Syllabus for
Master of Science (Chemistry)
Academic Year  (2021)

The two-year (four semesters) Masters Programme in Chemistry (specialization in Organic Chemistry) aims at providing a comprehensive study of various branches of chemistry to develop a critical and analytical approach to all major areas of the subject. The various courses in the first two semesters are presented in such a way as to give the students a harmonious view of the subject followed by the specialization courses of organic chemistry along with an industrial/institutional project in the third semester. Equal importance is given to both theory and practicals. The teaching methodology includes lectures, demonstration, seminars, projects and presentations.

Programme Outcome/Programme Learning Goals/Programme Learning Outcome:

PO2: Interpret and explain the chemistry of physical characteristics, chemical reactivity, and biological impact of various systems

PO3: Apply the knowledge of chemistry to solve problems in academia, industry and environmental protection.

PO4: Examine and analyze structure-property relationships and their implications

PO5: Perceive, deduce, and justify the chemical properties of various forms of matter from their structure and reactivity.

Continuous internal assessment (CIA) forms 50% and the end semester examination forms the other 50% of the marks in both theory and practical. CIA marks are awarded based on their performance in assignments (written material to be submitted and valued), mid-semester test (MST), and class assignments (Quiz, presentations, problem solving etc.) The mid-semester examination and the end semester examination for each theory course will be for two and three hours duration respectively. The CIA for practical sessions is done on a day to day basis depending on their performance in the pre-lab, the conduct of the experiment, and presentation of lab reports. Only those students who qualify with minimum required attendance and CIA will be allowed to appear for the end semester examination.

This introductory course on mathematics intends to provide the students the required mathematical support to understand the various topics in chemistry.

Vectors: Vectors, dot, cross and triple products etc. The gradient, divergence and curl. Vector calculus, gauss theorem, divergence theorem etc.

Matrix Algebra: Addition and multiplication: inverse, adjoint and transpose of matrices, special matrices (symmetric, skew symmetric, hermitian, skew hermitian, unit, diagonal, unitary etc) and their properties. Matrix equations: Homogenous, non homogenous*, linear equations and conditions for the solution, linear dependence and independence.

Introduction to vector spaces, matrix eigenvalues and eigenvectors, diagonalization, determinants (examples from Huckel theory).

Introduction to tensors: polarizability and magnetic susceptibility as examples.

Functions, continuity and differentiability, rules for differentiation, applications of differential calculus including maxima and minima ( examples related to maximally populated rotational energy levels, Bohr’s radius and most probable velocity from maxwell’s distribution etc), exact and inexact differentials with their applications to thermodynamic properties.

Integral calculus, basic rules for integration*, integration by parts, partial fraction and substitution. Reduction formulae, applications of integral calculus.

Functions of several variables, partial differentiation, coordinate transformations (eg Cartesian to spherical polar), curve sketching.

Variables- separable and exact first order differential equations, homogenous, exact and linear equations. Applications to chemical kinetics, secular equilibria, quantum chemistry etc. Solutions of differential equations by the power series method, fourier series, solutions of harmonic oscillator and legendre equation etc, spherical harmonics, second order differential equations and their solutions.

Different types of series, Fourier series, theory behind Fourier transform: Legendre polynomials, Lagranche undetermined multipliers, Stirling approximation.

Permutations and combinations, probability and probability theorems, probability curves, average, root mean square and most probable errors, examples from the kinetic theory of gases etc, curve fitting (including least squares fit etc) with a general polynomial fit.

[2]    Doggett and Sutcliffe, Mathematics for chemistry, Longman group Ltd, 1995.

[3]    Farrington Daniels, Mathematical preparation for physical Chemistry, Mc Graw Hill,  2003.

[4]    D.M.Hirst, Chemical mathematics, Longman.

[2]    Peter Tebbutt, Basic mathematics for chemists, 2^nd Edition, John Wiley and Sons, 1998.

This course on general research methodology intends to make the students get an idea about research, its methods and its significance.

Introduction - meaning of research - objectives of research - motivation in research– research :a way of examining your practice-types of research - research approaches - significance of research -research methods versus methodology - research and scientific method- importance of knowing how research is done - research processes - criteria of good research -defining research problem - selecting the problem - necessity of defining the problem- techniques involved in defining a problem - research design - meaning of research design - need for research design - features of good design - different research designs - basic principles of experimental design.

Originality in Research: Resources for research - research skills - time management - role of supervisor and scholar - interaction with subject experts.

Source for literature: books -journals – proceedings - thesis and dissertations. On-line Searching: Database – SciFinder – Scopus - Science Direct - Searching research articles.

i) Computer Searches of Literature: ASAP Alerts, CA Alerts, ChemPort, Patent search 
     including STN International; Google Scholar

ii)Steps to publishing scientific articles in journals: types of publications-
    communications, articles, reviews; where to publish, specific format required for
    submission, organization of the material, letters to editor and emails.

iii) Writing a review article- Significance of review of literature, steps of searching the literature, Identification of topic, organization of the content, Conclusion and future pespectives, Language focus

Relationship of review of literature to theory, research, education and practice.

Contents of a research proposal, introduction, The problem - relevance to the society, objectives, study design, methods, analysis, structure of the report, limitations, ethical issues.

Course enrichment activities

Assignment on literature review

Assignment on project proposal writing

[2]  R. Panneerselvam, Research Methodology, New Delhi: PHI, 2005.

[3]  P. Oliver, Writing Your Thesis, New Delhi:Vistaar Publications, 2004.

[4]        J. W. Creswell, Research Design: Qualitative, Quantitative, and Mixed Methods
Approaches, 3nd. ed. Sage Publications, 2008.

[2] B. C. Nakra and K. K. Chaudhry, Instrumentation, Measurement and Analysis, 2nd. ed.
New Delhi: TMH publishing Co. Ltd., 2005.

[3] Gregory, Ethics in Research, Continuum, 2005.

This introductory course on inorganic chemistry intends to make the students understand the basic concepts like chemical bonding, chemistry of elements and nuclear chemistry.

Prelearning: Periodic properties of elements, Types of bonds: ionic, covalent, and coordinate bonds

Slater’s rules and effective nuclear charge, Octet rule, VSEPR model, shapes of molecules; concepts of resonance and hybridization, Electronegativity, Scales of electronegativity (Pauling’s scale, Alred and Rochow’s approach, Mulliken’s approach), Fajans’ rules, coordinate bond, multicentre bond, quadruple bond, synergic bond, Agostic interaction with examples, Hydrogen bond – types and detection; Intermolecular force, metallic bond, Semiconductors and superconductors. 

MO Theory: σ, π and δ molecular orbitals, MOs of diatomic molecules- NO, CO, triatomic molecules- H₂O, NO₂, BeH_2; Walsh diagram, Molecular term symbols of H₂ to O₂.

Ionic bond, Lattice energy, Born-Lande equation (derivation), radius–ratio rules, structures of simple solids-NaCl, CsCl, ZnS, CaF₂, TiO₂, unit cell and number of ions in sphalerite, Spinels and Perovskites. 

