UG Chemistry Syllabus 2025

SEMESTER - I

CHEMISTRY MAJOR-1

PART ‘A’

THEORY COURSE CONTENTS:

UNIT-I: Atomic Structure: (10 Lectures)

Bohr’s theory, its limitations and atomic spectrum of hydrogen atom. Wave mechanics: de’ Broglie equation, Heisenberg’s Uncertainty Principle and its significance, Schrödinger’s wave equation, significance of ψ and ψ2. Quantum numbers and their significance. Normalized and orthogonal wave functions. Sign of wave functions. Radial and angular wave functions for hydrogen atom. Radial and angular distribution curves. Shapes of s, p, d and f orbitals. Contour boundary and probability diagrams. Pauli’s Exclusion Principle, Hund’s rule of maximum multiplicity, Aufbau’s principle and its limitations, Variation of orbital energy with atomic number.

UNIT-II: Periodicity of Elements: (10 Lectures)

s, p, d, f block elements, the long form of periodic table. Detailed discussion of the following properties of the elements, with reference to s and p-block. Effective nuclear charge, shielding or screening effect, Slater rules, variation of effective nuclear charge in periodic table. , Atomic radii (Vander Waals) ,Ionic and crystal radii, Covalent radii (octahedral and tetrahedral) Ionization enthalpy, Successive ionization enthalpies and factors affecting ionization energy. Applications of ionization enthalpy, Electron gain enthalpy, trends of electron gain enthalpy. Electronegativity, Pauling, Mullikan, Allred Rachow scales, electronegativity and bond order, partial charge, hybridization, group electronegativity, Sanderson electron density ratio.

UNIT-III: Chemical Bonding: (22 Lectures)

a) Ionic bond: General characteristics, types of ions, size effects, radius ratio rule and its limitations. Packing of ions in crystals. Born-Lande equation with derivation, Madelung constant, expression for lattice energy, Kapustinskii equation. Born-Haber cycle and its application, Solvation energy.

b) Covalent bond: Lewis structure, Valence Shell Electron Pair Repulsion Theory (VSEPR), Shapes of simple molecules and ions containing lone and bond pairs of electrons multiple bonding, sigma and pi-bond approach, Valence Bond theory, (Heitler-London approach). Hybridization containing s, p and s, p, d atomic orbitals, shapes of hybrid

orbitals, Bents rule, Resonance and resonance energy, Molecular orbital theory, Molecular orbital diagrams of simple homonuclear and heteronuclear diatomic molecules: N₂, O₂, C₂, B₂, F₂, CO, NO, and their ions. Covalent character in ionic compounds; polarization, polarizing power and polarizability. Fajan rules. Ionic character in covalent compounds: Bond moment and dipole moment, ionic character from dipole moment and electronegativities.

c) Metallic Bond: Qualitative idea of free electron model, Semiconductors, Insulators.

d) Weak Chemical Forces: Vander Waals, ion-dipole, dipole-dipole, induced dipole dipole-induced dipole interactions, hydrogen bond, effects of hydrogen bonding on melting and boiling points, solubility, dissolution

UNIT-IV: Oxidation-Reduction and Volumetric Analysis: (3 Lectures)

Redox equations, Balancing by Ion electron method & Oxidation number method. Disproportionation Reaction. Principles involved in volumetric analysis(Acidimetry, Permagentometry, Dichromatometry).

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

1. Acid-Base Titrations

a. Estimation of oxalic acid present in the supplied sample.

b. Estimation of sodium hydroxide present in given sample.

c. Estimation of amount of acetic acid in vinegar solution.

d. Estimation of carbonate and hydroxide present together in mixture.

e. Estimation of carbonate and bicarbonate present together in a mixture.

f. Estimation of free alkali present in different soaps/detergents.

2. Oxidation-Reduction Titrimetry

a.Estimation of Fe(II) in supplied solution using standardized KMnO4 solution.

b.Estimation of oxalic acid using standardized KMnO4 solution.

c.Estimation of percentage of Fe(II) in Iron fillings with standard K2Cr2O7

SEMESTER - II

CHEMISTRY MAJOR-2

PART ‘A’

THEORY COURSE CONTENTS:

UNIT-I: Gaseous state: (18 Lectures)

Kinetic Molecular model of a gas: Postulates and derivation of the kinetic gas equation, collision frequency, collision diameter, mean free path and viscosity of gases, their temperature and pressure dependence, relation between mean free path and coefficient of viscosity, calculation of σ from η, variation of viscosity with temperature and pressure. Maxwell distribution and its use in evaluating molecular velocities (average, root mean square and most probable) and average kinetic energy, law of equipartition of energy, degrees of freedom and molecular basis of heat capacities.

Behaviour of real gases: Deviation from ideal gas behaviour, Compressibility factor, Z , Variation of compressibility factor with pressure at constant temperature (plot of Z vs P) for different gases ( H₂, CO₂, CH₄ and NH₃), Causes of deviation from ideal behaviour. van der Waals equation of state, its derivation and application in explaining real gas behaviour. Boyle’s temperature. Isotherms of real gases and their comparison with van der Waals isotherms, continuity of states, critical state, critical and van der Waals constants, law of corresponding states.

UNIT-II: Liquid State: (5 Lectures)

Structure and physical properties of liquids; vapour pressure, surface tension, viscosity, and their dependence on temperature, Effect of addition of various solutes on surface tension, cleansing action of detergents. Structure of water.

UNIT-III: Solid State: (7 Lectures)

Nature of the solid state, law of constancy of interfacial angles, law of rational indices, Miller indices, elementary ideas of symmetry, symmetry elements and symmetry operations, qualitative idea of point and space groups, seven crystal systems and fourteen Bravais lattices, X-ray diffraction, Bragg's law, a simple account of rotating crystal method and powder pattern method. Analysis of powder diffraction patterns of NaCl, CsCl and KCl. Various types of defects in crystals, Glasses and liquid crystals.

UNIT-IV: Ionic Equilibrium: (15 Lectures)

Concept of Equilibrium. Le Charliers’ principle and its applications. Relationships between K_p, K_cand K_x for reactions involving ideal gases (Kinetic derivation). Equilibrium between ideal gases and a pure condensed phase.

Strong, moderate and weak electrolytes, degree of ionization, factors affecting degree of ionization, ionization constant and ionic product of water. Ionization of weak acids and bases, pH scale, common ion effect, dissociation constants of mono-, di- and tri-protic acids. Salt hydrolysis, hydrolysis constants, degree of hydrolysis and pH of different salt solutions. Buffer solutions, Henderson equation, buffer capacity, buffer range, buffer action, applications of buffers in analytical chemistry, Solubility and solubility product.

Qualitative treatment of acid–base titration curves (calculation of pH at various stages). Theories of indicators, selection of indicators and their limitations. Multistage equilibria in polyelectrolytes.

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

Surface Tension Measurements.

1. Determine the surface tension by (i) Drop number (ii) Drop weight method.

2. Study the variation of surface tension of detergent solutions with concentration.

3. Study the effect of the addition of solutes on the surface tension of water at room temperature and explain the observations in terms of molecular interactions:

4. (i)sugar (ii) ethanol (iii) sodium chloride

5. Study the variation of surface tension with different concentration of sodium chloride solutions.

Viscosity measurements using Ostwald’s viscometer.

1. Determination of viscosity of aqueous solution of (i) polymer (ii) ethanol and (iii) sugar at room temperature.

2. Viscosity of sucrose solution with the concentration of solute.

Ionic Equilibrium and pH measurements

1. Preparation of buffer solutions of different pH

i. Sodium acetate-acetic acid

ii. Ammonium chloride-ammonium hydroxide

2. pH metric titration of (i) strong acid vs. strong base, (ii) weak acid vs. strong base.

3. Determination of dissociation constant of a weak acid.

4. Measurement of pH of different solutions like aerated drinks, fruit juices, shampoos and soaps (use dilute solutions of soaps and shampoos to prevent damage to the glass electrode) using pH-meter.

SEMESTER - III

CHEMISTRY MAJOR-3

PART ‘A’

THEORY COURSE CONTENTS:

UNIT-I: Basics of Organic Chemistry: (13 Lectures)

Organic Compounds: Classification and Nomenclature, Hybridization, shape of molecules, influence of hybridization on bond properties. Electron Displacement Effects: inductive, electromeric, resonance and mesomeric effects. Tautomerism, hyperconjugation and their applications. Dipole moment, Organic acids and bases, their relative strength. Homolytic and Heterolytic fission with suitable examples. Curly arrow rules, formal charges, Electrophiles and Nucleophiles, Nucleophilicity and basicity, Types, shape and relative stability of reaction intermediates (Carbocations, Carbanions, Free radicals and Carbenes). Aromaticity in benzenoid and non-benzenoid compounds, alternant and non-alternant hydrocarbons, Huckel’s rule, annulenes, antiaromaticity, Y-aromaticity, homo-aromaticity, bonding in fullerenes, crown ether complexes and cryptands, inclusion compounds, cyclodextrins, catenanes and rotaxanes. Organic reactions and their mechanism: Addition, Elimination and Substitution reactions.

UNIT-II: Stereochemistry: (9 Lectures)

Concept of asymmetry, Fischer Projection, Newmann and Sawhorse projection formulae and their interconversions; Geometrical isomerism: cis–trans and, syn-anti isomerism E/Z notations with C.I.P rules. Optical Isomerism: Optical Activity, Specific Rotation, Chirality/Asymmetry, Enantiomers, Molecules with two or more chiral-centres, Distereoisomers, meso structures, Racemic mixtures, Relative and absolute configuration: D/L and R/S designations. Threo & Erythreo isomers.

Cycloalkanes and stability, Baeyer strain theory, Conformation analysis, Energy diagrams of cyclohexane: Chair, Boat and Twist boat forms.

UNIT-III: Chemistry of Aliphatic Hydrocarbons: (12 Lectures)

a) Alkanes: Formation of alkanes, Wurtz Reaction, Corey House Synthesis, Kolbe’s Synthesis, Free radical substitutions: Halogenation - relative reactivity and selectivity. Lengthening and shortening of carbon chain in alkanes.

b) Alkenes and Alkynes: Formation of alkenes and alkynes by elimination reactions, Mechanism of E1, E2, E1cb reactions. Saytzeff and Hofmann eliminations. Reactions of alkenes: Electrophilic additions their mechanisms (Markownikoff/ Anti Markownikoff addition), mechanism of oxymercuration demercuration, hydroboration-oxidation, ozonolysis, reduction (catalytic and chemical), syn and anti-hydroxylation (oxidation), reaction with NBS, 1, 2- and 1, 4- addition reactions in conjugated dienes and, Diels Alder reaction; Allylic and benzylic bromination and mechanism, e.g. propene, 1-butene, toluene, ethyl benzene. Reactions of alkynes: Acidity, Electrophilic and Nucleophilic additions. Relative reactivity of alkenes and alkynes.,

UNIT-IV: Chemistry of Aromatic Hydrocarbons: (11 Lectures)

a) Aromatic Hydrocarbons: Aromaticity: Aromatic character of arenes, cyclic carbocations/carbanions and heterocyclic compounds with suitable examples. Electrophilic aromatic substitution: halogenation, nitration, sulphonation and Friedel-Craft's alkylation/acylation with their mechanism. Directing effects of substituent groups.

b) Polynuclear Hydrocarbons: Reactions of naphthalene and anthracene: Structure, Preparation and structure elucidation and important derivatives of naphthalene and anthracene.

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

I. Common Procedures

1. Heating/Boiling with and without condenser, Filtration techniques, Separation techniques, Crystallization techniques.

2. Purification of organic compounds (say naphthalene & others) by crystallization using the following solvents:

a. Water b. Alcohol c. Alcohol-Water d. Acetone e. Hexane f. Toluene

3. Determination of the melting and boiling points

a. Determination of the melting points of above compounds and unknown organic compounds

b. (Kjeldahl method and electrically heated melting point apparatus)

c. Effect of impurities on the melting point – mixed melting point of two unknown organic compounds

d.Determination of boiling point of liquid compounds. (Boiling point lower than and more than 100 °C by distillation and capillary method).

SEMESTER - IV

CHEMISTRY MAJOR-4

PART ‘A’

THEORY COURSE CONTENTS:

UNIT-I: Acids, Bases and Salts: (12 Lectures)

Arrhenius concept of acid and base and its limitations, Bronsted-Lowry concept of acid and base and its limitations, Solvated proton, Relative strengths of acids and bases, Levelling effect and levelling solvents, Types of acid-base reactions, Salts and their classifications, Lewis concept of acid and base and its limitations, Classification of Lewis acids and bases into hard and soft categories, Hard and Soft Acid Base (HSAB) principle and its implications, Theoretical basis of hardness and softness, Electronegativity and hardness and softness, Acid -base strength and hardness and softness, Lux-Flood concept of acid and bases.

UNIT-II: General Principle of Metallurgy: (8 Lectures)

Standard Electrode Potential and its application to inorganic reactions. Occurrence of metals based on standard electrode potentials. Latimer diagrams and Frost diagrams and their applications, Ellingham diagrams for reduction of metal oxides using carbon or carbon monoxide as reducing agent. Electrolytic Reduction, Hydrometallurgy. Methods of purification of metals: Electrolytic Kroll process, Parting process, van Arkel- de Boer process and Mond’s process, Zone refining.

UNIT-III: Chemistry of s and p Block Elements: (10 Lectures)

Inert pair effect, Relative stability of different oxidation states, diagonal relationship and anomalous behaviour of first member of each group. Allotropy and catenation. Complex formation tendency of s and p block elements. Hydrides and their classification ionic, covalent and interstitial. Basic beryllium acetate and nitrate.

Structure, bonding, preparation, properties and uses. Boric acid and borates, boron nitrides, borohydrides (diborane) carboranes and graphitic compounds, silanes, Oxides and oxoacids of nitrogen, Phosphorus and chlorine. Per-oxo acids of Sulphur inter-halogen compounds, poly- halide ions, pseudo-halogens, properties of halogens.

UNIT-IV: Noble Gases: (9 Lectures) & Inorganic Polymers: (6 Lectures)

Occurrence and uses, rationalization of inertness of noble gases, Clathrates; preparation and properties of XeF₂, XeF₄ and XeF₆, Bonding in noble gas compounds (Valence bond and MO treatment for XeF2), Shape of noble gas compounds (VSEPR theory).

Types of inorganic polymers, comparison with organic polymers, synthesis, structural aspects and applications of silicones and siloxanes. Borazines, silicates and phosphazenes, and polysulphates.

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

I. Gravimetric Analysis:

a. Estimation of Nickel (II) using Dimethylglyoxime (DMG).

b. Estimation of Barium as BaSO₄

c. Estimation of Magnesium in pyrolusite

d. Estimation of Iron in Fe₂O₃ by precipitating iron as Fe(OH)₃.

