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GOVT. COLLEGE (AUTONOMOUS), RAJAHMUNDRY DEPARTMENT OFCHEMISTRY NEW CBCS SYLLABUS (AKNU)

FOR B.Sc. FIRST YEAR FROM 2016–17 ONWARDSSEMESTER I

INTRODUCTORY GENERAL & ORGANIC CHEMISTRY

GENERAL CHEMISTRY

UNIT -1 THEORY OF QUANTITATIVE ANALYSIS & ATOMIC STRUCTURE,ELEMENTARY QUANTUM MECHANICS

Theory of Quantitative Analysis 8 hrs

Volumetric Analysis:

Principles of volumetric analysis – Standard solution , Indicators , End point, Titration

error, Titration curves.

Types of titrations : 1. Acid – Base titrations , Theories of acid – base Indicators.

Principles and selection of indicators of : Redox titrations, Complexo metric

titrations and Iodo metric titrations.

Gravimetric Analysis:

Principles of gravimetric analysis – Precipitation, Coagulation , Peptization , Co –

precipitation, post precipitation , digestion , filtration and washing of Precipitate , drying

and ignition, precipitation from homogeneous solutions, requirements of gravimetric

analysis.

Additional input: Storage and preservation of solutions in Volumetric analysis.

Atomic Structure and Elementary Quantum Mechanics 6 hrs

Blackbody radiation, Planck's radiation law, photoelectric effect, Compton Effect, de

Broglie's hypothesis, Heisenberg's uncertainty principle. Postulates of quantum mechanics.

Schrödinger wave equation derivation.

Additional input: Shapes of Orbitals.

UNIT- 2 CHEMICAL BONDING and STEREOCHEMISTRY OF CARBON COMPOUNDS

Chemical Bonding 6 hrs

Valence bond theory as applied to ClF3, BrF5, Ni(CO)4, XeF2. Dipole moment and

structure of molecules. Molecular orbital theory - LCAO method, construction of M.O.

diagrams for homo-nuclear and hetero-nuclear diatomic molecules (N2, O2, HCl, CO and

NO). Comparison of VB and MO theories.

Additional input: M.O. diagrams of B2, C2, Ne2, HF molecules.

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Stereochemistry of Carbon Compounds 10 hrs

Molecular representations- a) Wedge, b) Fischer, c) Newman and d) Saw- Horse

formulae.

Optical activity- plane polarized light, optical rotation and specific rotation.

Chiral molecules-definition and criteria (symmetry elements. Definition of

enantiomers and diastereomers. Explanation of optical isomerism with molecules

Glyceraldehyde, Lactic acid, Alanine, tartaric acid and 2, 3-dibromopentane.

D.L and R, 1S configuration: Cahn-Ingold-Prelog rules. Racemic mixture-

racemization and resolution techniques.

Geometrical isomerism with reference to alkenes- cis, trans and E, Z-configuration.

Additional input: Optical Activity and physiological activity of Natural Products.

ORGANIC CHEMISTRYUNIT -3 STRUCTURAL THEORY IN ORGANIC CHEMISTRY 10hrs

Types of bond fission and organic reagents (Electrophilic, Nucleophilic, and free radical

reagents including neutral molecules like H2O. NH3 & AlCl3).

Free radicals, carbonium ions, carbanions. Carbenes, allenes, and nitrenes.

Bond polarization: Inductive effect. Application of inductive effect (a) Basicity of amines

(b) Acidity of carboxylic acids (c) Stability of carbonium ions. Resonance or Mesomeric

effect, application to (a) acidity of phenol, and (b) acidity of carboxylic acids. Hyper

conjugation and its application to stability of carbonium ions.

Types of Organic reactions: (mechanism not required) Addition - Electrophilic,

Nucleophilic and free radical. Substitution -Electrophilic, Nucleophilic and free radical.

Elimination- Examples.

Additional input: sN1,sN2 mechanisms

UNIT – 4 UNSATURATED HYDROCARBONS and ALICYCLIC HYDROCARBONS

Acyclic Hydrocarbons 10 hrs

Alkenes - Preparation of alkenes (a) by dehydration of alcohols (b) by dehydro

halogenation of alkyl halides (c) by dehalogenation of 1,2 dihalides (brief mechanism),

Saytzev's rule. Properties:1) Addition of hydrogen - heat of hydrogenation and stability

of alkenes. 2) Addition of halogen and its mechanism,3) Addition of HX, Markonikov's

rule,4) addition of H2O. 5) HOX,6) H2SO4 with mechanism and 7) addition of HBr in the

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presence of peroxide (anti - Markonikov's addition ). 8) Oxidation -9) hydroxylation by

KMnO4 ,10) OsO4, 11)per acids (via epoxidation )12) hydroboration

Alkadienes - Types of dienes, reactions of conjugated dines - 1,2 and 1,4 addition of

HBr to 1,3 - butadiene and Diel’s - Alder reaction.

Additional input: Ozonolysis, Polymerisation, polymers in daily life

Alkynes - Preparation by 1) dehydrohalogenation of dihalides,2) dehalogenation of

tetrahalides; Properties; Acidity of acetylenic hydrogen (formation of Metal acedtylides).

Preparation of higher acetylenes, Metal ammonia reductions Physical properties.

Chemical reactivity - Electrophilic addition of 1) X2, 2) HX, 3) H2O (Tautomerism), 4)

Oxidation with KMnO4, 5) OsO4, 6) reduction and 7) Polymerization reactions of

acetylene.

Additional input: Ozonolysis

Alicyclic Hydrocarbons (Cyclo Alkanes) 4 hrs

Nomenclature, Preparation by 1) Freunds methods,2) heating dicarboxylic metal salts.

Properties - reactivity of cyclopropane and cyclobutane by comparing with alkanes.

Stability of cyclo alkanes -1) Baeyer's strain theory, 2)Sachse and Mohr predictions and

Conformational structures of cyclohexane.

Additional input: Conformers of cyclo pentane

UNIT -5 BENZENE AND ITS REACTIVITY 6 hrs

Concept of Aromaticity - Aromaticity (definition), Huckel's rule - application to

Benzenoid (Benzene, Naphthalene) and Non - Benzenoid compounds (cyclopropenyl cation,

cyclopentadienyl anion and tropylium cation). Antiaromaticity-examples.

Reactions - General mechanism of Electrophilic substitution, mechanism of nitration.

Friedel Craft's alkylation and acylation.

Orientation of aromatic substitution - Definition of ortho, para and meta directing

groups. Ring activating and deactivating groups with examples (Electronic interpretation of

various groups like NO2 and Phenolic).

Orientation of (i). Amino, methoxy and methyl groups (ii) . Carboxy, nitro, nitrile,

carbonyl and Sulfonic acid groups. (iii) . Halogens (Explanation by taking minimum of

one example from each type).

Additional input: Hammic and Illingworth’s rules.

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GOVT. COLLEGE (AUTONOMOUS), RAJAHMUNDRY

DEPARTMENT OF CHEMISTRY NEW CBCS SYLLABUS (AKNU)

FOR B.Sc. FIRST YEAR FROM 2016–17 ONWARDS

SEMESTER II

INTRODUCTORY INORGANIC & PHYSICAL CHEMISTRY

INORGANIC CHEMISTRY

UNIT - 1 ORGANOMETALLIC CHEMISTRY & S-BLOCK ELEMENTS

Organometallic Chemistry 8hrs

Definition and classification of Organo metallic compounds-nomenclature, preparation,

properties and applications of alkyls of I, 2 and 13 group elements (Li,Mg,Al) With special

reference to Grignard reagent (RMgX) and Gilman reagent (R2CuLi).

Additional input : Organo cadmium compounds

S-block elements 4hrs

Hydrides-reducing properties, Alkali metal ions in liquid ammonia, complexation of

alkali metal ions by crown ethers and cryptands, diagonal relationship between Li &

Mg, Be & Al.

Additional input: Special properties of Li.

UNIT- II P-BLOCK ELEMENTS

P-block elements 18hrs

General characteristics of elements of groups 13, 14, 15, 16 and 17 with

special reference to metallic, acidic nature, oxidation states, I.P, E.A., E.N

Group - 13: Synthesis and structure of diborane and higher boranes (B4H10 and B5H9),

Boron-Nitrogen compounds (B3N3H6 and BN), carboranes

Group - 14: C60 and its compounds-Intercalation compounds of graphite, Preparation

and application of Carbides, Silicones and silicates

Group - 15: Preparation and reactions of 1.Hydrazine, 2.Hydroxylamine, 3.

