Name: ______________________
Class: _________________
Date: _________
ID: A
EOC review Chpt 9/10
Matching
Match each item with the correct statement below.
a. monatomic ion
f. cation
b. acid
g. binary compound
c. base
h. anion
d. law of definite proportions
i. polyatomic ion
e. law of multiple proportions
____
1. consists of a single atom with a positive or negative charge
____
2. atom or group of atoms having a negative charge
____
3. atom or group of atoms having a positive charge
____
4. tightly-bound group of atoms that behaves as a unit and carries a net charge
____
5. produces a hydrogen ion when dissolved in water
____
6. produces a hydroxide ion when dissolved in water
Match each item with the correct statement below.
a. molar volume
b. molar mass
c. atomic mass
____
7. the number of grams of an element that is numerically equal to the atomic mass of the element in amu
____
8. the mass of a mole of any element or compound
____
9. the volume occupied by a mole of any gas at STP
Match each item with the correct statement below.
a. representative particle
d. percent composition
b. mole
e. standard temperature and pressure
c. Avogadro's number
f. empirical formula
____ 10. the number of representative particles of a substance present in 1 mole of that substance
____ 11. an atom, an ion, or a molecule, depending upon the way a substance commonly exists
____ 12. the SI unit used to measure amount of substance
____ 13. 0°C and 1 atm
____ 14. the percent by mass of each element in a compound
____ 15. the smallest whole number ratio of the atoms in a compound
1
Name: ______________________
ID: A
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____ 16. When Group 2A elements form ions, they
a. lose two protons.
b. gain two protons.
c. lose two electrons.
d. gain two electrons.
____ 17. When naming a transition metal ion that can have more than one common ionic charge, the numerical
value of the charge is indicated by a
a. prefix.
b. suffix.
c. Roman numeral following the name.
d. superscript after the name.
____ 18. Aluminum is a group 3A metal. Which ion does A1 typically form?
3−
a. Al
3+
b. Al
5−
c. Al
5+
d. Al
____ 19. The
a.
b.
c.
d.
ions formed by nonmetals in Groups 6A and 7A
have a numerical charge that is found by subtracting the group number from 8.
have a numerical charge that is found by subtracting 8 from the group number.
all have a numerical charge of – 1.
all have a name that ends in -ate.
____ 20. Which of the following is a cation?
a. SO3 2b. sulfate
c.
d.
2+
Ca
chlorite
____ 21. In which of the following are the symbol and name for both of the ions given correctly?
+
+
a.
NH 4 : ammonia; H : hydride
b.
C 2 H 3 O 2 − : acetate; C 2 O 4 − : oxalite
c.
d.
OH − : hydroxide; O : oxide
3−
3−
PO 3 : phosphate; PO 4 : phosphite
____ 22. An
a.
b.
c.
d.
2−
-ate or -ite at the end of a compound name usually indicates that the compound contains
fewer electrons than protons.
neutral molecules.
only two elements.
a polyatomic anion.
2
Name: ______________________
ID: A
____ 23. How are chemical formulas of binary ionic compounds generally written?
a. cation on left, anion on right
b. anion on left, cation on right
c. Roman numeral first, then anion, then cation
d. subscripts first, then ions
____ 24. Which of the following is true about the composition of ionic compounds?
a. They are composed of anions and cations.
b. They are composed of anions only.
c. They are composed of cations only.
d. They are formed from two or more nonmetallic elements.
____ 25. Which of the following formulas represents an ionic compound?
a. CS 2
b.
BaI 2
c.
N2 O4
d.
PCl 3
____ 26. Which of the following shows correctly an ion pair and the ionic compound the two ions form?
a.
Sn
4+
,N
3−
; Sn 4 N 3
b.
Cu
2+
,O
2−
; Cu 2 O 2
c.
Cr
3+
, I − ; CrI
d.
