Thermodynamics Flashcards
Enthalpy of formation
Enthalpy change when one mole of a substance is formed from its constituent elements with all substances in their standards states
Exothermic (usually)
Enthalpy of combustion
Enthalpy change when one mole of a substance undergoes complete combustion in oxygen with all substances in their standard states
Exothermic
Enthalpy of neutralisation
Enthalpy change when one mole of water is formed in a reaction between an acid and alkali under standard conditions
Exothermic
First ionisation enthalpy
Enthalpy change when each atom in a one mole of gaseous atoms loses one electron to form one mole of gaseous 1+ ions
Endothermic
First electron affinity
Enthalpy change when each atom in one mole of gaseous atoms gains one electron to form one mole of gaseous 1- ions
Exothermic for most non-metals
Second electron affinity
Enthalpy change when each atom in one mole of gaseous 1- atoms gains one electron to form one mole of gaseous 2- ions
Endothermic
Enthalpy of atomisation
Enthalpy change when one mole of gaseous atoms is produced from an elements in its standard state
Endothermic
Hydration enthalpy
Enthalpy change when one mole of gaseous ions become hydrated (converted to aqueous ions)
Exothermic
Enthalpy of solution
Enthalpy change when one mole of an ionic solid dissolves in an amount of water large enough so that the dissolved ions are well seperated and do not interact with each other
Bond dissociation enthalpy
Enthalpy change when one mole of covalent bonds is broken in the gaseous state
Endothermic
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
Lattice enthalpy of dissociation
Enthalpy change when one mole of a solid ionic compound is broken up into its constituent ions in the gas phase
Endothermic
Enthalpy of vapourisation
Enthalpy change when one mole of a liquid is turned into a gas
Endothermic
Enthalpy of fusion
Enthalpy change when one mole of a solid is turned into a liquid
Endothermic
What does a gap between experimental and theoretical lattice enthalpies mean?
The larger the gap, the greater the covalent character of the compound and the more distorted the ions