15.1.1

Define and apply the terms standard state, standard enthalpy change of formation () and standard enthalpy change of combustion ().

2

15.1.2

Determine the enthalpy change of a reaction using standard enthalpy changes of formation and combustion.

3

15.2.1

Define and apply the terms lattice enthalpy and electron affinity.

2

15.2.2

Explain how the relative sizes and the charges of ions affect the lattice enthalpies of different ionic compounds.

3

The relative value of the theoretical lattice enthalpy increases with higher ionic charge and smaller ionic radius due to increased attractive forces.

15.2.3

Construct a Born–Haber cycle for group 1 and 2 oxides and chlorides, and use it to calculate an enthalpy change.

3

15.2.4

Discuss the difference between theoretical and experimental lattice enthalpy values of ionic compounds in terms of their covalent character.

3

A significant difference between the two values indicates covalent character.

15.3.1

State and explain the factors that increase the entropy in a system.

3

15.3.2

Predict whether the entropy change (ΔS) for a given reaction or process is positive or negative.

3

15.3.3

Calculate the standard entropy change for a reaction () using standard entropy values ().

2

15.4.1

Predict whether a reaction or process will be spontaneous by using the sign of .

3

15.4.2

Calculate for a reaction using the equation

and by using values of the standard free energy change of formation, .

2

15.4.3

Predict the effect of a change in temperature on the spontaneity of a reaction using standard entropy and enthalpy changes and the equation .

3