FINAL EXAM PRACTICE TEST
Multiple Choice
Identify the choice that best completes the statement or answers the question.
1. Na, K, Li, and Cs all share similar chemical properties. In the periodic table of elements, they most likely belong
to the same
a) row.
*c) group.
b) period.
d) element.
2. Which of the following substances is a mixture?
a) baking soda
c) salt
*b) gasoline
d) sugar
3. Which is the state of matter that has an indefinite shape and indefinite volume?
a) solid
*c) gas
b) liquid
*d) plasma
4. Which one is comprised of the other three?
a) proton
*b) atom
c) electron
d) neutron
5. Which has a charge of +1?
*a) proton
b) atom
c) electron
d) neutron
6. Which one(s) have a mass of 1 amu?
a) electron
b) proton
*c) proton and neutron
d) electron and proton
Atom
1
2
3
4
Protons
8
10
9
8
Atoms
Neutrons
10
9
9
11
Electrons
8
10
9
8
7. Which two are isotopes of one another?
a) Atoms 1 & 2
b) Atoms 2 & 3
c) Atoms 1 & 3
*d) Atoms 1 & 4
8. Which is the smallest part of an element that retains all the properties of the element?
a) proton
c) electron
b) neutron
*d) atom
Atom
Sodium
Chlorine
Protons
17
Atoms
Neutrons
12
Electrons
17
Mass Number
23
35
9. How many neutrons are in an atom of chlorine?
a) 17
c) 34
*b) 18
d) 35
10. How many electrons are in an neutral atom of sodium?
a) 22
c) 12
*b) 11
d) 23
11. Which element has 14 protons?
a) Nitrogen
*b) Silicon
c) Aluminum
d) Sulfur
12. According to the modern concept of the atom, which are located in the nucleus of an atom?
a) electrons and protons
c) neutrons and electrons
b) protons only
*d) protons and neutrons
13. Which is the correct number of valence electrons in the element Gallium (Ga)?
a) 13
c) 1
b) 31
*d) 3
14. Which is the correct number of valence electrons in the element Sulfur (S)?
a) 16
c) 2
*b) 6
d) 4
15. Which element has the electron configuration 1s22s22p63s23p64s23d4?
a) Titanium (Ti)
c) Sulfur (S)
*b) Chromium (Cr)
d) Selenium (Se)
16. Which is the correct electron configuration for the element Molybdenum (Mo)?
a) 1s22s22p63s23p64s23d4
b) 1s22s22p63s23p64s23d104p65s6
c) 1s22s22p63s23p64s24d104p65s25d4
*d) 1s22s22p63s23p64s23d104p65s24d4
17. Which of these elements has 5 valence electrons?
a) Boron (B)
c) Vanadium (V)
b) Rubidium (Rb)
*d) Arsenic (As)
18. Which is the correct electron dot diagram for the element Silicon (Si)?
*a) A is correct
c)
19. Which is the correct electron dot structure for the element Fluorine (F)?
a)
*b) B is correct
c)
d)
20. How many valence electrons are present in silicon?
a) One
*c) Four
b) Two
d) Six
21. Which category of elements is commonly used to make computer chips and solar cells due to their ability to
conduct electricity only under certain conditions?
