2Vocab 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
3Solubility RulesIons that are soluble and do NOT form a precipitate in the reactionGroup 1 metals are solubleNitrates and acetates are soluble
4Which 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!
5Complete 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
6Net 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
7After 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