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Course Detail

Course Name General Chemistry
Course Code 22CHY103
Semester 1
Credits 4


Unit 1

Atomic structure

Bohr’s model of hydrogen atom, Ritz combination principle, hydrogen spectrum, Bohr-Sommerfeld theory. Planck’s quantum theory of radiation, dual character of electrons – de Broglie’s equation, Heisenberg’s uncertainty principle, photoelectric effect, Compton, Zeeman and Stark effects. Schrodinger wave equation, Eigen values, significance of wave function (ψ and ψ2) and quantum numbers. Schrodinger wave equation for hydrogen and hydrogen-like systems, probability distribution of electrons around the nucleus, distribution of electrons in orbitals, shapes of atomic orbitals – s, p, d and f. Aufbau principle, Hund’s rule, Pauli’s exclusion principle, electronic configuration of elements.

Unit 2

Chemical bonding

Electrovalency and ionic bond formation, ionic compounds and their properties, lattice energy. Born-Lande equation and Born-Haber cycle and their applications, solvation enthalpy and solubility of ionic compounds. Covalent bonding, formation of H2, orbital theory of covalency. Hybridisation – VSEPR theory, sigma and pi bonds, formation of covalent compounds. Properties of covalent compounds. Molecular orbital theory – homo and hetero diatomic molecules. Polar and non-polar covalent bonds, polarization of covalent bond – polarizing power, polarisability of ions and Fajan’s rule, dipole moment, percentage ionic character from dipole moment, dipole moment and structure of molecules. Co-ordinate covalent compounds and their characteristics. Metallic bond – free electron, valence bond and band theories.

Unit 3

Acids, Bases and Non-aqueous solvents

Concepts of acids and bases – conjugate acids and bases, hard and soft acids and bases – Pearson’s concept, HSAB principle and its application. Non-aqueous solvents – general characteristics of non-aqueous solvent – melting point, boiling point, latent heat of fusion and vaporization, and dielectric constant. Reactions in non-aqueous solvents like liquid ammonia, liquid SO2 and liquid HF – complex formation, redox, precipitation and acid base type.

Unit 4

Chemical analysis and stoichiometric calculation

Titrimetry – fundamental concepts, theory of indicators. Acid base, redox, precipitation and complexometric titrations. Problems based on stoichiometry. Gravimetry principle and calculations involving estimation of barium, calcium and nickel. Data analysis, significant figures, precision and accuracy. Types of errors, mean and standard deviation.

Unit 5

Functional groups and Nomenclature of organic compounds

Calculation of empirical and molecular formula, determination of molecular weights – physical and chemical methods. Classification and nomenclature of organic compounds. Structure, nomenclature, isomerism in alkanes, alkenes and alkynes. General methods of preparation of alkanes, alkenes and alkynes. Introduction to functional groups.


  1. Atkins, P. and Overton, T., 2010. Shriver and Atkins’ inorganic chemistry. Oxford University Press, USA.
  2. Catherine E. H. and Alan G. S. 2012. Inorganic Chemistry (Fourth Edition), Pearson, UK.
  3. Marion Clyde Day Jr,‎ Joel Selbin,‎ Harry H Sisler. 2012. Theoretical Inorganic Chemistry. LLC.
  4. Vogel, A. I. and Jeffery, G.H. 2009. Vogel’s Quantitative Chemical Analysis, 6th Ed. Wiley.
  5. Solomons, T. G. and Fryhle, C. B., 2008. Organic chemistry. John Wiley & Sons.
  6. F. A. Cotton and G. Wilkinson. 1987. Advanced Inorganic Chemistry, 5th edition, John Wiley and Sons, New York.

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