1. 5 types of reactions

2.  + O O What do you observe about this reaction?
What are the atoms doing?
This rxn is known as….

3. Combination/Synthesis+  O C
Combination/Synthesis
A B  AB
multiple reactants
forms
always 1 product
Mg3N2 (s)
Mg (s) + N2 (g) ®

4.  + Cl Cl Na Na What do you observe about this reaction?
What are the atoms doing?
This rxn is known as….

5. Decomposition  + Cl Na Cl Na AB  A + B NiCO3 (aq)  + Ni (s) CO2 (g)
Always 1 reactant breaks down into multiple products
Compound falls apart
NiCO3 (aq) 
+ Ni (s)
CO2 (g)

6.  + + Zn Cl Cu Cl Zn Cu What do you observe about this reaction?
What are the atoms doing?
This rxn is known as….

7. Single Replacement/Displacement Zn Cl Cu + Cl Zn Cu +
Single Replacement/Displacement
AB C  CB A
STRONGER single element
kicks out
weaker
forms
new compound & new single element

8. Single Replacement/Displacement Zn Cl Cu + Cl Zn Cu +
Single Replacement/Displacement
When determining strength..
**Look at Activity Series –table 3 pg 286

9. Activity Series of Metals Activity Series of NonMetals
F2 Fluorine
Cl2 Chlorine
Br2 Bromine
I2 Iodine
Activity
Series of
Metals
Activity
Series of
NonMetals

10. Single Replacement/Displacement Zn Cl Cu + Cl Zn Cu +
Single Replacement/Displacement
When replacing an element….
**Metal kicks out Metal
**Nonmetal kicks out Nonmetal
2Na + SrCl2 ®
Sr + 2NaCl
F2 + LiCl ®
LiF + Cl2

11.  + + O Mg Ca O Mg Ca What do you observe about this reaction?
What are the atoms doing?
This rxn is known as….

12. Double Replacement/Displacement Mg Ca + O S Mg Ca +
Double Replacement/Displacement
AB + CD  AD CB
Compounds “switch”
partners
forms
2 new compounds
ZnS HCl ®
ZnCl + H2S

13. What do you need to make fire?
Can you light a fire on the moon?
What are the products of fire?

14. Combustion CxHy + O2  CO2 + H2O
Hydrocarbon always  always always
oxygen carbon dioxide water
C3H8 + O2 ® CO2 + H2O

15. Acid –Base (Neutralization)
Acid (H+) Base (OH-) → Salt H2O
Ionic compound
NaOH + HCl → NaCl + H2O

16. Na(s) + H2O (l)  NaOH ( aq) + H2 (g)
2.CO(g) + O2(g)  CO2
3.FeS(s) + HCl(aq)  FeCl2 (aq) + H2S (g)
4. NaNO3 (s)  NaNO2 (s) + O2 (g)
5. CH4(g) + O2(g)  CO2(g) + H2O (g)
6. Fe(s) + CuNO3(aq)  Cu(s) + Fe(NO3)2 (aq)
7. KI(aq) + Cl2 (g)  KCl (aq) + I2(aq)
8. Al(s) + S(s)  Al2S3 (s)
9. KClO3 (s)  KCl(s) + O2 (g)
10. C4H10 (g) + O2(g)  CO2(g) + H2O (g) SR
SYN DR
DECOMP
COMBUS SR SR
SYN
DECOMP
COMBUS

17. How to recognize which type
Look at the reactants
Element(E), Compound(C)
E + E C
E + C
C + C
Acid + Base
Look at the Products
CO2 + H2O
Synthesis
Decomposition
Single replacement
Double replacement
Acid/Base reaction
Combustion

18. Examples Synthesis H2 + O2 ® H2O ® Decomposition AgNO3 + NaCl ®
Double replacement
Zn + H2SO4 ®
Single replacement
HgO ®
Decomposition
KBr +Cl2 ®
Single replacement
Mg(OH)2 + H2SO3 ®
Double replacement

19. Examples Acid/Base HNO3 + KOH ® Decomposition CaPO4 ® AgBr + Cl2 ®
Single replacement
Zn + O2 ®
Synthesis
HgO + Pb®
Single replacement
HBr + NH4OH ®
Acid/Base
Cu(OH)2 + KClO3 ®
Double replacement