National Post Graduate (Autonomous) College, Lucknow Chemistry Department

Theory and Practical papers in each semester
B.Sc. Semester-1
Paper-I -  CH-101: Inorganic Chemistry
Paper-II-  CH-102: Physical Chemistry
B.Sc. Semester- II
Paper -I - CH-201: Organic Chemistry
Paper - II-CH-202: Practical
B.Sc. Semester- III
Paper-I  -CH-301: Organic Chemistry 
Paper - II - CH-302: Practical
B.Sc. Semester- IV
Paper -I - CH-401: Inorganic Chemistry
Paper - II - CH-402: Physical Chemistry
B.Sc. Semester- V
Paper -1 - CH-501: Inorganic Chemistry
Paper - II - CH-502: Physical Chemistry
Paper-III  -CH-503: Practical
B.Sc. Semester- VI
Paper-I  -CH-601: Organic Chemistry
Paper-II  -CH-602: General Chemistry
Paper-III  -CH-603: Practical

CHEMISTRY

CH-101
Inorganic Chemistry
Atomic Structure: Quantum mechanics based structure of atom in brief, shapes of s, p and d orbitals, aufbau and Pauli exclusion principles, Hund's Multiplicity rules. Electronic configurations of the elements, effective nuclear charge,
Periodic Properties and Classification based upon electronic configuration:   Diagonal relationship, inert pair effect, atomic   and   ionic   radii, van der waal radii,  ionization   energy,   electron   affinity   and electronegativity : definition, method of determination, trends in periodic table and applications in predicting and explaining chemical behaviour.

Unit II
Chemical Bonding
(a) Covalent bond: valence bond theory and its limitations, directional characteristic of covalent bond. Hybridization and shapes of simple molecules and ions. Valence Shell Electron Pair Repulsion (VSEPR) theory to simple molecules and ions. Molecular Orbital theory for homonuclear and heteronuclear (CO and NO) diatomic molecules, multi-center bonding in electron deficient molecules, bond strength and the bond energy, % ionic character from dipole moment and electro negativity difference.
(b) Weak interactions: hydrogen bonding, van der Waals forces.
Unit III
(a) Ionic solid: ionic structures, radius ratio effect and coordination number, limitation of ratio rule, Lattice defects, Lattice energy and Born-Haber cycle, solvation energy and solubility of ionic solids, polarizing power and polarizability of ions. Fajan's rule, Metallic bond free electron, Valence bond and Band theories.
(b)        s-Block elements: Comparative study,  salient features of hydrides, salvation and complexation tendencies of cations of alkali and alkaline earth matter including their function in biosystems, an introduction to alkyls and aryls of Li & Mg.
(c)        Noble Gases: Chemical properties of the noble gases, discovery of O2+PtF6- and O2XeF6 chemistry of xenon, structure and bonding in xenon compounds.
UNIT IV
p-Block Elements:- Comparative study (including diagonal relationship) physical and chemical behaviour of group 13-17 elements, compounds like hydrides, oxides, oxyacids and halides of group 13-16, diborane, boronitride a, b forms, Fullerenes, silicates (structural principle) and structures of oxides and oxyacids of phosphorus and sulphur, interhalogens and polyhalides.
Text Books (Theory Courses):
1.         Concise Inorganic Chemistry, J.D. Lee.
2.         Inorganic Chemistry, Puri & Sharma.
3.         Pradeep's Inorganic Chemistry, K.K.Bhasin, Pradeep Publication.
Reference Books:
1. Inorganic Chemistry, J.E.Huheey, Ellen A. Keiter, Richard L. Keiter, Addison Wesley Longma (Singapore) Pte. Ltd.
2. Inorganic Chemistry, D.E.Shriver, P W. Atkins and C.HL Langford, Oxford.
3. Basic Inorganic Chemistry, F.A. Cotton, G. Wilkinson and P.L. Gaus, Wiley.
4.  Concepts of Models of Inorganic Chemistry, B.Douglas, D.McDaniel and J Alexander, John Wiley.
5. Inorganic Chemistry, WW. Porterfteld, Addison - Wesley.
6. Inorganic Chemistry, A.G. Sharpe, ELBS
7. Inorganic Chemistry, G.L. Meissler and D.A. Tarr, Prentic-Hali.

