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Sample NEET Chemistry Vol 1 Study Materials from SURA'S Main Books 2018

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Detailed Theory 2017

Original

Venkatesan 2016 QuestiOn

PaPers

Exhaustive MCQAs

EDITION

2015 2014

exPlanatOry

with

answers

Target

NEET Chemistry

Volume-I

and

2018

E 117 Vol ISURA COLLEGE OF COMPETITION ChennaiTirunelveliErnakulam ThiruvananthapuramBengalooru

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09

17

1000

© PUBLISHERS

Target NEET - CHEMISTRY Vol-I

ISBN : 978-93-86485-44-1

Code : E 117

[NO ONE IS PERMITTED TO COPY OR TRANSLATE IN ANY OTHER LANGUAGE

THE CONTENTS OF THIS BOOK OR PART THEREOF IN ANY FORM WITHOUT THE WRITTEN PERMISSION

OF THE PUBLISHERS]

SURA COLLEGE OF COMPETITION

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E 117 Vol I



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CONTENTS

NEET Solved Original Question Paper - 2017 ... 1 - 8

NEET

Solved

Original

Question

Paper

- 2016

...

9

- 15

NEET

Solved

Original

Question

Paper

- 2015

...

16

- 22

NEET

Solved

Original

Question

Paper

- 2014

...

23

- 28

VOLUME - I

CHAPTER 1 : BASIC CONCEPTS ............................................. 1 - 69

CHAPTER 2 : ATOMIC STRUCTURE ......................................... 70 - 98

CHAPTER 3 : PERIODIC PROPERTIES ...................................... 99 - 152

CHAPTER 4 : CHEMICAL BONDING ....................................... 153 - 194

CHAPTER

5 :

STATES OF MATTER..........................................

195

- 258

CHAPTER

6 :

THERMODYNAMICS ...........................................

259

- 287

CHAPTER

7 :

CHEMICAL EQUILIBRIUM ....................................

288

- 351

CHAPTER

8 :

REDOX REACTIONS...........................................

352

- 361

CHAPTER

9 :

HYDROGEN.....................................................

362

- 382

CHAPTER

10 :

S - BLOCK ELEMENTS .......................................

383

- 469

CHAPTER

11 :

P – BLOCK ELEMENTS .......................................

470

- 495

CHAPTER

12 :

GENERAL ORGANIC CHEMISTRY & ISOMERISM .........

496

- 615

CHAPTER

13 :

HYDROCARBONS ..............................................

616

- 683

CHAPTER

14 :

ENVIRONMENTAL CHEMISTRY ..............................

684

- 720

E 117 Vol I (iii)



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NEET – National Eligibility cum Entrance Test

INTRODUCTION

The Medical Council of India (MCI) has restored the National Eligibility cum

Entrance Test (NEET) to select the aspiring candidates, who are seeking higher

education opportunities in Medical(MBBS) and Dental(BDS) Colleges/Universities across

the country. This book with its extensive and accurate question bank and answers

will enable students to understand the concept followed in the test thoroughly and

enhance their scores.

TEST PATTERN

1. Number of Questions/ Subjects : The question paper will consist

of a total of 180 Multiple choice

questions with 45 questions from

Physics and Chemistry each and

90 questions from Biology.

2. Scoring Pattern : 4 marks will be awarded for each

correct answer And 1 mark will

be deducted for each incorrect

Answer. A maximum of 720 marks

has been set as the upper limit.

3. Duration and Mode : The test duration will be 3 hours

in Pen & Paper Mode.

4. Languages : The test will be conducted in

10 (TEN) languages.

5. Core Syllabus : The Medical Council of India

(MCI) Recommends the following

syllabus for NEET for Admission

to MBBS/BDS courses after

reviewing Various State Board

Syllabi and those of CBSE & NCERT.

E117 Vol I (iv)



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1. BASIC CONCEPTS


Introduction

Chemistry is the science of substances, their properties, structures and their transformation. As all objects in the

universe are made of matter. Chemistry is the branch of the science which deals with the study of material object.

Study of chemistry is very interesting. It covers various aspects of our culture and environment. All development in

any science are based on scientific approach as in chemistry too. In order to achieve correct results, one has to

rely upon the various skills connected with the measurements of quantities during a physical or chemical change.

The degree of accuracy is closely linked with precision of the measuring instrument as well as on the skill of

the person engaged in measurement. So we should be first familiar with some terminology used in chemistry.

Physical Property:

The property which can be measured without changing the chemical composition of the substance is known as

physical property like mass, volume, density, refractive index etc.

Chemical property:

The property which can be evaluated at the cost of matter itself is known as chemical property. For example

combustible nature of hydrogen gas can be verified by burning of hydrogen. The sweet taste of sugar is recognised

by consuming it.

Units of Measurement:

All physical quantities have to be measured. The value of a physical quantity is expressed as the product of the

numerical value and the unit in which it is expressed.

