Inorganic Chemistry I, 22UCHC22, PDF

ARUL ANANDAR COLLEGE (AUTONOMOUS), KARUMATHUR – 625 514 DEPARTMENT OF CHEMISTRY INORGANIC CHEMISTRY-I Class : I B.Sc. Chemistry Part : III Core-2 Semester : II...

ARUL ANANDAR COLLEGE (AUTONOMOUS), KARUMATHUR – 625 514 DEPARTMENT OF CHEMISTRY INORGANIC CHEMISTRY-I Class : I B.Sc. Chemistry Part : III Core-2 Semester : II Hours : 90 Subject Code : 22UCHC22 Credits : 5 Course Specific Objectives The course enables the students to 1. state and define the basic concepts of Inorganic Chemistry 2. explain and illustrate the types of chemical bonding 3. describe and apply the theories of chemical bonding 4. describe, apply and generalise the theories of acids, bases and non-aqueous solvents 5. apply various concepts of nuclear chemistry UNIT-I Basic Concepts of Inorganic Chemistry (18 Hours) Mole concept and stoichiometry –Balancing chemical equations – limiting reagents – Calculations based on chemical equations – Covalency – Oxidationnumber – Rules for calculating oxidation number – Oxidation and reduction – redox reactions and half reactions – oxidizing and reducing agents – disproportionation reaction – Balancing redox equation – oxidation number and ion-electron methods –Molecular weight and equivalent weight– Equivalent weights of acids, bases, salts, oxidants and reductants – Calculations. UNIT-II Chemical Bonding–I (18 Hours) Types of Bonds – ionic, covalent, coordinate and metallic bonds – Properties. Ionic compounds – illustration of the formation of ionic compound (NaCl, CaCl2, MgO) –Lattice energy – Factors affecting lattice energy – Born-Lande Equation (No derivation) – Born-Haber cycle – Formation of NaCl. Covalent compounds – Lewis Structures of homo and heteronuclear molecules (O2, N2, F2, HF, CH4 and NH3) – Partial covalency in ionic compounds – Polarisation and Fajans’ rules. Electronegativity scales – Pauling & Mulliken. Coordinate bond – illustration in O3, NH4+ and H3O+ ions – Hydrogen bonding in H2O, NH3 and HF molecules. UNIT-III Chemical Bonding–II (18 Hours) Theories of covalent bond – Sidgwick-Powell theory – Valance Bond theory – Postulates – Hybridisation and geometry of molecules – sp, sp2, sp3, sp3d, sp3d2, sp3d3 hybridisations – VSEPR theory – Postulates – Structure of BeCl2, BF3, CH4, NH3, H2O, PCl3, PCl5, SF4, SF6, IF7, ClF3 and BrF5. Molecular orbital theory – criteria of orbital overlap – types of molecular orbitals – Construction of MO diagrams – MO diagram for simple homo diatomic (H2, He2, B2, C2, N2, O2 and F2) and hetero diatomic (CO and NO) molecules – Bond order and magnetic properties – stability of molecules. Unit-IV Concepts of Acids, Bases and Non-aqueous Solvents (18 Hours) Theories of Acids and bases – Arrhenius concept – Brönsted-Lowry concept– Conjugate acid-base pairs – Relative order of acidity of halogen acids and oxyacids – Lewis concept – Lux-Flood concept – Usanovich’s concept – definition, applications and limitations – Pearson’s classification as Hard and Soft Acids and Bases (HSAB) – applications and limitations. Non-aqueous solvents – protic and aprotic solvents – Ammonia – solutions of alkali and alkaline earth metals in ammonia – Liq. SO2 as solvent. Unit-V Nuclear Chemistry (18 Hours) Introduction – elementary particles – concept of nuclides – representation of isobars, isotones, isotopes with examples – Radioactivity – Stable and unstable nuclei – n/p ratio – magic numbers – mass defect and binding energy – binding energy curve – packing fraction – mass-energy relationships. Radioactive Elements – modes of decay – Neutron, Positron Theory of α, β and γ emission – characteristics of α, β and γ particles – Theories of radioactivity – Soddy’s group displacement law – half-life period – average life – radioactive disintegration series. Nuclear reactions – Nuclear fission – atomic bomb – Nuclear fusion – stellar energy, hydrogen bomb – Nuclear reactor. Applications of radioactivity in medicine, agriculture and industry – Radiocarbon dating. Text Books 1. B. R. Puri, L. R. Sharma and K. C. Kalia, Shoban Lal, Principles of Inorganic Chemistry, Nagin Chand and Co., New Delhi, (2018). 2. Satyaprakash, G. D. Tuli, S. K. Basu, R. D. Madan, Advanced Inorganic Chemistry, Vol. I, S. Chand & company, 5th Edition, New Delhi (2017). Reference Books 1. John D. Lee, “Concise Inorganic Chemistry”, 5th Edition, Blackwell Science, New Delhi (2018). 2. B. R. Puri, L. R. Sharma and K. C. Kalia, “Principles of Inorganic Chemistry”, 31st Edition, Milestone Publishers and Distributors, New Delhi, India (2014). 3. James E. Huheey, Ellen A. Keiter, Richard L. Keiter & Okhil K. Medhi, “Inorganic Chemistry – Principles of Structure and Reactivity”, 4th Edition, Pearson Education, New Delhi (2018). 4. B.Douglas, D.McDaniel, J.Alexander, Concepts and Models of Inorganic Chemistry, 3rd Edition, John Wiley (1994).