Pre learning: Periodicity and general trends in properties

Allotropes of carbon and their applications-Structure and property correlation in  diamond and graphite, carbon nanotubes and fullerens-types and synthesis, Polymorphism of phosphorous and sulphur; properties, structure and bonding in boranes, Styx number-formulae for arriving at the number of 2-centre and 3-centre bonds in boranes, Wade’s rule, carboranes and their classification, Properties, structure and bonding in borazines, phosphazenes, Xenon  compounds, Interhalogen compounds, Silicates–Principles of silicate structures,classification and structures, isomorphous replacement, pyroxenes, silicate glasses, borosilicate glass, silica gel, zeolites and molecular sieves*, polyhalides. Oxyacids of nitrogen, phosphorous, sulphur and halogens**

Bronsted and Lewis concept of acids and bases, Luxflood acid base theory, HSAB concept, acid – base concept in non- aqueous media, levelling effect, super acids, non-aqueous solvents-NH_3, sulphuric acid, glacial acetic acid and anhydrous HF.

Role of metal ions in biological systems-essential and trace metal, ion transport across membranes, sodium potassium pump*, ionophores, oxygen transport mechanism- haemoglobin and myoglobin*, metalloenzymes-carboxypeptidase, carbonic anhydrase, alcohol dehydrogenase, vitamin B₁₂, metal complexes in medicine (cisplatin).

Sub-atomic particles and their properties, nuclear stability (Binding Energy, Packing fraction, Meson theory, Characteristics of nuclear forces), Liquid drop model and shell model of the nucleus. 

Course enrichment activities

CSIR Based problems will be solved in the class

[2]  J. E. Huheey, E. A. Keiter and R. L. Keiter, Inorganic Chemistry – Principles of Structure and Reactivity, 4th ed., Pearson Education Asia Pvt. Ltd., 2000.

[3]  D. F. Shriver, P. W. Atkins and C.H. Langford. Inorganic chemistry, 3^rd ed., ELBS: Oxford University Press, Oxford, UK, 1999. 

[4] N. N. Greenwood and A. E. Earnshaw, Chemistry of the elementals, 2^nd ed., Butterworth
Heinemann, 1997.

[5] D. M. P. Mingos, Essential Trends in Inorganic chemistry, Oxford Univ. Press, 1998.

[6] J. D. Lee, Concise inorganic chemistry, 5^th ed., Chapman & Hall: Hong Kong,Reprint 2009.

[7] K. F. Purcell and J C. Kotz, Inorganic Chemistry, Indian reprint, Cengage Learning India  Pvt Ltd, 2010.

[2] K. Hussain Reddy, Bioinorganic Chemistry, New age International publishers, Reprint
2007.

[3] Asim K. Das, Bioinorganic Chemistry, 1^st ed., Books and Allied P ltd., 2010.

[4] Bertini, H.B. Gray, S.J. Lippard and J.S.Valentine, Bioinorganic Chemistry, Viva Books,
1998.

[5] H. J. Arnikar, Essentials of nuclear chemistry, 4^th ed., NAIL Pub, 1995.

[6] William M Portfield, Inorganic Chemistry-An Unified Approach (Indian Reprint) Academic
Press, 2005.

This course on organic chemistry intends to make the students understand the basic concepts like nature of bonding in organic molecules, reaction mechanisms, stereochemistry, free radical chemistry, natural products and vitamins.

Hybridization, Delocalized chemical bonding*: Conjugation, cross conjugation, resonance, hyper conjugation. Field effects, steric effects and their influence on the properties of organic molecules (dipole moment, acidity, etc). Consequences of delocalized chemical bonding on bond length, bond angle, dipole moment, acidity and basicity. Tautomerism.  Huckel’s rule. Aromaticity in benzenoid, meso-ionic compounds and non-benzenoid compounds- Introduction, preparation of cyclopropenyl cations, cyclobutadienyl dications, cyclopentadienyl anions, cycloheptatrienium cation, cyclooctatatraenyl dication, Frost diagrams, [10], [14], and [18]-annulenes, azulene. Energy level of π–molecular orbital, antiaromaticity, homo-aromaticity.

Types of reactions and mechanisms.  Potential energy diagrams, transition states and intermediates, Thermodynamic and kinetic requirements, Hammond’s postulate, Curtin-Hammett principle, methods of determining mechanisms, isotope effects, hard and soft acids and bases.

Generation, structure, stability and reactivity of carbocations*, carbanions, carbenes and nitrenes.

Effect of structure on reactivity –The Hammett equation and linear free energy relationship, substituents and reaction constants, Taft equation.

Nucleophilic substitution reaction at a saturated carbon: SN¹, SN² and SNⁱ mechanisms, Effect of substrate structure, attacking nucleophile, and leaving groups, Neighbouring group participation, ambident nucleophiles and substrates.

Generation of free radicals: Thermal homolysis of per esters and azo compounds,       photochemical methods. Hydrogen abstraction, chain process. Stability: Steric, resonance and hypercojugative effects. Structure and stereochemistry of free radicals. Free radical reactions: Addition, elimination, rearrangement and electron transfer reactions. Use of free radicals in organic synthesis. SET reactions.

Fischer, Newman, Sawhorse and flying wedge projections and their interconversions. Optical isomerism: Elements of symmetry and chirality. D-L and R-S conventions. Cram’s and Prelog’s rules. Felkin-anh model. Conformational analysis of acyclic compounds: ethane, propane, n-butane and  1,2–disubstituted ethanes.  Cyclic alkanes: cyclopropane, cyclobutane, cyclohexanes (monomethyl, iso-propyl, tert-butyl and di-substituted cyclohexanes e.g., dialkyl, dihalo, diols), and cycloheptane. Conformations of fused and bridged ring systems. Prochirality: Enantiotropic and disastereotropic groups and faces. 

Geometrical isomerism: cis–trans and E-Z conventions.  Methods of interconversion of E and Z isomers. 

Determination of configuration of the monosaccharide. Conformational analysis of glucose and galactose*.   Structural elucidation of sucrose and maltose. Synthesis of aldonic, uronic, aldaric acids and alditols.  Structures of gentiobiose, meliobiose, and chitin.  Photosynthesis of carbohydrates.  Industrial and biological importance of glycosides.       

Biological importance and synthesis of Vitamins A*, Vit. B₁ (thiamine), Vit. B₆ (pyridoxine), Vit. C, Vitamin E (α-tocopherol), Vit. H (biotin), Vit. K₁, K₂, folic acid, pantothenic acid and riboflavin. 

Conducting Polymers: Synthesis, properties and applications of polyaniline, polypyrrole, polythiophene and poly(p-phenylenevinylene).

Bio-polymers: Basic concepts of biopolymers/biodegradable polymers (polylacetic acid, poly caprolactone, starch, etc.), hydrogels, smart hydrogels and their applications, Recycling.

Course enrichment activities

CSIR Based problems will be solved in the class

[2] A. Carey Francis and J. Sundberg Richard, Advanced Organic Chemistry, 5^th ed., Springer, 2007.

[3] Stykes Peter, A guide book to mechanism in organic chemistry, Orient Longman Limited, 2000.

[4]  C. K. Ingold, Structure and mechanism of organic chemistry, Cornell University  Press, 1999.

[5]  H. Pine Stanley, Organic Chemistry, Tata McGraw-Hill Education, 2007.

[6]  R. T. Morrison and  R. N. Boyd, Organic chemistry, 7^th-Edition,Fifth impression, Prentice-Hall, 2014.