Fe , O
3+
2−
; Fe 2 O 3
____ 27. In which of the following is the name and formula given correctly?
a. sodium oxide, NaO
b. barium nitride, BaN
c. cobaltous chloride, CoCl 3
d.
stannic fluoride, SnF 4
____ 28. Which of the following compounds contains the lead(II) ion?
a. PbO
b. PbCl4
c. Pb2 O
d. Pb2 S
____ 29. What is the correct formula for potassium sulfite?
a. KHSO 3
b.
KHSO 4
c.
K 2 SO 3
d.
K 2 SO 4
3
Name: ______________________
ID: A
____ 30. Molecular compounds are usually
a. composed of two or more transition elements.
b. composed of positive and negative ions.
c. composed of two or more nonmetallic elements.
d. exceptions to the law of definite proportions.
____ 31. What is the ending for the names of all binary compounds, both ionic and molecular?
a. -ide
b. -ite
c. -ade
d. -ate
____ 32. Binary molecular compounds are made of two ____.
a. metallic elements
b. nonmetallic elements
c. polyatomic ions
d. cations
____ 33. Which of the following correctly shows a prefix used in naming binary molecular compounds with its
corresponding number?
a. deca-, 7
b. nona-, 9
c. hexa-, 8
d. octa-, 4
____ 34. Which of the following formulas represents a molecular compound?
a. ZnO
b. Xe
c. SO 2
d.
BeF 2
____ 35. When dissolved in water, acids produce ____.
a. negative ions
b. polyatomic ions
c. hydrogen ions
d. oxide ions
____ 36. When naming acids, the prefix hydro- is used when the name of the acid anion ends in ____.
a. -ide
b. -ite
c. -ate
d. -ic
____ 37. Which of the following shows both the correct formula and correct name of an acid?
a. HClO 2 , chloric acid
b.
HNO 2 , hydronitrous acid
c.
H 3 PO 4 , phosphoric acid
d.
HI, iodic acid
4
Name: ______________________
ID: A
____ 38. What is the name of H 2 SO 3 ?
a.
b.
c.
d.
hyposulfuric acid
hydrosulfuric acid
sulfuric acid
sulfurous acid
____ 39. What is the formula for sulfurous acid?
a. H 2 SO 4
b.
H 2 SO 3
c.
H 2 SO 2
d.
H2 S
____ 40. What is the formula for phosphoric acid?
a. H 2 PO 3
b.
H 3 PO 4
c.
HPO 2
d.
HPO 4
____ 41. What is the formula for hydrosulfuric acid?
a. H 2 S2
b.
H 2 SO 2
c.
HSO 2
d.
H2 S
____ 42. Which of the following are produced when a base is dissolved in water?
a. hydronium ions
b. hydroxide ions
c. hydrogen ions
d. ammonium ions
____ 43. How are bases named?
a. like monatomic elements
b. like polyatomic ions
c. like ionic compounds
d. like molecular compounds
____ 44. Select the correct formula for sulfur hexafluoride.
a. S2 F 6
b.
F 6 SO 3
c.
F 6 S2
d.
SF 6
5
Name: ______________________
ID: A
____ 45. What is the correct name for the compound CoCl 2 ?
a.
b.
c.
d.
cobalt(I) chlorate
cobalt(I) chloride
cobalt(II) chlorate
cobalt(II) chloride
____ 46. Suppose you encounter a chemical formula with H as the cation. What do you know about this compound
immediately?
a. It is a polyatomic ionic compound.
b. It is an acid.
c. It is a base.
d. It has a +1 charge.
____ 47. What is the correct formula for barium chlorate?
a. Ba(ClO) 2
b.
Ba(ClO 2 ) 2
c.
Ba(ClO 3 ) 2
d.
BaCl 2
____ 48. What is the correct formula for calcium dihydrogen phosphate?
a. CaH 2 PO 4
b.
Ca 2 H 2 PO 4
c.
Ca(H 2 PO 4 ) 2
d.
