Name: ___ANSWER KEY____________
Block: _____ Date: _________________
Honors Chemistry Unit 5 Test Review
Chemical Reactions
1. For the following reactions, write, balance, and/or classify the type of reaction. Include phase
states when indicated.
a. 2KOH(aq) + H2 SO 4(aq)  K 2 SO 4(aq) + H2 O (l) Acid/Base
b. 2SiO  2Si + O 2
Decomposition
c. Ca (s) + 2CuNO 3(aq)  Ca(NO 3 ) 2(aq) + 2Cu (s)
d. 4Al (s) + 3O 2(g)  2Al 2 O 3(s)
Single Replacement
Synthesis
e. Aqueous silver nitrite reacts with aqueous potassium bromide to yield aqueous potassium
nitrite and solid silver bromide.
AgNO 3(aq) + KBr (aq)  KNO 3(aq) + AgBr (s)
Double Replacement
f. Hydrofluoric acid reacts with aqueous copper (II) hydroxide to produce water and aqueous
copper (II) fluoride.
HF (aq) + Cu(OH) 2(aq)  H 2 O (l) + CuF 2(aq)
Acid/Base
g. Titanium (IV) bromide reacts with chlorine gas to produce titanium (IV) chloride and
bromine gas.
TiBr 4(aq) + Cl 2(g)  TiCl 4(aq) + Br 2(g)
Single Replacement
2. What are the coefficients for the following reaction?
6
3
2
3. What type of reaction:
a. Produces water and a salt?
Acid/Base
b. Breaks apart a substance into smaller substances?
c. Can produce a precipitate, gas, or liquid?
Decomposition
Double Replacement
d. Would you use the activity series to predict the products?
Single Replacement
e. Takes place in the presence of oxygen and produces carbon dioxide and water?
Combustion
f. Combines two or more substances to form a different substance?
g. Can net ionic equations be written from?
Synthesis
Double Replacement
4. Why do chemical equations need to be balanced?
Because of the Law of Conservation of Matter, chemical equations need to be balanced in order
to show all the elements involved in a chemical reaction.
5. Use any of the following elements or compounds to write and balance a combustion reaction.
C 5 H12 , Na, CO 2 , OH-, H+, K, Cl 2 , O 2 , C 4 H8
C 5 H 12 + 8O 2  5CO 2 + 6H 2 O
or
C 4 H 8 + 6O 2  4CO 2 + 4H 2 O
6. Use any of the following elements to write and balance a reaction that is an acid-base reaction.
Mg, Na, K, Al, OH-, H+, Br, Cl, I
HBr, Cl, or I + Mg, Na, K, or AlOH  Salt + H 2 O
One example: HCl + Mg(OH) 2  MgCl 2 + H 2 O
7. What are the four symbols for the different phase states and what do the each represent?
s – solid
aq – aqueous (dissolved solution)
