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Patkai Christian College 1

DEPARTMENT OF CHEMISTRY REVISED SYLLABUS FOR B.Sc. CHEMISTRY

Approved by Board of Studies, Chemistry, Meeting held on 2nd November 2012

COURSE STRUCTURE B. Sc. PASS & HONOURS (Credits 30; Marks 600) Semester Course Course Code Course Title Credits

Theory + Practical

Marks Theo. Prac.

1 1 CHM(P&H) 101 General Chemistry 1 4 + 1 70 30 2 2 CHM(P&H) 102 General Chemistry 2 4 + 1 70 30 3 3 CHM(P&H) 205 General Chemistry 3 4 + 1 70 30 4 4 CHM(P&H) 206 General Chemistry 4 4 + 1 70 30 5 5 CHM(P&H) 309 General Chemistry 5 4 + 1 70 30

6 7 CHM(P&H) 310 General Chemistry 6 4 + 1 70 30 B. Sc. HONOURS (Credits 30; Marks 600) Semester Course Course Code Course Title Credits

Theory + Practical

Marks Theo. Pract.

1 1 CHM(H) 103 Advanced Chemistry 1 4 + 1 70 30







SYLLABUS FOR B.Sc. CHEMISTRY (PASS AND HONOURS) COURSES

SEMESTER I CHM (P&H) 101 General Chemistry 1 100 Marks Physical Chemistry Unit 1: Thermodynamics- I 10 hours

Types of systems, thermodynamics process, first law of thermodynamics, heat capacity, heat capacity at constant volume and pressure and their relationship, Joule Thompson effect and coefficient, inversion temperature. Thermochemistry: standard state, standard enthalpy of formation – Hess’s Law of heat summation and its application, enthalpy of neutralization, bond dissociation energy and its calculation from thermo-chemical data, temperature dependence of enthalpy: Kirchoff’s equation (derivation and application). (Numerical problems based on the topics).

Unit2: Gaseous States –I 10 hours

Postulates of kinetic theory of gases, deviation of real gas from ideal behaviour, van der Waals and Viral equation of state, Critical phenomena, principle of corresponding states, equation of reduced states; liquefaction of gases, distribution of molecular speeds, collision between molecules in a gas- collision diameter, collision number, collision frequency, mean free path, specific heat of solids.

Inorganic Chemistry Unit 3: 10 hours

(a) Atomic Structure Idea of de Broglie matter waves, Heisenberg uncertainty principle, Schrödinger

wave equation (derivation not required), significance of ψ and 2ψ , quantum

numbers, atomic orbitals, shapes of s, p, and d orbitals. Aufbau and Pauli exclusion principles, Hund.s multiplicity rules. Electronic configurations of the elements, effective nuclear charge.

(b) Periodic Properties: Atomic and ionic radii, periodic trends in ionic radii, ionization

energy, factors determining ionization energies, variation of ionization energies in the periodic table, electron Affinity, variation of electron affinity, successive electron affinities, electronegativity: definition, method of determination (Allred and Rochow`s method and Mulliken`s method), trends in periodic table and applications.

Unit 4: Ionic Bond 10 hours

Lewis dot symbols, formation of ionic bond, energy of ionic bond formation, general properties of ionic compounds (physical and chemical), proof for the ionic nature of compounds, structure of ionic crystals, radius ratio rules and its limitations, hydration energy and factors influencing hydration energy, Born-Lende equation, Born-Haber cycle w.r.t. NaCl, trends in lattice energies, applications of lattice energy in estimation of electron affinity, proton affinities, enthalpies and dispropotionation; study of


solubilities, transition ion polarization-polarisation, polarizing power and polarizability, Fajan’s rule, consequence of transition from ionic to covalent bonding, variable electrovalency- unstable electronic configuration of core, pseudo-inert gas configuration, inert pair effect, metallic bond – free electron, valence bond and band theory; factors affecting the shape of molecules, regular and irregular geometries – NH3, H2O, H3O

+, SO4-2, ClO4

-, ClO3-, Ni(CN)4

-2, PF6, ICl2-, SF4, ClF3.

Organic Chemistry Unit 5: 10 hours

(a) Bonding and shape of organic molecules Hybridization of orbitals, implication of hybridization on the concept of bond length, bond angle, shape of molecules (CH4, H3O

+, CH3-, RNH2, C2H4, CH3

+, carbonyl compounds, C2H2, RCN, allene, ketene. Nature of covalent bond and its orbital representation in molecules listed above; conjugation, resonance, hyperconjugation (propene and toluene), homolytic and heterolytic bond cleavage; Reagents- electrophiles, nucleophiles; Reactive intermediates- carbocations, carbanions, free radicals, carbenes and their generation, stability and shape (with examples). (b) Stereochemistry Isomerism- configuration and conformation isomerism; Fischer, Newman and Saw-horse projection formula with suitable example; geometrical isomerism- configuration, E and Z nomenclature, geometric isomers of oximes; configuration – optical activity, chiral carbon atom, relative and absolute configuration, optical isomerism of lactic and tartaric acids, enantiomerism and diastereomerism, meso compounds, racemic mixture, resolution of racemic mixture.

Unit 6: Alkanes and Cycloalkanes 10 hours

IUPAC nomenclature, classification, isomerism in alkanes, sources, and methods of preparation ( with special reference to Wurtz, Kolbe., Corey.House, reactions and decaroxylation of carboxylic acids). Physical properties and chemical reactions of alkanes. Mechanism of free radical halogenation of alkanes. Cycloalkanes: nomenclature, methods of preparations, chemical reactions. Bayer’s strain theory and its limitations. ring strain in cyclopropane and cyclobutanes. Theory of strainless rings. Cyclohexane - chair and boat conformations, axial and equatorial bonds, Newman projection and Saw horse formulae, Fischer and Flying wedge formulae. Conformation of mono substituted cyclohexanes.

Inorganic Chemistry Practical 15 hours Part 1: Macro/semi-micro qualitative analysis of salt mixture including one interfering radical. Part 2: Separation of cations by paper chromatography. Preparation of ferrous alum.


SEMESTER II CHM (P&H) 102 General Chemistry 2 100 marks Physical Chemistry Unit 1: Liquid state I 10 hours

Liquid states: Intermolecular forces – dipole-dipole, dipole-induced dipole, London forces, hydrogen bonding (inter and intra bonding), structure of liquids (a qualitative description), Liquid crystals: Difference between liquid crystal, solid and liquid. Classification, structure and properties of smectic, nematic and cholestic phases. Thermography.

Unit 2: Colloids, Adsorption and Catalysis 10 hours

Colloids: Definition, classification of colloids. Solids in liquids (sols): properties- Kinetic, optical and electrical ; stability of colloids, protective action, Hardy-Schulz law, gold number. Liquids in liquids (emulsions) types of emulsions, preparation. Emulsifier. Liquids in solids (gels): classification, preparation and properties, inhibition, general applications of colloids. Adsorptions: Theories of adsorption – Freundlich and Langmuir adsorption isotherm (derivation and limiting cases), ion exchange adsorption and its application. Catalysis: Characteristics of catalysed reactions, types of catalysis with examples, theories of catalysis, acid base catalysis, mechanism of enzyme catalyzed reaction- Michaelis Menten equation.

