Enthalpy Definitions

Definitions for all the enthalpy changes.

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  • Created by: Hannah
  • Created on: 22-05-14 14:49

Enthalpy of formation:

The standard molar enthalpy of formation, is the enthalpy change when one mole of a compound is formed from its constituent elements under standard conditions, all reactants and products in their standard states.

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Enthalpy of atomisation:

The standard enthalpy of atomisation, is the enthalpy change which accompanies the formation of one mole of gaseous atoms from the element in its standard state under standard conditions.

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Enthalpy of ionisation:

First ionisation energy, is the standard enthalpy change when one mole of gaseous atoms is converted into a mole of gaseous ions each with a single positive charge.

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Enthalpy of the first electron affinity:

The first elecron affinity, is the standard enthalpy change when a mole of gaseous atoms is converted to a mole of gaseous ions, each with a single negative charge.

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Enthalpy of the second electron affinity:

The second electron affinity, is the enthalpy change when a mole of electrons is added to a mole of gaseous ions each with a single negative charge to form ions each with two negative charges.

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Enthalpy of lattice formation:

Lattice formation enthalpy, is the standard enthalpy change when one mole of solid ionic compound is formed from its gaseous ions.

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Enthalpy of hydration:

Enthalpy of hydration, is the standard enthalpy change when water molecules surround one mole of gaseous ions.

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Enthalpy of solution:

Enthalpy of solution, is the standard enthalpy change when one mole of solute dissolves completely in sufficient solvent to form a solution in which the molecules or ions are far enough apart not to interact with each other.

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Enthalpy of mean bonds:

Mean bond enthalpy, is the enthalpy change when one mole of gaseous molecules breaks a covalent bond to form two free radicals, averaged over a range of compounds.

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