Course Objective(s):
This course will enable the students to -
Course Outcomes (COs):
Course Outcomes |
Teaching Learning Strategies |
Assessment Strategies |
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On completion of this course, the students will be able to- CO1: explain Bohr’s theory and concept of wave function and quantum numbers CO2: calculate the radius ratio of ionic molecules and determine the ionic structures of the type AX and AX2 CO3: appraise the concept of Born-Haber cycle and predict the lattice energy, ionization energy and stability of the ionic compounds. CO4: 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. CO5: construct molecular orbital diagrams of homo and hetero nuclear diatomic molecules and determine the bond order with the help of M.O. diagram. CO6: discuss the different theories of metallic bonding, hydrogen bonding and Van der Waals interaction. |
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Bohr’s theory to hydrogen-like atoms and ions, quantum numbers, qualitative approach of Schrödinger equation and its application to hydrogen atom, 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 configuration.
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.
Ionic Bond - general characteristics, size effects, radius ratio rules and their limitations, packing of ions in crystals, ionic compounds of the type AX (ZnS, NaCl, CsCl) and AX2 (CaF2-fluorite) lattice energy, Born–Landé equation and its applications, Born-Haber cycle and its applications, solvation energy and solubilities of ionic compounds, polarizing power and polarizability, ionic potential, Fajans’ rules.
Covalent Bond- Lewis structures, octet rule and its exceptions, Valence Bond Theory (Heitler and London approach) and its limitations, concept of resonance and resonating structures of simple inorganic molecules, directional character of covalent bonds, hybridizations, 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
Self-Study- defects in solids.
Molecular orbital concept of bonding (elementary pictorial approach)-sigma and pi-bonds, multiple bonding, MO diagrams of homo diatomic (H2, Li2, Be2, B2 C2, N2, O2 and F2), and hetero diatomic molecules (CO, NO, CN and HF) and their ions, bond orders, bond lengths, coordinate bonding- Lewis acid-base adducts.
Metallic bond- qualitative idea of free electron theory and band theory, conducting, semi conducting and insulating properties with examples from main group elements.
Weak Chemical Forces-
Van der Waals interactions - ion-dipole, dipole-dipole, induced-dipole, instantaneous dipole – induced dipole interactions
Hydrogen bonding- types, theories and properties of H-bond, effects of H-bond on physical properties.
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