Phosphazenes.

Group - 16: Classification of oxides based on (i) Chemical behaviour and

(ii) Oxygen content- Structures of oxo acids of sulfur.

Group - 17: Classification, preparation and structures of interhalogen compounds-

definition and examples of pseudohalogens.

Additional input: Hydrazoic acid; Polyhalides and their structures.

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PHYSICAL CHEMISTRY

UNIT- 3 FLUID CHEMISTRY

Gaseous State 8hrs

Deviation of real gases from ideal behavior, van der Waal's equation of state, P-V Isotherms

of of carbon dioxide. Critical phenomena. The van der Waal's equation and the critical

state (Relationship between critical constants and vander Waal's constants). The law of

corresponding stales and reduced equation of states. Joule-Thomson effect. Liquefaction of

gases: i) Linde's method and ii) Claude's method.

Additional input: Cp/Cv ratio, Numerical problems

Solutions 8 hrs

Solutions of liquids in liquids - Raoult's law- ideal solutions, non-ideal solutions. Vapour

pressure - composition curves for ideal and non-ideal solutions. Vapour pressure -

composition and temperature- composition curves of completely miscible binary solutions

(Azeotropes-HCl-H2O, ethanol-water systems) - fractional distillation. Partially miscible

liquids-phenol-water, tri methyl amine-water, nicotine-water systems. Effect of impurity on

consulate temperature. steam distillation. Nernst distribution law and its applications.

Solutions of gases in liquids- Henry's law.

Additional input: Types of Solutions

UNIT - 4 SURFACE CHEMISTRY and SOLID STATE CHEMISTRY

Surface Chemistry 6hrs

Definition of colloids. Solids in liquids (sols), preparation, properties -kinetic, optical,

electrical. Stability of colloids, Hardy-Schulze law, protective colloid. Liquids in liquids

(emulsions) preparation, properties, uses. Liquids in solids (gels) preparation, uses.

Adsorption: Physical adsoption, chemisorption. Freundlich, Langmuir adsorption isotherms.

Applications of adsorption

Additional input: Factors effecting adsorption.

Solid State Chemistry 8 hrs

Types of Solids-symmetry in crystal systems-space lattice and unit cell- Bravias lattices-

crystal systems -law of rational indices-Miller indices-interplanar spacings in a crystal

system-X-ray diffraction- Bragg’s equation; Quasi crystals.

Defects in crystals-point and line defects; Schottky and Frenkel defects.

Additional input: Color centers.

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GOVERNMENT COLLEGE (A), RAJAHMUNDRY

B.Sc. SECOND YEAR CHEMISTRY SYLLABUS(With effect from the academic year 2016-2017)

III SEMESTER SYLLABUSAdvanced General Chemistry & Advanced Organic Chemistry

Module—I (Advanced Organic Chemistry-I)

I.HALOGEN COMPOUNDS: 4 hrs Nomenclature and Classification of Alkyl halides into:

a. Primary, Secondary, Tertiary.b. Aryl, aralkyl,allyl,vinyl,benzyl halides.

Chemical reactivity of alkyl halides. Formation of RMgX Classification of Nucleophilic Substitution reactions of alkyl halides into SN1 and SN2. Mechanism and Energy profile diagram of SN1 and SN2 reactions. Stereochemistry of SN2 (Walden Inversion) and SN1 (Racemisation) reactions by taking theexample of optically active alkyl halide, 2-Bromobutane. Comparison of reactivity of alkyl halides with:

a. Benzyl b. Allyl c. Vinyl and d. Aryl halides (with respect to Hydrolysis).ADDITIONAL INPUT: Nucleophilic Aromatic Substitution-

Bimolecular Displacement mechanism.II. HYDROXY COMPOUNDS: 6 hrs

Nomenclature and Classification of Hydroxy compounds Preparation of Alcohols: a. Hydroboration reaction.b. Grignard synthesis of alcohols

Preparation of Phenols : a. From diazonium salt.b. From aryl sulphonates.

c. From cumene. Physical properties of alcohols:

a. Hydrogen bonding (Inter and Intramolecular) with two examples.b. Effect of hydrogen bonding on boiling point and solubility in water.

Chemical properties:a. Acidic nature of phenols by taking phenol as an example.b. Formation of alkoxides and phenoxides – their reaction with RX.

(WITHOUT MECHANISM)c. Replacement of –OH group of alcohols:

1. by –X using PC15, PCl3, PBr3, SOC12 and with HX /ZnCl2. (The above reactions without mechanisms)

d. Esterification of alcohols by carboxylic acids. (WITH MECHANISM)e. Oxidation of alcohols by CrO3 and KMnO4

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f. Dehydration of alcoholsg. Special reactions of Phenols:

1. Bromination 2. Kolbe – Schmidt reaction 3. Riemer – Tiemannreaction. (BOTH WITH MECHANISMS)

4. Azo Coupling 5. Fries Rearrangment. (WITHOUT MECHANISM) Identification of primary , secondary and tertiary alcohols with KMnO4 and Lucasreagent, Ceric ammonium nitrate. Identification of phenols (taking phenol as an example) by rection with neutral

FeCl3

Pinacol – Pinacolone rearrangement (WITH MECHANISM).

ADDITIONAL INPUT:1. Preparation of o- & p- nitrophenols from phenol by Nitration.

2. Reactions of o- & p- nitrophenols with:a. Bromine water and b. Nitration Mixture.

III CARBONYL COMPOUNDS: 10 hrs Nomenclature of aliphatic and aromatic carbonyl compounds. Structure of the Carbonyl group. Synthesis of aldehydes and ketones:

Synthesis of aldehydes from acid chloride ,Synthesis of ketones from nitriles and from carboxylic acids ,Synthesis of aldehydes and ketones by using 1, 3-dithianes.

Physical Properties:Comparison of MP and BP of carbonyl compounds with analogous alcholos.

Keto-enol tautomerism. Chemical Properties:

a. Comparison of reactivity of carbonyl group in aliphatic aldehydes and ketonesb. Nucleophilic Addition Reactions of aliphatic aldehydes and ketones with:

1. NaHSO3 2. HCN 3. NH2OH 4. PhNHNH2 5. 2, 4 – DNPH6. RMgX 7. Alcohols (Formation of hemi-acetal and acetal)

c. Halogenation of aliphatic aldehydes and ketones using PCl5.(WITHOUT MECHANISM)

d. Base catalysed Reactions:1. Aldol Condensation 2. Cannizzaro Reaction3. Perkin Reaction 4. Benzoin Condensation5. Haloform Reaction

( All the above 5 reactions (WITH MECHANISMS)6. Knoevenagel Reaction

e. Oxidation Reactions:1. Oxidation of aliphatic aldehydes with KMnO4.2. Baeyer – Villiger Oxidation of ketones.( The above two reactions WITHOUT MECHANISMS)

f. Reduction Reactions:1. Clemmensen Reduction 2. Wolf – Kishner Reduction3. MPV Reduction 4. Reduction with LiAlH4 and NaBH4 .(The above four reactions WITHOUT MECHANISMS)

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g. Analysis of aldehydes and ketones with:a. 2 , 4 – DNP test b. Tollen’s test c. Fehling’s testd. Schiff’s test e. Haloform test

ADDITIONAL INPUT: Exercises in Interconversions in the above mentioned topics.IV. CARBOXYLIC ACIDS AND THEIR DERIVATIVES: 6hrs Nomenclature and classification Structure of Mono carboxylic acids. Preparation of carboxylic acids:1. Methods of preparation of mono carboxylic acids by:

a. Hydrolysis of nitriles,amides and esters.b. Carbonation of Grignard Reagents.

(The above two reactions WITHOUT MECHANISMS)

2. Special methods of preparation of aromatic acids by:a. Oxidation of side chain. b. Hydrolysis of Benzotrichlorides.c. Kolbe Reaction.

(The above 3 reactions WITHOUT MECHANISMS) Physical Properties:a. Hydrogen bonding-dimeric associationb. Acidity – Strength of acids with examples of trimethyl acetic acid and trichloro aceticacid.c. Relative differences in the acidities of aromatic and aliphatc acids.Chemical Properties:

a. Reactions involving – H , - OH and - COOH groups.1. Salt formation2. Anhydride formation

3. Acid Chloride formation4. Amide formation.

(All the above 4 reactions WITHOUT MECHANISMS)5. Esterification (WITH MECHANISM)

b. Degradation of Carboxylic acids by:1. Huns – Diecker Reaction. (WITH MECHANISM)2. Decarboxylation by Schmidt Reaction.