CHEMISTRY

CH-102
Physical Chemistry
UNIT-I
Mathematical Concepts :- Logarithmic relations, curves stretching, linear graphs and calculation of slopes, Differentiation of functions like x, ex, xn, sinx, logx; maxima and minima, partial differentiation and reciprocity relations. Integration of some useful/relevant functions; permutations and combinations. Factorials, Probability.
Computers: General introduction to computers, different components of a computer. Hardware and software, input-output devices, binary numbers and arithmetic; introduction to computer languages. Programming and operating systems.
UNIT-II
Gaseous State: Postulates of kinetic theory of gases, deviation from ideal behavior, van der Waals equation of State.
Critical phenomenon: PV isotherms of real gases, continuity of states, the isotherms of van der Waals equations, relationship between critical constants and van der Waals constants, the law of corresponding states, reduced equation of states.
Molecular Velocities: Root mean square, average and most probable velocities. Qualitative discussion of the Maxwell's distribution of molecular velocities, collision numbers, mean free path and collision diameter. Liquification of gases (based on Joule Thomson effect).
Liquid State:-Intermolecular forces, structure of liquids (a qualitative description) Structural differences between solids, liquids and gases.
Liquid crystals: Difference between liquid crystal, solid and liquid. Classification, structure of nematic and cholestic phases. Thermography and seven segment cell.
Unit-III
Solid State: Definition of space lattice, Unit cell.
Laws of crystallography, (i) Law of constancy of interfacialangles (ii) Law of rationality of indices (iii) Law of symmetry. Symmetry elements in crystals.
Diffraction X-ray diffraction by crystals. Derivation of Bragg's equation. Determination of crystal structure of NaCl, KC1 and CsCI (Laue’s method and powder method) and simple structure of ZnS,CaC2,diamond graphite.
Colloidal State: Definition of colloids, 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.
Unit-IV
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, first order, second 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.
Experimental methods of chemical kinetics-conductometric, potentiometic, optical methods, polarimetry and spectrophotometery.
Theories of chemical kinetics: effect of temperature on rate of reaction, Arrhenius equation, concept of activation energy. Simple collision theory based on hard sphere model, transition state theory (equilibrium hypothesis) Expression for the rate constant based on equilibrium constant and thermodynamic aspects.
Catalysis: Catalysis, characteristics of catalysed reactions, classification of catalysis, Miscellaneous examples.
Text Books (Theory Courses):
1.   Physical Chemistry,.Puri Sharma & Pathania.
2.   Pradeep Physical Chemistry, Khetrapal, Pradeep Publication.
3.  Computers and Common Sense, R. Hunt and Shelly, Prentice Hall.
Reference Books:
1. Physical Chemistry. G.M. Barrow. International Student Edition, McGrawHill
2. Physical Chemistry, R.A. Alberty, Wiley Eastern Ltd.
3. The Elements of Physical Chemistry, P.W. Atkins, Oxford.
4. Physical Chemistry Through problems, S.K. Dogra and S. Dogra, Wiley Eastern Ltd.
5. Basic Programming with Application, V.K. Jain, Tata McGraw Hill.
6. Physical Chemistry, Glaston                                                                                                                 

CHEMISTRY

CH-201
Organic Chemistry
Unit – I
Structure and bonding: Hybridization, bond lengths, bond angles, bond energy, localised and delocalized π bonds, resonance, inductive and field effects, hydrogen bonding, inclusion compounds, clathrates, charge transfer complexes.
Types of reagents: Electrophiles and nucleophiles. Reactive intermediates – carbocations, carbanions, free radicals, carbenes, arynes. Assigning formal changes on intermediates and other ionic species.
Mechanism of organic reactions: Types of organic reactions,  methods of determination of reaction mechanism. Energy considerations. Curved arrow rotation, drawing electro movement with arrows, homolytic and heterolytic bond breaking.
Unit – II
Optical isomerism : Elements of symmetry, molecular chirality, optical activity, stereogenic centres, enantiomers, chiral and achiral molecules with two stereogenic centres, diastereomers, meso compounds, resolution of enantiomers, racemization. Relative and absolute configurations. Sequence rules. D, L and R, S nomenelature.
Geometrical isomerism : E, Z system, geometrical isomerism in oximes and alicyclic compounds.
Saw-horse and flying wedge formulae, Fischer and Newman projections.
Cycloalkanes : Nomenclature, methods of preparation. Baeyer's strain theory. Ring strain in cyclopropane and cyclobutane. Conformational analysis of ethane, n-butane and cyclohexane.
Unit – III
Alkanes: Nomenclature, methods of formation with special reference to Wurtz, Kolbe, Corey-House reactions and decarboxylation. Physical properties and chemical reactions. Mechanism of free radical halogenation of alkanes.
Alkenes: Nomenclature, methods of formation. Mechanisms of dehydration of alcohols and dehydrohalogenation of alkyl halides. Ragio-selectivity in alcohol-dehydration. Saytzeff's rule, Hofmann elimination.
Physical properties and relative stabilities of alkenes. Chemical reactions. Mechanisms involved in hydrogenation, electrophilic and free-radical additions. Markownikoff's rule. Hydroboration-oxidation, oxymercuration-reduction, epoxidation, ozonolysis, hydrations, hydroxylation and oxidation, polymerization. Substitutions at allylic and vinylic positions of alkenes. Industrial applications of ethylene and propene.
Alkynes: Nomenclature, structure and bonding in alkynes. Methods of formation, chemical reactions and acidity of alkynes. Mechanism of electrophilic and mucleophilic addition reactions, hydroboration-oxidation and polymerization.
Unit – IV
Halogen compounds : Alkyl halides – Nomenclature, methods of formationi, chemical reactions. Mechanism of nucleophilic substitution reactions (,) with energy profile diagrams, chloroform and carbon tetrachloride. Aryl halides – Methods of formation, nuclear and side chain reactions. Mechanisms of nucleophilic aromatic substitutions. Relative reactivities of alkyl halides versus allyl, vinyl and aryl halides. Synthesis and uses of DDT, BHC and Freon.
Arenes and aromaticity : Nomenclature of benzene derivatives. Activating and deactivating substituents. Orientation and ortho/para ratio. Structure of benzene and its stability, carbon-carbon bond lengths, resonance structure, MO picture of benzene. Aromaticity-Huckel’s rule and aromatic ions. Mechanism of Aromatic electrophilic substitutions, such as nitration, halogenation, sulphonation, mercuration and Frieded-Crafts reaction. Energy profile diagrams. Birch reduction. Methods of formation and chemical reactions of alkylbenzenes, alkynylbenzenes and biphenyl.
Text Books (Theory Courses) :
1.         Organic Chemistry, Vol. I, I.L. Finar, Pearson Education.
2.         Organic Chemistry, M.K. Jain, Shoban Lal & Co.
3.         Pradeep's Organic Chemistry, S.N. Dhawan, Pradeep Publication.
Reference Books :
1.         Organic Chemistry, Morrison and Boyd, Prentice Hall.
2.         Organic Chemistry, L.G. Wade Jr. Prentice Hall.
3.         Fundamentals of Organic Chemistry Solomons, John Wilev.
4.         Organic Chemistry, Vol. I, II, III S.M. Mukherji, S.P. Singh and R.P. Kapoor, Wiley Eastern Ltd. (New Age International)
5.         Organic Chemistry, F.A. Carey, McGraw-Hill Inc.
6.         Introduction to Organic Chemistry, Streitwiesser, Hathcock and Kosover, Macmillan.  

