Thermodynamics Flashcards
Define lattice formation of enthalpy
Enthalpy change when 1 mole of a solid ionic compound is formed from its gaseous ions
Define lattice dissociation enthalpy
Enthalpy change when 1 mole of a solid ionic compound is completely dissociated into its gaseous ions
What does a big difference in theoretical and experimental enthalpy change tell you?
Shows ionic bonds are strongly polarised with a large degree of covalency
Enthalpy change of formation
Enthalpy change when 1 mole of a compound is formed from its elements in their standard states
Bond dissociation enthalpy
Enthalpy change when all the bonds of the same type in 1 mole of gaseous molecules are broken
Enthalpy change of atomisation of an element
Enthalpy change when 1 mole of gaseous atoms is formed from an element in its standard state
Enthalpy change of atomisation of a compound
Enthalpy change when 1 mole of a compound in its standard state is converted to gaseous atoms
1st ionisation energy
Enthalpy change when 1 mole of gaseous 1+ ions is formed from 1 mole of gaseous atoms
2nd ionisation energy
Enthalpy change when 1 mole of gaseous 2+ ions is formed from 1 mole of gaseous 1+ ions
1st electron affinity
Enthalpy change when 1 mole of gaseous 1- ions is formed from 1 mole of gaseous atoms
2nd electron affinity
Enthalpy change when 1 mole of gaseous 2- ions is made from 1 mole of gaseous 1- ions
Enthalpy change of hydration
Enthalpy change when 1 mole of aqueous ions is formed from gaseous ions
Enthalpy change of solution
Enthalpy change when 1 mole of an ionic substance dissolves enough solvent to form an infinitely dilute solution
Define entropy
The measure of the disorder of a system
Equation for S, entropy change
Unit?
What does a positive value for Ssystem tell you?
Ssystem = Sprod - Sreac
JK-1mol-1
Right side of the reaction is favoured