ChE104 INORGANIC AND PHYSICAL CHEMISTRY
| Lectures: 3 Periods/Week |
Sessional Marks: 30 |
| University Exam: 3 Hours |
University Examination Marks: 70 |
PART-A: INORGANIC CHEMISTRY
UNIT-I
Mole concept, oxidation numbers, balancing of equations, stoichiometry (Mass-mass, Mass-volume, Volume-volume)
Chemical bonding- ionic and covalent bonding, Molecular orbital and valence bond approaches for diatomic molecules, VSEPR theory, Hybridization and shapes of molecules, Resonance, dipole moment, structure parameters such as bond length, angle & energy, Hydrogen bonding, Vanderwaal's interactions, Ionic solids, Ionic radii, lattice energy (Born-Haber cycle), Metal-ligand bonding and importance,
Planck's Quantum theory, Wave particle duality, Uncertainty principle, Quantum mechanical model of hydrogen atom, Periodic Table and properties, Ionization energy, Electron negativity, Atomic size, Coordination complexes, nomenclature, crystal field theory, color, geometry and magnetic properties.
UNIT-II
Chemistry of representative s and p- block elements: Electronic configuration, general properties and oxidation states, Oxides, Halides and Hydrides of Alkali, Alkaline earth metals, Boron-Aluminum, Carbon-Silicon, Nitrogen-Phosphorus, Sulphur.
d- block elements: Electronic configuration, general characteristics and oxidation states.
Inner transition elements: General discussion, oxidation states and Lanthanide contractions.
PART-B: PHYSICAL CHEMISTRY
UNIT-III
Thermodynamics: First law, reversible and irreversible processes, internal energy, enthalpy, Kirchoff's equation, heat of reaction, Hess's law, heat of formation,
Second law, entropy, free energy and work function. Gibb's-helmholtz equation, Clausius-Clapeyron equation, free energy change and equilibrium constant, Trouton's rule, Third law of thermodynamics.
Phase and chemical equilibria: Phase rule, phase diagram of water, two component systems with a simple eutectic-Pb, Ag system and construction of phase diagram by thermal analysis.
Colligative properties: Raoult's law, elevation of boiling point, depression of freezing point, osmotic pressure (no thermodynamic derivations) elementary treatment of vapor pressure.
Chemical equilibria: Reversible reactions, law of mass action, Lechatelier principle, Effect of temperature on equilibrium-Van't Hoff equation, Ionic Equilibria: Solubility, solubility product, common ion effect, Hydrolysis of salts, pH, buffer and their application in chemical analysis, equilibrium constants (Kc, Kp, Kx) for homogeneous reactions.
UNIT-IV
Galvanic cells: Thermodynamics of galvanic cells, half cell potentials, e.m.f. of cells, Nernst equation, Commercial applications of galvanic cells
Electrolytes: Conductance, effect of concentration, Kohlrausch law.
Kinetics of chemical reactions: Rate constant, order of reaction, molecularity, activation energy, Zero, First and Second order kinetics and elementary enzyme reactions.
Catalysis: Characteristics of catalyst, promoter, negative catalyst, catalytic poison, heterogeneous catalysis, intermediate compound formation theory, activated complex theory, acid, base and enzyme catalysis.
Text Books
- A new concise Inorganic chemistry, J.D.Lee, ELBS and Van, 3rd edition Nostrand Reinhold Co. Ltd., London.
- Physical Chemistry, P.W.Atkins, 3rd Edition, Oxford University Press.
Reference Books
- University General Chemistry, C.N.R.Rao, MacMillan India.
- Elements of Physical Chemistry, Samuel Glastone and David Lewsis, 2nd edition MacMillan & Co., London.
- Principles of Chemistry, Paul Ander & Anthony J.Sonnessa, Collier-MacMillan Ltd., London.