a) metals
c) nonmetals
*b) metalloids
d) noble gases
22. Which region is referred to as the p-block on the diagram?
a) A
c) C
b) B
*d) D
23. Which region is referred to as the f-block on the diagram?
a) A
c) C
*b) B
d) D
24. Which region contains the halogen family of elements?
a) A
c) C
b) B
*d) D
25. Which region contains elements with two valence electrons?
*a) A
c) C
b) B
d) D
26. Which region contains elements with an electron configuration that ends with p3?
a) A
*c) C
b) B
d) D
27. Which block on the periodic table contains the actinide series of elements?
a) s-block
c) d-block
b) p-block
*d) f-block
28. Which diagram correctly depicts the trend in electronegativity?
a) a
c) c
*b) b
d) d
29. Which diagram correctly depicts the general trend in first ionization energy?
a) a
c) c
*b) b
d) d
30. Which element has an electron configuration that ends in the fourth energy level?
a) A
c) C
*b) B
d) D
31. Which element is the most metallic?
*a) A
b) B
c) C
d) D
32. Which of the following is representative of a heterogeneous mixture
a) pizza dough
b) milk
*c) chicken noodle soup
d) water
33. Which block is element Y most likely found in?
Element Block Characteristics
X
s
Soft, shiny grey metal; highly
reactive, lightweight
Y
?
Liquid at room temperature; has the
highest electronegativity in its period
Z
p
Used as a semiconductor due to its
electricity-conducting properties
a) s
*b) p
c) d
d) f
34. Which is defined as the energy required to remove an electron from an atom of an element in the gaseous state?
*a) ionization energy
c) ionic radius
b) electronegativity
d) law of octets
35. In which pair is the one on the left larger than the one on the right?
a) Na, Rb
c) Br, Brb) S, Mg
*d) K, K+
36. Identify the period and group numbers of the element with the electron configuration. [Ne]3s23p4
a) Period 2, Group 4
*c) Period 3, Group 16
b) Period 3, Group 4
d) Period 2, Group 16
37. Which correctly describes elements in the same group?
*a) They have the same number of valence electrons.
b) They have electrons in the same outermost energy level.
c) They have the same atomic radius.
d) They must be in the same state of matter.
38. Which is the halogen that is in Period 5?
a) Bromine (Br)
b) Strontium (Sr)
*c) Iodine (I)
d) Xenon (Xe)
39. Which metalloid is in the fourth period and the same group as Carbon?
a) Silicon
c) Tin
*b) Germanium
d) Boron
40. Which is a transition element with five d-block electrons in energy level 4?
a) Niobium (Nb)
c) Manganese (Mn)
b) Renium (Re)
*d) Technicium (Tc)
41. Which is the most important characteristic in detemining an element’s chemical properties?
a) the number of protons and neutrons in its nucleus
b) which period it is found in
*c) the number of valence electrons it contains
d) its outermost energy level
42. Which property describes how much energy must be added to an atom to remove an outermost electron?
a) atomic radius
c) electronegativity
b) ionic radius
*d) ionization energy
43. Which is the charge that results when oxygen becomes an ion?
a) +2
c) +3
b) -3
*d) -2
44. Group 13 elements tend to acquire which charge when they form ions?
+a) +3
c) +5
b) -5
d) -3
45. Which is true of binary ionic compounds?
a) They consist of only two atoms.
*b) They consist of atoms of only two elements.
c) They contain two different anions.
d) They have bonds that share two valence electrons.
46. Which is the correct formula for the compound formed between beryllium and nitrogen?
a) BeN
*c) Be3N2
b) Be3N
d) Be2N3
47. What is the correct formula for the compound formed between magnesium and the phosphate ion?
a) MgPO4
*c) Mg3(PO4)2
b) Mg3PO2
d) MgP2O8
48. Which is the correct formula for the compound Manganese (III) Fluoride?
a) MnF
*c) MnF3
b) Mn3F
d) Mn3F3
49. Which is the correct formula for the compound Chromium (II) Nitrate?
a) (Cr)2NO3
c) CrNO2
b) Cr2NO3
*d) Cr(NO3)2
50. Which is the correct name for the compound FeS?
a) Iron Sulfide
*c) Iron (II) Sulfide
b) Iron (I) Sulfide
d) Iron (II) Sulfide (II)
