Name_____________________________ Date_________________________
Period_________________
Chemistry-Exam 2 Review
Select the best answer choice for each question.
1. Which of these elements has the highest electronegativity?
a. Potassium (K)
b. Calcium (Ca)
c. Bromine (Br)
d. Krypton (Kr)
2. Which pair of elements will form ionic bonds in a ratio of 2:1?
A.
B.
C.
D.
calcium (Ca) and sulfur (S)
sulfur (S) and chlorine (Cl)
potassium (K) and sulfur (S)
potassium (K) and chlorine (Cl)
3. The white pigment in many paints is titanium dioxide (TiO2). It is made by burning titanium (IV) chloride. The
other product in this reaction is chlorine gas. What is the balanced equation for this reaction?
A.
B.
C.
D.
4. What is the empirical formula for a compound that contains 17.34% hydrogen and 82.66% carbon?
A. C5H
B. C2H5
C. CH3
D. CH2
5. Evan is comparing Carbon-12 and Carbon-14 atoms. Which statement correctly compares the subatomic particles
in the carbon atoms?
a. The carbon-14 atom has the same number of electrons, protons, and neutrons as the carobon-12 but more
mass.
b. The carbon-14 atom has two more electrons than the carbon-12 atom, but they have the same number of
protons and neutrons.
c. The carbon-14 atom has two more electrons and two more protons than the carbon-12 atom, but they have the
same number of neutrons.
d. The carbon-14 atom has two more neutrons than the carbon-12 atom, but they have the same number of
electrons and protons.
6. Mr. Noto wants to confirm the metal used in a ring. The volume of the ring is 1.35 cubic
centimeters (cm3). What is the metal composition of the
ring?
A.
B.
C.
D.
Sterling silver
18ct white gold
Pure gold
Platinum
Name________________________________Date_______________________
Period_______________
7. What is the Lewis dot structure for nitrogen trifluoride (NF3) ?
A.
C.
B.
D.
8. What physical property is used in distillation to separate the components?
a.
b.
c.
d.
melting point
boiling point
chemical energy
ignition temperature
9. What is the formula for Iron (III) Oxide?
A. Fe3O2
B. I3O2
C. Fe2O3
D. FeO3
10. Which of the following substances is less dense than air?
A. Water
B. Helium
C. Ice
D. Gold
11. According to the law of conservation of matter, what happens to the atoms in a chemical reaction
A. The atoms are rearranged with no loss in mass.
B. Some atoms are destroyed, resulting in mass being converted to energy.
C. There is a small gain in mass as new atomic bonds are formed.
D. The atoms remain unchanged with no change in mass.
12. The half-life of a radioisotope is the amount of time it takes for
a.
b.
c.
d.
half the sample to decay
all the sample to decay
the age of an artifact to be calculated
detectable radiation to be absorbed by a sample
Name________________________________Date_______________________
13. Use the table to answer the question.
Period_______________
The table above provides some information about an unidentified element. Based
on this information, the unidentified element is best classified as which of the
following?
A.
B.
C.
D.
a metal in group 1 (1A)
a metal in group 14 (4A)
a nonmetal in period 4
a metalloid in period 5
14. Which Lewis dot structure accurately represents a formula unit of magnesium chloride (MgCl 2)?
A.
C.
B.
D.
15. In the name carbon dioxide, the prefix of the second word indicates that a molecule of carbon dioxide contains
a. two carbon atoms
b. two oxygen atoms
c. a polyatomic ion
d. an ionic bond
16. Use the table to answer the question.
The table shows the procedures for and the results of two experiments using
copper (II) chloride, CuCl2. Which of the following conclusions can be made
based on the results of the experiments?
A. Physical changes occurred in both experiments.
B. A chemical change occurred in experiment 1, and a physical change
occurred in experiment
C. A physical change occurred in experiment 1, and a chemical change
occurred in experiment 2
D. Chemical changes occurred in both experiments.
17. Use the table to answer the question.
The table shows the electronegativities of four elements. Which of the following
bonds is the most polar?
A. carbon-hydrogen
B. hydrogen-oxygen
C. fluorine-fluorine
D. carbon-fluorine
18. A student determined that the density of a sample of tin is 8.00 g/mL, when the actual density of tin is 7.28 g/mL.
What was the percent error in the student’s calculation?
A.
B.