[7]  R. O. C. Norman and J. M. Coxon, Principles of organic synthesis, Blackie Academic and Professional, 1996.

[8] P. Y. Bruice, Organic Chemisty,7^th edition,10^th impression, Pearson Education, 2019.

[9] D. Nasipuri, Stereochemistry of organic compounds, New Delhi, New-Age International, 1999.

[10] E. L. Eliel, S. H. Wilen and L. N. Mander, Stereochemistry of carbon compounds, John Wiley 2011.

[11] György Inzelt, Conducting Polymers A New Era in Electrochemistry,Springer, 2008.

[2] I. L. Finar, Stereochemistry and the Chemistry the Natural Products, 5^th ed., Pearson Education Ltd., 2009.

[3]  N. Selwad and  H-D Jakubke, Peptides: Chemistry and Biology, Wiley – VCH, 2002.

[4]  J. Apsimon, Total synthesis of natural products,  Vol. I – Vol. VI, NY,  John Wiley, 2007.

Assessment Pattern for Theory

This course on physical chemistry intends to make the students aware of topics like quantum mechanics, chemical dynamics and surface chemistry.

a. Formulation of quantum mechanics: Wave particle duality of material particles, de Broglie’s relation, Heisenberg’s uncertainty principle. Equations of wave motion: Progressive and stationary waves, wave equation for a stationary wave (stretched string).

       Schrödinger wave equation. (Time–independent and time-dependent Schrödinger equations).  Eigen function and eigen value.  Physical interpretation of wave function. Concept of operators. Linear, Laplacian, Hamiltonian, commutator and Hermitian operators. Angular momentum operators and their properties. Normalization, orthogonality and orthonormality of wave functions. Postulates of quantum mechanics. Average (expectation) values Solutions of Schrödinger equation for a free particle, particle in a one-dimensional box and three-dimensional box. Quantum mechanical degeneracy, tunneling (no derivation).   (12 Hrs)                                                                                                                 

b. Application of Schrödinger equation to harmonic oscillator and rigid rotator. Eigenfunctions and eigenvalues of angular momentum. Ladder operator method for angular momentum. Schrödinger equation to hydrogen atom in spherical polar coordinates. Solution of Φ, θ equations and statement of solution of R equation. Total wave function of hydrogen atom. Quantum numbers and their characteristics. List of wave functions for initial states of hydrogen-like atoms. Diagrams of radial and angular wave functions. Radial and angular distribution functions and their significance.  Electron spin (Stern – Gerlach experiment) *, spin orbital, antisymmetry and Pauli’s exclusion principle, Slater determinants. Coupling of angular momenta. Russell-Saunders and JJ-coupling, term symbols.  Spin-orbit interaction and explanation of term multiplicities (Na-D doublet), Zeeman effect*.  (12 Hrs)                                                                                                                                                                                                                                     

c.          Approximate methods: Need for approximate methods. Perturbation method. Application to electron in a box under the influence of an electric field. Application to He atom. Variation theorem- Statement and proof.  Application of variation method to particle in a one dimensional box, linear oscillator and He atom. Slater type orbitals, expressions for Slater orbitals for 1s, 2s, 3s, 2p and 3d electrons (no derivation).  Slater’s rules for calculation of effective nuclear charge.  STOs, for He, C and N. SCF method for many electron atoms. HOMO theory for conjugated systems. Application to ethylene, allyl anion, allyl cation, allyl free radical, butadiene and benzene .  (8 Hrs)                                                                                

a. Macroscopic and microscopic kinetics: Empirical rate laws and temperature dependence, Methods of determination of order and rate laws, Collision theory of reaction rates-limitations. Transition state theory. Comparison of collision theory and transition state theory, reaction between ions: influence of ionic strength-primary and secondary kinetic salt effects. Diffusion and activation controlled reactions in solution. Thermodynamical formulation of reaction rates (Wyne-Jones and Eyring treatment).   (3 Hrs)

 b. Steady state kinetics: Theories of unimolecular reactions, Lindemann theory, RRKM theory (qualitative treatment only), Chain reactions-general characteristics, chain length and chain inhibition (Self study). Mechanisms of thermal reactions (hydrogen-chlorine, pyrolysis of acetaldehyde, decomposition of ethane) and photochemical reactions (H₂ - Br₂ and H₂–Cl₂). Comparative study of thermal and photochemical hydrogen-halogen reactions.   (5 Hrs)                                                                                                                                                                                                                                                                                                                

c. Theory of homogeneous catalysis, Enzyme catalysis-comparison of enzyme with chemical  catalysts, mechanism (lock and key theory), Henri-Michaelis-Menten treatment, significance of Michaelis constant, Lineweaver-Burk plot. Effects of concentration, pH, temperature, activators   and inhibitors on enzyme activity (Self Study).  Theory of homogeneous catalysis. Add the following: Acid-base catalysis: specific and general catalysis, Skrabal diagram, Bronsted catalysis law, prototropic and protolytic mechanism with examples, acidity function.   (6 Hrs)                                                                                                                                               

d.     Kinetics of fast reactions-study of fast reactions by stopped flow technique, relaxation method, flash photolysis and NMR method.   (3 Hrs) 

Effect of temperature on adsorption, mechanical adsorption, Types of adsorption isotherms, BET and Gibbs adsorption isotherms, estimation of surface area using BET equation, vapour pressure of droplets (Kelvin equation). Application of photoelectron spectroscopy*, ESCA and Auger spectroscopy for the study of surfaces. Mechanisms of heterogeneous catalysis: unimolecular and bimolecular surface reactions, mechanisms of catalyzed reactions like ammonia synthesis, Fischer-Tropsch reactions.

Introduction, Synthesis – laser ablation chemical vapour transport method (CVT) and sol gel method, synthesis of metal oxides and its composite nanoparticles by solvo thermal and hydrothermal method.

Course Enrichment Activities

CSIR-based problems will be solved in the class.

[2] Mc Quarrie and Simon, Physical chemistry: A molecular approach, New Delhi: Viva, 2011.

[3] A. K. Chandra, Introduction to quantum chemistry, New Delhi: Tata McGraw Hill, 2001.

[4] Levine, N. Ira, Quantum chemistry, New Jersey: Prentice Hall, 2009.

[5] R. K. Prasad, Quantum chemistry. 2^nded. New Delhi: New Age International, 2011.

[6] R. K. Prasad, Quantum chemistry through problems and solutions, 1^sted. New Delhi: New Age International, 2009.

[7] K. J. Laidler, Chemical Kinetics, 2^nd ed. Inc. New York: McGraw Hill, 2012.

[8] J. E. House and M. C. Brown, Principles of Chemical Kinetics, 2^nd ed. Elsevier India Pvt.ltd,  2012.

[9] C. Kalidas, Chemical Kinetic Methods, 1^st ed. New Delhi: New Age International Publisher, 2010.

[10] J. Kuriakose and J Rajaraman. Kinetics and mechanism of chemical transformation. New Delhi: McMillan Publishers, 2009.

[2] C. N. R. Rao, Nanoscience and technology, Navakarnataka Publications Pvt Ltd, 2011.

[3] A. K. Bandyopadyay, Nanomaterials, NAI publishers, 2010.

[4] K. Krishna Reddy and Balakrishna Rao, Nanotechnology Nanostructures & Nanomaterials,Campus Books International, 2007.

