a) Discovery of sub-atomic particles (electron, proton and neutron) a) Discovery of sub-atomic particles (electron, proton and neutron) b) Thomson Model of Atom and Its Limitations b) Thomson Model of Atom and Its Limitations c) Rutherford Model of Atom and Its Limitations c) Rutherford Model of Atom and Its Limitations d) Nature of electromagnetic radiation d-1) photoelectric effect e) Spectrum of hydrogen atom e-1) Bohr model of hydrogen atom - its postulates, derivation of the relations for energy of the electron and radii of the different orbits, limitations of Bohr’s model e-1) Bohr model of hydrogen atom - its postulates, derivation of the relations for energy of the electron and radii of the different orbits, limitations of Bohr’s model f) Dual nature of matter f-1) de-Broglie’s relationship f-2) Heisenberg uncertainty principle g) Elementary ideas of quantum mechanics g-1) quantum mechanical model of atom, its important features, concept of atomic orbitals as one electron wave functions; Variation of ? and ?2 with r for 1s and 2s orbitals; various quantum numbers (principal, angular momentum and magnetic quantum numbers) and their significance; shapes of s, p and d - orbitals, electron spin and spin quantum number g-1) quantum mechanical model of atom, its important features, concept of atomic orbitals as one electron wave functions; Variation of ? and ?2 with r for 1s and 2s orbitals; various quantum numbers (principal, angular momentum and magnetic quantum numbers) and their significance; shapes of s, p and d - orbitals, electron spin and spin quantum number g-1) quantum mechanical model of atom, its important features, concept of atomic orbitals as one electron wave functions; Variation of ? and ?2 with r for 1s and 2s orbitals; various quantum numbers (principal, angular momentum and magnetic quantum numbers) and their significance; shapes of s, p and d - orbitals, electron spin and spin quantum number g-1) quantum mechanical model of atom, its important features, concept of atomic orbitals as one electron wave functions; Variation of ? and ?2 with r for 1s and 2s orbitals; various quantum numbers (principal, angular momentum and magnetic quantum numbers) and their significance; shapes of s, p and d - orbitals, electron spin and spin quantum number g-2) Rules for filling electrons in orbitals - aufbau principle, Pauli’s exclusion principle and Hund’s rule, electronic configuration of elements, extra stability of half-filled and completely filled orbitals. g-2) Rules for filling electrons in orbitals - aufbau principle, Pauli’s exclusion principle and Hund’s rule, electronic configuration of elements, extra stability of half-filled and completely filled orbitals.
1. Physical Chemistry 2. Atomic Structure 3. Chemical Bonding and Molecular Structure 4. Chemical Thermodynamics 5. Solutions 6. Equilibrium 7. Redox Reactions and Electrochemistry 8. Electrochemical cells 9. Chemical Kinetics 10. Surface Chemistry INORGANIC CHEMISTRY