Chemistry General Syllabus of Kalyani University

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B.Sc Chemistry General Syllabus:

Part – I Paper – I (Theory) - 100 marks
Group A : General Chemistry (50 marks)
Group B : Organic Chemistry (25 marks)
Group C : Physical Chemistry (25 marks )

Part – II Paper – II(Theory) - 100 marks
Group A : Inorganic Chemistry (50 marks)
Group B : Organic Chemistry (25 marks)
Group C : Physical Chemistry (25 marks )

Paper – III (Practical) - 100 marks
Group A : Inorganic Chemistry (50 marks)
Group B : Organic Chemistry (50 marks)

Part – III Paper – IV
Theory – 60 marks
Group A : Principles of biological chemistry
Group B : Application oriented chemistry
Group C : Catalysis and Phase rule
Practical -- 40 marks
Physical Chemistry
Kalyani Univ B.Sc Chemistry General syllabus
PART – I
1. Atomic structure (extra nuclear) 12L
Bohr’s atomic model and its limitations, Sommerfeld’s modifications, de Broglie
matter waves, Heisenberg uncertainty principle and its significance. Schrodinger
wave equation, quantum numbers, ra dial and angular wave functions, probability
distribution curves, shapes of orbitals (mathematical details excluded), Aufbau and
Pauli exclusion principles, Hund multiplicity rule, sequence of energy levels,
electronic configuration of atoms, ground state term symbols of atoms and ions.
2. Periodic properties 10L
Atomic and ionic radii, crystal radii, covalent radii, different electro negativity scales,
ionization, enthalpy, electron attachment enthalpy and their periodic trends, screening
effect, effective nuclear charge, Slater’s rule, inert pair effect.
3. The nature of chemical bond – 1 23L
Ionic bonding : size effect, radius ratio rules and their limitations, atomic packing, hcp
and ccp arrangements, voids in crystal lattice, packing ef ficiency, some ionic crystal
lattices : rock salt, zinc blende, wurtzite and fluorite; layer lattice, lattice energy,
Born-Lande equation, Born-Haber cycle and its applications, polarizing power,
polarizibility, Fajans’ rule and its applications.
Some mixed oxide structure : perovskite, ilmenite and spinels, stoichiometric crystal
defect : Frenkel and Schottky defects – electrical property – concentration of Schottky
defect.
Bonding in metals : free electron and band models of solids (qualitative idea),
conductors, insulators and semiconductors – their band diagrams, weak chemical
forces : hydrogen bonding and its importance in biological systems, vander Waals
forces.
Group B : Nuclear chemistry and radio activity, chemistry of elements, acid -
bases and solvents (37½ Marks ) 45 L
4. Nuclear chemistry and radioactivity 10 L
Nuclear stability, nuclear binding energy, mass defect and packing fraction,
nuclear forces, meson field theory, artificial radi o activity, different types of nuclear
reactions, fission and fusion, nuclear energy, nuclear fuels, trans uranium elements,
radio isotopes in structure determination, study of reaction mechanisms, solubility
determination, radio carbon dating.
5. Chemistry of elements : 23L
a) Comparative study : I) Al, Ga, In and Tl, i i) Si, Ge, Sn and Pb – group trends
with reference to electronic configuration, size, oxidation states and in
compounds such as hydrides, oxides, oxyacids, halides and complexes
b) Diagonal relationship : Li and Mg; Be and Al; B and Si.
c) Extraction, purification, uses and essential compounds of Ti, V, Cr, Ni and U.
d) Preparation, properties, bonding and stereochemistry of following except
where specific aspects are mentioned
i) electron deficiency and acceptor behaviour of boron; diboranes,
borohydrides, boron nitrides, perborates and its oxidizing behaviour.
ii) Fluoro carbons – Their effect on earth’s ozone shields, freons and
Teflons, silicones; structural properties of various silicates.
iii) Hydrazine, hydroxylamine and hydrazoic acid; phosphazenes;
iv) Peracids and per salts of sulphur and halogens and their applications.
v) Structure, bonding and reactivity of xenon fluorides.
6. Acid – bases and solvents 12L
Lewis concept of acids and bases, HSAB principle, PH and its calculations,
buffer solution-buffer effect; neutralization curves, acid-base indicator, choice of
indicator-indicator error.
Solvent properties of water and liquid ammonia -reactions in liquid ammonia,