II.Inorganic Preparations:

i. Tetraamminecopper (II) sulphate, [Cu(NH₃)₄]SO₄.H₂O

ii. Cis and trans K[Cr(C₂O₄)₂. (H₂O)₂] Potassiumdioxalatodiaquachromate (III)

iii. Tetraamminecarbonatocobalt (III) ion

iv. Potassium tris (oxalate) ferrate(III)

CHEMISTRY MAJOR-5

PART ‘A’

THEORY COURSE CONTENTS:

UNIT-I: Philosophical Foundations of Chemistry in IKS (9 Hours)

Historical development of Indian chemistry: Pre-Vedic to Medieval periods, Philosophical schools and atomic theories: Vaisheshika, Samkhya, Nyaya, Concept of atoms (Anu), molecules (Dvyanuka), motion, and transformation, Space, time, matter, and causality in Vaisheshika-Sutras, Classification of Dravyas and Gunas with chemical parallels

UNIT-II: Rasashastra and Alchemical Traditions (10 Hours)

Origin and goals of Rasashastra: health, longevity, immortality, Classification of Rasa, Dhatu, Mula, Uparasas, and Bhasmas, Processes of Shodhana, Marana, Bhasmikarana: scientific analysis, Case Study: Swarna Bhasma – preparation, modern chemical analysis, pharmacological evaluation, Mercury in Indian alchemy: symbolic vs. chemical understanding

UNIT-III: Advanced Indian Metallurgy and Material Chemistry (8 Hours)

Design of traditional furnaces (Kosthi, Musha): thermochemical insights, Metallurgical excellence in Zinc (Zawar), Iron (Delhi Pillar), Wootz Steel, Alloy technology: Panchaloha, Bidriware, Bronze, Ancient welding, quenching, and surface treatment techniques, Materials characterization using modern instrumentation (AAS, SEM, XRD) for ancient artifacts

UNIT-IV:

a) Ayurvedic Chemistry and Pharmaceutical Science (9 Hours)

Rasa-Aushadhi and Rasa preparation: compound classification, process optimization, Bhaishajya Kalpana: formulation science and solubility, bioavailability, Role of minerals, salts, and metals in disease management: chemistry behind Bhasma, Nano-scale interpretations of Bhasmas – TEM/XRD evidence, Ethics and toxicity management in ancient pharmacopeia

b) Applied Chemistry in IKS and Sustainability (9 Hours)

Chemistry of natural dyes and mordants: indigo, turmeric, madder, katha

Chemistry in ritual and lifestyle: incense, cosmetics, perfumery, alkali ash, Food processing, fermentation, and preservation: curd, pickles, kanji, Traditional water purification, eco-remediation (ash, sand, moringa), Integrating IKS in green chemistry and sustainable development goals

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

List of Suggeted Experiments:

1. Preparation and characterization of Swarna/Mukta Bhasma (simulated) – Nanoparticles, Thermolysis

2. Extraction of Indigo dye and study of redox behavior – Natural dyes, oxidation-reduction

3. Shodhana of sulfur using ghee/milk – safety, yield, and purity testing – Elemental purification

4. Analysis of pH and microbial activity of Kanji – Fermentation and biochemistry

5. Surface analysis of copper before and after “Shodhana” using SEM/XRD (demo/report) – Metallurgy, material science

6. Herbal alkali preparation from plant ash and soap synthesis – Acid-base chemistry

7. Green distillation method using earthen apparatus (miniature) – Thermal distillation

8. Reproduction of ancient black iron oxide ink – Inorganic pigment chemistry

9. TLC analysis of Ayurvedic extracts (Triphala, Ashwagandha) – Phytochemical screening

10. Study of corrosion resistance of traditional alloys – Electrochemistry

CHEMISTRY MAJOR-6

PART ‘A’

THEORY COURSE CONTENTS:

UNIT-I: Introduction & First Law of thermodynamics: (10 Lectures)

Intensive and extensive properties, thermodynamic variables, state and path functions, isolated, closed and open systems, reversible, irreversible and cyclic processes. Zeroth law of thermodynamics. First law of Thermodynamics: Concept of heat, q, work, w, internal energy, enthalpy, relation between heat capacities, calculations of q, w, U and H for reversible and irreversible processes. Expression for work done under free expansion of gases for isothermal and adiabatic conditions.

UNIT-II: Thermochemistry: (10 Lectures)

Heat of reactions: standard states, enthalpy of formation of molecules and ions. Enthalpy of reactions (combustion, neutralization, solution etc) and its applications, calculation of bond energy, bond dissociation energy and resonance energy from thermochemical data, effect of temperature (Kirchhoff's equations) and pressure on enthalpy of reactions.

UNIT-III: Second & Third Law of Thermodynamics: (8 Lectures)

Concept of entropy, thermodynamic scale of temperature, statement of the second law of thermodynamics, molecular and statistical interpretation of entropy. Calculation of entropy change for reversible and irreversible processes.

Third Law: Statement of third law, concept of residual entropy, calculation of absolute entropy of molecules.

UNIT-IV:

a) Free Energy Functions: (8 Lectures)

Gibbs and Helmholtz energy, variation of S, G, A with T, V, P, Free energy change and spontaneity. Relation between Joule-Thomson coefficient and other thermodynamic parameters, inversion temperature, Gibbs Helmholtz equation, Maxwell relations, thermodynamic equations of state.

b) Partial molar quantities: (9 Lectures)

Partial molar quantities, dependence of thermodynamic parameters on composition, Gibbs- Duhem equation, chemical potential of ideal mixtures, change in thermodynamic functions in mixing of ideal gases.

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

1. Checking the calibration of the thermometer

2. Purification of organic compounds by crystallization using the following solvents: a. Water b. Alcohol c. Alcohol-Water

3. Determination of the melting points of above compounds and unknown organic compounds (Kjeldahl method and electrically heated melting point apparatus)

4. Determination of boiling point of liquid compounds. (boiling point lower than and more than 100 °C by distillation and capillary method)

5. Thermochemistry

(a) Determination of heat capacity of a calorimeter for different volumes using change of enthalpy data of a known system (method of back calculation of heat capacity of calorimeter from known enthalpy of solution or enthalpy of neutralization).

(b) Determination of heat capacity of the calorimeter and enthalpy of neutralization of hydrochloric acid with sodium hydroxide.

(d) Determination of heat capacity of the calorimeter and integral enthalpy (endothermic and exothermic) solution of salts.

(e) Determination of basicity/proticity of a polyprotic acid by the thermochemical method in terms of the changes of temperatures observed in the graph of temperature versus time for different additions of a base. Also calculate the enthalpy of neutralization of the first step.

(f) Determination of enthalpy of hydration of copper sulphate.

(g) Study of the solubility of benzoic acid in water and determination of H. Any other experiment carried out in the class.

CHEMISTRY MAJOR-7

PART ‘A’

THEORY COURSE CONTENTS:

UNIT-I: Chemistry of Halogenated Hydrocarbons: (10 Lectures)

Alkyl halides: Methods of preparation, nucleophilic substitution reactions – SN¹, SN² and SNi mechanisms with stereochemical aspects and effect of solvent etc. Nucleophilic substitution vs. elimination.

Aryl halides: Preparation from diazonium salts. nucleophilic aromatic substitution, SNAr, Benzyne mechanism. Relative reactivity of alkyl, allyl/benzyl, vinyl and aryl halides towards nucleophilic substitution reactions.

Organometallic compounds of Mg and Li and their use in synthesis.

UNIT-II: Alcohols, Phenols, Ethers and Epoxides: (10 Lectures)

Alcohols: preparation, properties and relative reactivity of 1°, 2°, 3°- alcohols, Bouveault-Blanc Reduction, Preparation and properties of glycols and glycerol. Pinacol-Pinacolone rearrangement.

Phenols: Preparation and properties, Acidic nature and factors affecting it, Ring substitution reactions, Reimer–Tiemann and Kolbe's–Schmidt Reactions, Fries and Claisen rearrangements with mechanism.

Ethers and Epoxides: Preparation and reaction with acids. Reaction of epoxides with alcohols, ammonia derivatives and LiAlH4

UNIT-III: Carbonyl Compounds: (11 Lectures)

Structure, reactivity and preparation of Carbonyl compounds. Nucleophilic additions, Nucleophilic addition elimination reactions with ammonia derivatives with mechanism. Aldol and Benzoin condensation, Knoevenagel condensation, Claisen-Schmidt, Perkin, Cannizzaro and Wittig reaction, Beckmann and Benzil- Benzilic acid rearrangements, haloform reaction and Baeyer Villiger oxidation, α-substitution reactions, oxidations and reductions (Clemmensen, Wolff- Kishner, LiAlH4, NaBH4, MPV, PDC and PGC), Addition reactions of unsaturated carbonyl compounds: Michael addition.

UNIT-IV:

a) Carboxylic Acids and their Derivatives: (10 Lectures)

Preparation, physical properties and reactions of monocarboxylic acids, Typical reactions of dicarboxylic acids,hydroxy acids and unsaturated acids: succinic/phthalic, lactic, malic, tartaric, citric, maleic and fumaric acids,Preparation and reactions of acid chlorides, anhydrides, esters and amides, Comparative study of nucleophilic substitution at acyl group, Mechanism of acidic and alkaline hydrolysis of esters, Claisen condensation, Dieckmann and Reformatsky reactions, Hofmann bromamide degradation and Curtius rearrangement.

b) Chemistry of Active methylene groups: (4 Lectures)

Active methylene compounds: Keto-enol tautomerism. Preparation and synthetic applications of diethyl malonate and ethyl acetoacetate.

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

Suggested List of Experiments:-

1.Detection of extra elements in organic compounds.

2.Functional group test for nitro, amine and amide groups

3.Functional group tests for alcohols, phenols, carbonyl and carboxylic acid group.

4.Qualitative analysis of unknown organic compounds containing simple functional groups (alcohols, carboxylic acids, phenols and carbonyl compounds)

Organic preparations:

a. Oxidation of Benzaldehyde to benzoic acid.

b. Hydrolysis of amides and esters.

c. Preparation of Semi carbazone derivatives of the following compounds: acetone, ethyl methyl ketone, cyclohexanone, benzaldehyde.

d. Preparation of methyl orange.

SEMESTER - V

CHEMISTRY MAJOR-8

PART ‘A’

THEORY COURSE CONTENTS:

UNIT-I: d-Block Elements: Transition Elements: (15 Lectures)

General group trends with special reference to electronic configuration, colour, variable valency, magnetic and catalytic properties, and ability to form complexes. Stability of various oxidation states and e.m.f. (Latimer & Bsworth diagrams). Difference between the first, second and third transition series. Oxidation states displayed by Cr, Fe, Co, Ni and Co. A study of the following compounds (including preparation and important properties); Peroxo compounds of chromium, K₂Cr₂O₇, KMnO₄, K₄[Fe(CN)₆], sodium nitroprusside, [Co(NH₃)₆]Cl₃, Na₃[Co(NO₂)₆].

UNIT-II: f-Block elements: Lanthanoids and Actinides: (10 Lectures)

Electronic configuration, oxidation states, color, spectra and magnetic behavior, lanthanide contraction, separation of lanthanides (ion-exchange method only).

UNIT-III: Coordination Chemistry: (25 Lectures)

Werner’s theory, EAN rule, IUPAC nomenclature of coordination compounds, isomerism in coordination compounds. Stereochemistry of complexes with the coordination number 4 and 6, Chelate effect.valence bond theory (inner and outer orbital complexes), Crystal field theory, d-orbital splitting, weak and strong fields, pairing energies, factors affecting the magnitude of (Δ). Octahedral vs. tetrahedral coordination, tetragonal distortions from octahedral geometry Jahn-Teller theorem, square planar complexes, d orbital splitting in trigonal bipyramidal, square pyramidal and cubic ligand field environments, CFSE, Variation of lattice energies, enthalpies of hydration and crystal radii variations in halides of first and second row transition metal series, Qualitative aspect of Ligand field theory, MO diagrams of representative coronation complexes

UNIT-IV: Non-Aqueous Solvents:(10 Lectures)

Solvents and their role during chemical reactions, Classification of solvents on the basis of various criteria, General properties of ionizing solvents, Different types of chemical reactions taking place in a solvent, Different types of chemical reactions taking place in liquid NH₃ and their comparison to those taking place in aqueous medium , liquid SO₂ as a solvent, liquid HF as a solvent, liquid N₂O₄ as a solvent and glacial acetic acid as a solvent.

SUGGESTED READINGS:

1. Purcell, K.F & Kotz, J.C. Inorganic Chemistry W.B. Saunders Co, 1977. Huheey, J.E., Inorganic Chemistry, Prentice Hall, 1993.

2. Lippard, S.J. & Berg, J.M. Principles of Bioinorganic Chemistry Panima Publishing Company 1994.

3. Cotton, F.A. & Wilkinson, G, Advanced Inorganic Chemistry Wiley-VCH, 1999

4. Basolo, F, and Pearson, R.C. Mechanisms of Inorganic Chemistry, John Wiley & Sons, NY, 1967. Greenwood, N.N. & Earnshaw A. Chemistry of the Elements, Butterworth-Heinemann, 1997.

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

1 Experiment = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

Analysis of Salt Mixture

Qualitative semi micro analysis of mixtures containing 3 anions and 3 cations. Emphasis should be given to the understanding of the chemistry of different reactions. The following radicals are suggested: CO₃ ^{2 -}, NO₂ ^-, S^2-, SO₃ ^2-,S₂O₃ ^2
-, CH₃COO^-, F^-, Cl^-, Br^-, I^-, NO₃ ^-, BO₃ ^3-,C₂O₄^2-, PO₄^3-, NH₄⁺, K⁺, Pb²⁺, Cu²⁺, Cd²⁺, Bi³⁺, Sn²⁺, Sb³⁺, Fe³⁺, Al³⁺, Cr³⁺,Zn²⁺, Mn²⁺, Co²⁺, Ni²⁺, Ba²⁺,Sr²⁺, Ca²⁺, Mg^{2+ .}Mixtures should preferably contain one interfering anion, or insoluble component (BaSO₄, SrSO₄, PbSO₄, CaF₂ or Al₂O₃) or combination of anions e.g. CO₃^2-and SO₃^2-, NO₂^- and NO₃^-, Cl^- and Br^-, Cl^- and I^-, Br^- and I^- , NO₃ ^- and Br- , NO₃- and I-.(Spot tests should be done whenever possible.)

CHEMISTRY MAJOR-9

PART ‘A’

THEORY COURSE CONTENTS:

UNIT-I: Dilute solutions: (10 Lectures)

Dilute solutions, lowering of vapour pressure, Raoult's and Henry's Laws and their applications. Colligative properties of solutions, abnormal colligative properties, Van’t Hoffs factor. Thermodynamic derivation using chemical potential to derive relations between the (i) relative lowering of vapour pressure, (ii) elevation of boiling point, (iii) Depression of freezing point, (iv) osmotic pressure and amount of solute. Applications in calculating molar masses of normal, dissociated and associated solutes in solution. Azeotropes.

UNIT-II: Thermodynamics of Chemical Equilibrium (12 Lectures)

Criteria of thermodynamic equilibrium, degree of advancement of reaction, chemical equilibria in ideal gases, concept of fugacity. Thermodynamic derivation of relation between Gibbs free energy of reaction and reaction quotient. Coupling of exoergic and endoergic reactions. Equilibrium constants and their quantitative dependence on temperature, pressure and concentration. Free energy of mixing and spontaneity; thermodynamic derivation of relations between the various equilibrium constants Kp, Kc and Kx.

UNIT-III: Phase Equilibria: (20 Lectures

Concept of phases, components and degrees of freedom, derivation of Gibbs Phase Rule for nonreactive and reactive systems; Clausius-Clapeyron equation and its applications to solid-liquid, liquid-vapour and solid-vapour equilibria, phase diagram for one component systems, with applications. Phase diagrams for systems of solid-liquid equilibria involving eutectic, congruent and incongruent melting points, solid solutions. Three component systems, water-chloroform- acetic acid system, triangular plots. Binary solutions: Gibbs-Duhem-Margules equation, its derivation and applications to fractional distillation of binary miscible liquids (ideal and nonideal), azeotropes, lever rule, partial miscibility of liquids, CST, miscible pairs, steam distillation.

UNIT-IV: Distribution law: (3 Lectures)

Nernst distribution law: its derivation and applications.

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

List of Experiments:-

1. Distribution of acetic acid /benzoic acid between water & cyclohexane.

2. Determination of critical solution temperature and composition of the phenol-water system and to study the effect of impurities on it.

