Thermodynamics - Enthalpy definitions 0.0 / 5 ? ChemistryEnthalpyA2/A-levelAQA Created by: AnnaFHarrisonCreated on: 20-10-15 19:05 Enthalpy change of formation The heat change when one mole of a compound is formed from its elements in their standard states under standard conditions. 1 of 13 Bond dissociation enthalpy The heat change when all the bonds of the same type in one mole of gaseous molecules are broken. 2 of 13 Enthalpy change of atomisation of an element The heat change when one mole of gaseous atoms is formed from an element in its standard state, 3 of 13 Enthalpy change of atomisation of a compound The heat change when one mole of compound is its standard state is converted into gaseous atoms. 4 of 13 First ionisation enthalpy The heat change when one mole of electrons are removed from one mole of gaseous atoms to form one mole of gaseous unipositive (1+) ions. 5 of 13 Second ionisation enthalpy The energy change when one mol of electrons are removed from one mole of gaseous unipositive ions to form one mole of gaseous 2+ ions. 6 of 13 First electron affinity The energy change when one mole of gaseous 1- ions are formed from one mole of gaseous atoms. 7 of 13 Second electron affinity The energy change when one mol of gaseous 2- ions are formed from one mole of gaseous 1- ions. 8 of 13 Enthalpy change of hydration The heat change when one mole of aqueous ions are formed from one mole of gaseous ions. 9 of 13 Enthalpy change of solution The heat change when one mole of solute is dissolved in a sufficient solvent so that no further enthalpy change occurs upon further dilution. 10 of 13 Lattice formation enthalpy The enthalpy change when one mole of a solid ionic compound is formed from its gaseous ions under standard conditions. 11 of 13 Lattice dissociation enthalpy The enthalpy change when one mole of a solid ionic compound is completely dissociated into its gaseous ions under standard conditions. 12 of 13 Mean bond enthalpy The heat change when a covalent bond is broken, averaged over a wide variety of different molecules, under standard conditions. 13 of 13
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