(WITHOUT MECHANISM)c. Arndt – Eistert Synthesis. (WITH MECHANISM)d. Halogenation by Hell – Volhard – Zelinsky Reaction.

(WITH MECHANISM)Hydrolysis of carboxylic acid derivatives: acid chlorides, anhydrides, amides and esters.

V. ACTIVE METHYLENE COMPOUNDS: 4 hrs

Acetoacetic ester:

a. Preparation by Claisen Condensation ( WITH MECHANISM).b. Keto – enol Tautomerism.c. Explanation of Acid hydrolysis and ketonic hydolysis.d. Synthetic Applications:

Preparation of :Monocarboxylic acids:(Ex: Propionic acid , n – Butyric acid)Dicarboxylic acids. (Ex: Succinic acid , Adipic acid) Reaction with Urea.

Malonic ester:a. Preparation from acetic acid (WITHOUT MECHANISM).

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b. Synthetic Applications:Preparation of:

1. Monocarboxylic acids. (Ex: Propionic acid , n – Butyric acid)

2. Dicarboxylic acids. (Ex: Succinic acid , Adipic acid)

3. α , β – Unsaturated carboxylic acids. (Ex: Crotonic acid)

c. Reaction with Urea..ADDITIONAL INPUT: Preparation of Ketones from Acetoacetic ester.

( Ex: 2 – Hexanone , 4 – methyl – 2 – pentanone )Module-II Advanced GENERAL CHEMISTRY:

I General Principles of Inorganic qualitative analysis 6hrs

Solubility product, common ion effect,

characteristic reactions of selected anions, -a) Sodium carbonate extract

b) Halides-Chromile chloride reaction c) MnO2/H2SO4 d) AgNO3 test-solubility of the

precipitate for chloride, Bromide ,Iodide

d) Nitrate-Con. H2SO4, Cu turnings/H2SO4 ,Brown ring test

e) Acetate–rubbing test, esterification test f)Borate– BF3 test ,Ethyl borate test

g) Confirmation reactions and elimination of Oxalate ,Tartrate, Phosphate,

Separation of cations into groups, group reagents,

One confirmation test for the following selected cations– Pb ,Cu, Fe, Al, Mn,Zn,Ni, Co,

Ca,Ba,K,Mg,NH4+

Additional input: Importance of Char coal test, Borax bead test in the identification of cationsII Nuclear Chemistry 4hrs1. Introduction on Isotopes, Isobars and Isotones

2. Factors affecting stability of atomic nucleus: mass defect, binding energy, average

binding energy, N/P ratio, magic numbers.3. Radioactivity, natural radioactivity, properties of

radiations. 4. Types of radioactivity decay.

5. Group displacement law 6. Radioactive disintegration series. 7. Rate of radioactive decay, half

– life. 8. Radioactive dating 9. Nuclear reactions: nuclear fission and nuclear fusion with

examples.10. Artificial radioactivity. 11. Applications of radio isotopes

Additional inputs: Nuclear reactor.

III INTRODUCTORY TREATMENT TO:

a. PERICYCLIC REACTIONS: 4 hrsConcerted reactions , Molecular orbital Theory , Symmetry properties of reactant and

product orbitals , HOMO,LUMO. Types of pericyclic reactions – Electrocyclic , Cycloaddition and Sigmatropic reactions– One example each.

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b. SYNTHETIC STRATEGIES: 4 hrs

Definition of the following terms with one exampleeach: Disconnection (dix) , Symbol ( ) , Synthon ,

Synthetic equivalent , (SE) , Functional groupinterconversion (FGI)Linear , Convergent and Combinatorial syntheses ,Target molecule (TM).

Retrosynthesis of the following molecules:1. Acetophenone 2. Cyclohexene.

ADDITIONAL INPUT: Explanation of [2+2] and [4+2] Cycloadditions with one exampleeach by Frontier Orbital Theory.

IV INTRODUCTORY TREATMENT TO:a) ASYMMETRIC SYNTHESIS: 4 hrs

Definitions of : Asymmetric synthesis , Enantiomeric excess , DiastereomericExcess. Stereospecific reaction – Definition with an example of Dehalogenation of 1,2 –dibromides. Stereoselective reaction – Definition with an example of Acid – catalyseddehydration of 1 – phenylpropanol.

b) MOLECULAR SYMMETRY: 4 hrs Concept of symmetry in chemistry – Symmetry Operations , Symmetry elements. Rotational axis of symmetry and types of rotational axes. Planes of symmetry and types of planes. Improper rotational axis of symmetry , Inversion centre , Identity

element. Identification of point groups.

ADDITIONAL INPUT: One application of stereospecific reaction inPharmaceutical Industry.

Point Groups – C2v (Ex: H2O) , C3v (Ex: NH3)------------o-------------

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GOVERNMENT COLLEGE ( A), RAJAHMUNDRY B.Sc II YEAR CHEMISTRYSYLLABUS

(With effect from the academic year 2016-2017)FOURTH SEMESTER SYLLABUS

(ADVANCED INORGANIC Chemistry & ADVANCED PHYSICAL Chemistry)

Module- I Advanced Inorganic Chemistry

I. CHEMISTRY OF d-BLOCK ELEMENTS:. 7 hrsSpecial characteristics of d-block elements with reference to:

a. Electronic Configuration b.Variable valencyc. Magnetic Properties d. Catalytic Properties e. Colour andf. Ability to form complexes. Comparative treatment of Second and Third Transition series with their 3danalogues with reference to electronic configuration and oxidation states.ADDITIONAL INPUT: Spectral properties of d- block elements.II. CHEMISTRY OF f- BLOCK ELEMENTS: 7 hrs

A. Chemistry of Lanthanides: Special characteristics of lanthanides with reference to:a. Electronic configuration b. Oxidation states c. Lanthanide Contraction –

Consequences of lanthanide contraction and d. Magnetic Properties. Separation of lanthanides by Ion exchange method and solvent extraction.

B. Chemistry of Actinides: Position of actinides in the periodic table. Special characteristics of actinides with reference to:

a. Electronic Configuration b. Oxidation states c. Actinide Contraction andd. Magnetic Properties.

Similarities and differences between lanthanides and actinides

ADDITIONAL INPUT: Applications of lanthanides.

III THEORIES OF BONDING IN METALS: 6 hrs

Free electron Theory , Explanation of thermal and electrical conductivity on the basisof this theory ;It’s limitations. Valence Bond Theory , Explanation of metallic properties on the basis of this theory ;It’s limitations. Band Theory , Formation of bands , Explanation of conductors , semiconductors andinsulators.

ADDITIONAL INPUT: Superconductivity (Elementary Treatment)

IV METAL CARBONYLS AND RELATED COMPOUNDS: 6 hrs

EAN rule – It’s application to any two metal carbonyls , Classification of metalcarbonyls.

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Structures and shapes of metal carbonyls of : Cr - Cr(CO)6, Mn - Mn2(CO)10, Fe - Fe(CO)5 , Co - Co2(CO)8 , Ni – Ni(CO)4

Metallocenes (only ferrocenes) Metal nitrosyls.

ADDITIONAL INPUT: One Method of preparation of V(CO)6 , Cr(CO)6 , Mn2(CO)10 ,Fe(CO)5 , Co2(CO)8 , Ni(CO)4

Module- II Advanced Physical Chemistry

I PHASE RULE: 8 hrs

Definition of the following terms with 2 examples each:a. Phase b. Components c. Degrees of Freedom

Phase rule , Condensed Phase rule. Phase equilibrium of one – component system – Water System. Phase equilibrium of two – component system , solid liquid equilibrium. Simple Eutectic diagram of Pb – Ag system ; Desilverisation of lead. Solid solutions: a. Compound with Congruent melting point.

(Mg – Zn system)b. Compound with Incongruent meiting point.

(NaCl – Water system)

Freezing Mixtures.ADDITIONAL INPUT: Application of phase rule to partially miscible liquid systems.

II. DILUTE SOLUTIONS: 8 hrs Colligative Properties. Roult’s law , Relative lowering of vapour pressure – It’s relation to molecularweight of non – volatile solute ; Experimental determination of relative lowering ofvapour pressure by Ostwald - Walker’s method. Elevation of boiling point and depression of freezing point ; Derivation ofrelation between molecular weight and elevation in boiling point and depression infreezing point. Osmosis , Osmotic pressure ; Experimental determination of osmotic pressureby Berkeley Hartley’s method. Theory of dilute solutions. Determination of molecular weight of non – volatile solute from osmotic pressure. Abnormal colligative properties. Van’t Hoff factor , degree of dissociation and association.

