Syllabus (CHEMISTRY)

Course Type: MAJ-4

Semester: 4

Course Code: BCEMMAJ04C

Course Title: Inorganic Chemistry – II

(L-P-Tu): 4-2-0

Credit: 6

Practical/Theory: Combined

Course Objective: COURSE OBJECTIVE OF MAJOR - 4: The syllabus of Major -4 has been designed to provide the students with in-depth knowledge of Chemical bonding, including Ionic bonding, Covalent Bonding, Co-ordinate covalent bonding and other weak bonding interactions. Thi

Learning Outcome: COURSE OUTCOMES OF MAJOR – 4: CO- 4.1 Thorough understanding of Chemical Bonding with special Emphasis on Ionic, Covalent bonding and Concepts of weak bonds like Hydrogen Bond, van der Waals bond. CO- 4.2 Understanding the concepts of Molecular Orbit

THEORY:

CHEMICAL BONDING-I: (20 L)

1. Ionic bond: General characteristics, types of ions, size effects, radius ratio rule and its application and limitations. Packing of ions in crystals. Born-Landé equation with derivationn for lattice energy, Madelung Constant, Born-Haber cycle and its application, Solvation energy. Defects in solids (elemementary idea). Solubility energetics of dissolution process.

2. Covalent bond: Polarizing power and polarizability, ionic potential, Fajan’s rules. Lewis structures, formal charge. Valence Bond Theory. The hydrogen molecule (Heitler-London approach), directional character of covalent bonds, hybridizations, equivalent and non- equivalent hybrid orbitals, Bent’s rule, Dipole moments, VSEPR theory, shapes of molecules and ions containing lone pairs and bond pairs (examples from main groups chemistry) and multiple bonding (σ and π bond approach).

Chemical Bonding-II (25L)

1. Molecular orbital concept of bonding (The approximations of the theory, Linear combination of atomic orbitals (LCAO)) (elementary pictorial approach): sigma and pi- bonds and delta interaction, multiple bonding. Orbital designations: gerade, ungerade, HOMO, LUMO. Orbital mixing,. MO diagrams of H2, Li2, Be2, B2, C2, N2, O2, F2, and their ions wherever possible; Heteronuclear molecular orbitals: CO, NO, NO+, CN-, HF, BeH2, CO2 and H2O. Bond properties: bond orders, bond lengths.

2. Metallic Bond: Qualitative idea of valence bond and band theories. Semiconductors and insulators, defects in solids.

3. Weak Chemical Forces: van der Waals forces, ion-dipole forces, dipole-dipole interactions, induced dipole interactions, Instantaneous dipole-induced dipole interactions. Repulsive forces, Intermolecular forces: Hydrogen bonding (theories of hydrogen bonding, valence bond treatment), receptor-guest interactions, Halogen bonds. Effects of chemical force, melting and boiling points.

CO-ORDINATION CHEMISTRY-I: (15 L)

Coordinate bonding: double and complex salts. Werner’s theory of coordination complexes, Classification of ligands, Ambidentate ligands, chelates, Coordination numbers, IUPAC nomenclature of coordination complexes (up to two metal centers), Isomerism in coordination compounds, constitutional and stereoisomerism, Geometrical and optical isomerism in square planar and octahedral complexes.

READING REFERENCES:

1. Lee, J. D. Concise Inorganic Chemistry ELBS, 1991.
2. Douglas, B.E. and McDaniel, D.H. Concepts & Models of Inorganic Chemistry Oxford, 1970.
3. Atkin, P. Shriver & Atkins’ Inorganic Chemistry 5th Ed. Oxford University Press (2010).
4. Cotton, F.A., Wilkinson, G. and Gaus, P.L., Basic Inorganic Chemistry 3^rd Ed.; Wiley India.
5. Sharpe, A.G., Inorganic Chemistry, 4th Indian Reprint (Pearson Education), 2005.
6. Huheey, J. E.; Keiter, E.A. & Keiter, R.L. Inorganic Chemistry, Principles of Structure andReactivity 4th Ed., Harper Collins 1993, Pearson,2006.
7. Das, Asim. K.; Fundamentals Concepts of Inorganic Chemistry, Vol 1-7, 3^rd Ed., CBS Publishers.
8. Miessler, G. L., Fischer, P. J., Tarr, D. A., Inorganic Chemistry, Pearson, 5th Edition.

PRACTICALS:

1. Estimation of Cu(II) by Iodometric method.
2. Determination of available Chlorine in bleaching powder by Iodometric method.
3. Estimation of Oxalic acid and Sodium oxalate by KMnO4.
4. Estimation of Fe(III) & Cu(II) by K2Cr2O7.

REFERENCES FOR PRACTICALS:

1. Mendham, J., A. I. Vogel’s Quantitative Chemical Analysis 6th Ed., Pearson, 2009.
2. Mukherjee, G. N., University Handbook of Undergraduate Chemistry Experiments, University of Calcutta, 2003.

3. Nad, Mahapatra and Ghoshal, An Advance Course in Practical Chemistry, New Central Book Agency, Kolkata.