Physical- Energetics and Thermodynamics

Enthalpy Change (kJmol⁻¹)
ΔH

Standard Enthalpy Change

Hess' Law

Enthalpy Change of Formation
ΔH(f)

Explain why an experimental ΔH(f) will differ from the value given by a data book

Enthalpy Change of Combustion
ΔH(c)

Bond Dissociation Enthalpy
ΔH(diss)

Explain why ionic bond enthalpies are not found in any data book

Enthalpy of Atomisation
ΔH(at)

Explain why ΔH(at) is half of ΔH(diss) for diatomic molecules

1st Ionisation Enthalpy
ΔH(i1)

2nd Ionisation Enthalpy
ΔH(i2)

1st Electron Affinity
ΔH(ea1)

2nd Electron Affinity
ΔH(ea2)

Lattice Enthalpy of Formation
ΔH(L)

Trends in Lattice Enthalpy

The Perfect Ionic Model

Explain partial covalent bonding in ionic compounds

Trends in polarisation

Enthalpy of Solution
ΔH(soln)

Enthalpy of Hydration
ΔH(hyd)

How do you find enthalpy of solution?
ΔH (soln)

Factors affecting solubility

What processes does dissolving involve?

Entropy (Jmol⁻¹K⁻¹)
ΔS

Factors affecting entropy

Formula to find entropy change

When is the entropy of an element zero?

What causes differences in entropy between substances in the same physical state?

Why is ΔS for boiling/condensing > ΔS for melting/freezing?

What is the relationship between ΔS and ΔH?

Gibbs free energy change (kJmol⁻¹)
ΔG

Formula to find ΔG

Conditions required for a reaction to be feasible

Reasons why a reaction with ΔG ≤ 0 may not occur

How to find the minimum temperature at which a reaction will be feasible