Fundamental units:

Fundamental units are those units which can neither be derived from one another nor they can be further re-

solved unit any other units

The seven fundamental units of measurement in SI system.

Quantity Name of unit Abbreviation

Mass Kilogram Kg

Length Metre M

Temperature Kelvin K

Amount of substance Mole Mol

Electric current Ampere A

Luminous intensity Candela Cd

Derived unit:

Some quantities are expressed as a function of more than one fundamental units known as derived units. For

example, velocity, acceleration, work, energy etc.

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2. ATOMIC STRUCTURE


6

INTRODUCTION:

Fundamental Particles:

Atoms are made up-essentially, of three fundamental particles, which differ in mass and electric charge

as follows:

Electron Proton Neutron

Symbol e or e- p n

Approximate relative mass 1/1836 1 1

Approximate relative charge -1 +1 0

Mass in kg 9.109534 × 10-31 1.6726485 × 10-27

1.6749543 × 10-27

Mass in amu 5.4858026 × 10-4 1.007276471 1.008665012

Actual charge / C −1.6021892 × 10-19 +1.6021892 × 10-19

0

The atomic mass unit (amu) is 1/12th of the mass of an individual atom of

C12, i.e. 1.660565 × 10-27 kg. The

neutron and proton have approximately equal masses of 1 amu and the electron is about 1836 times lighter; its

mass can sometimes be neglected as an approximation. The electron and proton have equal, but opposite, electric

charges; the neutron is not charged.

The existence of electrons in atoms was first suggested, by J.J. Thomson, as a result of experimental work on the

conduction of electricity through gases at low pressures, which produces cathode rays and x-rays, and a study of

radioactivity by Becquerel, Curie and Rutherford.

An atom is electrically neutral, and if it contains negatively charged electrons it must also contain some positively

charged particles, and the supposition that they existed within atoms came about as a result of Rutherford’s

experiments in which the elements are bombarded with the a-rays given off by radioactive elements. The neutron

was discovered in 1932 by James Chadwick by bombarding beryllium with a rays.

Rutherford’s Atomic Model:

A beam of alpha particles, di-positive helium ions, was obtained from a source containing the element polonium.

Rutherford’s experiment was to place thin sheets of metal in the path of the alpha ray in order to see how various

metals would affect the alpha-particle trajectory. Rutherford found that some of the alpha particles were deflected

at astonishingly large angles. A few were actually reflected back towards the source. According to Rutherford, the

only way to account for the large deflections would be to say that the “positively charge centre” and mass in the

metal foil are concentrated in very small regions.

Although most of the alpha particles go through without any deflection, occasionally one comes very close to a

high concentration of positive charge.

To explain his observations, Rutherford suggested that an atom has a nucleus, or centre, in which its positive

charge and mass are concentrated. The quantitative results of scattering experiments such as Rutherford’s indicate

that the nucleus of an atom has a radius of about 10-13 cm, which is only about one hundred thousandth the size

generally ascribed to atoms.

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3. PERIODIC PROPERTIES


Introduction

The classification of elements in periodic form is a great achievement in the history of chemistry. It is difficult

to study individually the chemistry of more than one hundred natural or synthetic elements and millions of their

compounds. The periodic table provides systematic and organized chemical behaviour of the elements into few

simple and logical patterns. In periodic table elements are arranged in rows & columns. From the position of

element it is possible to predict its chemistry. In this unit, we will study the historical development of modern

periodic table, its function and some of the periodic trends in the physical and chemical properties of the elements.

History of Development of the Periodic Table

All earlier attempts on the classification of the elements were based upon their atomic weights.

Dobereiner’s Triads:

The first attempt towards the classification of elements was made by John Dobereiner a German chemist in 1829.

He classifies the elements with similar properties in the groups of three elements (Triads). He could succeed in

making only a few triads. In the triads of elements the atomic weight of the middle element was the arithmetic

mean of the atomic weights of the other two. Some of the triads are as under.

Li Na K Ca Sr Ba

7 23 39 40 88 137

P As Sb Cl Br I

31 75 120 35.5 80 123

The major drawback of Dobereiner’s classification was that the concept of triads could be applied only for the

limited number of elements.

Newland’s Law of octaves:

The English chemist John Newland in 1865 − 66, developed the law of octaves. He pointed out that, if the

elements are arranged in order of their increasing atomic weights, every eighth element had similar properties

to first one like the first and eighth note of the musical scale. For example

sa re ga ma pa dha ni sa

Li Be B C N O F Na

Na Mg Al Si P S Cl K

This generalization was also discarded since it could not be applied to elements having atomic weight greater than

that of calcium i.e. 40 a.m.u Furthermore with the discovery of noble gas, the properties of the eighth elements

were no longer similar to the first one.