CHEMISTRY

CH-202
Chemistry Practical
Inorganic Chemistry
Calibration of fractional weights, pipettes and burettes, Preparation of standard solutions. Dilution- 0.1 M to 0.001 M solutions.
Quantitative Analysis
Volumetric Analysis
(a)        Determination of acetic acid in commercial vinegar using NaOH
(b)        Determination of alkali content - antacid tablet using HCl.
(c)        Estimation of calcium content in chalk as calcium oxalate by permanganometry
(d)        Estimation of hardness of water by EDTA
(e)        Estimation of ferrous ions by dichromate method
(f)        Estimation of copper using thiosulphate.
Gravimetric Analysis
(a)        Ba as BaSO4 in the given solution of BaCl2
(b)        Analysis of Cu as CuSCN and Ni as Ni dimethylgloxime
Physical
1.         Preparation of solutions of various concentrations, NaOH, HCl, H2SO4.
2.         To determine the velocity constant (specific-reaction rate) of hydrolysis of methylacetate/ethyl acetate catalyzed by hydrogen ions at room temperature.
3.         To study the effect of acid strength on the hydrolysis of an ester.
4.         To compare the strength of HCl and H2SO4 by studying the kinetics of hydrolysis of an ester.
5.         To study kinetically the reaction rate of decomposition of iodide by H2O2.
6.         Determination of surface tension/percentage composition of given binary organic mixture using surface tension method.
7.         Determination of viscosity/percentage composition of given organic mixture    using viscosity method.
Organic
1.         Distillation
2.         Crystallization
3.         Detection of extra elements (N, S and halogens) 2 elements,   functional groups (phenolic, carboxylic, carbonyl, esters, carbohydrates, amines, amides, nitro and anilide) in simple organic
Record and Viva

