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EEE
energy electrons and enthalpy
Term | Definition |
---|---|
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 |