|
 Academic Year:
| 2013/4 |
| Owning Department/School:
| Department of Chemistry |
| Credits:
| 12 |
| Level:
| Certificate (FHEQ level 4) |
| Period: |
Academic Year |
| Assessment:
| EX 80%, MC 20%, OT 0% |
| Supplementary Assessment: |
CH10133 EXAM (where allowed by programme regulations) |
| Requisites:
| While taking this unit you must take CH10135 and take CH10137 and in taking this unit you cannot take CH10134 |
| Description:
| Aims: The Unit will provide an introduction to the basics of the nature of the atom, elementary bonding theory, solid-state structural chemistry, periodic trends in main group chemistry and the electronic structure of transition metal compounds. Learning Outcomes: After studying this unit, students should be able to: * Name the first 36 elements, their symbols and electronic configurations. * Name the four quantum numbers and their allowed values. * Draw radial and angular functions for s, p, d orbitals. * Describe the bonding in diatomic molecules using molecular orbital (MO) theory * Construct MO energy level diagrams and be able to extract chemical information from them * Derive the shapes of molecules using the VSEPR method. * Define basic crystallographic concepts. * Describe the main types of inorganic structures through cell-projection diagrams. * Provide a theoretical treatment for lattice energies. * Describe the basic principles of s- and p-block chemistry, including hydrogen. * Use the redox properties of the s- and p-block elements to predict and rationalise chemical reactions. * Describe the basic chemistry of elements from Groups 15, 16 and 17. * Solve basic problems in quantitative inorganic analysis. Skills: Numeracy (F, A); Problem solving (T, F, A); Oral communication (F). Content: Bohr model of the atom, quantization, properties of waves, Schrödinger equation and its solutions, angular and radial functions, quantum numbers. The Periodic Table, Aufbau Principle, Hund's Rules; ionisation energy, electron affinity and electronegativity. Molecular orbital theory for homo- and di- atomic molecules. VSEPR, hybridisation. Coordination chemistry: definitions, shapes, ligand classification, nomenclature and conformations; chelate complexes. Coordination numbers and geometries, isomerism. Solid state structures, radius ratio rule, cell projections for common structural types, lattice energy. Chemical bonding theory, shapes of molecules. The s-block elements, properties related to reactivity and size. H-bonding. Oxidation states of the p-block elements, stability, lone-pair effect, free energy (Frost) diagrams. Chemistry of the halogens and noble gases and their inter-relationship. Hydrides of O, S, N, P and halogens. Properties of co-ordination compounds. Tetrahedral, square planar, and octahedral complexes; Introduction to Crystal Field Theory and splitting of d orbitals in octahedral and tetrahedral complexes. Chemical formulae, moles, molarity, oxidation and reduction. Application of mathematical methods to solving chemical problems. |
| Programme availability: |
CH10133 is Compulsory on the following programmes:Department of Chemistry
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