Inorganic Chemistry Unit 3: Chemical Bonding 10 hours

Covalent bond- theories of bonding (VBT and MOT), VBT- formation and properties of covalent bond, types of orbital overlap – sigma bond (H2O, NH3), Pi bond (O2, N2), representation of bonds, dot and cross diagrams for diatomic molecuules like HCl, H2O, CO2, PCl3, CH4, hybridization of orbitals (sp, sp2, sp3, sp3d, d2sp3, sp3d2, sp3d3) bond pair and lone pair, VSEPR theory (SF4, ClF3, ICl4

-), partial ionic characters of covalent bonds (from dipole moment and electronegativity), polarity trends- molecules and ions BeCl2, BCl3, CH4, PCl5, SF6, IF7, percentage of ionic character, directional bonding, resonance in inorganic molecules- resonance and molecular properties (O3, N2O, NO3

-, SO3, SO2), polar interactions (ion- induced dipole, dipole – induced dipole, dipole – dipole, ion – dipole), H bonding, van der Wall’s forces; MOT for homonuclear and heteronuclear diatomic molecules (H2, N2, O2, F2, CO, NO).

Unit 4: 10 hours

(a) Acids and bases Acids and bases- different concepts and their limitations (Arhenius, Bronsted-Lowry, Solvent System, Lewis), substituent’s effect on strength of acids and bases, leveling solvent, classification of acids and bases as Hard and Soft, Pearson’s HSAB principle and application, symbiosis, basis of hard-hard and soft-soft interactions.


(b) Oxidation and Reduction Oxidation, reduction, oxidation states, oxidizing agents, reducing agents, calculation of equivalent weight of oxidizing and reducing agents, balancing redox reactions, study of potassium permanganate, potassium dichromate, nitric acid, hydrogen peroxide as oxidizing agents; oxalic acid, sodium thiosulphate ferrous sulphate as reducing agents.


(a) Alkenes and Alkynes Nomenclature of alkenes, methods of formation, Satyzeff’s rule, Hofmann elimination, physical properties and stabilities of alkenes, chemical reactions of alkenes – mechanisms involved in hydrogenation, electrophilic and free radical additions, Markovnikoff’s rule, hydroboration-oxidation, epoxidation, ozonolysis, hydration, hydroxylation and oxidation with KMnO4, polymerization of alkenes.

(c) Arenes and Aromaticity Nomenclature of benzene derivatives. The aryl group, Aromatic nucleus and side chain, Structure of benzene molecular formula and Kekule’s structure. Stability and carbon-carbon bond lengths of benzene, resonance structure, MO picture. Aromaticity: Huckel rule, aromatic ions, Aromatic electrophilic substitution- Mechanism of nitration, halogenation. Sulphonation, Friedel-Crafts reaction, effect of substituents (activating and deactivating substituents, direct influence).

Unit 6: 10 hours (a) Organic reaction mechanism

Generation, reactions and stability of free radicals, carbocations, carbanions, carbenes, nitrenes and benzynes; electrophiles and nucleophiles; SN1, SN2, factors affecting substitution reactions (structures of substrate, nature of nucleophile, solvent, role of leaving group), mechanism of nucleophilic substitution reaction of alkyl halides- SN1 and SN2; differences between nucleophiles and bases; elimination reactions- orientation (Satyzeff’s and Hoffmann’s rule).

(b) Alkyl halides Nomenclature and class of alkyl halides, methods of formation, chemical reactions (hydrogenolysis, aqueous KOH and alcoholic KOH, NH3, KCN, AgCN, KNO3, AgNO2, RCOOAg, RONa, Mg, Li, Na. Polyhalogen compounds ( Chloroform, Carbon tetrachloride).

Organic Chemistry Practical 15 hours Systematic qualitative analysis of organic compound with two functional groups.

1. Detection of elements (N, S, Cl, Br, I) 2. Detection of functional group (carbonyl, carboxyl, phenolic, amino, nitro, sulphonic,

amide) 3. Determination of melting point / boiling point 4. Identification of compounds.


SEMESTER III CHM(P&H)205 General Chemistry 3 Physical Chemistry Unit 1: Phase Rule and its application 10 hours

Phase, component, degree of freedom; derivation of phase rule, phase equilibrium and metastable equilibrium; phase diagram involving one component system (water and sulphur); phase equilibria of two components systems, solid-liquid equilibria, simple eutectic Pb-Ag systems and desilverization of silver.

Unit 2: Electrochemistry 10 hours

Electrical transport- conduction in metals and in solution, specific conductance and equivalent conductance, measurement of equivalent conductance, variation of specific and equivalent conductance with dilution, Kohlrausch law, migration of ions, transport number; Arrhenius theory of electrolyte dissociation and its limitations, weak and strong electrolytes, Ostwald’s dilution law – uses and limitations.

Inorganic Chemistry Unit 3: s-Block Elements 10 hours

Introduction, lattice energy, comparison between lattice energy and heat of formation, factors affecting lattice energy of ionic compounds, lattice energy of sulphates, chlorides, nitrates of alkaline earth metals, solubility/insolubility of ionic solids in polar and nonpolar solvents, solubilities of halides of alkali metals and hydroxides and fluorides and fluorides of alkaline earth metal, solubilities of sulphates, oxalates, phosphates of alkali and alkaline earth metals, melting points and boiling points of ionic solids, solvation energy and hydration energy, explanation of properties based on hydration values, hydrides of alkali and alkaline earth metals, variations in properties of s-block elements (atomic radii, reducing character, colors imparted to the flame, metallic character)reactions with water and formation of oxides, basic strength of hydroxides, diagonal relationship (Li-Mg, Be-Al), difference of Li and Be from other elements of the respective group, characteristics of oxides, hydrides, halides, carbonates and bicarbonates, alkyls and aryls of alkali metals and their applications, complexes, roles of Mg+2 and Ca+2 in biological system.

Unit 4: p-Block Elements Part-I 10 hours

Comparative study (of electronic configuration, valency, atomic radii, ionization energies, electronegativities, metallic properties, oxidizing and reducing properties, melting and boiling points), variation in basic and acidic character of hydroxides, diagonal relationship of B and Si, Fajan’s rule, inert pair effect, oxidation states (Sn and Pb, Sb and Bi), similarities and dissimilarities of B and Al, trends in acid and basic nature of oxides of p block, hydrides, halides, relative strengths of BF3, BCl3 and BBr3 as lewis acids, study of following: fullerenes, carbides (types, calcium carbide, silicon carbide), tetrasulphur tetranitride, fluorocarbons.



(a) Aryl halides: Methods of formation of aryl halides, nuclear and side chain reaction, addition-elemination and elimination-addition mechanism of nucleophilic aromatic substitution reactions; synthesis and uses of DDT.

