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EEE

energy electrons and enthalpy

TermDefinition
Enthalpy of formation enthalpy change when one mole of substance is formed from its constituent elements with all substances in their standard states
Enthalpy of combustion enthalpy change when one mole of substance undergoes complete combustion in oxygen with all substances in standard states
Ionisation enthalpy first ionisation energy is the enthalpy change when one mole of gaseous atoms loses one electron per atom to produce gaseous 1+ ions
Electron affinity the first electron affinity is the enthalpy change when one mole of gaseous atoms gains one electron per atom to produce gaseous 1- atoms
enthalpy of atomisation enthalpy change when one mole of gaseous atoms is produced from an element in its normal state
hydration enthalpy enthalpy change when one mole of gaseous ions became hydrated (dissolved in water) forming one mole of aq ions
Enthalpy of solution enthalpy change when one mole of ionic solid dissolves in an amount of water large enought that the dissolved ions are well separated and do not interact with each other
bond dissociated enthalpy enthalpy change when one mole of covalent bonds is broken in the gaseous state
lattice enthalpy of formation ethalpy change when one mole of solid ionic compound is formed from its constituent ions in the gas phase
lattice enthalpy of dissociation enthalpy change when one mole of a solid ionic compound is broken into its constituent ions in the gas phase
enthalpy energy change
Lattice enthalpy enthalpy change that accompanies the formation of one mole of ionic compound from its gaseous ions under standard conditions
Hess' law if a reaction can take place by more than one and the inital and final conditions are the same, the total enthalpy change is the same for each route.
enthalpy change of neutralisation enthalpy change that occurs when one mole of water is formed from adding an alkali and an acid together under standard conditions
Created by: 07blandforderin
 

 



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