2Net-ionic EquationsNet ionic equations are useful in that they show only those chemical species directly participating in a chemical reactionThe keys to being able to write net ionic equations are the ability to recognize monatomic and polyatomic ions, the solubility rules, and the rules for electrolyte behavior.
3Net ionic equations Complete ionic equations An ionic equation that shows all of the particles in a solution as they realistically exist2 Na+ (aq) + 2OH- (aq) + Cu+2 (aq) + 2Cl- (aq) 2 Na + (aq) + 2 Cl- (aq) + Cu(OH)2 (s)Note that the sodium ions and the chloride ions are both reactants and products, therefore they do not participate in the reactionIons that do not participate in the reaction are called spectator ions
4Net-ionic EquationsIonic equations that include only the particles that participate in the reaction are called net ionic equationsNet ionic equations are written form complete ionic equations by crossing out all spectator ionsExample:2 Na+ (aq) + 2OH- (aq) + Cu+2 (aq) + 2Cl- (aq) 2 Na + (aq) + 2 Cl- (aq) + Cu(OH)2 (s)
5Net-ionic EquationsA net ionic equation is what remains after the sodium and chloride ions are crossed out of this complete ionic equation2OH- (aq) + Cu +2 (aq) Cu(OH)2Only the hydroxide and copper ions are left in the net ionic equation shown above
6Example:Write the chemical, complete ionic, and net ionic equations for the rxn between aqueous solutions of barium nitrate and sodium carbonate that forms the precipitate barium carbonate.Complete Ionic Equation:Ba(NO3)2 (aq) + Na2CO3 (aq) BaCO3 (s) + NaNO3 (aq)Balance the equation above:Ba(NO3)2(aq) + Na2CO3 (aq) + BaCO3 (s) + 2 NaNO3 (aq)
7Example continued: Show the ionic states of the reactants and products Ba+2 (aq) + 2NO3- (aq) + 2Na+ + CO3-2 (aq) BaCO3 (s) + 2 Na+ (aq) + 2NO3- (aq)Cross out the spectator ions from the complete ionic equation:
8Example continued: The net ionic equation is: Ba+2 (aq) + CO3-2 (aq) BaCO3 (s)
9PracticeWork on problems on pg. 294 of your chemistry book