51. Which is the correct name for the compound CaClO2?
a) Calcium Chloride
b) Calcium Chloroxide
*c) Calcium Chlorite
d) Calcium Chlorate
52. Which is the correct name for the compound Na3P?
*a) Sodium Phosphide
c) Sodium Phosphate
b) Sodium Phosphite
d) Sodium (III) Phosphide
53. Which is the correct name for the compound CoCO3?
a) Carbon Oxygen Carbonate
c) Cobalt Carbonate
*b) Cobalt (II) Carbonate
d) Cobalt Carbonoxide
54. Which is the correct name for the compound (NH4)2SO4?
a) Nitrogen Hydrogen Sulfate
c) Ammonium (II) Sulfate
b) Nitrogen Hydrosulfate
*d) Ammonium Sulfate
55. Which is NOT a diatomic molecule?
a) Fluorine
b) Nitrogen
c) Bromine
*d) Boron
56. Which type of bond has one pair of electrons shared between atoms?
*a) single covalent
c) double covalent
b) coordinate covalent
d) metallic
57. How many single covalent bonds can carbon form?
a) 1
c) 3
b) 2
*d) 4
58. Which is the correct name for the compound PCl5?
a) monophosphorus tetrachloride
*c) phosphorus pentachloride
b) phosphorus chloride
d) pentaphosphorus chloride
59. Which is the correct name for the compound N2O4?
a) tetranitrogen dioxide
c) dinitrogen quadoxide
*b) dinitrogen tetroxide
d) nitrogen oxide
60. Which is the correct formula for the compound dinitrogen monoxide?
a) NO2
c) N2O1
b) (NO)2
*d) N2O
61. Which is the formula for the compound sulfur hexachloride?
a) S6Cl
c) SCl5
*b) SCl6
d) S2Cl3
62. Which is the correct name for the compound HClO3?
a) hydrogen chlorate
c) hydrogen chloride trioxide
*b) chloric acid
d) hydrochloric acid
63. Which is the correct name for the compound HNO2?
a) hyponitrous acid
*c) nitrous acid
b) hydronitrogen dioxide
d) hydronitric acid
64. Which is the correct formula for the compound phosphoric acid?
a) H3P
*c) H3PO4
b) HPO3
d) H3PO3
65. What is the correct ratio of coefficients to balance this chemical equation?
a) 1:2:3
b) 1:2:1.5
*c) 2:4:3
d) 1:1:2
66. Which type of chemical reaction is shown?
a) double replacement
c) synthesis
b) combustion
*d) decomposition
67. Which type of reaction is Al + O2  Al2O3?
*a) synthesis
c) single replacement
b) decomposition
d) combustion
68. Which type of reaction is SiO2 + HF  SiF4 + H2O?
a) synthesis
c) single replacement
*b) double replacement
d) combustion
69. What are the correct coefficients when this equation is balanced? Sb + O2  Sb4O6
a) 1, 2, 10
*c) 4, 3, 1
b) 4, 6, 1
d) 10, 5, 1
70. What are the correct coefficients when this equation is balanced? K + Br 2  KBr