CHEMISTRY

CH-301
Organic Chemistry

Electromagnetic Spectrum Absorption Spectra - Ultraviolet (UV) absorption spectroscopy -  absorption laws (Beer-Lambert law); molar absorptivity, presentation and analysis of UV spectra, types of electronic transitions, effect of conjugation. Concept of chromophore and auxochrome, Bathochromic, hypsochromic, hyperchromic and hypochromic shifts. U.V.spectra of conjugated enes and enones.
Infrared (I.R.) absorption spectroscopy- Molecular vibrations, Hook's law, Selection  rules, intensity and position of I.R. bands,  measurement of I.R. spectrum, fingerprint region, characteristic absorptions of various functional groups and interpretation of I.R. spectra of simple organic compounds.
Unit II
Alcohols: Monohydric alcohols - Classification, nomenclature, methods of formation by reduction of aldehydes, Ketones, Carboxylic acids and Esters, Hydrogen bonding, Acidic nature, Reactions of alcohols.
Dihydric alcohols - Nomenclature, methods of formation, chemical reactions of vicinal glycols, oxidative cleavage [Pb(OAc)4 and HIO4] and pinacole-pinacolone rearrangement.
Trihydric alcohols - Nomenclature and methods of formation, chemical reactions of glycerol.
Phenols:-Nomenclature, structure and bonding, Preparation of phenols, physical properties and acidic character. Comparative acidic strengths of alcohols and phenols, resonance stabilization of phenoxide ion. Reactions of phenols -electrophilic aromatic substitution, acylation and carboxylation. Mechanisms of Fries rearrangement, Claisen rearrangement, Gatterman synthesis, Hauben-Hoesch reaction, Lederer-Manasse reaction and Reimer-Tiemann reaction.
Unit III
Ethers and Epoxides: Nomenclature of ethers and methods of their formation, physical properties. Chemical reactions - cleavage and autoxidation, Ziesel's method. Synthesis of epoxides, Acid and base-catalyzed ring opening of epoxides, orientation of epoxide ring opening, reactions of Grignard and organolithium reagents with epoxides.
Aldehydes and Ketones: Nomenclature and structure of the carbonyl groups, synthesis of aldehydes and ketones with particular reference to the synthesis of aldehydes from acid chlorides, synthesis of alkedydes and ketones using 1,3-dithianes, synthesis of ketones from nitrites and from carboxylic acids. Physical properties. Mechanism of nucleophillic additions to carbonyl group with particular emphasis on benzoin, aldol, Perkin and Knoevenagel condensations, Condensation with ammonia and its derivatives. Wittig reaction, Mannich reaction. Use of acetals as protecting group, Oxidation of aldehydes, Baeyer-Viliiger oxidation of Ketones, Cannizzaro reaction, MPV, Clemmensen, Wolff-Kishner, LiAlH4 and NaBH4 reductions. Halogenation of enolizable ketones. An introduction to a,b-unsaturated aldehydes and ketones.
Unit IV
Carboxylic Acids: Nomenclature, structure and bonding, physical properties, acidity of carboxylic acids, effects of substituents on acid strength. Preparation of carboxylic acids, Reactions of carboxylic acids, Hell-Volhard-Zelinsky reaction, Synthesis of acid chlorides, esters and amides. Reduction of carboxylic acids, Mechanism of decarboxylation. Methods of formation and chemical reactions of halo acids,
Hydroxy acids: Malic, tartaric and citric acids. Methods of formation and chemical reactions of unsaturated monocarboxylic acids. Dicarboxylic acids: Methods of formation and effect of heat and dehydrating agents.
Carboxylic Acid Derivatives: Structure and nomenclature of acid chlorides, esters, amides (urea) and acid anhydrides. Relative stability of acyl derivatives.
Physical properties, interconversion of acid derivatives by nucleophilic acyl substitution. Preparation of carboxylic acid derivatives, chemical reactions. Mechanisms of esterification and hydrolysis (acidic and basic).
Organic Compounds of Nitrogen: Preparation of nitroalkanes and nitroarenes. Chemical reactions of nitroalkanes. Mechanisms of nucleophilic substitution in nitroarenes and their reductions in acidic, neutral and alkaline media. Picric acid.
Amines and Diazonium salts: Reactivity, structure and nomenclature of amines, physical properties. Stereochemistry of amines. Separation of a mixture of primary, secondary and tertiary amines. Structural features effecting basicity of amines. Amine salts as phase-transfer catalysts. Preparation of alkyl and aryl amines (reduction of nitro compounds, nitriles), reductive amination of aldehydic and ketonic compounds. Gabriel -phthalimide reaction, Hofmann bromamide reaction. Reactions of amines, electrophilic aromatic substitution in aryl amines, reactions of amines with nitrous acid. Synthetic transformations of aryl diazonium salts, azo coupling.

Books Suggested (Theory Courses)
1.         Organic Chemistry, Morrison and Boyd, Prentice Hall.
2.         Organic Chemistry, L.G. Wade Jr. Prentice Hall
3.         Fundamentals of Organic Chemistry Solomons, John Wilev.
4.         Organic Chemistry, Vol. I, II, III, S.M. Mukherji, S.P. Singh and R.P. Kapoor, Wiley Eastern Ltd. (New Age International).
5.         Organic Chemistry, F.A. Carey, McGraw-Hill Inc.
6.         Introduction to Organic Chemistry, Streitwiesser, Hathcock and Kosover, Macmillan.
7.         Organic Chemistry, Vol. I, II, I.L. Finar
8.         Spectrometric Identification of organic compounds. Robert M. Silverstein, Clayton G. Bassler, Terence C. Morril, John Wiley.

CHEMISTRY

CH-302
Chemistry Practical

Inorganic
1.         Identification cations and anions in a mixture inorganic compounds soluble in water/dilute acids (Macro/semi-micro analysis- cation analysis, separation of ions from group I-VI, anion analysis).
2.         Separation of cations by paper chromatography
Organic Chemistry
Laboratory Techniques
A.  Thin Layer Chromatography
Determination of Rf value and Identification of organic compounds.
(a)        Separation of green leaf pigments (spinach leaves may be used)
(b)        Preparation and separation of 2,4-dinitrophenylhydrazones of acetone, 2-butanone hexan-2- and 3-one using toluene and light petroleum (40:60).
(c)        Sepearation of a mixture of dyes using cyclohexane and ethyl acetate (8.5:1.5).
B.         Paper Chromatography: Ascending and Circular
Determination of Rf values and identification of organic compounds,
(a)        Separation of a mixture of phenylalanine and glycine. Alanine and aspartic acid. Leucine and glutamic acid. Spray reagent – ninhydrin.
(b)        Separation of a mixture of D,L-alanine, glycine, and L-Leucine using n-butanol: acetic acid: water (4:1:5). Spray reagent – ninhydrin.
(c)        Separation of monosaccharides - a mixture of D-galactose and D - fructose using n-butanol:acetone:water (4:5:1). Spray reagent - aniline hydrogen phthalate.
Qualitative Analysis
Identification of an organic compound through the functional group analysis, determination of melting point and preparation of suitable derivatives.
Physical Chemistry
Transition Temperature
1.         Determination of    the    transition    temperature    of   the   given    substance by thermometric/dialometric method (e.g. MnCl2.4H2O/SrBr2.H2O).
Phase Equilibrium
1.         To study the affect of a solute (e.g. NaCl, succinic acid) on the critical solution temperature of two partially miscible liquids (e.g. phenol-water system) and to determine the concentration of that solution in the given phenol-water system.
2.         To construct the phase diagram of two component (e.g. diphenylamine -benzophenone) system by cooling curve method.
Thermochemistry
1.         To determine the solubility of benzoic acid at different temperatures and to determine the dissolution process.
2.         To determine the enthalpy of neutralisation of a weak acid/weak base versus strong base/strong acid and determine the enthalpy of ionisation of the weak acid/weak base.
3.         To determine the enthalpy of solution of solid calcium chloride and calculate the lattice energy of calcium chloride from its enthalpy data using Born Haber cycle.
Record and Viva.

