1. We will study 5 types of reactions
Decomposition
Synthesis
Combustion
Single-Replacement
Double-Replacement

2. Decomposition Reactions (split)
One substance breaks into 2 or more substances
AB  A + B
Examples
H2O 
MgCl2  Mg (s) + Cl2(g)

3. Synthesis Reactions (combine)
2 reactants  1 product
A + B  AB
Examples
Na + Cl2 
Fe + O2 

4. Combustion reactions
A substance combines with oxygen and produces heat/energy
There are 2 types combustion reactions
Synthesis
metal plus oxygen  oxide
Mg + O2 
Fuel + O2  CO2 + H2O
C2H6 + O2  CO2 + H2O
CxHy coefficient is 1 for odd x and 2 for even x

5. Practice 1) predict product 2) type of reaction 3) balance the equation
Hydrogen (g) + chlorine (g) 
Decane (C10H22) (l) + oxygen (g) 
Magnesium chlorate (s) 
Iron (III) + oxygen (g) 

6. Single displacement reactions
Atoms of an element switch places with atoms of another element in a compound.
A + BX  AX + B
Not all replacements are possible
The single element must be higher on the activity series than the element in the compound

7. Underline the element that would replace the other in a single replacement reaction.
a. calcium, tin
b. bromine, fluorine
c. aluminum, potassium
d. zinc, sodium
e. iron, copper
f. iodine, chlorine
g. silver, lead

8. Single Replacement (displacement) reactions
Al (s) + CuCl2 
Cu + NaCl 
Zn + SnCl2 
K (s) + ZnCl2 (aq) 
Cl2 (g) + HF (aq) 
Pb (s) + H2O (aq) 

9. Double (displacement) Replacement
Exchange of ions between 2 compounds
AX + BY  AY + BX
Can form a precipitate (solid), determined by solubility rules
PbSO4 + HCl 
Hg(NO3)2 + KI 

10. Classify These Reactions
1) CH4 (g) + O2 (g)  CO2 (g) + H2O (l)
2) Mg (s) + AlCl3(aq)  Al (s) + MgCl2(aq)
3) Al (s) + S (s)  Al2S3 (s)
4) H2 (g) + O2(g)  H2O (g)
5) F2(g) + NaBr(aq)  NaF (aq) + Br2 (l)
6) NaN3 (s)  Na (s) + N2 (g)