[5] Thomas Engel and Philip Reid, Physical Chemistry, Pearson Education, Inc, 2006.

This course on analytical chemistry intends to enlighten the students on topics like separation techniques, optical methods of chemical analysis, electro analytical techniques and thermal methods of analysis. This course will help students to understand the basic routine experiments in all the industrial and research labs.

Classifications of analytical methods, factors influencing choice of analytical method, toxic chemicals sampling and handling hazards, material safety data sheets. Miniaturization of analytical methods and its significance in modern chemical analysis. Replicate analysis, reliability of analytical data, mean and median & range precision and accuracy, methods of expressing precision and accuracy: deviation, mean deviation, relative mean deviation, and standard deviation. Detection limits, Quantitation limits, Errors, absolute error, relative error. Determinate errors, classification of determinate errors and their minimization, indeterminate error and normal frequency distribution curve.

Statistical treatment of analytical data: confidence limits, students T-test, rejection of data: Q test, 4d rule and 2.5d rule. Graphical representation of results, methods of averages, methods of least squares. Significant figures, Reporting of analytical data.

Solvent extraction, efficiency, selectivity*, Nernst distribution law, distribution coefficient, derivation for the most efficient extraction, applications and numerical problems. Methods- batch and continuous extraction of liquids, continuous solid- liquid extraction (Soxhlet extraction of phytochemicals).

Chromatography – classification, mechanisms-adsorption, partition. ion exchange, size exclusion and affinity chromatography.  retention in chromatography, Plate theory, Retention parameters, efficiency, resolution, Peak asymmetry- Gaussian and skew profile, tailing and fronting, peak broadening- van Demeter equation.

Principle and applications of thin layer chromatography.

Gas chromatography- Theory and instrumentation detectors used in GC, temperature programming in GC, Applications, High performance liquid chromatography-Theory and instrumentation. Bonded stationary phases, Normal phase and reversed phase liquid chromatography, Detectors in HPLC: absorbance detector, refractive index detector, electrochemical detector, HPLC-MS, Chiral stationary phases

 Theory and application of Electrophoresis.

Pre-learning topics: Beer-Lambert’s law and derivation. Interaction of electromagnetic radiation with matter, Beer-Lambert’s law, verification, deviations, molar extinction coefficient

choice of solvents, photometric titrations, Single beam and double beam UV-Vis spectrophotometer.

Atomic absorption spectroscopy- instrumentation and application in quantitative and qualitative analysis, Numerical problems.

Principle, instrumentation and applications of fluorimetry, turbidimetry and nephelometry.

Potentiometry- electrode systems, potentiometric titrations- acid- base, precipitation and redox titrations.

Polarography* and Voltammetry- three electrode system, role of supporting electrolyte, Diffusion currents, deposition potential, residual current half-wave potentials, characteristics of the DME.

Amperometric titration and applications of polarography.  Electrogravimetry, Coulometry, Coulometry at constant potential, applications.    Conductometric titrations- ionic conductances, acid-base titrations. Chemically modified electrodes and their Quantitative applications.

Theory, instrumentation and applications of TGA, DTA and DSC.

Pre Learning topics: working principles of scintillation counter, GM counter.

Radioactivity, ionization, germanium detectors, working principles of scintillation counter, GM counter, Radio analytical methods- neutron activation analysis, isotopic dilution analysis, radiotracer technique. Applications of all these techniques use of radioactive isotopes in solving analytical and physico chemical problems*.

Course enrichment Activities:

Preparation of material safety data sheet for selected compounds, which will help in understanding the sense of safety and practice in the experimental lab. 

This activity is in alignment with our graduate attributed GA7 and GA 8

[2]  Douglas A. Skoog and F. James Holler, Timothy A. Nieman, Principles of instrumental analysis, 1998.

[3]  H.H. Willard, L.L. Merrit, J.A. Dean and F.A. Settle, Instrumental methods of analysis, CBS Publishers: 7th ed., 1986.

[4] A.J. Bard and I.R. Faulkner, Electrochemical methods, 2nd ed., Wiley: New York, 2000.

[5] Wilson Keith and John Walker, Principles and techniques of Biochemistry and Molecular biology, 6th ed., Cambridge, 2005.

[6] Skoog, West, Holler and Crouch. Fundamentals of analytical chemistry, 8th ed. Thomson Asia Pvt. Ltd, 2004.

[2] S. M. Khopkar, Basic concepts of analytical chemistry, 3ed ed., New age international,  2009.

[3] Robert A. Meyers, Encyclopedia of Analytical Chemistry: Applications, Theory, and  Instrumentation, 15 volume Set, Wiley, 2011.

[4]   Robinsen, Undergraduate instrumental analysis 6th ed, Taylor and francies, 2004

This practical course on inorganic chemistry intends to provide the students scientific skills in qualitative and preparative techniques.  

Semi-micro qualitative analysis of mixtures containing i) two common cations ii) two anions out of which one is interfering anion and iii) one of the following less familiar elements: W, Mo, Ce, Th, Zr, V, U and Li.

1.       Ferrous oxalate

2.       Potassium trioxalatoferrate(III)trihydrate.

3.       Hexammine cobalt(III)chloride.

4.       Cis and trans-potassium dioxalatodiaquochromate(III).

5.       Preparation of a coordination complex using Schiff base ligand and characterization by UV and IR spectroscopic methods.

 [2]   J. Bassett, G.H. Jeffery and J. Mendham, and R.C. Denny, Vogel’s text book of qualitative  chemical analysis, 5^th ed., Longman Scientific and Technical, 1999.

This practical course on physical chemistry is aimed to develop experimental skills in students in topics like chemical kinetics, colorimetry, cryoscopy and adsorption. This course imparts team building, imagination leads to new explanations and new solutions.

1.       Determination of the velocity constant, catalytic coefficient, temperature coefficient, t_1/2 and energy of activation for the acid hydrolysis of methyl acetate.

2.       Evaluation of Arrhenius parameters for the reaction between potassium persulphate and potassium iodide (1^st order).

3.       Velocity constant for the saponification of ethyl acetate.

4.       Determination of the order of reaction between hydrogen peroxide and potassium iodide (clock reaction).

5.       Determination of relative strength of acids (HCl) by ester hydrolysis.

6.       Determination of equilibrium constant for acid hydrolysis of an ester.

7.       Determination of equilibrium constant of keto-enol tautomerism. (ethyl acetoacetate and acetoyl acetone, AcAc)

8.       Determination of Transport number of Ag+ and NO₃ ^– by Hittorf’s method. 

9.       Study the primary salt effect on the kinetics of ionic reactions and test the Bronsted relationship (iodide ion is oxidized by persulphate ion).

Colorimetry 

1.       Test for the validity of Beer–Lambert Law and determination of the unknown concentration of a solution. Calculation of molar extinction coefficient.

2.       Titration of ferrous ammonium sulfate with potassium permanganate colorimetrically.

3.       Simultaneous estimation of Mn and Cr in a solution of KMnO₄ and K₂Cr₂O₇.

4.       Kinetics of reaction between K₂S₂O₈ – KI Colorimetrically. 

5.       Determination of concentration of Fe by spectrophotometric titration using EDTA.

Cryoscopy 

6.       Determination of molecular weight of a solute by cryoscopy.

7.       Determination of degree of dissociation of an electrolyte and association of benzoic acid in benzene.

Partial Molal Volume

8.       Determination of partial molal volume of ethanol by reciprocal density method.

9.       Determination of PMV by apparent molar volume method, NaCI – H₂O system.

Phase diagram

10.   Construction of phase diagram of a two–component system and determination of eutectic temperature and eutectic composition.

