Review Sheet – Chemistry, Level 3 – Ch. 9: Chemical Reactions
Name: ____________________
Date:___________
Period:___
This test covers materials in the textbook in Chapters 9 (pp. 279-297). You are always responsible for the topics
on the previous tests.
. Test Expectations
The student should be able:
 Write balanced chemical equations starting from word equations, formula equations, or just reactants.
 Classify chemical reactions as one of the five common types of reactions.
1. Define each of the following terms clearly and completely.
(a) product –
(f) balanced chemical equation–
(b) reactant –
(g) word equation –
(c) coefficients –
(h) diatomic element –
(d) chemical reaction –
(i) conservation of mass –
(e) combustion –
(j) precipitation –
a)
b)
c)
d)
Product – A substance that is produced during a chemical change.
Reactant – A substance that is consumed during a chemical change.
Coefficients – A numerical prefix indicating the number of each reactant or product in a chemical equation.
Chemical Reaction – Change that takes place when two or more substances (reactants) interact to form new
substances (products).
e) Combustion – A chemical reaction between a fuel and an oxidizing agent that produces heat (and usually, light).
f) Balanced Chemical Equation – A description of a chemical reaction that gives the chemical formulas of the
reactants and the products of the reaction, with coefficients introduced so that the number of each type of
atom and the total charge is unchanged by the reaction.
g) Word Equation – An equation in which the reactants and products in a chemical reaction are represented by
words.
h) Diatomic Element – A molecule that contains only two atoms.
i) Conservation of Mass – The principle stating that matter is not created or destroyed during a chemical reaction.
j) Precipitation – Precipitation is the formation of a solid in a solution during a chemical reaction.
2. Balance each of the following chemical equations. Then write the name of the type of chemical reaction on
the line provided.
A. 2 O2 + N2 
N2O4
_____synthesis_________________
B. 2 NaF 
2 Na + F2
_____decomposition______________
C. 2 NaI + Pb(NO3)2  2 NaNO3 + PbI2
2 F2 
D. CS2 +
E. Li3PO4 
3 Li
F. C8H16 + 12 O2
G. 2 Al
+
CF4
+
+
P
2S
+
H. C6H12 + 9 O2
_____single replacement_________
2 O2
 8 CO2 + 8 H2O
3 FeO  Al2O3 +
______double replacement_____
3 Fe
 6 CO2 + 6 H2O
_____ decomposition _______
_____combustion_______________
______ single replacement ________
______ combustion _____________
3. Write the balanced chemical equation for the chemical reaction between water and calcium. The reaction
produces calcium hydroxide and hydrogen.
Ca + 2 H2O  Ca(OH)2 + H2
4. Bromine combines with nitrogen to produce gaseous nitrogen tribromide. Write the balanced chemical
equation for this reaction.
N2 + 3 Br2  2 NBr3
5. Write the balanced chemical equation for the direct combination (synthesis) reaction that occurs when
ammonia vapor and hydrogen sulfide gas react to produce solid ammonium sulfide ((NH4)2S).
2 NH3 + H2S  (NH4)2S
6. For the following reactions:
I.
Determine the type of reaction
II.
Complete the word equation
III.
Write correct formulas and balance the equations.
A. Mg + Cu(NO3)2
 Mg(NO3)2 + Cu
(single replacement)
B. BaBr2 + Na2CO3  BaCO3 + 2 NaBr (double replacement)
C. C6H8 + 8 O2  6 CO2 + 4 H2O
(combustion)
D. calcium chloride + gold (I) oxide  calcium oxide + gold (I) chloride
CaCl2 + Au2O  CaO + 2 AuCl
(double replacement)
E. potassium carbonate  carbon dioxide + potassium oxide
K2CO3  CO2 + K2O
(decomposition)
F. chlorine + potassium bromide  bromine + potassium chloride
Cl2 + 2 KBr  Br2 + 2 KCl
(single replacement)
G. iron (III) oxide + potassium carbonate  iron(III) carbonate + potassium oxide
Fe2O3 + 3 K2CO3  Fe2(CO3)3 + 3 K2O
(double replacement)
H. potassium + nitrogen  potassium nitride
6 K + N2  2 K3N (synthesis)
I. iron (III) hydroxide  water + iron (III) oxide
2 Fe(OH)3  3 H2O + Fe2O3
(decomposition)
J. gold + potassium chloride  No Rxn. (single replacement)
K. aluminum + silver nitrate  silver + aluminum nitrate
Al + 3 AgNO3  3 Ag + Al(NO3)3
(single replacement)
L. calcium hydroxide + nitric acid  water + calcium nitrate
Ca(OH)2 + 2 HNO3  2 H2O + Ca(NO3)2 (double replacement)