Course Contents

Theory History of Periodic Table (Dobereiner, Spiral, Newlands, Meyer’s, Mendeleeve, Moseley Periodic Table), Modern Periodic law and Periodic Table, Atomic No. and Modern Periodic Table, (X-Rays), Quantum Numbers, Hunds Rule, Pauli’s exclusion principle, Auf bau principle. Atomic Structure and Periodic Table, Periods, Groups (A + B) Classification of elements based on s, p, d & f orbitals. Group Anomalies, Artificial (Man made) elements. Oxidation states of Lanthanide and Actinides. Screening Effect, Shielding effect, Penetration of orbitals, Effective Nuclear Charge, Group Trend & Periodicity, and Size of atoms & ions, Isoelectronic species. Covalent Radii, ionic radii, Vander wall radii, Lanthanide contraction, Ionization energy (definition, unit, example successive I.P variation in Periodic Table) Electron Affinity (definition, unit, example, variation in Periodic Table), Charge Density, Polarizability and polarizing power. Electronegativity, Electropositivity, Redox Potential, Oxidation, Reduction,Standard Hydrogen Electrode. Electrochemical Series, its Applications, Trend of Redox potential in Periodic Table. Types of Chemical Bond, Ionic Bond (NaCl, CsCl), Lattice Energy, Born Haber Cycle, Factors responsible for the stability of ionic compounds, Characteristic features, Variable valency, Covalent Bond, Characteristic features, Characteristic features of Co-ordinate Covalent bond, Vander Waals Forces. Hydrogen Bonding, Nature of Hydrogen Bonding, Importance of Hydrogen Bonding, Valence Bond Theory (VBT), Postulates, (Mathematical Derivation) and its application, (F2, O2, HCl), Hybridization of orbitals (sp, sp2, sp3) Hybridization (dsp2, dsp3, d2sp3, d3sp3), sigma and Pi Bond, Molecular orbital Theory (MOT) bonding and Antibonding Molecular orbitals, Application of MOT Formation of H2 Molecule. Application of MOT Formation of He2, Li2, O2, N2, F2, HF, difference between VBT and MOT, Resonance. Valence shell electron pair repulsion (VSEPR) Theory, postulates AB2, AB3, AB2E, AB4, AB3E, AB2E2, AB5, AB4E, AB3E2, AB2E3, AB6, AB5E, AB7. Exercise and discussion. Acid and Bases, Definition, Arhernius Concept, Lowry Bronsted Concept, Lewis Concept, Lux-Flood Concept, Usanovich Concept, Strength of acid and Base, pH, PKa and PKb, Buffers, Indicators (Acid-base, Redox and adsorption). Soft and Hard Acid-base (SHAB Concept), Characteristic features of Soft and hard acid-bases, applications of soft and hard acid-bases. Law of Mass action, Application of law of mass action, Solubility Product, Common ion effect and its application.

Course Synopsis

The course aims to help the students to review undergraduate inorganic chemistry and prepare them for advanced Chemistry courses. It is assumed that students taking this course have basic knowledge of general inorganic chemistry at the undergraduate level. We will cover topics relating to periodic table, chemical boding, acids and bases and chemical equilibrium.

Course Learning Outcomes

Having successfully completed this module students will be able to: • debate the atomic structure Categorize matter Illustrate the explanation of atomic structure Explain electronic structure of atom Relate the quantum numbers and atomic orbitals • evaluate the periodic properties of elements Relate periodic properties of elements Express the periodic properties of elements Categorize elements • estimate molecular structure Relate the molecular structure and Lewis dot notation Calculate formal charge • Demonstrate the resonance forms of molecules Calculate bonding energy • estimate types of chemical bonding Adapt Valance Bond theory to molecule structure • Explain the covalent bond with hybridization Adapt the Molecular Orbital theory to molecular structure Explain the molecular geometry with VSEPR theory • Illustrate the explanation of Acids and Bases