11.   Construction of phase diagram of a three–component system and etermination of the % of the components in the given mixture.

Adsorption 

12.   Adsorption of oxalic on charcoal. Verification of Langmuir adsorption isotherm.

Polymers

13.   Determination of molecular weight of a polymer material by viscosity method.

[2]  Shoemaker and Garland. Experiments in physical chemistry. McGraw Hill International edn: 1996.

[3]  J. B. Yadav, Advanced practical chemistry, Krishna Prakashan Media Pvt. Ltd, Meerut, 2010. 

[4]  Wilson, Newcomb and others, Experimental physical chemistry.  Pergamon Press: New York, 1962.

[2]        V.D. Athawale and Parul mathur. Experimental physical chemistry. New Age International: New Delhi, 2001. 

This practical course on organic chemistry intends to provide the students scientific skills in qualitative and preparative techniques.

Separation of a binary mixture of organic compounds and identification of the separated components by systematic qualitative organic analysis. 

Preparation of the following compounds: 

1. p- Nitro aniline from acetanilide.

2. p-Bromoaniline from acetanilide.

3. m-Nitro benzoic acid from methyl benzoate.

4. Anthranilic acid from phthalic anhydride.

5. Cannizarro reaction: Benzaldehyde 

6. Friedel - Crafts reaction

[1]           B. B. Dey, M. V. Sitaraman and T. R. Govindachar, Laboratory manual of organic chemistry, New Delhi: Allied Publishers, 1996.

[2]        A. I. Vogel, Text book of practical organic chemistry, 1996.

[3]        V. K. Ahluwalia and R. Aggarwal, Comprehensive practical organic chemistry: Preparations and Quantitative analysis, University press, 2004.

[2]  A. I. Vogel, Text book of practical organic chemistry, 1996.

[3]  V. K. Ahluwalia and R. Aggarwal, Comprehensive practical organic chemistry: Preparations and Quantitative analysis, University press, 2004.

Course description

This course on computers for chemists intends to provide the students the required knowledge and skill to use the various tools and software packages which are helpful in studying the various topics in chemistry.

Introduction to computational chemistry: As a tool and its scope.

Non-quantum mechanical computational methods - Molecular mechanics: Force fields - bond stretching, angle bending, torsional terms, non-bonded interactions, electrostatic interactions and the corresponding mathematical expressions. Commonly used force fields - AMBER and CHARMM.

 Semi empirical methods: Huckels and extended Huckel methods. Strengths and weaknesses. PPP, ZDO, NDDO, INDO, MNDO (AM1, PM3) and CNDO approach.(Mentioning only).

 Quantum mechanical computational methods - Abinitio methods:

Hatree Fock Methods: Introduction to SCF. RHF, ROHF and URH. (no need for derivation). Wave functions for open shell state, Slater determinants, Roothan concept. Electron correlation and Post Hatree Fock Methods- Configruation interaction, coupled cluster methods, Moller-Plesset perturbation theory, quadratic configuration interaction, composite methods like G2, G3, CBS.

Basis functions-Slater type orbitals (STO) and Gaussian type orbitals (GTO) basiis sets: minimal, split valence, polarized and diffuse basis sets, contracted basis sets, Pople’s style basis sets and their nomenclature, Dunning’s basis sets, Aldrich’s basis sets.

Density functional theory methods (DFT) –Basics- Hohenberg-Kohn theorems, Exchange correlation functional Kohn-Sham orbitals, Local density approximation. Generalized gradient approximation, hybrid and double hybrid functionals. (Rigorous mathematical treatment not needed).

 Types of calculations- single point, geometry optimization, frequency. Potential energy surface-stationary point, saddle point or transition state, local and global minima.

Introduction to molecular dynamics.

Introduction to the following methods with practical experience.

Introduction of the following packages

Visualization software: Avogadro, Chimera, UCLA

Molecular mechanics and docking: AMBER/TINKER Autodock and Autodock Vina, HEX

Semi empirical studies: Gaussian / MOPAC

Abinitio and DFT studies: GAMESS/ Gaussian / ORCA

Molecular dynamics: GROMACS (optional)

Data mining and analysis, QSAR, QSPR, Data analysis, introduction to machine learning and artificial intelligence in Chemistry

2. F Jensen, Introduction to Computational Chemistry, Wiley

3. Ramesh Kumari and Narosa. Computers and their applications to Chemistry, Narosa, 2^nd Edition, Reprint 2011.

2. F Jensen, Introduction to Computational Chemistry, Wiley

3. Ramesh Kumari and Narosa. Computers and their applications to Chemistry, Narosa, 2^nd Edition, Reprint 2011.

This course gives an overview of different aspects of scientific communication like written communication, poster and oral presentations and writing grant proposals.

Research – What is it? How do researchers communicate? Types of scientific communication.

Searching the scientific literature using Pubmed, Web of ScienceUsing online search

engines. What is a refereed journal? Plagiarism and how to avoid it. 

Establishing the constraints-Organizing the writing-Preparing outlines Standard formats and types of scientific papers.

Creating a literature review-Preparing other sections of a research report (abstract, introduction, materials and methods, results and discussion, conclusions)-Including and summarizing research data. 

Scientific writing style-First-person vs. Third-person; Passive vs. active voice Avoiding excessive wording-Grammar-Avoiding misuse of words.

How to use references- Within the text - How to make lists of references. 

Dealing with revisions-Accepting criticism-Making sense of reviewers’ comments. Making the changes-What to do if you don’t agree with reviewers’ comments.

Other types of scientific writing- research proposals- creating a fact sheet/bulletin articles for popular press- memos, letters and emails.

Organization and formats for posters Using Microsoft PowerPoint.

Designing and preparing slides for an oral presentation- Importing tables, charts and graphs from Excel- Optimizing pictures for use in presentations-Using visual aids without overdoing it.

Team assignment for oral presentation of a scientific paper.

Individual assignment for grant proposal writing.

[2]. J. E. Harmon and A. G. Gross, The Craft of Scientific Communication, Chicago Guides to Writing, Editing, and Publishing, 2010.

[2]. Cheng, M. Claessens, T. Gascoigne, J. Metcalfe, B. Schiele, and S. Shi, Communicating Science in Social Contexts: New models, New Practices, (eds.), New York: Springer, 2008. 

This course on inorganic chemistry intends to enlighten the students on topics in coordination chemistry like theories of metal ligand bonding, metal-ligand equilibria, electronic and magnetic properties of metal complexes.

Step-wise and overall formation constants and their relationship, trends in step-wise constant, kinetic and thermodynamic stability of metal complexes, factors affecting the stability of metal complexes with reference to the nature of the metal ion and ligand, chelate and macrocylic effects*and their thermodynamic origin, determination of binary formation constants by spectrophotometry, polarography and ion exchange methods.