3. Study of equilibrium of at least one of the following reactions by the distribution method:

a) I₂(aq) + I^- → I₃-(aq) b) 𝐶𝑢⁺⁺(aq) + 𝑛 𝑁𝐻₃ → [Cu(NH₃)n]²⁺

CHEMISTRY MAJOR-10

PART ‘A’

THEORY COURSE CONTENTS:

UNIT-I: Nitrogen Containing Functional Groups (15 Lectures)

Preparation and important reactions of nitro and compounds, nitriles and isonitriles Amines: Effect of substituent and solvent on basicity; Preparation and properties: Gabriel phthalimide synthesis, Carbylamine reaction, Mannich reaction, Hoffmann’s exhaustive methylation, Hofmann- elimination reaction; Distinction between 1°, 2° and 3° amines with Hinsberg reagent and nitrous acid. Diazonium salts: Preparation and synthetic applications.

UNIT-II: Sulphur Containing Compounds: (4 Lectures)

Preparation and reactions of thiols, thioethers including 1,3-dithiane and sulphonic acids

UNIT-III: Heterocyclic Compounds: (15 Lectures)

Classification and nomenclature, Structure, aromaticity in 5-numbered and 6-membered rings containing one heteroatom; Synthesis, reactions and mechanism of substitution reactions of Furan, Pyrrole (Paal-Knorr synthesis, Knorr pyrrole synthesis, Hantzsch synthesis), Thiophene, Pyridine (Hantzsch synthesis), Pyrimidine, Structure elucidation of indole, Fischer indole synthesis and Madelung synthesis), Structure elucidation of quinoline and isoquinoline, Skraup synthesis, Friedlander’s synthesis, Knorr quinoline synthesis, Doebner-Miller synthesis, Bischler- Napieralski reaction, Pictet-Spengler reaction, Pomeranz-Fritsch reaction Derivatives of furan: Furfural and furoic acid.

UNIT-IV:

a) Alkaloids (6 Lectures)

Natural occurrence, General structural features, Isolation and their physiological action Hoffmann’s exhaustive methylation, Emde’s modification, Structure elucidation and synthesis of Hygrine and Nicotine. Medicinal importance of Nicotine, Hygrine, Quinine, Morphine, Cocaine, and Reserpine.

b) Terpenes (5 Lectures)

Occurrence, classification, isoprene rule; Elucidation of stucture and synthesis of Citral, Neral and α-terpineol.

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

1. Functional group test for nitro, amine and amide groups

2. Qualitative analysis of unknown organic compounds containing simple functional groups (nitro, amide, nitriles and isonitriles, amines)

3. Acetylation of one of the following compounds: amines (aniline, o-, m-, p-toluidines and o-, m-p-anisidine) and phenols (β-naphthol, vanillin, salicylic acid) by any one method: (Using conventional method and Using green chemistry approach).

4. Benzolyation of one of the amines (aniline, o-, m-, p- toluidines and o-, m-, p- anisidine) and one of the phenols (β-naphthol, resorcinol, p-cresol) by Schotten-Baumann reaction.

5. Oxidation of ethanol/ isopropanol (Iodoform reaction).

6. Bromination (any one)

a. Acetanilide by conventional methods.

b. Acetanilide using green approach (Bromate-bromide method)

7. Nitration: (any one)

a. Acetanilide/nitrobenzene by conventional method.

b. Salicylic acid by green approach (using ceric ammonium nitrate).

8. Selective reduction of meta dinitrobenzene to m-nitroaniline.

9. Reduction of p-nitrobenzaldehyde by sodium borohydride.

10. Aldol condensation with either conventional or green method.

11. Benzil-Benzilic acid rearrangement.

12. Collected solid samples may be used for recrystallization, melting point and TLC.

CHEMISTRY MAJOR-11

PART ‘A’

THEORY COURSE CONTENTS:

UNIT-I: Organometallic Compounds: (10 Lectures)

Definition and classification of organometallic compounds on the basis of bond type. Concept of hapticity of organic ligands. Metal carbonyls: 18 electron rule, electron count of mononuclear, polynuclear and substituted metal carbonyls of 3d series. General methods of preparation (direct combination, reductive carbonylation, thermal and photochemical decomposition) of mono and binuclear carbonyls of 3d series.

UNIT-II: Ferrocene & Zeise's salt: (8 Lectures)

Preparation and reactions (acetylation, alkylation, metallation, Mannich Condensation). Structure and aromaticity. Comparison of aromaticity and reactivity with that of benzene. Preparation & structure of Zeise’s salt. Evidences of synergic effect and comparison of synergic effect with that

in carbonyls.

UNIT-III: Metal Alkyls: (7 Lectures)

Important structural features of methyl lithium (tetramer) and trialkyl aluminium (dimer), concept of multicentre bonding in these compounds. Role of triethylaluminium in polymerisation of ethene (Ziegler – Natta Catalyst). Species present in ether solution of Grignard reagent and their structures, Schlenk equilibrium.

UNIT-IV:

a. Bioinorganic Chemistry: (12 Lectures)

A brief introduction to bio-inorganic chemistry. Geochemical effect on distribution of metals. Role of metal ions present in biological systems with special reference to Na⁺, K⁺ and Mg²⁺ ions: Na/K pump, Role of Mg²⁺ ions in energy production and chlorophyll. Iron and its application in bio- systems, Haemoglobin, Myoglobin, Storage and transfer of iron. Role of Ca²⁺ in blood clotting, stabilization of protein structures and structural role (bones).

b. Catalysis by Organometallic Compounds (8 Lectures)

Study of the following industrial processes and their mechanism:

1. Alkene hydrogenation (Wilkinsons Catalyst)

2. Hydroformylation (Co salts)

3. Wacker Process

4. Synthetic gasoline (Fischer Tropsch reaction)

5. Synthesis gas by metal carbonyl complexes

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

Estimations

1. Determination of temporary hardness in supplied sample of water.

2. Determination of permanent hardness in supplied sample of water.

3. Determination of total hardness of water by Complexometry.

4. Estimation of Magnesium and Calcium in a mixture by Complexometry.

5. Estimation of Copper & Zn in mixture by Gravimetry.

6. Estimation of Cu & Ni in a mixture by Gravimetry

SEMESTER - VI

CHEMISTRY MAJOR-12

PART ‘A’

THEORY COURSE CONTENTS:

UNIT-I: Chemical Kinetics – Basic Concepts (12 Lectures)

Introduction to reaction kinetics: Rate of reaction, rate constant, molecularity and order of a reaction.Integrated rate laws for zero, first, second and third order reactions (with derivation and examples).Pseudo-first order reactions. Determination of order and rate constant using experimental methods: graphical, half-life and initial rate methods. Temperature dependence of reaction rates: Arrhenius equation, activation energy, and concept of transition state theory. Effect of pressure and ionic strength on reaction rates

UNIT-II: Complex Reactions and Reaction Mechanisms (10 Lectures)

Opposing (reversible), consecutive, and parallel reactions. Steady-state approximation and its application in reaction mechanisms. Chain reactions: Hydrogen-Bromine reaction and explosions. Unimolecular reactions (Lind’s theory). Fast reactions: Relaxation methods and stopped-flow technique. Enzyme catalysis: Michaelis–Menten mechanism and Lineweaver–Burk plot.

UNIT-III: Catalysis (10 Lectures)

Introduction and types of catalysis: Homogeneous and heterogeneous.Acid-base catalysis and general vs specific acid/base catalysis.Enzyme catalysis: characteristics and mechanisms.Industrial catalysis: Hydrogenation, polymerization, Haber’s process, etc.Auto-catalysis and inhibition of catalysis.Mechanisms of surface catalysis (Langmuir-Hinshelwood model).

UNIT-IV: Surface Chemistry and Adsorption (13 Lectures)

Adsorption: Physical vs chemical adsorption; Factors affecting adsorption.Freundlich and Langmuir adsorption isotherms (derivations and limitations).BET (Brunauer–Emmett–Teller) isotherm and surface area determination.Surface tension and surface energy.Colloids: Classification, preparation, properties (Tyndall effect, electrophoresis, coagulation), applications.Micelles and critical micelle concentration (CMC).

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

A. Chemical Kinetics Experiments

1. To study the kinetics of acid hydrolysis of methyl acetate using HCl as a catalyst.

2. To study the rate of reaction between potassium iodate and sodium sulphite using starch as indicator.

3. To study the kinetics of the reaction between acetone and iodine in acid medium.

B. Catalysis Experiments

5. To study the catalytic decomposition of hydrogen peroxide using MnO₂ or KI as catalyst.

6. To study the autocatalytic reaction of potassium permanganate and oxalic acid.

C. Surface Chemistry Experiments

7. To study adsorption of acetic acid on activated charcoal and verify Freundlich isotherm.

8. To study the adsorption of oxalic acid on activated charcoal and plot Langmuir isotherm.

9. To prepare a colloidal solution (e.g., arsenious sulphide or ferric hydroxide) and study its properties.

CHEMISTRY MAJOR-13

PART ‘A’

THEORY COURSE CONTENTS:

UNIT-I: Amino acids, Peptides and Proteins: (20 Lectures)

Amino acids: Classification of Amino Acids, α-Amino acids- synthesis, ionic properties and reactions, Zwitter-ion structure, pKa -values, isoelectric point and electrophoresis.

Study of peptides: Determination of primary structure by end group analysis, Synthesis of peptides by using N-protecting, C-protecting and C-activating groups, Merrifield solid phase peptide synthesis.

Proteins: General characteristics, Classification of proteins, Overview of Primary, Secondary, Tertiary and Quaternary structure of proteins.

UNIT-II: Enzymes: (10 Lectures)

General characteristics, Mechanism of enzyme action, factors affecting enzyme action, Coenzymes and cofactors and their role in biological reactions, Specificity of enzyme action (including stereospecificity).

Enzyme inhibitors and their importance, phenomenon of inhibition (competitive and non- competitive inhibition including allosteric inhibition).

UNIT-III: Lipids (5 Lectures)

Introduction to lipids, classification. Oils and fats: Common fatty acids present in oils and fats, Omega fatty acids, Trans fats, Hydrogenation, Saponification value, Iodine number. Biological importance of triglycerides, phospholipids, glycolipids, and steroids (cholesterol)

UNIT-IV:

a) Nucleic Acids (10 Lectures)

Definition and general characteristics, Components of nucleic acids, nucleosides and nucleotides, Structure of nucleic acids, The chemical basis of heredity- Replication of DNA, Synthesis of adenine, guanine, cytosine, uracil and thymine.

b) Pharmaceutical Compounds-Structure and Importance:(10 Lectures)

Definition, Classification, Structure and Therapeutic use of

Antipyretics: Paracetamol (with synthesis)

Analgesics: Ibuprofen (with synthesis)

Antimalarials: Chloroquine (with synthesis)

Antibiotics: Chloramphenicol (with synthesis)

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

List of Practical Experiments

(Minimum 8 experiments to be performed)

1. Preparation of α-amino acid derivative (e.g., N-acetyl glycine or benzoyl glycine).

2. Separation of amino acids by paper chromatography.

3. Determination of isoelectric point of glycine.

4. Colour reactions of amino acids and proteins (Ninhydrin test, Biuret test, Xanthoproteic test).

5. Estimation of proteins by Biuret or Lowry method.

6. Effect of pH and temperature on enzyme activity (e.g., action of salivary amylase on starch).

7. Study of enzyme inhibition (e.g., competitive inhibition using urease or sucrase).

8. Saponification of lipids and determination of saponification value.

9. Determination of iodine value of an oil/fat sample.

10. Tests for unsaturation and identification of lipid classes (qualitative).

11. Qualitative detection of functional groups in pharmaceutical compounds (e.g., phenol, amine, carboxylic acid in paracetamol, aspirin, ibuprofen).

CHEMISTRY MAJOR-14

PART ‘A’

THEORY COURSE CONTENTS:

UNIT-I: Reaction Mechanism of Transition Metal Complexes (14 Lectures)

Energy profile of a reaction, reactivity of metal complexes, inert and labile complexes, kinetic application of valence bond and crystal field theories, kinetics of octahedral substitution, acid hydrolysis, factors affecting acid hydrolysis, base hydrolysis, conjugate base mechanism, direct and indirect evidences in favour of conjugate mechanism, anation reactions, reactions without metal ligand bond cleavage. Substitution reactions in square planar complexes, the trans effect, mechanism of the substitution reaction. Redox reactions, electron transfer reactions, mechanism of one electron transfer reactions, outer- sphere type reactions, cross reactions and Marcus-Hush theory, inner sphere type reactions

UNIT-II: Metal-Ligand Bonding in complexes (7 Lectures)

Limitation of crystal field theory, molecular orbital theory, octahedral, tetrahedral and square planar complexes, π-bonding and molecular orbital theory.

UNIT-III: Electronic Spectra and Magnetic Properties of Transition Metal Complexes (14 Lectures)

Spectroscopic ground states, Term symbol, Selection rule, correlation, Orgel and Tanabe-Sugano diagrams for transition metal complexes (d1- d9 states), calculations of dq and β parameters, charge transfer spectra, spectroscopic method of assignment of absolute configuration in optically active metal chelates and their stereochemical information, anomalous magnetic moments, magnetic exchange coupling and spin crossover.

UNIT-IV:

a) Metal Clusters (5 Lectures)

b) Metal 𝝅-Complexes (12 Lectures)

Metal carbonyls, structure and bonding, vibrational spectra of metal carbonyls for bonding and structural elucidation, important reactions of metal carbonyls; preparation, bonding, structure and important reactions of transition metal nitrosyl, dinitrogen and dioxygen complexes: tertiary phosphine as ligand.

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

List of Experiments (Minimum 6 to be performed)

1. Study of acid hydrolysis of cis- and trans-[Co(en)₂Cl₂]+ complexes.

2. Determination of relative reactivity and trans-effect.

3. Kinetic study of substitution of [Co(NH₃)₅Cl]²⁺ by thiocyanate ion.

4. Base hydrolysis of [Co(NH₃)₅Cl]²⁺.

5. Study of oxidation of [Fe(CN)₆]⁴⁻ by cerium(IV) sulfate using iodometry.

6. Electronic Spectrum of d⁹ Complex (e.g., [Cu(H₂O)₆]²⁺)

7. Determination of λ_maxand calculation of 10Dq.

8. Assignment of bands and correlation with Tanabe-Sugano diagram.

9. Comparison of [Fe(H₂O)₆]²⁺ and [Fe(CN)₆]³⁻ spectra.

10. Synthesis of [Ni(NH₃)₆]²⁺

11. Determination of geometry (octahedral/tetrahedral) from spectral data.

CHEMISTRY MAJOR-15

PART ‘A’

THEORY COURSE CONTENTS:

UNIT-I: Conductance: (16 Lectures)

Arrhenius theory of electrolytic dissociation. Conductivity, equivalent and molar conductivity and their variation with dilution for weak and strong electrolytes. Molar conductivity at infinite dilution. Kohlrausch law of independent migration of ions. Debye-Huckel-Onsager equation, Wien effect, Debye-Falkenhagen effect, Walden's rules. Ionic velocities, mobilities and their determinations, transference numbers and their relation to ionic mobilities, determination of transference numbers using Hittorf and Moving Boundary methods. Applications of conductance measurement: (i) degree of dissociation of weak electrolytes, (ii) ionic product of water (iii) solubility and solubility product of sparingly soluble salts (iv) hydrolysis constants of salts etc.

UNIT-II: Electrochemistry: (12 Lectures)

Quantitative aspects of Faraday’s law. Applications of electrolysis in metallurgy and industry. Half-cell potential, Chemical cells, reversible and irreversible cells with examples. Electromotive force of a cell and its measurement, Nernst equation, Standard electrode (reduction) potential and its application of different kind of half-cells. Electrified interfaces, overpotential, Electrocatalysis- influence of various parameters. Hydrogen electrode.

UNIT-III: Application of EMF measurements: (12 Lectures)

Application of EMF measurements in determining (i) free energy, enthalpy and entropy of a cell reaction, (ii) equilibrium constants, and (iii) pH values, using hydrogen, quinone-hydroquinone, glass and SbO/Sb₂O₃ electrodes. Concentration cells with and without transference, liquid junction potential, determination of activity coefficients and transference numbers. Qualitative discussion of potentiometric titrations (acid-base, redox, precipitation).

