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Chapter 6: Chemical Reactions – Study Guide
*Do not forget about the extra resources available to help you study and prepare for this test!
 Textbook pages 233 – 247
 Mastering Chemistry Study Area: http://www.pearsonmylabandmastering.com/northamerica/
 Miss Marnik’s Website: http://www.northallegheny.org/Page/16665
 Labs, problem packets, and homework assignments
Overall Review:
1. Match the following terms with the phrases below:
a. Reaction that occurs in a liquid and forms a gas
1. acid-base reaction
b. Reaction in which electrons are transferred from one
substance to another
2. activity series
c. A list of elements that compare reactivities
3. balanced equation
d. Reactions that form one or more solid substances in water
4. combustion reaction
e. Chemical equation with coefficients such that the number of
each type of atom is equal on both sides
5. complete ionic equation
f.
Solution that contains a complete dissolved ionic compound
g. Empirical rules that look at the ability of many compounds to
dissolve in water
6. decomposition reaction
7. double displacement reaction
8. gas producing reaction
h. A reaction in which something reacts with elemental oxygen,
often producing CO2 and H2O
9. net ionic equation
i.
Chemical equation showing all of the species as they are
actually present in the solution
10. redox reaction
j.
Equation showing only the species that actually change during
the reaction
k. Reaction between two solutions that forms water and a salt
l.
Reaction in which simpler substances combine to form a more
complex substance
m. Reaction in which a more complex substance breaks down to
form two or more simpler substances
11. precipitation reaction
12. single displacement reaction
13. solubility rules
14. strong electrolyte solution
15. synthesis reaction
n. Reaction in which one element displaces another in a
compound
o. Reaction in which two elements or groups of elements in two
different compounds exchange places to form two new
compounds
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Section 1 – Reaction and Equations: (text pages 205-214)
Need to be able to:
 Identify a chemical reaction.
 Write balanced chemical equations.
Practice Problems:
2. What are four observations you can make to determine if a chemical reaction is taking place?
3. For each statement, write “yes” if evidence of a chemical reaction is present. Write “no” if there is no
evidence of a chemical reaction.
a) __________A tomato smells rotten.
b) __________A drinking glass breaks into smaller pieces.
c) __________A piece of ice melts.
d) __________Drain cleaner is mixed with water and the solution becomes warm.
e) __________Candle wax burns.
f)
__________Molten candle wax solidifies.
g) __________Green leaves turn yellow and red as the seasons change.
h) __________Baking powder produces a gas that makes a cake rise.
4. Balance each of the following chemical equations:
a.
Na2S(aq) +
Cu(NO3)2(aq) 
NaNO3(aq) +
b.
HCl(aq) +
O2(g) 
c.
BaO2(s) +
H2SO4(aq) 
d.
Li2O(s) +
e.
Co(NO3)3(aq) +
H2O(l) 
H2O(l) +
CuS(s)
Cl2(g)
BaSO4(s) +
H2O2(aq)
LiOH(aq)
(NH4)2S(aq) 
Co2S3(s) +
NH4NO3(aq)
5. For each of the following chemical reactions, write a balanced chemical equation. Be sure to show the
state of each reactant and product. Classify each reaction in as many ways as possible.
a. Solid lead (II) sulfide reacts with aqueous hydrochloric acid to form solid lead (II) chloride and
dihydrogen sulfide gas.
b. Solid iron (III) oxide reacts with hydrogen gas to form solid iron and liquid water.
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c. Solid calcium reacts with aqueous nitric acid to form aqueous calcium nitrate and hydrogen
gas.
Section 2 – Classifying Reactions: (text pages 228-232)
Need to be able to:
 Classify chemical reactions.
Practice Problems
6. Assume that Q, T, X, and Z are symbols for elements. Match each equation in Column A with the
reaction type it represents in Column B.
Column A
Column B
____ Q  XZ  X  QZ
a. decomposition
____ Q  Z  QZ
b. double-displacement
____ QT  Q  T
c. single-displacement
____ QT  XZ  QZ  XT
d. synthesis
7. Classify each chemical reaction as synthesis, decomposition, single displacement, or double
displacement.
a. K2S(aq) + Co(NO3)2(aq)  2KNO3(aq) + CoS(s)
b. 3H2(g) + N2(g)  2NH3(g)
c. Zn(s) + CoCl2(aq)  ZnCl2(aq) + Co(s)
d. CH3Br(g)  CH3(g) + Br(g)
e. 2Na(s) + O2(g)  Na2O2(s)
Section 3 – Single Displacement Reactions:
Need to be able to:
 Identify and predict single displacement reactions.
Practice Problems:
8. Examine each of the following pairs of potential reactants. If a reaction occurs, write the balanced
equation. If no reaction occurs, write NR.
a. Ca and H2O
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b. Rb and LiCl(aq)
c. K and Al2O3(aq)
d. silver and aqueous calcium nitrate
e. fluorine and aqueous potassium iodide
f.
aqueous magnesium bromide and chlorine
g. copper and aqueous iron (III) sulfate
Section 4 – Aqueous Solutions: (text pages 214-217)
Need to be able to:
 Determine if a compound is soluble.