levelling and differentiating solvents.
PAPER – II Full Marks : 75
Group A (Organic) : Bonding features, acids and bases, reaction mechanism I &
II, stereochemistry – I, Synthesis, properties (37½ Marks)
45 L
1. Bonding features in organic molecules : 7 L
Formation of and bonds, hybridization, conjugation, hyper conjugation,
inductive and field effects, resonance, bond distance, bond angle, bond energy,
bond polarities, bond Polaris ability, steric and angular strain, orbital pictures of
representative compounds .
2. Organic acids and bases : 3 L
Bronsted and Lewis concepts, acid -base catalysis, effect of structure and
substitutes, medium on relative acid and base strength of substituted alkenes,
alkynes, alcohols, phenols, enols, carbonyl compou nds, carboxylic acids,
amines, HSAB principle.
3. Tauto merism : 2L
Prototropic shifts, ring-chain tautomerism, valence tautomerism, relative
stability of tautomers with reference to bond energy, hydrogen bonding,
resonance energy, solvent effects.
4. Reaction mechanism – I : 7 L
Classification of reagents: electrop hiles and nucleophiles, reaction intermediates
: carbocations, carbanions, radicals, carbenes, nitrenes and benzynes.
Classification of reaction : substitution, addition, elimination, rearrangement;
Some methods of determining reaction mechanism : Kinetic study, study of
intermediates, crossover experiment, isotope labelling, kinetic isotope effects;
Thermodynamic requirements of reaction : ∆G, ∆H, ∆S, free energy profile
diagrams for one step and two step reaction.
5. Stereochemistry – I : 11 L
Representation of molecules in Fischer, Newman, Sawhorse and flying wedge
notations and their inter conversions.
Elements of symmetry : simple axis, plane of symmetry, center of symmetry,
alternate axis of symmetry, chirality, optical activity, specific rotation, optical
purity;
Stereoisomerism : enantiomers and diastereo-isomers, dl / meso, D / L, R / S,
threo / erithro, syn / anti and E / Z notations; isomerism involving two (AA and
AB types), three (ABA, ABC systems) chirl centers; conformation analysis of
ethane, propane, butane, propyl halide, 1, 2 – dihalo ethane, 1, 2 – glycols.
6. Reaction mechanism – II : 11 L
Nucleophilic substitution at a saturated carbon : S N1, SN2, SN21, SN11
mechanisms; neighbouring group participation; aromatic nucleophilic
substitution, cine substitution; nucleophilic substitution at carbonyl carbonl
(carboxylic acids and derivatives) tetrahedral mechanism; electrophilic addition
to C – C multiple bonds, aromatic electrophilic substitution.
Elimination reaction : , and - eliminations; E1, E 2 and E1cB mechanism,
elimination vs substitution.
7. Synthesis, physical properties and reactions of following classes of compounds 4L
Alkanes, alkenes, alkadienes and arencs, alkyl halides, vinyl halides, allyl and
benzyl halides.
Group B (Physical): Kinetic theory and gaseous state, chemical thermodynamics,
chemical equilibrium, colligative properties, liquid state (37½ Marks)
45L
1. Kinetic theory and gaseous state : 12L
Concept of temperature and pressure, nature of distribution of veloc ities in one,
two and three dimensions, Max well’s distribution of speeds (no derivation) and
translational kinetic energy, distribution curves, calculation of number of
molecules having energies E; calculation of average speed, most probable
speed and root mean square speed; principle of equipartition of energy and its
application to calculate the classical limit of molar heat capacity of gases;
variation of molar heat capacity with temperature.
Collision diameter, frequency of binary collisions (simila r and different
molecules), mean free path, wall collision and rate of effusion; viscosity of
gases. Real gases : compressibility factor, deviation from ideality, coefficient of
thermal expansion and coefficient of compressibility, vander Waals and virial
equation of state, critical phenomena and critical constants, reduced equation of
state, significance of second virial coefficient, Boyle temperature;
intermolecular forces (Keesom, Debye, London) and potentials, liquifaction of
gases.
2. Chemical thermodynamics : 16 L
Definition of thermodynamic terms : intensive and extensive variables, isolated,
open and closed systems, concept of heat and work, thermodynamic processes :