Crystal field theory*, stereochemistry and splitting of metal d-orbitals in complexes with coordination numbers 3 to 8, structural evidences for CF splitting-hydration, ligation and lattice energies, Spectrochemical series, Factors affecting 10 Dq, Jahn–Teller distortion in metal complexes and metal chelates, Limitations of CFT, evidences for metal–ligand orbital overlap, Nephelauxetic effect and series, ESR, NMR and NQR spectral evidences for M-L covalency. MO theory, 18 e rule, Group theoretical approaches based MO energy level diagrams of H₂O, tetrahedral and octahedral complexes (including π-bonding), Structure and bonding of Zeise’s salt.

Hydride, dihydrogen, simple metal carbonyl, nitrosyl, dinitrogen and tertiary phosphine complexes, stereochemical non-rigidity*, self-assembly in supramolecular chemistry*; stereoisomerism-chirality, optical activity, CD, ORD, cotton effect and magnetic circular dichroism, absolute configurations.

Types of electronic transitions, Spectroscopic ground states, selection rules, term symbols for dⁿ ions, Racah parameters, Orgel, correlation and Tanabe-Sugano diagrams, spectra of 3d metal aqua complexes of trivalent V, Cr, divalent Mn, Co and Ni, [CoCl₄]^2-; calculation of Dq, B and β and x parameters, charge transfer spectra, spectra of lanthanides and actinides.

Origin and types of magnetic behaviour- diamagnetism, paramagnetism, ferro and antiferromagnetism, magnetic susceptibility and its measurement by the Guoy method, temperature dependence of magnetism– Curie and Curie-Weiss laws, types of paramagnetic behaviour – spin-orbit coupling, magnetic behaviour of lanthanide ions, quenching of orbital contribution and spin only behavior.

Course enrichment activities

CSIR Based problems will be solved in the class

[2]  F. A. Cotton, G. Wilkinson, Advanced inorganic chemistry, 6^th ed., John Wiley & sons,
2009.

[3]  J. E. Huheey, E. A. Keiter and R. L. Keiter, Inorganic Chemistry – Principles of Structure
and Reactivity, 4th edition, Pearson Education Asia Pvt. Ltd., 2000.

[4]  D. F. Shriver, P. W. Atkins and C.H. Langford, Inorganic chemistry, 3^rd ed., ELBS: Oxford
University Press, Oxford, UK, 1999. .

[5]  N. N. Greenwood and A. E. Earnshaw, Chemistry of the elementals, 2^nd ed., Butterworth
Heinemann, 1997.

[6]  D. M. P. Mingos, Essential Trends in Inorganic chemistry, Oxford Univ. Press, 1998.

[7]  J. D. Lee, Concise inorganic chemistry, 5^th ed., Chapman&Hall: Hong Kong, Reprint 2009.

[2]  G. L. Miessler and D. A. Tarr, Inorganic Chemistry, 4^th ed., Prentice Hall, 2010.

[3]  D. N. Sathyanarayana, Electronic absorption spectroscopy and related techniques,
Universities Press: 2001.

[4]  William M Portfield, Inorganic Chemistry-An Unified Approach (Indian Reprint) Academic
Press, 2005.

This course on organic chemistry intends to make the students understand topics like aromatic substitution, addition, elimination and rearrangement reactions, peptide chemistry and nucleic acids. This course helps the students to develop logical approach to solve problems.

Electrophilic substitution reactions: The arenium ion mechanism, orientation and reactivity, energy profile diagrams.  The ortho/para ratio, ipso attack, orientation in other ring systems.  Quantitative treatment of reactivity in substrates and electrophiles.  Diazonium coupling, Vilsmeier reaction, Gattermann-Koch reaction. 

Nucleophilic substitution reactions: The S_N Ar, S_N¹, benzyne and SR_N¹ mechanisms. Reactivity – effect of substrate structure, leaving group and attacking nucleophile. The von Richter, Sommelet-Hauser and Smiles rearrangements.

Addition to carbon multiple bonds: Mechanistic and stereochemical aspects of addition reactions involving electrophiles, nucleophiles and free radicals. Regio, stereo and chemoselectivities.  Orientation and reactivity.  Addition to cyclopropane ring.  Hydrogenation of double and triple bonds, hydrogenation of aromatic rings. Hydroboration, Michael reaction*. 

Addition to carbon-heteroatom multiple bonds: Mechanism of metal hydride reduction of saturated and unsaturated carbonyl compounds, acids, esters and nitriles. Additional of Grignard reagents and organo lithium reagents to carbonyl compounds and unsaturated carbonyl compounds.  Addition of water and formation of acetals, ketals, oximes and hydrazones from carbonyl compounds, Wittig reaction*. Mechanism of condensation reactions involving enolates-Aldol, knoevenagel, Clasisen, Mannich, Benzoin, Perkin and Stobbe reactions*. Ammonolysis of esters, hydrolysis amides. 

The E2, E1 and E1cB mechanisms. Orientation of the double bond.  Reactivity – effects of substrate structure, attacking base, the leaving group and the medium. Mechanism and orientation in pyrolytic elimination.

Introduction to types of rearrangements, Wagner–Meerwein, Pinacol–Pinacolone, Wolff, Beckmann, Hofmann*, Curtius, Lossen and Schmidt rearrangements.

Introduction, protecting groups for hydroxyl group in sugar, amino group in the base and phosphate functions. Methods of formation of internucleotide bonds: DCC and phosphodiester approaches, phosphoramide method, Solid phase synthesis of oligonucleotides.

Classification and nomenclature. Sanger and Edman methods of sequencing. Cleavage of peptide bond by chemical and enzymatic methods.  Peptide synthesis – Protection of amino group (Boc-, Z- and Fmoc-) and carboxyl group as alkyl and aryl esters.  Use of EDHCl, EEDQ, HOBt and active esters, acid halides, anhydrides in peptide bond formation reactions.  Deprotection and racemization in peptide synthesis. Solution and solid phase techniques.  Synthesis of oxytocin.  Introduction to peptidomimetics. 

Enzymes-enzyme catalyzed organic reactions.

Definition and significance. Structures and function of receptors with molecular clefts. Molecular tweezers*, receptors with multiple hydrogen bonding sites, cyclophanes, calixarenes and cyclodextrins.

[2]A. Carey Francis andSundberg Richard, Advanced Organic Chemistry, 5th ed., Springer,
2007.

[3] Sykes Peter, A guide book to mechanism in organic chemistry, Orient Longman Limited,
2000.

[4] C. K. Ingold, Structure and mechanism of organic chemistry, Cornell University Press,
1999.

[5] T. W. Graham Solomons and Craig Fryhle, Organic Chemistry, 8th Edition, Wiley
 publication 2004.

[6]  H. Pine Stanley , Organic Chemistry, Tata McGraw-Hill Education, 2007.

[7]  R. T. Morrison and R. N Boyd, Organic chemistry, Prentice-Hall, 6^th-Edition, 2008.

[8]  R. O. C Norman and  J. M Coxon,  Principles of organic synthesis,  Blackie Academic and
 Professional, 1996.

[9]   M.  Bodansky, Peptides chemistry: A practical text book, NY, Springer-Verlag, 1998.

[10]  N. Selwad and H. D  Jakubke, Peptides: Chemistry and Biology, Wiley – VCH, 2002.