(b) Alcohols and phenols Classification and nomenclature; monohydric alcohols- nomenclature, methods of preparation by reduction of aldehydes, ketones, carboxylic acids and esters (including hydroboration and mercuration); hydrogen bonding, acidic nature, reactions of alcohols, distinction between primary, secondary and tertiary alcohols (Victor Meyer’s test); methods of formation, chemical reactions of ethylene glycol and glycerol; nomenclature, preparation, physical properties and acidic characters of phenol; comparative acidic and properties of alcohol and phenol; resonance stabilized phenoxide ion, reactions of phenols- electrophilic aromatic substitution, acylation, and carboxylation; Gatterman synthesis, Reimer- Tiemann reaction.

Unit 6: 10 hours (a) Aldehydes and Ketones

Nomenclature and structure of the carbonyl group, synthesis of aldehydes and ketones (aldehydes from acid chlorides, ketones from nitriles and from carboxylic acid). Chemical reactivity of carbonyl group, general mechanism of nucleophilic additions and addition-elemination reactions, reactions with HCN, NaHSO3, NH2OH, NH2NH2, C6H5NHNH2, NH2CONHNH2, and Cannizzaro reaction; Perkin condensation, condensation with ammonia, oxidation of aldehydes, oxidation of ketones, Clemmensen reduction, Wolf Kishner reductions.

(b) Ethers and Epoxides Nomenclature of ethers and methods of their formation, physical properties; chemical reactions, cleavage and auto-oxdation; Ziesel’s method (ethoxy and methoxy estimation).

Physical Chemistry Practical 15 hours

(i) Determination of heat of neutralization of strong acid by strong base. (ii) Determination of molecular weight by Rast’s method. (iii) Study of heat of dilution of H2SO4 and to determine the strength of an unknown

acid (iv) Determination of velocity constant of reaction between hydrogen peroxide and

potassium permanganate using ferric chloride as catalyst. (v) Determination of solubility of salt (BaCl2/Benzoic acid) at two different

temperatures and to determine heat of solution. (vi) Study of adsorption of oxalic acid on charcoal and verification of Fruendlich’s

adsorption isotherm. (vii) Verification of Hardy-Schultze law: preparation and coagulation of arsenic

sulphide (As2S3) sol using NaCl, BaCl2 and AlCl3 solutions.


SEMESTER IV CHM (P&H)206 General Chemistry 100 marks Physical Chemistry Unit-1: 10 hours

(a) Chemical Kinetics Chemical kinetics and its scope, rate of a reaction, factors influencing the rate of a reaction- concentration, temperature, pressure, solvent, light, catalyst concentration dependence of rates, mathematical characteristics of simple chemical reactions- zero order, pseudo order, half life and mean life Determination of the order of reaction differential method, method of integration, method of half life period and isolation method.

(b) Macromolecules Characteristics of macromolecules, concept of number average and mass average molecular weight. Determination of molecular weight of macromolecules.

Unit 2: 10 hours (a) Thermodynamics-II

Second law of thermodynamics- need of the law, different statements; Carnot cycle and its efficiency, Carnot theorem, Thermodynamic scale of temperature- statement, derivation; entropy - as a state function, as a function of V & T, as a function of P & T; entropy change for a spontaneous process in a physical change, Clausius inequality, entropy as a criteria of spontaneity and equilibrium, entropy change in ideal gases and mixing of gases.

(a) Solid State

Definition of solid, amorphous solids, properties of solids, (heterogeneity, anisotropy, double refraction, melting, sublimation, rigidity, thermoluminescence, fluorescence-phosphorescence,pyro-piezoelectricity, atomic heat etc.), first law and second law of crystallography, weiss indices Miller indices, equation of plane, parallel planes, elements of crystals, third law of chrystallography, elements of symmetry, unit cells, space lattice, density of solids in term of edge lengths.

Inorganic Chemistry Unit 3: p-Block Elements Part-II 10 hours

Hydrides: structure of diborane,Study of: Borazine (preparation from diborane, borazole, borontrichloride; reaction with water, addition and substitution reactions, and structure), silicates (structure, classification, feldspar, zeolites, ultramarine), basic properties of halogens, piculiarities of fluorine, interhalogen compounds structure, preparation, uses(AX – ICl, IBr, AX3- ICl3, BrF3, AX5- IF5, AX7- IF7), polyhalides.

Unit 4: Noble Gases 10 hours

Introduction, discovery, separation and isolation from liquid air by fractionation method, properties (molecular ions, clathrate formation,boiling point, uses) chemistry of Xe, study of the following compounds: XeF2, XeF4, XeF6, XeO3, XeOF4, structure and bonding in Xe compounds.



(a) Carboxylic acid and its derivatives Nomenclature, structure and bonding, physical properties, acidity of carboxylic acids, effects of substituents on acid strength; preparation of carboxylic acid, reactions of carboxylic acids, Hell – Volhard – Zelinsky reaction; reduction of carboxylic acids. Structure, nomenclature and preparation of esters, amides (urea), acid anhydride, physical and chemical properties of esters, amides, acid anhydrides; methods of formation and chemical reactions of Malic acid, citric acid.

(b) Active methylene compounds Tautomerism (keto – enol), difference between tautomerism and resonance, synthetic application of diethyl malonate, ethyl acetoacetate, ethyl cyanoacetate.

Unit 6: 10 hours (a) Nitro compounds

General methods of preparation, chemical reaction of nitroalkanes, reduction in acidic, neutral and alkaline media, hydrolysis, reaction with nitrous acid, acidic nature, Picric acid.

(b) Amines Structure and nomenclature of amines, preparation of amines, physical properties, structural features affecting basicity of amines, preparation of alkyl and aryl amines (reduction nitro compounds, nitriles), reductive amination of aldehydes and ketones); Chemical reactivity of alkyl amines, elctrophilic aromatic substitution in aryl amines, reactions of alkyl and aryl amines; characterization of primary, secondary and tertiary amines and their separations, preparation of amines by Gabriel Phthlimide reaction and Hofmann bromide reaction.

Inorganic Chemistry Practical 15 hours Volumetric analysis 1. Estimation of Cl- ion by Mohr`s method 3. Estimation of Cu+2 ion by iodometry 4. Estimation of Fe+2 and Fe+3 by dichromate method 5. Estimation of Zn+2 as Zn(EDTA) by complexation


SEMESTER V CHM (P&H)309 General Chemistry 100 marks Physical Chemistry Unit -1: Gaseous State II 10 hours

Real gases-deviation from ideality, compressibility factor, Maxwell’s distribution law of molecular speeds, molecular speeds and energy distribution as a function of temperature, calculation of most probable velocity, root mean square velocity, average velocity from Maxwell’s distribution law, Maxwell-Boltzmann law of distribution of molecular velocities, degrees of motion, principle of equipartition of energy, viscosity of gases, Boyle temperature, critical phenomena- critical constant, p-v isotherm of CO2, continuity of state, law of corresponding states and reduced equation of state, methods of liquefaction of gases.

Unit 2: Liquid State II 10 hours

Physical properties of liquids – vapour pressure, surface tension, viscocity, refractive index (definition and description), determination of surface tension, viscocity and refractive index of liquids; physical properties and chemical constitution – additive and constitutive properties, molar volume, parachore, specific and molar refraction; polar and non polar liquids, dielectric constant.

