Course Content (Syllabus)
Matter and energy, mass and weight. Units
, measurement and equations. Distinguish elements, compounds, mixtures. Atomic and molecular mass. Calculate a percentage composition from formula. Empirical and molecular formulae. Balance chemical equations. Mole, molarity, normality, Avogadro's number. Characteristic properties of solids, liquids and gases. Endothermic and exothermic reactions. Structure of the nuclear atom and isotopes. Atomic structure, electronic shells and subshells, and orbitals. Energy level diagram for the hydrogen atom, and spectrum of atomic hydrogen. Quantum numbers for the hydrogen atom, and for other elements. Interpret orbitals in terms of probability s, p, and d electrons. Aufbau principle, Pauli principle and Hund's rules to build up electron configurations of the elements of the Periodic Table. Periodicity from configuration across and down the Table, and explain trends in radii, ionisation enthalpies, electron affinities and electronegativities. IUPAC Nomenclature of Inorganic Compounds. Classification of Inorganic Compounds. Ionic and covalent bonding. Metallic bonding and relate to metallic properties. Hybridisation of an atom in a given molecule. Lewis structures for simple molecules. Distinguish sigma and pi bonds. Orbital overlap of s, p, and d electrons, bond order. Molecular orbital energy-level diagram. Non-bonding and antibonding orbitals from s, p, and d combinations. Theories of resonance and p-orbital overlap. Dipoles in polar molecules. Covalent or ionic bonds. Occurrence of intermolecular interactions (van der Waals forces, and hydrogen-bonding). Inter- and intra-molecular hydrogen bonding and van der Waals (London) forces in a molecule. State the Bronsted and Lewis acid-base theory and its applications to salt hydrolysis, buffers and solubility. The theory of redox reactions.
Atomic structure, Molecules, Chemical bond, Nomenclature, Chemical equilibrium, Thermochemistry, Acids-bases, Red-ox