CHEMISTRY

CH-401
Inorganic Chemistry

Unit - I
Chemistry of Elements of First Transition Series: Characteristic properties of d-block elements. Binary compounds (hydrides, carbides and oxides) of the elements of the first transition series and complexes with respect to relative stability of their oxidation states, coordination number and geometry.
Chemistry of Elements of Second and Third Transition series: General characteristics, comparative treatment of Zr/Hf, Nb/Ta , Mo/W in respect of ionic radii, oxidation states, magnetic behavior, spectral properties and stereochemistry.
Unit - II
Coordination Compounds: Werner's coordination theory and its experimental verification, effective atomic number concept, chelates, nomenclature of coordination compounds, isomerism in coordination compounds, valence bond theory of transition metal complexes.
Unit-III
Chemistry of Lanthanide Elements: Electronic structure, oxidation states and ionic radii and lanthanide contraction,  complex formation, occurrence and isolation, cerie ammonium sulphate and its analytical uses.
Chemistry  of  Actinides:   Electronic  conformation,   oxidation   states  and magnetic properties, chemistry of separation of Np, Pu and Am from U.
Unit IV
Oxidation and Reduction: Electrode potential, electrochemical series and its applications. Principles involved in the extraction of the elements.
Acids and Bases : Arrhenius, Bronsted-Lowry, the Lux-Flood, solvent system and Lewis concept of acids and bases.
Non-aqueous Solvents: Physical properties of a solvent, types of solvents and their general characteristics, Reactions in non-aqueous solvents with reference to liquid NH3 and liquid SO2.
Books Suggested (Theory Courses)
1.         Basic Inorganic Chemistry, FA Cotton9 G. Wilkinson and P.L. Gaus, Wiley.
2.         Concise Inorganic Chemistry, J.D. Lee, ELBS*
3.         Concepts of Models of Inorganic Chemistry, B.Douglas, D.McDaniel and J Alexander, John Wiley.
4.         Inorganic Chemistry, D.E.Shriver, P.W. Atkins and C.HL Langford, Oxford.
5.         Inorganic Chemistry, WW. Porterfield, Addison - Wesley,
6.         Inorganic Chemistry, A.G. Sharpe, ELBS
7.         Inorganic Chemistry, G.L. Meissier and D.A. Tarr, Prentice-Hall

CHEMISTRY

CH-402
Physical Chemistry

Unit - I
Thermodynamics-1
Definition of thermodynamic terms: System, surroundings etc. Types of systems, intensive and extensive properties. State and path functions and their differentials. Thermodynamic process. Concept of heat and work.
First Law of Thermodynamics: Statement, definition of internal energy and enthalpy. Heat capacity, heat capacities at constant volume and pressure and their relationship.  Joule's  law - Joule-Thomson  coefficient  and  inversion temperature. Calculation of w,q, dU & dH for the expansion of ideal gases under isothermal and adiabatic conditions for reversible process.
Thermo chemistry: Standard state, standard enthalpy of formation - Hess's Law of heat summation and its applications. Heat of reaction at constant pressure and at constant volume. Enthalpy of neutralization. Bond dissociation energy and its calculation from thermo-chemical data, temperature dependence of enthalpy. Kirchhoff s equation.
Unit II
Thermodynamics - II
Second law of thermodynamics: Need for the law, different statements of the law. Carnot's cycle and its efficiency, Carnot's theorem. Thermodynamic scale of temperature. Clapeyron-Clausius equation and its applications
Concept of entropy: Entropy as a state function, entropy as a function of V & T, entropy as a function of P & T, entropy change in physical change, Clausius inequality, entropy as a criteria of spontaneity and equilibrium change in ideal gases and mixing of gases.
Gibbs and Helmholtz functions: Gibbs function (G) and Helmholtz function (A) as thermodynamic quantities, A & G as criteria for thermodynamic equilibrium and spontaneity, their advantage over entropy change. Variation of G and A with P, V and T.
Third law of thermodynamics: Nernst heat theorem, statement and concept of residual entropy. Nernst distribution law - thermodynamic derivation, applications.
Unit III
Electrochemistry -1:
Electrical transport - Conduction in metals and in electrolyte solutions, specific conductance   and   equivalent   conductance,    measurement   of   equivalent conductance, variation of equivalent and specific conductance with dilution. Migration   of  ions  and   Kohlrausch's  law,  Arrhenius  theory  of electrolyte dissociation and its limitations, weak and strong electrolytes , Ostwald's dilution law its  uses  and  limitations.  Debye-Huckel-Onsager's equation for strong electrolytes  (elementary treatment only).  Transport  number,  definition  and determination by Hittorfs method and moving boundary method.
Applications of conductivity measurements: Determination of degree of   dissociation, determination of Ka of acids, determination of solubility product of a sparingly soluble salt, conductometric titrations.
Unit IV
Electrochemistry - II:
Types of reversible electrodes- Gas-metal ion, metal-ion, metal-insoluble salt-anion and redox electrodes. Electrode reactions, Nernst equation, derivation of cell E.M.F. and single electrode potential, standard hydrogen electrode reference electrodes- standard electrode potential, sign conventions, electrochemical series and its significance.
Electrolytic and Galvanic cells- Reversible and irreversible cells, conventional representation of electrochemical cells.
EMF of a cell and its measurements- Computation of cell EMF. Calculation of thermodynamic quantities of cell reactions (DG, DH and K)
Concentration cell with and without transport, liquid junction potential, application of concentration cells, valency of ions, solubility product and activity coefficient, potentiometric titrations.
Definition of pH and pKa, determination of pH using hydrogen, quinhydrone and glass electrodes, by potentiometric methods.
Buffers - Mechanism of buffer action, Henderson-Hazel equation. Hydrolysis of salts.

