Enthalpy of Formation
One mole of COMPOUND is formed from its constituent ELEMENTS
Delta Hf = products - reactants
C(s)+ O2 (g) - CO2 (g)
Enthalpy change when one mole of SUBTANCE undergoes COMPLETE COMBUSTION in EXCESS oxygen.
Enthalpy change when One mole of GASEOUS ATOMS is produced from an ELEMENT.
Na (s) => Na (g)
1/2 H2 (g) => H (g)
Energy Required to remove one mole of Electrons from one mole of GASEOUS ATOMS.
Produces a 1+ ion.
M (g) => M+ (g) + e-
Enthalpy change when one mole of GASEOUS ATOMS gains ONE ELECTRON per ATOM
X (g) + e- =>X-
When one mole of GASEOUS IONS is converted into AQUEOUS IONS
hydration = -lattic enthalpy - sum of solution enthalpies
One mole of SOLUTE DISSOLVES in a LARGE AMOUNT of WATER enough to prevent IONS INTERACTING
Solution = -lattice enthalpy + sum of hydration enthalpies
Enthalpy change when M+ (g) + X- (g) => MX(s) occurs
Exothermic in forwards direction.
One mole of COVALENT BOND is BROKEN in the GASEOUS STATE forming 2 FREE RADICALS
Atomisation of Cl
Ionisation of Sodium Lattice enthalpy of NaCl
Atomisation of Sodium
Formation of NaCl