Ca(H 2 HPO 4 ) 2
____ 49. Which of the following is the correct name for N 2 O 5 ?
a.
b.
c.
d.
nitrous oxide
dinitrogen pentoxide
nitrogen dioxide
nitrate oxide
____ 50. What is the correct name for Sn 3 (PO 4 ) 2 ?
a.
b.
c.
d.
tritin diphosphate
tin(II) phosphate
tin(III) phosphate
tin(IV) phosphate
____ 51. What SI unit is used to measure the number of representative particles in a substance?
a. kilogram
b. ampere
c. kelvin
d. mole
6
Name: ______________________
ID: A
____ 52. How many hydrogen atoms are in 5 molecules of isopropyl alcohol, C 3 H 7 O?
23
a.
b.
c.
5 × (6.02 × 10 )
5
35
d.
35 × (6.02 × 10 )
____ 53. If a
a.
b.
c.
d.
23
dozen Clementine oranges have a mass of 744 g, what will be the mass of 15 Clementines?
11.16 kg
595 g
896 g
930 g
____ 54. Which of the following elements exists as a diatomic molecule?
a. neon
b. lithium
c. nitrogen
d. sulfur
____ 55. Which of the following is equal to Avogadro's number?
a. the number of atoms of bromine in 1 mol Br 2
b.
the number of molecules of chlorine in 0.50 mol Cl 2
c.
the number of molecules of nitrogen in 1 mol N 2
d.
the number of atoms in 1 mol CO
____ 56. How many moles of tungsten atoms are in 4.8 × 10
atoms of tungsten?
2
a.
8.0 × 10 moles
b.
8.0 × 10 moles
c.
1.3 × 10
−1
moles
1.3 × 10
−2
moles
d.
25
1
____ 57. How many atoms are in 0.075 mol of titanium?
a. 1.2 × 10-25
b.
2.2 × 10
24
c.
6.4 × 10
2
d.
4.5 × 10
22
____ 58. The
a.
b.
c.
d.
atomic masses of any two elements contain the same number of ____.
atoms
grams
ions
milliliters
7
Name: ______________________
ID: A
____ 59. What is true about the molar mass of chlorine gas?
a. The molar mass is 35.5 g.
b. The molar mass is 71.0 g.
c. The molar mass is equal to the mass of one mole of chlorine atoms.
d. none of the above
____ 60. What is the molar mass of AuCl3 ?
a. 96 g
b. 130 g
c. 232.5 g
d. 303.6 g
____ 61. What is the mass in grams of 5.90 mol C 8 H 18 ?
a.
b.
c.
d.
0.0512 g
19.4 g
389 g
673 g
____ 62. What is the number of moles of beryllium atoms in 36 g of Be?
a. 0.25 mol
b. 4.0 mol
c. 45.0 mol
d. 320 mol
____ 63. For which of the following conversions does the value of the conversion factor depend upon the formula
of the substance?
a. volume of gas (STP) to moles
b. density of gas (STP) to molar mass
c. mass of any substance to moles
d. moles of any substance to number of particles
____ 64. What is the mass of oxygen in 250 g of sulfuric acid, H 2 SO 4 ?
a.
b.
c.
d.
____ 65. The
a.
b.
c.
d.
0.65 g
3.9 g
16 g
160 g
volume of one mole of a substance is 22.4 L at STP for all ____.
gases
liquids
solids
compounds
____ 66. Which combination of temperature and pressure correctly describes standard temperature and pressure,
STP?
a. 0°C and 101.3 kPa
b. 1°C and 0 kPa
c. 0°C and 22.4 kPa
d. 100°C and 100 kPa
8
Name: ______________________
____ 67. The
a.
b.
c.
d.
ID: A
molar mass of a substance can be calculated from its density alone, if that substance is a(n) ____.
element
gas at STP
liquid
solid
____ 68. What is the volume, in liters, of 0.500 mol of C 3 H 8 gas at STP?
a.
b.
c.
d.
