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June 20th, 2016, 08:46 AM
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Syllabus of Chemistry Honours in Calcutta University

Hello sir I am Harsh and I am here as I want to get the Syllabus of the Module I General and Physical Chemistry of Bio-Chemistry Honours of University of Calcutta so will you please provide me the syllabus?

Hey Harsh!!! As per your demand here I am providing you Syllabus of the Module I General and Physical Chemistry of Bio-Chemistry Honours of University of Calcutta

Unit I
1. Atomic Structure

Extra nuclear structure: Bohr’s theory of atomic structure and its limitations, Summerfeld’s modification, application of Bohr’s theory to hydrogen like atoms and ions, Spectrum of hydrogen atom. Quantum numbers. Preliminary idea of de Broglie matter waves, concept of atomic orbital, shapes of s, p and d orbitals, radial and angular probability of s, p and d orbitals (qualitative idea). Many electron atoms, Pauli Exclusion Principle, Hund’s rule of maximum multiplicity, exchange energy, Aufbau (building up) principle and its limitations, Electronic energy levels and electronic configurations of hydrogen like and polyelectronic atoms and ions (concept only), Ground state term symbols of atoms and ions (concept only).

2. Intermolecular forces
a. Ionic bonding
Size effects- radius ratio rules and their limitations. Packing of ions in crystals, Lattice energy (concept only), Born- Lande equation (derivation not required) and its applications; Born-Haber cycle (derivation not required) and its application. Preliminary ideas of solvent energy, polarizing power and polarisibility, ionic potential and Fajan’s rules

b. Covalent bonding
Lewis structures, formal charge, Preliminary idea of Valence Shell Electron Pair Repulsion (VSEPR) Theory, shapes of molecules and ions containing lone pairs and bond pairs. Partial ionic character of covalent bonds, bond moment and dipole moment, Partial ionic character from dipole moment values and electro negativity differences, Preliminary idea of valence Bond Theory ( Heitler- London approach). Directional character of covalent bonds, hybridization, equivalent and non equivalent hybrid orbital, Bent’s rule; Concept of resonance, resonance energy, resonance structures.bonding, non-bonding,antibonding molecular orbitals( concept only) elementary pictorial approach of H2 and O2 molecular orbitals , sigma and pi bonds, multiple bonding. Concept of Bond order, bond length, bond strength, bond energy

c. Weak Chemical Forces
Van der Waal’s forces, ion-dipole, dipole–dipole interactions, London forces, Hydrogen bonding; Effect of chemical forces on physical properties

d. Co-ordination compounds
Double salts and complex salts, Werner’s theory, ambidentate and polydentate ligands, chelate complexes, Naming of co-ordination compounds (up to two metal centres). Isomerism of co-ordination compounds: Constitutional, geometrical and optical isomerism in respect co-ordination numbers 4 and 6. Determination of configuration of cis-, trans-, isomers by chemical methods,

Reference Books
1. General &Inorganic Chemistry-R.P.Sarkar
2. Inorganic Chemistry-R.L.Dutta
3. New Concise Inorganic Chemistry-J.D.Lee

Unit II:
Biophysical properties

(a) Viscosity:
General features of fluid flow (streamlined and turbulent), nature of viscous drag for streamlined motion. Definition of viscosity coefficient. Origin of viscosity of liquids, expression for viscosity coefficient of liquids (with derivation): Poiseuille’s equation, temperature dependence of viscosity coefficient of liquids. Stoke’s law and terminal velocity. Determination of viscosity coefficient of liquids. Diffusion of solutes in solution, Fick’s law.

(b) Surface tension:
Definition, angle of contact, interfacial tension, capillary rise, determination of surface tension, temperature effect.

(c) Preliminary idea of Chemical equilibrium:
Equilibrium constant, Le Chatelier’s principle and its simple applications.

Ionic equilibrium:
Standard solution, Molar, Normal, Molal, Formal and percent strengths, Hydrolysis of weak acids and bases. pKa, pKb, pH, pOH acid- base neutralization curves, Buffer action definition, Henderson -Hasselbalch equation and preparation of buffers, buffer capacity, Solubility product principle and application.

Unit-III
Electrochemistry:

Flow of electrical charge: Electrical conductance, cell constant, specific conductance and equivalent conductance. Variation of equivalent conductances of strong and weak electrolytes with dilution, Kohlrausch’s law of independent migration of ions, ion conductances and ionic mobility, Equivalent conductances at infinite dilution for weak electrolytes and determination of dissociation constants of weak electrolytes from conductance measurements.Basic concepts of electrochemical cell and cell reactions.EMF of cell (no derivation), types of electrode,glass electrode,determination of pH of a solution and potentiometric titration,redox reaction.

Chemical Kinetics

(a) Concepts of rate, rate constant, order and molecularity of a reaction, integrated form of rate expressions; half-life period and its significance.

(b) Pseudo-unimolecular reactions, multi step reactions, rate determining step, zero and fractional orders, rate expressions for complex reactions, Steady-State approximation. Opposing reaction, parallel reaction and consecutive reaction. Temperature dependence of rate constant, Arrhenius’equation, Energy of Activation; Concept of Collision theory and Transition State theory of reaction rate.

(c) Catalytic reactions: Homogeneous catalysis, acid –base catalysis, primary salt effects, Autocatalysis, Adsorption of gases on solids, Langmuir adsorption isotherm, Heterogeneous catalysis, examples.

Reference Books

1. Physical Chemistry-P.C.Rakshit
2. Lehninger Principles of Biochemistry-Nelson &Cox
3. Text Book of Physical Chemistry-K.L.Kapoor(Vol-II,V)
4. Physical Chemistry-Hrishikesh Chatterjee(Vol-I)

Contact Detail:
University of Calcutta  
Senate House, 87/1, College Street, Kolkata, West Bengal 700073
Phone: 033 2241 0071

Last edited by Neelurk; June 29th, 2020 at 10:11 AM.
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