C.
D.
0.72%
9.0%
9.9%
91%
Name________________________________Date_______________________
19. Use the diagram to answer the question.
The diagram above shows two targets that have been struck by 4 darts each.
Select the statement below which is correct.
Period_______________
A. Target A has been hit with a high degree of precision, yet a low
degree of accuracy.
B. Target B has been hit with a high degree of precision, yet a low
degree of accuracy.
C. Target A has been hit with a high degree of accuracy, yet a low
Target A
degree of precision.
D. Target B has been hit with a high degree of accuracy, and a high degree of precision.
Target B
20. Four lab groups measured the pH of juice from a watermelon.
Their results are shown in the table. The actual pH of the
watermelon juice is 5.27. Which group had the greatest precision
in their measurements?
a. Group 1
b. Group 2
c. Group 3
d. Group 4
21. Alkali metals, alkaline earth metals, and aluminum all form ions with positive charges equal to
a.
b.
c.
d.
atomic number
group number
period
atomic mass
22. Use the diagram to answer the question.
The diagram shows a partial periodic table. The electron configuration of
oxygen is 1s22s22p4. On the periodic table, fluorine is one space to the right of
oxygen. Which of the following electron configurations represents fluorine?
A.
B.
C.
D.
1s22s22p3
1s22s22p5
1s22s22p63s23p3
1s22s22p63s23p5
23. Which of the following atoms has the largest atomic radius?
a. Barium (Ba)
b. Chlorine (Cl)
c. Iodine (I)
d. Magnesium (Mg)
24. Zinc carbonate is an odorless, white, sand-like solid. It is used in cosmetics, lotions, porcelains, pottery, and
rubber. What is the chemical formula for zinc carbonate?
A. ZnCO3
B. Zn (CO3)2
C. Zn2CO3
D. Zn3CO2
Name________________________________Date_______________________
25. Which of the following atoms has six valence electrons?
a. Magnesium (Mg)
c. Sulfur (S)
b. Silicon (Si)
d. Argon (Ar)
Period_______________
26. What is the correct name for the acid whose chemical formula is H2SO4?
A. hydrosulfuric acid
B. hydrosulfurous acid
C. sulfurous acid
D. sulfuric acid
27. Uranium Hexafluoride is used to extract uranium-235 (U-235) from uranium to make the fuel for nuclear reactors
and to make nuclear bombs. What is the chemical formula of uranium hexafluoride?
A. UF
C. UF6
B. UHF
D. U2H6
28. Carbon tetrachloride was once commonly used as a solvent for dry cleaning and in fire extinguishers before more
environmentally friendly compounds were developed. What is the chemical formula for carbon tetrachloride?
A. CCl
C. C4Cl
B. CTeCl
D. CCl4
29. The name iron (II) indicates that a compound contains
a.
b.
c.
d.
iron ions with an 11+ charge
iron ions with a 2+ charge
iron ions with a negative charge
two types of iron ions
30. What is the name of the compound with the formula PCl5?
A. phosphorus (I) chloride
B. phosphorus (V) chlorine
31. What is the formula for the hydronitric acid?
A. HNO3
B. HNO2
C. phosphorus pentachlorate
D. phosphorus pentachloride
C. H3N
D. HN3
32. What group in the periodic table has a tendency to form ions with a +2 charge?
A. Group 1 – alkali metals
B. Group 2 – alkaline earth metals
C. Group 17 - halogens
D. Group 18 – noble gases
33. Which statement explains why a molecule of CH4 is nonpolar?
A.
B.
C.
D.
The bonds between the atoms in a CH4 molecule are polar.
The bonds between the atoms in a CH4 molecule are ionic.
The geometric shape of a CH4 molecule distributes the charges symmetrically.
The geometric shape of a CH4 molecule distributes the charges asymmetrically.
34. A student found that the empirical formula of an unknown compound is CH2O and that its molar mass is 210
grams per mole. What is the molecular formula of the compound?
A. C5H10O5
B. C6H12O6
C. C7H14O7
D. C8H16O8
Name________________________________Date_______________________
35. In the compound MgCl2, the subscript 2 indicates that
a.
b.
c.
d.