UNIT-IV: Electrical & Magnetic Properties of Atoms and Molecules: (5 Lectures)

Basic ideas of electrostatics, Electrostatics of dielectric media, Clausius-Mosotti equation, Lorenz-Laurentz equation, Dipole moment and molecular polarizabilities and their measurements. Diamagnetism, paramagnetism, magnetic susceptibility and its measurement, molecular interpretation.

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

List of Experiments

1. Conductometric titration of a strong acid vs strong base.

2. Conductometric titration of a weak acid vs strong base.

3. Determination of the solubility and solubility product of a sparingly soluble salt (e.g., BaSO₄ or AgCl).

4. Determination of the equivalent conductance at infinite dilution for a weak electrolyte using Kohlrausch’s Law.

5. Determination of the degree of dissociation and dissociation constant of a weak acid by conductance measurements.

6. Determination of transference number of ions using the Hittorf method.

7. Potentiometric titration of a strong acid with a strong base using a glass electrode.

8. Potentiometric redox titration (e.g., KmnO₄ vs FeSO₄).

9. Determination of pH using a quinhydrone or glass electrode.

10. Determination of cell EMF and calculation of ΔG, ΔH, and ΔS.

SEMESTER - VII

CHEMISTRY MAJOR-16

PART ‘A’

THEORY COURSE CONTENTS:

UNIT-I: Organic Spectroscopy:(22 Lectures)

General principles and introduction to absorption and emission spectroscopy.

a) UV-VIS Spectroscopy: Basic principle, Absorption laws, Types of electronic transitions, 𝜆_𝑚𝑎𝑥, Chromophores and Auxochromes, Bathochromic and Hypsochromic shifts, Intensity of absorption bands- Hyperchromic and Hypochromic shifts, Effect of solvent on electronic spectra, Woodward-Fieser rules and their applications in the calculation of 𝜆_𝑚𝑎𝑥 of

a) α, β-unsaturated aldehydes, ketones, carboxylic acids and esters

b) Conjugated dienes with or without extended conjugation.

c) Distinction between cis- and trans- isomers

b) IR Spectroscopy: Basic principle, Molecular vibrations, Fingerprint region and its significance, Group frequency region and its importance, Infrared absorption frequencies of organic molecules with functional groups containing O, N and S (such as ketones, aldehydes, esters, amides, acids, anhydrides, lactones, lactams, thiols, thioethers, etc.); Effect of H-bonding, resonance/conjugation and ring-size on IR absorptions.

c)NMR Spectroscopy: Basic principle, Reference in proton magnetic resonance spectroscopy and Chemical shift, Chemical shifts of H atoms bonded to carbon atoms (aliphatic, olefinic aldehydic and aromatic) and other nuclei (alcohols, phenols, enols, carboxylic acids, amines, amides, mercapto), Spin-spin coupling, Chemical exchange, effect of deuteration.

d) Mass Spectrometry: Basics of fragmentations in organic compounds. Discussion of molecular ion peak, base peak and metastable ions, McLafferty rearrangement. Nitrogen rule, Index of hydrogen deficiency. Application of fragmentation in characterization of organic compounds.

e) Electronic Spectroscopy:

Franck-Condon principle, electronic transitions, singlet and triplet states, fluorescence and phosphorescence.

f) Atomic Absorption spectroscopy: Theory and application (with some example).

g) Problem Solving: Problems on structure elucidation of organic compounds based on

spectral data. Applications of IR, UV, NMR and Mass spectra for identification of simple organic molecules. Solving problems for the elucidation of molecular structure with the help of mixed spectral data.

UNIT-II: Carbohydrate: (14 Lectures)

Occurrence,Definition, classification and their biological importance.

a) Monosaccharides: Constitution and absolute configuration of glucose and fructose, epimers and anomers, mutarotation, determination of ring size of glucose and fructose, Haworth projections and conformational structures, Interconversions of aldoses and ketoses, Killiani- Fischer synthesis and Ruff degradation.

b) Disaccharides: Structure elucidation of maltose, lactose and sucrose.

c)Polysaccharides: Elementary treatment of starch, cellulose and glycogen excluding their structure elucidation.

UNIT-III: Dyes, Food Colours:(9 Lectures)

Classification, Colour and constitution, Mordant and Vat Dyes, Chemistry of dyeing,

Synthesis and applications of

a) Azo dyes: Methyl Orange and Congo Red (mechanism of Diazo Coupling)

b) Triphenyl Methane Dyes: Malachite Green, Rosaniline and Crystal Violet

c)Phthalein Dyes: Phenolphthalein and Fluorescein,

d)Natural dyes –Structure elucidation and synthesis of Alizarin and Indigotin,

Natural and synthetic food colours with examples, Natural food colours carotenoids, chlorophyll, anthocyanin, betanin and turmeric, Preparation of Natural food colours (Red Pink, Green, Orange, yellow, Blue, Purle, Brown,Tan and Black. . Synthesis and study of Tartrazine, Quinoline yellow, Sunset yellow, Amarnanth, Erythrosine, Indigo carmine.

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

Suggested List of Experiments: -

1. Interpretation of UV, IR, NMR, and Mass Spectra of known organic compounds.

2. Structure elucidation exercises using mixed spectral data (UV, IR, NMR, MS).

3. Identification of functional groups using IR spectra.

4. Simulation software (if available): Use of tools like Chem Sketch or online NMR prediction software for interpreting spectra.

5. Detection of reducing and non-reducing sugars (Fehling’s and Benedict’s tests).

6. Osazone formation for identification of glucose and fructose.

7. Mutarotation of glucose using polarimeter (if available).

8. Hydrolysis of disaccharides (e.g., sucrose) and identification of products by TLC or qualitative test.

9. Synthesis of methyl orange (azo dye) and observation of pH-dependent color change.

10. Synthesis of phenolphthalein (phthalein dye) and study of pH effect.

11. Preparation of natural dyes from turmeric, spinach (chlorophyll), beetroot (betalains), and hibiscus (anthocyanins).

12. Paper chromatography/TLC of natural food colors.

13. Synthesis of Tartrazine or Congo Red (demonstration or lab scale).

14. Dyeing of cotton/wool fabrics using synthesized dyes (mordant and vat method).

SEMESTER - VII

CHEMISTRY MAJOR-17

PART ‘A’

THEORY COURSE CONTENTS:

UNIT-I: Industrial Gases and Inorganic Chemicals (14 Lectures)

Industrial Gases: Large scale production, uses, storage and hazards in handling of the following gases: oxygen, nitrogen, argon, neon, helium,hydrogen, acetylene, carbon monoxide, chlorine, fluorine, sulphur dioxide and phosgene.

Inorganic Chemicals: Manufacture, application, analysis and hazards inhandling the following chemicals: hydrochloric acid, nitric acid, sulphuricacid, caustic soda, common salt, borax, bleaching powder, sodiumthiosulphate, hydrogen peroxide, potash alum, chrome alum, potassiumdichromate and potassium permanganate.

UNIT-II: Environment and its segments (30 Lectures)

Ecosystems. Biogeochemical cycles of carbon, nitrogen and sulphur.

Air Pollution: Major regions of atmosphere. Chemical and photochemical reactions in atmosphere. Air pollutants: types, sources, particle size and chemical nature; Photochemical smog: its constituents and photochemistry. Environmental effects of ozone, Major sources of air pollution.Pollution by SO2 , CO2, CO, NOx, H2S and other foul smelling gases.Methods of estimation of CO, NOx, SOx and control procedures.

Effects of air pollution on living organisms and vegetation. Greenhouse effect and Global warming, Ozone depletion by oxides of nitrogen,

chlorofluorocarbons and Halogens, removal of sulphur from coal. Control of particulates.

Water Pollution: Hydrological cycle, water resources, aquatic ecosystems, Sources and nature of water pollutants, Techniques for measuring water pollution, Impacts of water pollution on hydrological and ecosystems.Water purification methods.

Effluent treatment plants (primary, secondary and tertiary treatment). Industrial effluents from the following industries and their treatment: electroplating, textile, tannery, dairy, petroleum and petrochemicals, agro, fertilizer, etc. Sludge disposal.

UNIT-III: Energy & Environment (10 Lectures)

Sources of energy: Coal, petrol and natural gas. Nuclear Fusion / Fission,

Solar energy, Hydrogen, geothermal, Tidal and Hydel, etc. Nuclear Pollution:

Disposal of nuclear waste, nuclear disaster and its management.

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

Suggested List of Experiments: -

1. Estimation of available chlorine in bleaching powder (iodometric method).

2. Estimation of strength of hydrogen peroxide by redox titration using KMnO₄.

3. Preparation and standardization of hydrochloric acid and determination of purity.

4. Analysis of borax for boron content using Mannitol-acid titration method.

5. Quantitative estimation of sulphate ion in an industrial sample (gravimetric or turbidimetric method).

6. Determination of percentage purity of sodium thiosulphate by iodometric titration.

7. Determination of free acidity in industrial alum sample (potash or chrome alum).

8. Study of safe handling techniques and storage requirements for chlorine and phosgene (demonstration/discussion-based activity).

9. Measurement of pH, conductivity and total dissolved solids (TDS) of water samples (tap, industrial effluent, pond).

10. Estimation of dissolved oxygen (DO) in water using Winkler’s method.

11. Estimation of Chemical Oxygen Demand (COD) of an effluent sample.

12. Estimation of Biological Oxygen Demand (BOD) of a water sample over 5-day incubation.

13. Estimation of sulphur dioxide (SO₂) from air using West-Gaeke method.

14. Colorimetric estimation of nitrate/nitrite (Nox) in a water or air sample.

15.Analysis of heavy metals (Pb²⁺/Cd²⁺) in wastewater using spot test or colorimetric kit (demonstration-based).

CHEMISTRY MAJOR-18

PART ‘A’

THEORY COURSE CONTENTS:

UNIT-I: Quantum Chemistry (Hours: 22)

Postulates of quantum mechanics, quantum mechanical operators and commutation rules, Schrödinger equation and its application to free particle and particle in a box rigorous treatment), quantization of energy levels, zero-point energy and Heisenberg Uncertainty principle; wave functions, probability distribution functions, nodal properties, Extension to two and three- dimensional boxes, separation of variables, degeneracy.

Qualitative treatment of simple harmonic oscillator model of vibrational motion: Setting up of Schrödinger equation and discussion of solution and wave functions. Vibrational energy of diatomic molecules and zero-point energy.

Angular momentum. Rigid rotator model of rotation of diatomic molecule. Schrödinger equation in Cartesian and spherical polar coordinates (derivation not required). Separation of variables. Spherical harmonics. Discussion of solution (Qualitative).

UNIT-II: Hydrogen Atom (08 Hours)

Qualitative treatment of hydrogen atom and hydrogen-like ions: setting up of Schrödinger equation in spherical polar coordinates, radial part and quantization of energy (only final energy expression). Average and most probable distances of electron from nucleus. Zeeman effect, Introduction of spin quantum number and magnetic spin quantum number Setting up of Schrödinger equation for many electron atoms (He, Li), Indistinguishability of electrons and Pauli exclusion principle, Need for approximation methods. Statement of variation theorem and application to simple systems (particle-in-a-box, harmonic oscillator, hydrogen atom).

UNIT-III: Covalent bonding (15 Hours)

Setting up of Schrödinger equation, Born-Openheimer approximation, LCAO-MO treatment of H²⁺ and its qualitative extension to H₂, Valence bond (VB) treatment of H₂, Comparison of LCAO-MO and VB wave functions of H₂ and their refinements, Qualitative description of LCAO-MO of homonuclear and heteronuclear diatomic molecules-HF and LiH.

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

One Activity/ Experiment = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

Suggested List of Activity/Experiments:-

1. Plot the radial wavefunctions and probability distribution for H atom's 1s, 2s, 2p orbital using software like EXCEL.

2. Using a software such as ArgusLab, Avogadro, PyMOL, AutoDock etc to plot HOMO, LUMO and ESP maps of various molecules.

3. Draw probability plots for a particle in a 1-dimensional box for different values of quantum number n - commenting on the number of points of zero probability and then correlate them with the correspondence principle.

4. Plot the electron density contour maps of sigma molecular orbitals for diatomic homonuclear molecules.

5. Plotting of the wave function and probability curve for simple harmonic m

CHEMISTRY MAJOR-19

THEORY COURSE CONTENTS:

UNIT-I: Molecular Spectroscopy:(35 Lectures)

Quantization of molecular energies, Boltzmann distribution, Interaction of electromagnetic radiation with molecules and various types of spectra, Born- Oppenheimer approximation.

a) Rotation spectroscopy: The rotation of molecules and classification of molecules on the basis of principal moments of inertia, Rotational spectra of rigid diatomic molecules, Selection rules, Intensities of spectral lines, Determination of bond lengths of diatomic and linear triatomic molecules, Effect of isotopic substitution on rotational spectra, Centrifugal distortion and rotational spectra of non-rigid rotor.

b) Vibrational spectroscopy: Classical equation of vibration, computation of force constant, amplitude of diatomic molecular vibrations, anharmonicity, Morse potential, dissociation energies, fundamental frequencies, overtones, hot bands, degrees of freedom for polyatomic molecules, modes of vibration, concept of group frequencies, Breakdown of Born-Oppenheimer approximation – interaction between rotations and vibrations of molecules, Vibration-rotation spectroscopy, diatomic vibrating rotator, P, Q, R branches.

c) Raman spectroscopy: Introduction, Raman effect, Classical and quantum theories of Raman effect, Rotational Raman spectra, Effect of nuclear spin on rotational Raman spectra, Vibrational Raman spectra, Stokes & anti-Stokes lines and their intensity difference, Rule of mutual exclusion.

d) Electronic Spectroscopy: Franck-Condon principle, Electronic transitions, Selection rules for electronic transitions, Electronic spectra of diatomic molecules, Vibrational coarse structure of electronic spectra, Rotational coarse structure of electronic spectra, Singlet & triplet states of molecules and their characteristics, Fluorescence and phosphorescence, Dissociation and predissociation, Electronic spectra of polyatomic molecules.

UNIT-II: Photochemistry:(10 Lectures)

Laws of photochemistry, Quantum yield, Jablonski diagrams, Franck-Condon principle, Law of photochemical equivalence, Quantum efficiency, Low and high quantum efficiency, Kinetics of photochemical reactions (H₂ + Br₂ = HBr, 2HI = H₂ + I₂), energy transfer in photochemical reactions (photosensitization and quenching), fluorescence, phosphorescence, chemiluminescence, Discussion of Electronic spectra and photochemistry (Lambert-Beer law and its applications).