Inorganic Chemistry Unit-3: Transition Elements 10 hours

Characteristic properties of d-block element, Properties of the elements of the first transition series (electronic configuration, oxidation states, ionic radii, m.pt., b.pt., ionization energies, color, magnetic properties, catalytic properties) their Binary compounds such as Carbides, Oxides and Sulphides (general properties only), preparation and uses of potassium dichromate and potassium permanganate. Chemistry of Elements of Second and Third Transition Series:- General characteristics, comparative treatment with their 3d-analogues in respect of electronic configuration, ionic radii, oxidation states, magnetic behaviour.

Unit-4: 10 hours (a) Coordination Compounds

Complexes, coordination number and geometry. Werner's coordination theory and its experimental verification, effective atomic number concept, chelates, nomenclature of coordination compounds, isomerism in coordination compounds (coordination number 4 and 6), valence bond theory of transition metal complexes.

(b) Metal Carbonyls Pi acid ligands, pi acid complexes, metal carbonyls: bonding, general method of preparation, chemical reactions (substitution reaction, formation of anionic, cationic, carbonyl halides, carbonyl hydrides complexes), structure of some monomeric, dimeric metal carbonyls, effective atomic number rule.


(a) Organometallic compounds Organometallic compounds- formation of Grignard reagent, synthesis of alkanes, alcohols, carboxylic acids, aldehydes, ketones and amines with Grignard’s reagent; organolithium compounds-preparation and synthesis of alkyl lithium.


(b) Amino acids, Peptides and Proteins Classification, structure and stereochemistry of amino acids; acid base behavior, isoelectric point and electrophoresis; preparation and reaction of α-amino acids (Gabriel phthlimide and Strecker’s method); structure and nomenclature of peptides and proteins; classification of proteins.

Unit 6: Carbohydrates I 10 hours Classification and nomenclature; Haworth’s projection formula of D-Glucose; monosaccharides: mechanism of osazone formation, interconversion of glucose and fructose, chain lengthening and chain shortening of aldoses; configuration of monosaccarides (D, L and threo and erythro); conversion of glucose into mannose; formation of glycosides, ethers and esters; cyclic structure of D(+) glucose; mechanism of mutarotation. Organic Chemistry Practical 15 hours

1. Separation of organic compounds by sublimation. 2. Preparation of organic compounds

SEMESTER VI CHM (P&H)310 General Chemistry 100 marks Physical Chemistry Unit 1: 10 hours

(a) Chemical Equilibria Law of mass action, equilibrium constant from thermodynamic derivation of law of mass action, temperature and pressure dependence of equilibrium constants – Van’t Hoff equation, relation between KP and KC, equilibria in homogeneous and heterogeneous system, le Chatelier’s principle, Clausius-Clapeyron equation and its applications.

(b) Photochemistry Introduction, difference between thermal and photochemical process, Beer-Lambert’s law, Laws of photochemistry- Grothus Draper’s law, Stark-Einstein law, Quantum efficiency and quantum yield, Jablonski diagram depicting various process occurring in the excited state, fluorescence, phosphorescence, nonradiative process (internal conversion, intersystem crossing), Photosensitized reactions- energy transfer process (simple example).

Unit 2: Thermodynamics III 10 hours Third law of thermodynamics, Nernst heat theorem, statement and concept of residual entropy, evaluation of absolute entropy from heat capacity data; Gibbs and Helmholtz equation; G and A as thermodynamics quantities, A and G as criteria for thermodynamic equilibrium and spontaneity, their advantage over entropy change, variation of G and A with P, V and T; Trouton’s rule, Clausious Clapeyron equation, derivation of phase rule for the concept of chemical potential, partial molar quantities, variation of chemical potential with T and P, chemical potential of an ideal gas, Gibbs-Duhem equation; application of chemical potential.


Inorganic Chemistry Unit-3: Chemistry of Lanthanides and Actinides 10 hours

Electronic structure, oxidation states and ionic radii and lanthanide contraction, complex formation, occurrence and isolation of lanthanide compounds General features and chemistry of actinides, chemistry of separation of Np, Pu, and Am from U, similarities between the later actinides and the later lanthanides.

Unit 4: Nuclear Chemistry 10 hours

Fundamental particles (electron, proton, positron, neutron, and meson), nuclear binding energy, mass defect and packing fraction, half life and average life period, applications of radioisotopes, unit of radioactivity, group displacement law, balancing of nuclear reaction, artificial radioactivity, elementary idea of fission, fusion, controlled fission reactions, atomic energy and nuclear reactors.


(a) Carbohydrates II Determination of ring size of D-Glucose; structure of ribose and deoxyribose; introduction to dissacharides (maltose, sucrose), their reactions and structures; structure of starch and cellulose, preparation of cellulose nitrate, cellulose acetate, rayon and cellophane.

(b) Synthetic dye Color and constitution (electronic concept); classification of dyes, chemistry and synthesis of methyl orange, congo red, malachite green, crystal violet, phenolphthalein, fluorescein, alizarin and indigo.

Unit 6: 10 hours

(a) Fats oils and detergents Natural fats, edible and industrial oils of vegetable origin, common fatty acids, glycerides, hydrogenation of unsaturated oils, saponification value, soap, synthetic detergents.

(b) Diazo compounds Preparation and stability of diazo compounds (aliphatic and aromatic); reactions of benzene diazonium chloride; preparation and reaction of diazomethane.

Physical Chemistry practical 15 hours

1. To study the kinetics of iodination of acetone. 2. To study the kinetics of second order reaction (saponification of ethyl acetate). 3. Determination of critical solution temperature and composition of the phenol

water system and to study the effect of impurities on it. 4. Determination of enthalpy of hydration of copper sulphate. 5. pH metric titration of (i) strong acid and strong base, (ii) weak acid and strong base.


Books Suggested

1. Madan, R.L. Chemistry for degree students B Sc First year, S.Chand Basic 2. Gopalan, R. Inorganic Chemistry, University Press (India). 3. Chandra, S. Comprehensive Inorganic Chemistry, New age publication, vol. I, vol. II. 4. Aggarwal, R.C. Modern Inorganic Chemistry, Kitab Mahal, Allahabad. 5. Malik, Tuli, Madan, Selected topics in Inorganic Chemistry, S. Chand. 6. Prakash, Tuli, Madan, Basu, Advanced Inrganic Chemistry, S. Chand, vol. I, vol. II. 7. Gurdeep R, Advanced Inrganic Chemistry, Krishna Prakashan, Meerut, vol. I, vol. II. 8. Puri, Sharma, Kalia, Principles of Inorganic Chemistry, Vishal Publication. 9. Cotton, Wilkinson, Gaus, Basic Inorganic Chemistry, John Wiley & Sons, New York. 10. Lee, J.D. Concise Inorganic Chemistry, Chapmann and Hall. 11. Shriver, Atkins, Langford, Inorganic Chemistry, Oxford. 12. Sharpe, A.G. Inorganic Chemistry, Pearson Education. 13. Huheey, J.E. Keiter, E.A. Keiter, R.L. Inorganic Chemistry, Harper Collins. 14. Morrison, Boyd, Organic Chemistry, Prentice Hall. 15. Bahl, A. Bahl, B. Organic Chemistry, S. Chand. 16. Sanyal, S.N. Reactions, Rearrangements and Reagents, Bharati Bhawan, Patna. 17. Kalsi, P.S. Stereochemistry, New Age Internal publisher. 18. Kalsi, P.S. Organic Reactions and their mechanisms, New Age Internal publisher. 19. Jain, Sharma, Modern Organic Chemistry, Vishal Publishing co. 20. Jagadamba, Yadav, Undergraduate organic Chemistry, Pragati Prakashan, Merut, vol. I, vol.

