Coming soon
Inorganic Chemistry (Theory)
Course Objectives:
This course will enable the students to –
- recall the general trends in the periodic table of elements.
- equip with the knowledge of gradation in properties of main group elements and theoretical concepts of different titrations of volumetric analysis like principle, applications and indicators used etc.
Course Outcomes (COs):
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Course |
Learning outcomes (at course level) |
Learning and teaching strategies |
Assessment Strategies |
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Course Code |
Course Title |
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CNST 103 |
Inorganic Chemistry (Theory) |
The students will be able to –
CO:1. explain Bohr’s theory and concept of wave function and quantum numbers
CO:2. calculate the radius ratio of ionic molecules and determine the ionic structures of the type AX and AX2
CO:3. appraise the concept of Born-Haber cycle and predict the lattice energy, ionization energy and stability of the ionic compounds.
CO:4. predict physical and chemical characteristics of elements in various groups and periods according to ionic size, charge, etc. and position in periodic table and describe various types of hybridization and geometry of molecules.
CO:5. construct molecular orbital diagrams of homo and hetero nuclear diatomic molecules and determine the bond order with the help of M.O. diagram.
CO:6. discuss the different theories of metallic bonding, hydrogen bonding and Van der Waals interaction.
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Approach in teaching:
Interactive sessions, Discussion, problem solving in Tutorials, Demonstration
Learning activities for the students: Self-learning assignments, Effective questions, Simulation, Seminar presentation, Solving numericals.
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Class test, Semester end examinations, Quiz, Solving problems, Assignments, Presentations
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Bohr’s theory to hydrogen-like atoms and ions; spectrum of hydrogen atom. Quantum numbers. Introduction to the concept of atomic orbitals; shapes, radial and angular probability diagrams of s, p and d orbitals (qualitative idea). Many electron atoms and ions: Pauli’s exclusion principle, Hund’s rule, exchange energy, Aufbau principle and its limitation. Electronic energy level diagram and electronic configurations of hydrogen-like and polyelectronic atoms and ions up to atomic number
Periodic table, group trends and periodic trends in physical properties.Classification of elements on the basis of electronic configuration. Modern IUPAC Periodic table. General characteristic of s, p, d and f block elements. Position of hydrogen and noble gases in the periodic table. Effective nuclear charges, screening effects, Slater’s rules, atomic radii, ionic radii (Pauling’s univalent), covalent radii. Ionization potential, electron affinity and electronegativity (Pauling, Mulliken and Allred-Rochow scales) and factors influencing these properties. Inert pair effect.
Lewis structures, formal charge. Valence Bond Theory, directional character of covalent bonds, hybridizations, equivalent and non-equivalent hybrid orbitals, Bent’s rule, VSEPR theory, shapes of molecules and ions containing lone pairs and bond pairs (examples from main groups chemistry), partial ionic character of covalent bonds, bond moment, dipole moment and electronegativity differences. Concept of resonance, resonance energy, resonance structures.