SUGGESTED READINGS:

1. Laideler K. J. and Meiser J. M. Physical Chemistry Third Edition (International)1999.

2. Levine I. N., Physical Chemistry, Fourth Edition), McGraw-Hill (International), 1995.

3. McQuarrie D. A. and Simon J. D. Physical Chemistry- A Molecular Approach, University Science Books, 1998.

4. Chandra, A. K. Introductory Quantum Chemistry Tata McGraw-Hill (2001).

5. House, J. E. Fundamentals of Quantum Chemistry 2nd Ed. Elsevier: USA (2004).

6. Laideler K. J. and Meiser J. M. Physical Chemistry Third Edition (International)1999.

7. Rohatgi-Mukherjee K. K. Fundamentals of Photochemistry, New age (revised second edition).

8. Banwell, C. N. & McCash, E. M. Fundamentals of Molecular Spectroscopy 4th Ed. Tata McGraw-Hill: New Delhi (2006).

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

Suggested List of Experiments:-

1. Verify Lambert-Beer’s law and determine the concentration of

2. CuSO₄/KMnO₄/K₂Cr₂O₇ in a solution of unknown concentration

3. Determine the concentrations of KMnO₄ and K₂Cr₂O₇ in a mixture.

4. Interpretation of IR spectra of organic/inorganic compounds.

5. Identification of functional groups via group frequencies.

6. Analysis of rotational spectra of diatomic molecules.

7. Calculation of bond length and moment of inertia from given spectra.

8. Photoreduction of potassium ferrioxalate and comparison with actinometer.

9. Determination of quantum yield of a photochemical reaction.

10. Study of kinetics of H₂ + Br₂ → HBr or decomposition of HI under UV light (via simulation or data).

SEMESTER - VIII

COURSE: MAJOR – 20(MJ-20) TOTAL CREDITS: THEORY-03, PRACTICAL-01

PAPER NAME: DISSERTATION TEACHING HOURS: THEORY-45, PRACTICAL-30

EVALUATION
	External Exam	Internal Exam	Practical
Full Marks	60	15	25
Full Marks	60	(10 Written + 5 Attendance/Overall Class Performance)	25
Duration of Exam	3 Hours	1 Hour	6 Hours
Pass Marks	30 Marks		10 marks

Course Objectives:

Enhance students' communication skills through active participation in seminars and group discussions. Prepare them for academic and professional environments where effective communication and teamwork are vital for success. Foster confidence, clarity, and coherence in expressing ideas, enabling students to engage meaningfully in collaborative and interdisciplinary settings.

Course Outcomes:

1. Develop effective verbal and non-verbal communication skills through seminars and group discussions.

2. Demonstrate confidence, clarity, and coherence in presenting and articulating ideas.

3. Collaborate successfully in academic and professional settings, applying interpersonal skills and teamwork strategies in diverse and interdisciplinary environments.

PART ‘A’

Course Contents:

The Head of the Department and faculty members will assign topic to the students from the course content of semester VII and VIII. Students will have to work under the supervision of a teacher of the department. Each and every student has to submit electronically typed hardbound dissertation along with the raw data on a week before the examination.

Evaluation Process: Presentation and the report submitted by the students will be evaluated by one external member and one internal member. The External Member may be a Permanent faculty members working in the postgraduate department of the university or other colleges or Retired Professor/Associate Professor/Assistant Professor of the university.

Distribution of marks:

Dissertation Report	25 marks
Presentation	50 marks
Subject Knowledge	25 marks

*********

SEMESTER - VII

COURSE: ADVANCE MAJOR – 1(AMJ-1) TOTAL CREDITS: THEORY-03, PRACTICAL-01

PAPER NAME: ANALYTICAL CHEMISTRY OGY TEACHING HOURS: THEORY-45, PRACTICAL-30

EVALUATION
	External Exam	Internal Exam	Practical
Full Marks	60	15	25
Full Marks	60	(10 Written + 5 Attendance/Overall Class Performance)	25
Duration of Exam	3 Hours	1 Hour	6 Hours
Pass Marks	30 Marks		10 marks

COURSE OUTCOMES:

1. Familiarization with fundamentals of analytical chemistry.

2. Basics of spectroscopic, thermal, electrochemical techniques

3. Learning basics of separation techniques and its applications.

4. Understanding analytical tools, statistical methods applied to analytical chemistry.

5. Understanding principle of UV-Vis spectroscopy and its applications.

6. Understanding principles of thermo-gravimetric analysis and study of thermal decomposition of materials/characterization of materials.

7. Understanding basics of electro-analytical techniques and its applications.

8. Understanding principles of separation technology and its use in advanced instrumentations.

PART ‘A’

THEORY COURSE CONTENTS:

UNIT-I: Qualitative and Quantitative Aspects of Analysis: (4 Lectures)

Tools in analytical chemistry and their applications, Sampling, evaluation of analytical data, errors, accuracy and precision, statistical test of data; F, Q and t-test, rejection of data, and confidence intervals.

UNIT-II: Spectroscopy Instrumentation (8 Lectures)

Origin of spectra, interaction of radiation with matter, fundamental laws of spectroscopy and selection rules, validity of Beer-Lambert’s law.

Vibration spectroscopy: Basic principles of instrumentation, sampling techniques. Application of IR spectroscopy for characterization through interpretation of data, Effect and importance of isotope substitution. Introduction to Raman spectra

UV-Visible Spectrometry: Basic principles of instrumentation, principles of quantitative analysis using estimation of metal ions from aqueous solution, Determination of composition of metal complexes using Job’s method of continuous variation and mole ratio method.

UNIT-III: Thermal Analysis (4 Lectures)

Theory of thermogravimetry (TG and DTG), instrumentation, estimation of Ca and Mg from their mixture.

UNIT-IV:

a) Electroanalytical Methods (5 Lectures)

Classification of electroanalytical methods, basic principle of pH metric, potentiometric and conductometric titrations. Techniques used for the determination of equivalence points. determination of pKa values.

b) Separation Techniques (12 Lectures)

Solvent extraction: Classification, principle and efficiency of the technique. Mechanism of extraction: extraction by solvation and chelation. Technique of extraction: batch, continuous and counter current extractions. Qualitative and quantitative aspects of solvent extraction: extraction of metal ions from aqueous solution, extraction of organic species from the aqueous and non-aqueous media.

Chromatography techniques: Classification, principle and efficiency of the technique. Mechanism of separation: adsorption, partition & ion exchange. Development of chromatograms: frontal, elution and displacement methods. Qualitative and quantitative aspects of chromatographic methods of analysis using LC, GLC, TLC and HPLC.

c) Sample Analysis: (12 Lectures)

Analysis of soil: Composition of soil, Concept of pH and pH measurement, Complexometric titrations, Chelation, Chelating agents, use of indicators

a. Determination of pH of soil samples.

b. Estimation of Calcium and Magnesium ions as Calcium carbonate by complexometric titration.

Analysis of water: Definition of pure water, sources responsible for contaminating water, water sampling methods, water purification methods.

a. Determination of pH, acidity and alkalinity of a water sample.

b. Determination of dissolved oxygen (DO) of a water sample.

Analysis of food products: Nutritional value of foods, idea about food processing and food preservations and adulteration.

a. Identification of adulterants in some common food items like coffee powder, asafoetida, chilli powder, turmeric powder, coriander powder and pulses, etc.

b. Analysis of preservatives and colouring matter.

Analysis of cosmetics: Major and minor constituents and their function

a. Analysis of deodorants and antiperspirants, Al, Zn, boric acid, chloride, sulphate.

b. Determination of constituents of talcum powder: Magnesium oxide, Calcium oxide, Zinc oxide and Calcium carbonate by complexometric titration.

SUGGESTED READINGS:

1 Mendham, J., A. I. Vogel’s Quantitative Chemical Analysis 6th Ed., Pearson, 2009.

2 Willard, H.H. et al.: Instrumental Methods of Analysis, 7th Ed. Wardsworth Publishing California, USA, 1988.

4 Harris, D.C.: Exploring Chemical Analysis, 9th Ed. New York, W.H. Freeman, 2016.

5 Skoog, D.A. Holler F.J. & Nieman, T.A. Principles of Instrumental Analysis, Saunder College Publications, (1998).

6 Mikes, O. Laboratory Hand Book of Chromatographic & Allied Methods, Elles Harwood

John Wiley 1979.

7 Ditts, R.V. Analytical Chemistry; Methods of separation, van Nostrand, 1974.

8 Khopkar, S. M., Basic Concepts of Analytical Chemistry, New Age (Second edition)1998

9.N. Manivasakam and S.K. Singh,Physico-Chemico Analysis of water,wastewater and industrial effluents ,Pragati Prakashan,Merrut, India.

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

Suggested List of Experiments:-

1. Determination of Ca and Mg from their salt mixtures using TG data.

(Alternate: Data interpretation from provided TG/DTG graphs if instrument unavailable.)

2. Determination of dissociation constant (pKa) of a weak acid (e.g., acetic acid).

3. Extraction of metal ion (e.g., Cu²⁺ or Fe³⁺) using suitable organic solvent and determination of distribution coefficient.

4. Separation of metal ions (Fe³⁺, Al³⁺, Cr³⁺) using paper chromatography or TLC,

5. Separation of amino acids or sugars by paper chromatography.

(Demonstration of HPLC or GLC if instruments are available.)

6. Measurement of pH of soil sample using pH meter.

7. Estimation of Ca²⁺ and Mg²⁺ as CaCO₃ by complexometric titration using EDTA

8. Determination of pH, acidity and alkalinity of water sample.

9. Estimation of dissolved oxygen (DO) using Winkler’s method.

10. Detection of adulterants in common food items (turmeric, chilli powder, coffee, pulses, etc.).

11. Identification of preservatives and synthetic colours in food items using chemical tests.

12. Estimation of aluminium, zinc, chloride, sulphate in deodorants and antiperspirants.

13. Determination of magnesium oxide, calcium oxide, zinc oxide in talcum powder using complexometric titration.

Reference Books:

Vogel’s Textbook of Quantitative Chemical Analysis, 6th Ed., G.H. Jeffery, J. Bassett, J. Mendham, R.C. Denney – Pearson Education
Quantitative Chemical Analysis – Daniel C. Harris, W.H. Freeman and Co.
Fundamentals of Analytical Chemistry – Skoog, West, Holler, Crouch – Cengage
Instrumental Methods of Analysis – H.H. Willard, L.L. Merritt, J.A. Dean, F.A. Settle – CBS Publishers
Analytical Chemistry: Principles and Techniques – John H. Kennedy, Saunders College Publishing
A Textbook of Analytical Chemistry – G.R. Chatwal, Anand – Himalaya Publishing
Practical Chemistry – O.P. Pandey, D.N. Bajpai, S. Giri – S. Chand
Laboratory Manual in Analytical Chemistry – H. Kaur – Pragati Prakashan

9. Physico-Chemico Examination of water,wastewater and industrial effluents By N. Manivasakam and S. K. Singh ,Pragati Prakashan,Meerut, India.

SEMESTER - VIII

COURSE: ADVANCE MAJOR – 2(AMJ-2) TOTAL CREDITS: THEORY-03, PRACTICAL-01

PAPER NAME: GREEN AND SUSTAINABLE CHEMISTRY TEACHING HOURS: THEORY-45, PRACTICAL-30

EVALUATION
	External Exam	Internal Exam	Practical
Full Marks	60	15	25
Full Marks	60	(10 Written + 5 Attendance/Overall Class Performance)	25
Duration of Exam	3 Hours	1 Hour	6 Hours
Pass Marks	30 Marks		10 marks

COURSE OBJECTIVES:

1. Green chemistry and its principles.

2. Green synthesis and reactions.

3. Green chemistry for sustainable solutions.

4. Understanding principles of green chemistry.

5. Understanding design of chemical reactions/chemical synthesis using green chemistry principles.

6. Atom economy and design of chemical reactions using the principle.

7. Understanding the use of green chemistry principle and processes in laboratory reactions.

COURSE OUTCOMES:

1. Use of green chemistry in designing new laboratory experiments.

2. Use of principle of atom economy and design experiments using the principle.

PART ‘A’

THEORY COURSE CONTENTS:

UNIT-I: Introduction to Green Chemistry (4 Lectures)

What is Green Chemistry? Need for Green Chemistry. Goals of Green Chemistry. Limitations/ Obstacles in the pursuit of the goals of Green Chemistry.

UNIT-II: Principles of Green Chemistry and Designing a Chemical synthesis (15 Lectures)

Twelve principles of Green Chemistry with their explanations and examples; Designing a Green Synthesis using these principles; Prevention of Waste/ byproducts; maximum incorporation of the materials used in the process into the final products (Atom Economy); prevention/ minimization of hazardous/ toxic products; designing safer chemicals – different basic approaches to do so; selection of appropriate auxiliary substances (solvents, separation agents), green solvents, solventless processes, immobilized solvents and ionic liquids.

Energy requirements for reactions - use of microwaves, ultrasonic energy; selection of starting materials; avoidance of unnecessary derivatization – careful use of blocking/protecting groups; use of catalytic reagents (wherever possible) in preference to stoichiometric reagents; designing of biodegradable products; prevention of chemical accidents; strengthening/ development of analytical techniques to prevent and minimize the generation of hazardous substances in chemical processes.

UNIT-III: Examples of Green Synthesis/ Reactions (18 Lectures)

1.Green Synthesis of the following compounds: adipic acid, catechol, BHT, methyl methacrylate, urethane, aromatic amines (4-aminodiphenylamine), benzyl bromide, acetaldehyde, disodium iminodiacetate (alternative to Strecker synthesis), citral, ibuprofen, paracetamol, furfural.

2.Microwave assisted reactions in water: Hofmann Elimination, Hydrolysis (of benzyl chloride, benzamide, n-phenyl benzamide, methylbenzoate to benzoic acid), Oxidation (of toluene, alcohols).

Microwave assisted reactions in organic solvents: Esterification, Fries rearrangement, Orthoester Claisen Rearrangement, Diels-Alder Reaction, Decarboxylation.

Microwave assisted solid state reactions: Deacetylation, Deprotection. Saponification of esters, Alkylation of reactive methylene compounds, reductions, synthesis of nitriles from aldehydes; anhydrides from dicarboxylic acid; pyrimidine and pyridine derivatives; 1,2-dihydrotriazine derivatives; benzimidazoles.

3.Ultrasound assisted reactions: Esterification, saponification, substitution reactions, Alkylations, oxidation, reduction, coupling reaction, Cannizaro reaction, Strecker synthesis, Reformatsky reaction.

4.Selective methylation of active methylene group using dimethylcarbonate: Solid-state polymerization of amorphous polymers using diphenylcarbonate; Use of “Clayan”, a nonmetallic oxidative reagent for various reactions; Free Radical Bromination; Role of Tellurium in organic syntheses; Biocatalysis in organic syntheses.

UNIT-IV: Future Trends in Green Chemistry (8 Lectures)

Oxidation reagents and catalysts; Biomimetic, multifunctional reagents; Combinatorial green chemistry; Proliferation of solventless reactions ss; Green chemistry in sustainable development.

SUGGESTED READINGS:

1. V.K. Ahluwalia & M.R. Kidwai: New Trends in Green Chemistry, Anamalaya Publishers (2005).

2. P.T. Anastas & J.K. Warner: Oxford Green Chemistry- Theory and Practical, University Press (1998).

3. A.S. Matlack: Introduction to Green Chemistry, Marcel Dekker (2001).

4. M.C. Cann & M.E. Connely: Real-World cases in Green Chemistry, American Chemical Society, Washington (2000).

5. M.A. Ryan & M. Tinnesand, Introduction to Green Chemistry, American Chemical Society, Washington (2002).

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

List of Suggested Experiments:-

1. Preparation of biodiesel from vegetable/ waste cooking oil.

2. Use of molecular model kit to stimulate the reaction to investigate how the atom economy illustrates Green Chemistry.

3. Reactions like addition, elimination, substitution and rearrangement may also be studied for the calculation of atom economy.

4. Benzoin condensation using Thiamine Hydrochloride as a catalyst (instead of cyanide).

5. Extraction of D-limonene from orange peel using liquid CO₂ prepared form dry ice.

6. Mechanochemical solvent free synthesis of azomethines

7. Solvent free, microwave assisted one pot synthesis of phthalocyanine Cu (II) complex.

8. Photoreduction of benzophenone to benzopinacol in presence of sunlight.

References:

1. Mendham, J., A. I. Vogel’s Quantitative Chemical Analysis 6^th Ed., Pearson, 2009.

2. Willard, H.H. et al.: Instrumental Methods of Analysis, 7^th Ed. Wardsworth

Publishing Company, Belmont, California, USA, 1988.

3. Christian, G.D. Analytical Chemistry, 6^th Ed. John Wiley & Sons, New York, 2004.

4. Harris, D.C. Exploring Chemical Analysis, 9^th Ed. New York, W.H. Freeman, 2016.

5. Khopkar, S.M. Basic Concepts of Analytical Chemistry. New Age International

Publisher, 2009.