Period_______________
there are two magnesium ions for each ion of chlorine
the chlorine ion is twice the size of the magnesium ion
magnesium and chlorine form a double covalent bond
there are two chlorine ions for each magnesium ion
36. A compound is 40.0% carbon, 53.3% oxygen, and 6.66% hydrogen. What is its empirical formula?
A. C4H5H7
C. COH2
B. CO2H3
D. None of these is the correct empirical
formula
37. A compound contains 6.0 g of carbon and 1.0 g of hydrogen. The percent composition of the compound is
A. 14% hydrogen and 86% carbon
C. 17% hydrogen and 83% carbon
B. 86% hydrogen and 14% carbon
D. 83% hydrogen and 17% carbon
38. What is the total number of atoms contained in 2.00 moles of nickel?
A. 58.9
C. 6.02 x 1023
B. 118
D. 1.2 x 1024
39. The formation of an ionic bond involves the
a. transfer of electrons
b. transfer of neutrons
c. transfer of protons
d. sharing of electrons
40. Use the Lewis dot structures to answer the question.
What charge will the gallium atoms have if they react with the oxygen atoms to form ionic bonds?
C. +2
A. -3
D. +3
B. +1
41. What is the name of the compound with the chemical formula CrCl3?
A. chromium tetrachloride
B. chromium trichloride
C. chromium (II) chloride
D. chromium (III) chloride
42. Chlorine forms a 1- ion, but sulfur forms a 2- ion. What is the main reason for this difference in these two
atoms?
A. Chlorine and sulfur are part of two different periods of the periodic table, and these periods will form ions
with different charges.
B. Chlorine and sulfur are part of two different groups of the periodic table, and these groups will form ions with
different charges.
C. Chlorine is part of the oxygen group that only needs one more electron to reach a stable electron
configuration.
D. Sulfur is part of the halogen group that only needs two more electrons to reach a stable electron configuration.
Name________________________________Date_______________________
43. N2S3 is properly named:
A. Nitrogen sulfide
B. Nitrogen (III) sulfide
C. Nitrogen (II) sulfide
D. None of these
Period_______________
44. Which of the following atoms has the largest ionization energy?
a. Barium (Ba)
b. Chlorine (Cl)
c. Iodine (I)
d. Magnesium (Mg)
45. Which of the following elements would form a cation?
a. Bromine (Br)
b. Helium (He)
c. Lithium (Li)
d. Sulfur (S)
46. What is the mass in grams of 2.50 moles K2CO3?
A. 345 g
B. 265 g
C. 247.5 g
D. 167.5 g
47. Some students are modeling covalent bonds with brief descriptions and Lewis dot diagrams, using arrows to
show electron movement. Which model best demonstrates covalent bonding in bromine chloride (BrCl)?
a.
c.
b.
d.
48. Lacey uses R, T, X, and Z to represent four different unknown elements in the periodic table. The dots represent
valence electrons. Which unknown element will most likely form an ionic bond with Fluorine?
a.
b.
c.
d.
49. Sulfur would have chemical properties most like
a. Manganese
b. Tellurium
c. Chlorine
d. Xenon
50. Which of the following elements is a metal?
a. Bromine (Br)
b. Helium (He)
c. Lithium (Li)
d. Sulfur (S)
51. Which numbered bond in the diagram
represents an ionic bond?
a. Bond 1
b. Bond 2
c. Bond 3
d. Bond 4
Name________________________________Date_______________________
Period_______________
52. Which of the following correctly shows how carbon and hydrogen bond to form a compound?
A
.
C.
B.
D.
53. Which of the following has the strongest intermolecular force?
A.
B.
C.
D.
hexane with London Dispersion Force
ethanol with one H-bond
methane with London Dispersion Force
ammonia with Dipole-Dipole
54. What is the molar mass of (NH4)3PO4?
A. 113 g
B. 121 g
C. 149 g
D. 404 g
55. Which of the following statements describes a difference between a mixture and a pure substance?
A. A mixture tends to be homogeneous, while a pure substance tends to heterogeneous.
B. A mixture has a specific melting point, while the melting point of a pure substance can vary.
C. The density of a mixture can change with temperature, but the density of a pure substance cannot change.
D. The composition of a mixture can vary from sample to sample, but the composition of a pure substance is
always the same.
56. What is the correct formula for Calcium Carbonate?
A. Ca2(CO3)2
B. CaCO3
C. Ca2CO3
D. Ca2CO5
57. What is the formula for carbonic acid?
A. CO32B. H4C
C. H2CO3
D. HCO3
58. A 2 cm-thick piece of cardboard placed over a radiation source would be most effective in protecting against
which type of radiation?
