1. Types of Chemical Reactions
Ch. 8 – Chemical Reactions
Types of Chemical Reactions

2. Describing Chemical Reactions
Evidence of a chemical change…
Production of heat and light
Formation of a gas
Formation of a precipitate, a solid product.
Color change

3. Describing Chemical Reactions
A+B  AB
REACTANTS
PRODUCTS

4. Describing Chemical Reactions

5. A. Combination / Synthesis (marriage)
the combination of 2 or more substances to form a compound
only one product
A + B  AB

6. A. Combination / Synthesis
Product:
Must be a compound
Mg(s) + O2(g) 
MgO(s)

7. B. Decomposition (divorce)
a compound breaks down into 2 or more simpler substances
only one reactant
AB  A + B

8. B. Decomposition H2O2 (aq)  Products: Can be elements or compounds
H2O(l) + O2(g)

9. C. Single Replacement (affair)
one element replaces another in a compound
Metal replaces metal
Nonmetal replaces nonmetal
A + BC  B + AC

10. C. Single Replacement
Zn(s) + HCl(aq) 
H2(g) + ZnCl2(aq)

11. D. Double Replacement (Jerry Springer)
ions in two compounds “change partners”
cation of one compound combines with anion of the other
AB + CD  AD + CB

12. D. Double Replacement Pb(NO3)2(aq)+ NaI(aq)  PbI2(s)+ NaNO3(aq)
Products:
Are compounds
Sometimes one of the products is water
Pb(NO3)2(aq)+ NaI(aq) 
PbI2(s)+ NaNO3(aq)

13. CxHy + O2  CO2 + H2O E. Combustion
the burning of a hydrocarbon to produce heat
CxHy + O2  CO2 + H2O

14. E. Combustion Products: During complete combustion the
products are CO2 + H2O
C12H22O11 + 3O2 
9C + 3CO2 + H2O

15. Warm up (practice)
Reaction Types

16. Cu(s) + 2AgNO3(aq)  Cu(NO3)2(aq) + 2Ag(s)1.
Single Replacement
Cu(s) + 2AgNO3(aq)  Cu(NO3)2(aq) + 2Ag(s)

17. 2.
Decomposition
2 H2O(l)  2 H2(g) + O2(g)

18. Combination / Synthesis3.
Combination / Synthesis
H2(g) + Cl2(g)  2 HCl(g)

19. Pb(NO3)2(aq) + K2CrO4(aq)  PbCrO4(s) + 2KNO3(aq)4.
Double Replacement
Pb(NO3)2(aq) + K2CrO4(aq)  PbCrO4(s) + 2KNO3(aq)

20. 5.
Combustion
C2H6 + O2  CO2 + H2O