Introduction, radius ratio rules- calculation of limiting radius ratio values for coordination number 3,4 ,6 and 8; close packing; classification of ionic structures, ionic compounds of the type AX (ZnS, NaCl, CsCl) and AX2 (CaF2-Fluorite), limitations of radius ratio rule; calculation of lattice energy, factors affecting lattice energy, the Born Haber cycle and its application; solvation energy and solubilities of ionic substances; stoichiometric and non stoichiometric defects.
The Lewis theory, octet rule, explanations for the failure of octet rule,exceptions to octet rule; valence bond theory (Heitler and London approach) and its limitations; resonance; directional character of covalent bond, various types of hybridization ( sp, sp2, sp3, sp3d,sp3d2, dsp2, sp3d3) and shapes of molecules; VSEPR theory, isoelectronic principle, examples using VSEPR theory, polarizability of ions, Fajan’s rule and consequences of polarization, dipole moment and percentage ionic character in covalent compounds ( electronegativity difference and dipole moment method), bond energy and bond length.
Introduction, LCAO approach, combination of orbitals (s-s, s-p, p-p, non-bonding combination of orbitals), examples of molecular orbital treatment for homonuclear diatomic molecules – H2+, H2, He2, B2, C2, N2, Be2, O2, O2+1, O2-1, O2-2, F2, examples of molecular orbital treatment for heteronuclear diatomic molecules- NO, NO+, CO, CO+, CN molecule, comparison of VBT and MOT.
Multicentred bonding in electron deficient molecule; general properties of metals– conductivity, lustre, malleability, ductility, crystal structures; theories of bonding in metals – free electron theory, valence bond theory and band theory – conductors, insulators and semi-conductors; superconductors.
Van der Waal’s forces: ion-dipole forces, dipole-dipole interactions, induced dipole interactions, instantaneous dipole – induced dipole interactions, repulsive forces.
Hydrogen bond: types, theories and properties of H-bond, effects of H-bond on physical properties.