Chemistry STPM Sem 2 - Chapter 1 Chemical Energetics

7 Chemical Energetics	Candidates should be able to:
7.1 Enthalpy changes of reaction, ΔH	(a) Explain that most chemical reactions are accompanied by enthalpy changes (exothermic or endothermic); (b) Define enthalpy change of reaction, ΔH, and state the standard conditions; (c) Define enthalpy change of formation, combustion, hydration, solution, neutralisation, atomisation, bond energy, ionisation energy and electron affinity; (d) Calculate the heat energy change from experimental measurements using the relationship: heat change, q mc T or q = mc ; (e) Calculate enthalpy changes from experimental results.
7.2 Hess’ law	(a) State Hess’ law, and its use to find enthalpy changes that cannot be determined directly, e.g. an enthalpy change of formation from enthalpy changes of combustion; (b) Construct energy level diagrams relating the enthalpy to reaction path and activation energy; (c) Calculate enthalpy changes from energy cycles.
7.3 Born-Haber cycle	(a) Define lattice energy for simple ionic crystals in terms of the change from gaseous ions to solid lattice; (b) Explain qualitatively the effects of ionic charge and ionic radius on the numerical magnitude of lattice energy values; (c) Construct Born-Haber cycle for the formation of simple ionic crystals.
7.4 The solubility of solids in liquids	(a) Construct energy cycles for the formation of aqueous solutions of ionic compounds; (b) Explain qualitatively the influence on solubility of the relationship between enthalpy change of solution, lattice energy of solid and enthalpy change of hydration or other solvent-solute interaction.

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