[11] P. Y. Bruice, Organic Chemisty,7^th edition,10^th impression, Pearson Education, 2019.

[2] Nasipuri, Stereochemistry of organic compounds, New Delhi, New-Age International,
1999.

[3] L. Eliel and L. Norman Allinger, Stereochemistry of carbon compounds vol-VII, John
Wiley 2007.

[4] I. L Finar, Stereochemistry and The Chemistry Natural Products, 5^th edition volume-2,
Pearson Education Ltd., 2009.

This physical chemistry course intends to enlighten the students on topics like classical and statistical thermodynamics and electrochemistry. This course induces to understand the energy concerns.

Concepts of distribution, thermodynamic probability and most probable distribution. Distribution laws. Derivation of Maxwell Boltzmann, Bose-Einstein and Fermi-Dirac  distribution equations (using Lagrange's method of undetermined multipliers). Comparison of the three statistics. Concept of an ensemble-Canonical, grand canonical and microcanonical ensembles.

Partition functions – translational, rotational, vibrational and electronic partition functions. Calculation of thermodynamic properties in terms of partition functions. Applications of partition functions. 

Theory of heat capacity of solids – Einstein’s theory and Debye theory. Application of Fermi-Dirac statistics to metal for the interpretation of electronic heat capacity. Application of Bose-Einstein statistics to helium.  

Thermodynamics of irreversible processes with simple examples. Criteria for non-equilibrium states. Uncompensated heat and its physical significance. Entropy production- rate of entropy production, entropy production in chemical reactions, the phenomenological relations. The principle of microscopic reversibility, the Onsager reciprocal relations. Thermal osmosis. Thermoelectric phenomena.

Brief resume of concepts of laws of thermodynamics – free energy, chemical potential and entropies. Partial molar properties – partial molar free energy, partial molar volume, and their significance. Thermodynamics of mixing, Gibbs-Duhem-Margules equation. Determination of these quantities. Concept of fugacity and its determination by graphical method and compressibility factor method.  Non ideal systems–Excess functions for non-ideal solutions. Activity and activity coefficient. Relationship between mole fraction, molality, molarity and activity coefficients*. Determination of activity coefficient by EMF and solubility methods.  Phase rule – Derivation of phase rule from the concept of chemical potential, application of phase rule to three component systems.  

Ionic atmosphere, physical significance of χ (Chi), Debye-Huckel theory to the problem of activity coefficient, Debye Huckel limiting law*, the Huckel and Bronsted equation, qualitative verification of Debye-Huckel equation, Debye-Huckel Onsager conductance equation, Bjerrum theory of ion association-triples ion-conductance minima.

Introduction to electrode – electrolyte interface, parallel plate capacitor model of double layer, Diffuse double layer, Stern Theory of double layer, thermodynamics of electrified interfaces, concept of surface excess, determination of charge density on the electrode. Electrocapillary curves- Lipmann equation (derivation). 

Conversion and storage of electrochemical energies-Batteries, Primary and secondary fuel cells, Corrosion and prevention*.       

Course enrichment activities

CSIR based problems will be discussed in the class. Structure and working of batteries will be demonstrated.    

Irreversible electrode process: polarization and over voltage, types of overvoltages.  Electrolytic polarization, dissolution and deposition potential.  Determination of anode and cathode overpotential, concentration polarization, Variation of current with cell voltage, metal deposition overvoltage, Thickness of the diffusion layer, Derivation of Butler- volmer equation, Exchange current density factors affection exchange current density. Influence of current density, pH, temperature, rate of growth of deposits on over voltage.

Theories of overvoltage: Bubble formation, Combination of atoms, Ion discharge and proton transfer as slow process.*     

[1]   J. Rajaraman and J. C. Kuriakose, Kinetics and mechanism of chemical transformation,
 Macmillan Publishers India Ltd, 2000.

[2]    McQuarrie, A. Donald and John D Simon. Molecular thermodynamics. California:
University Science Books 1999.

[3]    S. Glasstone, Thermodynamics for Chemists, New Delhi:  Maurice Press, 2008.

[4]   Rajaraman and Kuriacose, Thermodynamic, East West, 1986.

[5]   M.C. Gupta, Statistical Thermodynamics, Wiley eastern Ltd., 1993.

[6]   N. D. Smith, Elementary Statistical Thermodynamics, N.Y: Plenum press, 1982.

[7]   L.K. Nash, Elements of Classical and Statistical Thermodynamics, Addison-Wiley, 1970.

[8]   Samuel Glasstone. Textbook of Physical Chemistry. 2^nd ed. New Delhi: MacMillan Ltd., 1991.

[9]   Samuel Glasstone, An Introduction to Electrochemistry, New Delhi:  East-West edition, 1942. Reprint BiblioBazaar, 2011.

[2]   O. M. Bockris, John Reddy and K. N. Amulya, Modern Electrochemisty 2A, Fundamentals of  Electrodics, Springer, New Delhi, 2006.

[3]   O. M. Bockris, John Reddy and K. N. Amulya, Modern Electrochemistry 2B: Electrodics in Chemistry, Springer, New Delhi, 2006.

[4]   O. M. Bockris, John Reddy and K. N. Amulya, Modern Electrochemistry, Springer, New Delhi, 2006.

[5]   Gordon M Barrow, Physical chemistry Tata Mcgraw-hill, New Delhi, special Indian edition 2007.

This introductory course on spectroscopy intends to make the students get an idea on topics like symmetry and group theory, microwave, infrared, Raman and electronic spectroscopy.  This course intended to serve as a resource to enhance student learning in the field of theoretical spectroscopy, which helps them in their higher education and research career.

Symmetry elements and symmetry operations, Definition of group, point groups, cyclic groups, subgroups, symmetry Classes, Simple theorems in group theory. Schöenflies notation, Representations of groups by matrices, Reducible and irreducible representations, Great Orthogonality theorem (without proof) and its applications, derivation of the orthonormalization conditions.       Mulliken symbols for irreducible representations. Construction of character tables and their uses (representation for the Cn, Cnv, Cnh, Dnh etc groups to be worked out). Reducible representation to irreducible representation using reduction formula. Direct products, Applications of group theory to quantum mechanics and spectroscopy.Chemical applications of Group theory for molecular vibrations. Molecular vibration of symmetrical AB₂ (bent) molecule, Symmetry of normal modes of ethylene.

 Interaction of electromagnetic radiation with matter, Rotation of molecules, types of rotors, diatomic rigid rotor- rotational energy expression energy level diagram, spectrum of a rigid diatomic rotor, selection rules, expression for the energies of spectral lines, consideration of intensities, effect of isotopic substitution, centrifugal distortion and the spectrum of a non-rigid rotor. Rotational spectra of polyatomic, linear and symmetric top molecules. Applications, Stark effect. Instrumentation*, Quadrupole hyperfine interaction, Detection of Interstellar molecule. 

Molecular Vibrations, Simple diatomic harmonic and anharmonic oscillators- vibrational energy expression, energy level diagram. Fundamental and hot transitions, Selection rules, Overtones and combination bands, Fermi resonance. Effect of isotopic substitution*. Vibrational wave functions and their symmetry, selection rules.

