Atomic structure: the atom as a nucleus with orbital atoms; interaction with electromagnetic radiation. Bohr theory; atomic spectra of hydrogen and hydrogen like atoms (one electron species); refinements to Bohr theory; the dual nature of electrons; the Heisenberg’s uncertainty principle. The Schrödinger equation: solutions for a particle in a box; the physical significance of the wave function; Solutions of the Schrödinger equation for hydrogen-like atoms, many electron atoms; quantum numbers, radial functions, radial distribution functions, charge clouds and orbitals. Many electron systems: Aufbau principle, energy levels, electron configurations. The periodic table: periodic properties of elements; Atomic size; ionic and crystal radii; Ionization energy; electron affinity; electronegativity.
Types of bonds: ionic; covalent; coordinate; metallic. The ionic bond: structure of ionic solids; coordination numbers; classification of ionic crystal structures and calculation of lattice energies, ionic sizes and salvation energies. The covalent bond: Theories of covalent bonding; Lewis; octet rule; Sidgwick-Powell theory; the valence Shell electron pair repulsion (VSEPR) theory; Valence bond theory and Molecular orbital theory for simple molecules and ions. The metallic bond: Crystal structures of metals. Theories of bonding in metals: free electron theory; valence bond theory; band (molecular) theory; conductors; insulators; semi-conductors: ionic compounds; interstitial alloys; substitutional alloys; super conductivity.Practicals will include proper handling of analyticsl balance, use of standardized solutions, acid base titrations, redox titrations and EDTA titrations