1. Metal ligand bonding in Transition metal complexes:
Limitations of valance bond theory, an elementary idea of crystal field theory, crystal field splitting in octahedral, tetrahedral and square planer complexes, factors affecting the crystal field parameters.
2. Magnetic Properties of Transition Metal complexes:
Types of magnetic behaviours, method of determining magnetic susceptibility, spin only formula, L-S coupling, correlation of m and meffective values, orbital contribution to magnetic moments, applications ofmagnetic moment data for 3d-metal complexes.
CHE C – 512
Paper II : Organic Chemistry
15 Hrs (1 Hrs/week)
Introduction and classification, osazone formation, mutual transformation, epimerisation, cyclic structure of glucose and fructose, mutarotation, General idea about disaccharides andpolysaccharides, structure of sucrose, maltose, lactose and starch.
Introduction, classification of amino acids, acid base behaviours, iso-electric point of amino acids, a-amino acid-preparation, properties and physiological importance, peptide synthesis – classical and solid phase . End group analysis of amino acids, detection, classification and importance of proteins.
Introduction, colours and constitution, chromospheres, auxoxhrome and valence bond theory, synthesis of methyl orange, congored, malachite green, crystal violet, phenolphthalein, fluorescein, indigo
CHE C – 513
Paper III: Physical Chemistry
30 Hrs (2 Hrs/week)
Black body radiation, Plank’s radiation law, photoelectric effect, heat capacity of solids, Bohr’s model of Hydrogen atom (no derivation) and its defects, Compton Effect
De-Broglie hypothesis, Heisenberg’s uncertainty principle, sinusoidal wave equation, Hamiltonian operator, Schrödinger equation and its importance, physical interpretation of the wave function, postulates of quantum mechanism, particle in one dimensional box.
Schrodinger wave equation for H- atom, separation into three equations (without derivation), quantum numbers and their importance, Hydrogen like wave functions, radial wave function, angular wave function
Molecular orbital theory, basic idea- criteria for forming MO from AO, construction of MO’s by LCAO-H2+ ion, calculation of energy levels from wave function, physical picture of bonding – anti bonding, wave function, concept of s, s*, p, p*orbital’s and their characteristics. Hybrid orbitals – sp, sp2, sp3, calculation of coefficient of AO’s used in these hybrid orbitals. Introduction to valance bond models of H2, comparison of MO and VB models.
Introduction; electromagnetic radiation of the spectrum, basic features of different spectrometers, statement of Born-Oppenheimer Approximation, degree of freedom
Di atomic molecules, energy levels of a rigid rotors (semi classical principles), Selection rules, spectral intensity, distribution using population distribution (Maxwell-Boltzmann distribution) determination of bond length, qualitative description of non-rigid rotor, isotope effect.
Infra red spectrum, energy levels of simple harmonic oscillators, selection rules, purevibrational spectrum, intensity, determination of force constant and qualitative relation of force constant and bond energies, effect of anharmonic motion and isotope on spectrum, idea of vibrational frequencies of different functional groups.
Concept of polarizability, pure Rotational and pure vibrational Raman spectra of diatomic molecules, selection rules
CHE C – 514
Laboratory Course in Chemistry
Synthesis and Analysis
a.Preparation of sodium trioxalato ferrate (III) Na3[Fe(C2O4)3] and determination of its composition by permangnetometry
b.Preparation of [Ni(II)-(DMG)2]
c.Preparation of Copper tetra-amine complex, [Cu(NH3)4]SO4
d.Preparation of cis and trans bisoxalato diaqua chromate (III) ion.
Separation of fluorescein and methyl blue; leaf pigments from spinach leaves.
Analysis of an organic mixture containing two solid components using water or NaHCO3 for separation and preparation of soluble derivatives.
a.Conductometrically determine the strength of the given acid using standard alkali solution
b.Conductometrically determine the solubility of a sparingly soluble electrolyte
c.Conductometrically determine the saponification of ethyl acetate
d.Conductometrically determine the ionisation constant of a weak acid
e.To titrate potentiometrically the given FAS ferrous ammonium sulphate solution using KMnO4 / K2Cr2O7 as titrant and calculate the redox- potential of Fe++/ Fe+++ system on the hydrogen scale.
1.Organic Chemistry, I. L. Finar, ELBS Publication
2.Organic Chemistry, Morrison and Boyed, Prentice-Hall.