Unit 1: Atomic structure[14 h]Bohrs model of hydrogen atom, Ritz combination principle, hydrogen spectrum, Bohr-Sommerfeld theory. Plancks quantum theory of radiation, dual character of electrons – de Broglies equation, Heisenbergs uncertainty principle, photoelectric effect, Compton, Zeeman and Stark effects. Schrodinger wave equation, Eigen values, significance of wave function (? and ?2) and quantum numbers. Schrodinger wave equation for hydrogen and hydrogen-like systems, probability distribution of electrons around the nucleus, distribution of electrons in orbitals, shapes of atomic orbitals – s, p, d and f. Aufbau principle, Hunds rule, Paulis exclusion principle, electronic configuration of elements. Unit 2: Chemical bonding[16 h]Electrovalency and ionic bond formation, lattice energy. Born-Lande equation and Born-Haber cycle and their applications, solvation enthalpy and solubility of ionic compounds. Covalent bonding, formation of H2, orbital theory of covalency. Hybridisation VSEPR theory, sigma and pi bonds, formation of covalent compounds. Properties of covalent compounds. Molecular orbital theory homo diatomic molecules and hetero di and triatomic molecules. Polar and non-polar covalent bonds, polarization of covalent bond – polarizing power, polarisability of ions and Fajans rule, dipole moment, percentage ionic character from dipole moment, dipole moment and structure of molecules. Co-ordinate covalent compounds and their characteristics. Metallic bond – free electron, valence bond and band theories. Unit 3: Structure and Bonding in Solids[14 h]Crystalline and amorphous solids, isotropy and anisotropy, indices – Miller indices, space lattice and unit cell, types of crystals – molecular, covalent, metallic and ionic crystals. Close packing of spheres hexagonal, cubic and body centered cubic packing density, coordination numbers, tetrahedral and octahedral holes. Body centered and primitive structures. Interstices in packing. Defects in crystals stoichiometric, non-stoichiometric, extrinsic and intrinsic defects. Bonding in crystals – metallic, ionic and covalent bonding. Crystal systems – Bravais lattices, reciprocal lattice, interplanar spacing in different crystal systems and fractional coordinates. Ionic solids – structures of MX, MX2 and MX3. Unit 4: Acids, Bases and Non-aqueous solvents[10 h]Conjugate acids and bases, hard and soft acids and bases – Pearsons concept, HSAB principle and its application. Buffer solutions. Non-aqueous solvents – general characteristics of non-aqueous solvent – melting point, boiling point, latent heat of fusion and vaporization, and dielectric constant. Reactions in non-aqueous solvents like liquid ammonia, liquid SO2 and liquid HF – complex formation, redox, precipitation and acid base type. Unit 5: Chemical Analysis and Stoichiometric Calculation [6 h]Titrimetry – fundamental concepts, theory of indicators. Acid base, redox, precipitation and complexometric titrations. Problems based on stoichiometry. Gravimetry principle and calculations involving estimation of barium, calcium and nickel. Data analysis, significant figures, precision and accuracy. Types of errors, mean and standard deviation.
