Energetics

Standard enthalpy change of formation

Enthalpy change when 1 mol of compound form from its elements in their standard states under standard conditions

Standard enthalpy change of neutralisation

Enthalpy change when an acid is neutralised by a base to form 1 mol of water under standard conditions

Standard enthalpy change of combustion

Enthalpy change when 1 mol of substance burns completely in oxygen under standard conditions

Standard enthalpy change of reaction

Enthalpy change when molar quantities of reactants (as stated in the equation) react under standard conditions

Bond enthalpy

Energy required to break 1 mol of covalent bonds in the gas state

1st electron affinity

Enthalpy change when 1 mol of gaseous atoms gains 1 mol of electrons to form 1 mol of gaseous ions

Enthalpy

Amount of chemical energy in a system that can be converted to heat energy

Specific heat capacity

Heat energy required to raise the temperature of 1g of substance by 1C

Hess's law

Enthalpy change for any reaction is independent of the route taken from reactants to products, providing starting and final conditions are the same

Standard enthalpy change of atomisation

Enthalpy change when 1 mol of gaseous atoms is formed from its element in standard states

Standard enthalpy of solution

Enthalpy change when 1 mol of compound is dissolved in water under standard conditions

Standard enthalpy change of hydration

Enthalpy change when 1 mol of isolated gaseous ions dissolves in water to form 1 mol of aqueous ions under standard conditions

Lattice energy

Heat energy released when 1 mol solid ionic compound in standard state forms from its ions in the gaseous state under standard conditions