Honors Chemistry Final Exam Review
Fall
Here are some important points about your final exam:

You will be given
o a periodic table
o a common ion sheet
o solubility rules
o oxidation states rules
o If I forgot something, ask me if you will have it for the exam.

Because your final exam is all multiple choice questions, I believe completing this
review will help you to see what multiple choice chemistry questions are like.

I could not cover every type of problem we did over the semester on this review,
or the review would have been a lot longer. Therefore, look over your quizzes,
tests, and notes.

An answer key with worked out answers is on my website.
Material covered:
 Chapter 1
 Chapter 1
 Chapter 2
 Chapter 2
 Chapter 3
 Chapter 3
 Chapter 4
Answers:
1. A
2. B
3. D
4. B
5. D
6. A
7. D
8. D
9. C
10. D
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
Measurement and Chemical Math (not temp.)
Matter
Atomic Structure (not the periodic table intro.)
Nomenclature
The Mole
Reactions and Stoichiometry
Aqueous Solutions and Solution Stoichiometry
C
D
C
D
A
E
D
B
E
D
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
A
C
B
A
D
D
A
A
C
C
31.
32.
33.
34.
35.
36.
37.
38.
39.
40.
1
B
B
C
E
B
C
A
B
D
A
41. D
42. A
43. A
44. C
45. C
46. D
47. D
48. B
49. B
50. C
51.
52.
53.
54.
55.
56.
57.
B
D
A
D
D
C
C
Honors Chemistry Final Exam Review
Fall
Measurement and Matter
9. A student measures the temperature of
a sample three times. Her
measurements are given below.
1. Which formula represents a mixture?
a. NaCl(aq)
b. NaCl(s)
c. H2O(l)
d. H2O(s)
Trial #
1
2
Temp.
25C
48C
Average Temperature = 45C
3
62C
2. The SI unit for the measurement of mass
is the
a. ounce
b. kilogram
c. meter
d. liter
If the actual temperature of the sample is
45C, are her measurements
a. accurate and precise?
b. inaccurate and precise?
c. accurate and imprecise?
d. inaccurate and imprecise?
3. Which pure substance cannot be broken
down by a chemical change?
a. sodium chloride
b. ethanol
c. propane
d. calcium
10. Which set consists only of compounds?
a. Na, Ca, He
b. H2O, S, NaCl
c. NaCl, CH4, Na+
d. H2S, CuCl2, KI
11. A sample of metal has a mass of 27.24
g and a volume of 2.2 mL. What is the
correct value of its density using these
data?
a. 60. g/mL
b. 0.081 g/mL
c. 12 g/mL
d. 25 g/mL
e. 29 g/mL
4. Which quantity must be conserved in all
chemical reactions?
a. density
b. mass
c. volume
d. temperature
5. Which of the following is a chemical
change?
a. boiling water
b. crushing sodium chloride
c. ripping paper
d. burning a match
12. Write 4,251 in scientific notation.
a. 42.51 X 102
b. 4.251
c. 4.251 X 104
d. 4.251 X 103
6. Which of the following is a physical
property?
a. conductivity
b. burns in oxygen
c. produces a precipitate with NaCl
d. fails to react with hydrogen
Atomic Structure
13. Which substance contains only one kind
of atom?
a. water
b. glucose
c. aluminum
d. carbon dioxide
7. Which of the following is an extensive
property?
a. boiling point
b. malleability
c. density
d. mass
14. Every chlorine atom has
a. 7 electrons
b. 17 neutrons
c. a mass number of 35
d. 17 protons
8. Which statement describes a chemical
property of silicon?
a. Silicon has a blue-gray color.
b. Silicon is a brittle solid at 20C.
c. Silicon melts at 1414C.
d. Silicon reacts with fluorine.
2
Honors Chemistry Final Exam Review
Fall
15. What is the total number of electrons in
a Mg2+ ion?
a. 10
b. 2
c. 12
d. 24
21. What is the correct name of Pb(NO3)2?
a. lead(II) nitrate
b. lead(II) dinitrate
c. lead nitrate
d. lead dinitrate
22. The correct formula for ammonium
sulfate is
a. (NH4)2SO3
b. NH4SO3
c. (NH4)2SO4
d. NH4SO4
16. Which of the following conclusions can
be drawn from Rutherford’s gold foil
experiment?
a. the atom is mostly empty space
b. the atom is composed of a positive
cloud with electrons evenly
distributed throughout
c. there is a positive central nucleus
d. a and b
e. a and c
23. What is the correct formula for sulfur
hexafluoride?