a) 1, 1, 1
*c) 2, 1, 2
b) 1, 2, 1
d) 2, 1, 1
71. What are the correct coefficients when this chemical equation is balanced?
P4 + O2  P2O5
a) 4, 2, 7
c) 2, 5, 4
b) 1, 1, 1
*d) 1, 5, 2
72. Which type of chemical reaction would this be classified as:
C3H8 + O2  CO2 + H2O
a) synthesis
b) double replacement
*c) combustion
d) decomposition
73. Identify the type of reaction shown by this chemical equation:
Al + HCl  AlCl3 + H2
*a) single replacement
b) synthesis
c) double replacement
d) decomposition
74. Which type of chemical reaction is this an example of?
Fe2(SO4)3 + KOH  K2SO4 + Fe(OH)3
a) synthesis
*b) double replacement
c) single replacement
d) combustion
75. Identify the type of chemical reaction demonstrated by this equation:
KClO3  KCl + O2
*a) decomposition
b) synthesis
c) combustion
d) single replacement
76. What type of reaction takes place when fluorine reacts with sodium bromide?
*a) Single-replacement
c) Combination
b) Double-replacement
d) Decomposition
77. Which is the percent composition of bromine in the compound NaBr?
a) 81.6%
c) 84.1%
b) 79.9%
*d) 77.7%
78. Which is the percent composition by mass of phosphorus in Zn3(PO4)2?
*a) 16.1 %
c) 50.1 %
b) 9.66 %
d) 24.01 %
79. Which is the molar mass of the element Calcium?
a) 20 g/mol
*c) 40.078 g/mol
b) 40 g/mol
d) 20.180 g/mol
80. Which is the correct molar mass for the compound CaBr2?
a) 120 g/mole
c) 240 grams
b) 200 moles
*d) 200 g/mole
81. Which is the mass of 8 moles of sodium chloride?
a) 7.3 grams
c) 0.137 g/mole
*b) 468 grams
d) 468 moles
82. Which is the percent composition by mass of bromine in the compound NaBr?
a) 81.6%
c) 84.1%
b) 79.9%
*d) 77.7%
83. Which term is described as the lowest whole-number ratio of elements in a compound?
a) hydrate
*c) empirical formula
b) molecular formula
d) percent composition
84. How many molecules are in 3.6 grams of NaCl?
a) 0.06
c) 1.3  1026
b) 1.0  1021
*d) 3.7  1022
85. How many grams are in 1.946 moles of NaCl?
*a) 113.8 g
c) 0.033 g
b) 30.1 g
d) 44.7 g
86. Calculate the number of molecules in 4.0 mol H2O.
a) 0.60  1023 molecules
c) 2.4  10–23 molecules
*b) 2.4  1024 molecules
d) 2.4  1023 molecules
87. How many moles of Ag contain 4.49  1023 atoms Ag?
a) 0.745  1024 mol
*c) 0.745 mol
b) 0.745  1023 mol
d) 27.0 mol
88. Copper (Cu) is a transition element used in the making of coins. Calculate the mass in grams of 0.0420 moles of
copper.
