Course

Unit I

Atomic Structure I: Bohr model of hydrogen atom, Bohrs equation for the energy of electron in hydrogen atom, the hydrogen spectrum, limitations of Bohr theory, photoelectric effect, idea of de Broglie matter waves, Heisenbergs uncertainity principle and its significance

Unit II

Atomic Structure II: Schrodinger wave equation (derivation not expected), wave functions, significance of ? (psi) and ?2, atomic orbitals, Nodal planes in atomic orbitals, quantum numbers (n, l, m), Zeeman effect, Stern-Gerlac experiment, spin quantum number (s), shapes of s, p and d orbitals. Aufbau and Paulis exclusion principles, Hunds rule, energy level diagram of a multielectron atom, concept of effective nuclear charge, Slaters rules and applications, Electronic configuration of atoms.

Unit III

Periodic Properties: Classification of elements into s, p, d, and f-blocks, cause of periodicity. Atomic radius: Covalent, ionic and Vanderwaals radii. Variation in a group and in a period. Variation of ionic radii in isoelectronic ions. Ionization enthalpy: Successive ionization enthalpy, factors affecting ionization enthalpy, variation in group and in a period. Electron gain enthalpy: Successive electron gain enthalpy variation in period and in a group. Electronegativity: Variation of electronegativity in a group and in a period. Factors determining electro negativity (charge on the atom and hybridization). Pauling, Mulliken and Allred-Rochow scale of electronegativity. Applications of electronegativity.

Unit IV

Chemical Bonding-I : Ionic bond: Factors that favor the formation of ionic bonds, Lattice energy, Born-Landes equation (no derivation), Born-Haber cycle, setting up of Born-Haber cycle for 1:1 ionic solids. Numerical calculations of LE and EA based on Born-Haber cycle for 1:1 ionic solids, uses of Born-Haber cycle. Role of lattice energy and hydration energy and their importance in the context of stability and solubility of ionic solids. Covalent bond: Factors favoring the formation of covalent bond (ionization energy, electron affinity, electronegativity, nuclear charge, inter nuclear distance and number of valence electrons). Valence bond approach explanation with examples to illustrate valence bond approach. Sigma and Pi bonds. Fajans rules of polarization and their explanation. Bond length, bond order, bond energy and their significance, polarity of covalent bonds, polar and non-polar molecules, Dipole moment and polarity of molecules to be explained by taking HCl, CO2, CCl4 and H2O as examples.

Unit V

Chemical Bonding II: Hybridization-directional property and geometry of sp, sp2, sp3, sp3d and sp3d2 hybrid orbitals with examples respectively. VSEPR theory. Coordinate bond: with examples. Molecular Orbital Theory: An elementary account of MOT, linear combination of atomic orbitals (no mathematical approach). Bonding and antibonding molecular orbitals, conditions for the combination, energy levels of molecular orbitals, Molecular orbital structures and bond orders of simple molecules and ions, prediction of magnetic properties .

OBJECTIVES: To develop an understanding of principles of atomic structure and chemical  bonding. To develop an understanding of the Periodic trends and to relate the properties of compounds in terms of their chemical bonding.

Course Outcome:

CO-PO Mapping:

TEXTBOOKS:1. J. D. Lee, Concise Inorganic Chemistry, 5th edn., Blackwell Science, London 2. B. R. Puri, L. R. Sharma, Kalia, Principles of Inorganic Chemistry, Milestone Publishers, New Delhi 3. B. R. Puri, L. R. Sharma, M. S. Pathania, Elements of Physical chemistry, Vishal Pub. Co. JalandharREFERENCES:1. C. N. R. Rao, University General Chemistry, Macmillan, India 2. F. A. Cotton, G. Wilkinson and P.L. Gaus, Basic Inorganic Chemistry, 3 rdedn., John Wiley3. D. F. Shriver and P. W. Atkins, Inorganic Chemistry, 3 rdedn., Oxford University Press 4. B. Douglas, D. Mc Daniel, J. Alexander, Concepts and models in Inorganic Chemistry