II, vol. III. 21. Jagadamba, Yadav, Advanced organic Chemistry, Pragati Prakashan, Merut. 22. Pillai, C.N. Text Book of Organic Chemistry, University Press. 23. Bruice, P.Y. Organic Chemistry, Prentice-Hall, Interrrnational Edition. 24. Wade, L.G. Organic Chemistry, Prentice Hall 25. Solomons, Fundamentals of Organic Chemistry, John Wilev. 26. Carey, F.A. Organic Chemistry, McGraw-Hill Inc. 27. Streitwiesser, Hathcock, Kosover, Introduction to Organic Chemistry, Macmillan. 28. Mukherji, S.M. Singh S.P. Kapoor, R.P. Organic Chemistry, Wiley Eastern Ltd. (New Age

International) vol. I, vol. II, vol. III. 29. Finar, Organic Chemistry, ELBS and Longman Ltd., New Delhi, vol. I, vol II. 30. Saunders, Organic Polymer Chemistry, Chapman & Hall, London. 31. Sykes, P. A Guide Book to Mechanism in Organic Chemistry, Orient Longman Ltd., New

Delhi.. 32. Puri, B.R. Sharma L.R. Pathania, M.S. Principles of Physical Chemistry, Shoban Lal Nagin

Chand & Co., Jalandhar. 33. Bajpai, Advanced Physical Chemistry, S.Chand and Co. 34. Rastogi, Misra, An Introduction to Chemical thermodynamics, Vikas Publication. 35. Rakshit, Physical Chemistry, Sarat Book House, Calcutta. 36. Barrow, Physical Chemistry, International Student Edition, McGraw Hill. 37. Alberty, Physical Chemistry, Wiley Eastern Ltd. 38. Atkins, The Elements of Physical Chemistry, Oxford. 39. Dogra, S. Dogra, Physical Chemistry Through problems, Wiley Eastern Ltd. 40. Laidler, Meiser, Physical Chemistry, Houghton Mifflin Comp., New York, International

Edition. 41. Levine, Physical Chemistry, Mc Graw-Hill Inc., New York. 42. De, Environmental Chemistry, Wiley Eastern, New Delhi. 43. Arnikar, H. J. Essentials of Nuclear Chemistry, New Age International (p) Ltd., New Delhi. 44. Gurdeep Raj, Advanced Practical Inorganic Chemistry, Goel publishing house. 45. Pandey, Bajpai, Giri, Practical Chemistry, S. Chand. 46. Gutru, Kapur, Advanced Practical Chemistry, S. Chand, vol. I, II, III,.


SYLLABUS FOR B.Sc. CHEMISTRY HONOURS COURSES

SEMESTER I CHM (H)103 Advanced Chemistry 1 Marks 100 Physical Chemistry Unit1: Mathematical Concepts 10 hours

Logarithmic relations, curves stretching, linear graphs and calculation of slopes, Differentiation of functions like Kx, ex, xn, sinx, logx; maxima and minima, partial differentiation and reciprocity relations; Integration of some useful/relevant functions and line integration; permutations and combinations, Factorials, Probability.

Unit 2: Gaseous State 10 hours

Maxwell’s distribution law of molecular speeds, molecular speeds and energy distribution as a function of temperature, calculation of most probable velocity, root mean square velocity, average velocity from Maxwell’s distribution law, Maxwell – Boltzmann law of distribution of molecular velocities, degrees of motion, principle of equipartition of energy, viscosity of gases, Boyle temperature, critical phenomena- critical constants, p-v isotherm of CO2, continuity of state, methods of liquefaction of gases.

Inorganic Chemistry Unit 3. Statistical Evaluation : 10 hours

Significant figures and rounding off of numerical expression, errors, absolute errors, relative errors, determinate errors-instrumental errors, method errors and personal errors, constant errors and proportional errors, methods for minimizing errors, Indeterminate errors, random error distribution curve. Average, deviation, average deviation from mean, standard deviation, relative and standard deviation, accuracy and precision, Testing of results- F-test, t-test, rejection of results- Q-test.

Unit 4. Theory of Quantitative analysis: 10 hours Law of mass action, Chemical equilibria (acid-base, solubility, distribution) and equilibrium constants, ionic product of water, relationship between Ka, Kb and KW, Hydrogen ion concentration and pH, common ion effects, buffer activity, application of solubility product, precipitations, gravimetry, Formation and desirable properties of gravimetric precipitates, Contamination in precipitates - co precipitation, post precipitation, methods for removing impurities in precipitates; Separation and estimation (Fe-Ca, Ca-Ba, and Fe-Cu). Indicators (acid-base, redox, adsorption); Principles of argentometric, complexometric and iodine titration.


Organic Chemistry Unit 5: Introduction to organic synthesis 10 hours

Formation of carbon-carbon bond, electrophilic and nucleophilic carbon species, acid assisted reaction and base assisted condensations (Knoevenagel, Michael, Wittig reaction, Reformatsky reaction, Claisen-Schmidt reaction, Mannich reaction) Formation and acid assisted cleavage of acetals and ketals, mechanism and formation and hydrolysis of esters and amides (acylic and cylic). Use of inorganic reagents in organic synthesis: LiAlH4, NaBH4, B2H6, Na/ liqNH3, Aluminium isopropoxide, KMnO4, HIO4, Lead tetra acetate.

Unit 6: 10 hours

(a) Introductin to Dienes Cojugated, isolated and cumulated dienes (alkenes), structures, preparation and reactions of conjugated dienes (1,3-butadiene and isoprene). (b) Polynuclear Aromatic Hydrocarbons

Introduction, molecular orbital structure of naphthalene, resonance, mechanism and orientation of electrophilic substitution. Preparations and reactions of α- and ß- naphthols (azo-coupling, reactions and with FeCl3). Preparation and properties of anthracene.

(c) Organosulphur Compounds: Nomenclature, structural features, methods of formation and chemical reactions of thiols, thioethers, sulphonic acids, sulphonamides and sulphaguanidine.

Inorganic Chemistry Practical 15 hours

A. Gravimetric eastimation of single component (a) Analysis of Cu as CuSCN (b) Ni as Ni(DMG)2 (c) Zn as ZnO (d) Cr as Cr2O3 (e) Fe as Fe2O3 B. Gravimetric analysis of double components (a) Iron- Calcium (b) Iron copper (c) Copper-zinc (d) Calcium-barium (e) Copper- nickel.