6. Skoog, D.A. Holler F.J. and Nieman, T.A. Principles of Instrumental Analysis,

Cengage Learning India Edition.

7. Mikes, O. & Chalmes, R.A. Laboratory Handbook of Chromatographic & Allied

Methods, Elles Harwood Ltd. London.

8. Ditts, R.V. Analytical Chemistry: Methods of separation. Van Nostrand, New York,

9. Anastas, P.T & Warner, J.C. Green Chemistry: Theory and Practice, Oxford UniversityPress (1998).

10. Kirchoff, M. & Ryan, M.A. Greener approaches to undergraduate chemistry experiment. American Chemical Society, Washington DC (2002).

11. Ryan, M.A. Introduction to Green Chemistry, Tinnesand; (Ed), American Chemical Society, Washington DC (2002).

12. Sharma, R.K.; Sidhwani, I.T. and Chaudhari, M.K. I.K. Green Chemistry Experiment: A monograph, International Publishing ISBN 978-93-81141-55-7 (2013).

13. Cann, M.C. and Connelly, M. E. Real world cases in Green Chemistry, American Chemical Society (2008).

14. Lancaster, M. Green Chemistry: An Introductory Text RSC Publishing, Second Edition, 2010.

SEMESTER - VIII

COURSE: ADVANCE MAJOR – 3(AMJ-3) TOTAL CREDITS: THEORY-03, PRACTICAL-01

PAPER NAME: INORGANIC MATERIALS & NANOCHEMISTRY LTEACHING HOURS: THEORY-45, PRACTICAL-30

EVALUATION
	External Exam	Internal Exam	Practical
Full Marks	60	15	25
Full Marks	60	(10 Written + 5 Attendance/Overall Class Performance)	25
Duration of Exam	3 Hours	1 Hour	6 Hours
Pass Marks	30 Marks		10 marks

COURSE OBJECTIVES:

The objectives of this course are as follows:

1. To make students understand the diverse roles of inorganic materials in the industry and to give an insight into how these raw materials are converted into products used in day-to-day life.

2. To make students learn about silicates, fertilizers, surface coatings, batteries, engineering materials for mechanical construction.

3. To develop the interest of students in the frontier areas of inorganic and material chemistry.

COURSE OUTCOMES:

By studying this course, the students will be able to:

1. State the composition and applications of the different kinds of glass.

2. State the composition of cement and discuss the mechanism of setting of cement.

3. Defend the suitability of fertilizers for different kinds of crops and soil.

4. Explain the process of formulation of paints and the basic principle behind the protection offered by the surface coatings.

5. Describe the principle, working and applications of different batteries.

6. Evaluate the synthesis and properties of nano-dimensional materials, various semiconductor and superconductor oxides.

PART ‘A’

THEORY COURSE CONTENTS:

UNIT-I: Silicate Industries (6 Hours)

Glassy state and its properties, classification (silicate and non-silicate glasses). Manufacture and processing of glass. Composition and properties of the following types of glasses: Soda lime glass, lead glass, armoured glass, different types of safety glass, borosilicate glass, fluorosilicate glass, coloured glass, photosensitive glass, photochromic glass, glass wool and optical fibre.

UNIT-II: Fertilizers( 5 Hours)

Different types of fertilizers (N, P and K). Importance of fertilizers, chemistry involved in the manufacture of the following fertilizers: urea, calcium ammonium nitrate, ammonium phosphates, superphosphate of lime and potassium nitrate.

UNIT-III: Surface Coatings( 12 Hours)

Brief introduction to and classification of surface coatings, paints and pigments: formulation, composition and related properties, pigment volume concentration (PVC)and critical pigment volume concentration (CPVC), fillers, thinners, enamels and emulsifying agents. Special paints: heat retardant, fire retardant, eco-friendly paints, plastic paints, water and oil paints. Preliminary methods for surface preparation, metallic coatings (electrolytic and electroless with reference to chrome plating and nickel plating), metal spraying and anodizing.

Contemporary surface coating methods like physical vapor deposition, chemical vapor deposition, galvanising, carburizing, sherardising, boriding, nitriding and cementation.

UNIT-IV:

a) Batteries (9 Hours)

Primary and secondary batteries, characteristics of an Ideal Battery, principle, working, applications and comparison of the following batteries: Pb- acid battery, Li-metal batteries, Li- ion batteries, Li-polymer batteries, solid state electrolyte batteries, fuel cells, solar cells and polymer cells.

b) Introduction to nanoscience, nanostructure and nanotechnology: (13 Hours)

Basic idea; Overview of nanostructures and nano-materials, classification, (cluster, colloid, nanoparticles, and nanostructures, Spheroid, Wire, Rod, Tube, and Quantum Dot. Carbon nanotubes and inorganic nanowires. Calculation of percentage of surface atom and surface to volume ratio of spherical, wire, rod and disc shapes nanoparticles.

Synthesis of Nanomaterials: Brief introduction about Top-down and Bottom-up approaches & self-assembly techniques of nanoparticles synthesis, Solvothermal process, Examples of preparation of gold and silver metallic nanoparticles, self- assembled nanostructures-control of nanoarchitecture-one dimensional control. Carbon nanotubes and inorganic nanowires.

SUGGESTED READINGS:

1. 1West, A. R. (2014),Solid State Chemistry and Its Application, Wiley

2. Smart, L. E.; Moore, E. A. (2012),Solid State Chemistry An Introduction, CRC Press Taylor & Francis.

3. Atkins,P.W.; Overton,T.L.; Rourke, J.P.;Weller,M.T.;Armstrong, F.A.(2010),Shriver and Atkins Inorganic Chemistry, W. H. Freeman and Company.

4. Kent, J. A. (ed) (1997), Riegel’s Handbook of Industrial Chemistry, CBS Publishers, New Delhi.

5. Poole Jr.; Charles P.; Owens, Frank J.(2003), Introduction to Nanotechnology, John Wiley and Sons.

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

List of suggested Experiments:-

1. Detection of constituents of Ammonium Sulphate fertilizer (Ammonium and Sulphate ions)

by qualitative analysis and determine its free acidity.

2. Detection of constituents of CAN fertilizer (Calcium, Ammonium and Nitrate ions) fertilizer and estimation of Calcium content.

3. Detection of constituents of Superphosphate fertilizer (Calcium and Phosphate ions) and estimation of phosphoric acid content.

4. Analysis of (Cu, Ni) in alloy or synthetic samples (methods involving Gravimetry and Spectrophotometry).

5. Analysis of (Cu, Zn) in alloy or synthetic samples (Multiple methods involving Iodometry, and Potentiometry).

6. Synthesis of pure ZnO and Cu doped ZnO nanoparticles.

7. Synthesis of silver nanoparticles by green and chemical approach methods and its characterization using UV-visible spectrophotometer

Reference Books:-

1. Svehla, G.(1996),Vogel’s Qualitative Inorganic Analysis, Prentice Hall.

2. Banewicz, J. J.; Kenner, C.T. Determination of Calcium and Magnesium in Limestones and Dolomites, Anal. Chem., 1952, 24 (7), 1186–1187.

3. Ghorbani, H. R.; Mehr, F.P.; Pazoki, H.; Rahmani B. M. Synthesis of ZnO Nanoparticles by Precipitation Method. Orient J Chem 2015;31(2).

4. Orbaek, W.; McHale, M.M.; Barron, A.R. Synthesis and characterization of silver nanoparticles for an undergraduate laboratory, J. Chem. Educ. 2015, 92, 339−344.

SEMESTER - VII

COURSE: RESEARCH METHODOLOGY – 1(RM-1) TOTAL CREDITS: THEORY-04

PAPER NAME: RESEARCH METHODOLOGY IN CHEMISTRY TEACHING HOURS: THEORY-60

EVALUATION
	External Exam	Internal Exam
Full Marks	75	25
		(20 Written + 5 Attendance/Overall Class Performance)
Duration of Exam	3 Hours	1 Hour
Pass Marks	40 Marks

COURSE OBJECTIVES:

1. To introduce students to the fundamentals of scientific research, especially within the field of chemistry.

2. To develop skills in formulating a research question, reviewing literature, and planning experiments.

3. To train students in writing research proposals and selecting appropriate methodologies.

4. To familiarize students with techniques for data analysis, referencing, ethical research practices, and scientific communication.

COURSE OUTCOMES:

1. Understand the purpose and structure of a research proposal.

2. Conduct an effective literature review using online and offline databases.

3. Formulate a clear hypothesis or research question.

4. Design experiments using proper methodology, instrumentation, and controls.

5. Apply fundamental techniques for data collection and interpretation in chemistry.

6. Demonstrate awareness of ethical issues in research and academic integrity.

7. Draft and present a comprehensive research proposal with proper formatting and citations.

PART ‘A’

THEORY COURSE CONTENTS:

UNIT-I: Fundamentals of Research in Chemistry (9 Hours)

Definition, Scope, and Importance of Research, Types of Research: Basic, Applied, Interdisciplinary, Research in Chemical Sciences: Areas and Trends, Identification and Formulation of a Research Problem, Setting Objectives and Hypothesis Formulation

UNIT-II: Literature Review and Information Sources (6 Hours)

Purpose and Process of Literature Review, Layout of a Research Paper, Journals in chemistry, Impact factor of journals, Use of Encyclopaedias, Research Guides, Handbook etc., Academic databases for concerned discipline. Use of tools / techniques for Research: methods to search required information effectively, Reference Management Software like Zotero/Mendeley, Software for paper formatting like LaTeX/MS Office, When and where to publish? Ethical issues related to publishing, Plagiarism and Self-Plagiarism. software for detection of Plagiarism.

UNIT-III: Research Planning (12 Hours)

Research Design and Planning, Sampling Techniques and Control Experiments, Variables, Parameters, and Standardization, Use of Laboratory Notebooks and Research Logs, Safety Measures and Risk Assessment in Chemical Research.

UNIT-IV:

a) Reporting and Thesis writing: 7 Lectures

Structure and components of scientific reports - Types of report - Technical reports and thesis - Significance - Different steps in the preparation - Layout, Structure and Language of typical reports - Illustrations and tables - Bibliography, referencing and footnotes - Oral presentation - Planning - Preparation - Practice - Making presentation - Use of visual aids - Importance of effective communication

b) Techniques and Tools in Chemical Research (9 Hours)

Instrumentation Overview: Spectroscopy (UV-Vis, IR, NMR), Chromatography (GC, HPLC), Electrochemical Methods, Computational Tools in Chemistry: Molecular Modeling, ChemDraw, Origin, Excel, Data Collection and Analysis: Accuracy, Precision, Errors, Interpretation and Presentation of Results

c) Writing a Research Proposal and Scientific Communication (9 Hours)

Structure and Format of a Research Proposal (Title, Abstract, Introduction, Objectives,Methodology, Budget, Timeline, References),Drafting and Revising a Proposal, Writing Abstracts and Research Papers, Preparing Posters and Presentations for Conferences, Ethics in Research and Academic Writing

SUGGESTED READINGS:

1. Kothari, C.R. – Research Methodology: Methods and Techniques, New Age International, 2nd Ed.

2. Leedy, P.D. & Ormrod, J.E. – Practical Research: Planning and Design, Pearson Education.

3. Day, R.A. & Gastel, B. – How to Write and Publish a Scientific Paper, Cambridge University Press.

4. Turabian, K.L. – A Manual for Writers of Research Papers, Theses, and Dissertations, University of Chicago Press.

5. ACS Style Guide – Effective Communication of Scientific Information, American Chemical Society.

6. Ranjit Kumar – Research Methodology: A Step-by-Step Guide for Beginners, SAGE Publications.

Bates, B. – Writing with Precision: How to Write So That You Cannot Possibly Be Misunderstood, Penguin.

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

Course Objectives:

· To expose students to practical aspects of scientific research in chemistry.

· To enable students to design and conduct small-scale experiments or survey-based investigations.

· To develop skills in scientific presentation, data handling, and reporting.

· To encourage field-based and lab-based observational learning in research contexts.

Course Outcomes:

· Demonstrate capability in planning and executing small experimental designs or field surveys.

· Interpret and analyze experimental or observational data with scientific reasoning.

· Present research findings in oral/poster format and submit written reports.

· Identify and comply with ethical practices in chemical research.

Components of Practical / Field / Presentation Work (30 Hours):

1. Designing a Mini Research Project: Framing objectives, hypothesis, and methodology based on any chemistry topic.

2. Field Visit / Laboratory Exposure: Visit to chemical research labs/industries/institutes or demonstration of instrumental techniques.

3. Experimental Planning and Data Collection: Performing basic chemistry experiments relevant to the research theme .

4. Data Analysis and Interpretation: Tabulation, graphical analysis, and drawing inferences

5. Preparation of Research Proposal / Report: Structuring a written proposal or short report

6. Presentation and Viva-Voce: Oral/poster presentation of the project followed by viva .

Reference Books:

1. Kothari, C.R. – Research Methodology: Methods and Techniques, New Age International Publishers, 2nd Edition

2. Ranjit Kumar – Research Methodology: A Step-by-Step Guide for Beginners, SAGE Publications

3. Day, R.A. & Gastel, B. – How to Write and Publish a Scientific Paper, Cambridge University Press

4. Turabian, K.L. – A Manual for Writers of Research Papers, Theses, and Dissertations, University of Chicago Press

5. ACS Style Guide – Effective Communication of Scientific Information, American Chemical Society

6. Bates, B. – Writing with Precision: How to Write So That You Cannot Possibly Be Misunderstood, Penguin Books

7. Sundaram, K.P.M. & Datt, R. – Research and Report Writing, S. Chand & Co.

8. McMillan, V.E. – Writing Papers in the Biological Sciences, Bedford/St. Martin’s

9. Lampman, G.M., Pavia, D.L., Kriz, G.S., & Engel, R.G. – Introduction to Organic Laboratory Techniques: A Small Scale Approach, Brooks/Cole

10. Pallavi Jain & Ashutosh Jain – Scientific Writing and Communication Skills, S. Chand Publishing

SEMESTER - VIII

COURSE: RESEARCH PROJECT/DISSERTATION – 1(RP/D-1) TOTAL CREDITS: 08

PAPER NAME: RESEARCH PROJECT/DISSERTATION Full Marks=200, Pass Marks=80

Guidelines for distribution of marks may be as follows or as appropriate:

Assessment of project synopsis/ Field Visit: 50 marks

Assessment of project thesis/dissertation: 100 marks

Viva-voce/Presentation: 50 marks

Course Objectives:

1. To facilitate students in conducting independent research projects in the field of Chemistry, allowing them to apply theoretical knowledge to practical experimentation.

2. To guide students in developing research skills, including problem identification, formulation of hypotheses, experimental design, data collection, analysis, and interpretation.

3. To foster critical thinking and analytical skills among students through the exploration of research methodologies and scientific literature.

4. To enhance students' communication abilities by requiring them to effectively present their research findings through written reports and oral presentations.

5. To cultivate ethical awareness and responsibility in research practices, including proper citation, acknowledgment of sources, and adherence to ethical guidelines and regulations.

Course Outcomes:

1. Students will demonstrate proficiency in designing and conducting independent research projects in Chemistry, from problem identification to data analysis.

2. Students will develop advanced skills in critical thinking, analytical reasoning, and problem-solving through the exploration of complex scientific questions.

3. Students will exhibit competency in utilizing various research methodologies and techniques appropriate for addressing specific research questions in Chemistry.

4. Students will effectively communicate their research findings through well-organized written reports and articulate oral presentations.

5. Students will demonstrate ethical conduct in research, including proper citation practices, avoidance of plagiarism, and adherence to ethical guidelines and regulations governing scientific research in Chemistry.

