Syllabus (CHEMISTRY)

Course Type: MAJ-1

Semester: 1

Course Code: BCEMMAJ01C

Course Title: Inorganic Chemistry – I

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

Credit: 6

Practical/Theory: Combined

Course Objective: COURSE OBJECTIVE OF MAJOR - 1: The syllabus of Major -1 has been designed to provide the students with the basic ideas of General Inorganic and Physical Chemistry. The four modules consisting of Atomic Structure, Periodic Properties, Acid-Base and Redox

Learning Outcome: COURSE OUTCOMES OF MAJOR – 1: CO-1.1 Gather an in-depth knowledge about atomic structure. CO-1.2 Understand the periodic properties of the elements. CO-1.3 Understand the concepts of a redox reaction. CO- 1.4 Explain various phenomenon of redox r

THEORY:

1. ATOMIC STRUCTURE: (15L)

Bohr’s theory, its limitations and atomic spectrum of hydrogen atom; Sommerfeld’s Theory, de Broglie equation, Heisenberg’s Uncertainty Principle, Photoelectric Effect, A brief introduction to wave mechanical model of atomic structure (Schrodinger Equation only) Auf-Bau Principle, Hund’s Rule of Maximum Spin Multiplicity, Pauli’s Exclusion Principle, Electronic configuration of elements (upto Z = 30). Determination of Ground State Term Symbols of elements and ions (upto Z=30).

2. PERIODIC PROPERTIES: (20L)

Modern IUPAC Periodic table, Effective nuclear charge, screening effects andpenetration, Slater’s rules, atomic radii, ionic radii. Ionization potential, electron affinity andelectronegativity (Pauling’s, Mulliken’s and Allred- Rochow’s scales). Group trends and periodic trends in these properties in respect of s-, p-block elements.

3. CONCEPT OF ACID-BASE THEORIES: (15L)

Acid-Base concept: Arrhenius concept, theory of solvent system (in H2O, NH3,SO2 and HF), Bronsted-Lowry’s concept, relative strength of acids, Pauling’s rules.Lux-Flood concept, Lewis concept, HSAB principle. Thermodynamic acidity parameters, Drago-Wayland equation.

4. REDOX CHEMISTRY: (10L)

Ion-electron method of balancing equation of redox reaction. Elementary idea onstandard redox potentials with sign conventions, Nernst equation (without derivation).

Influence of complex formation, precipitation and change of pH onredox potentials;formal potential. Feasibility of a redox titration, redox potential at theequivalencepoint, redox indicators. Redox potential diagram (Latimer and Frost diagrams) ofcommon elements and their applications. Disproportionation and comproportionationreactions (typical examples).

Solubility product principle, common ion effect and their applications to theprecipitation and separation of common metallic ions as hydroxides, sulfides,phosphates, carbonates, sulfates and halides.

READING REFERENCES:

1. Lee, J. D. Concise Inorganic Chemistry ELBS, 1991.
2. Douglas, B.E. and McDaniel, D.H. Concepts & Models of InorganicChemistry Oxford, 1970.
3. Atkin, P. Shriver & Atkins’ Inorganic Chemistry 5th Ed. Oxford UniversityPress (2010).
4. Cotton, F.A., Wilkinson, G. and Gaus, P.L., Basic Inorganic Chemistry 3^rdEd.; 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, Principlesof Structure andReactivity 4th Ed., Harper Collins 1993, Pearson,2006.
7. Das, Asim. K.; Fundamentals Concepts of Inorganic Chemistry, Vol 1-7, 3^rdEd., CBS Publishers.

PRACTICALS:

1. Estimation of carbonate and hydroxide present together in mixture.
2. Standardization of KMnO4 by Oxalic acid.
3. Estimation of Fe(II) using standardized KMnO4 solution.
4. Estimation of Fe(II) using standardized K2Cr2O7 solution.

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.