COURSE STRUCTURE WITH CREDIT WEIGHTAGE OF CHEMISTRY FOR BACHELORS IN SCIENCE (GENERAL) 2020 AND ONWARDS: B.Sc. 1 st SEMESTER DISCIPLINE SPECIFIC COURSE (CORE) CH120C: CHEMISTRY Max. Marks: 60 Course Weightage: 04 Credit (Theory) No. of Contact Hours: 60 Course Objectives: To introduce students to basic concepts of chemical bonding, S-block elements, general organic chemistry and states of matter. Course outcomes: The students after learning the course will be able to: 1. Understand the nature and strength of forces between chemical constituents. 2. Understand the applications of different theories of chemical bonding. 3. Gain knowledge about the chemical reactivity of S-Block elements. 4. Understand stereochemical aspects of organic molecules. 5. Acquire knowledge of aromaticity and reaction intermediates. 6. Understand the structural and behavioral aspects of matter in solid, liquid and gaseous states. UNIT-I: Chemical Bonding and Molecular Structure (15 Contact hours) Ionic bond: Lattice energy and Born Haber Cycle. Factors affecting the structure of ionic solids; Radius ratio effect; Coordination number and limitations of radius ratio rule. Solvation energy and solubility of ionic solids. Covalent bond: Formation of hydrogen molecule, Polarity in covalent bonds, Covalent-character of ionic bond, Fajan’s rules, Percentage ionic character of a polar covalent bond. Dipole moment. Valence bond theory: Directional characteristics of covalent bond and types of hybridizations. Limitations of VB theory. VSEPR theory: Assumptions; geometry of covalent molecules (BeF2, BF3, CH4, PCl5, SF6, SnCl2, NH3, H2O, SF4, ClF3 and XeF2). Molecular orbital theory: MO treatment of homo & hetero nuclear diatomic molecules (N2, O2, CO & NO). Energy level diagrams, Bond order and applications. UNIT II: S-Block Elements (15 Contact hours) Electronegativity and electron affinity: Determination and applications. Effective nuclear charge, slater rules and its applications. Position of hydrogen in periodic table. Isotopes of hydrogen. Chemical reactivity of s-block elements towards water, oxygen, nitrogen and halogens. Anomalous behaviour and diagonal relationships (Lithium, Beryllium, Magnesium and Aluminum). Solubility of alkali metals in ammonia, Ionic conductance. Chemical characteristics of the compounds of alkali and alkaline earth metals; oxides and hydroxides, carbonates, sulphates, halides. Hydrides and their classification. SEM COURSE CODE COURSE TITLE COURSE TYPE CREDIT WEIGHTAGE THEORY PRACTICAL I CH120C CHEMISTRY DSC-1 4 2 II CH220C CHEMISTRY DSC-2 4 2 III CH320C CHEMISTRY DSC-3 4 2 IV CH420C CHEMISTRY DSC-4 4 2 V CH520DA NUCLEAR CHEMISTRY, HETEROATOMS AND SOLUTION THERMODYNAMICS DSE-5 4 2 V CH520DB CHEMISTRY OF BIO-MOLECULES DSE-6 4 2 VI CH620DA SPECTROSCOPY DSE-6 4 2 VI CH620DB ENVIRONMENTAL AND GREEN CHEMISTRY DSE-6 4 2
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COURSE STRUCTURE WITH CREDIT WEIGHTAGE OF CHEMISTRY FOR BACHELORS IN
SCIENCE (GENERAL) 2020 AND ONWARDS:
B.Sc. 1st SEMESTER
DISCIPLINE SPECIFIC COURSE (CORE)
CH120C: CHEMISTRY Max. Marks: 60
Course Weightage: 04 Credit (Theory) No. of Contact Hours: 60
Course Objectives:
To introduce students to basic concepts of chemical bonding, S-block elements, general organic chemistry and
states of matter.
Course outcomes: The students after learning the course will be able to:
1. Understand the nature and strength of forces between chemical constituents.
2. Understand the applications of different theories of chemical bonding.
3. Gain knowledge about the chemical reactivity of S-Block elements.
4. Understand stereochemical aspects of organic molecules.
5. Acquire knowledge of aromaticity and reaction intermediates.
6. Understand the structural and behavioral aspects of matter in solid, liquid and gaseous states.
UNIT-I: Chemical Bonding and Molecular Structure (15 Contact hours)
Ionic bond: Lattice energy and Born Haber Cycle. Factors affecting the structure of ionic solids;
Radius ratio effect; Coordination number and limitations of radius ratio rule. Solvation energy and
solubility of ionic solids.
Covalent bond: Formation of hydrogen molecule, Polarity in covalent bonds, Covalent-character of
ionic bond, Fajan’s rules, Percentage ionic character of a polar covalent bond. Dipole moment.
Valence bond theory: Directional characteristics of covalent bond and types of hybridizations.