a. SF4
b. SF6
c. S6F
d. S6F6
17. Which element of the following exists as
a monoatomic gas at room temperature
and standard pressure?
a. hydrogen
b. nitrogen
c. fluorine
d. neon
24. What is the formula for hydrosulfuric
acid?
a. H2S
b. H2SO4
c. H2SO3
18. A sample of element X contains 90.0%
X-35 atoms, 8.00% X-37 atoms, and
2.00% X-38 atoms. The average atomic
mass for X is
a. 36.2 amu
b. 35.2 amu
c. 68.7 amu
d. 37.0 amu
25. What is the correct name for HClO3?
a. hydrochloric acid
b. hydrochlorous acid
c. chlorous acid
d. chloric acid
The Mole
26. What is the molar mass of Al(OH)3?
a. 61.0 g/mol
b. 46.0 g/mol
c. 88.0 g/mol
d. 78.0 g/mol
19. The number of neutrons in an atom of
an element is
a. the same in each isotope
b. the same as the atomic number
c. equal to the number of electrons
d. equal to the number of protons
e. equal to the difference between the
mass number and the atomic number
27. Calculate the mass of 3.50 mol of SO2.
a. 224 g
b. 2.10 X 1024 g
c. 18.3 g
d. 0.0546 g
Nomenclature
28. How many atoms are in 73.2 g of Ag?
a. 4.08 X 1023 atoms
b. 4.08 atoms
c. 4.41 X 1025 atoms
d. 1.13 X 10-24 atoms
20. What is the correct name of CBr4?
a. carbon bromide
b. monocarbon tetrabromide
c. carbon quadribromide
d. carbon tetrabromide
3
Honors Chemistry Final Exam Review
Fall
29. A gas is 92.3% carbon and 7.7%
hydrogen by mass. What is its empirical
formula?
a. C12H
b. CH4
c. CH
d. C2H4
35. What are the correct products for the
reaction shown below?
AlCl3 + BaSO4 
a.
b.
c.
d.
30. If a compound has an empirical formula
of C2H2O and the compound’s molar
mass is 126.0 g/mol, what is the
molecular formula for this compound?
a. C2H2O
b. C4H4O2
c. C6H6O3
d. C2H2O2
36. Calculate the mass of carbon dioxide
produced from 11.2 g of octane reacting
with oxygen in the following reaction:
2 C8H18 + 25 O2  16 CO2 + 18 H2O
a.
b.
c.
d.
e.
31. What is the percent (by mass) of carbon
in C6H12O6?
a. 20.0%
b. 40.0%
c. 53.3%
d. 6.7%
58.9 g
17.3 g
34.6 g
89.6 g
46.2 g.
37. In a college chemistry lab, the reaction
between a given amount of CO and
Fe3O4 is calculated to have a theoretical
yield of 47.2 g Fe. When a student
carries out the reaction, the actual yield
is 39.9 g Fe. What is the percent yield?
a. 84.5%
b. 118%
c. 15.5%
d. 18%
Reactions and Stochiometry
32. When the following equation is
balanced correctly, what is the number
in front of the AgCl?
FeCl2 + Ag3PO4  Fe3(PO4)2 + AgCl
a.
b.
c.
d.
AlSO4 + BaCl
Al2(SO4)3 + BaCl2
Al2Ba3 + Cl2SO4
AlCl3 + BaSO4
12
6
2
4
38. In the reaction,
Zn + 2 HCl  ZnCl2 + H2,
25.0 grams of Zn are reacted with 17.5 g
of HCl. How many grams of H2 will be
produced?
33. What is the correct balanced equation
for the reaction between calcium and
oxygen to produce calcium oxide?
a. Ca + O  CaO
b. Ca + O2  CaO2
c. 2 Ca + O2  2 CaO
d. Ca2 + O2  2 CaO
a.
b.
c.
d.
0.38 g of H2
0.48 g H2
0.76 g H2
25 g H2
39. From question 38, how many grams of
what substance will be left over?
a. 0.285 g of HCl
b. 7.5 g of Zn
c. 15.7 g Zn
d. 9.3 g Zn
34. What is the classification of the reaction
shown below?
2 HgO  2 Hg + O2
a. single displacement
b. combustion
c. synthesis
d. double displacement
e. decomposition
4
Honors Chemistry Final Exam Review
Fall
Solution Stoichiometry
45. The following data were collected at the
endpoint of a titration performed to find
the molarity of an HCl solution.
40. Given the redox reaction:
2I-(aq) + Br2(l) → 2Br-(aq) + I2(s)
What occurs during this reaction?