ADDITIONAL INPUT: Some effects of Osmosis and Semipermeability.

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III ELECTROCHEMISTRY-I: 10 hrs

Specific conductance , Equivalent conductance , Measurement of Equivalentconductance , Variation of Equivalent conductance with dilution.

Arrhenius theory and Ostwald’s dilution law. Migration of ions , Kohlrausch’s law. Debye – Huckel’s theory of strong electrolytes. Definition of Transport number , Determination of transport number by Hittorf’smethod. Two applications of Conductivity measurements:

a. Determination of dissociation constant (Ka) of an acid.b. Determination of solubility product of sparingly soluble salt.

Conductometric titrations.

IV ELECTROCHEMISTRY-II: 8hrs

Electrode reactions , Nernst equation , Single electrode potential , Standard Hydrogen Electrode , Reference electrodes – Calomel electrode and Quinhydrone electrode. Standard electrode potential , Sign convention , Electrochemical series and itssignificance. Reversible and Irreversible cells , Conventional representation of electrochemical cells. EMF of a cell and its measurements , Computation of cell EMF , Two applications ofEMF measurements – a. Solubility of a sparingly soluble salt.

b. Valency of ions in doubtful cases. Calculation of thermodynamic quantities of cell reactions. (ΔG , ΔH and K) Potentiometric titrations.

ADDITIONAL INPUT: Types of reversible electrodes.

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GENERAL ELECTIVE PAPER (II B.A., B.Com., B.Sc.)

W.E.F.IV SEMESTER 2015-16

45 HOURS (3HOURS/WEEK) CREDIT 2

Preamble

Chemistry is a practical art. In our everyday life we come across with many utility materials

which all are contributions of Chemistry whether it is food, cloth, drugs, cosmetics and what

not. A common knowledge of all the fundamental chemistry behind these utility products will

enable us to choose what is essential and discard what are harmful to our life. For example, the

cosmetics .These are today, myriads of products in the market, which claims to increase your

quality of life and well being. Are they actually as advantageous as they claim? A study of this

subject will give you information regarding this. What difference in the cleansing property of

toilet soaps - the very costly and moderately priced ones? How the detergents function? What

types of unwanted, nonnutritive chemicals are present in the packed food items, the soft drinks

and the like that are available in the market? The above useful information will be obtained if

you have the chance to study this particular subject offered as an elective paper.

Objectives:

> To know the basics of chemistry in our life

> To know about the food preservatives, Plastics, drugs etc

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GOVT. COLLEGE (AUTONOMOUS), RAJAMAHENDRAVARAMDEPARTMENT OF CHEMISTRY

GENERAL ELECTIVE PAPER (II B.A., B.Com., B.Sc.)IV SEMESTER W.E.F. 2016-17

EVERY DAY CHEMISTRY

45 HOURS (3HOURS/WEEK) CREDIT 2

SYLLABUS

UNIT: I – Basic concepts of Chemistry 12hrs

1.1 About Elements: Total number, naturally occurring, total metals, non-metals, gaseouselements, liquid elements, metalloids, most abundant in earth crust, superlatives in elements-lightest gas, lightest metal, best conductor, most ductile, with high melting point.

Atom-Molecule-Ion, Symbol–Formulae, Element-Compound –Mixture, Physical and ChemicalProperties, Physical change and Chemical change, Exothermic-Endothermic reaction, AtomicWeight- Molecular Weight, Chemical equation and its significance.

1.2 Laws of Chemical combination: Law of Conservation of Mass, Law of DefiniteProportion, Law of Multiple Proportions, Definitions of Mole, Avogadro number, Gram MolarVolume.

1.3. Types of Chemical reactions: Chemical Combination (Synthesis), Decomposition,Displacement, Double Displacement, Photo Chemical Changes, Combustion, Reversible andirreversible reactions.

1.4 Distinguish between chemical terms: Gas-Vapour, Metal-Non-metal-Metalloid,Oxidation – Reduction, Solvent – Solute, Un Saturated – Saturated– Super Saturated Solution,Oil–Fat, Soap- Detergent, Acid–Base, Strong Acid-Weak Acid, Strong Acid–Concentrated Acid,Alloy–Amalgam, Metal–Non Metal, Metal–Metalloid, Dry Ice–Wet Ice, Water Gas– ProducerGas, Mono Saccharide– Poly Saccharide, Ideal Gas–Real Gas, Hard Water–Heavy Water,Temporary Hardness-Permanent Hardness , Evaporation–Sublimation, Nuclear Fission –Fusion, Isotope– Isobar-Isotone.

UNIT: II – Solutions and Mixture Separation Methods 06hrs

2.1 Solutions: Definition, Types of Solutions- Gaseous, Liquid, Solid Solutions, Solubility of Gasin Liquid- Henry’s Law, Effect of Temperature on solubility.

2.2 Methods of Separation of Mixtures: Filtration, Sublimation, Distillation, Fractionaldistillation, Steam distillation, Crystallization, Solvent extraction.

UNIT: III – Industrial Chemistry 17hrs

3.1 Metallurgy: Ore-Mineral, Calcination- Roasting, Flux, Slag, Alloys-Composition of Brass,Bronze, Bell Metal-Gun Metal, Nichrome–Invar, Wrought Iron- Cast Iron ,Stainless steel, Solder,Uses.

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3.2 Chemicals used in medicines: Drug definition, With one examples each andPhysiological importance of each type of Some important drugs : Analgesics, Tranquilizers,Antiseptics, Disinfectants, Antimicrobials, Anti fertility drugs, Antibiotics, Antacids,Antihistamines.

3.3 Plastics–Polymers: Classification–natural, synthetic, Thermosetting and Thermoplasticpolymers, Some important polymers- Polyethene, Nylon, Polyesters, Bakelite, Rubber, Plastics indaily use, Recycling of plastics, Biodegradable plastics, Environmental hazards of plastics.

UNIT: IV – Chemistry in daily life 10hrs

4.1 General Chemicals used in daily life: Acetylene , Alum, Anti freeze, Aquaregia, Backing

soda, Backing powder, Black lead or plumbago, Bleaching powder, Laundry bleach, Blue vitriol,

Bone black, Boric acid, Cane sugar, Glucose, Carbogen, Carbolic acid, Carborundum, Caustic

soda, DAP, Etching acid, Liquid paper, Formalin, Fruit sugar, Gamaxin, Gypsum, Pop, Gun

powder, Hypo, LPG, Laughing gas, Lime water, Marble, Mica, Asbestos, Marsh gas, Methylated

spirit, Milk of magnesia, msg moth balls, Oil of vitriol, PVC, Phosgene, Red phosphorous, Quartz,

Rectified spirit-Beer, Whisky, Smelling salt, TNT, TEL ,Tincture iodine, Urea, Vinegar, Water gas,

Wood Spirit, Rubbing alcohol, Washing soda, Hydrogen peroxide, Cement, Ceramics, Glass.

4.2 Food Adulterants: Adulterants identification in Milk, Ghee, Oil, Coffee powder, Tea,

Asafetida, Chili powder, Pulses and Turmeric powder, Artificial sweetening agents.

Reference Books:

1) General and Inorganic chemistry Fifteenth edition by P.K. Dutt.

2) Separation methods by M.N. Sastri.

3) University Chemistry Third edition by Bruce H. Mahan

4) Industrial Chemistry by B. K. Sharma.

5) Polymer Science by V. R. Gowariker, N. V. Viswanathan and Jayadev Sreedhar

6) Fundamental concepts of Applied Chemistry by Jayashree Ghosh.

7) Analytical Chemistry by B. K. Sharma.

17

GOVT. COLLEGE (AUTONOMOUS) , RAJAMAHENDRAVARAMDEPARTMENT OF CHEMISTRY

NEW CBCS SYLLABUS FOR B.Sc. THIRD YEAREFFECTIVE FROM 2016–17 ONWARDS

Paper – III SEMESTER- V SYLLABUSApplied Inorganic Chemistry and Organic Chemistry

Module-I (Inorganic Chemistry)

1. Coordination Chemistry 10 hrs

IUPAC nomenclature of co – ordination compounds.

Bonding theories of co – ordination compounds –

Review of Werner’s theory and Sidgwick’s concept of coordination

Valence bond theory - geometries of any two complexes with coordination numbers

4 (tetrahedral and Square planar) and 6 (octahedral) –limitations of valence bond

theory.