Lothar Meyer’s Atomic Volume Curve 1869:

Lothar Meyer a German chemist plotted a graph between atomic weight and atomic volume (i.e. atomic weight

in solid state/density) and he find out that elements with similar properties occupied the similar positions on the

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4. CHEMICAL BONDING

Introduction

Every system in nature wants to attain stability. Atoms always want to attain stability by attaining the configuration

of nearest noble gas and combine to form molecule. A molecule is made of two or more atoms joined together

by some force acting between them. This force is termed as chemical bond.

A molecule is formed if it is more stable and has lower energy than the individual atoms. Normally only electrons

in the outermost shell of an atom are involved in bond formation and in this process each atom attains a stable

configuration of inert gas. Atoms may attain stable electronic configuration, by gaining or by sharing electrons.

There are several different theories which explain the electronic structure and shapes of known molecules, and

attempt to predict the shapes of molecules whose structures are so far unknown. Each theory has its own virtues

and shortcomings. None is rigorous. The value of a theory lies more in its usefulness than in its truth. Being

able to predict the shape of a molecule is important. In many cases all the theories give the correct answers.

The Lewis Theory

The Octet Rule

The Lewis theory gave the first explanation of a covalent bond (in terms of electrons) that was generally accepted.

If two electrons are shared between two atoms, this constitutes a bond and binds the atoms together. For many

light atoms, a stable arrangement is attained when the atom is surrounded by eight electrons.

This octet can be made up from some electrons which are totally owned and some electrons which are ‘shared’.

Thus atoms continue to form bonds until they have made up an octet of electrons. This is called the ‘octet rule’.

The octet rule explains the observed valencies in a large number of cases. For example nitrogen atom has 5 outer

electrons and in NH3 it shares three of these, forming three bonds and thus attaining an octet, hydrogen has only

one electron and by sharing one electron it attains a stable arrangement of two electrons.

Lewis Symbols

N

3 [H]

H N H

Lewis introduced simple notations to represent valence electrons in an atom. They are called Lewis symbols.

In these symbols valence electrons are represented by dots.

Lewis structure of elements:

No. of valence

electrons

Example Lewis structure

1 Hydrogen / Group IA H / Li

2 Helium/Group IIA ⋅Be ⋅

3 Group III A

B

4 Group IV A

⋅C⋅

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5. STATES OF MATTER


a a

Introduction

Matter can be classified into three categories depending upon its physical state namely solid, liquid and gaseous

states. Solids have a definite volume and shape; liquids also have a definite volume but no definite shape; gases

have neither a definite volume nor a definite shape.

Distinction between Three States of Matter

Sl. No. Solids Liquids Gases

1. Particles are very closely

packed

Particles are loosely packed Particles are very loosely

packed

2. Voids are extremely small Voids are relatively larger Voids are very large

3. Inter particle forces are large Inter particle forces are inter-

mediate

Intermediate forces are negli-

gible

4. Particle motion is restricted to

vibratory motion.

Particle motion is very slow Particle motion is very rapid

and also random.

Measurable Properties of Gases

Mass, volume, temperature are the important measurable properties of gases.

Mass: The mass of the gas is related to the number of moles as

n = w M

Where n = number of moles

w = mass of gas in grams

M = molecular mass of the gas

Volume: Since gases occupy the entire space available to them, therefore the gas volume means the

volume of the container in which the gas is enclosed.

Units of Volume: Volume is generally expressed in litre or cm3 or dm3 1m3 = 103 litre

= 103 dm3 = 106 cm3.

Pressure: The force exerted by the gas per unit area on the walls of the container is equal to its pressure.

Units of Pressure: The pressure of a gas is expressed in atm, Pa, Nm–2, bar or, lb/In2 (psi).

760 mm = 1 atm = 10132.5 KP

= 101325 P

= 101325 Nm–2

760 mm of Hg = 1.01325 bar = 1013.25 milli bar = 14.7 lb/2n2 (psi)

Temperature: Temperature is defined as the degree of hotness. The SI unit of temperature is Kelvin. On

the Celsius scale water freezes at 0°C and boils at 100°C where as in the Kelvin scale water freezes

at 273 K and boils at 373 K.

Gas Laws

The state of a sample of gas is defined by 4 variables i.e. P, V, n & T. Gas laws are the simple relationships

between any two of these variables when the other two are kept constant.

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6. THERMODYNAMICS


2 1

Limitations of the first law. Need for the second law

A major limitation of the first law of thermodynamics is that it merely indicates that in any process there is an

exact equivalence between the various forms of energies involved, but it provides no information concerning the

spontaneity or feasibility of the process. For example, the first law does not indicate whether heat can flow from

a cold end to a hot end or not.

The answers to the above questions are provided by the second law of thermodynamics.

Spontaneous and non – spontaneous processes

If in the expansion of a gas the opposing pressure is infinitesimally smaller than the pressure of the gas, the

expansion takes place infinitesimally slowly i.e. reversible. If however, the opposing pressure is much smaller

than the pressure of the gas the expansion takes place rapidly i.e. irreversibly. Natural processes are spontane-

ous and irreversible.

