1. Structure of Atom:
Black body radiation, Photoelectric effect, Bohr's atomic model and its application to hydrogen atom, Limitations of Bohr's atomic model, Bohr's Sommerfield model of atom, deBroglie hypothesis, Experimental verification of wave nature of atom, Heisenberg's uncertainty principle, wave mechanic,,1 model of atom, Postulates of quantum and Schrodinger's Wave Equation, Derivation and importance of equation, Eigen values and Eigen functions, Bornoppenhemer approximations, Physical significance of the wave function. Quantum numbers. Aufbau principle. Electronic structure of various elements having abnormal configurations - possible reasons for doing so.
2. Periodicity:.
Periodicity of properties of elements -Atomic Radii, Ionization Potential, Electron affinity, electro negativity, magnetic properties. 3. Chemical Bonding:
(a) Recapitulation of different types of bond formation and only elementary concept to explain the nature of bond formation (Nature of the bonds between elements and electronic configuration of elements forming the bonds) - a correlation and its reasons ­interpretation in terms of electro negativity. Size ofthe atom in the bonded state (ionic and covalent bonds).
(b) Structure of elements (Non-metals) in solid state. Structure of non-metal in their various allotropic forms (diamond, graphite, fluorine, nitrogen and phosphorous, oxygen and sulphur.
4. (a) Structure of very simple molecules of non-metals (eg, AB" AB" AB4. AB, and AB, type; A and B, both non metals; A-non metal and metal).
(b) The structure of above type molecules and their approximate correlation with the electronic structure of the element A and B. Concept of hybridization, VSEPR theory. Their strong and weak points-Partial Ionic character in a bond and electron negatively. Inference of Ionic character of bond in the molecular properties. Gradation in properties of the compounds along the group in the periodic table. Polarizability of an atom is a bonded state and its effect on the molecular properties like solubility etc. of a compound. Lattice forces and solubility.
5. Bond energy and stability of Ionic state of elements in their compounds. Inert pair effect and its relationship with the oxidising and reducing properties of various elements.
Non-metals:
6. Hydrogen - general Chemistry, Hydrogen Bond and its effect on the properties of compounds. General chemistry of Water and hydrogen peroxide.
7. Chemistry of B, C, and Si. General survey of their rec trends in their properties and their explanations on the electronic structure. Special emphasis on those properties which show diagonal relationship and which are abnormal.
8. Chemistry of N, P and As. General survey of their reactions. Tendancy of their ion formation and correlation with electronic structures. Chemistry of nitrogen halides, NH3, PH3, AsH3 oxides and oxyacids. The trends in their properties with special emphasis on abnormal properties down the group and across the periodic table and their correlation with electronic structures. Liquid NH3 as a non aqueous solvent.
9. Chemistry of oxygen and sulphur-General survey of their reactions. Trend in their properties down the group. Difference among the properties of oxygen, sulphur and selenium their reasons based on the electronic structures. Oxides of and its oxyacids. General survey of various oxides and sulphides. Thiosulphates as an analytical reagent.
10. Chemistry of halogens - General survey of the reactions, in their properties and their explanation on the basis oftheir electronic structure. oxides and oxyacids.lnterhalogen. and Iodimetry. Properties ofl+ion.
11. A general discussion. about hydrides, halides, oxide oxyacids, Borides, Carbides and' silicides, Various and silicates their structures glass, molecular sieves, seolites, thiocanats (SC,N) as an analytical ion.
12.Chemistry of p-block elements with special reference to Ga, In, TI, Ge, Sn, Pb and As, Sb, Bi. General characteristics, their important compounds, preparation, properties, uses and structures.
13. General reactions of inert gases, their simple compounds and structures. Analytical
14. (a)Caliberations, error and deviations, significant figures.
(b) Basic principles involved in the qualitative analysis of anions and cations.
(c) Numerical problems pertaining to volumetric analysis (acidbase, oxidation-reduction titrations).