Crystal field theory - splitting of d-orbitals in octahedral, tetrahedral and square-

planar complexes (with one example each) – low spin and high spin complexes –

factors affecting crystal-field splitting energy - merits and demerits of crystal-field

theory.

Isomerism in coordination compounds – structural isomerism and stereo

Isomerism (with two examples each) - stereochemistry of complexes with 4 and 6 co-

ordination numbers (with two examples each)

2. Stability of metal complexes 4 hrs

Thermodynamic stability and kinetic stability.

Any five factors affecting the stability of metal complexes.

Chelate effect.

Determination of composition of complex by: Job’s method & mole ratio method.

Additional input: Any four factors influencing the complex formation.

3. Spectral and magnetic properties of metal complexes

4hrs

Electronic absorption spectrum of [Ti(H2O)6]3+ ion.

Types of magnetic behavior, spin-only formula, calculation of magnetic moments

(taking any four examples), experimental determination of magnetic susceptibility –

Gouy method.

Additional input: Any four applications of complex compounds.

18

4. Reactivity of metal complexes 4 hrs

Labile and inert complexes (with two examples each) ,

ligand substitution reactions – SN1 and SN2,

Substitution reactions of square planar complexes (with two examples)

Trans effect and applications of trans effect.

5. Hard and soft acids bases (HSAB) 4 hrs

1. Classification of hard and soft acids and bases.

2. Pearson’s concept of hardness and softness.

3. Two applications of HSAB principles – Stability of compounds / complexes, predicting

the feasibility of reaction.

Additional input: Acid base strength of HSAB.

6. Bioinorganic chemistry 3 hrs

Essential elements – definition & classification.

Any four biological functions of Na, K, Ca, Fe, Co, and chloride (Cl-).

Metalloporphyrins – Hemoglobin, structure and function, Chlorophyll - it’s role in

photosynthesis.

Additional input: Cyanocobalamine (Vitamin B12) – functions.

Module-II (Organic Chemistry)1. Nitrogen compounds 9 hrs

Nitro hydrocarbons

Nomenclature, classification and structure of aliphatic nitro hydrocarbons.

Tautomerism of nitroalkanes leading to aci and keto form.

Any two preparations of Nitroalkanes

Reactivity of nitroalkanes –

1. Halogenation (without mechanism).

2. Reaction with HONO (Nitrous acid)- (without mechanism).

3. Nef reaction (without mechanism).

4. Mannich reaction (without mechanism)

5. Mannich reaction leading to Michael addition and Reduction (without

mechanism)

Amines

Aliphatic amines:

I. Nomenclature, Classification into 10, 20, 30 Amines and Quarternary ammonium

compounds.

II. Preparative methods of primary amines: –

19

o For 10, 20, 30 Amines : Reductive amination (without mechanism)

o For 10 Amines :

1. Ammonolysis of alkyl halides (without mechanism)

2. Gabriel synthesis (without mechanism)

3. Hoffman’s bromamide reaction (with mechanism).

III. Chemical properties:

Hinsberg separation of mixture of 10, 20, 30 amines.

Alkylation of primary and secondary amines(without mechanism).

Acylation of primary and secondary amines (without mechanism)

Carbylamine reaction of primary amines (without mechanism)

Reaction with Nitrous acid of 10, 20, 30 (without mechanism)

Oxidation of primary amines (without mechanism)

Aromatic amines

I. Nomenclature, Classification into 10, 20, 30 Amines and Quarternary

ammonium compounds.

II. Preparative methods of primary aromatic amines: –

o Amination of aryl halides (without mechanism)

o From carboxylic acids – Schmidt reaction (without mechanism)

o Hoffman’s degradation reaction – from amides (without mechanism).

III. Chemical properties of primary aromatic amines:

Alkylation (without mechanism).

Acylation (without mechanism)

Carbylamine reaction (without mechanism)

Reaction with Nitrous acid (without mechanism)

Oxidation (without mechanism)

Physical properties and basic character of amines –

Substituent effect (Electron releasing, Electron withdrawing groups) on basicity of

amines taking one example for each substituent group

Steric effect - Comparative basic strength of N-methylaniline and N-ethylaniline

oComparative basic strength of Ammonia, methyl amine, dimethyl amine, trimethyl

amine and aniline.

oComparative basic strength of aniline, N-methylaniline and N,N-

dimethyl aniline (in aqueous medium)

Applications of amines in biological systems

Definition, Two Examples and two functions of the following:

20

Hormones: Adrenalin and noradrenaline.

Neurotransmitters: Dopamine and Serotonine.

Analgesic alkaloids: Morphine and Codeine.

Additional input: Sulphonation of Aniline–Importance of Sulphanilic acid in

Sulpha drugs

2. Heterocyclic Compounds 5hrs

Five - membered ringcompounds

Introduction and definition: Simple 5 - membered ring compounds with

one hetero atom Ex. Furan, Thiophene and pyrrole.

Numbering the ring systems of Furan, Thiophene and pyrrole as per

Greek letter and Numbers.

Aromatic character of Furan, Thiophene and pyrrole – 6- electron

system (four-electrons from two double bonds and a pair of non-bonded electrons

from the hetero atom).

Resonance structures of Furan, Thiophene and pyrrole : Indicating

electron surplus carbons and electron deficient hetero atom.

2. Preparation of furan, Pyrrole and thiophene from 1,4,- dicarbonyl

compounds only (Paul-Knorr synthesis).

Physical properties - Explanation of feebly acidic character of pyrrole.

Chemical properties –

1. Electrophilic substitution of furan, Pyrrole and thiophene at 2 or

5 position - Halogenation, Nitration and Sulphonation under

mild conditions. (with out mechanism)

2. Reactivity of furan as 1,3-diene, Diels Alderreaction

3. Sulphonation of thiophene (withoutmechanism)

Six – Membered rings

Pyridine: 1. Resonance structure of pyridine

2. Basicity of pyridine – Comparison withpyrrole .

3. Any one Electrophilic and one Nucleophilic

Reactions of pyridine. (without mechanisms)

Additional input: Importance of heterocyclic ring system in natural products like

Haemoglobin, Chlorophyll, antibiotics like Penicillins.

21

GOVT. COLLEGE (AUTONOMOUS) , RAJAMAHENDRAVARAMDEPARTMENT OF CHEMISTRY

CBCS SYLLABUS FOR B.Sc. THIRD YEAREFFECTIVE FROM 2016–17 ONWARDS

Paper – III SEMESTER- VI

Applied Physical Chemistry and Organic Chemistry

Module I (Applied Physical Chemistry)

1. Chemical Kinetics: 8 hrs

Rate of reaction, factors influencing the rate of a reaction-concentration, temperature,

light, catalyst.

Any one experimental method to determine the rate of reaction.

Definition of order and molecularity of simple reactions with two examples each.

Derivation of rate constants and time half change for first, second (where 2A

Products i.e; when both reactants are same) and zero order reactions.

Two examples each for first, second and and zero order reactions.

Any one method to determine the order of reactions.

Effect of temperature on rate of reaction, Arrhenius equation, concept of activation

energy.

Theories of reaction rates - collision theory of bimolecular gaseous reactions- The

transition state theory of bimolecular reactions (elementary treatment).

ADDITIONAL INPUT : Order and molecularity of complex reactions.

2. Thermodynamics: 16 hrs Some basic concepts of Thermodynamics –

1. System and surroundings

2. Types of thermodynamic systems

3. Macroscopic system and macroscopic properties

4. State of a system and state variables

5. Extensive and intensive properties

6. Types of thermodynamic processes

7. Reversible and irreversible processes

8. Internal energy and enthalpy

9. State and path functions

The first law of thermodynamics-statement

Heat capacities and their relationship.

Joule’s law

22

Joule-Thomson coefficient.

Calculation of w, q for the expansion of perfect ideal gas under isothermal and

adiabatic conditions for reversible processes.

Temperature dependence of enthalpy of formation-Kirchoff’s equation.

Second law of thermodynamics - Different Statements of the law.

Carnot cycle and its efficiency.

Carnot theorem.

Concept of entropy- entropy as a state function

Entropy changes in reversible, and irreversible processes

Maxwell’s relations

The Gibbs (G) and Helmholtz (A) energies.

Variation of G with P, V and T.

Gibbs - Helmholtz equations – one application of Gibbs - Helmholtz equations

A & G as criteria for thermodynamic equilibrium and spontaneity-advantage over

entropy change.

ADDITIONAL INPUT : Different statements of First law of Thermodynamics.

3. Photochemistry: 5 hrs

Differences between thermal and photochemical processes.