10. Advanced Physical Chemistry Experiments; J. N. Gurtu, A. Gurtu, PragatiPrakashan, 2008.
11. Inorganic Chemistry Practical; D. Pant, Bookrix, 2010.
B.Sc. 3rd SEMESTER
DISCIPLINE SPECIFIC COURSE (CORE)
CH320C: CHEMISTRY Max. Marks: 60
Course Weightage: 04 Credit (Theory) No. of Contact Hours: 60
Course Objectives:
To introduce students to basic concepts of periodic table (d-block), chemistry of alcohols, phenol,
ethers, thermodynamics and its applications to equilibria.
Course outcomes: The students after learning the course will be able to understand:
1. The trends in the chemical and physical properties of transition and inner transition elements
along with their compounds.
2. The preparation and chemical reactions of alcohols, phenols and ethers.
3. Laws of thermodynamics and their application to chemical and phase equilibria.
UNIT I: Transition and Inner Transition Elements (15 Contact hours)
Transition elements: Variable-oxidation states. Standard electrode Potentials of M2+/M and M3+/
M2+systems.
Ionic / Covalent and Acidic / Basic character of transition metal oxides in various oxidation states.
Stabilization of unusual oxidation states.
Spectral and magnetic Properties; Calculation and uses of magnetic moment value.
Interstitial hydrides and oxides of first transition series: Preparation, properties &uses.
Inner-Transition elements: Electronic configuration, oxidation states, Magnetic properties and
complexing behaviour of inner-transition elements.
Cause and consequences of Lanthanoid/Actinoid Contractions.
Separation of lanthanoids: Fractional crystallization, Ion–exchange and solvent extraction-methods.
UNIT II: Chemistry of Oxygen Bearing Compounds-I (15 Contact hours)
Alcohols: Classification, relative reactivity of 1o, 2o, 3o alcohols involving cleavage of C-O and O-H
bonds. Reactions of alcohols: Esterfication, alkylation, acetylation, dehydration, oxidation, reaction
with thionyl chloride and Bouvaelt-Blanc-Reduction, Vicinal Diols: Oxidation by per-iodic acid and
lead tetraacetate. Pinacol-Pinacolone rearrangement.
Phenol: Preparation of phenol from cumene. Acidity of phenol and effect of substituents on acidity.
Mechanism of bromination of phenol, Kolbe-Schmidt reaction.
Ethers: Williamson’s ether synthesis. Cleavage of ethers.
Epoxides: Preparation of epoxides. Mechanism of acid/base catalyzed ring openings of epoxides.
Reactions of Grignard and organolithium reagents with epoxides.
UNIT-III: Chemical Thermodynamics (15 Contact hours)
Thermodynamic functions: State and path functions and their differentials. Heat capacity, heat
capacities at constant volume and constant pressure and their relationship, Joule-Thomson effect,
Calculation of w, q, ΔU & ΔH for the expansion of ideal gases under isothermal and adiabatic
conditions. Kirchhoff’s equation.
Second law of thermodynamics: Different statements of the law. Carnot cycle and its efficiency,
Carnot theorem. Concept of entropy, entropy as a function of V&T, and as a function of P&T.
Clausius inequality; entropy as criteria for spontaneity and equilibrium. Entropy change in physical
processes, ideal gas expansion and entropy of mixing of ideal gases. Third law of thermodynamics: Gibbs function (G) and Helmholtz function (A) and spontaneity,
Gibbs-Helmholtz equation, Variation of G and A with P, V and T. Nernst heat theorem, third law of
thermodynamics.
UNIT IV: Chemical and Phase Equilibria (15 Contact hours)
Equilibrium: Relationship between equilibrium constant and free energy change. Thermodynamic
derivation of law of mass action. Clausius-Clapeyron equation, applications.
Phase Equilibria: Meaning of the terms: phase, component and degree of freedom, Phase rule.
Phase diagrams of one component system – water and Sulphur systems. Phase equilibria of two component system: Solid-liquid equilibria, simple eutectic system (Pb-Ag), desilverisation of lead. Partially miscible liquids: Lower and upper consolute temperatures, (examples of phenol-water,
trimethylamine-water, nicotine-water systems). Nernst distribution law and its applications
11. Senior Practical Physical Chemistry PB; B. D. Khosla; V. C. Garg; A. R. Gulati; R. Chand &
Co, 2008.
12. Advanced Physical Chemistry Experiments; J. N. Gurtu, A. Gurtu, PragatiPrakashan, 2008.
13. Inorganic Chemistry Practical; D. Pant, Bookrix, 2010.
B.Sc. 4th SEMESTER
DISCIPLINE SPECIFIC COURSE (CORE)
CH420C: CHEMISTRY Max. Marks: 60
Course Weightage: 04 Credit (Theory) No. of Contact Hours: 60
Course Objectives:
To introduce students to coordination chemistry, carbonyl group chemistry and electrochemistry and
introductory quantum chemistry.