SEMESTER II CHM (H) 104 Advanced Chemistry 2 Marks 100 Physical Chemistry Unit 1: Phase Equilibria 10 hours

Ideal liquid mixtures, azeotropes (ethanol – water system), partially miscible liquids- lower and upper critical solution temperature (phenol –water, trimethylamine-water system), steam distillation (aniline – water system), solid solutions – compound formation with congruent melting point (Mg-Zn) and incongruent melting point, (FeCl3-H2O) and (CuSO4-H2O) system, freezing mixture, acetone-dry ice; Nernst distribution law – thermodynamic derivation, application.

Unit 2: Physical Properties and Molecular Structure 10 hours Optical activity, polarization – Clausius Mossatti equation, orientation of dipoles in electric field, dipole moment, induced dipole moment, measurement of dipole moment – temperature and refractivity method, dipole moment and structure of molecules, magnetic properties – paramagnetism, diamagnetism and ferromagnetism.

Inorganic Chemistry Unit 3: Molecular Symmetry 10 hours

Symmetry elements and symmetry operations: symmetry planes and reflections, inversion center, proper axis and proper rotations, improper axis and improper rotations; molecular point groups; point groups of H2O, NH3, BCl3, H2O2, BeCl2, and R2NH; symmetry of tetrahedron and square planar complexes.

Unit 4: Bio-inorganic Chemistry 10 hours

Essential and trace elements in biological systems, metalloporphyrins, heme proteins (haemoglobin and myoglobin), role of cobalt in vitamin B12, enzymes, metalloenzymes (Zn) and their characteristic and functions; non complexing cations in biochemical processes (Na and K), role of metals and nonmetals in metabolism, Biological role of alkali and alkaline earth metal ions with special reference to Ca++, Nitrogen fixation.

Organic Chemistry Unit 5: Synthetic polymers 10 hours

Addition or chain growth polymerization, free radical vinyl polymerization, ionic vinyl polymerization, Ziegler-Natta polymerization and vinyl polymers. Condensation or step growth polymerization. Polyesters, polyamides, phenol formaldehyde resins, epoxy resins and polyurethanes.

Unit 6: Pericyclic Reactions 10 hours

Definition of pericyclic reactions, molecular orbitals and pericyclic reactions (i) Electrocyclic reactions: Introduction, stereochemistry of electrocyclic reaction,

Conrotatory-disrotatory ring closure and ring opening (with examples 1,4-(2E,4E) hexatriene, 1,4-(2E,4Z) hexatriene, (2E,4Z,6Z) octatriene, (2E,4Z,6E) octatriene. Woodward Hoffmann`s rule for electrolytic reactions, Frontier Molecular Orbital Theory (no correlation diagram required)


(ii) Cycloaddition reaction: Definition of dienes and dinophiles, supra-supra, antara-antara modes of cycloadditions [4+2] Diels-Alder reaction and [2+2] cycloaddition reactions by taking examples of simple dienes and dinophiles.

Organic chemistry Practical: 15 hours

Preparation and purification of organic compounds. 1. Preparationof acetanilide from aniline. 2. Preparation of aspirin from salicylic acid 3. Preparation of benzanilide from aniline 4. Preparation of 2,4,6- tribromophenol from phenol 5. Preparation of methyl orange Recrystallize, find melting point and report yield.

SEMESTER III CHM(H) 207 Advanced Chemistry 3 Marks 100 Physical Chemistry Unit 1: Solid State 10 hours

X-ray diffraction by crystals, Derivation of Bragg’s equation; determination of crystal structure by single crystal method and powder method (NaCl and KCl), typical crystal structures, principles of closest packing, space occupied by particles in bcc, fcc, voids, radius ratio, imperfections in crystals (Frenkel defect, Schottkey defect), liquid crystals.

Unit 2: Chemical Kinetics 10 hours

Kinetic equation for complex reactions: chain, parallel, opposing and consecutive reactions; experimental methods of chemical kinetics – potentiometric, spectrophotometric and optical method; rate constant for simple bimolecular reactions; collision theory; activated complex theory; reactions in solutions: diffusion controlled and activated controlled reactions; thermodynamic formulation of rate constant, expression of rate constant based on equilibrium constants.

Inorganic Chemistry Unit 3 : Metal ligand bonding in transition metal complexes 10 hours

A brief review of Valance Bond Theory, Limitations of valence bond theory, crystal field theory, Crystal field splitting in octahedral, tetrahedral and square planar complexes, high spin, low spin complexes, crystal field stabilization energy, factors affecting the Crystal field parameters, spectrochemical series, Tetragonal distortion, Jahn Teller effect.

Unit 4: Thermodynamics and kinetic aspects of metal complexes 10 hours

A brief outline of thermodynamic stability of metal complexes and factors affecting the stability, substitution reactions in octahedral complexes, SN1 and SN2 mechanism, types of intermediate formed during SN1 and SN2 reactions, labile and inert complexes, factors controlling lability, substitution reactions of square planner complexes, trans effect.


Organic Chemistry Unit 5: Heterocyclic Compounds I 10 hours

Introduction: Molecular orbital picture and aromatic characteristics of pyrrole, furan, thiophene, and pyridine. Methods of synthesis and chemical reactions with particular emphasis on the mechanism of electrophilic substitution. Mechanism of nucleophilic substitution reactions in pyridine derivatives. Comparison of basicity of pyridine, piperidine and pyrrole.

Unit 6: Heterocyclic Compounds II 10 hours

Introduction to condensed five and six-membered heteroeyclic compounds. Preparation and reactions of Indole, quinoline and isoquinoline with special reference to Fischer indole synthesis, Skraup synthesis and Bischler-Napieralski synthesis. Mechanism of electrophilic substitution reactions of indole, quinoline and isoquinoline.


(a) Determination of surface tension of a liquid/ solution by drop-weight method. (b) Determination of viscosity – composition (v/v) curve of ethanol-water system and to

determine the composition (v/v) of a given mixture. (c) Determination of partial coefficient of a solute between two immiscible solvents (e.g.,

iodine in water/ organic solvent; benzoic acid in water/benzene). (d) Determination of velocity constant of the hydrolysis of the methyl acetate catalysed

by an acid. (e) Conductometric titrations of an acid by a base. Acid base titration using

potentiometer. (f) Determination of heat of solution of solid calcium chloride by Born Haber Cycle. (g) Determination of critical solution temperature of the phenol water system. (h) Study of the kinetics of reaction between potassium persulphate and potassium iodide

at two temperatures. (i) Decomposition of hydrogen peroxide using ferric chloride as catalyst and to

determine the activation energy.


SEMESTER IV CHM (H) 208 Advanced Chemistry 4 100 marks Physical Chemistry Unit 1: Thermodynamics of Solutions: 10 hours

Partial molal quantities, chemical potential, the Gibbs-Duhem equation, determination of partial molal quantities, variation of chemical potential with temperature and pressure, chemical potential in case of a system of ideal gases, chemical potential of real gases and fugacity, activity and activity coefficient (concept and physical significance), reference and standard states. Variation of fugacity with temperature and pressure, Lewis-Randall rule, thermodynamic functions of mixing (AGmix , ASmix , AVmix , AHmix).