Laws of photochemistry-Grothus-Draper’s law and Stark-Einstein’s law of

photochemical equivalence.

Quantum yield.

Photochemical hydrogen- chlorine, hydrogen-bromine reactions.

Jablonski diagram depicting various processes occurring in the excited state,

qualitative description of fluorescence, phosphorescence, non-radiative processes

(internal conversion, intersystem crossing).

Photosensitized reactions- energy transfer processes (simple example) .

ADDITIONAL INPUT : Applications of fluorescence & Phosphorescence processes.

Module II ( Applied Organic Chemistry)

1. Carbohydrates : 6 hrsMonosaccharides: All discussion to be confined to (+) glucose as an example of aldo

hexoses and (-) fructose as example of ketohexoses.

Structural elucidation of D-(+) glucose

23

Evidences for straight chain pentahydroxy aldehyde structure (Acetylation, reduction to n-

hexane, cyanohydrin formation, reduction of Tollen’s and Fehling’s reagents and

oxidation to gluconic and saccharic acid).

Configuration of glucose based on D-glyceraldehyde as primary standard (no proof for

configuration is required).

Evidence for cyclic structure of glucose (some negative aldehydes tests and mutarotation).

Cyclic structure of glucose.

Decomposition of cyclic structure (Pyranose structure, anomeric Carbon and anomers).

Proof for the ring size (methylation, hydrolysis and oxidation reactions). Different ways of

writing pyranose structure (Haworth formula and chair conformational formula).

Structural Elucidation of Fructose:

Interconversion of Monosaccharides:

Aldopentose to aldo hexose – eg: Arabinose to D-Glucose, D-Mannose (Kiliani -

Fischer method).

Epimers, Epimerisation – Lobry de bruyn van Ekenstein rearrangement.

Aldohexose to Aldopentose eg: D-glucose to D-arabinose by Ruff’f degradation.

Aldohexose (+) (glucose) to ketohexose (-) (Fructose) and Ketohexose (fructose) to

aldohexose (Glucose).

ADDITIONAL INPUT : Disaccharide – Sucrose (Elementary treatment).

2.Biomolecules:Amino acids and proteins – Nucleic acids 6 hrsAminoacids

Introduction:

Definition of Amino acids.

Classification of Amino acids into :

1. Alpha, beta, and gama amino acids.

2. Natural and essential amino acids – definition and examples,

3. Classification of alpha amino acids into acidic, basic and neutral amino acids

with two examples each.

Methods of synthesis:

General methods of synthesis of alpha amino acids (specific examples – Glycine, and

leucine) by following methods:

a) From halogenated carboxylic acid (without mechanism)

b) Malonic ester synthesis (without mechanism)

c) Strecker’s synthesis. (without mechanism)

24

Physical properties:

Optical activity of naturally occurring amino acids: L-configuration, irrespective of

sign rotation

Zwitterion structure – salt like character

solubility, melting points, amphoteric character

Definition of isoelectric point.

Chemical properties:

Two reactions of alpha aminoacids involving both amino and carboxyl groups – Action

of heat, action with metallic ions. (without mechanism)

Peptides and Proteins -

definition and primary structures with two examples each.

Nucleic acids – Elementary treatment:

Definition and two examples of the following:

Nucleic acids

Nucleosides

Nucleotides

Nitrogen bases

ADDITIONAL INPUT : Importance of amino acids in biological systems.

3. Mass Spectroscopy: 5 hrs

Basic principles–Molecular ion /parent ion, fragment ions/daughter ions.

Theory – formation of parent ions.

Representation of mass spectrum.

Identification of parent ion, (M+1), (M+2), base peaks (relative abundance 100%)

Mass spectra of ethylbenzene, acetophenone.

ADDITIONAL INPUT : Instrumentation of mass spectroscopy (Elementary treatment).

-------s-------

25

GOVERNMENTCOLLEGE (AUTONOMOUS) - RAJAHMUNDRY

B.Sc.III YEAR CHEMISTRY,2016-17

ELECTIVE –I Paper IV - SEMESTER - V - SYLLABUS

Paper IV (Elective I)-SEMESTER-V- SYLLABUS

Chemistry and Industry

Unit – I( Spectrophotometry , Molecular Spectroscopy )

1. Spectrophotometry: 4 h

General features of absorption – spectroscopy.

Beer-Lambert’s law and its limitations, transmittance, Absorbance, and molar absorptivity.

Single and double beam spectrophotometers – block diagrams

Application of Beer-Lambert law for quantitative analysis of

1. Chromium in K2Cr2O7 2. Iron (III) with thiocyanate.

3. Manganese in manganoussulphate

ADDITIONAL INPUT :Different detectors – elementary treatment.

2. Molecular spectroscopy 14 h

(i ) Electronic spectroscopy:

Interaction of electromagnetic radiation with molecules .

Types of molecular spectra.

Potential energy curves for bonding and antibonding molecular orbitals.

Energy levels of molecules (σ,π, n) .

Selection rules for electronic spectra.

Types of electronic transitions in molecules.

Effect of conjugation.

Concept of Chromophore and Auxochrome

(ii) Infra red spectroscopy:

Energy levels of simple harmonic oscillator.

Molecular vibration spectrum.

Hooke’s law and determination of force constant.

Selection rules.

26

Modes of vibrations in polyatomic molecules.

Characteristic absorption bands of various functional groups.

Finger print nature of infrared spectrum.

(iv) Proton magnetic resonance spectroscopy:

Principles of nuclear magnetic resonance.

Equivalent and non-equivalent protons.

Position of signals.

Chemical shift.

NMR splitting of signals.

Spin-spin coupling, coupling constants.

Applications of NMR with suitable examples –

i. ) Ethyl bromide ii.) Ethanol iii.)Acetaldehyde iv.) Toluene

v.) Acetophenone.Vi.)1,1,2- tribromoethane vii.) Ethylacetate

ADDITIONAL INPUT: Simple problems in NMR spectroscopy.

UNIT :II PETROCHEMICALS 5h

Definition of petrochemicals.

Petroleum composition – nature of crude oil – fractional distillation of crude oil-different

fractions and their uses.

Cracking – thermal and catalytical

Knocking – Octane number and Cetane number-aviation gasoline – kerosene

Composition of LPG

Classification of petrochemicals -1st ,2nd and 3rd generations with examples and uses.

Unit-III: (Macromolecules, Food Adulteration & Qualitative Food Analysis )

1. Macromolecules: 10h

Classification of polymers

Chemistry of polymerization ---

i.) Chain polymerization

ii.) Step polymerization

iii.) Co - polymerization.

Tacticity -Definition , types.

Molecular weight of polymers:

---Number average and weight average molecular weight.

27

---Determination of molecular weight of polymers by

i) Viscometry,

ii) Osmometry

iii) Light scattering method.

Preparation and industrial applications:

i.) Polyethylene ii.)PVC iii.) Teflon iv.) Nylon66. V.) Terelene vi.) Polyacrilonitrile

Introduction to biodegradability – PHBV

ADDITIONAL INPUT : Polymerization techniques, Ziegler – Natta catalyst

2. Food Adulteration Qualitative Food Analysis: 12h

Food Adulteration

1) Food adulteration

2) Common food adulterants of main food stuffs

3) Detection or microscopic examination adulterants in some common food stuffs

a) Cereals b) Pulses c) Beverages d)Milk e) Vegetable oils and fats, pure ghee, Sweets g)

Spices and Condiments

4) Food Additives

5) Contamination of food stuffs

6) Sampling of can contents

7) Direct microscopic examination

8) Interpretation of Results

Qualitative Food Analysis:

Introduction – Qualitative analysis – Organic substances, Qualitative analysis, Test for proteins,

Colour test for proteins, Test for carbohydrates.

----------OO---------

28

GOVERNMENT COLLEGE (AUTONOMOUS) -RAJAHMUNDRYB.Sc. III YEAR CHEMISTRY,2016-17

Elective II Paper IV-SEMESTER-V- SYLLABUS

ANALYTICAL METHODS IN CHEMISTRY

Credits: 02 Theory: 45 Hours

Module I: Qualitative and Quantitative Aspects of Analysis: 5 Hours

Sampling, evaluation of analytical data, errors, accuracy and precision. Treatment of analytical data, including error analysis. Types of errors, methods of determining accuracy, their expression, normal law of

distribution if indeterminate errors, statistical test of data; F, Q and t test, rejection of data, and confidence intervals. Classification of analytical methods and the types of instrumental methods.