Course outcomes: The students after learning the course will be able to understand;
1. The structure, bonding and isomerism in various types of complexes.
2. The preparation and chemical reactions of carbonyl compounds.
3. The electrochemistry of electrodes and cells.
4. The limitation of classical mechanics and importance of quantum mechanics.
UNIT I: Coordination Chemistry (15 Contact hours)
Introduction, experimental verification of Werner’s theory. Effective atomic number: Stability of
coordination compounds (Thermodynamic and Kinetic) and the factors affecting stability. Chelate and
macrocyclic effects.
Stereochemistry of coordination compounds with coordination numbers 2-6; Optical and
Geometrical isomerism.
Bonding in coordination compounds: Valence bond theory, Limitations, Crystal Field theory, crystal
field splitting in tetrahedral, square planar and octahedral systems. Calculation of CFSE, Factors
affecting magnitude of CFSE; pairing energy and CFSE under weak and strong field ligands.
Spectrochemical series. Magnetic and electronic properties of transition metal complexes. Limitations
of crystal field theory.
UNIT II: Chemistry of Oxygen Bearing Compounds-II (15 Contact hours)
Aldehydes and ketones: Structure and reactivity of carbonyl group. Synthesis of aldehydes starting
from acid chlorides and those of ketones from nitriles, carboxylic acids and 1, 3-dithianes. Reactions
of carbonyl compounds with HCN, ROH, NaHSO3, NH2 -G derivatives. Mechanisms involved in
Benzoin, Aldol/Cross Aldol, Perkin, Knoevenagel and Cannizzaro. Condensations / reactions.
Clemmenson and Wolf-Kishner reductions, and Baeyer–Villegar oxidation.
Carboxylic acids and their derivatives: Mechanistic details of preparation of carboxylic acids using
Grignard reagent, hydrolysis of nitriles andoxidation of alkyl benzenes. Factors affecting acid strength
of carboxylic acids. Mechanisms involved in the HVZ reaction, conversion of acids to its derivatives.
Relative stabilities and interconversion of acid derivatives into one another.
UNIT III: Electrochemistry (15 Contact hours)
Arrhenius theory of electrolyte dissociation and its limitations. Kohlrausch’s law. Debye-Huckel-
Onsager's equation for strong electrolytes (elementary treatment without derivation). Transport
number, definition and determination by Hittorf’s and moving boundary methods. Application of
conductivity measurements: determination of degree of dissociation and dissociation constants of
acids, solubility product of a sparingly soluble salt, conductometric titrations. Electrochemical reaction and electrode potential. Nernst equation and its use for estimation of
Course Weightage: 04 Credit (Theory) No. of Contact Hours: 60
Course Objectives:
To provide basic knowledge of spectroscopy and its applications.
Course outcomes: The students after learning the course will be able to understand;
1. The regions of electromagnetic spectrum and its interactions with matter.
2. The underlying principles involved in transitions (rotational, vibrational, electronic NMR),
interpretation of the corresponding spectra and applications
THEORY: 4 CREDITS
Unit- I Spectroscopy-I (15 Contact hours)
Spectroscopy: Electromagnetic radiation, regions of the spectrum, Representation of molecular spectrum, Peak position, intensity and width. Types of peak broadening. Statement of Born-Oppenheimer approximation. Rotational spectrum: Moment of inertia, classification of molecules on the basis of moment of inertia.
Energy of a rigid diatomic rotor, selection rules for rotational transition and associated spectrum,
relative population of rotational levels and spectral intensity, determination of bond length in diatomic
molecules.
Unit-II Spectroscopy-II (15 Contact hours)
Vibrational Spectrum: Classical and quantum mechanical (qualitative) treatment of simple harmonic
oscillator, selection rules for vibrational transition, pure vibrational spectrum of a diatomic molecule,
determination and relation of force constant with bond length and bond energy.
Molecular vibrations, IR transitions and selection rules. Group frequency and fingerprint regions and
its significance. Effect of resonance, inductive effect and H-bonding on infrared absorptions.
8. John R. Dyer: Applications of Absorption Spectroscopy of Organic Compounds, Prentice Hall.
9. Spectrometric Identification of Organic Compounds; R. M. Silverstein, F. X. Webster, D. J.
Kiemle, D. L. Bryce; 8thEdn., John Wiley & Sons, 2014.
B.Sc. 6th SEMESTER-CHEMISTRY
LAB COURSE (OPTION-I)
CH620DA: PRACTICALS Max. Marks: 30
Course Weightage: 02 Credit No. of Contact Hours: 60
Part 1: Spectrophotometry
1. To determine the λmax of KMnO4 and K2Cr2O7 and calculate the energies of two absorption
bands in these molecules in different units.
2. Verify Lambert-Beer’s law
3. Determination of unknown concentration of CuSO4/KMnO4/K2Cr2O7 in a solution using
spectrophotometer.
4. Spectrophotometric determination of Fe (II), using 1, 10-Phenanthroline.
Part 11: Refractometry
1. To determine refractive index of a liquid by using Abbe’s refractometer. 2. To determine percentage composition of a mixture of two liquids by refractometry