Volume of acid (HCl) used = 14.4 mL
Volume of base (NaOH) used = 22.4 mL
Molarity of standard base (NaOH) = 0.20 M
a. The I- ion is oxidized, and its
oxidation number increases.
b. The I- ion is oxidized, and its
oxidation number decreases.
c. The I- ion is reduced, and its
oxidation number increases.
d. The I- ion is reduced, and its
oxidation number decreases.
What is the molarity of the acid solution?
a. 1.6 M
b. 0.64 M
c. 0.31M
d. 0.13M
46. A precipitate is expected to be formed
when an aqueous solution of sodium
sulfate is added to an aqueous solution
of :
41. What is the oxidation number of carbon
in NaHCO3?
a.
b.
c.
d.
+6
+2
-4
+4
a.
b.
c.
d.
42. What is the reducing agent in the
following reaction?
47. A strong electrolyte is one that
__________ completely in solution.
Cu(s) + 4H+(aq) + SO42+(aq)
 Cu2+(aq) + 2 H2O(l) + SO2(g)
a.
b.
c.
d.
a. Cu
b. H+
c. SO42d. Cu2+
e. SO2
HCl
NaCl
LiOH
KOH
44. When the following reaction is balanced
in an acidic solution, what is the
coefficient of water?
-
-
reacts
associates
disappears
ionizes
48. When aqueous solutions of iron(III)
chloride and sodium sulfide are mixed,
a precipitate forms. Write the net ionic
equation for this reaction.
a. Na+(aq) + Cl-(aq)  NaCl(s)
b. 2 Fe3+(aq) + 3 S2-(aq)  Fe2S3(s)
c. Fe3+(aq) + S2-(aq)  (Fe3)2S(s)
d. 2 FeCl3(aq) + 3 Na2S(aq)  Fe2S3(s) +
6 NaCl(aq)
e. 2 Fe(aq) + 3 S(aq)  Fe2S3(s)
43. Which substance can be classified as
an Arrhenius acid?
a.
b.
c.
d.
iron(III) chloride
potassium chloride
magnesium chloride
barium chloride
49. The concentration of iodide ions in a
0.193 M solution of barium iodide is
-
NO3 + I → IO3 + NO2
a. 1
b. 2
c. 3
d. 4
e. 5
a.
b.
c.
d.
e.
5
0.193 M
0.386 M
0.0965 M
0.579 M
0.0643 M
Honors Chemistry Final Exam Review
Fall
50. How many grams of solid NaCl must be
added to 25.0 mL of 0.366 M AgNO3
solution to completely precipitate the
silver ions?
54. Heating 2.68 g of a hydrate of sodium
sulfate drives off 1.26 g of water. What
is the formula of the hydrate?
a. Na2SO4•H2O
b. Na2SO4•2H2O
c. Na2SO4•4H2O
d. Na2SO4•7H2O
a. 9.15 X 10-3 g
b. 1.57 × 10-4 g
c. 0.535 g
d. 0.157 g
e. 6.39 × 103 g
55. The purpose of filtration is to
a. form precipitates
b. remove water from solutions.
c. separate dissolved ions from the
solvent.
d. separate precipitates from a solution.
51. The following equation describes the
oxidation of ethanol to acetic acid by
potassium permanganate:
56. Which of the following is a beaker?
3 C2H5OH + 4 KMnO4 →
a.
3 CH3COOH + 4 MnO2 + 4 KOH + H2O
b.
If 5.00 g of ethanol (C2H5OH) are
reacted with an excess of aqueous
KMnO4, and 5.94 g of acetic acid
(CH3COOH) are produced, what is the
percent yield?
a.
b.
c.
d.
e.
c.
100. %
91.1 %
30.4 %
8.86%
74.9 %
52. Consider the reaction between 15.0 mL
of 1.00 M AgNO3 and 10.0 mL of 1.00 M
K2CrO4. When these react, a precipitate
is formed. Which ions/molecules are
present in the solution after the reaction
is complete? Note: The precipitate is
not considered to be in the solution.
a.
b.
c.
d.
e.
Fall 2016 – Do Not Do #57
57. The graph below represents data from a
Boyle’s Law experiment.
Ag+, NO3-, K+, CrO42-, H2O
Ag+, NO3-, K+, H2O
K+, CrO42-, H2O
NO3-, K+, CrO42-, H2O
H2O
Laboratory Skills
53. Which of the following would you use to
measure the volume of a liquid?
a. graduated cylinder
b. beaker
c. Erlenmeyer flask
d. balance
The best title for the graph above would be
a. Boyle’s Law Experiment Data
b. Volume vs. Pressure
c. Pressure vs. Volume
6