22.1 - Lattice Enthalpy
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Why are solid ionic compounds stable?
Strength of ionic bonds, and the electrostatic attraction between oppositely charged ions in the ionic lattice structure
Lattice enthalpy
Energy change that accompanies the formation of one mole of an ionic compound from its gaseous ions under standard conditions
Is lattice enthalpy endothermic or exothermic?
Exothermic Energy change is always negative
Standard enthalpy change of formation
Enthalpy change that takes place when one mole of compound is formed from its elements under standard conditions - with all reactants and products in their standard states
Standard enthalpy change of atomisation
Enthalpy change that takes place for the formation of one mole of gaseous atoms from the element in its standard state under standard conditions
Enthalpy change of formation
Always endothermic (positive) Bonds are broken
First ionisation energy
Enthalpy change required to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions
Electron affinity
Energy to gain electrons
First electron affinity
Enthalpy change that takes place when one electron is added to each atom in one mole of gaseous atoms to form one mole of gaseous 1- ions
Is first electron affinity endothermic or exothermic?
Exothermic - electron is attracted to the positive nucleus
Second electron affinity
Endothermic Electron is being gained by a negative ion - repels electron away