1. Net Ionic Equations

2. Net Ionic Equations
Net ionic equations are used to show which ions participate in the reaction.
Ions that do NOT participate in the reaction are spectator ions.

3. Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq) → AgCl(s) + Na+(aq) + NO3- (aq)
Net Ionic Equations
Overall equation: AgNO3 (aq) + NaCl (aq) → AgCl (s) + NaNO3 (aq)
Separate all of the ions:
Compounds that are soluble (AKA - aq) will separate into their ions. Precipitates (AKA - s) DO NOT separate.
Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq) → AgCl(s) + Na+(aq) + NO (aq)
Cross out all spectator ions - the ions that appear on both the reactant and product side of the equation.

4. Net Ionic Equations
Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq) → AgCl(s) + Na+(aq) + NO3- (aq)
What remains is the net ionic equation:
Ag+(aq) + Cl-(aq) → AgCl (s)
Balancing Net Ionic Equations: must be balanced with respect to both coefficients and charge

5. FeCl3 (aq) + KOH (aq) →
Predict the products of the following reaction.
Write the FULL ionic equation. (Yes - the long one)
Write the NET IONIC EQUATION.
What are the spectator ions.

6. ANSWERS FeCl3 (aq) + KOH (aq) →
Predict the products of the following reaction.
Fe (OH )3+ KCl
b. Write the FULL ionic equation. (Yes - the long one)
FeCl3 (aq) + KOH (aq) → Fe (OH)3 (s) + KCL (aq)
NOW… BALANCE
FeCl KOH  Fe(OH)3 + 3KCL c. Write the NET IONIC EQUATION.
Fe+3 (aq) + Cl-1 (aq) + 3K+1 (aq) + 3 OH-1 (aq) -- Fe (OH)3 (s) + 3K+1 (aq) + 3 Cl-1 (aq)
d. What are the spectator ions. Cl -, K+

7. Practice from equations we just did
Net Ionic Equations
Practice from equations we just did

8. Today’s Agenda ???? TEST TOMORROW!!!!!
Turn in Double Replacement lab to the tray ASAP!
Have out Study Guide homework to be checked.
We are going over the study guide. What questions do you have?
Re-Quiz
Reactions partner activity.
TEST TOMORROW!!!!!