(Semester – II)
CH2B01: Theoretical and Inorganic Chemistry
Credits- 2 (36 Hrs)
Aim
To impart essential theoretical knowledge on atomic structure, periodic properties, chemical bonding, and nuclear chemistry.
Objectives:
To study the various atom models
To understand the important features of the quantum mechanical model of the atom.
To study the periodic properties of elements
To explain the formation of different types of bonds To predict the geometry of simple molecules
To explain the different types of hybridisation and draw shapes of simple covalent molecules
To understand the molecular orbital theory of diatomic molecules To develop interest in various branches of inorganic chemistry. To study nuclear models and nuclear reactions.
- Atomic Structure (9 hrs)
Bohr model of hydrogen atom, Bohr’s equation for the energy of electron in hydrogen atom, the hydrogen spectrum, limitations of Bohr theory, photoelectric effect, idea of de
Broglie matter waves, Heisenberg’s uncertainity principle and its significance, Schrodinger wave equation (derivation not expected), wave functions, significance of ψ (psi) and ψ2, 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 Pauli’s exclusion principles, Hund’s rule, energy level diagram of a multielectron atom, concept of effective nuclear charge, Slater’s rules and applications,
Electronic configuration of atoms.
References
- D. Lee, Concise Inorganic Chemistry, 5th edn., Blackwell Science, London (Chapter 1)
- R. Puri, L. R. Sharma, Kalia, Principles of Inorganic Chemistry, Milestone Publishers, New Delhi(Chapter 1)
- N. R. Rao, University General Chemistry, Macmillan,India (Chapter 1)
- A. Cotton, G. Wilkinson and P.L. Gaus, Basic Inorganic Chemistry, 3rd edn., John Wiley(Chapter 2).
- F. Shriver and P. W. Atkins, Inorganic Chemistry, 3rd edn., Oxford University Press(Chapter 1)
- Douglas, D. Mc Daniel, J. Alexander, Concepts and models in Inorganic Chemistry(Chapter 1)
- Periodic properties (3 hrs)
Periodic trends in atomic volume, atomic and ionic radii, ionisation enthalpy, electron affinity(electron gain enthalpy), electronegativity and metallic character, Pauling’s electronegativity scale, Classification of elements as s,p,d & f block.
References
- D. Lee, Concise Inorganic Chemistry, 5th edn., Blackwell Science, London(Chapter 1,6)
- R. Puri, L. R. Sharma, Kalia, Principles of Inorganic Chemistry, Milestone Publishers, New Delhi(Chapter 2)
- N. R. Rao, University General Chemistry, Macmillan India (Chapter 3)
- A. Cotton, G. Wilkinson and P. L. Gaus, Basic Inorganic Chemistry, 3rd edn., John Wiley(Chapter 2).
- Douglas, D. Mc Daniel, J. Alexander, Concepts and models in Inorganic Chemistry(Chapter 1).
3 Chemical Bonding (15 hrs)
Ionic bond – nature of ionic bond, properties of ionic compounds, radius ratio and coordination number, factors favouring the formation of ionic compounds. Lattice energy, Born-Lande equation with derivation, factors affecting lattice enthalpy, Born-Haber cycle and its applications, solvation enthalpy and solubility of ionic compounds.
Covalent bond- valence bond theory and its limitations, concept of resonance, resonance energy, hybridisation and shapes of simple molecules (BeF2, PCI3, PCI5, SF6 , CH4, Ethane, ethane and ethyne) VSEPR theory, shapes of molecules and ions (NH3, XeF6, CIF3, NH4+, H3O+). Molecular orbital theory – LCAO method, molecular orbital energy diagram and properties of homo and hetero diatomic molecules (N2, O2, CO and NO), bond strength and bond energy. Polarisation of covalent bond, polarising power and polarisability of ions, Fajan’s rule.
Dipole moment and molecular structure – percentage ionic character from dipole moment.
Metallic bonding – free electron theory, valence bond theory and band theory, explanation of metallic properties based on these theories.
Weak chemical forces – hydrogen bond, inter and intra molecular hydrogen bonds, effects of hydrogen bonding, van der Waals forces
References
- D. Lee, Concise Inorganic Chemistry, 5th edn., Blackwell Science, London(Chapter 2-5)
- R. Puri, L. R. Sharma, Kalia, Principles of Inorganic Chemistry, Milestone Publishers, New Delhi(Chapter 4,5)
- N. R. Rao, University General Chemistry, Macmillan India(Chapter 3)
- A. Cotton, G. Wilkinson and P. L. Gaus, Basic Inorganic Chemistry, 3rd edn., John Wiley(Chapter 3,4).
- F. Shriver and P. W. Atkins, Inorganic Chemistry, 3rd edn., Oxford University Press(Chapter 2,3)
4 Nuclear Chemistry (9 hrs)
Nuclear particles, nuclear forces, nuclear size, nuclear density, stability of nucleus, binding energy, magic numbers, packing fraction, n/p ratio. Nuclear models – liquid drop model and shell model.
Natural radioactivity, modes of decay, decay constant, half life period, average life, radioactive equilibrium, Geiger-Nuttal rule, units of radioactivity, radiation dosage.
Induced radioactivity, nuclear reactions induced by charged projectiles, neutrons and γ rays, fission reactions, fusion reactions, spallation reactions, preparation of transuranic elements, Q values of nuclear reactions. Fertile and fissile isotopes, chain reaction, stellar energy.
References
- R. Puri, L. R. Sharma, Kalia, Principles of Inorganic Chemistry, Milestone Publishers, New Delhi(Chapter 38)
- J. Arnikar, Essentials of Nuclear Chemistry,New Age(Chapter3- 5)
- Gopalan, Elements of Nuclear Chemistry, Vikas Publ. House.
Further Reading
- E. Huheey, E. A. Keiter, R. L. Keiter, Inorganic Chemistry, 4th edn., Harper Collins, 1993.
- Wulfsberg, Inorganic Chemistry, Viva Books
- L Jolly, Inorganic Chemistry, Ttata Mc Graw Hill
- D. Lee, New concise inorganic chemistry,
- N. Greenwood and A. Earnshaw, Chemistry of the elements 2nd edn, Butterworth
- Manas Chanda, Atomic structure and chemical bonding
- J. Emeleus, A. G. Sharpe, Modern Aspects of Inorganic Chemistry, Universal Book Stall
- J David Brown, The Chemical Bond in Inorganic Chemistry,Oxford Science Publication
Practical: CH2B01 Volumetric Analysis
Credit- 1 (36 hrs)
- Permanganometry
- Estimation of Ferrous iron
- Estimation of Oxalic acid
- Estimation of Hydrogen Peroxide
- Estimation of Calcium
- Dichrometry
- Estimation of Ferrous iron using internal indicator
- Estimation of Ferrous iron using external indicator
- Estimation of Ferric iron – reduction with SnCl2
- Iodometry and Iodimetry
- Standardisation of thiosulphate using KIO3, electrolytic copper and potassium dichromate.
- Estimation of As2O3 and arsenite.
- Estimation of Cu in a copper salt.
References
- A. Skoog, D. M. West, and S. R. Crouch, Fundamentals of Analytical Chemistry 8th edn, Brooks/Cole Nelson (Chapters 13,14)
- Vogel’s Textbook of Quantitative Chemical Analysis 6th edn, Pearsons Education Ltd.(Chapter 10)
- D. Christian, Analytical Chemistry, JohnWiley and Sons(Chapter12)
- D. Day, A. L. Underwood, Quantitative analysis,6th Edn.,Prentice Hallof India Pvt. Ltd(Chapter 11)