Unit 2: Statistical Thermodynamics: 10 hours

Limitation of classical thermodynamics, concepts of distribution of energy, thermodynamic probability, Boltzmann distribution law, partition function and thermodynamic parameters; relation between molecular and molar partition function, translational partition function, rotational partition function for linear and non linear molecules, vibrational partition function, electronic partition function, reference state of zero energy for evaluating partition function, equilibrium constants in terms of partition function, heat capacity of solids.

Inorganic Chemistry Unit 3: Magnetic properties of transition metal complexes 10 hours

Explanation of diamagnetism, paramagnetism, ferromagnetism and antiferromagnetism, Curie law, Curie Weiss law, Bohr Magneton; electron spin moment, orbital angular moment, coupling of single electron angular momentum, spin-spin, coupling, orbital coupling, L-S coupling, terms, ground state terms; magnetic susceptibility, methods of determining magnetic susceptibility by Guoy`s method and Faraday method, explaination of magnetic behavior of the following- K4[Fe(CN)6], K3[Fe(CN)6], [Co(NH3)6]Cl3, K2[Ni(CN)4], K3[CoF6], K3[MnF6], Ni(CO)4.

Unit 4: Electron spectra of transition metal complexes 10 hours

Basic concept of electronic spectroscopy of transition metal complexes, Types of electronic transitions: d-d transition, charge transfer transition (Metal to Ligan, Ligan to metal), selection rules for d-d transition: spin selection rule, Laporte selection rule, relaxation of selection rule, Orgel energy level diagram for d1 - d9 states, use of Orgel diagram, discussion of the electronic spectrum of [Ti(H2O)6]

3+, study of spectra of octahedral complexes of d1 to d9 system, Charge transfer spectra.

Organic Chemistry Unit 5: Organic Photochemistry: 10 hours

Molecular energy and photochemical energy, excitation of molecules, Frank-Condon principle, dissipation of energy and Jablonsky diagram and singlet triplet states, photosensitization and quenching, quantum yield. Introduction to photochemical reactions of carbonyl compounds, Patterno-Buchi reaction, Norrish Type I and Type II cleavages, photoreduction.


Unit 6 10 hours (i) Molecular Rearrangements: Carbonium ion rearrangement (Pinacol-pinacolone,

Beckmann, Wolff, Hofmann, Curtius, Benzil-Benzilic acid, Fries rearrangements. (ii) Organic Synthesis via Enolates: Organic Synthesis via Enolates Acidity of α -

hydrogens, alkylation of diethyl malonate and ethyl acetoacetate. Synthesis of ethyl acetoacetate, the Claisen condensation. Alkylation of 1.3-dithianes. Alkylation and acylation of enamines.

Inorganic Chemistry Practical 15 hours Preparation of Inorganic Compounds

a. Tetraamine Cu(II) sulphate b. Hexaamine Ni(II) chloride c. Potassium trioxalato ferrate (III) d. Potassium trioxalato chromate (III) e. Cu(thiourea) complex f. Nitropentaamine cobalt (III) chloride g. Potassium trioxalato chromate (III) h. Potassium chlorochromate

Recrystallize the compound prepared, report yield and verify presence of anoin and cation by qualitative analysis.

SEMESTER V

CHM(H) 311 Advanced Chemistry 5 100 marks Physical Chemistry Unit 1: Quantum Mechanics I 10 hours

Operator, Schrodinger wave equation and solution of �� = �� for particle in 1–D box, normalization and orthogonality of�, postulates of quantum mechanics, Schrodinger wave equation for H-atom, nodes in excited state and calculation of average value <x>, <x2>, <p> and <p2>, hydrogen like wave functions, radial wave functions, angular wave functions.

Unit 2: Quantum Mechanics II 10 hours Molecular orbital theory., basic ideas - criteria for forming M.O. from A.O, construction of M.O.'s by LCAO- hydrogen (H2

+) ion. Calculation of energy levels from wave functions, physical picture of bonding and antibonding wave functions, Concept of �, �∗, , ∗ orbitals and their characteristics. Introduction to valence bond model of H2, comparison of M.O. and V.B. models.


Inorganic Chemistry Unit 3: Organometallic Chemistry 10 hours

Synthesis, structure, bonding and reactivity of transition metal complexes with olifins, cyclopentadienyl, cyclopentadiene, benzenoid, pi-allyl and enyl systems; transition metal -bond: metal-alkyls, metal-carbenes and metal carbines.

Unit 4: Metal Ligand Equilibria in solution: 10 hours Stepwise and Overall formation constants, trends in stepwise formation constants, determination of binary formation constant by spectrophotometry, factors affecting stability of metal complexes and chelate effects.

Organic Chemistry Unit 5: Absorption spectra 10 hours

Ultraviolet absorption spectroscopy: Types of electronic transitions, effect of conjugation, concept of chromophore and auxochrome; Bathocromic, hypsochromic and hypochromic shift; UV spectra of enes and enones. Infrared (IR) absorption spectroscopy: Molecular vibrations. Hooke's law, selection rules, intensity and position of IR bands, measurement of IR spectrum, fingerprint region, characteristic absorptions of various functional groups and interpretation of IR spectra of simple organic compounds.

Unit 6: NMR Spectroscopy 10 hours

Proton magnetic resonance(!H NMR) spectrescopy. nuclear shieding and deshielding, chemical shift and molecular structure, spin-spin splitting and coupling constants, areas of signals. Interpretation of PMR spectra of simple organic molecules such as ethyl bromide, ethanol, acetaldehyde, acetaldehyde, 1,1,2-tribromoethane, ethylacetate, toluene and acetophenone. Problems pertaining to the structure elucidation of simple organic compounds using UV, IR and PMR spectroscopic techniques.

Organic Chemistry Practical 15 hours

A. Chromatography: 1. Separate and identify monosaccharides present in the given mixture

(glucose and fructose) by paper chromatography. Report the RF value. 2. Chromatographic separation of active ingredients of plant, flower and

juices by TLC. B. Systematic qualitative analysis of organic compounds containing two

functional groups:


a. Detection of elements (N, Cl, Br, I, S). b. Detection of the following functional groups (with systematic

reporting): Carbonyl, Carboxyl, Phenolic, amino, nitro, sulphonic, and amide group.

c. Determination of melting point / boiling point. d. Identification of compounds with the help of reference book e. Preparation of derivative and determination of melting point

Or Project relevant can be taken up.

SEMESTER VI CHM(H) 312 Advanced Chemistry 6 100 marks Unit 1: Spectrophotometry 10 hours

Derivation of Beer-Lambert Law, nomenclature and units (T, A, €, c, l associated calculations); general instrumentation for spectroscopy, spectrophotometric determination of one component (iron, chromium, manganese, nickel, titanium, and phosphorus) system, spectrophotometric determination of dissociation constants of an indicator, photometric errors and RINGBOM-AYERS plots.