Course Contents:

Students who achieve a minimum of 75% marks across the first six semesters and express a desire to engage in undergraduate research may opt for a research stream during their fourth year of study. The Head of the Department (HOD) is responsible for assigning a supervisor to these students, chosen from the permanent faculty members holding a PhD degree. Subsequently, students, in consultation with their supervisor, select a research problem relevant and problem solving in nature to the local community/Industry, environment and may be related to innovation/novel method/idea with interdisciplinary approach to submit a synopsis or research proposal to the department for review.

Following this, the HOD convenes a meeting of the Departmental Research Council, where students present their synopsis or research proposal for approval or rejection. Upon approval, students commence their research work under the guidance of their supervisor and in accordance with the approved proposal.

At the conclusion of the semester, Each and every student has to submit the soft copy and the electronically typed hardbound copy of the project thesis/Dissertation with the Plagiarism Report strictly adhering to the University Grants Commission (Promotion of Academic Integrity and Prevention of Plagiarism in Higher Educational Institutions) Regulations, 2018 F. 1-18/2010(CPP-II). Published in THE GAZETTE OF INDIA: EXTRAORDINARY [PART III—SEC. 4] dated 23rd July, 2018 [web link :https://www.ugc.gov.in/pdfnews/7771545_academic-integrity-Regulation2018.pdf and the originality declarations of the supervisor and the student along with the raw data as date notified/affixed by the Head of the Department.

The department then forwards the thesis to an external evaluator, who provides a report on the work. Following receipt of the external report, the department shall arrange an open viva voce examination for the student, with both external and internal members present to assess the student's work.

The Department Research Committee shall be constituted from the following persons:

1. HOD of the Department–Chairmen

2. Dean, Faculty of Science- External member

3. HOD, University Department- External member

4. At list two permanent faculty member of the department (Nominated by HOD)- Members External members can be any of the following:

5. Permanent professors working in the postgraduate department of the university or other colleges who have the qualification to become PhD supervisors.

Retired Professor/Associate Professor/Assistant Professor of the university who has been supervising PhD scholar/s.

Professor/Associate Professor/Assistant Professor of the outside university who has been supervising PhD scholar/s.

Note- Minimum three external examiner lists will be sent by HOD through concerned College Principal to the Controller of Examination, SKMU, Dumka for final approval. In that list priority will be given as per order mentioned above.

Assessment of project synopsis	75 marks
Assessment of project Thesis	100 marks
Viva-voce	25 marks

******************

The project thesis shall be evaluated under the heads as per the standard LaTex/Word format made available by the Head of the Department which may include the following sections:

1. Title Page:

• Title of the thesis

• Author's name

• Affiliation

• Date

2. Abstract:

• A brief summary of the research work, including the objectives, methods, results, and conclusions.

3. Table of Contents:

• Lists all the major sections and subsections of the thesis, along with their respective page numbers.

4. List of Figures and Tables:

• Enumerates all the figures and tables included in the thesis, along with their page numbers.

5. Introduction:

• Provides background information on the research topic.

• States the research problem and objectives.

• Reviews relevant literature and previous research in the field.

• Outlines the structure of the thesis.

6. Experimental Methods:

• Describes the experimental procedures and methodologies used in the research.

• Includes details on materials, equipment, and techniques employed.

• Provides sufficient information to allow for replication of the experiments.

7. Results and Discussion:

• Presents the findings of the research.

• Organizes results logically, often using figures, tables, and graphs.

• Analyses and interprets the results in the context of the research objectives.

• Discusses the implications of the findings and their significance in the field.

8. Conclusion:

• Summarizes the key findings of the research.

• Restates the research objectives and addresses whether they were achieved.

• Offers insights into the broader implications of the research.

• Suggests avenues for future research.

9. References:

• Lists all the sources cited in the thesis, following a specific citation style (e.g., APA, MLA, Chicago).

• Includes journal articles, books, conference proceedings, and other relevant literature.

10. Appendices:

• Contains additional supplementary information that is relevant to the thesis but not essential to the main text.

• Includes raw data, detailed experimental procedures, calculations, or any other supporting material.

**********************

CHEMISTRY ASSOCIATED CORE AND ELECTIVE SYLLABI

SEMESTER –I/II

COURSE: ASSOCIATED CORE (CHEMISTRY) TOTAL CREDITS: THEORY-03, PRACTICAL-01

PAPER NAME: INTRODUCTORY CHEMISTRY TEACHING HOURS: THEORY-45, PRACTICAL-30

EVALUATION
	External Exam	Internal Exam	Practical
Full Marks	60	15	25
Full Marks	60	(10 Written + 5 Attendance/Overall Class Performance)	25
Duration of Exam	3 Hours	1 Hour	6 Hours
Pass Marks	30 Marks		10 marks

PART ‘A’

Instruction to Question Setter for

Semester Internal Examination (SIE 10+5=15 marks):

There will be two group of questions.

The Semester Internal Examination shall have two components. (a) One Semester Internal Examination Written Test (SIE) of 10 Mark. Question No.1 will be very short answer type in Group A consisting of five questions of 1 mark each. Group B will contain descriptive type two questions of five marks each, out of which any one to answer. (b) Class Attendance Score (CAS) including the behaviour of the student towards teachers and other students of the College of 5 marks.

End Semester Examination (ESE 60 marks):

There will be two group of questions. Group A is compulsory which will contain three questions. Question No.1 will be very short answer type consisting of five questions of 1 mark each. Question No.2 & 3 will be short answer type of 5 marks. Group B will contain descriptive type five questions of fifteen marks each, out of which any three are to answer.

Note: There may be subdivisions in the questions of group B.

Section A: Physical Chemistry

UNIT I: Chemical Energetics: (8 classes each of 60 minutes duration)

Important principles and definitions of thermochemistry. Concept of standard state and standard enthalpies of formations. Calculation of bond energy, bond dissociation energy from thermochemical data. Statement of Third Law of thermodynamics and calculation of absolute entropies of substances.

UNIT II: Chemical Kinetics: (7 classes each of 60 minutes duration)

The concept of reaction rates. Effect of temperature, pressure, catalyst and other factors on reaction rates. Order and molecularity of a reaction. Derivation of integrated rate equations for zero, first and second order reactions (both for equal and unequal concentrations of reactants). Half–life of a reaction. General methods for determination of order of a reaction. Concept of activation energy and its calculation from Arrhenius equation.

Section B: Inorganic Chemistry

UNIT III: Atomic Structure: (5 classes each of 60 minutes duration)

What is Quantum mechanics? Time independent Schrodinger equation and meaning of various terms in it. Significance of ψ and ψ² , Schrodinger equation for hydrogen atom. Radial distribution functions and the concept of the most probable distance with special reference to 1s and 2s atomic orbitals. Significance of quantum numbers, orbital angular momentum and quantum numbers ml and m_s. Shapes of s, p and d atomic orbitals, nodal planes. Discovery of spin, spin quantum number (s) and magnetic spin quantum number (m_s). Rules for filling electrons in various orbitals, Electronic configurations of the atoms. Stability of half-filled and completely filled orbitals, concept of exchange energy. Relative energies of atomic orbitals, Anomalous electronic configurations.

UNIT IV: Chemical Bonding and Molecular Structure: (10 classes each of 60 minutes duration)

Ionic Bonding: General characteristics of ionic bonding. Energy considerations in ionic bonding, lattice energy and solvation energy and their importance in the context of stability and solubility of ionic compounds. Polarizing power and polarizability. Fajan’s rules, ionic character in covalent compounds, bond moment, dipole moment and percentage ionic character.

Covalent bonding: VB Approach: Shapes of some inorganic molecules and ions on the basis of VSEPR and hybridization with suitable examples of linear, trigonal planar, square planar, tetrahedral, trigonal bipyramidal and octahedral arrangements.

Section C: Organic Chemistry

UNIT V: Fundamentals of Organic Chemistry: (3 classes each of 60 minutes duration)

Inductive Effect, Electromeric Effect, Resonance and Hyperconjugation. Cleavage of Bonds: Homolysis and Heterolysis. Structure, shape and reactivity of organic molecules: Nucleophiles and electrophiles. Reactive Intermediates: Carbocations, Carbanions and free radicals.

Aromaticity: Benzenoids and Hückel’s rule.

UNIT VI: Aliphatic hydrocarbons:

Alkanes: (4 classes each of 60 minutes duration) (Upto 5 Carbons)

Preparation: Catalytic hydrogenation, Wurtz reaction, Kolbe’s synthesis, from Grignard reagent. Reactions: Free radical Substitution: Halogenation

Alkenes: (3 classes each of 60 minutes duration) (Upto 5 Carbons)

Preparation: Elimination reactions: Dehydration of alkenes and dehydrohalogenation of alkyl halides (Saytzeff’s rule), Reactions: cis-addition (alk. KMnO4) and trans-addition (bromine), Addition of HX (Markownikoff’s and antiMarkownikoff’s addition), Hydration, Ozonolysis, oxymecuration-demercuration, Hydroboration-oxidation.

Alkynes: (3 classes each of 60 minutes duration) (Upto 5 Carbons)

Preparation: Acetylene from CaC2 and conversion into higher alkynes, by dehalogenation of tetra halides and dehydrohalogenation of vicinal-dihalides.

Reactions: Formation of metal acetylides, addition of bromine and alkaline KMnO4, ozonolysis and oxidation with hot alkaline KMnO4.

UNIT VII: Aromatic hydrocarbons: (5 classes each of 60 minutes duration)

Preparation of benzene: from phenol, by decarboxylation, from acetylene, from benzene sulphonic acid. Reactions of benzene: Electrophilic substitution: nitration, halogenation and sulphonation. Friedel-Craft’s reaction (alkylation and acylation). Side chain oxidation of alkyl benzenes (upto 4 carbons on benzene)

Reference Books:

1. J. C. Kotz, P. M. Treichel & J. R. Townsend: General Chemistry, Cengage Lening India Pvt. Ltd., New Delhi (2009)

2. Lee, J. D. Concise Inorganic Chemistry, Wiley, 5th Edn.

3. Douglas, B.E., McDaniel, D.H., Alexander J.J., Concepts & Models of Inorganic Chemistry, (Third Edition) John Wiley & Sons,1999.

4. Atkins, P. W. and De Paula, J. Physical Chemistry, Tenth Edition, Oxford University Press, 2014.

5. Douglas, B.E, Mc Daniel, D.H. & Alexander, J.J. Concepts & Models of Inorganic Chemistry 3rd Ed., John Wiley Sons, N.Y. 1994.

6. Peter Sykes, A Guide Book to Mechanism in Organic Chemistry, Longman.

7. C. K. Ingold, Structure and Mechanism in Organic Chemistry, Cornell University Press.

8. R. T. Morrison and R. N. Boyd, Organic Chemistry, Prentice-Hall.

9. H. 0. House, Modern Organic Reactions, Benjamin.

10. 0. C. Norman and J. M. Coxon, Principles of Organic Synthesis, Blackle Academic & Professional.

11. Ali, Hashmat, Reaction Mechanism in Organic Chemistry, S Chand

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

Section A: Physical Chemistry: Thermochemistry

1. Determination of heat capacity of calorimeter.

2. Determination of enthalpy of neutralization of hydrochloric acid with sodium hydroxide.

3. Determination of enthalpy of hydration of copper sulphate.

Section B: Inorganic Chemistry - Volumetric Analysis

1. Acid-Base Titrations

a) Estimation of carbonate and hydroxide present together in mixture

b) Estimation of carbonate and bicarbonate present together in a mixture.

2. Oxidation-Reduction Titrimetry

a) Estimation of Fe(II) in supplied solution using standardized KMnO₄ solution.

b) Estimation of oxalic acid using standardized KMnO4 solution.

Section C: Organic Chemistry

1.Purification of organic compounds by crystallization (from water and alcohol) and distillation.

2.Criteria of Purity: Determination of melting and boiling points.

3.Recrystallisation, determination of melting point and calculation of quantitative yields to be done.

Reference Books:

1.Vogel’s Qualitative Inorganic Analysis, A.I. Vogel, Prentice Hall, 7th Edition.

2.F. G. Mann & B. C. Saunders, Practical Organic Chemistry, Orient Longman (1960).

3.B.D. Khosla, Senior Practical Physical Chemistry, R. Chand & Co.

4.S. M. Khopkar, Environmental Pollution Analysis: Wiley Eastern Ltd, New Delhi.

SEMESTER –III/IV

COURSE: ELECTIVE COURSE (CHEMISTRY)-1 TOTAL CREDITS: THEORY-03, PRACTICAL-01

PAPER NAME: EQUILIBRIA & FUNCTIONAL GROUPS TEACHING HOURS: THEORY-45, PRACTICAL-30

EVALUATION
	External Exam	Internal Exam	Practical
Full Marks	60	15	25
Full Marks	60	(10 Written + 5 Attendance/Overall Class Performance)	25
Duration of Exam	3 Hours	1 Hour	6 Hours
Pass Marks	30 Marks		10 marks

PART ‘A’

Instruction to Question Setter for

Semester Internal Examination (SIE 10+5=15 marks):

There will be two group of questions.

End Semester Examination (ESE 60 marks):

Note: There may be subdivisions in the questions of group B.

Section A: Physical Chemistry

UNIT I: Equilibrium: (15 classes each of 60 minutes duration)

Chemical Equilibria: Le Chatelier’s principle. Relationships between Kp, Kc and Kx for reactions involving ideal gases.

Ionic Equilibria: Strong, moderate and weak electrolytes, degree of ionization, factors affecting degree of ionization, ionization constant and ionic product of water. Ionization of weak acids and bases, pH scale, common ion effect. Buffer solutions. Solubility and solubility product of sparingly soluble salts

Section B: Inorganic Chemistry (8 classes each of 60 minutes duration)

MO Approach: Rules for the LCAO method, bonding and antibonding MOs and their characteristics for s-s, sp and p-p combinations of atomic orbitals, nonbonding combination of orbitals, MO treatment of homonuclear diatomic molecules of 1st and 2nd periods.

Section C: Organic Chemistry

UNIT II: Alkyl and Aryl Halides

Alkyl Halides (Upto 5 Carbons) (5 classes each of 60 minutes duration) Types of Nucleophilic Substitution (SN¹, SN² and SN_i) reactions. Preparation: from alkenes and alcohols. Reactions: hydrolysis, nitrite & nitro formation, nitrile & isonitrile formation. Elimination vs substitution.

Aryl Halides (3 classes each of 60 minutes duration)

Preparation: (Chloro, bromo and iodo-benzene case): from phenol, Sandmeyer & Gattermann reactions. Reactions (Chlorobenzene):

Reactivity and Relative strength of C-Halogen bond in alkyl, allyl, benzyl, vinyl and aryl halides.

Alcohols: (4 classes each of 60 minutes duration)

Preparation: Preparation of 1^o, 2^о and 3^o alcohols: using Grignard reagent, Ester hydrolysis, Reduction of aldehydes, ketones, carboxylic acid and esters.

Reactions: With sodium, HX (Lucas test), esterification, oxidation (with PCC, alk. KMnO₄, acidic dichromate, conc. HNO₃). Oppeneauer oxidation Diols: (Upto 6 Carbons) oxidation of diols. Pinacol-Pinacolone rearrangement.

Phenols: (3 classes each of 60 minutes duration)

Preparation: Cumene hydroperoxide method, from diazonium salts.

Reactions: Electrophilic substitution: Nitration, halogenation and sulphonation. Reimer- Tiemann Reaction, Gattermann-Koch Reaction, Houben–Hoesch Condensation, Schotten – Baumann Reaction.

Ethers (aliphatic and aromatic): (2 classes each of 60 minutes duration) Methods of Preparations aliphatic and aromatic ethers, Williamson’s ether synthesis: Cleavage of ethers with HI.

Aldehydes and ketones (aliphatic and aromatic): (5 classes each of 60 minutes duration) (Formaldehye, acetaldehyde, acetone and benzaldehyde) Preparation: from acid chlorides and from nitriles. Reactions– Reaction with HCN, ROH, NaHSO₃, NH₂-G derivatives. Iodoform test. Aldol Condensation, Cannizzaro’s reaction, Clemensen reduction and Wolff Kishner reduction.