Practice Problems:
9. Is each compound soluble or insoluble? For the soluble compounds, identify the ions present in
solution.
a. NaC2H3O2
e. (NH4)2S
b. Sn(NO3)2
f.
c. AgI
g. ZnS
d. Na3PO4
h. Pb(C2H3O2)2
CuCO3
Section 5 – Precipitation Reactions: (text pages 218-223)
Need to be able to:
 Predict and write equations for precipitation reactions.
 Write molecular, complete ionic, and net ionic equations.
Practice Problems:
10. Complete and balance each equation. If no reaction occurs, write NO REACTION.
a.
KI(aq) +
b.
K2SO4(aq) +
c.
NaCl(aq) +
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BaS(aq) 
BaBr2(aq) 
Hg2(C2H3O2)2(aq) 
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d.
NaC2H3O2(aq) +
Pb(NO3)2(aq) 
11. Write a molecular equation for the precipitation reaction that occurs (if any) when each pair of
solutions is mixed. If no reaction occurs, write NO REACTION.
a. sodium carbonate and lead (II) nitrate
b. potassium sulfate and lead (II) acetate
c. copper (II) nitrate and barium sulfide
d. calcium nitrate and sodium iodide
12. Write balanced complete ionic and net ionic equations for each of the following reactions.
a.
AgNO3(aq) +
b.
HI(aq) +
KCl(aq) 
KOH(aq) 
AgCl(s) +
H2O(l) +
KNO3(aq)
KI(aq)
c. Acetic acid reacts with a solution sodium carbonate to produce water, carbon dioxide gas, and
a solution of sodium acetate.
Section 6 – Acid-Base Reactions: (text pages 223-224)
Need to be able to:
 Identify and write equations for acid-base reactions.
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Practice Problems:
13. How can you identify if a substance is an acid or a base?
14. Complete and balance each equation.
Ba(OH)2(aq) 
a.
HCl(aq) +
b.
H2SO4(aq) +
KOH(aq) 
c.
NaOH(aq) +
HC2H3O2(aq) 
15. Write a molecular equation for each acid-base reaction.
a. Perchloric acid and aqueous sodium hydroxide
b. Sulfuric acid and aqueous barium hydroxide
Section 7 – Gas Producing Reactions: (text pages 224-226)
Need to be able to:
 Identify and write equations for gas producing reactions.
Practice Problems:
16. What are the five gases that are commonly produced during gas producing reactions?
17. Which compounds will typically decompose into gases once they are formed in solution?
18. Complete and balance each equation.
a.
HBr(aq) +
b.
NH4I(aq) +
c.
HNO3(aq) +
d.
HI(aq) +
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NaHCO3(aq) 
KOH(aq) 
K2SO3(aq) 
Li2S(aq) 
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19. Write a molecular equation for each gas producing reaction.
c. Perchloric acid and aqueous potassium carbonate
d. Acetic acid and aqueous lithium bisulfite
Section 8 – Oxidation-Reduction Reactions: (text pages 226-228)
Need to be able to:
 Identify redox reactions.
 Identify and write equations for combustion reactions.
Practice Problems:
20. How can a redox reaction be identified?
21. Which types of reactions are always considered to be redox reactions?
22. Which of the following reactions are redox reactions? For the ones you identify as redox, show how
the electrons are transferred between reactants.
a. Al(s) + 3Ag+(aq)  Al3+(aq) + 3Ag(s)
b. 4K(s) + O2(g)  2K2O(s)
c. HCl(aq) + NaOH(aq)  H2O(l) + NaCl(aq)
d. Mg(s) + Br2(l)  MgBr2(s)
23. Complete and balance combustion reaction.
O2(g) 
a.
C2H6(g) +
b.
Ca(s) +
c.
C3H8O(l) +
d.
S(s) +
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O2(g) 
O2(g) 
O2(g) 
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Overall Review:
Predict the products for each reaction and balance the equation, if it takes place. Classify each reaction
(if it takes place) in as many ways as possible.
KOH(aq)  _________________________________________________
24.
HBr(aq) +
25.
CsOH(aq) +
26.
Ca(s) +
27.
Ba(NO3)2(aq) +
28.
NH4Cl(aq) +
29.
KOH(aq) +
30.
C2H2(g) +
H2SO4(aq)  ______________________________________________
H2O(l)  _________________________________________________________
NaCl(aq)  ______________________________________________
Pb(NO3)2(aq)  ___________________________________________
HCl(aq)  ________________________________________________
O2(g)  _______________________________________________________
31. A solution of sodium iodide reacts with a solution of lead (II) acetate.
32. A solution of sodium sulfide is mixed with a solution of copper (II) nitrate.
33. Solid zinc is mixed with a solution of nickel (II) bromide.
34. Nitric acid reacts with a solution of sodium carbonate.
35. Phosphoric acid and a solution of lithium hydroxide react.