Unit 2: Rotational Spectroscopy 10 hours

Introduction : electromagnetic radiation, regions of the spectrum, basic features of different spectrometers, statement of the Born-Oppenheimer approximation, degrees of freedom. Rotational Spectrum Diatomic molecules. Energy levels of a rigid rotor (semi-classical principles), selection rules, spectral intensity, distribution using population distribution (Maxwell-Bo!tzmann distribution), determination of bond length, qualitative description of non-rigid rotor, isotope effect

Unit 3: Vibrational Specroscopy 10 hours

Vibrational Spectrum (Infrared spectrum) : Energy levels of simple harmonic oscillator, selection rules, pure vibrational spectrum, intensity, determination of force constant and qualitative relation of force constant and bond energies, effect of anharmonic motion and isotope on the spectrum, idea of vibrational frequencies of different functional groups


Unit 4: 10 hours (a) Atomic Absorption Spectroscopy

Types, atomizer, absorption and emission spectroscopy, general idea of theory and application.

(b) Mass spectrometry: Principle, types of ions produced in mass spectrophotometer, molecular ion peak, base peak and metastable ion; determination of molecular weight of organic compounds.

Unit 5: 10 hours (a) Stereo isomeric separation and analysis

Measurement of optical rotation, calculation of enantiomeric excess (ee) / diastereomeric excess (de) ratios and determination of enantiomeric composition using nmr, chiral solvents and chiral shift reagents.

(c) Development of Chromatogram: Frontal, elution and development methods, qualitative and quantitative

methods of analysis: IC, GLC, GPC, TLC, and HPLC. Unit 6: 10 hours

(a) Electro analytical methods Classification of electro analytical methods, basic principle of pH metric, potentiometric and conductometric titration; techniques used for determination equivalent point, techniques used for determination of PKa values.

(b) Thermal method of analysis Theory of thermogravimetry (TG), basic principle of instrumentation, technique for quantitative estimation of Ca and Mg from their mixture.

(c) Radio analytical methods: Elementary theory, isotope dilution and neutron activation methods and application.


(a) Varification of Beer Lambart’s law using Coper sulphate solution or FeSO4.5H2O solution colorimetrically and determine the concentration of the solution.

(b) Determination of order of reaction, rate constant and energy of activation for saponification of an ester by NaOH, conductometrically

(c) Determination of strength of strong and weak acids in a mixture conductometrically.

(d) Determination of critical micellar concentration of sodium lauryl sulphate from the measurement of conductivities at different concentrations.

(e) Determination of strength of halides in a misture potentiometrically. (f) Determination of the strength of a given ferrous sulphate solution

potentiometrically.


Recommended Books 1. Prakash, Tuli, Madan, Basu, Advanced Inorganic Chemistry, S. Chand & Co. New Delhi, vol.

I and vol.II. 2. Malik, Tuli, Madan, Selected Topics in Inorganic Chemistry, S. Chand, New Delhi. 3. Puri, Sharma, Kalia, Principles of Inorganic Chemistry, Vishal, Jalandhar. 4. Agarwal, Modern Inorganic Chemistry, Kitab Mahal. 5. Gurdeep R, Advanced Inorganic Chemistry, Krishna Prakashan, Meerut, vol. I, vol. II. 6. Sharma, B. K. Analytical Chemistry, Krishna Prakash, Meerut. 7. Cotton, Wilkinson, Gaus, Basic Inorganic Chemistry, Wiley. 8. Lee, Concise Inorganic Chemistry, Chapmann & Hall 9. Sharpe, Inorganic Chemistry, Pearson. 10. Huheey, Keiter, Keiter, Inorganic Chemistry, Addision & Wesley 11. Shriver, Atkin, Inorganic Chemistry, Oxford University Press 12. Chatwal, Anand, Instrumental Methods of Chemical Analysis, Himalaya Publishing House. 13. Banwell, Fundamental of Molecular Spectroscopy, Tata McGraw Hills. 14. Budhiraja, Separation Chemistry, New Age International (P) Ltd. 15. Gutru, Kapoor, Advanced Experimental Chemistry, S. Chand & Co., vol.I, vol.II, vol.III. 16. Gurdeep, advanced preactical Inorganic Chemistry, Goel, Meerut. 17. Kamboj, University practical Chemistry, Vishal, Jalandhar. 18. Morrison, Boyd, Organic Chemistry, Prentice Hall, New Delhi. 19. Bruce, Organic Chemistry, Prentice Hall, New Delhi. 20. Bahl, Bahl, Organic Chemistry, S. Chand, New Delhi. 21. Moody, Whitham, Reactive Intermidiates, Oxford University Press. 22. Eliel, Stereochemistry of Carbon Compounds, Tata McGraw Hills, New Delhi. 23. Kalsi. Stereochemistry, New age international, New Delhi. 24. Kalsi. Organic Reactions and their mechanism, New age international, New Delhi. 25. Mukherji, Singh, Reaction Mechanism, McMillan india Ltd. 26. Mukherji, Singh, Kapoor, Organic Chemistry, New Age, vol.I, vol.II, vol.III 27. Banshal, Heterocyclic Chemistry, New Age, new Delhi. 28. Jain, S.-C. Sharma, Modern Organic Chemistry, Vishal, Jalandhar. 29. Balaji, Advanced Organic Chemistry, Vishal, Jalandhar. 30. Jagadamba, Yadab, Undergraduate Organic Chemistry, Pragati Prakashan, Meerut. 31. Jagadamba, Yadab, Advanced Organic Chemistry, Pragati Prakashan, Meerut. 32. Finar, I. L. Organic Chemistry, ELBS and Longman Ltd., New Delhi. vol.I, II. 33. Puri, Sharma, Pathania, Principles of Physical Chemistry, Vishal, Jalandhar. 34. Bajpai, Advanced Physical Chemistry, S. Chand, New Delhi. 35. Rastogi, Misra, An introduction to Chemical Thermodynamics, Vikash, New Delhi. 36. Atkins, Physical Chemistry, Oxford University Press. 37. Pahari, Physical Chemistry, New central Book Agency, Kolkotta, vol.I, vol.II. 38. Rakshit, Physical Chemistry, Sarat Book House, Kolkotta. 39. Pecsock, Shields, Cairns, McWilliam, Modern Methods of Chemical Analysis, John Wiley,

New York. 40. Khopkar, S. M. Basic Concepts of Analytical Chemistry, New Age International Publications,

New Delhi. 41. Willard, H. H. Merritt, L. L. Dean, J. A. Instrumental Methods of Analysis, CBS Publishers

& Distributors, Shahdara, Delhi. 42. Christian, G. D. Analytical Chemistry, John Wiley & Sons, New York. 43. Walton, H. F. Principles and Methods of Chemical Analysis, Prentice Hall, New Delhi. 44. Gurdeep, Chatwal, Anand, Instrumental method of chemical analysis, Himalaya Publishing

House. 45. Banwell & McCash, Fundamentals of molecular spectroscopy, Tata McGraw Hills company

ltd., New Delhi. 46. William Kemp, Organic spectroscopy, ELBS. 47. Sharma, B.K. Spectroscopy, Krishna Prakashan.

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