5.1 Thermodynamics Flashcards
Definition of first ionisation enthalpy
The enthalpy change required remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous +1 ions
Definition of second ionisation enthalpy
Enthalpy change required to remove one mole of electrons from one mole of gaseous +1 ions to produce one mole of gaseous 2+ ions
Definition of enthalpy of atomisation
The enthalpy change when one mole of gaseous atoms are formed from their elements or compounds, in its standard state
Definition of bond dissociation enthalpy
The enthalpy change when one mole of a covalent bonds are broken into gaseous atoms
Definition of first electron affinity
The enthalpy change when one mole of gaseous atoms gain one mole of electrons to form one mole of gaseous 1- ions
Definition of second electron affinity
The enthalpy change when one mole of gaseous 1- ions gain one mole of electrons to produce one mole of gaseous 2- ions
Definition of enthalpy of lattice formation
The enthalpy change when one mole of an ionic crystal lattice is formed from its constituent ions in gaseous state
Definition of the enthalpy of lattice dissociation
The enthalpy change when one mole of an ionic crystal lattice is separated into its constituent ions in gaseous form
Definition of enthalpy of hydration
Enthalpy of change when one mole of gaseous ions becomes aqueous ions
The definition of enthalpy of solution
The enthalpy change when one mole of an ionic solid dissolves in excess water
Enthalpy of formation =
Sum of all other enthalpy values
Enthalpy of solution =
Total enthalpy of hydration - enthalpy of lattice formation
OR
Total enthalpy of hydration + enthalpy of lattice dissociation
Mean bond enthalpy =
Total bond enthalpy (reactants) - Total bond enthalpy (products)
Entropy change =
Total entropy of products - total entropy of reactants
Gibbs free energy equation
Delta G = Delta H - T Delta S