0.0335 L
11.2 L
16.8 L
22.4 L
____ 69. What is the density at STP of the gas sulfur hexafluoride, SF 6 ?
a.
b.
c.
0.153 g/L
6.52 g/L
3270 g/L
d.
3.93 × 10
24
g/L
____ 70. Which of the following gas samples would have the largest number of representative particles at STP?
a. 12.0 L He
b. 7.0 L O 2
c.
d.
0.10 L Xe
0.007 L SO 3
____ 71. Which of the following gases at STP would have the greatest volume?
a. 4.00 mole of He
b. 1.00 mole of O 2
c.
0.200 mole of SO 3
d.
5.00 mole of H 2
____ 72. To
a.
b.
c.
d.
determine the formula of a new substance, one of the first steps is to find the
molar mass.
percent composition.
volume at STP.
number of particles per mole.
____ 73. What information is needed to calculate the percent composition of a compound?
a. the weight of the sample to be analyzed and its density
b. the weight of the sample to be analyzed and its molar volume
c. the formula of the compound and the atomic mass of its elements
d. the formula of the compound and its density
9
Name: ______________________
ID: A
____ 74. If 60.2 grams of Hg combines completely with 24.0 grams of Br to form a compound, what is the
percent composition of Hg in the compound?
a. 28.5%
b. 39.9%
c. 71.5%
d. 60.1%
____ 75. The
a.
b.
c.
d.
lowest whole-number ratio of the elements in a compound is called the ____.
empirical formula
molecular formula
binary formula
representative formula
____ 76. Which of the following is an empirical formula?
a. C 2 N 2 H 8
b.
C3 H 8 O
c.
Be 2 (Cr 2 O 7 ) 2
d.
Sb4 S6
____ 77. Which of the following compounds have the same empirical formula?
a. CO 2 and SO 2
b.
C 7 H 14 and C 10 H 20
c.
C 4 H 10 and C 10 H 4
d.
C 6 H 12 and C 6 H 14
____ 78. What is the empirical formula of a compound that is 40% sulfur and 60% oxygen by weight?
a. SO
b. SO 2
c.
SO 3
d.
S6 O 4
____ 79. What is the empirical formula of a substance that is 53.5% C, 15.5% H, and 31.1% N by weight?
a. C 3 HN 2
b.
C 4 H 14 N 2
c.
C2 H 8 N
d.
CH 4 N 7
____ 80. Which of the following sets of empirical formula, molar mass, and molecular formula is correct?
a. CH, 78 g, C 13 H 13
b.
CH 4 N, 90 g, C 3 H 12 N 3
c.
CaO, 56 g, Ca 2 O 2
d.
C 3 H 8 O, 120 g, C 3 H 8 O 2
10
ID: A
EOC review Chpt 9/10
Answer Section
MATCHING
1. ANS:
OBJ:
BLM:
2. ANS:
OBJ:
BLM:
3. ANS:
OBJ:
BLM:
4. ANS:
OBJ:
BLM:
5. ANS:
OBJ:
6. ANS:
OBJ:
A
PTS: 1
DIF: L1
REF: p. 264
9.1.1 Explain how to determine the charges of monatomic ions.
knowledge
H
PTS: 1
DIF: L1
REF: p. 265
9.1.1 Explain how to determine the charges of monatomic ions.
knowledge
F
PTS: 1
DIF: L1
REF: p. 264
9.1.1 Explain how to determine the charges of monatomic ions.
knowledge
I
PTS: 1
DIF: L1
REF: p. 268
9.1.2 Explain how polyatomic ions differ from and are similar to monatomic ions.
knowledge
B
PTS: 1
DIF: L1
REF: p. 285
9.4.1 Determine the name and formula of an acid.
BLM: knowledge
C
PTS: 1
DIF: L1
REF: p. 287
9.4.2 Determine the name and formula of a base.
BLM: knowledge
7. ANS:
OBJ:
BLM:
8. ANS:
OBJ:
BLM:
9. ANS:
OBJ:
BLM:
C
PTS: 1
DIF: L1
REF: p. 313
10.1.3 Determine the molar mass of an element and of a compound.
knowledge
B
PTS: 1
DIF: L1
REF: p. 314
10.1.3 Determine the molar mass of an element and of a compound.
knowledge
A
PTS: 1
DIF: L1
REF: p. 320
10.2.2 Convert the volume of a gas at STP to the number of moles of the gas.
knowledge
10. ANS: C
PTS: 1
DIF: L1
REF: p. 308
OBJ: 10.1.2 Explain how chemists count the number of atoms, molecules, or formula units in a
substance.
BLM: knowledge
11. ANS: A
PTS: 1
DIF: L1
REF: p. 308
OBJ: 10.1.2 Explain how chemists count the number of atoms, molecules, or formula units in a
substance.
BLM: knowledge
12. ANS: B
PTS: 1
DIF: L1
REF: p. 308
OBJ: 10.1.2 Explain how chemists count the number of atoms, molecules, or formula units in a
substance.
BLM: knowledge
13. ANS: E
PTS: 1
DIF: L1
REF: p. 320
OBJ: 10.2.2 Convert the volume of a gas at STP to the number of moles of the gas.
BLM: knowledge
14. ANS: D
PTS: 1
DIF: L1
REF: p. 325
OBJ: 10.3.1 Calculate the percent by mass of an element in a compound.
BLM: knowledge
1
ID: A
15. ANS: F
PTS: 1
DIF: L1
REF: p. 330
OBJ: 10.3.2 Calculate the empirical formula of a compound.
BLM: knowledge
MULTIPLE CHOICE
16. ANS: C
PTS: 1
DIF: L2
REF: p. 264 | p. 265
OBJ: 9.1.1 Explain how to determine the charges of monatomic ions.
BLM: comprehension
17. ANS: C
PTS: 1
DIF: L2
REF: p. 265 | p. 266
OBJ: 9.1.1 Explain how to determine the charges of monatomic ions.
BLM: comprehension
18. ANS: B
PTS: 1
DIF: L2
REF: p. 264 | p. 265
OBJ: 9.1.1 Explain how to determine the charges of monatomic ions.
BLM: comprehension
19. ANS: B
PTS: 1
DIF: L2
REF: p. 265
OBJ: 9.1.1 Explain how to determine the charges of monatomic ions.
BLM: comprehension
20. ANS: C
PTS: 1
DIF: L2
REF: p. 268
OBJ: 9.1.2 Explain how polyatomic ions differ from and are similar to monatomic ions.
BLM: application
21. ANS: C
PTS: 1
DIF: L2
REF: p. 264 | p. 265 | p. 268
OBJ: 9.1.1 Explain how to determine the charges of monatomic ions. | 9.1.2 Explain how polyatomic
ions differ from and are similar to monatomic ions.
BLM: application
22. ANS: D
PTS: 1
DIF: L2
REF: p. 268 | p. 269
OBJ: 9.1.2 Explain how polyatomic ions differ from and are similar to monatomic ions.
BLM: application
23. ANS: A
PTS: 1
DIF: L2
REF: p. 272
OBJ: 9.2.1 Apply the rules for naming and writing formulas for binary ionic compounds.
BLM: comprehension
24. ANS: A
PTS: 1
DIF: L2
REF: p. 272
OBJ: 9.2.1 Apply the rules for naming and writing formulas for binary ionic compounds.
BLM: comprehension
25. ANS: B
PTS: 1
DIF: L2
REF: p. 272 | p. 280
OBJ: 9.2.1 Apply the rules for naming and writing formulas for binary ionic compounds. | 9.3.1 Apply
the rules for naming and writing formulas for binary molecular compounds.
BLM: application
26. ANS: D
PTS: 1
DIF: L2
REF: p. 272 | p. 273
OBJ: 9.2.1 Apply the rules for naming and writing formulas for binary ionic compounds.