Diatomic vibrating rotor, Selection rules, vibration-rotation spectra of diatomic molecules. P, Q and R branchesVibrations of polyatomic molecules: Normal coordinates, vibrational energy levels. Vibration-rotation spectra of polyatomic molecules- parallel- and perpendicular vibrations of linear and symmetric top molecules. Instrumentation- FTIR and sampling techniques.

Raman Effect: Basic principles, selection rules, polarizability ellipsoids, quantum mechanical theory of the Raman effect, Classical theory of Raman Effect, explanation of Rayleigh and Raman lines based of classical theory. Vibrational Raman spectra, Mutual exclusion principle. Pure rotational Raman spectra of linear and symmetric top molecules. Advantages of Raman spectroscopy*. Structural determination from Raman and IR spectroscopy-AB₂ and AB₃ molecules. Instrumentation and sampling procedure.  

Born- Oppenheimer approximation, Electronic transition, vibrational coarse structure, rotational fine structure of electronic transition, Fortrat diagram, Franck-Condon principle, Franck-Condon factor, Dissociation and pre-dissociation. Electronic structure of diatomic molecules- basic results MO theory, potential energy diagrams, term symbols for linear molecules, selection rules, spectra of singlet and triplet molecular hydrogen. Electronic spectra of polyatomic molecules- localized MOs, Decay of excited states, Jablonski diagram, fluorescence and phosphorescence spectroscopy and non-radiative decay.

Course enrichment activities

A demonstration of UV-Vis, IR, and Raman Spectrometers will be organised for the students in batches.

[1]  F. A. Cotton, Chemical Applications of Group Theory, Wiley Eastern, 1990.

[2]  D. S. Schonland, Molecular Symmetry,Van Nostrand 1965.

[3] C. N. Banwell and E.M. McCash, Fundamentals of Molecular Spectroscopy, TMH Edition, 2012.

[4] G. M. Barrow, Introduction to Molecular Spectroscopy. McGraw Hill, Int. Students Edition. 1988.

[5]  J. D. Graybeal, Molecular Spectroscopy, McGraw Hill Int. Student Edition, 1990.

[6]  M. S. Gopinathan and V Ramakrishnan, Group Theory in Chemistry, Vishal Publishing Co,  2011.

[2]  K. Veera Reddy, Symmetry and Molecular Spectroscopy, New Age International Publishers, 2012.

[3]  J. M. Hollas, Modern Spectroscopy, Wiley India Pvt. Ltd, 2010.  

[4]  D. N. Sathyanarayana, Vibrational Spectroscopy: Theory and Applications, New Age International Publishers, 2004.

Assessment Pattern for Theory

This practical course on inorganic chemistry intends to provide the students scientific skills in quantitative techniques.

1.      Gravimetric determination of Fe in an iron ore as Fe₂O₃.

2.      Volumetric/redox and gravimetric determination of the following mixtures:                   

(a) Copper and nickel (b) Copper and iron (C) Copper and Zinc (d) Nickel and zinc (e) Iron and chromium.

3.      Analysis of alloys: (a) German silver (b) Steel (c) Solder.

4.      Analysis of ores: (a) Haematite, (b) Dolomite, (c) Pyrolusite

5.      Flame photometric determination of Na/K in cement and soil samples.

6.      Estimation of copper/iron by spectrophotometric method.

7.      Determination of ionic nature of coordination complex by ion exchange chromatography and conductivity methods.

8.     Determination of ground state dipole moment of various compounds.

[1]        F. A. Cotton, G. Wilkinson, Advanced inorganic chemistry, 6^th ed., John Wiley & sons,
2009.

[2]        J. E. Huheey, E. A. Keiter and R. L. Keiter, Inorganic Chemistry – Principles of Structure and Reactivity, 4th edition, Pearson Education Asia Pvt. Ltd., 2000.

[3]        J. Bassett., G. H. Jeffery J. Mendham, and R. C. Denny, Vogel’s text book of quatitative chemical analysis. 5^th edition, Longman Scientific and Technical, 1999.

[4]        G. Marr and B.W. Rockett, Practical inorganic chemistry, Von Nostrand Reinhold: 1972.

[1]        K. F. Purcell and J. C. Kotz, Inorganic Chemistry, Indian reprint, Cengage Learnining India Pvt Ltd, 2010.

[2]        G. L. Miessler and D. A. Tarr, Inorganic Chemistry, 4^th ed., Prentice Hall, 2010.

[3]     D. N. Sathyanarayana, Electronic absorption spectroscopy and related techniques,
Universities Press: 2001.

[4]        William M Portfield, Inorganic Chemistry-An Unified Approach (Indian Reprint) Academic
Press, 2005.

Course description

This practical course on organic chemistry intends to provide the students scientific skills in the analysis of organic mixtures and separation of organic compounds. 

Separation of a binary mixture of bifunctional organic compounds and identification of the    separated components by systematic qualitative organic analysis.

● Separation of p-rosaniline and methyl red by column chromatography.

● Separation of amino acids by column chromatography.

● Separation of carbohydrates by thin layer chromatography. 

[1]B. B. Dey, M. V. Sitaraman and T. R. Govindachari, Laboratory manual of organic chemistry, New Delhi: Allied Publishers, 1996.

[2]A. I. Vogel, Text book of practical organic chemistry, 1996.

[3]V. K. Ahluwalia and R. Aggarwal, Comprehensive practical organic chemistry:Preparations and Quantitative analysis, University press, 2004.

[2]A. I. Vogel, Text book of practical organic chemistry, 1996.

[3]V. K. Ahluwalia and R. Aggarwal, Comprehensive practical organic chemistry:Preparations and Quantitative analysis, University press, 2004.

Course description

This practical course on physical chemistry intends to provide the students with scientific skills in conductometric and potentiometric experiments.

1.       Determination of the solubility of sparingly soluble salt.

2.       Titration of mixture of strong and weak acids against strong base.

3.       Titration of mixture of strong acid, weak acid and salt (copper sulfate) against strong base.

4.       Titration of weak acid against weak base.

5.       Precipitation titration: Lithium sulfate against barium chloride.

6.       Dissociation constant of weak electrolyte (weak base – NH₄OH; weak acid – CH₃COOH).

7.       Verification of Onsager’s equation – determination of λ₀ of an electrolyte.

8.       Determine the solubility of lead iodide in presence of varying concentration of salt KNO₃

9.       Determination of strength of acetic acid and commercial vinegar by Conductometric method.

10.    Determination of single electrode potential of Cu²⁺ / Cu and Zn²⁺ / Zn and testing the validity of Nernst equation.

11.    Determination of pH of buffers by using quinhydrone electrode and comparison of the pH values obtained with glass electrode.

12.    Potentiometric titration of ferrous ammonium sulfate against potassium dichromate – calculation of formal redox potential of Fe³⁺ / Fe²⁺. 

13.    Potentiometric titration of potassium iodide against potassium permanganate. 

14.    Titration of silver nitrate against potassium chloride.

15.    Determination of EMF of a concentration cell and calculation of solubility product of AgCl.

16.    Titration of weak acid against a strong base using quinhydrone electrode and calculation of pK_a value of the weak acid.

17.    Titration of a mixture of HCI and CH₃COOH potentiometrically and determination of the composition of the mixture.

18.    Estimation of acetyl salicylic acid in the given aspirin tablet by titrating against 0.1N alcoholic KOH potentiometrically.

19.    Estimation of Cu by electrogravimetric method.