Module II: Optical Methods of Analysis: 20 Hours

Introduction, Electro-magnetic radiations and Electro-magnetic spectrum

Spectrophotometry: Introduction of Spectroscopy, Spectrophotometry and the spectrum, interaction of

radiation with matter, General features of absorption – spectroscopy, fundamental laws of

spectroscopy.

Beer-Lambert’s law and its limitations, transmittance, Absorbance, and molar

absorptivity.

Basic principles of instrumentation (choice of source, monochromator and detector) Single and

double beam spectrophotometers – block diagrams

Application of Beer-Lambert law for quantitative analysis of

1. Chromium in K2Cr2O7

2. Iron (III) with thiocyanate.

3. Manganese in manganous sulphate

Infrared Spectrometry:Basic principles of instrumentation (choice of source, monochromator & detector) for single anddouble beam instrument;sampling techniques. Structural illustration through interpretation of data, Effect and importanceof isotope substitution.Flame Photometry: Introduction, General principle of Flame photometry,Applications, limitations and instrumentation.Atomic Absorption Spectroscopy: Basic Theory, Instrumentation, Flame and Non-Flametechniques.

29

Atomic Absorption Spectroscopy: Basic Theory, Instrumentation, Plasma Emission spectroscopy.

Module III: Classification of Electro Analytical Methods: 10 HoursBasic principle of pH metric, potentiometric and conductometric titrations. Techniques

used for the determination of equivalence points. Techniques used for the determination of pKa

values.

Module IV: Separation Techniques: 10 Hours

Solvent Extraction: Classification, principle and efficiency of the technique. Mechanism ofextraction: extraction by solvation and chelation-Technique of extraction: batch, continuous andcounter current extractions. Qualitative and quantitative aspects of solvent extraction: extractionof metal ions from aqueous solution, extraction of organic species from the aqueous andnonaqueous media. Applications – Determination of Iron (III)

Chromatography: Principles of differential migration

Mechanism of separation: adsorption, partition & ion exchange-

Development of chromatograms: frontal, elution and displacement methods

Nature of adsorbents

Solvent systems

Stationary and mobile phases

Rf values - factors effecting Rf values.

b. Paper Chromatography:

Principles -Experimental procedures -Choice of paper

Developments of chromatogram –i. Ascending ii.Descending iii Radial

iv. Two dimensional

Applications.

c. Thin layer Chromatography (TLC):

Advantages - Principles - factors effecting Rf values- Experimentalprocedures -Preparation of plates-Development of the chromatogram -Detection of the spots-Applications.

*****

30

GOVERNMENT COLLEGE (AUTONOMOUS) - RAJAHMUNDRY .

SEMESTER VI B.Sc.III YEAR CHEMISTRY,2015-16

ELECTIVE - I Paper IV - SYLLABUS

Chemistry and Industry

Unit – I (Physico Chemical methods of analysis)

1. Separation techniques 11 h

2. Solvent extraction:

Principle and process

Batch extraction, continuous extraction and counter current extraction.

Applications – Determination of Iron (III)

3. Chromatography:

Classification of chromatography methods

Principles of differential migration

Adsorption phenomenon

Nature of adsorbents

Solvent systems

Stationary and mobile phases

Rf values - factors effecting Rf values.

a. Paper Chromatography:

Principles -Experimental procedures -Choice of paper

Developments of chromatogram –i. Ascending ii. Descending iii Radial iv. Two dimensional

Applications.

b. Thin layer Chromatography (TLC):

Advantages - Principles - factors effecting Rfvalues- Experimental procedures -Preparation

of plates-Development of the chromatogram -Detection of the spots- Applications.

c. Column Chromatography:

Principle and experimental procedure

Applications

d. High Performance Liquid Chromatography (HPLC):

Principles and Applications.

e. Gas Liquid Chromatography (GLC):

Principles and Applications

Additional input:Dynamics of Chromatography,Reverse phase chromatography

31

Unit – II (Drugs, formulations, pesticides )

1. Drugs : 15 h

1. Introduction:

Drug - disease (definition) -Sources – i.)Plant ii.)Animal iii.) synthetic

2. Terminology:

Pharmacy - Pharmacology – Pharmacophore - Pharmacodynamics - Pharmacokinetics

(ADME, Receptors – brief treatment) - Metabolites and Anti metabolites.

3. Nomenclature:i.) Chemical name ii.) Generic name and iii.) Trade names with examples

4. Classification: Classification based on i.) structures and ii.) Therapeutic activity with one

example each.

5. Synthesis: Synthesis and therapeutic activity of the following drugs:

i.) L-Dopa ii.) Chloroquin iii.) Omeprazole iv.) Ciprofloxacin.

6. Drug Development: Pencillin: Separation and isolation, structures of different pencillins.7. HIV-AIDS: Immunity – CD-4 cells, Retrovirus, replication in human body. Investigation available, prevention of AIDS. Drugs available – examples with structures:PIS: Indinavir (Crixivan), Nelfinavir (Viracept) NNRTIS:

Efavirenz (Susrtiva), Nevirapine (Viramune) NRTIS:Abacavir

(Ziagen), Lamivudine (Epivir, 3TC) Zidovudine

Monographs of drugs: egi.)Paracetamol

2. FORMULATIONS : 3 h

1. Need of conversion of drugs into medicine. Additives and their role (brief account only)2. Different types of formulations3. PESTICIDES: 5 h

1. Introduction to pesticides:

Types – i.)Insecticides ii.)Fungicides iii.)Herbicides iv.) Weedicides v.) Rodenticides

Pheremones and Hormones. - Brief discussion with examples, Structure and uses.

2. Synthesis and present status of the following :

i.) DDT ii.)BHC iii.) Malathion iv.) Endrinv.)Baygonvi.) 2,4-D vii.) Parathion

viii.) Endosulphon

Additional input: Theories of Drugs and their action.

32

4.GREEN CHEMISTRY 5h

Introduction:

Definition of green Chemistry-Need of green chemistry-Basic principles of green chemistry.

Green synthesis:

Evaluation of the type of the reaction.

i) Rearrangements (100% atom economic), ii) Addition reaction (100% atom economic),

iii)Pericyclic reactions (no by-product).

Selection of solvent:i.)Aqueous phase reactions

a) Reactions in ionic liquids.

b) Solid supported synthesis

c) Solvent free reactions (solid phase reactions)

ii.) Green catalysts:

a) Phase transfer catalysts (PTC)

b) Biocatalysts

Microwave and Ultrasound assisted green synthesis:

1.)Aldol condensation 2.) Cannizzaro reaction 3.) Diels-Alder reactions 4.) Willaimson

synthesis 5.) Strecker synthesis 6. ) Dieckmann condensation

ADDITIONAL INPUT :Green house effect, Global warming and its effects,

Pollution control.

Unit-III:

Quantitative Food Analysis 6h

Determination of Moisture, Ash, Crude fat or ether-extract, Soluble extractor, Crude protein,

True protein, Crude fiber, Starch, Analysis of Sugars (Carbohydrate), Estimation of Sucrose in a

given sample of cane sugar, Determination of Phosphorous in plant or food material, Destruction

of organic matter, Important points, Determination of total Na, K, Ca and Mg in food materials

by flame photometry.

********

33

GOVERNMENT COLLEGE(A) RAJAHMUNDRYSEMESTER-VI B.Sc.III YEAR CHEMISTRY 2016-17

Paper IV SYLLABUS

(Elective- II) INSTRUMENTAL METHODS OF CHEMICAL ANALYSIS

Credits: 02 Theory: 45Hours

Module I: Molecular spectroscopy: 25 Hours

Electronic spectroscopy:

Interaction of electromagnetic radiation with molecules .

Types of molecular spectra.

Potential energy curves for bonding and antibonding molecular orbitals.

Energy levels of molecules (σ,π, n) .

Selection rules for electronic spectra.

Types of electronic transitions in molecules.

Effect of conjugation.

Concept of Chromophore and Auxochrome

Woodward-Fieser rules

Applications of ultra-violet spectroscopy

Infra red spectroscopy:

Energy levels of simple harmonic oscillator

Molecular vibration spectrum

Hooke’s law and determination of force constant

Selection rules

Modes of vibrations in polyatomic molecules

Characteristic absorption bands of various functional groups

Finger print region of infrared spectrum

Raman Spectroscopy:

Introduction, Theory of Raman Spectra (stoke’s and Antistoke’s lines)

Conditions of Raman Spectroscopy

Raman spectra of Diatomic molecules

Rule of mutual exclusion principle

Applications of Raman spectroscopy

34

Proton magnetic resonance spectroscopy:

Principles of nuclear magnetic resonance.

