General Chemistry 2021/2022

The atomic theory: properties of the electron; the Bohr model of the atom; energy levels in atoms; quantum mechanics model of the atom; atomic orbitals; electron configurations for atoms and periodicity; trends on the Periodic Table. The chemical bond: ions and the compounds they form; writing and naming ionic formulas; covalent bonding; the valence bond (VB) theory; hybridisation; VSEPR theory; shapes of molecules;molecular orbitals (LCAO theory). Chemical reactions; stoichiometry and chemical equations. The gas state; Boyle's law; Charles's law; Gay-Lussac's law; the universal law for ideal gases and the universal gas law constant (R); Van der Waals equation; the kinetic theory. The liquid state; intermolecular forces and attraction; London dispersion forces; polar attractions; hydrogen bond and its importance in Biology. Vapour pressure; evaporation; Boiling point; boiling points change with changes in pressure. The solid state; the ordered structure of crystalline solids; ionic solids, metallic solids; covalent solids. Amorphous solids. Phase diagrams; the phase (P-T) diagrams for water and carbon dioxide. The solution process; solubility; water: the universal solvent; the concentration of solutions; vapor pressure lowering; boiling point elevation; freezing point depression; solution of non-electrolytes and electrolytes. Chemical kinetics; collision theory and the kinetic-molecular theory; activation energy barrier; catalysis. Chemical equilibrium; Rate of forward reaction and rate of reverse reaction; the equilibrium constant; mathematics with equilibrium expressions.The effects of applying stress to reactions at equilibrium: Le Châtelier’s Principle. The effects of pressure, volume and temperature. Acids and bases according to Arrhenius, Brønsted and Lewis; strong and weak acids and bases; water ionization; pH and pOH in water solutions; weak acid-base equilibria in water; the strength of conjugate acids and bases; hydrolysis of salts; buffers; the buffer in blood. Slightly soluble salts. Solubility product constant (Kps); mathematics for Kps. Thermodynamics; Enthalpy; Hess's law of heat summation; Entropy; spontaneous processes; Gibbs Free Energy and spontaneity of chemical processes. Electrochemistry; oxidation and reduction; balancing redox reactions using the oxidation number; spontaneous redox reactions; electrochemical cells; the Nernst equation; the standard hydrogen half-cell; the electrochemical measurement of pH.