Unit 5 - Energetics, Redox, Inorganic Chemistry (THERMODYNAMICS)
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P - Thermodynamics
Definitions:
Enthalpy change of formation: Enthalpy change when one mole of a compound
is formed from its constituent elements in standard conditions with the reactants
and products in standard states (= 0 by definition for elements)
Enthalpy change of combustion: Enthalpy change when one mole of compound
is fully burned in oxygen in standard conditions with all reactants and products in
their standard states under standard conditions
Enthalpy change of neutralisation: Enthalpy change when one mole of water is
formed when an acid and base neutralise each other under standard conditions
with all reactants and products in their standard states
Enthalpy change of atomisation: Enthalpy change when one mole of gaseous
atom are formed from the element in its standard state under standard
conditions.
Enthalpy change of first ionisation energy: Enthalpy change when one mole of
electrons are removed from one mole of gaseous atoms to form one mole of 1+
ions in their gaseous states under standard conditions.
Enthalpy change of second ionisation energy: Enthalpy change when one
mole of electrons are removed from one mole of gaseous 1+ ions to form 1 mole
of gaseous 2+ ions under standard conditions
Enthalpy change of first electron affinity: Enthalpy change when one mole of
electrons are gained by one mole of gaseous atoms to form one mole of 1-
gaseous ions under standard conditions
Enthalpy change of second electron affinity: Enthalpy change when one mole
of electrons are gained by 1 mole of gaseous 1- ions to form one mole of
gaseous 2- ions under standard conditions.
Lattice enthalpy of formation: Enthalpy change when one mole of a solid ionic
compound is formed from its constituent ions in the gaseous state under
standard conditions.
Lattice enthalpy of dissociation: Enthalpy change when one mole of solid
ionic compound is dissociated into its constituent ions in the gaseous states
under standard conditions
P - Thermodynamics 1
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