Books Suggested (Theory Courses)
1.         Physical Chemistry. G.M. Barrow. International Student Edition, McGraw Hill.
2.         Physical Chemistry, R.A. Alberty, Wiley Eastern Ltd.
3.         The Elements of Physical Chemistry, P.W. Atkins, Oxford.
4.         Physical Chemistry Through problems, S.K. Dogra and S. Dogra, Wiley Eastern Ltd.

CHEMISTRY

CH-501
Inorganic Chemistry

Unit - I
Metal-ligand bonding in Transition Metal Complexes: Limitation of valence bond theory, an elementary idea of crystal field theory, crystal field splitting in octahedral, tetrahedral and square planar complexes, factors effecting the crystal field parameters. Effect of CFSE on lattice energy, Ionic radii.
Unit – II
Thermodynamic and Kinetic Aspects of Metal Complexes: A brief outline of thermodynamic stability of metal complexes and factors affecting the stability. Substitution reaction of square planar complexes. Trans effect.
Magnetic Properties of Transition Metal Complexes : Types of magnetic behaviour, methods of determining magnetic susceptibility, spin only formula, L-S coupling, spectroscopic ground state. Correlation of MS and Meff values. Orbital contribution to magnetic moments. Application of magnetic moment data for 3d metal complexes.
Unit – III
Organometallic Chemistry : Definition, types of organometallic compound and their general methods of preparation. alkyls and aryls of Li, Hg, Mg. Metal carbonyls. 18 electron rule, preparation, structure and nature of bonding in the mononuclear carbonyls.
Unit – IV
Hard and Soft Acids and bases (HSAB) : Classification of acids and bases as hard and soft. Pearson's HSAB concept, acid base strength and hardness and softness. Symbiosis, theortical basis of hardness and softness.
Bioinorganic Chemistry : Introduction, metalloenzyme / carboxypeptidase, carboxy-anhydrase. Metalloporphyrens with special reference to haemoglobin and myoglobin (structure, cooperative effect, Bohr's effect).
Books Suggested (Theory Courses)
1.         Basic Inorganic Chemistry, F.A. Cotton G. Wilkinson and P.L. Gaus, Wiley.
2.         Concise Inorganic Chemistry, J.D. Lee, ELBS
3.         Concepts of Models of Inorganic Chemistry, B.Douglas, D.McDaniel and J Alexander, John Wiley.
4.         Inorganic Chemistry, D.E. Shriver, P&W Atkins and C.HL Langford, Oxford.
5.         Inorganic Chemistry, WW, Porterfield, Addison – Wesley.
6.         Inorganic Chemistry, A.G. Sharpe, ELBS
7.         Inorganic Chemistry, G.L. Meissler and D.A. Tarr, Prentic-Hall

CHEMISTRY

CH-502
Physical Chemistry

Unit - I
Introductory Quantum Mechanics, Physical properties and Molecular Structure:
Introductory Quantum Mechanics : Black-body radiation, Plank's radiation law, photoelectric effect, heat capacity of solids, Bohr's model of Hydrogen atom (no derivation) and its defects, compton effect.
Physical Properties and Molecular Structure : Optical activity, polarization (clausius-Mossotti equation), orientation of dipoles in an electric field, dipole moment, induced dipole moment, measurement of dipole moment, temperature method and refractivity method, dipole moment and structures of molecules, magnetic properties – paramagnetism, diamagnetism and ferromagnetism.
Unit – II
Elementary Quantum Mechanics : de Broglie's hypothesis, the Heisenberg's uncertainty principle, Hamiltonian operator. Statement of Born-oppenheimer approximation, degree of freedom. Schrodinger wave equation and its importance. Physical interpretation of wave function, postulates of quantum mechanics, particle in one dimensional box. Schrodinger wave equation for H atom. Separations into three equation (without derivation), quantum numbers and their importance like wave function, radial wave functions, angular wave functions.
Unit – III
Molecular orbital theory, basic ideas – criteria for forming M.Os.’ from A.Os.’ construction of M.O's by LCAO – H2+ ion, calculation of energy levels from wave functions, physical picture of bonding and antiboding wave functions, concept of   orbitals and their characteristics Hybrid Orbitals – sp, sp2, sp3 , calculation of coefficients of A.O's used in sp and sp2 hybrid orbitals. Introduction to valence bond model of H2, comparison of M.O. and V.B. models.
Unit – IV
Solutions, Dilute Solutions and Colligative Properties : Ideal and non-ideal solutions, methods of expressing concentration of solutions, activity and activity coefficient, Dilute solution, colligative properties, Raoult's law, relative lowering of vapour pressure, molecular weight determination, Osmosis, law of osmotic pressure and its measurement, determination of molecular weight from osmotic pressure, Elevation of boiling point and depression of freezing point. Thermodynamic derivation of relation between molecular weight and elevation in boiling point and depression in freezing point. Experimental methods of determining various colligative properties. Abnormal molar mass, degre of dissociation and association of solutes.
Books suggested (Theory Courses)
1.        Physical Chemistry, G.M. Barrow, International Student Edition, McGraw Hill.
2.        Physical Chemistry, R.A. Alberty, Wiley Eastern Ltd.
3.        The Elements of Physical Chemistry, P.W. Atkins, Oxford.
4.        Physical Chemistry Through Problems, S.K. Dogra and S. Dogra Wiley Eastern Ltd.
                                                                           