SECOND LAW OF THERMODYNAMICS

The second law of Thermodynamics helps us to determine the direction in which energy can be transformed.

It also helps us to predict whether a given process or chemical reaction can occur spontaneously or not.

According to II law of thermodynamics it is impossible to have a machine or heat engine which converts the

input energy completely into output energy or output work without any amount of heat or energy being ab-

sorbed the machine.

T % efficiency 1 2

100.

T1

By II law, T < T % efficiency less than 100.

Entropy, like any other thermodynamics property such as internal energy U and enthalpy H is a state function

and S is independent of path.

Whenever heat is added to the system, it increases molecular motions causing increased randomness in the

system. Thus heat (q) has randomizing influence on the system. Can we then equate S with q ? Wait ! Ex-

perience suggests us that the distribution of heat also depends on the temperature at which heat is added

to the system. A system at higher temperature has greater randomness in it than one at lower temperature. Thus,

temperature is the measure of average chaotic motion of particles in the system. Heat added to a system at

lower temperature causes greater randomness than when the same quantity of heat is added to it at higher

temperature. This suggests that the entropy change is inversely proportional to the temperature. S

with q and t for a reversible reaction as :

is related

q S rev

T

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7. CHEMICAL EQUILIBRIUM

Introduction

It is an experimental fact that most of the process including chemical reactions, when carried out in a closed

vessel, do not go to completion. They proceed to some extent leaving considerable amounts of reactants &

products. When such stage is reached in a reaction, it is said that the reaction has attained the state of equilibrium.

Equilibrium represents the state of a process in which the properties like temperature, pressure, concentration

etc of the system do not show any change with passage of time. In all processes which attain equilibrium, two

opposing processes are involved. Equilibrium is attained when the rates of the two opposing processes become

equal.

If the opposing processes involve only physical changes, the equilibrium is called Physical Equilibrium. If the

opposing processes are chemical reactions, the equilibrium is called Chemical Equilibrium.

Some common physical equilibria are:

Solid Liquid

Liquid Gas

Gas Solution

Generally, a chemical equilibrium is represented as

aA + bB xX + yY

Where A, B are reactants and X, Y are products.

Note:

The double arrow between the left hand part and right hand part shows that changes is taking place in

both the directions.

On the basis of extent of reaction, before equilibrium is attained chemical reactions may be classified into three

categories.

(a) Those reactions which proceeds almost completion.

(b) Those reactions which proceeds almost only upto little extent.

(c) Those reactions which proceed to such an extent, that the concentrations of reactants and products at equi-

librium are comparable.

Equilibrium in physical Process The different types of physical Equilibrium are briefly described below

(a) Solid – liquid Equilibrium

The equilibrium exist between ice and water is an example of solid – liquid equilibrium. In a close system, at

0 C ice and water attain equilibrium. At that point rate of melting of ice is equal to rate of freezing of water.

The equilibrium is represented as

H2O(s) H2O( )

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8. REDOX REACTIONS


H

H

2

H 2

2

2

2

INTRODUCTION

An oxidation-reduction (redox) reaction is a type of chemical reaction that involves transfer of electrons between two

species. The reaction is, any chemical reaction in which the oxidation number of a molecule, atom or ion changes

by gaining or losing an electron.

• Oxidation is gain of oxygen

• Reduction is loss of oxygen

Ex.:

Redn.

Fe O + 3CO 2Fe + 3CO2 3 2

Oxdn.

This reaction is known as redox reaction, because, both reduction and oxidation are going on side-by-side.

• In terms of electron transfer,

• Oxidation is loss of electrons

• Reduction is gain of electrons

Ex.:

Cu2+ + Mg Cu + Mg2+

These two processes cannot occur without the other. If there is a reduction reaction there must be an oxidation

reaction. Adding electrons is called reduction because the overall charge is reduced, more electrons means the

substance becomes more negative.

The formation of Hydrogen Fluoride is an easy simple and example of a redox reaction.

+ F 2HF

2H+ + 2e–

Fe + 2e– 2F–

+ F 2H+ + 2F– 2HF

Oxidising agents give oxygen to another substance or remove hydrogen from it.

Reducing agents remove oxygen from another substance or give hydrogen to it.

Oxidising agent is termed as Oxidant.

Reducing agent is termed as reductant.

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9. HYDROGEN


3 4 2 2

2 2

Introduction

Hydrogen is the first element in the periodic table and is also the lightest element known. Its atomic form exists

only at high temperatures. In the normal element form, it exists as a diatomic molecule, i.e. H2 .

Unique Position of Hydrogen in the Periodic Table

A proper position could not be assigned to hydrogen either in the Mendeleev’s periodic table or Modern periodic

table because of the following reason:

In some properties, it resembles alkali metals and in some properties it resembles halogens. So hydrogen can

be placed both in group 1 and group 17 with alkali metals and halogen respectively.