a) 0.00697 g
*c) 2.67 g
b) 0.252 g
d) 6.61 g
89. How many moles are present in 21.2 g hydrochloric acid?
*a) 0.582 mol
c) 21.0 mol
b) 1.72 mol
d) 128 mol
90. What is the mass in grams of 1.02  1024 atoms manganese (Mn)?
a) 0.112  101 g
c) 9.30  10–1 g
1
b) 0.169  10 g
*d) 9.30  101 g
91. Determine the number of moles present in 32.5 g aluminum chloride.
*a) 0.244 mol
c) 1.21 mol
b) 4.10 mol
d) 720 mol
92. What is the mass of 2.25 moles of sulfuric acid (H2SO4)?
a) 50.0 g
c) 112 g
b) 98.0 g
*d) 220 g
93. Which is both an empirical formula AND a molecular formula?
a) C2H4O2
*c) C3H6O2
b) C6H12O6
d) C4H8
94. Which would be an exothermic process
a) solid to liquid
b) liquid to gas
*c) gas to liquid
d) solid to gas
95. Which element has the greatest attraction for electrons in a chemical bond?
a) P
*c) S
b) Si
d) Al
96. At standard temperature and pressure (STP) which will have the same total number of atoms as 1.0 L of argon
a) 1.5 L He
c) 0.5 L Ne
*b) 1.0 L Xe
d) 2.0 L Rn
97. How many moles of carbon dioxide are produced when 19.3 mol of propane gas is burned in excess oxygen?
a) 6.43 mol
*b) 57.9 mol
c) 32.2 mol
d) 6.84 mol
98. How many grams of H2O will be produced if 750 grams of Fe are produced?
a) 17.9 g
*b) 322 g
c) 563 g
d) 241 g
99. How many grams of water are produced when 2.50 mol oxygen reacts with hydrogen?
a) 0.277 g
c) 45.0 g
b) 22.5 g
*d) 90.0 g
100. Calculate the average atomic mass of element X, based on teh information in the table below:
Isotope
X-6
X-7
a) 6.48 amu
*b) 6.94 amu
Mass (amu)
6.015
7.016
c) 64.8 amu
d) 69.4 amu
Relatve abundance
7.59%
92.41%
FINAL EXAM PRACTICE TEST
Answer Section
MULTIPLE CHOICE
1. ANS: C
PTS: 2
2. ANS: B
PTS: 2
3. ANS: C
PTS: 1
DIF: Bloom's Level 1|DOK 1
NAT: B.2
STA: SC1
4. ANS: B
PTS: 1
DIF: Bloom's Level 2|DOK 1
NAT: B.1
STA: SC3.a
5. ANS: A
PTS: 1
DIF: Bloom's Level 1|DOK 1
NAT: B.1
STA: SC3.a
6. ANS: C
PTS: 1
DIF: Bloom's Level 2|DOK 1
NAT: B.1
STA: SC3.a
7. ANS: D
PTS: 1
DIF: Bloom's Level 4|DOK 1
NAT: UCP.2 | B.1 STA: SC3.d
8. ANS: D
PTS: 1
DIF: Bloom's Level 2|DOK 1
NAT: B.1
STA: SC3
9. ANS: B
PTS: 1
DIF: Bloom's Level 3|DOK 1
NAT: B.1
STA: SC3
10. ANS: B
PTS: 1
DIF: Bloom's Level 3|DOK 1
NAT: B.1
STA: SC3.c
11. ANS: B
PTS: 1
DIF: Bloom's Level 2|DOK 2
NAT: B.1
STA: SC3.c
12. ANS: D
PTS: 1
DIF: Bloom's Level 2|DOK 1
NAT: B.1
STA: SC3
13. ANS: D
PTS: 1
DIF: Bloom's Level 3|DOK 2
NAT: UCP.2 | B.1 STA: SC3.b
14. ANS: B
PTS: 1
DIF: Bloom's Level 3|DOK 2
NAT: UCP.2 | B.1 STA: SC3.b
15. ANS: B
PTS: 1
DIF: Bloom's Level 4|DOK 2
NAT: UCP.2 | B.1 STA: SC3.b
16. ANS: D
PTS: 1
DIF: Bloom's Level 3|DOK 2
NAT: UCP.2 | B.1 STA: SC3.b
17. ANS: D
PTS: 1
DIF: Bloom's Level 4|DOK 2
NAT: UCP.2 | B.1 STA: SC3.b
18. ANS: A
PTS: 1
DIF: Bloom's Level 3|DOK 2
NAT: UCP.2 | B.1
19. ANS: B
PTS: 1
DIF: Bloom's Level 3|DOK 2
NAT: UCP.2 | B.1
20. ANS: C
The electron configuration of silicon is 1s22s22p63s23p2.
Feedback
A
B
C
Silicon is a group 4A element.
Silicon is a group 4A element.
Correct!
D
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PTS:
STA:
TOP:
KEY:
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Silicon is a group 4A element.
1
DIF: Bloom's Level 2|DOK 2
NAT: B.1 | B.6
SC3.b
Define valence electrons and draw electron-dot structures representing an atom's valence electrons.