Equivalent and non-equivalent protons.

Position of signals.

Chemical shift.

NMR splitting of signals.

Spin-spin coupling, coupling constants.

Applications of NMR with suitable examples –

a) Ethyl

bromide b)

Ethanol

c)

Acetaldehyde

d) Toluene

e) Acetophenone.

f) 1,1,2-

tribromoethane g)

Ethylacetate

ADDITIONAL INPUT: Simple problems in NMR spectroscopy.

Module II : Analysis of Samples: 16 Hours

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).Column Chromatography:

Principle and experimental procedure

Applications

Ion Exchange Chromatography:

Introduction, Principle

Cation & Anion exchangers

Applications of Ion Exchange chromatography.

High Performance Liquid Chromatography (HPLC):

Principles andApplications.

35

Gas Liquid Chromatography(GLC):

Principles and Applications

Detection: simple vs. specific (gas and liquid)

Detection as a means of further analysis(use of tags and coupling to IR and MS),

Mass Spectrometry:

Basic principles–Molecular ion /parent ion, fragment ions/daughter ions.

Theory – formation of parent ions.

Representation of mass spectrum.

Identification of parent ion, (M+1), (M+2), base peaks (relative abundance 100%)

Mass spectra of ethylbenzene, acetophenone.

ADDITIONAL INPUT : Instrumentation of mass spectroscopy (Elementary treatment).

MODULE III: Basic principles of Quantitative Analysis: (4 Hours)

Quantitative Analysis by classical methods and instrumentation methods Estimation of metal ions from aqueous solution Determination of composition of metal complexes using Job's method of

continuous variation and mole ratio method. Redox titrations, dichrometry and iodometric titrations.

------------OOO-----------

36

Recommended Text Books and Reference Books

Inorganic Chemistry :

1. Concise Inorganic Chemistry by J.D.Lee

2. Basic Inorganic Chemistry by Cotton and Wilkinson

3. Advanced Inorganic Chemistry Vol-I by Satyaprakash, Tuli, Basu and Madan

4. Inorganic Chemistry by R RHeslop and P.L. Robinson

5. Modern Inorganic Chemistry by C F Bell and K A K Lott

6. University Chemistry by Bruce Mahan

7. Qualitative Inorganic analysis by A.I.Vogel

8. A textbook of qualitative inorganic analysis by A.I. Vogel

9. Inorganic Chemistry by J.E.Huheey

10. Inorganic Chemistry by Chopra and Kapoor

11. Coordination Chemistry by Basalo and Johnson

12. Organometallic Chemistry – An introduction by R.C.Mehrotra and A.Singh

13. Inorganic Chemistry by D.F.Shriver, P.W.Atkins and C.H.Langford

14. Inorganic Chemistry by Philips and Williams, Lab Manuals

15. Introduction to inorganic reactions mechanisms by A.C.Lockhart

16. Theoretical inorganic chemistry by McDay and J.Selbin

17. Chemical bonding and molecular geometry by R.J.Gillepsy and P.L.Popelier

18. Advanced Inorganic Chemistry By Gurudeep Raj

19. Analytical chemistry by Gary D Christian, Wiley India

20. Analytical Chemistry by G.L.DavidKrupadanam, et al, Univ. Press

21. Selected topics in inorganic chemistry by W.D.Malik, G..D.Tuli, R.D.Madan

22. Concepts and models of Inorganic Chemistry by Bodie Douglas, D.McDaniel

and J.Alexander

23. Modern Inorganic Chemistry by William L. Jolly

24. Concise coordination chemistry by Gopalan and Ramalingam

25. Satyaprakash’s modern inorganic chemistry by R.D.Madan.

Organic Chemistry :

1. Organic Chemistry By R T Morrison and R.N.Boyd

2. Organic Chemistry by T.J.Solomons

3. Organic Chemistry by L.G.WadeSr

4. Organic Chemistry by D.Cram, G.S.Hammond and Herdricks

5. Modern Organic Chemistry by J.D.Roberts and M.C.Caserio

6. Text book of Organic Chemistry by Ferguson

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7. Problems and their solutions in organic Chemistry by I.L.Finar

8. Reaction mechanisms in Organic Chemistry by S.M.Mukherji and S.P.Singh

9. A guide book to mechanisms in Organic Chemistry by Peter Sykes

10. Organic spectroscopy by J.R.Dyer

11. Organic Spectroscopy by William Kemp

12. Fundamentals of organic synthesis amd retrosynthetic analysis by Ratna Kumar Kar

13. Comprehensive practical organic qualitative analysis byV.K.Ahluwalia&SumtaDhingra

14. Comprehensive practical organic chemistry: Preparation and quantitative analysis by

V.K.Ahluwalia and Reena Agarwal.

15. Organic Chemistry by Janice Gorzynski

16. Organic Chemistry by Stanley H Pine

17. Fundamentals of Organic Chemistry by John Mc Murray, Eric Simanek

18. Organic Chemistry by Francis A Carey

19. Text book of Organic Chemistry by K.S.Mukherjee

20. Organic Chemistry by BhupinderMeha&Manju Mehta

21. Organic Chemistry by L.G.Wade Jr, Maya Shankar Singh

22. Elementary organic spectroscopy by Y.R. Sharma

23. Chemistry & Industry by Gurdeep R. Chatwal

24. Applied Chemistry by Jayashree Ghosh

25. Drugs by David Krupadanam

26. Pharmacodynamics by R.C.Srivastava, Subit Ghosh

27. Analytical Chemistry by David Krupadanam

28. Green Chemistry – V.K.Ahluwalia

29. Organic Synthesis by V.K.Ahluwalia and R.Agarwal

30. New trends in Green Chemistry –by V.K.Ahluwalia&M.Kidwai

31. Industrial Chemistry by B.K.Sharma.

32. Industrial Chemistry by Banerji

33. Industrial Chemistry byM.G.Arora

34. Industrial Chemistry by O.P.Veramani&A.K.Narula

35. Synthetic Drugs by O.D.Tyagi&M.Yadav

36. Medicinal Chemistry by Ashutoshkar

37. Medicinal Chemistry by P.Parimoo

38. Pharmacology &Pharmacotherapeutics by R.S Satoshkar&S.D.Bhandenkar

39. Medicinal Chemistry by Kadametal P-I & P.II

40. European Pharmacopoeia

41. Vogel’s Qualitative organic analysis.

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Physical chemistry :

1. Physical chemistry A molecular approach by Donald A. Mcquarrie and

John D. Simon.

2. Physical chemistry by G M Barrow

3. Principles of physical chemistry by Prutton and Marron

4. Physical chemistry by Peter Atkins, Julio D. Paula

5. Physical Chemistry by Ira N Levine

6. Elements of Physical Chemistry by Peter Atkins, Julio D. Paula

7. Text book of Physical Chemistry by P.L.Soni, O.P.Dharmarha and Q.N.Dash

8. Solid State Chemistry and its applications by Anthony R. West

9 Text book of physical chemistry by K L Kapoor

10. Thermodynamics for Chemists by S Glasston

11. Chemical Kinetics by K J Laidler

12. An Introduction to Electrochemistry by S Glasston

13. Physical chemistry through problems By S K Dogra

14. Thermodynamics by J Jayaram and J C Kuriakose

15. Introductory Quantum Chemistry by A K Chandra

16. Physical Chemistry by J W Moore

17. Kinetics and mechanism by J W Moore and R G Pearson

18. Fundamentals of photochemistry by K KRohtagiMukharjee

19. Chemical thermodynamics by R P Rastogi and S SMisra

20. Advanced physical chemistry by Gurudeep Raj

21. Physical chemistry by G W castellan22. Physical chemistry by Silbey, Alberty and Bawendi.

23. Elements of physical chemistry by Glasstone and Lewis

24. Text book of physical chemistry by S Glasstone

25. Fundamentals of Molecular spectroscopy by C.N.Banwell and E.M.McCash

26. Nanochemistry by Geoffrey Ozin and Andre Arsenault

27. Catalysis: Concepts and green applications by GadiRotherberg

28. Green Chemistry: Theory and practice by P.T.Anastas and J.C.Warner

29. Polymer Science by Gowriker, Viswanathan and Jayadev Sridhar

30. Introduction polymer Chemistry By G.S.Misra

31. Polymer Chemistry by Bilmayer

32. Kinetics and Mechanism of Chemical Transformations by Rajaram and Kuriacose.

33. Senior practical physical chemistry by Khosla

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