1. Synthesis Reactions Also known as direct combination reactions.
Two or more reactants form a single product.
Generic Example:
A + B  AB

2. Synthesis Reactions K+1 and Cl-1 Example: K + Cl2  2 2 KCl
Remember to Balance!

3. Synthesis Reactions Al+3 and Br-1 Example: Al + Br2  2 3 2 AlBr3
Remember to Balance!

4. Decomposition Reactions
A single reactant is broken down into two or more products.
Generic Example:
AB  A + B

5. Decomposition Reactions
Diatomic!!!
Example: NaCl  2 2 Na
+ Cl2
Remember to Balance!

6. Decomposition Reactions
Diatomic!!!
Example: Al2O3  2 4 Al
+ O2 3
Remember to Balance!

7. Single-Replacement Rxns
A single element replaces an element in a compound to form a new compound and element.
Generic Example:
A + BX  AX + B
Click here for a video that shows Ag replacing Cu

8. Single-Replacement Rxns
You must use the Activity Series to determine if a reaction will work!
Metals will replace other metals that appear below them
(Pg. 295) [

9. Single-Replacement Rxns
Mg+2 and NO3-1
Mg + AgNO3 2
Mg(NO3)2
+ Ag 2
Replaced Metal
Mg is above Ag, so the reaction will work! [

10. Single-Replacement Rxns
“No Reaction”
Cu + FeSO4 NR
Cu is below Fe, so the reaction will NOT work! [

11. Single-Replacement Rxns
Non-metals will replace other non-metals that are below them on the periodic table. [

12. Single-Replacement Rxns
K+1 and Cl-1
Cl2 + KI 2 2
KCl
+ I2
Diatomic!
Cl is above I, so the reaction will work! [