UG Chemistry Syllabus 2025

       

 Semester wise Subject Combination for B.Sc. (CHEMISTRY)

Semester	Course Category	Code	Papers	Credits
First Semester	Major	MJ-1	Atomic Structure, Chemical Bonding & Redox Reactions	4
	Associated Core/Associated Vocational	AC-1A	Select any one subject from the Associated Core Table with the guidance of the Class Teacher.	4
	Multidisciplinary Course	MDC-1	Choose any one of the following: • Mathematical and Computational Thinking Analysis • Gender Studies • Goods and Services Tax (GST) • Pollution Control and Waste Management	3
	Ability Enhancement Course	AEC-1	Hindi (Compulsory)	2
	Skills Enhancement Course	SEC-1	Introduction to Computer and IT (Compulsory)	2
	Value Added Course	VAC-1	Understanding India (Compulsory)	3
	Indian Knowledge System	IKS-I	Indian Knowledge System (Compulsory)	2
Second Semester	Major	MJ-2	Theory-Mj-2: States Of Matter & Concept Of Ionic Equilibrium	4
	Associated Core/Associated Vocational	AC-2B	Select any one subject either from the Associated Core subjects not studied in Semester-I or from the Associated Vocational subjects, with the guidance of the Class Teacher.	4
	Multidisciplinary	MDC-2	Choose any one of the following: ·        Nutrition and Health education ·        Digital Marketing ·        Introduction to Indian Values and Ethics ·        Santhal Tribes and Culture	3
	Ability Enhancement	AEC-2	English (Compulsory)	2
	Skills Enhancement	SEC-2	Digital Communication and Data Management (Compulsory)	3
	Value Added Course	VAC-2	Environmental Studies (Compulsory)	2
	Indian Knowledge System	IKS-2	Social Awareness (Compulsory)	2
Third Semester	Major	MJ-3	General Organic Chemistry And Hydrocarbons	4
		MJ-4	THEORY-MJ-4: ACID, BASES, SALTS, METALLURGY, S & P-BLOCK ELEMENTS, INORGANIC POLYMERS	4
	Elective Course	ELC-1A	Elective Paper-1 from the Chosen Associated Core Subject in Semester I	4
	Multidisciplinary	MDC-3	Choose any one of the following: ·        Indian Philosophy ·        Indian Cultural Studies ·        Kautilya's Arthashastra ·        Vedic Mathematics	3
	Ability Enhancement	AEC-3	Select One Language Course: Students must choose one of the following languages: Hindi, English, Bangla, Sanskrit, Urdu, Santali, Persian, or Maithili. Note: Students are required to study Paper-I of the language they choose.	2
	Skills Enhancement	SEC-3	Computer Software, Programming and AI (Compulsory)	3
Fourth Semester	Major	MJ-5	Chemistry In Indian Knowledge System	4
		MJ-6	Thermochemistry & Chemical Thermodynamics-I	4
		MJ-7	Functional Groups Containing F, Cl, Br & O	4
	Elective Course	ELC-1B	Elective Paper-1 from the Chosen Associated Core/Associated Vocational Subject in Semester-II	4
	Ability Enhancement	AEC-4	Paper-2 of Selected Language course in Semester-III	2
	Value Added Course	VAC-3	Health& Wellness, Yoga Education, Sports & Fitness (Compulsory)	2
Fifth Semester	Major	MJ-8	d- &f- BLOCK ELEMENTS, COORDINATION CHEMISTRY & NON-AQUEOUS SOLVENTS	4
		MJ-9	Thermodynamics-2-Dilute Solutions, Equilibrium and Phase Equilibrium	4
		MJ-10	Functional Groups Containing N & S, Hetrocyclic Compounds, Alkaloids, Terpenes	4
		MJ-11	Organometallic And Bioinorganic Chemistry	4
	Elective Course	ELC-2A	Elective Paper-2 from the Chosen Associated Core Subject in Semester I	4
Sixth Semester	Major	MJ-12	Chemical Kinetics, Catalysis & Surface Chemistry	4
		MJ-13	Bio-Organic Chemistry: Amino Acids, Lipids, Enzymes, Nucleic Acids & Pharmaceutical Compounds	4
		MJ-14	Reaction Mechanisms & Electronic Spectra In Inorganic Chemistry	4
		MJ-15	Electrochemistry, Electrical And Magnetic Properties Of Materials	4
	Elective Course	ELC-2B	Elective Paper-2 from the Chosen Associated Core/Associated Vocational Subject in Semester-II	4
·        In the fourth year, students have two pathways: they can either complete their graduation with Honours, or with Honours with Research. ·        Those who wish to graduate with Honours only must follow Table-A, while those opting for Honours with Research must follow Table-B.
TABLE-A FOR HONOURS ONLY FOURTH YEAR
Seventh Semester	Major	MJ-16	Organic Spectroscopy, Carbohydrates & Dyes	4
		MJ-17	Industrial Chemicals And Environment	4
		MJ-18	Quantum Chemistry And Covalent Bonding	4
	Advance Major	AMJ-1	Analytical Chemistry	4
	Elective Course	ELC-3A	Elective Paper-3 from the Chosen Associated Core Subject in Semester I	4
Eighth Semester	Major	MJ-19	Molecular Spectroscopy & Photochemistry	4
		MJ-20	Group Discussion And Dissertation	4
	Advance Major	AMJ-2	Green And Sustainable Chemistry	4
		AMJ-3	Inorganic Materials & Nanochemistry	4
	Elective Course	ELC-3B	Elective Paper-3 from the Chosen Associated Core/Associated Vocational Subject in Semester-II	4
TABLE-B FOR HONS WITH RESEARCH FOURTH YEAR
Seventh Semester	Major	MJ-16	Organic Spectroscopy, Carbohydrates & Dyes	4
		MJ-17	Industrial Chemicals And Environment	4
		MJ-18	Quantum Chemistry And Covalent Bonding	4
	Research Methodology	RC-1	Research Methodology In Chemistry	4
	Elective Course	ELC-3A	Elective Paper-3 from the Chosen Associated Core Subject in Semester I	4
	Major	MJ-19	Molecular Spectroscopy & Photochemistry	4
Eighth Semester		MJ-20	Group Discussion And Dissertation	4
	Research Project/ Dissertation	RC-2	Research Project/Fieldwork/Dissertation	8
	Elective Course	ELC-3B	Elective Paper-3 from the Chosen Associated Core/Associated Vocational Subject in Semester-II	4
Compulsory Summer Internship: 1.   If a student exits after Semester II, IV, or VI: To receive a Certificate/Diploma/Bachelor’s Degree, students must complete a summer internship/project/dissertation worth 4 credits. This should be done during the summer break of any semester within the first three years. Note: The Certificate/Diploma/Bachelor’s Degree will not be awarded without completing this internship. 2.   If a student exits after Semester VIII: Under the National Education Policy (NEP), all students must complete a 4-credit summer internship to get a Bachelor’s Hons/Hons with Research/P.G. Diploma Degree. There are two ways to complete this requirement:      a. Two internships of 4 weeks each (2 credits each), or      b. One internship of 8 weeks (4 credits total) The college will help arrange the internship, and students can complete it any time between Semester 1 and Semester 6 Summer Vacation. Note: The Bachelor (Hons)/Hons with Research, or P.G. Diploma will not be awarded without completing the internship.