Resemblance with Alkali Metals

1. Electronic configuration

Hydrogen contains one electron in the valence shell like alkali metals

H : 1s1

Li : He2s1

Na : Ne3s1

K : Ar 4s1

Rb : Kr 5s1

2. Electropositive character

Like alkali metal, hydrogen also loses its only electron to form hydrogen ion, i.e, H

H 1s1

Na

H e

1s0

Na

e

1s2

2s2

2p6

3s1

1s2

2s2

2p6

3. Oxidation state

Like alkali metals, hydrogen exhibits an oxidation state of +1 in its compounds.

H Cl Na Cl K Br Hydrogen chloride Sodium chloride Potassium chloride

4. Reducing agent

Alkali metals act as reducing agents because of their tendency to lose valence electron. Hydrogen is

also a very good reducing agent as evident from the following reactions:

Fe O 4H 3Fe 4H O

CuO H Cu H O

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10. S - BLOCK ELEMENTS


Introduction

The elements in the long form of the periodic table has been divided into four blocks, namely s, p, d & f blocks.

The elements of group I & II receive their last electron in S – orbital. So they are called as s – block elements.

The metals Lithium (Li), sodium (Na), potassium (K), rubidium (Rb), caesium (Cs) and francium (Fr) which have

one electron in their outermost shell belongs to group I and are called alkali metals as they react with water to

form hydroxides which are strong bases or alkalies.

The elements of group II are Berryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), Barium (Ba) and

Radium (Ra) which have two electrons in their outermost shell. All these elements are also metallic in nature

and are commonly known as alkaline earth metals with the exception of beryllium. Because of their low density,

alkali metals and alkaline earth metals are called lighter metals. Both alkali and alkaline earth metals are highly

reactive and hence do not occur in free state but found in combined state. Whereas alkali metals mostly occurs

as halides, oxides, silicates, borates and nitrates, alkaline earth metals mainly occur as silicates, carbonates,

sulphates and phosphates. Some alkali & alkaline earth metals occur abundantly in nature. Calcium is the fifth,

magnesium is the sixth, sodium is seventh and potassium is eighth, barium is the fourteenth and strontium is

the fifteenth most abundant element by weight in the earth’s crust. Sodium and magnesium are also present in

sea water brine wells and few salt lakes.

Anamalous behaviour of first element

The first element of a group differs considerably from the rest of the elements of the same group. This anoma-

lous behaviour is due to

(i) Smaller size of their atoms

(ii) Their higher ionization energies

(iii) Their higher electronegativites

(iv) Absence of vacant d – orbitals is their valence shell

(v) High polarizing power of its cation.

Thus Li differes from the rest of alkali metals (Na, K, Rb & Cs) and Be differs from rest of the alkaline earth

metals (Mg, Ca, Sr & Ba)

Diagonal relationships

On moving diagonally some members show similar properties with the members of next higher group which is

particularly seen in the elements of second and third periods of the periodic table. However the similarities shown

are far less pronounced than the similarities with in a group.

Group1 Group2 Group13 Group14

Period-2

Period-3

Li Be B

Mg Al Si

The main reasons for the diagonal relationship are

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11. P – BLOCK ELEMENTS


Introduction:

The right side of the periodic table having group number 13, 14, 15, 16, 17 and 18 are known as p – block

elements. These elements have 3, 4, 5, 6, 7 and 8 electrons in their outer most shell, respectively. The last

electron of these groups’ elements occupies the position in p – sub shell that is why they are called as p – block

elements. Their general configuration is ns2np1-6.

PROPERTIES OF P- BLOCK ELEMENTS

1. Electron affinity

Electron affinity increase from left to right along the period amongst the p – block elements and it

decreases from top to bottom. But group 15 is having exceptionally low values of electron affinity and

it is due to extra stability because of the presence of exactly half filled orbital in their valence shell.

Similarly, elements of group 18 (noble gases) have zero affinities due to presence of complete octet

which provides them stability.

2. Metallic Character

The metallic character is governed by

(i) Size of atoms and

(ii) Ionization energy.

The elements having bigger size and low ionization energy has a greater metallic character. After combin-

ing both above mentioned factors we observe that the elements with above two properties are located

in left corner of p – block and strong non – metallic elements are located at right corner and a diagonal

strip of elements separates thus two, having in between properties are called as metalloids.

3. Oxidation state

The p – block elements shows variety of oxidation states both positive and negative. Some of the p –

block elements show different oxidation state due to inert – pair effect, where their lower oxidation state

is more predominant.

4. Diagonal relationship

On moving diagonally across the periodic table the element show certain similarities

Li Be B C

Na Mg Al Si

Note: Elements of 2nd period differ from their own group elements in some of the properties. This is due to

the following reasons:

(a) Small size

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Chain Length Root word Chain Length Root word

C Meth- C Undec-

C Eth- C Dodec-

C Prop- C Tridec-

C But- C Tetradec-

C Pent- C Pentadec-

C Hex- C Hexadec-

C Hept- C Eicos-

C Oct- C Triacont-

C Non- C Tetracont-

C Dec- C Pentacont-

5

12. GENERAL ORGANIC

CHEMISTRY & ISOMERISM

Nomenclature of Organic Compounds

IUPAC System [International union of pure and applied chemistry]

The most important feature of this system is that any given molecular structure has only one IUPAC name which

denotes only one molecular structure.

