Syllabus (CHEMISTRY)

Course Type: ME-6

Semester: 5

Course Code: BCEMMEB35C

Course Title: Inorganic & Physical Chemistry– I

(L-P-Tu): 3-1-0

Credit: 4

Practical/Theory: Combined

Course Objective: COURSE OBJECTIVE OF MINOR - 6: The syllabus of Minor -6 has been designed to provide the students with in-depth knowledge of Chemical bonding, including Ionic bonding, Covalent Bonding, Co-ordinate covalent bonding. This course will also give the students

Learning Outcome: COURSE OUTCOMES OF MINOR – 6: CO- 6.1: Thorough understanding of Chemical Bonding with special Emphasis on Ionic, Covalent bonding. Understanding the concepts of Molecular Orbital Theory. CO- 6.2: This module deals with the theories involved in explain

THEORY:

1. CHEMICAL BONDING – (15 L):

a) Ionic bond: General characteristics, types of ions, size effects, radius ratio ruleand its application and limitations. Born-Landéequation without derivation. Madelung Constant, Born-Haber cycle and its application.

b) Covalent bond: Polarizing power and polarizability, ionic potential, Fajan’s rule. Lewis structures, formal charge. Valence Bond Theory. 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 lonepairs and bond pairs (examples from main groups chemistry) and multiple bonding (sand π bond approach). MO diagrams of B₂, C₂, N₂ and O₂ molecules and their simple applications.

2. KINETIC THEORY OF GAS – (20 L):

a. Concept of pressure and temperature; Collision of gas molecules; Collision diameter; Collision number and mean free path; Frequency of binary collisions (similar and different molecules); Rate ofeffusion.

b. Nature of distribution of velocities, Maxwell’s distribution of speed and kineticenergy; Average velocity, root mean square velocity and most probable velocity; Principle of equipartition of energy and its application to calculate the classical limit of molar heat capacity of gases.

c. Deviation of gases from ideal behavior; compressibility factor; Boyle temperature; Andrew’s and Amagat’s plots; van der Waals equation and its features; its derivation and application in explaining real gas behaviour; Existence of critical state, Critical constants in terms of van der Waals constants; Law of corresponding states.

d. Viscosity of gases and effect of temperature and pressure on coefficient of viscosity (qualitative treatment only).

3. Liquids (10 L):

Definition of Surface tension, its dimension and principle of its determination using stalagmometer; Viscosity of a liquid and principle of determination of coefficient of viscosity using Ostwald viscometer; Effect of temperature on surface tension and coefficient of viscosity of a liquid (qualitative treatment only).

READING REFERENCES:

1. Misra, S.; Giri, G. C.; Roy, S. K.; Chanda, G., SnatakRasayan, B.Sc. Semester-I, II, III, IV, Santra Publication.

2. A. Ghoshal, General and Physical Chemistry, Books and Allied (P) Ltd. Kolkata

3. Physical Chemistry, G. W. Castellan, Narosa Publication House

4. A Text Book of Physical Chemistry, K. L. Kapoor, Vol. 1-5, Macmillan Indian Ltd. New Delhi.

5. Chemical Kinetics, K. J. Laidler, Pearson Education.

6. Physical Chemistry, P. C. Rakshit, Sarat Book House, Kolkata.

7. Physical Chemistry, Hrishikesh Chatterjee, Vol. 1-2, Platinum Publishers.

8. Lee, J. D. Concise Inorganic Chemistry ELBS, 1991.

9. Cotton, F.A., Wilkinson, G. and Gaus, P.L., Basic Inorganic Chemistry 3rd Ed.; Wiley India.

10. Sharpe, A.G., Inorganic Chemistry, 4th Indian Reprint (Pearson Education) 2005.

11. R. P. Sarkar, General and Inorganic Chemistry, Part-1 & 2, New Central Book Agency (P) Ltd. Kolkata.

PRACTICALS:

1. Determination of the surface tension of a liquid or a dilute solution using a Stalagmometer.

2. Determination of relative and absolute viscosity of a liquid or dilute solution using an Ostwald’s viscometer.and CHCl₃.

REFERENCES FOR PRACTICALS:

1. S. P. Dey, SnatakParikhyagareRasayan, Vol-I, Santra Publication, Kolkata.