1. Practice What type of reaction is described by the following equation?
6Li + N2  2Li3N
2C8H18(l) + 25 O2(g)  16CO2(g) + 18H2O(l)
2NaCN(aq) + H2SO4(aq)  2HCN(s) + Na2SO4(aq)
2HgO(s)  2 Hg(l) + O2(g)
Br2(aq) + NaI(aq)  NaBr(aq) + I2(aq)

2. Predicting Products
Now that you have learned about some of the basic reaction types, you can predict the products of many reactions.
The number of elements and/or compounds in the reactants is a good indicator of possible reaction type and thus the possible products.

3. Practice Predicting Products
Predict the products for the following reactions and balance the equations:
Al + Cl2 
C2H2 + O2 
Ag + HCl 
MgCl2 
CaI2 + Hg(NO3)2 
Na2S + Cd(NO3)2 

4. Net Ionic Equations NOTES #11
Aqueous solutions  It means something is dissolved in water!
Example:
AgNO3(aq) + NaCl(aq)  AgCl(s) + NaNO3(aq)
(aq) means it is dissolved in water.
Why is there a solid? (s)
It represents that a reaction has occured.

5. Whenever a solid is formed, we call this a precipitate
To show this reaction, we do the NET IONIC EQUATION.
Beginning Equation:
AgNO3(aq) + NaCl(aq)  AgCl(s) + NaNO3(aq)
Complete Ionic Equation:
Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq) 
AgCl(s) + Na+(aq) + NO3-(aq)

6. Cancel out spectator ions on each side: Never cancel out the solid.
When that happens, you will have your NET IONIC EQUATION
It only shows what is important.
Ag+(aq) + Cl-(aq)  AgCl(s)
A REACTION ONLY OCCURS IN AQUEOUS SOLUTIONS WHEN A PRECIPITATE FORMS.

7. Practice Give the net ionic equation: Na3PO4(aq) + FeCl3(aq) 
How will you know which is the precipitate?
Refer to table 11.3 on page 344.