1. Types of Chemical Reactions
Single Replacement, Double Replacement, and Combustion Reactions

2. Single Replacement Reactions

3. Single Replacement Reactions
one element replaces another in a compound
metal replaces metal (+)
nonmetal replaces nonmetal (-)
A + BC  B + AC
A + BC  C + BA

4. Activity Series of Metals & Halogens
Single Replacement
Activity Series of Metals & Halogens
free element must be more active
(check activity series) Li K Ca Na Mg Al Zn Fe Pb H Cu Hg Ag F Cl Br I
Decreasing reactivity ←

5. Single Replacement N.R. Cu(s)+ FeSO4(aq) Br2(l)+ NaCl(aq) 
Fe(s)+ CuSO4(aq) 
Cu(s)+ FeSO4(aq)
Br2(l)+ NaCl(aq) 
N.R.

6. Single Replacement Problems
1) Zn(s) + H2SO4 (aq) →
2) Sn(s) + NaNO3 (aq) →
3) Cl2(g) + NaBr(aq) →
4) Mg(s) + LiNO3(aq) →
ZnSO4 (aq) + H2 (g)
No reaction
NaCl (aq) + Br2 (l)
No reaction

7. Double Replacement Reactions

8. Double Replacement Reactions
ions in two compounds “change partners”
cation of one reactant combines with anion of the other reactant
AX + BY  AY + BX

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

10. Double Replacement Products
one product is insoluble and precipitates (check solubility table)
Na2S(aq) + Cd(NO3)2(aq) →
CdS(s) + NaNO3(aq) 2
NaNO3(aq)+ KI(aq) 
NaI(aq) + KNO3(aq)
No precipitate – No reaction

11. Double Replacement Products
One product is a gas that bubbles out of the mixture 2
NaCN(aq) + H2SO4(aq) → 2
HCN(g) + Na2SO4(aq)
NaHCO3(aq) + HC2H3O2(aq) →
H2CO3(aq) + NaC2H3O2(aq) ↓
CO2(g) + H2O(l)

12. Double Replacement Products
One product is a molecular compound such as water
Example:
An antacid neutralizes stomach acid.
Ca(OH)2(aq) + HCl(aq) → 2
CaCl2(aq) + H2O(l) 2

13. Double Replacement Practice
Predict the products. Determine the precipitate.
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) 
HNO3(aq) + AgCl(s)
Ca3(PO4)2(s) + NaCl(aq)
PbCl2(s) + Ba(NO3)2(aq)
Fe(OH)3 (s) + NaCl (aq)
H2O (l) + Na2SO4 (aq)
K2SO4 (aq) + Cu(OH)2(s)

14. Going Backwards…
Fill in the appropriate reactants based on the given products.
1) → AgBr(s) + KNO3(aq)
2) → BaSO4(s) + 2NaCl(aq)
3) → KCl(aq) + CaSO4 (s)

15. Combustion Reactions

16. A + O2  B S(s) + O2(g)  SO2(g) Combustion Reactions
the burning of any substance in O2 to produce heat
A + O2  B
S(s) + O2(g)  SO2(g)

17. CxHy + O2  CO2 + H2O Combustion Reactions
hydrocarbons combine with oxygen to form CO2 + H2O
CxHy + O2  CO2 + H2O
CH4(g) + 2O2(g)  CO2(g) + 2H2O(g)

18. Combustion
Products in combustion are carbon dioxide and water. (although incomplete burning does cause some by-products like carbon monoxide)
Combustion is used to heat homes and run automobiles (octane, as in gasoline, is C8H18)

19. Combustion 8 5 6 C5H12(g) + O2(g)  CO2 + H2O 4 2 Na(s)+ O2(g) 
Examples
C5H12(g) + O2(g) 
CO2 + H2O
Na(s)+ O2(g) 
Na2O(s)
C3H8(g)+ O2(g) 
CO2(g)+ H2O(g)

20. Combustion Practice C6H6 + O2  CH3OH + O2  Mg + O2  CO2 + H2O