1. Types of Chemical Reactions
Predicting Products from the Reactants

2. Types of Reactions Synthesis reactions Decomposition reactions
Single displacement reactions
Double displacement reactions
Combustion reactions
You need to be able to identify each

3. 1. Synthesis
Example C + O2 O C +  O C
Synthesis: A + B  AB

4. Criss Cross the Charges to Balance
Mg + N  ?
Mg = +2
N = -3
Mg N 
Synthesis: A + B = AB
Mg3N2

5. Ex. Synthesis Reaction

6. Practice Predict the products: Na(s) + Cl2(g)  Mg(s) + F2(g) 
Al(s) + F2(g)  2 2
NaCl(s)
MgF2(s) 2 3 2
AlF3(s)
Now, balance them. (Criss-Cross!)

7. But WAIT! What Does the (s) and (aq) and (g) Mean???
(s) in a chemical equation signifies a SOLID
(g) in a chemical equation is a GAS
(aq) means “aqueous” (LIQUID)
Why do you need to note that? Because sometimes… a phase can change in a reaction!

8. Compound = Element + Element
2. Decomposition
Example: NaCl  Cl Na Cl + Na
General: AB  A + B
Compound = Element Element

9. Ex. Decomposition Reaction

10. Went from neutral (0) to (+2) Went from (+2) to Neutral (0)
3. Single Displacement
Example: Zn + CuCl2
Zn was oxidized
Went from neutral (0) to (+2)  Zn Cl Cu + Cl Zn Cu +
Cu was reduced
Went from (+2) to Neutral (0)
General: AB + C  AC + B
Compound + Element = New Compound + New Element

11. But WAIT! What do “oxidized” and ”reduced” Mean?
Remember?
LEO the lion says GER
Lose electrons = oxidation = LEO
Gain electrons = reduction = GER
Metals LOSE electrons
Non-metals GAIN electrons

12. Ex. Single Replacement Reaction

13. Single Replacement Reactions
Write and balance the following single replacement reaction equations:
Zn(s) HCl(aq)  2
ZnCl2 + H2(g)
NaCl(s) + F2(g) 
Al(s)+ Cu(NO3)2(aq) 2 2
NaF(s) + Cl2(g) 2 3 3
Cu(s)+ Al(NO3)3(aq) 2

14. 4. Double Displacement General: AB + CD  AD + CB Example: MgO + CaS 

15. Double Replacement Reactions
Think about it like “foil”ing in algebra, first and outer ions go together + inside ions go together
Example:
AgNO3(aq) + NaCl(s)  AgCl(s) + NaNO3(aq)
Another example:
K2SO4(aq) + Ba(NO3)2(aq)  KNO3(aq) + BaSO4(s) 2

16. Practice Predict the products: HCl(aq) + AgNO3(aq) 
CaCl2(aq) + Na3PO4(aq) 
Pb(NO3)2(aq) + BaCl2(aq) 
FeCl3(aq) + NaOH(aq) 
H2SO4(aq) + NaOH(aq) 
KOH(aq) + CuSO4(aq) 

17. 5. Combustion Reactions
Combustion reactions – when a hydrocarbon reacts with oxygen gas
This is also called BURNING!
In order to burn something you need the 3 things in the “fire triangle”:
1) Fuel (hydrocarbon) 2) Oxygen 3) Something to ignite the reaction (spark)

18. Combustion Reactions In general: CxHy + O2  CO2 + H2O
Products are ALWAYS
CARBON DIOXIDE AND WATER!
Combustion is used to heat homes and run automobiles (octane, as in gasoline, is a hydrocarbon: C8H18 )

19. Mixed Practice
State the type of reaction & predict the products (try to balance the equation!)
BaCl2 + H2SO4 
C6H12 + O2 
Zn + CuSO4 
Cs + Br2 
FeCO3 