CHEMISTRY

CH-503
Chemistry Practical

Unit - I
INORGANIC CHEMISTRY
Synthesis and Analysis
(a)        Preparation of sodium trioxalato feerrate (III), Na3[Fe(C2O4)3] and determination of its composition by permagnometry.
(b)        Preparation of Ni-DMG complex, [Ni(DMG)2]
(c)        Preparation of copper telraammine complex, [Cu(NH3)4]SO4
(d)        Preparation of cis-and trans-bisoxalato diaqua chromate (III) ion.
Instrumentation
Colorimetry
(a)        To verify Beer-Lambert law for KMnO4/K2Cr2O7 and determine the concentration of the given solution.
(b)        Determination of Fe3+ content by thiocynate method.
Solvent Extraction
            Separation and estimation of Mg(II) and Fe(II)
Ion Exchange Method
            Separation and estimation of Mg(II) and Zn(II). 

CHEMISTRY

CH-601
Organic Chemistry

Unit - I
Spectrosocpy : Nuclear magnetic resonance (NMR): Spectroscopy, proton magnetic resonance (1H NMR) spectroscopy, nuclear shielding and deshielding. Chemical shifts and molecular structure, spin-spin splitting and coupling constants, arears of signals, inerpretation of 'H NMR spectra of simple organic molecules such as ethyl bromide, ethanol, accetaldehyde, 1, 1, 2 bibronoethane, ethyl acetate, toluens and acetophenons. Problems pertaining to the structure elucidation of simple organic compounds using UV, IR and 1H NMR spectroscopy techniques.
Unit – II
Heterocyclic compounds
Introduction : Molecular orbital picture and aromatic characteristic of pyrrole, furan, thiophene and pyridine, methods of synthesis and chemical reactions with particular emphasis on the mechanism of electrophillic substitution, mechanism of nucleophilic substitution reaction in pyridine derivatives. Comparison of basicity of pyridine, piperidine and pyrrole. Introduction to condensed five and six membered heterocycles. Preparation and reactions of indols, quinoline and isoquinoline with special reference to Fisher Indols synthesis, Skraup synthesis and Bischler – Nepieralski synthesis. Mechanism of electrophilic substitution reaction of indole, quinoline and isoquinoline.
Organometallic Compounds : Organomagnesium compounds : the Grigard reagents, formation, structure and chemical reactions. Organozinc compounds; formation and chemical reactions. Organolithium compound formation and chemical reactions.

                                                                Unit – III
Carbohydrates: Classification and nomenclature, monosaccharides, mechanism of osazone formation, interconversion of glucose and fructose, chain lengthening and chain shortening of aldoses. Configuration of monosaccharides. Erythro and threo diastereomers, conversion of glucose into mannose. Formation of glycoside Ethers and esters. Determination of ring size of monosaccharides. Cyclic structure of D(+)  glucose. Mechanism of mutarotation structure of ribose and deoxyribose. An introduction to diasacel harides (maltose, sucrose, lactose) and polysaccharide/starch and cellulose) without involving structure determination.
Unit – IV
Amino Acids, peptides, proteins and Nucleic Acids : Classification, structure and sterochemistry of amino acids. Acid-base behaviour, isoelectric point and electrophoresis, Preparation and reaction of a amino acids, structure and nomenclature of peptides and proteins. Classification of proteins, peptides structure determination, and group analysis. Selective hydrolysis of peptides. Classical peptide synthesis, solid phase peptide synthesis. Structure of peptides and proteins level of protein structures. Protein denaturation/venaturation.
Nucleic Acids: Introduction – Classification of nucleic acids Riborueleosides and ribonucleotides. The double helical structure of DNA.
Books Suggested (Theory Courses)
1.         Organic Chemistry, Morrison and Boyd, Prentice Hall.
2.         Organic Chemistry, L.G. Wade Jr. Prentice Hall.
3.         Fundamentals of Organic Chemistry Solomons, John Wiley.
4.         Organic Chemistry, Vol. I, II, III, S.M.Mukherji, S.P. Singh and R.P. Kapoor, Wiley Eastern Ltd. (New Age International)
5.         Organic Chemistry, F.A. Carey,McGraw-Hill Inc.
6.         Introduction to Organic Chemistry, Streitwiesser, Hathcock and Kosover.

