1. Types of Chemical Reactions
Unit 3 Topic 3
Chapter 8.2 and 8.3

2. Types of Chemical Reactions
There are several ways to classify chemical reactions.
Synthesis
Decomposition
Single-displacement (replacement)
Double-displacement (replacement)
Combustion reactions

3. Synthesis Reactions A + B → AB Synthesis
two or more substances combine to form a new compound.
A + B → AB
A and B can be elements or compounds.
AB is a compound

4. Synthesis Reactions

5. Synthesis Reactions 4 Li + O2 → 2 Li2O 2Mg(s) + O2(g) → 2MgO(s)
One simple type of synthesis reaction is the combination of
an element with oxygen to produce an oxide.
Almost all metals react with oxygen to form oxides.
2Mg(s) + O2(g) → 2MgO(s)
Group 2 elements react to form oxides with the formula MO, where M represents the metal.
Group 1 metals form oxides with the formula M2O.
4 Li + O2 → 2 Li2O

6. Synthesis Reactions 16Rb(s) + S8(s) → 8Rb2S(s)
The Group 1 and Group 2 elements react similarly with sulfur, forming sulfides with the formulas M2S and MS, respectively.
16Rb(s) + S8(s) → 8Rb2S(s)
8Ba(s) + S8(s) → 8BaS(s)

7. Synthesis Reactions S8(s) + 8O2(g) → 8SO2(g) 2H2(g) + O2(g) → 2H2O(g)
Nonmetals also undergo synthesis reactions with oxygen to form oxides.
Sulfur reacts to form sulfur dioxide.
S8(s) + 8O2(g) → 8SO2(g)
Hydrogen reacts with oxygen to form dihydrogen monoxide (water).
2H2(g) + O2(g) → 2H2O(g)

8. Synthesis Reactions 2Na(s) + Cl2(g) → 2NaCl(s) Mg(s) + F2(g) → MgF2(s)
Group 1 metals react with halogens to form ionic compounds with the formula MX, where M is the metal and X is the halogen.
2Na(s) + Cl2(g) → 2NaCl(s)
Group 2 metals react with the halogens to form ionic compounds with the formula MX2.
Mg(s) + F2(g) → MgF2(s)

9. CaO(s) + H2O(l) → Ca(OH)2(s)
Synthesis Reactions
Oxides of active metals react with water to produce metal hydroxides.
Calcium oxide reacts with water to form calcium hydroxide.
CaO(s) + H2O(l) → Ca(OH)2(s)

10. Decomposition Reactions
a single compound undergoes a reaction that produces two or more simpler substances.
Decomposition reactions are the opposite of synthesis reactions.
AB → A + B
AB is a compound.
A and B can be elements or compounds.

11. Decomposition Reactions
Decomposition of Binary Compounds
Electrolysis.
2 H2O(l) → 2 H2(g) + O2(g)
electricity
Oxides of the less-active metals, which are located in the lower center of the periodic table, decompose into their elements when heated.
2 HgO(s) → 2 Hg(l) + O2(g) Δ

12. Electrolysis

13. Decomposition Reactions
Decomposition of Metal Carbonates Δ
CaCO3(s) → CaO(s) + CO2(g)
Decomposition of Metal Hydroxides Δ
Ca(OH)2 → CaO(s) + H2O(g)
Decomposition of Metal Chlorates Δ
2 KClO3(s) → 2 KCl(s) O2(g)

14. Decomposition Reactions
Decomposition of Acids
Certain acids decompose into nonmetal oxides and water.
H2CO3(aq) → CO2(g) + H2O(l)

15. Single-Displacement Reactions
In a single-displacement (replacement) reaction, one element replaces a similar element in a compound.
Many single-displacement reactions take place in aqueous solution.
Single-displacement reactions can be represented by the following general equations:
A + BX → AX + B, Y + BX → BY + X
A, B, X, and Y are elements. AX, BX, and BY are compounds.

16. How do we know if a replacement will occur?
We look at an activity series.

17. Activity Series of the Elements

18. Single-Displacement Reactions
Displacement of a Metal in a Compound by Another Metal
Al(s) + Pb(NO3)2(aq) →
Pb(s) + Al(NO3)3(aq)
2Al(s) + 3Pb(NO3)2(aq) → 3Pb(s) + 2Al(NO3)3(aq)

19. Single-Displacement Reactions
Displacement of Hydrogen in Water by a Metal
Na(s) + H2O(l) →
NaOH(aq) + H2(g)
2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)
Fe(s) + H2O(g) →
Fe2O3(s) + H2(g)
2Fe(s) + 3H2O(g) → Fe2O3(s) + 3H2(g)

20. Single-Displacement Reactions
Displacement of Hydrogen in an Acid by a Metal
Mg(s) + HCl(aq) →
H2(g) + MgCl2(aq)
Mg(s) + 2HCl(aq) → H2(g) + MgCl2(aq)

21. Single-Displacement Reactions
Displacement of Halogens
Fluorine is the most-active halogen, so it can replace any of the other halogens in their compounds.
In Group 17 each element can replace any element below it, but not any element above it.
Cl2(g) + 2KBr(aq) → 2KCl(aq) + Br2(l)
F2(g) + 2NaCl(aq) → 2NaF(aq) + Cl2(g)
Br2(l) + KCl(aq) → no reaction

22. Double-Displacement Reactions
In double-displacement reactions, the ions of two compounds exchange places in an aqueous solution to form two new compounds.
AX + BY → AY + BX
One of the compounds formed is usually a precipitate, an insoluble gas that bubbles out of the solution, or a molecular compound, usually water.
The other compound is often soluble and remains dissolved in solution.

24. Double-Displacement Reactions
KI(aq) + Pb(NO3)2(aq) →
PbI2 + KNO3
2KI(aq) + Pb(NO3)2(aq) → PbI2(s) + 2KNO3(aq)
FeS(s) + HCl(aq) →
H2S + FeCl2
FeS(s) + 2HCl(aq) → H2S(g) + FeCl2(aq)
HCl(aq) + NaOH(aq) →
NaCl + H2O
HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)

25. Combustion Reactions 2H2(g) + O2(g) → 2H2O(g)
In a combustion reaction, a substance combines with oxygen, releasing a large amount of energy in the form of light and heat.
Combustion of hydrogen
2H2(g) + O2(g) → 2H2O(g)
Combustion of propane (hydrocarbon)
C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g)

26. Combustion Reactions