1. Chapter 11: Chemical Reactions
Types of
Chemical Reactions

2. Learning Targets
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.
You will determine the solubility of a substance.
You will determine the activity of a metal or halogen when predicting the products of a chemical reaction.

3. Synthesis (Combination) Reactions
Synthesis reactions are reactions in which two or more substances combine and form ONE more complex substance. They have the general form:
A + X  AX
A and X can be elements or compounds
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.

4. Examples of Synthesis Reactions
Fe + S  FeS
2 Na + Cl2  2 NaCl
4 K + O2  2 K2O
Notice the reactants are synthesized to yield ONE product.
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.

5. Write balanced chemical equations for the following:
Examples
Write balanced chemical equations for the following:
K (s) + Cl2 (g)  ? (s)
Solid aluminum reacted with chlorine gas to yield a solid product
2 K (s) + Cl2 (g)  2 KCl (s)
2 Al (s) + 3 Cl2 (g)  2 AlCl3 (s)
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.

6. Write balanced chemical equations for the following:
Try on your own
Write balanced chemical equations for the following:
Solid cesium reacted with liquid bromine to yield a solid product
Mg (s) + O2 (g)  ? (s)
2 Cs (s) + Br2 (l)  2 CsBr (s)
2 Mg (s) + O2 (g)  2 MgO (s)
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.

7. Decomposition Reactions
Decomposition reactions are the opposite of synthesis reactions. ONE substance breaks down and forms two or more simpler substances. They have the general form:
AX  A + X
A and X can be elements or compounds
EXCEPTION: ammonium carbonate, due to its nonmetallic nature, decomposes differently:
(NH4) 2CO3  2 NH3 (g) + H2O (g) + CO2 (g)
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.

8. Examples of Decomposition Reactions
PbO2 (s)  Pb (s) + O2 (g)
2 AlN (s)  2 Al (s) + N2 (g)
2 H2O (l)  2 H2 (g) + O2 (g)
Notice ONE substance on the reactant side and multiple substances on the product side. The reactants decompose to yield the products
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.

9. Decomposition Reactions
Write balanced equations for the following:
Solid potassium chlorate decomposes to solid potassium chloride and oxygen gas
Solid barium carbonate decomposes to solid barium oxide and gaseous carbon dioxide
NI3  ?
2 KClO3 (s)  2 KCl (s) + 3 O2 (g)
BaCO3 (s)  BaO (s) + CO2 (g)
2 NI3  N2 + 3 I2
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.

10. Let’s check in …
Write the formula for the binary compound that decomposes to the products H2 and Br2?
Complete and balance this decomposition reaction.
HI 
Write and balance the equation for the formation of magnesium nitride (Mg3N2) from its elements.
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.

11. How did you do?
Write the formula for the binary compound that decomposes to the products H2 and Br2?
HBr (g)
Complete and balance this decomposition reaction.
2 HI  H2 (g) + I2 (g)
Write and balance the equation for the formation of magnesium nitride (Mg3N2) from its elements. 3 Mg (s) + N2 (g)  Mg3N2 (s)
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.

12. Hydrocarbon + oxygen  carbon dioxide (g) + water (g)
Combustion Reactions
Combustion reactions are called oxidation reactions. Most organic and some inorganic compounds will burn in air. If they ignite readily, they are considered flammable. Under normal conditions involving the oxidation of a hydrocarbon, the products are gaseous carbon dioxide and water vapor.
Hydrocarbon + oxygen  carbon dioxide (g) + water (g)
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.

13. Examples of Combustion Reactions
CH4 (g) + 2 O2 (g)  CO2 (g) + 2 H2O (g)
C2H5OH (l) + 3 O2 (g)  2 CO2 (g) + 3H2O(g)
2 C6H14 (l) + 19 O2 (g)  12 CO2 (g) + 14H2O(g)
Notice the products are
ALWAYS CO2 (g) + H2O (g)
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.

14. Write balanced equations for the following reactions:
Combustion Reactions
Write balanced equations for the following reactions:
Butane (C4H10) gas burns in oxygen
C2H6 (l) + O2 (g) 
C2H6O (l) + O2 (g) 
2 C4H10 (g) + 13 O2 (g)  8 CO2 (g) + 10 H2O (g)
2 C2H6 (l) + 7 O2 (g)  4 CO2 (g) + 6 H2O (g)
C2H6O (l) + 3 O2 (g)  2 CO2 (g) + 3 H2O (g)
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.

