Definition of
∆Hf - Formation
The enthalpy change when 1 mole of compound is formed from its elements in their standard states under standard conditions
Definition of
∆Hat - Atomisation
The enthaply change when 1 mole of gaseous atoms forms from their elements in their standard states under standard conditions
Definition of
∆Hi - 1st ionisation
The enthalpy change when 1 mole of e⁻ is removed from 1 mole of gaseous atoms to form 1 mole of gaseous 1+ ions under standard conditions
Definition of
∆Hi2 - 2nd ionisation
The enthalpy change when 1 mole of e⁻ is removed from 1 mole of gaseous 1+ ions to form 1 mole of gaseous 2+ ions under standard conditions
Definition of
∆Hea - Electron Affinity
The enthalpy change when 1 mole of e⁻ is added to 1 mole of gaseous atoms to form 1 mole of gaseous 1- ions under standard conditions
Definition of
∆Hea2 - 2nd Electron Affinity
The enthalpy change when 1 mole of e⁻ is added to 1 mole of gaseous 1+ ions to form 1 mole of gaseous 2- ions under standard conditions
Definition of
∆Hhyd - Hydration
The enthalpy change when 1 mole of aqueous ions are formed from 1 mole of gaseous ions under standard conditions
Definition of
∆Hsol - Solution
The enthalpy change when 1 mole of solute is dissolved in excess solvent to form a solution, in which the ions are far apart not to interact with each other under standard conditions
Definition of
∆HLE - Lattice Enthalpy
The enthalpy change when 1 mole of ionic compound is formed from its gaseous ions under standard conditions
Definition of
∆HL.D.E - Lattice Diss. Enthalpy
The enthalpy change when 1 mole of ionic compound dissociates into its gaseous ions under standard conditions
Strong Acids - Fully Dissociate
Name 3 Strong Acids
HCl | H₂SO₄ | H₃PO₄
Weak Acids - Partially Dissociate
Name 1
Carboxylic Acid (CH3COOH)
Strong Bases - Fully Dissociate
Name 3
NaOH
KOH
LiOH
Weak Bases - Partially Dissociate
Name 1
NH3 + H2O -> NH4^+ + OH^-