Salient features of IUPAC system

1. A given compound can be assigned only one name.

2. A given name can clearly direct in writing of one and only one molecular structure.

3. The system can be applied in naming complex organic compounds.

4. The system can be applied in naming multifunctional organic compounds.

5. This is simple, systematic and scientific method of nomenclature of organic compounds.

Rule for Naming

Prefix (alphabetically) root word (alk) primary suffix (ene, yne) secondary suffix (main functional group)

So IUPAC name of any organic compounds essentially consists of two or three parts.

(i) Root word (ii) Suffix (iii) Prefix

(i) Root Words

The basic unit is a series of root words which indicate linear or continuous chains of carbon atoms. Chains

containing one to four carbon atoms are known by special root words while chains from C

by Greek number roots.

onwards are known

1 11

2 12

2 13

4 14

5 15

6 16

7 20

8 30

9 40

10 50

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13. HYDROCARBONS

Alkanes

Alkanes are open-chain (acyclic) hydrocarbons comprising the homologous series with the general formula,

C H , where n is an integer. They have only single bonds and therefore are said to be saturated. n 2n+2

Free Rotation about the Carbon-Carbon Single Bond: Conformations:

H H

C H

1.53 Å

109.5o

H C

H

Ethane Molecule

109.5

H

Electron diffraction and spectroscopic studies have verified this structure in all respects, giving the following

measurements for the molecule : bond angles, 109.5o; C-H length, 1.10 Å; C-C length, 1.53 Å. Similar studies

have shown that with only slight variations, these values are quite characteristic of C-H and C-C bonds and of

carbon bond angles in alkanes.

This set of bond angles and bond lengths still does not limit the molecule of ethane to a single arrangement of

atoms, since the relationship between the hydrogens of one carbon and the hydrogens of the other carbon is

not specified. Different arrangements of atoms that can be converted into one another by rotation about single

bonds are called Conformations. Arrangement I is called the eclipsed conformation and arrangement II is called

its staggered conformation.

H H

H H H H

H H H

H

H H

Sawhorse representation

Eclipsed Staggered

H H H H

H H H

HH H

H

H Newman representation

Eclipsed Staggered

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14. ENVIRONMENTAL

CHEMISTRY

Introduction

In last 2 decades, the study of the phenomena related to the environment has gained enormous importance. Environ-

mental pollution has becomes one of the most important issue of global concern. The branch of chemistry which deals

with the study of various chemical phenomena occurring in the environment is called environmental chemistry. It is

a must disciplinary science which, refer to the study of sources transport, reactions, effect & fate of certain chemical

species on air, water & solid. The accessible components of environment are

(i) Atmosphere

This comprises a blanket of gaseous layer around earth.

(ii) Hydrosphere

This comprises about 96% of earths surface & includes all sources of water like oceans rivers lakes, glaciers,

ground water etc.

(iii) Lithosphere

It refers to earths solid crust containing the outer mineral cover. It comprise soil, minerals, organic matter etc.

(iv) Biosphere

It refers to the domain of living organism in covalent with atmosphere hydrosphere as well as lithosphere.

Thermosphere 85-500 KM

50-85 KM Mesosphere

11-50 KM Stratosphere

0-11 KM Troposphere

Lithosphere

Regions of the atomsphere

Illustration 1.

Name the different rexampleions of the atmosphere along with their altitudes and temperature ranges.

Solution: Troposphere ( 0 – 11 km, 15 to 56°C), stratosphere (11 – 50 km, - 56 to – 2°C), mesosphere

(50 – 85 km, - 2 to - 92°C), thermosphere ( 85 – 500 km, - 92 to 1200°C)

Illustration 2.

What do you mean by “Inversion temperature” in different rexampleions of the atmosphere?

Solution: When we go from one rexampleion of the atmosphere to the next adjoining rexampleion, the

trend of temperature changes from increase to decrease or vice versa. This is called inversion

temperature.

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Sura’s X NEET S CHEMISTRY


6 7

2

6 16

2. The result of ozone hole is

(a) acid rain (B) greenhouse effect

(C) global warming (D) the UV radiations reach to earth

3. Freon is not recommended to be used in refrigerators because they

(a) increase temperature (B) deplete ozone

(C) affect environment (D) affect human

4. Ozone in stratosphere is depleted by

(a) C F (B) C F

(C) CF Cl

(D) C H Cl2 2 6 6 6

5. Peeling of ozone umbrella, which protects us from UV rays is caused by

(a) PAN (B) CO

(C) CFCs (D) Coal burning

ANSWERS TO ASSIGNMENT PROBLEMS

TEST YOUR CONFIDENCE SUBJECTIVE

1. Peroxyacetyl nitrate (PAN) is one of the components of photo chemical smog and it is powerful eye

irritant.