cyclic, reversible, irreversible, isothermal, adiabatic process, thermodynamic
functions and their differentials, zeroth law of theromodynamics; fi rst law of
thermodynamics, internal energy (U), Joule’s experiment and its consequences,
Joule-Thomson experiment and its consequences, enthalpy (H), relation between
Cp and Cv, calculation of work (w), quantity of heat (q), dU and dH for
expansion of ideal and van der Waals gases, gas under isothermal and adiabatic
conditions for reversible and irreversible processes including free expansion.
Heat changes during various physico -chemical processes at constant pressure /
constant volume, Hess law, Kirchoff’s relation, concept of standard state, bond
dissociation energy, Born-Haber cycle for calculation of lattice energy.
Spontaneous process, heat engine, Carnot cycle and its efficiency, statements of
second law, refrigeration cycle, thermodynamic scale of tem perature, entropy as
a state function, Clausius inequality, calculation of entropy changes in different
processes, molecular interpretation of entropy.
Gibbs function (G) and Helmholtz function (A), criteria of thermodynamic
equilibria and spontaneity, va riation of G and A with P, V and T,
Thermodynamic equation of state, Clausius -Clapeyron equation, equilibrium
between different phases, system of variable composition, partial molar
quantities, chemical potential of a component in an ideal mixture,
thermodynamic functions of mixing of ideal gases, Gibbs -Duhem equation,
variation of chemical potential with T, P and mole fraction, thermodynamics of
real gases – fugacity and activity determination, Nernst heat theorem, Third law
of thermodynamics and concept of residual entropy.
3. Chemical equilibrium : 4L
Chemical equilibria in homogeneous and heterogeneous systems, vant Hoff
reaction isotherm (deduction from chemical potential, equilibrium constant and
standard Gibb’s free energy change), Le chatel ier’s principle (thermodynamic
approach) and its application. Vant Hoff equation and its applications.
4. Colligative properties of solution 5 L
Dilute solutions, Raoult’s law and Henry’s law, colligative properties,
thermodynamic derivation of coll igative properties of solutions and their inter
relationships, abnormal colligative properties
Liquid state : 8 L
Qualitative treatment of structure of liquid state, physical properties of liquids
including their method of determination vapour pressure, surface tension,
surface energy, excess pressure, capillary rise method of determination of
surface tension, work of cohesion and adhesion, spreading of liquid over other
surface, vapour pressure over curved surface, temperature dependence of
surface tension.
General features of fluid flow (stream line flow and turbulent flow, Reynold
number), nature of viscous drag from stream line motion, Newton’s equation,
viscosity coefficient, Poiseuille equation (with derivation), temperature
dependence of viscosity coefficient of liquids and comparison with that for
gases, Stoke’s law and terminal velocity, determination of viscosity coefficient
of liquids; Refractive index, liquid crystals (elementary discussion on
classification, structure and properties) .
PAPER – III (Organic Practical) Full Marks - 50
Time : 6 hours
1. Qualitative analysis of single organic compound 25
i) Detection of special elements (N, Cl, Br, I, S) by Lassigne test.
ii) Determination of m.p/b.p of the given compound
iii) Solubility test
iv) Determination of the following functional groups by systematic anal ysis :
phenolic OH, aldehyde, ketone, carboxylic acid ( -COOH), aromatic nitro,
aromatic amine (10 only), amido (-CONH2) anilido (-CONH Ph)
v) Preparation of at least one solid derivative of the given sample,
determination of melting point of the prepared der ivative (to be submitted
for evaluation)
2. Organic preparation : 15
a) Preaparation of m-dinitrobenzene from nitrobenzene
b) Preparation of p-nitro acctanilide from acetanilide
c) Oxidation of benzoin to benzil
d) Reduction of anthraquinone to anthrone
e) Preparation of adipic acid from cyclohexanol / cyclohe xa none
f) Preparation of dibenzal acetone from benzaldehyde
g) Preparation of 2-iodo benzoic acid from anthranilic acid
h) Preparation of methyl red
3. Laboratory note book 5
4. Viva-Voce 5
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