Thermodynamics definiitions
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Define enthalpy of formation:
Enthalpy change when one mole of a substance is formed from its constituent elements with all substances in their standard states. Exothermic
Define enthalpy of combustion:
Enthalpy change when one mole of a substance undergoes combustion in oxygen with all substances in their standard states. Exothermic
Define enthalpy of neutralisation
Enthalpy change when one mole of water is formed in a reaction between acid and alkali under standard conditions. Exothermic
Define ionisation energy:
Enthalpy change when one mole of gaseous atoms/ (n-1) ions loses one mole of electrons to form one mole of gaseous n+ ions. Endothermic
Define electron affinity:
Enthalpy change when one mole of gaseous atoms/ n+ ions gains one electron to form gaseous n-1 ions
Define enthalpy of atomisation:
Enthalpy change when one mole of gaseous atoms is produced from an element in its standard state. Endothermic
Define hydration enthalpy:
Enthalpy change when one mole of gaseous ions become hydrated (dissolved in water). Exothermic
Define enthalpy of solution:
Enthalpy change when one mole of an ionic solid dissolves in an amount of water large enough so that the dissolve ions are well separated and do not interact with each other.
Define bind dissociation energy:
Enthalpy change when one mole of covalent bonds is broken in a gaseous state. Endothermic
Define lattice enthalpy of formation:
Enthalpy change when one mole of a solid ionic compound is formed from its constituent ions in the gas phase. Exothermic
Define lattice enthalpy of dissociation:
Enthalpy change when one mole of solid ionic compound is broken up into its constituent ions in the gaseous phase. Endothermic
Define enthalpy of vaporisation
Enthalpy change when one mole of a liquid is turned into a gas. Endothermic
Define enthalpy of fusion:
Enthalpy change when one mole of a solid is turned into a liquid. Endothermic