Valence electrons
MSC: 2
B
PTS: 1
DIF: Bloom's Level 1|DOK 1
B.1 | B.2
STA: SC4.b
D
PTS: 1
DIF: Bloom's Level 2|DOK 2
UCP.2
STA: SC4
B
PTS: 1
DIF: Bloom's Level 2|DOK 2
UCP.2
STA: SC4
C
PTS: 1
DIF: Bloom's Level 2|DOK 2
UCP.2 | B.2 STA: SC4
A
PTS: 1
DIF: Bloom's Level 4|DOK 2
UCP.2 | B.1 | B.2
STA: SC4
C
PTS: 1
DIF: Bloom's Level 4|DOK 2
UCP.2 | B.1 | B.2
STA: SC4
D
PTS: 1
DIF: Bloom's Level 4|DOK 2
UCP.2 | B.1 | B.2
STA: SC4
B
PTS: 1
DIF: Bloom's Level 4|DOK 2
UCP.2 | B.1 STA: SC4.a
B
PTS: 1
DIF: Bloom's Level 4|DOK 2
UCP.2
STA: SC4.a
B
PTS: 1
DIF: Bloom's Level 4|DOK 2
UCP.2
STA: SC4
A
PTS: 1
DIF: Bloom's Level 2|DOK 2
UCP.2 | B.1 | B.2
STA: SC4.b
C
PTS: 2
B
PTS: 1
DIF: Bloom's Level 5|DOK 2
UCP.2 | B.2 STA: SC4.b
A
PTS: 1
DIF: Bloom's Level 1|DOK 1
UCP.2
STA: SC4.a
D
PTS: 1
DIF: Bloom's Level 3|DOK 2
B.1 | B.6
STA: SC4.a
C
PTS: 1
DIF: Bloom's Level 3|DOK 2
B.1 | B.2
STA: SC4
A
PTS: 1
DIF: Bloom's Level 2|DOK 1
B.1 | B.2
STA: SC4
C
PTS: 1
DIF: Bloom's Level 4|DOK 2
B.1 | B.2
STA: SC4
B
PTS: 1
DIF: Bloom's Level 4|DOK 2
B.1 | B.2
STA: SC4
D
PTS: 1
DIF: Bloom's Level 4|DOK 2
B.1 | B.2
STA: SC4
C
PTS: 1
DIF: Bloom's Level 3|DOK 1
B.1 | B.2
STA: SC4.b
D
PTS: 1
DIF: Bloom's Level 1|DOK 1
B.1 | B.2
STA: SC4.a
43. ANS:
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63. ANS:
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64. ANS:
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65. ANS:
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66. ANS:
NAT:
D
B.1
A
B.1 | B.2
B
B.1 | B.2
C
UCP.2 | B.2
C
UCP.2 | B.2
C
UCP.2 | B.2
D
UCP.2 | B.2
C
UCP.2 | B.2
C
UCP.2 | B.2
A
UCP.2 | B.2
B
UCP.2 | B.2
D
UCP.2 | B.2
D
B.1 | B.2
A
B.1
D
B.1
C
B.2
B
B.2
D
B.2
B
B.2
B
B.2
C
B.2
C
B.2
C
UCP.2 | B.3
D
UCP.2 | B.3;
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SC1.c
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SC1.d
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1
SC1.d
1
SC1.d
1
SC1.c
1
SC2.a
1
SC2.a
DIF: Bloom's Level 3|DOK 2
DIF: Bloom's Level 2|DOK 2
DIF: Bloom's Level 2|DOK 1
DIF: Bloom's Level 3|DOK 2
DIF: Bloom's Level 3|DOK 2
DIF: Bloom's Level 3|DOK 2
DIF: Bloom's Level 3|DOK 2
DIF: Bloom's Level 3|DOK 2
DIF: Bloom's Level 3|DOK 2
DIF: Bloom's Level 3|DOK 2
DIF: Bloom's Level 3|DOK 2
DIF: Bloom's Level 3|DOK 2
DIF: Bloom's Level 2|DOK 2
DIF: Bloom's Level 2|DOK 2
DIF: Bloom's Level 3|DOK 2
DIF: Bloom's Level 3|DOK 2
DIF: Bloom's Level 3|DOK 2
DIF: Bloom's Level 3|DOK 2
DIF: Bloom's Level 3|DOK 2
DIF: Bloom's Level 3|DOK 2
DIF: Bloom's Level 3|DOK 2
DIF: Bloom's Level 3|DOK 2
DIF: Bloom's Level 4|DOK 2
DIF: Bloom's Level 3|DOK 1
67. ANS: A
PTS: 1
