2 Vocab to know: Soluble – dissolves (goes away) in solution Precipitate – does not dissolve in solution, forms a chunky solid in the solutionSpectator Ions – ions that are soluble in solution and do not form a precipitate
3 Solubility RulesIons that are soluble and do NOT form a precipitate in the reactionGroup 1 metals are solubleNitrates and acetates are soluble
4 Which compound is the precipitate? AgNO3 + NaCl AgCl + NaNO3Na+ is a group 1 metal, so it is solubleNitrates (NO3-) are also solubleThe solubility rules do not say anything about silver or chloride, so this will form the precipitate!
5 Complete Ionic Equations Shows the dissolves particles as free ions in the solutionExample:AgNO3 + NaCl AgCl + NaNO3Ag+ + NO Na+ +Cl- AgCl + Na+ + NO3-Complete Ionic Reaction
6 Net Ionic Equations Shows only the ions that actual cause a reaction Cross out the “Spectator Ions”Example:Ag+ + NO Na+ +Cl- AgCl + Na+ + NO3-Ag+ + Cl- AgClNet Ionic Reaction
7 After reading Section 8.3, you should know: How to apply the solubility rules to determine which compound will form a precipitateHow to write a complete and net ionic equation