BLM: application
27. ANS: D
PTS: 1
DIF: L2
REF: p. 272 | p. 273 | p. 274 | p. 275
OBJ: 9.2.1 Apply the rules for naming and writing formulas for binary ionic compounds.
BLM: application
28. ANS: A
PTS: 1
DIF: L2
REF: p. 272 | p. 273
OBJ: 9.2.1 Apply the rules for naming and writing formulas for binary ionic compounds.
BLM: application
2
ID: A
29. ANS: C
PTS: 1
DIF: L2
REF: p. 276 | p. 277
OBJ: 9.2.2 Apply the rules for naming and writing formulas for compounds with polyatomic ions.
BLM: application
30. ANS: C
PTS: 1
DIF: L2
REF: p. 280
OBJ: 9.3.1 Apply the rules for naming and writing formulas for binary molecular compounds.
BLM: comprehension
31. ANS: A
PTS: 1
DIF: L2
REF: p. 265 | p. 275 | p. 280
OBJ: 9.2.1 Apply the rules for naming and writing formulas for binary ionic compounds. | 9.3.1 Apply
the rules for naming and writing formulas for binary molecular compounds.
BLM: comprehension
32. ANS: B
PTS: 1
DIF: L2
REF: p. 280
OBJ: 9.3.1 Apply the rules for naming and writing formulas for binary molecular compounds.
BLM: comprehension
33. ANS: B
PTS: 1
DIF: L2
REF: p. 281
OBJ: 9.3.1 Apply the rules for naming and writing formulas for binary molecular compounds.
BLM: comprehension
34. ANS: C
PTS: 1
DIF: L2
REF: p. 280
OBJ: 9.3.1 Apply the rules for naming and writing formulas for binary molecular compounds.
BLM: application
35. ANS: C
PTS: 1
DIF: L1
REF: p. 285
OBJ: 9.4.1 Determine the name and formula of an acid.
BLM: knowledge
36. ANS: A
PTS: 1
DIF: L2
REF: p. 286
OBJ: 9.4.1 Determine the name and formula of an acid.
BLM: comprehension
37. ANS: C
PTS: 1
DIF: L2
REF: p. 286 | p. 287
OBJ: 9.4.1 Determine the name and formula of an acid.
BLM: application
38. ANS: D
PTS: 1
DIF: L2
REF: p. 286 | p. 287
OBJ: 9.4.1 Determine the name and formula of an acid.
BLM: application
39. ANS: B
PTS: 1
DIF: L2
REF: p. 286 | p. 287
OBJ: 9.4.1 Determine the name and formula of an acid.
BLM: application
40. ANS: B
PTS: 1
DIF: L2
REF: p. 286 | p. 287
OBJ: 9.4.1 Determine the name and formula of an acid.
BLM: application
41. ANS: D
PTS: 1
DIF: L2
REF: p. 286 | p. 287
OBJ: 9.4.1 Determine the name and formula of an acid.
BLM: application
42. ANS: B
PTS: 1
DIF: L1
REF: p. 287
OBJ: 9.4.2 Determine the name and formula of a base.
BLM: knowledge
43. ANS: C
PTS: 1
DIF: L1
REF: p. 287
OBJ: 9.4.2 Determine the name and formula of a base.
BLM: knowledge
44. ANS: D
PTS: 1
DIF: L2
REF: p. 282 | p. 283 | p. 293 | p. 294
OBJ: 9.3.1 Apply the rules for naming and writing formulas for binary molecular compounds. | 9.5.2
List the general guidelines that can help you write the name and formula of a chemical compound.
BLM: application
45. ANS: D
PTS: 1
DIF: L2
REF: p. 272 | p. 273 | p. 293 | p. 294
OBJ: 9.2.1 Apply the rules for naming and writing formulas for binary ionic compounds. | 9.5.2 List the
general guidelines that can help you write the name and formula of a chemical compound.