l – liquid
g – gas
8. Find and correct the mistake in the equation Li 3 N + 3Cl  3LiCl + N.
Both Cl and N should be diatomic molecules: 2Li 3 N + 3Cl 2  6LiCl + N 2
9. Which metal will react spontaneously with HCl (aq) ? Au
Ag
Cu
Mg
10. Write a combination of two solutions that do NOT produce a reaction.
There are many different possibilities, just looking that all compounds are soluble. Here is one
possibility: NH 4 I (aq) + NaNO 3(aq)  NH 4 NO 3(aq) + NaI (aq)
11. Write the balanced molecular, complete ionic, and net ionic of the following equations, include
phase states:
a. Na 2 CO 3(aq) + Mg(OH) 2(aq)  2NaOH (aq) + MgCO 3(s)
Complete: 2Na+ (aq) + CO 3 2- (aq) + Mg2+ (aq) + 2OH- (aq)  2Na+ (aq) + 2OH- (aq) + MgCO 3(s)
Net Ionic: Mg2+ (aq) + CO 3 2- (aq)  MgCO3(s)
b. NaClO3(aq) + Ca3(PO4)2(aq)  Na3PO4(aq) + Ca(ClO3)2(s)
c. Hydrochloric acid reacts with sodium hydroxide
Molecular: HCl(aq) + NaOH(aq)  NaCl(aq) + H2O(l)
Complete: H+(aq) + Cl-(aq) + Na+(aq) + OH-(aq)  Na+(aq) + Cl-(aq) + H2O(l)
Net Ionic: H+(aq) + OH-(aq)  H2O(l)
d. Silver nitrate reacts with iron (II) phosphate
Molecular: 6AgNO3(aq) + Fe3(PO4)2(s)  2Ag3PO4(s) + 3Fe(NO3)2(aq)
Complete: 6Ag+(aq) + 6NO3-(aq) + Fe3(PO4)2(s)  2Ag3PO4(s) + 3Fe2+(aq) + 6NO3-(aq)
Net Ionic: 6Ag+(aq) + Fe3(PO4)2(s)  2Ag3PO4(s) + 3Fe2+(aq)
12. A reaction produces solid silver chloride. Write, balance, and draw a reaction that has two
aqueous reactants that will produce solid silver chloride and another product.
There are many different options for this answer, but here is one:
Molecular: 2AgNO3(aq) + MgCl2(aq)  Mg(NO3)2(aq) + 2AgCl(s)
Ag NO3
NO3- +
Ag
+
NO3Mg2+ NO3
2AgCl
Mg2+
ClCl
Complete: Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq) 
Na+(aq) + NO3-(aq) + AgCl(s)
Net Ionic: Ag+(aq) + Cl-(aq)  AgCl(s)
13. A reaction produces solid iron (II) carbonate. Write, balance and classify a reaction in which
aqueous iron (II) chloride reacts with another reactant to produce iron (II) carbonate and another
product.
There are many different options for this answer, but all should be double replacements. Here is
one option:
Molecular: FeCl2(aq) + Na2CO3(aq)  FeCO3(s) + 2NaCl(aq)
Complete: Fe3+(aq) + 2Cl-(aq) + 2Na+(aq) + CO32-(aq)  FeCO3(s) + 2Na+(aq) + 2Cl-(aq)
Net Ionic: Fe3+(aq) + CO32-(aq)  FeCO3(s)
14. Describe what a spectator ion is.
A spectator ion is an ion that does not participate in a reaction. It is present in both the
reactants and products.
15. Students preformed a lab to determine the reactivity of an unknown metal. Using the data below,
write out the activity series of the metals tested in the lab including the unknown metal. ((Do
yourself a favor and don’t look at an activity series except to check your answer)
Cu(NO3)2
Reaction
NR
Reaction
Reaction
Reaction
Reaction
X
Cu
Fe
K
Na
Zn
Fe(NO3)3
Reaction
NR
NR
Reaction
Reaction
Reaction
KNO3
NR
NR
NR
NR
NR
NR
NaNO3
NR
NR
NR
Reaction
NR
NR
Most reactive K, Na, Zn, X, Fe, Cu
Zn(NO3)2
NR
NR
NR
Reaction
Reaction
NR
Least Reactive
16. Predict the product, assign oxidation numbers, and identify the element that is oxidized and the
element that is reduced in the following equations:
a. Ba(s) + Mg(OH)2  Mg(s) + Ba(OH)2
0
+2 -2 +1
0
Oxidized – Ba
+2 -2 +1
Reduced – Mg
b. Iron (III) sulfide reacts with aluminum metal
Fe2S3 + Al(s)  Fe(s) + Al2S3
+3 -2
0
0
Oxidized – Al
+3 -2
Reduced – Fe
c. Calcium metal reacts with potassium oxide
Ca(s) + K2O  No Reaction
17. In which reaction are electrons transferred from one reactant to another reactant?
a. 2Ca(s) + O2(g)  2CaO(s)
0
0
b. AgNO3(aq) + KCl(aq)  AgCl(s) + KNO3(aq)
+2 -2
+1 +5 -2
b. HCl(aq) + NaOH(aq)  NaCl(aq) + H2O(l)
+1 -1
+1 -2 +1
+1 -1
+1 -2
+
c. H3O
+1 -2
(aq)
+
+1 -1
+1 -1
OH-(aq)
 2H2O(l)
-2 +1
+1 -2
+1 +5 -2