naphtha. Also discuss

present day procedure and its economics.

(3 x 6 =18)

Section D


56. Describe the manufacture of ethylene, acetylene and propylene by cracking.

57. Write a note on moulding of plastics and different techniques used for it in detail.

58. Describe the manufacture of Hydrogen and manufacture of Nitrogen compounds

from petroleum.

30. Explain the following with suitable examples and uses

a) Ammoxidation b) Hydration c) Hydroformylation d) Hydrogenation

(10 x 2 = 20)

194


Third Semester


CH3OCT04 MANUFACTURE OF PETROCHEMICALS-I


Section A

Answer any 9 questions .Each question carries 2 marks.

1. What are the important uses of HCN?

2. How is CS2 manufactured?

3. What are the engineering problems during the manufacture of triethanol amine?

4. What are the properties of ethylene oxide?

5. How is styrene purified?

6. What is carbon black?

7. What are the major products in steam naphtha cracking of hydrocarbon?

8. Briefly explain thermo pyrolysis.

9. How will you prepare vinyl chloride?

10. What is acetylene black?

11. Write down the structure of acrylonitrile and mention its uses.

12. Explain the terms power alcohol and rectified spirit.

(2 x 9 = 18)

Section B

Answer any Six Questions .Each question carries 4 marks.

13. Write a note on channel process.

14. Give a short account on the manufacture of acetylene by Sachse process.

195

15. Discuss briefly on the preparation and uses of vinyl acetate.

16. Write down the chemical equations involved in the manufacture of acrylonitrile.

17. Differentiate between furnace black and thermal black.

18. Give one method for the preparation of CCl4 and its two uses.

19. Discuss in detail the manufacture of ethanol by hydration.

20. How will you prepare chloromethanes from methane. Mention their uses.

21. Describe the manufacture of Ethanol from sucrose.

(4 x 6 = 24)

Section C

Answer any 3 questions .Each question carries 6 marks

22. Give an account on the production of methanol by catalytic hydrogenation of

methane.

23. Explain Thacker process.

24. Briefly explain the manufacture of acetaldehyde and the recent advances in the

process.

25. Briefly explain manufacture of ethylene glycol through chlorohydrin.

26. Discuss in detail on the manufacture of acetic acid. (3 x 6 =18)

PART-D

Answer any 2 questions. Each question carries 10 marks.

27. Describe the manufacture of ethanol amines and explain their properties and uses.

28. Explain the manufacture of HCN by Andrew sons process and Shawnigan process.

29. Describe the manufacture of styrene.

30. Explain the manufacture of acetylene by Wulf process. Give its properties and uses.

(10 x 2 = 20)

196


Fourth Semester


CH4OCT05 MANUFACTURE OF PETROCHEMICALS-II


Section A


1. What are the important uses of butadiene?

2. How is glycerine prepared from allyl alcohol?

3. Name the raw materials used for the preparation of vinyl chloride. How is it

prepared?

4. What are the physical properties of acetaldehyde?

5. How is chloroprene prepared?

6. What is cumene?

7. What is dealkylation ?

8. Briefly explain BTX aromatics.

9. How will you prepare glycerine from acrolein.

10. What is orlon. Give one method of preparation.

11. Write down the structure of PET and mention its uses.

12. What is saponification?

(2 x 9 = 18)

Section B


13. What is synthetic glycerine? How is it prepared?

14. Give a short account on C4 oligomers.

197

15. Discuss briefly on general reactions and side reactions of Linear alkyl benzene.

16. Explain Reppe’s synthesis of Acrylic acid.

17. What are the disadvantages in the preparation of Neoprene.

18. Give one method for the preparation of butadiene.

19. Discuss in detail the classification of detergents with examples.

20. How is Xylene commercially prepared from petroleum fractions?

21. How will you synthesis vinyl ether and acetonitrile.

(4 x 6 = 24)

Section C


22. Differentiate between soaps and detergents. Explain cleansing action of soaps.

23. Distinguish between chloroprene and isoprene.

24. Briefly explain the manufacture of acrylonitrile and mention its uses.

25. What do you mean by hydro dealkylation? Briefly explain manufacture of Benzene

by hydro dealkylation.

26. Discuss in detail on the manufacture of isopropanol by hydration process.

(3 x 6 =18)

Section D


27. Describe the manufacture of cumene from propylene and its purification. Explain

their uses.

28. Explain the manufacture of following.

(a) Vinyl chloride

(b) Acetaldehyde

29. Describe the production techniques of synthetic fibres. Explain the production of

polyester, polyamides and polycarbonates.

30. Explain the manufacture of Naphthalene. Give its properties and uses.

(10 x 2 = 20)

198


Fourth Semester


CH4OCT06 PETROLEUM INDUSTRIES IN INDIA

Time : 3 Hrs Max. Marks : 80

Section A


1. What is Ziegler catalyst?

2. Reforming process are usually done in presence of hydrogen.Why?

3. Name two catalysts used in petroleum industry?

4. What is meant by non conventional source of energy?

5. Give any two effects of oil pollution?

6. What is compressed natural gas?

7. What is hydrotreating ?

8. Briefly explain the term petrochemicals. Name two petrochemicals obtained from

butene.

9. What are the difficulties faced by Indian petrochemicals industries?

10. What is meant by geothermal energy?

11. Write two control measures for water pollution?

12. What are the advantages of using H2 as a fuel?

(2 x 9 = 18)

Section B


13. What is an enzyme catalyst? Discuss its selectivity and application.

14. Give a short account on tidal energy.

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15. Discuss briefly on major oil companies engaged in refining programme.

16. Discuss about hydro treating catalyst.

17. What are the difficulties faced by Indian petrochemicals industries in private sector?

18. Give one method for the preparation of Ziegler catalyst.

19. Write briefly on coal as an alternative to oil.

20. Briefly discuss on national standards of air and water pollution?

21. Discuss on future of petrochemical industry.

(4 x 6 = 24)

Section C


22. Briefly explain solar energy and bio gas. Mention their advantages.

23. Discuss the effect of fuel price in Indian Economy.

24. Explain briefly on nuclear fuels.

25. Discuss the role of polymers as catalyst.

26. Discuss in detail on the functions of ONGC. (3 x 6 =18)

Section D

Answer any 2 questions (Each question carries 10 marks).

27. Explain the following.

(a) General cost, capital cost and production cost.

(b) R & D economics.

28. Describe the role of catalyst in refining process.

29. Discuss briefly on non conventional sources of energy.

30. Discuss on the pollution from petroleum industries.

(10 x 2 = 20)

b.sc chemistry model i

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