Thermodynamics definitions

Thermodynamics definitions

1. Enthalpy change of formation: the energy transferred when one mole of the compound is formed from its elements under standard conditions with all of the reactants and products in their standard states

2. Enthalpy of atomisation: the enthalpy change when I mole of gaseous atoms is formed from the element in its standard state under standard conditions

3. Mean bond enthalpy: the enthalpy change when mole of gaseous molecules each breaks a covalent bond to form two free radicals averaged over a range of compounds.

4. First ionisation energy: the enthalpy change when one mole of gaseous atoms is converted to one mole of gaseous ions each with a single posistive charge

5. Second ionisation energy: the enthalpy change to remove one mole of electrons from one mole of gaseous +1 ions to produce a mole of gaseous +2 ions.

6. First electron affinity: the enthalpy change when one mole of gaseous atoms is converted, by gaining a mole of electrons, to a mole of gaseous ions each with a single negative charge.

7. Second electron affinity: the enthalpy change when one mole of electrons is added to a mole of gaseous ions each with a single negative charge to form ions with two negative charges

8. Lattic formation enthalpy: the enthalpy change when one mole of solid ionic compound is formed from its gaseous ions

9. Enthalpy of hydration: the enthalpy change when water molecules surround one mole of gaseous ions.

10. Enthalpy of solution: the 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.