DIF: Bloom's Level 3|DOK 1
NAT: B.3
STA: SC2.a
68. ANS: B
PTS: 1
DIF: Bloom's Level 3|DOK 1
NAT: B.3
STA: SC2.a
69. ANS: C
PTS: 1
DIF: Bloom's Level 3|DOK 2
NAT: UCP.3 | B.3 STA: SC2.a
70. ANS: C
PTS: 1
DIF: Bloom's Level 3|DOK 2
NAT: UCP.3 | B.3 STA: SC2.a
71. ANS: D
PTS: 1
DIF: Bloom's Level 3|DOK 2
NAT: UCP.3 | B.3 STA: SC2.a
72. ANS: C
PTS: 1
DIF: Bloom's Level 3|DOK 1
NAT: B.3
STA: SC2.a
73. ANS: A
PTS: 1
DIF: Bloom's Level 3|DOK 1
NAT: UCP.2 | B.3 STA: SC2.a
74. ANS: B
PTS: 1
DIF: Bloom's Level 3|DOK 1
NAT: UCP.2 | B.3 STA: SC2.a
75. ANS: A
PTS: 1
DIF: Bloom's Level 3|DOK 1
NAT: UCP.2 | B.3 STA: SC2.a
76. ANS: A
As fluorine replaces only bromide ions from sodium bromide and forms sodium fluoride as the product, the
reaction is a single-replacement reaction.
Feedback
A
B
C
D
77.
78.
79.
80.
81.
82.
83.
84.
PTS:
STA:
KEY:
ANS:
NAT:
ANS:
NAT:
ANS:
NAT:
ANS:
NAT:
ANS:
NAT:
ANS:
NAT:
ANS:
NAT:
ANS:
NAT:
Correct!
Since only one ion of more reactive halogen fluorine replaces one ion of less reactive
halogen bromine, it is a single ion replacement reaction.
Fluorine replaces bromine from its compound.
In a decomposition reaction, a single compound breaks into two or more elements or
compounds.
1
DIF: Bloom's Level 1|DOK 1
NAT: UCP.1 | B.3
SC2.a
TOP: Identify the characteristics of different classes of chemical reactions.
Replacement reaction
MSC: 2
D
PTS: 1
DIF: Bloom's Level 3|DOK 2
UCP.3 | B.2 STA: SC2.d
A
PTS: 1
DIF: Bloom's Level 3|DOK 2
UCP.3 | B.3 STA: SC2.d
C
PTS: 1
DIF: Bloom's Level 2|DOK 2
B.2
STA: SC2
D
PTS: 1
DIF: Bloom's Level 3|DOK 2
B.2
STA: SC2.c
B
PTS: 1
DIF: Bloom's Level 3|DOK 2
B.2
STA: SC2.d
D
PTS: 1
DIF: Bloom's Level 3|DOK 2
UCP.3 | B.2 STA: SC2.d
C
PTS: 1
DIF: Bloom's Level 1|DOK 1
UCP.2 | B.2 STA: SC2.c
D
PTS: 1
DIF: Bloom's Level 3|DOK 2
UCP.3 | B.2 STA: SC2.d
85. ANS: A
NAT: UCP.3 | B.3
86. ANS: B
PTS: 1
STA: SC2.d
DIF: Bloom's Level 3|DOK 2
Feedback
A
B
C
D
PTS:
STA:
TOP:
KEY:
87. ANS:
Multiply the number of moles by the number of molecules.
Correct!
Multiply the number of moles with the correct value of Avogadro's number.
The position of the decimal value is incorrect.
1
DIF: Bloom's Level 1|DOK 2
NAT: UCP.3
SC2.d
Convert moles to number of representative particles and number of representative particles to moles.
Converting moles to representative particles
MSC: 3
C
Feedback
A
B
C
D
PTS:
STA:
TOP:
KEY:
88. ANS:
Multiply the number of atoms by the inverse of Avogadro's number.
After multiplying the number of atoms by the inverse of Avogadro's number, the power
of the indices is nullified.
Correct!
Divide the number of atoms by Avogadro's number.