Reference Books:

1. T. W. Graham Solomons: Organic Chemistry, John Wiley and Sons.

2. Peter Sykes: A Guide Book to Mechanism in Organic Chemistry, Orient Longman.

3. I.L. Finar: Organic Chemistry (Vol. I & II), E. L. B. S.

4. R. T. Morrison & R. N. Boyd: Organic Chemistry, Prentice Hall.

5. Arun Bahl and B. S. Bahl: Advanced Organic Chemistry, S. Chand.

6. G. M. Barrow: Physical Chemistry Tata McGraw-Hill (2007).

7. G. W. Castellan: Physical Chemistry 4^th Edn. Narosa (2004).

8. J. C. Kotz, P. M. Treichel & J. R. Townsend: General Chemistry Cengage Lening India Pvt. Ltd., New Delhi (2009).

9. B. H. Mahan: University Chemistry 3^rd Ed. Narosa (1998).

10. R. H. Petrucci: General Chemistry 5^th Ed. Macmillan Publishing Co.: New York (1985).

11. Ali, Hashmat, Reaction Mechanism in Organic Chemistry ,S Chand

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

Section A: Physical Chemistry

Ionic equilibria pH measurements

1.Determine the pH of the given aerated drinks fruit juices, shampoos and soaps.

2.Preparation of buffer solutions:

a. Sodium acetate-acetic acid

b. Ammonium chloride-ammonium hydroxide

Section B: Organic Chemistry

1. Detection of hetero elements in organic compounds.

2. Functional group tests for alcohols, phenols, carbonyl and carboxylic acid group.

3. Preparation of 2,4 dinitrophenylhydrazone of aldehyde/ketone

Reference Books

1. B.D. Khosla, Senior Practical Physical Chemistry, R. Chand & Co.

2. A.I. Vogel: Textbook of Practical Organic Chemistry, 5^th edition, Prentice-Hall.

3. F. G. Mann & B. C. Saunders, Practical Organic Chemistry, Orient Longman (1960).

4. Waites M.J. (2008). Industrial Microbiology: An Introduction, 7^th Edition, Blackwell Science, London, UK.

5. Prescott S.C., Dunn C.G., Reed G. (1982). Prescott & Dunn’s Industrial Microbiology, 4^th Edition, AVI Pub. Co., USA.

6. Reed G. (2004). Prescott & Dunn’s industrial microbiology, 4^th Edition, AVI Pub. Co., USA.

7. JR Casida L.E. (2015). Industrial Microbiology, 3^rd Edition, New Age International (P) Limited Publishers, New Delhi, India.

8. Waites M.J., Morgan N.L., Rockey J.S. and Higton G. (2001) Industrial Microbiology: An Introduction. 1^st Edition, Blackwell Science, London, UK.

9. Pelczar M.J., Chan E.C.S. and Krieg N.R. (2003) Microbiology. 5^th Edition, Tata McGraw-Hill Publishing Company Limited, New Delhi.

SEMESTER –V/VI

COURSE: ELECTIVE COURSE (CHEMISTRY)-2 TOTAL CREDITS: THEORY-03, PRACTICAL-01

PAPER: CHEMISTRY OF s- & p-BLOCK ELEMENTS AND STATES OF MATTER

TEACHING HOURS: THEORY-45, PRACTICAL-30

EVALUATION
	External Exam	Internal Exam	Practical
Full Marks	60	15	25
Full Marks	60	(10 Written + 5 Attendance/Overall Class Performance)	25
Duration of Exam	3 Hours	1 Hour	6 Hours
Pass Marks	30 Marks		10 marks

PART ‘A’

Instruction to Question Setter for

Semester Internal Examination (SIE 10+5=15 marks):

There will be two group of questions.

End Semester Examination (ESE 60 marks):

Note: There may be subdivisions in the questions of group B.

SECTION-A: Inorganic Chemistry

UNIT I: General Principles of Metallurgy: (5 Lectures)

Chief modes of occurrence of metals based on standard electrode potentials. Ellingham diagrams for reduction of metal oxides using carbon as reducing agent. Hydrometallurgy, Methods of purification of metals (Al, Pb, Ti, Fe, Cu, Ni, Zn): electrolytic, oxidative refining, Kroll process, Parting process, van Arkel-de Boer process and Mond’s process.

UNIT II: s- and p-Block Elements: (5 Lectures)

Periodicity in s- and p-block elements with respect to electronic configuration, atomic and ionic size, ionization enthalpy, electronegativity (Pauling, Mulliken, and Alfred-Rochow scales). Allotropy in C, S, and P.

Oxidation states with reference to elements in unusual and rare oxidation states like carbides and nitrides), inert pair effect, diagonal relationship and anomalous behaviour of first member of each group.

UNIT III: Compounds of s- and p-Block Elements: (10 Lectures) Hydrides and their classification (ionic, covalent and interstitial), structure and properties with respect to stability of hydrides of p- block elements. Concept of multicentre bonding (diborane). Structure, bonding and their important properties like oxidation/reduction, acidic/basic nature of the following compounds and their applications in industrial, organic and environmental chemistry. Hydrides of nitrogen (NH₃, N₂H₄, N₃H, NH₂OH) Oxoacids of P, S and Cl. Halides and oxohalides: PCl₃, PCl₅, SOCl₂ and SO₂Cl₂

Section B: Physical Chemistry

UNIT IV: Kinetic Theory of Gases: (15 Lectures)

Postulates of Kinetic Theory of Gases and derivation of the kinetic gas equation. Most probable, average and root mean square velocities (no derivation). Collision number, collision frequency, collision diameter and mean free path of molecules. Maxwell Boltzmann distribution laws of molecular velocities and molecular energies.

Deviation of real gases from ideal behaviour, compressibility factor, causes of deviation. Van der Waals equation of state for real gases. Boyle temperature (derivation not required). Critical phenomena, critical constants and their calculation from van der Waals equation. Andrews isotherms of CO₂.

UNIT V: Liquids: (4 Lectures)

Surface tension and its determination using stalagmometer. Viscosity of a liquid and determination of coefficient of viscosity using Ostwald viscometer. Effect of temperature on surface tension and coefficient of viscosity of a liquid (qualitative treatment only)

UNIT VI: Solids (6 Lectures)

Forms of solids. Symmetry elements, unit cells, crystal systems, Bravais lattice types and identification of lattice planes. Laws of Crystallography – Law of constancy of interfacial angles, Law of rational indices. Miller indices. X–Ray diffraction by crystals, Bragg’s law. Structures of NaCl, KCl and CsCl (qualitative treatment only).

Reference Books:

1. G. M. Barrow: Physical Chemistry Tata McGraw-Hill (2007).

2. G. W. Castellan: Physical Chemistry 4^th Edn. Narosa (2004).

3. J. C. Kotz, P. M. Treichel & J. R. Townsend: General Chemistry Cengage Lening India Pvt. Ltd., New Delhi (2009).

4. B. H. Mahan: University Chemistry 3^rd Ed. Narosa (1998).

5. R. H. Petrucci: General Chemistry 5^th Ed. Macmillan Publishing Co.: New York (1985).

6. J. D. Lee: A New Concise Inorganic Chemistry, E.L.B.S.

7. F.A. Cotton & G. Wilkinson: Basic Inorganic Chemistry, John Wiley.

8. D. F. Shriver and P. W. Atkins: Inorganic Chemistry, Oxford University Press.

9. Gary Wulfsberg: Inorganic Chemistry, Viva Books Pvt. Ltd.

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

Section A: Inorganic Chemistry

Qualitative semi micro analysis

1. Semi-micro qualitative analysis using H₂S of mixtures- not more than four ionic species (two anions and two cations and excluding insoluble salts) out of the following:

Cations: NH4⁺, Pb²⁺, Ag⁺, Bi³⁺, Cu²⁺, Cd²⁺, Sn²⁺, Fe³⁺, Al³⁺, Co²⁺, Cr³⁺, Ni²⁺,Mn²⁺, Zn²⁺, Ba²⁺, Sr²⁺, Ca²⁺, K⁺

Anions : CO₃ ^2– , S^2–, SO^2–, S₂O₃^2–, NO₃ ^–, CH₃COO^–, Cl^–, Br^–, I^–, NO₃^–,SO₄^2-, PO₄^3-, BO₃^3-, C₂O₄ ^2-, F^-(Spot tests should be carried out wherever feasible)

Section B: Physical Chemistry

(I) Surface tension measurement (use of organic solvents excluded).

a) Determination of the surface tension of a liquid or a dilute solution using a stalagmometer.

b) Study of the variation of surface tension of a detergent solution with concentration.

(II) Viscosity measurement (use of organic solvents excluded).

a) Determination of the relative and absolute viscosity of a liquid or dilute solution using an Ostwald’s viscometer.

b) Study of the variation of viscosity of an aqueous solution with concentration of solute.

(III) Chemical Kinetics -Study the kinetics of the following reactions.

a Acid hydrolysis of methyl acetate with hydrochloric acid.

b. Saponification of ethyl acetate.

Reference Books

1. A.I. Vogel, Qualitative Inorganic Analysis, Prentice Hall, 7^th Edn.

2. A.I. Vogel, Quantitative Chemical Analysis, Prentice Hall, 6^th Edn. 3. B.D. Khosla, Senior Practical Physical Chemistry, R. Chand & Co.

SEMESTER –VII/VIII

COURSE: ELECTIVE COURSE (CHEMISTRY)-3 TOTAL CREDITS: THEORY-03, PRACTICAL-01

PAPER: CHEMISTRY OF d- & f-BLOCK ELEMENTS & MOLECULES OF LIFE

TEACHING HOURS: THEORY-45, PRACTICAL-30

EVALUATION
	External Exam	Internal Exam	Practical
Full Marks	60	15	25
Full Marks	60	(10 Written + 5 Attendance/Overall Class Performance)	25
Duration of Exam	3 Hours	1 Hour	6 Hours
Pass Marks	30 Marks		10 marks

PART ‘A’

Instruction to Question Setter for

Semester Internal Examination (SIE 10+5=15 marks):

There will be two group of questions.

End Semester Examination (ESE 60 marks):

Note: There may be subdivisions in the questions of group B.

Section A: Inorganic Chemistry

UNIT I: Transition Elements (3d series) (6 classes each of 60 minutes duration)

General group trends with special reference to electronic configuration, variable valency, colour, magnetic and catalytic properties, ability to form complexes and stability of various oxidation states.

UNIT II: Lanthanides and Actinides: (5 classes each of 60 minutes duration)

Electronic configuration, oxidation states, colour, spectra and magnetic behaviour of lanthanides and actinides. Lanthanide contraction, separation of lanthanides (ion-exchange method only).

UNIT III: Coordination Chemistry (5 classes each of 60 minutes duration)

Valence Bond Theory (VBT): Inner and outer orbital complexes of Cr, Fe, Co, Ni and Cu (coordination numbers 4 and 6). Structural and stereoisomerism in complexes with coordination numbers 4 and 6. Drawbacks of VBT. IUPAC system of nomenclature.

UNIT IV: Crystal Field Theory (4 classes each of 60 minutes duration)

Crystal field effect, octahedral symmetry. Crystal field stabilization energy (CFSE), Crystal field effects for weak and strong fields. Tetrahedral symmetry. Factors affecting the magnitude of Dq.

Section B: Organic Chemistry

UNIT V: Carbohydrates (8 classes each of 60 minutes duration) Classification of carbohydrates, reducing and non-reducing sugars, General properties of Glucose and Fructose, their open chain structure. Epimers, mutarotation and anomers. Determination of configuration of Glucose (Fischer proof). Cyclic structure of glucose. Haworth projections. Cyclic structure of fructose. Linkage between monosachharides, structure of disacharrides (sucrose, maltose, lactose) and polysacharrides (starch and cellulose) excluding their structure elucidation.

UNIT VI: Amino Acids, Peptides and Proteins (8 classes each of 60 minutes duration) Classification of Amino Acids, Zwitterion structure and Isoelectric point

Overview of Primary, Secondary, Tertiary and Quaternary structure of proteins.Synthesis of simple peptides (upto dipeptides) by N-protection (t- butyloxycarbonyl and phthaloyl) & Cactivating groups and Merrifield solid phase synthesis.

UNIT VII: Enzymes and correlation with drug action (6 classes each of 60 minutes duration)

Mechanism of enzyme action, factors affecting enzyme action, Coenzymes and cofactors and their role in biological reactions, Specificity of enzyme action (Including stereospecifity).

Enzyme inhibitors and their importance, phenomenon of inhibition (Competitive and Non- competitive inhibition including allosteric inhibition).

UNIT VIII: Lipids (3 classes each of 60 minutes duration) Introduction to lipids, classification. Oils and fats: Common fatty acids present in oils and fats, Omega fatty acids, Trans fats, Hydrogenation, Saponification value, Iodine number.

Biological importance of triglycerides, phospholipids, glycolipids, and steroids (cholesterol).

Reference Books:

1. J. C. Kotz, P. M. Treichel & J. R. Townsend: General Chemistry, Cengage Lening India Pvt. Ltd., New Delhi (2009).

2. B. H. Mahan: University Chemistry 3rd Ed. Narosa (1998).

3. R. H. Petrucci: General Chemistry 5th Ed. Macmillan Publishing Co.: New York (1985).

4. J. D. Lee: A New Concise Inorganic Chemistry, E.L.B.S.

5. F.A. Cotton & G. Wilkinson: Basic Inorganic Chemistry, John Wiley.

6. Gary Wulfsberg: Inorganic Chemistry, Viva Books Pvt. Ltd.

7. Morrison, R. T. & Boyd, R. N. Organic Chemistry, Dorling Kindersley (India) Pvt. Ltd. (Pearson Education).

8. Finar, I. L. Organic Chemistry (Volume 1), Dorling Kindersley (India) Pvt. Ltd. (Pearson Education).

9. Finar, I. L. Organic Chemistry (Volume 2), Dorling Kindersley (India) Pvt. Ltd. (Pearson Education).

10. Nelson, D. L. & Cox, M. M. Lehninger’s Principles of Biochemistry 7th Ed., W. H. Freeman.

11. Berg, J. M., Tymoczko, J. L. & Stryer, L. Biochemistry 7th Ed., W. H. Freeman.

12. Ali, Hashmat, Reaction Mechanism in Organic Chemistry ,S Chand

13. Sourav Kumar,Chemistry in daily life,Crown Publishing (2025

PART ‘B’

PRACTICAL COURSE CONTENTS:

End Semester Examination (ESE):

There will be one Practical Examination of 6 Hours duration. Evaluation of Practical Examination may be as per the following guidelines:

Two Experiments = 20 marks

Practical record notebook = 03 marks

Viva-voce = 02 marks

Section A: Inorganic Chemistry

1. Estimation of the amount of nickel present in a given solution as bis(dimethylglyoximato) nickel (II) or aluminium as oxinate in a given solution gravimetrically.

2. Estimation of (i) Mg or (ii) Zn by complexometric titrations using EDTA.

3. Estimation of total hardness of a given sample of water by complexometric titration.

Section B: Organic Chemistry

1. Separation of amino acids by paper chromatography

2. To determine the concentration of glycine solution by formylation method.

3. Study of titration curve of glycine

4. To determine the saponification value of an oil/fat.

5. To determine the iodine value of an oil/fat

6. Differentiate between a reducing/ nonreducing sugar.

Reference Books

1. A.I. Vogel, Qualitative Inorganic Analysis, Prentice Hall, 7th Edn.

2. A.I. Vogel, Quantitative Chemical Analysis, Prentice Hall, 6th Edn.

3. Vogel’s Textbook of Practical Organic Chemistry, ELBS.

4. Ahluwalia, V.K. & Aggarwal, R. Comprehensive Practical Organic Chemistry, Universities Press.

Department of Chemistry, A.S. College, Deoghar

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