BLM: application
46. ANS: B
PTS: 1
DIF: L2
REF: p. 285 | p. 293
OBJ: 9.4.1 Determine the name and formula of an acid. | 9.5.2 List the general guidelines that can help
you write the name and formula of a chemical compound.
BLM: comprehension
3
ID: A
47. ANS: C
PTS: 1
DIF: L2
REF: p. 276 | p. 277 | p. 293 | p. 294
OBJ: 9.2.2 Apply the rules for naming and writing formulas for compounds with polyatomic ions. |
9.5.2 List the general guidelines that can help you write the name and formula of a chemical compound.
BLM: application
48. ANS: C
PTS: 1
DIF: L2
REF: p. 276 | p. 277 | p. 293 | p. 294
OBJ: 9.2.2 Apply the rules for naming and writing formulas for compounds with polyatomic ions. |
9.5.2 List the general guidelines that can help you write the name and formula of a chemical compound.
BLM: application
49. ANS: B
PTS: 1
DIF: L2
REF: p. 281 | p. 282 | p. 292 | p. 293
OBJ: 9.3.1 Apply the rules for naming and writing formulas for binary molecular compounds. | 9.5.2
List the general guidelines that can help you write the name and formula of a chemical compound.
BLM: application
50. ANS: B
PTS: 1
DIF: L2
REF: p. 278 | p. 279 | p. 292 | p. 293
OBJ: 9.2.2 Apply the rules for naming and writing formulas for compounds with polyatomic ions. |
9.5.2 List the general guidelines that can help you write the name and formula of a chemical compound.
BLM: application
51. ANS: D
PTS: 1
DIF: L2
REF: p. 308
OBJ: 10.1.2 Explain how chemists count the number of atoms, molecules, or formula units in a
substance.
BLM: comprehension
52. ANS: C
PTS: 1
DIF: L2
REF: p. 310
OBJ: 10.1.2 Explain how chemists count the number of atoms, molecules, or formula units in a
substance.
BLM: analysis
53. ANS: D
PTS: 1
DIF: L2
REF: p. 306 | p. 307
OBJ: 10.1.1 Convert among the count, mass, and volume of something.
BLM: analysis
54. ANS: C
PTS: 1
DIF: L2
REF: p. 308
OBJ: 10.1.2 Explain how chemists count the number of atoms, molecules, or formula units in a
substance.
BLM: analysis
55. ANS: C
PTS: 1
DIF: L2
REF: p. 308
OBJ: 10.1.2 Explain how chemists count the number of atoms, molecules, or formula units in a
substance.
BLM: comprehension
56. ANS: B
PTS: 1
DIF: L2
REF: p. 309
OBJ: 10.1.2 Explain how chemists count the number of atoms, molecules, or formula units in a
substance.
BLM: analysis
57. ANS: D
PTS: 1
DIF: L2
REF: p. 311
OBJ: 10.1.2 Explain how chemists count the number of atoms, molecules, or formula units in a
substance.
BLM: analysis
58. ANS: A
PTS: 1
DIF: L2
REF: p. 308
OBJ: 10.1.2 Explain how chemists count the number of atoms, molecules, or formula units in a
substance.
BLM: comprehension
59. ANS: B
PTS: 1
DIF: L2
REF: p. 308 | p. 310 | p. 315
OBJ: 10.1.2 Explain how chemists count the number of atoms, molecules, or formula units in a
substance. | 10.1.3 Determine the molar mass of an element and of a compound.
BLM: analysis
60. ANS: D
PTS: 1
DIF: L2
REF: p. 314 | p. 315
OBJ: 10.1.3 Determine the molar mass of an element and of a compound.
BLM: analysis
4
ID: A
61. ANS: D
PTS: 1
DIF: L2
REF: p. 315 | p. 317 | p. 318
OBJ: 10.1.3 Determine the molar mass of an element and of a compound. | 10.2.1 Describe how to
convert the mass of a substance to the number of moles of a substance, and moles to mass.