1
DIF: Bloom's Level 1|DOK 2
NAT: UCP.3
SC2.d
Convert moles to number of representative particles and number of representative particles to moles.
Converting representative particles to moles
MSC: 3
C
Feedback
A
B
C
D
Instead of dividing the known number of moles of copper by Avogadro's number,
multiply it with the molar mass of copper.
Instead of multiplying the known number of moles of copper by Avogadro's number,
multiply it with the molar mass of copper.
Correct!
Multiply the known number of moles of copper by the molar mass of copper.
PTS: 1
DIF: Bloom's Level 1|DOK 2
NAT: UCP.3 | B.1
STA: SC2.d
TOP: Calculate the number of moles in a given mass of an element and the mass of a given number of moles of
an element.
KEY: Mole to mass conversion
MSC: 3
89. ANS: A
Feedback
A
B
C
D
Correct!
Divide the number of grams by the molar mass.
The molar mass of a compound is numerically equal to its atomic mass.
To calculate the number of moles, multiply the number of grams by the inverse of the
molar mass.
PTS: 1
DIF: Bloom's Level 1|DOK 2
NAT: UCP.3
STA: SC2.d
TOP: Calculate the number of moles of a compound from a given mass of the compound, and the mass of a
compound from a given number of moles of the compound.
KEY: Mass to mole conversion
MSC: 3
90. ANS: D
Feedback
A
B
C
D
PTS:
STA:
TOP:
KEY:
91. ANS:
Divide the number of atoms by Avogadro's number and then multiply it by the molar
mass of the element.
Multiply the calculated number of moles of the element by its molar mass.
Subtract 23 from the power of the element to obtain the correct power.
Correct!
1
DIF: Bloom's Level 2|DOK 2
NAT: UCP.3 | B.1
SC2.c
Calculate the number of moles of an element when given the number of atoms of the element.
Atoms to mass conversion
MSC: 3
A
Feedback
A
B
C
D
Correct!
Divide the number of grams by the molar mass.
The molar mass of a compound is numerically equal to its atomic mass.
To calculate the number of moles, multiply the number of grams by the inverse of the
molar mass.
PTS: 1
DIF: Bloom's Level 1|DOK 2
NAT: UCP.3
STA: SC2.d
TOP: Calculate the number of moles of a compound from a given mass of the compound, and the mass of a
compound from a given number of moles of the compound.
KEY: Mass to mole conversion
MSC: 3
92. ANS: D
Step 1:
Step 2:
Feedback
A
B
C
D
93.
94.
95.
96.
97.
98.
99.
The number of grams of sulfuric acid is 98.0 g.
Multiply the molar mass by 2.25 moles of sulfuric acid.
The atomic mass of oxygen is 16.
Correct!
PTS: 1
DIF: Bloom's Level 2|DOK 2
NAT: UCP.3
STA: SC2.d
TOP: Calculate the number of moles of a compound from a given mass of the compound, and the mass of a
compound from a given number of moles of the compound.
KEY: Converting moles of a compound to mass
MSC: 3
ANS: C
PTS: 2
ANS: C
PTS: 2
ANS: C
PTS: 2
ANS: B
PTS: 2
ANS: B
PTS: 1
DIF: Bloom's Level 3|DOK 2
NAT: UCP.3 | B.3 STA: SC2.d
ANS: B
PTS: 1
DIF: Bloom's Level 3|DOK 2
NAT: UCP.3 | B.3 STA: SC2.d
ANS: D
The balanced chemical equation is
.
Feedback
A
B
C
D
PTS:
STA:
KEY:
100. ANS:
Multiply the number of moles of water by the molar mass of water.
Multiply the number of moles by the mole ratio.
Balance the equation correctly.
Correct!
1
DIF: Bloom's Level 3|DOK 2
NAT: UCP.1 | UCP.3 | B.3
SC2.d
TOP: Use the steps to solve stoichiometric problems.
Stoichiometric mole-to-mass conversion
MSC: 3
B
PTS: 1