A. alpha
B. beta
C. gamma
D. x-ray
59. In which of the following sets is the symbol of the element, the number of protons, and the number of electrons
given correctly?
a. In, 49 protons, 49 electrons
c. Cs, 55 protons, 132.9 electrons
b. Zn, 30 protons, 60 electrons
d. F, 19 protons, 19 electrons
60. Which compound is made up of nonpolar molecules?
a. HBr
c. NH3
b. H2S
d. CH4
_________This is the end of the regular Multiple Choice Section, below begins the Reading Section_______
Name_____________________________ Date_________________________
Period_________________
A student performed 2 studies to investigate the factors that affect the germination of peony seeds.
Study 1: Peony seeds were placed in dry containers. Some of the containers were stored at 5°C for either 4, 6, 8, or
10 weeks. The temperature and time periods were defined as the storage temperature and the storage period, respectively.
The peony seeds were divided evenly so that there were 20 sets of 25 seeds. Twenty petri dishes were then prepared.
Each contained damp paper. Each set of seeds was placed in a separate petri dish. Each petri dish was maintained at 1 of
4 temperatures for 30 days. The temperature and time periods were defined as the germination temperature and
the germination period, respectively. Table 1 shows the number of seeds that germinated in each dish.
Storage
period
(weeks)
0
4
6
8
10
Number of peony seeds that germinated when
maintained at a germination temperature of:
13°C
18°C
23°C
28°C
0
0
3
7
15
0
2
8
22
24
0
0
6
18
21
0
0
0
0
1
Study 2: Peony seeds were placed in dry containers. The containers were stored at various temperatures for 10 weeks.
The peony seeds were divided evenly so that there were 20 sets of 25 seeds. Twenty petri dishes were then prepared.
Each contained damp paper. Each set of seeds was placed in a petri dish. The petri dishes were maintained at 1 of
4 temperatures for 30 days. Table 2 shows the number of seeds that germinated in each dish.
Storage
temperature
(°C)
0
5
10
15
20
Number of peony seeds that germinated when
maintained at a germination temperature of:
13°C
18°C
23°C
28°C
15
16
0
0
0
24
23
6
0
0
21
21
4
0
0
1
1
0
0
0
Name_____________________________ Date_________________________
Period_________________
61. In general, the results of Study 1 suggest that peony seeds that are placed in a petri dish containing damp paper
are most likely to germinate when they are maintained at which of the following temperatures?
A. 13°C
B. 18°C
C. 23°C
D. 28°C
62. Suppose another set of 25 peony seeds had been included in Study 2 and these seeds had a storage temperature of
25°C and a germination temperature of 18°C. Based on the information provided, the number of seeds that would
have germinated after being maintained for 30 days would most likely have been closest to:
A. 0.
B. 8.
C. 16.
D. 24.
63. In Study 2, at the storage temperature of 5°C, as germination temperature increased from 13°C to 28°C, the
number of seeds that germinated:
A. decreased only.
B. increased only.
C. decreased, then increased.
D. increased, then decreased.
64. Which of the following sets of seeds were exposed to the same conditions prior to being placed in the petri
dishes?
A.
B.
C.
D.
The seeds from Study 1 that were stored for 8 weeks and the seeds from Study 2 that were stored at 5°C
The seeds from Study 1 that were stored for 8 weeks and the seeds from Study 2 that were stored at 15°C
The seeds from Study 1 that were stored for 10 weeks and the seeds from Study 2 that were stored at 5°C
The seeds from Study 1 that were stored for 10 weeks and the seeds from Study 2 that were stored at 15°C
65. A student stored 100 peony seeds at a constant temperature for 10 weeks. The student then divided the seeds into
4 sets and maintained them as described in Study 2. The results were as follows:
Germination
temperature (°C)
Number of seeds
that germinated
13
18
23
28
1
6
3
0
These seeds most likely had a storage temperature of:
A. 0°C.
B. 5°C.
C. 10°C.
D. 15°C.
66. The experimental designs of Study 2 and Study 1 differed in that in Study 2:
A. storage temperature was held constant.
B. storage time was held constant.
C. germination temperature was varied.
D. germination time was varied.