BLM: analysis
62. ANS: B
PTS: 1
DIF: L2
REF: p. 317 | p. 319
OBJ: 10.2.1 Describe how to convert the mass of a substance to the number of moles of a substance,
and moles to mass. BLM: analysis
63. ANS: C
PTS: 1
DIF: L2
REF: p. 317 | p. 323
OBJ: 10.2.1 Describe how to convert the mass of a substance to the number of moles of a substance,
and moles to mass. | 10.2.2 Convert the volume of a gas at STP to the number of moles of the gas.
BLM: comprehension
64. ANS: D
PTS: 1
DIF: L3
REF: p. 318 | p. 319
OBJ: 10.2.1 Describe how to convert the mass of a substance to the number of moles of a substance,
and moles to mass. BLM: analysis
65. ANS: A
PTS: 1
DIF: L2
REF: p. 320
OBJ: 10.2.2 Convert the volume of a gas at STP to the number of moles of the gas.
BLM: comprehension
66. ANS: A
PTS: 1
DIF: L1
REF: p. 320
OBJ: 10.2.2 Convert the volume of a gas at STP to the number of moles of the gas.
BLM: knowledge
67. ANS: B
PTS: 1
DIF: L2
REF: p. 322 | p. 323
OBJ: 10.2.2 Convert the volume of a gas at STP to the number of moles of the gas.
BLM: comprehension
68. ANS: B
PTS: 1
DIF: L2
REF: p. 320 | p. 321
OBJ: 10.2.2 Convert the volume of a gas at STP to the number of moles of the gas.
BLM: analysis
69. ANS: B
PTS: 1
DIF: L2
REF: p. 322 | p. 323
OBJ: 10.2.2 Convert the volume of a gas at STP to the number of moles of the gas.
BLM: analysis
70. ANS: A
PTS: 1
DIF: L3
REF: p. 320 | p. 321
OBJ: 10.2.2 Convert the volume of a gas at STP to the number of moles of the gas.
BLM: analysis
71. ANS: D
PTS: 1
DIF: L2
REF: p. 320 | p. 321
OBJ: 10.2.2 Convert the volume of a gas at STP to the number of moles of the gas.
BLM: application
72. ANS: B
PTS: 1
DIF: L2
REF: p. 330 | p. 331
OBJ: 10.3.1 Calculate the percent by mass of an element in a compound.
BLM: comprehension
73. ANS: C
PTS: 1
DIF: L2
REF: p. 327
OBJ: 10.3.1 Calculate the percent by mass of an element in a compound.
BLM: comprehension
74. ANS: C
PTS: 1
DIF: L2
REF: p. 326
OBJ: 10.3.1 Calculate the percent by mass of an element in a compound.
BLM: analysis
75. ANS: A
PTS: 1
DIF: L1
REF: p. 330
OBJ: 10.3.2 Calculate the empirical formula of a compound.
BLM: knowledge
5
ID: A
76. ANS:
OBJ:
BLM:
77. ANS:
OBJ:
BLM:
78. ANS:
OBJ:
BLM:
79. ANS:
OBJ:
BLM:
80. ANS:
OBJ:
BLM:
B
PTS: 1
DIF: L2
REF:
10.3.2 Calculate the empirical formula of a compound.
application
B
PTS: 1
DIF: L2
REF:
10.3.2 Calculate the empirical formula of a compound.
application
C
PTS: 1
DIF: L2
REF:
10.3.2 Calculate the empirical formula of a compound.
analysis
C
PTS: 1
DIF: L2
REF:
10.3.2 Calculate the empirical formula of a compound.
analysis
B
PTS: 1
DIF: L2
REF:
10.3.3 Distinguish between empirical and molecular formulas.
application
6
p. 330
p. 330
p. 330 | p. 331
p. 330 | p. 331
p. 332 | p. 333