 INSTRUCTIONS FOR QUESTION SETTER

1.   Semester Internal Examination Question Pattern (15 Marks)

The Semester Internal Examination (SIE) will carry a total of 15 marks, which includes 10 marks for the internal test and 5 marks for class attendance. The question paper will have two groups.

Group A will have: Question 1: Five very short answer questions (1 mark each, total 5 marks)

Group B will have: Two descriptive-type questions of 5 marks each, out of which students must answer any one (total 5 marks) The remaining 5 marks will be based on class attendance, as per the following:

Ø  Up to 45% attendance: 1 mark

Ø  46% to 54%: 2 marks

Ø  55% to 64%: 3 marks

Ø  65% to 74%: 4 marks

Ø  75% and above: 5 marks

 

2.   End Semester University External Examination Question Pattern (60 Marks)

The End Semester Examination (ESE) will be of 60 marks and will also have two groups.

Group A (Compulsory) will include: Question 1: Five very short answer questions (1 mark each, total 5 marks)

Questions 2 and 3: Two short answer questions (5 marks each, total 10 marks) Group B will contain five descriptive-type questions of 15 marks each, out of which students must answer any three (total 45 marks)

Note: Questions may have sub-parts if needed in the theory examination.

 

3.   End Semester University Practical Examination Question Pattern (25 Marks)

The End Semester Practical Examination (ESE) will be of 6 hours duration. The total marks and evaluation should be done as per the following guidelines:

·        Experiment/Activity performed during the exam – 15 marks

·        Practical record notebook – 5 marks

·        Viva-voce (oral questions) – 5 marks

Students must score at least 10 marks to pass the practical examination.

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PROMOTION CRITERIA

·        All students will be promoted in odd Semesters (I, III, V & VII).

·        To get a promotion from Semester II to Semester III, from Semester IV to Semester V, and from Semester VI to Semester VII a student has to procure a minimum of 4 CGPA.

·        However, it will be necessary to obtain a minimum credit (4) to pass in each of the subjects individually before completion of the course.

CALCULATION OF MARKS FOR THE PURPOSE OF RESULT

The passing in a subject will be based on the combined marks obtained in both the internal and external examinations of the semester. However, the student must pass the theory and practical examinations separately.                                                            

  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_c and 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-II

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.

(c) Calculation of the enthalpy of ionization of ethanoic acid.

(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 rate. 

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)

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.

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_max and 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).

 

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

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

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

4.            Identification of functional groups via group frequencies.

5.           Analysis of rotational spectra of diatomic molecules.

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

7.           Photoreduction of potassium ferrioxalate and comparison with actinometer.

8.           Determination of quantum yield of a photochemical reaction.

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