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Standard enthalpy change of reaction
The enthalpy change when the number of moles of reactants as stated in the equation react under standard conditions of 100kPa and 298K.
Standard enthalpy change of formation
The enthalpy change when one mole of a compound is formed from its elements, in their most stable states, under standard conditions of 100kPa and 298K.
Standard enthalpy change of combustion
The enthalpy change when 1 mol of a substance is completely burned in oxygen under standard conditions, all reactants and products being in their standard conditions of 100kPa and 298K.
Standard enthalpy change of neutralisation
The enthalpy change, under standard conditions, when 1 mol of water is produces as a result of the reaction between an acid and an alkali.
Enthalpy change of solution
The enthalpy change when 1 mol of a compound completely dissolves in water under standard conditions.
Enthalpy change of hydration
The enthalpy change when 1 mol of gaseous ions is dissolved in water to form 1 mol of aqueous ions under standard conditions.
Enthalpy change of atomisation
The enthalpy change when 1 mol of gaseous atoms is formed from its element in its standard state.
Lattice enthalpy
The enthalpy change that takes place when 1 mol of an ionic solid is formed from its gaseous ions.
First electron affinity
Energy change that takes place when 1 mol of atoms in the gaseous state gain 1 mol of electrons to form 1 mol of gaseous 1- ions.
First ionisation energy
The energy change that takes place when one electron is lost from each of a mole of atoms in the gaseous state to form one mole of gaseous 1+ ions.
Hess’ Law
If the initial and final conditions are the same, then the total enthalpy change will be the same, regardless of the route taken between reactants and products.
Giant ionic lattice
Opposite charged ions are held together by strong electrostatic forces of attraction in a huge three-dimensional structure.
