the enthalpy change when one mole of an ionic lattice is formed from its gaseous ions under standard conditions
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Standard Enthalpy of Formation
the enthalpy change when one mole of a compound is formed from its elements in their standard states under standard conditions
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Standard Enthalpy of Atomisation
the enthalpy change when one mole of a gaseous atoms is formed from the element in its standard state, under standard conditions
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Standard Enthalpy of Hydration
enthalpy change when one mole of isolated gaseous ions reacts with water to produce one mole of aqueous ions
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Standard Enthalpy Change of Solution
enthalpy change when one mole of solute dissolves in a large excess of water under standard conditions (can be exothermic or endothermic)
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First Ionisation Enthalpy
the enthalpy change when one mole of gaseous atoms form one mole of gaseous unipositive ions under standard conditions
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Second Ionisation Enthalpy
enthalpy change when one mole of gaseous unipositive ions form one mole of gaseous dipositive ions under standard conditions
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First Electron Affinity
enthalpy change when one mole of gaseous atoms each gain an electron to form negative ions with a charge of 1- under standard conditions
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Second Electron Affinity
enthalpy change when one mole of gaseous 1- ions each gain an electron to form a 2- ion under standard conditions
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Hess's Law
states that the enthalpy change of a reaction is independent of the route taken, provided the initial and final conditions are the same
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Born Haber Cycle
an energy cycle which enables us to calculate lattice enthalpies of ionic compounds from enthalpies of formation, atomisation, ionisation and electron affinities (these are all experimentally determined values)
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Standard Enthalpy of Formation
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the enthalpy change when one mole of a compound is formed from its elements in their standard states under standard conditions
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