15. Let’s check in …
Write a balanced equation for the complete combustion of each compound.
Formaldehyde (CH2O (g))
Heptane (C7H16 (l))
Benzene (C6H6 (l))
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.

16. How did you do? CH2O (g) + O2 (g)  CO2 (g) + H2O (g)
Formaldehyde (CH2O (g))
CH2O (g) + O2 (g)  CO2 (g) + H2O (g)
Heptane (C7H16 (l))
C7H16 (l) + 11 O2 (g) 
7 CO2 (g) + 8 H2O (g)
Benzene (C6H6 (l))
2 C6H6 (l) + 15 O2 (g) 
12 CO2 (g) + 6 H2O (g)
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.

17. Quiz
Identify the type of reaction, predict the products and write balanced chemical equations for the following:
HgO (s) 
Cs (s) + F2 (g) 
C3H8 (g) + O2 (g) 
Ga (s) + N2 (g) 
H2O (l) 
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.

18. Answers Decomposition - 2 HgO (s)  2 Hg + O2
Synthesis - 2 Cs (s) + F2 (g)  2 CsF
Combustion –
C3H8 (g) + 5 O2 (g)  3 CO2 (g) + 4 H2O (g)
Synthesis - 2 Ga (s) + N2 (g)  2 GaN
Decomposition - 2 H2O (l)  2 H2 + O2
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.

19. Single Replacement Reactions
Single replacement (single displacement) reactions are reactions in which one substance is replaced in its compound by another substance. The general form for single replacement reactions are:
A + BX  AX + B or
Y + BX  BY + X
The two similar ions switch
*Consult activity series
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.
You will determine the activity of a metal or halogen when predicting the products of a chemical reaction.

20. Examples of Single Replacement Reactions
Fe2O3 (s) + 2 Al (s)  Al2O3 (s) + 2 Fe (s)
2 HCl (aq) + Zn (s)  H2 (g) + ZnCl2 (aq)
Zn (s) + CuSO4 (aq)  ZnSO4 (aq) +Cu(s)
Notice the single element replaces the similar ion in the compound to produce a new element and new compound
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.
You will determine the activity of a metal or halogen when predicting the products of a chemical reaction.

21. Let’s try together …
Predict the products and write balanced equations for the following reactions:
Zn (always has 2+ charge) + H2SO4 
Cl2 + KBr 
Zn + H2SO4  ZnSO4 + H2
Cl2 + 2 KBr  Br2 + 2 KCl
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.
You will determine the activity of a metal or halogen when predicting the products of a chemical reaction.

22. Try on your own …
Predict the products and write balanced equations for the following reactions:
F2 + NaBr 
Zn + H3PO4 
F2 + 2 NaBr  Br2 + 2 NaF
3 Zn + 2 H3PO4  Zn3(PO4)2 + 3 H2
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.
You will determine the activity of a metal or halogen when predicting the products of a chemical reaction.

23. Let’s check in …
Complete the equations for these single-replacement reactions in aqueous solution. Balance each equation. Write “no reaction” if a reaction does not occur.
Fe (s) (iron has a +2 charge) + Pb(NO3)2 (aq) 
Cl2 (aq) + NaI (aq) 
Ca (s) + H2O (l) 
Zn (s) + H2SO4 (aq) 
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.
You will determine the activity of a metal or halogen when predicting the products of a chemical reaction.

24. How did you do? Fe(NO3)2 (aq) + Pb (s) 2 NaCl (aq) + I2 (aq)
Fe (s) + Pb(NO3)2 (aq) 
Fe(NO3)2 (aq) + Pb (s)
Cl2 (aq) + 2 NaI (aq) 
2 NaCl (aq) + I2 (aq)
Ca (s) + 2 H2O (l) 
Ca(OH)2 (aq) + H2 (g)
Zn (s) + H2SO4 (aq)  ZnSO4 + H2
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.
You will determine the activity of a metal or halogen when predicting the products of a chemical reaction.

25. Double Replacement Reactions
Ions in solutions combine and form a product. These reactions are also known as ionic reactions with the following form:
AX (aq) + BY (aq)  AY + BX
In order for a reaction to have occurred the reactants must be soluble and a product must be formed. The product may be a solid, gas or liquid. CONSULT SOLUBILITY CHART!
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.
You will determine the solubility of a substance.