2. Ozone hole implies distribution of ozone layer by the Harmful UV radiations the depletion will virtualy

result.

In creating some sort of holes in the blanket of ozone which surround us. As a result, the harmful

radiations cause skin cancer, loss of sight and also affect our immune system.

3. 1. Damage the leaves of plants and retard the rate of photosynthesis.

2. Nitrogen dioxide is a lung irritant that can lead to an acute respiratory disease in children.

4. 1. It causes respiratory diseases e.g. Asthama bronchitis in human beings

2. It causes irritation to the eyes, resulting in tears and redness.

5. 1. Viable particulate:- They are minute living organisms that are dispersed in atmosphere.

Ex: Bacteria, fungi, moulds, algae etc ….

It may be noted that human being all allergic to some of the fungi found in air. Fungi can also cause

plant diseases

2. Non viable particulate: they are formed by the breakdown of larger materials or by condensation of

minute particles and droplets.

Ex: mists, smoke, fumes and dust.

6. A. It is used to control of malaria and other insect borne disease.

After the war, DDT is used in Agriculture to control the damages caused by insects, weeds and various

crop diseases

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3

2

2

However, due to adverse effects, its use has been banned India and it is no biodegradable and

carcinogenic.

7. Classical Smog Photochemical smog

It occurs in cool humid climate It occurs in warm dry and sunny climate

It is called reducing smog It is called oxidizing smog

8. It is hogly poisonous to living beings because of its ability to block the delivery of oxygen to the organs

and tissues. It binds to hemoglobin complex to form carboxyl hemoglobin (COHb) which is about 300 times

more stable than oxy-hemoglobin complex. In the blood when the concentration of carbon haemoglobin

reaches about 3-4 percent, the oxygen carrying capacity blood uis greatly reduced. This oxygen deficiency,

results in to headache, weak eyesight, nervousness and cardiovascular disorder CO does not combine

with haemoglobin and hence is less harmful as pollutant but it is the main contributor forwards green

house effect & global warming.

9. A. Pesticides: These are a mixture of two or more substances. They are used for killing pests. Pests

include insects, plants pathogens, weeds, mollusks etc….., that destroys the plant crop and spread

diseases

Ex: Aldrin and Dieldrin

Herbicides: These are chemicals specially meant for killing weeds. Ex. Sodium Chlorate (NaClO )

10. The addition of any undesirable material to air, water and soil by a nature source.

11. BOD: Biochemical oxygen demand is defined as the amount of oxygen required to oxidize the pollutants

presents in water.

Water having BOD less than 5ppm is clean water and greater than 17 ppm is polluted water

Photo Chemical smog: It consists of oxides of nitrogen which absorb light and form free radicals.

It is extremely harmful layer is depleted near Antarcrtica and it is called ozone hole.

12. Chemistry and chemical process involving the minimum use and generation of harmful substances is

called green chemistry.

Ex: Earlier tetrachlorothene themes was used as solvents for dry cleaning. This compound is carcinogenic;

therefore it has been replaced by liquefied CO along with a suitable detergent which is less harmful.

13. CFC’S (chloroflurocarbons) that are released in the atmosphere mix with the other atmospheric gases

and when eventually reach the stratosphere, gets broken down by UV radiations as follows

• •CF2Cl

2 → Cl + CF

2Cl

The chlorine radical reacts with ozone and breaks down ozone molecule as follows •

• •Cl + O3

→ ClO + O2

ClO• radical further reacts with atomic oxygen and produces more chlorine radicals as follows

ClO •

+ O → Cl •

+ O2

14. 1. N2( g) + O2( g) → 2NO(g)

2. 2NO( g) + O2( g) → 2NO2 (g)

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15. 1. 2SO2 + O2 → 2SO3

2. SO2 + O3 → SO3 + O2

3. SO2 + H2O2 → 2H2SO4

TEST YOUR CONFIDENCE OBJECTIVE

1.B 2.D 3.D 4.B 5.C 6.C 7.B 8.D 9.A 10.B

11.A 12.D 13.C 14.D 15.D

LEVEL - 1 SUBJECTIVE

1. It is oxidizing in nature.

2. H2SO4 ,HNO3 & HCl

3. Heat from the sun after being absorbed by the earth is remitted by the earth and absorbed by

then radiated back to the earth, thereby warming it.

4. Oil pollution

5. Mixing of soil or rock particles into water is called siltation.

6. Thermal power plants and nuclear plants.

7. Alkyl benzene sulphonates.

CO2

and

8. It removes hardness producing ion viz

Ca2+ & Mg2+ ion.

9. The amount of oxygen consumed by microorganisms in decomposing waste in a sample of sewage water

is called BOD.