CHEMISTRY

CH-602
General Chemistry

Unit - I
Spectroscopy :
Rotational Spectroscopy of Diatomic Molecules: Energy level of a rigid rotor (semi classical principles) selection rules, spectral intensity, distribution using population distribution (Maxwell – Boltzman distribution) determination of bond length, qualitative description of non rigid rotor, isotope effect.
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 an harmonic motion and isotope on the spectrum, idea of vibrational frequencies of different functional groups.
Raman Spectrum : Concept of polarizability, pure rotational and pure vibrational Raman spectra of diatomic molecules, selection rules.
Electronic spectroscopy : Types of electronic transition, selection rule, application to transition metal complexes – spectrochemical series, orgel energy level diagram for d1 and d9 states, discussion of electronic spectrum of [Ti(H2O)6]3+ complexion.
Unit – II
Fats, Oils and Detergents : Natural fats, edible and industrial oils of vegetable origin, common fatty acids, glycerides, hydrogenation of unsaturated oils, soaponification value, iodine value, acid value, soaps, synthetic detergents alkyl and aryl sulphonates.
Synthetic Polymers : 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, urea formaldehyde resin, epoxy resins and polyurithanes. Natural and synthetic rubbers.
Unit – III
Synthetic Dyes: Colour and constitution / electronic concept classification of dyes. Chemistry and synthesis of Methyl orange, conge red, Malachite green, crystal violet, phenophthalein, Fluorescin, Alizarin and Indigo.
Organic Synthesis via Enolate: Acidity of hydrogens, alkylation of diethyl malonates and ethyl acetoacetate. Synthesis of ethyl acetoacetate : the claisen condensation, Kelo enol tautomerism of ethyl/acetoacetate. Alkylation of 1,3 dithianes, Alkylation and acylation of enamines.
Organosulphur compounds: Nomenclature, structural, features, methods of formation and chemical reactions of thiols thiocthers, sulphonic acids, sulphonamides and sulphaguanidene.
Unit – IV
Photochemistry: Interaction of radiation with matter, difference between thermal and photochemical processes. Laws of photochemistry, Grothus – Drapper law, stark – Einstein law, Jablonski diagram depicting various processes occuring in the excited state, qualitative description of fluorescence, phosphorescence, nonradiative processes (internal conversion, intersystem crossing), quantum yield, photosensitized reaction, energy transfer processes (simple examples).
Book Suggested
1.         Basic Inorganic Chemistry, F.A. Cotton 9 G. Willkinson and P.L. Gaus Wiley.
2.         Concise Inorganic Chemistry, J.D. Lee, ELBS.
3.         Physical Chemistry G.M. Barrow. International Student Edition IMC Graw Hill.
4.         Organic chemistry, Morrison and Boyd, Prentice Hall.
5.         Fundamentals of organic chemistry Solomons / John Wiley.

CHEMISTRY

CH-603
Chemistry Practical

Unit - I
ORGANIC CHEMISTRY
Steam Distillation :
            Naphthalene from its suspension in water.
            Clove oil from cloves
            Separation of o- and p-nitrophenols
Column Chromatography
            Separation of fluorescein and methylene blue.
            Separation of leaf pigments from spinach leaves
            Resolution of racemic mixture of (+) mandelic acid.
Qualitative Analysis
            Analysis of an organic mixture containing two solid components, using water, NaHCO3, NaOH for separation and preparation of suitable derivatives.
Synthesis of Organic Compounds
(a)        Acetylation of salicylic acid, aniline, glucose and hydroquinone, Benzoylation of aniline and phenol.
(b)        Aliphatic electrophilic substitution. Preparation of ioodoform from ethanol and acetone.
(c)        Aromatic electrophilic substitution
            Nitration
                        Preparation of m-dinitrobenzene
                        Preparation of p-nitroacetanilide
            Halogenation
                        Preparation of p-bromoacetanilide
                        Preparation of 2,4,6 tribromophenol
(d)        Diazotization / coupling
            Preparation of methyl orange and methyl red
(e)        Oxidation
            Preparation of benzoic acid from toluene
(f)        Reduction
            Preparation of aniline from nitrobenzene
            Preparation of m-nitroaniline from m-dinitrobenzene.
Stereochemical Study of Organic Compounds via Models
            R and S configuration of optical isomers.
            E, Z configuration of geometrical isomers
            Conformational analysis of cyclohexanes and substituted cyclohexanes
PHYSICAL CHEMISTRY
Electrochemistry
(a)        To determine the strength of the given acid conductometrically using standard alkali solution.
(b)        To determine the solubility and solubility product of a sparingly soluble electrolyte conductometrically.
(c)        To study the saponification of ethyl acetate conductometrically.
(d)        To determine the ionisation constant of a weak acid conductometrically.
(e)        To titrate potentiometrically the given ferrous ammonium sulphate solution using KMnO4/K2Cr2O2 as titrant and calculate the redox potential of Fe++/Fe+++ system on the hydrogen scale.
Refractometry Polarimetry
(a)        To verify law of refraction of mixtures (e.g. of glycerol and water) using Abbe's refractometer.
(b)        To determine the specific rotation of a given optically active compound. 
Molecular Weight Determination
(a)        Determination of molecular weight of a non-volatile solute by Rast method/Beckmann freezing point method.
(b)        Determination of the apparent degree of dissociation of an electrolyte (e.g., NaCl) in aqueous solution at different concentrations by ebullioscopy.
Record and viva