26. Examples of Double Replacement Reactions
NaCl (aq) + AgNO3 (aq) NaNO3 (aq) + AgCl (s)
NaI (aq) + AgNO3 (aq)  NaNO3 (aq) + AgI (s)
BaCl2 (aq) + (NH4)2SO4 (aq) 2NH4Cl(aq) + BaSO4 (s)
Notice the like ions switch places to form new compounds.
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.
You will determine the solubility of a substance.

27. Double Replacement Reactions
Predict the products and write balanced equations for the following reactions
CuSO4 (aq) + Na2S (aq) 
LiOH (aq) + HCl (aq) 
AgNO3 (aq) + H2SO4 (aq) 
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.
You will determine the solubility of a substance.

28. Double Replacement Reactions
Predict the products and write balanced equations for the following reactions
CuSO4 (aq) + Na2S (aq)  CuS (s) + Na2SO4 (aq)
LiOH (aq) + HCl (aq)  LiCl (aq) + H2O (l)
2 AgNO3 (aq) + H2SO4 (aq)  Ag2SO4 (s) +2 HNO3 (aq)
Check the solubility of your products. Notice the similar ions switch to form new compounds.
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.
You will determine the solubility of a substance.

29. You will determine the solubility of a substance.
Let’s check in …
Write the products of these double-replacement reactions. Then balance each equation.
NaOH (aq) + Fe(NO3)3 (aq) 
Ba(NO3)2 (aq) + H3PO4 (aq) 
FeS (s) + HCl (aq)  (hydrogen sulfide gas (H2S) is formed.)
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.
You will determine the solubility of a substance.

30. You will determine the solubility of a substance.
How did you do?
3 NaOH (aq) + Fe(NO3)3 (aq) 
Fe(OH)3 (s) + 3 NaNO3 (aq)
3 Ba(NO3)2 (aq) + 2 H3PO4 (aq) 
Ba3(PO4)2 (s) + 6 HNO3 (aq)
FeS (s) + 2 HCl (aq) 
FeCl2 (s) + H2S (g)
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.
You will determine the solubility of a substance.

31. Quiz – identify, Predict, Write and Balance
Ag2O (s) 
Na (s) + N2 (g) 
Al (s) + H2SO4 (aq) 
Ba(NO3)2 (aq) + H2SO4 (aq) 
Al (s) + Br2 (l) 
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.
You will determine the solubility of a substance.
You will determine the activity of a metal or halogen when predicting the products of a chemical reaction.

32. You will determine the solubility of a substance.
Quiz Answers, 1-5
2 Ag2O (s)  4 Ag + O2
(decomposition)
6 Na (s) + N2 (g)  2 Na3N
(synthesis)
2 Al (s) + 3 H2SO4 (aq)  Al2(SO4)3 + 3 H2 (single replacement)
Ba(NO3)2 (aq) + H2SO4 (aq)  BaSO4 (s) + 2HNO3 (aq) (double replacement)
2 Al (s) + 3 Br2 (l)  2 AlBr3 (synthesis)
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.
You will determine the solubility of a substance.
You will determine the activity of a metal or halogen when predicting the products of a chemical reaction.

33. Quiz – identify, Predict, Write and Balance
CH4 (g) + O2 (g) 
H2SO4 (aq) + Ba(OH)2 (aq) 
Zn (s) + AgNO3 (aq) 
KBr (s) 
C2H2 (g) + O2 (g) 
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.
You will determine the solubility of a substance.
You will determine the activity of a metal or halogen when predicting the products of a chemical reaction.

34. You will determine the solubility of a substance.
Quiz Answers, 6-10
CH4 (g) + 2 O2 (g)  2 H2O (g) + CO2 (g)
(combustion)
H2SO4 (aq) + Ba(OH)2 (aq)  2H2O (l) + BaSO4 (s)
(double replacement)
Zn (s) + 2 AgNO3 (aq)  Zn(NO3)2 + 2 Ag
(single replacement)
2 KBr (s)  2 K + Br2
(decomposition)
2 C2H2 (g) + 5 O2 (g)  4 CO2 (g) + 2 H2O (g) (combustion)
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will predict the products of a chemical reaction when given the reactants and write a balanced chemical equation.
You will determine the solubility of a substance.
You will determine the activity of a metal or halogen when predicting the products of a chemical reaction.