10. COD stands for chemical oxygen demand. It is measured by treating the given sample with an oxidizing

agent.

11. Viable particulates are small size living organisms such as bacteria, fungi, moulds etc.

Non viable particulates are formed by disintexampleration of large size materials

example mist, smoke.

12. This is because in other parts of the stratosphere chlorine free radicals combine away but in Antarctica,

the compounds formed are converted back into chlorine free radicals which deplete the O3 layer.

13. During spring season (i.e. in months of September & October), depletion of ozone takes place and after

spring (i.e. in month of November) it is replenished.

14. A tight whirl pool of wind formed in the stratosphere which surrounds Antarctica is called Polar – Vortex.

15. Synthesis of Ibuprofen, dehydrogenation of diethanolamine for production of herbicide and replacement

of CFC’s by CO2 as blowing agent.

16. When the rain falls through polluted air, it comes across chemicals such as gaseous oxides of sulphur

(SO ), oxides of nitrogen (NO ), mist of hydrochloric acids & phosphoric acid etc. These substances x x

dissolve in falling rain making it more acidic than normal with pH ranging between (5.6 − 3.5).

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Harmful effect of acid rain

(i) Most of aquatic animals can not survive when pH is less than 4. Certain fishes die even when the

pH is less than 5.5.

(ii) Acidic water is dangerous for plants leaf pigments are decolourised, acid affects green pigments of

plants. Agricultural productivity is also decreased.

(iii) Metallic surfaces exposed to acid rain are readily corroded. Textile fabrics, paper & leather products

lose their material strength or disintexamplerate by the acid rain.

17. Atmosphere around the earth acts like a glass of the green house chamber. The gases present in the

atmosphere which cause green house effect are referred to as green house gases. The various green

house gases are:

CO2 ,H2O vapours, chlorofluoro carbons and oxides of nitrogen.

The green house gases in the atmosphere form a thick cover around the earth. The earth receives a

large amount of energy from the sun. The IR radiations coming from sun are not absorbed by atmospheric

gases. The earth absorbs these IR radiations of short wavelength. As a result of this the temperature

of earth stands rising. Eventually, earth starts emitting infra red radiations of longer wavelengths. The

partially radiated infra red radiations from the earth are absorbed by

heating of earths atmosphere.

CO2 . This results in excessive

18. The polluted water may contain large amounts of inorganic and organic compounds. Some of these can

be oxidised by dissolved oxygen in the presence of microorganisms.

BOD, is a measure of the dissolved oxygen that would be needed by the microorganisms to oxidise

these compounds. BOD, therefore is a measure of the total contamination caused by compounds which

can be oxidised in the presence of microorganisms.

19. Most of the land pollution is caused by pesticides and other chemicals which are added to the soil to

grow better crops often a pesticides poisons many more organism than those intended. Some of these

poisons pairs through food chains and eventually reach harmful proportions. Solid wastes is another

cause of land pollution.

Pesticides

(a) Insecticides

(b) Fungicides

20. Some of the achievements in this field are as follows:

(i) Development of dense phase, carbon dioxide: Dense phase CO2 has been recently developed chemical

product with amazing characteristics. It has ability to clean everything. It can be used as recyclable

solvent and finds number of applications in food industry.

(ii) Development of fuel cells for cellular phones which can last for the full life time of the phone.

(iii) Development of process involving use of

CO2 as a blowing agent for manufacture of poly styrene

foam. This technology eliminates the use of chloro fluoro carbon as blowing agent.

(iv) Development of safer marine antifouling compound sea-nine that dexamplerades more rapidly than

organotins which persists in marine environment and cause pollution Prob.s.

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x x

21. COD can be found in few minutes whereas BOD requires atleast 5days.

22. CO,NO

& SO

23. Volcanic eruptions, forest fires and pollen grains of flowers.

24. It forms carboxyhaemoglobin (HbCO) with blood.

25. It is because it is formed as a result of photo chemical reaction (i.e in presence of sunlight )

between oxides of nitrogen and hydrocarbons.

LEVEL-I OBJECTIVE

1.C

11.D

2.C

12.B

3.B

13.D

4.A

14.C

5.D

15.C

6.A 7.C 8.D 9.A 10.

LEVEL-II OBJECTIVE 1.A

11.D

2.C

12.D

3.A

13.B

4.A

14.C

5.D

15.D

6.B 7.A 8.B 9.D 10.A

LEVEL-II MULTIPLE ANSWER TYPE

1.B,C,D 2.A,B,C 3.B,C,D 4.A,B 5.A,B

6.A,B 7.A,D 8.B,C 9.B,C,D 10.A,B

LEVEL-II COMPREHENSION

Comprehension-1

1.A 2. 3.A

Comprehension-2

1. B 2. B 3. A 4. C

Comprehension-3

1.B 2.D 3.B 4.C 5.C

* Refer the text for which questions answers not provided.

uvuvu

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