AQA Year 2 Physical Definitions Flashcards
Enthalpy of Formation
The enthalpy change when 1 mol of a compound, is formed from its elements, Under standard conditions, all substances in standard states
Ionisation Enthalpy
The minimum amount of energy required to remove one mole of electrons from one mole of atoms in the gaseous state.
Enthalpy of Atomisation
The enthalpy change for the formation of one mole of gaseous atoms from the element in its standard state under standard conditions.
Bond Dissociation Enthalpy
Enthalpy change to break the bond in 1 mol of gaseous molecules, To form gaseous atoms
Mean Bond Enthalpy
Enthalpy change to break 1 mol of covalent bonds, averaged over a range of compounds
Electron Affinity
Enthalpy change when one mole of gaseous atoms Form one mole of gaseous negative ions
Lattice Dissociation Enthalpy
Enthalpy change to separate 1 mol of an ionic solid into its gaseous ions
Lattice Formation Enthalpy
Enthalpy change when one mole of a solid ionic compound is formed from its gaseous ions.
Enthalpy of Hydration
enthalpy change when 1 mol of gaseous ions is converted into aqueous ions
Enthalpy of Solution
Enthalpy change when one mole of solid dissolves in water to form aqueous ions
Enthalpy of Combustion
The enthalpy change when 1 mol of a substance, Is completely burned in oxygen, Under standard conditions, all substances in standard states
o(theta symbol) in o(theta)H?
standard conditions
Perfect Ionic Model
Ions can be regarded as perfect spheres
Order of Reaction
Power of concentration term (in rate equation)
Bronsted-Lowry acid
H+ donor
Bronsted-Lowry base
H+ acceptor
Ionic Product of Water
Kw = [H+][OH-]
Weak Acid / Weak Base
Slightly Dissociate
Strong Acid / Strong Base
Completely Dissociate
Buffer
A solution which maintains pH despite the addition of acid or base
