1. Spontaneous Decompositions n H 2 CO 3 (aq) -> H 2 0 (l) + CO 2 (g) n NH 4 OH (aq) -> H 2 O (l) + NH 3

2. Net Ionic Reactions : 3 steps n 1. Complete balanced equation n 2. Complete Ionic Equation  -break “aq” states into ions  -Cross out identical reactants and products n 3. Net ionic equation  If a No reaction, then no net ionic equation.

3. n Spectator Ion = an ion that appears on both sides of an equation and is not directly involved in the reaction

4. Single Replacement 1Cu (s) + 2AgNO 3 (aq) -> 1Cu(NO 3 ) 2 (aq) + 2Ag (s) 1Cu (s) + 2Ag 1+ ( aq) +2NO 3 1- (aq) -> 1Cu 2+ + 2NO 3 1- (aq) + 2Ag(s) 1Cu (s) + 2Ag 1+ ( aq) -> 1Cu 2+ + 2Ag(s) Complete: Net Balanced:

5. Double Replacement AgNO 3 (aq) + KCl(aq)  AgCl(s) + KNO 3 (aq) Ag + (aq) + NO 3 – (aq) + K + (aq) + Cl – (aq)  AgCl(s) + K + (aq) +NO 3 – (aq) Compelte: Balanced: Net Ag + (aq) + Cl – (aq)  AgCl(s)

6. Net Ionic Reactions! - DR Pb(NO 3 ) 2 (aq) +2LiCl(aq)  PbCl 2 (s) + 2LiNO 3 (aq) Pb +2 (aq) +2NO 3 – (aq) +2 Li + (aq) +2Cl – (aq)  PbCl 2 (s)+2Li + (aq) +2NO 3 – (aq) C: Balanced: Net: Pb +2 (aq) + 2Cl – (aq)  PbCl 2 (s)