Chapter 1 & 3 Review Worksheeet
Matching
Match each item with the correct statement below.
a. absolute zero
b. Kelvin temperature scale
c. Celsius temperature scale
d. weight
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1.
2.
3.
4.
5.
6.
7.
8.
e.
f.
g.
h.
mass
significant figure
precision
accuracy
closeness to true value
narrowness of range of measurements
known or estimated in a measurement
the quantity of matter an object contains
the lowest point on the Kelvin scale
the SI scale for temperature
the force of gravity on an object
the non-SI scale for temperature
Multiple Choice
Identify the choice that best completes the statement or answers the question.
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9. Which of the following would a chemist be most likely to study?
a. a leaf floating on water
c. a leaf being blown by the wind
b. a leaf changing color in autumn
d. a leaf being eaten by insects
10. Which of the following was a major contribution to chemistry by Antoine Lavoisier?
a. He showed that oxygen is required for material to burn.
b. He demonstrated the presence of phlogiston in air.
c. He encouraged scientists to form explanations based on philosophical arguments.
d. He developed the science of alchemy.
11. One characteristic of a scientific theory is that ____.
a. it can never be proved
c. it cannot be modified
b. it can be proved
d. it summarizes a set of observations
12. A theory is a ____.
a. proposed explanation for an observation
b. well-tested explanation for a broad set of observations
c. summary of the results of many observations
d. procedure used to test a proposed explanation
13. Which step in the scientific method requires you to use your senses to obtain information?
a. revising a hypothesis
c. making an observation
b. designing an experiment
d. stating a theory
14. The variable that is observed during an experiment is called what type of variable?
a. independent
c. controlling
b. manipulated
d. responding
15. Collaboration and communication are important in science because ____.
a. most research problems are not very complex
b. most scientists have the knowledge to solve any scientific problem
c. they increase the likelihood of a successful outcome
d. they keep scientists from having to repeat experiments
16. Which of these steps should always be followed for effective problem solving?
a. buying a larger quantity of material than estimated
b. performing metric conversions
c. developing a plan and then implementing the plan
d. using a trial-and-error approach and then evaluating
17. The step that usually comes last in solving numeric problems is ____.
a. calculate
c. evaluate
b. measure
d. analyze
____
18. The diameter of a carbon atom is 0.000 000 000 154 m. What is this number expressed in scientific notation?
a. 1.54 10 m
c. 1.54 10 m
b. 1.54 10
d. 1.54 10
m
m
____
19. The expression of 5008 km in scientific notation is ____.
a. 5.008 10 km
c. 5.008
b. 50.08 10 km
d. 5.008
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20.
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21.
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22.
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23.
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24.
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25.
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26.
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27.
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28.
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29.
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30.
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31.
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32.
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33.
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34.
10 km
10 km
The closeness of a measurement to its true value is a measure of its ____.
a. precision
c. reproducibility
b. accuracy
d. usefulness
Which of the following measurements contains two significant figures?
a. 0.004 00 L
c. 0.000 44 L
b. 0.004 04 L
d. 0.004 40 L
Which of the following measurements (of different masses) is the most accurate?
a. 3.1000 g
c. 3.122 22 g
b. 3.100 00 g
d. 3.000 000 g
Which group of measurements is the most precise? (Each group of measurements is for a different object.)
a. 2 g, 3 g, 4 g
c. 2 g, 2.5 g, 3 g
b. 2.0 g, 3.0 g, 4.0 g
d. 1 g, 3 g, 5 g
Three different people weigh a standard mass of 2.00 g on the same balance. Each person obtains a reading of 7.32 g for
the mass of the standard. These results imply that the balance that was used is ____.
a. accurate
c. accurate and precise
b. precise
d. neither accurate nor precise
Which of the following measurements is expressed to three significant figures?
a. 0.007 m
c. 7.30 10 km
b. 7077 mg
d. 0.070 mm
In the measurement 0.503 L, which digit is the estimated digit?
a. 5
b. the 0 immediately to the left of the 3
c. 3
d. the 0 to the left of the decimal point
How many significant figures are in the measurement 0.003 4 kg?
a. two
c. five
b. four
d. This cannot be determined.
How many significant figures are in the measurement 40,500 mg?
a. two
c. four
b. three
d. five
How many significant figures are in the measurement 811.40 grams?
a. two
c. four
b. three
d. five
Express the sum of 1111 km and 222 km using the correct number of significant digits.
a. 1300 km
c. 1333 km
b. 1330 km
d. 1333.0 km
Express the sum of 7.68 m and 5.0 m using the correct number of significant digits.
a. 12.68 m
c. 13 m
b. 12.7 m
d. 10 m
Express the product of 2.2 mm and 5.00 mm using the correct number of significant digits.
a. 10 mm
c. 11.0 mm
b. 11 mm
d. 11.00 mm
What is the measurement 111.009 mm rounded off to four significant digits?
a. 111 mm
c. 111.01 mm
b. 111.0 mm
d. 110 mm
What is the measurement 1042 L rounded off to two significant digits?
a. 1.0 10 L
c. 1050 L
b. 1040 L
d. 1.1 10 L
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35. When multiplying and dividing measured quantities, the number of significant figures in the result should be equal to the
number of significant figures in ____.
a. all of the measurements
b. the least and most precise measurements
c. the most precise measurement
d. the least precise measurement
36. What quantity is represented by the metric system prefix deci-?
a. 1000
c. 0.1
b. 100
d. 0.01
37. What is the metric system prefix for the quantity 0.000 001?
a. centic. kilob. decid. micro38. Which of the following units is NOT an official SI unit?
a. kilogram
c. mole
b. ampere
d. liter
39. Which of the following volumes is the smallest?
a. one microliter
c. one milliliter
b. one liter
d. one deciliter
40. What is the SI unit of mass?
a. liter
c. candela
b. joule
d. kilogram
41. What is the temperature of absolute zero measured in C?
a. –373 C
c. –173 C
b. –273 C
d. –73 C
42. Which temperature scale has no negative temperatures?
a. Celsius
c. Joule
b. Fahrenheit
d. Kelvin
43. What is the boiling point of water in kelvins?
a. 0 K
c. 273 K
b. 100 K
d. 373 K
44. Which of the following mass units is the largest?
a. 1 cg
c. 1 mg
b. 1 dg
d. 1 ng
45. The weight of an object ____.
a. is the same as its mass
c. is not affected by gravity
b. depends on its location
d. is always the same
46. What is the temperature –34 C expressed in kelvins?
a. 139 K
c. 239 K
b. 207 K
d. 339 K
47. If the temperature changes by 100 K, by how much does it change in C?
a. 0 C
c. 100 C
b. 37 C
d. 273 C
48. Chlorine boils at 239 K. What is the boiling point of chlorine expressed in degrees Celsius?
a. 93 C
c. –61 C
b. 34 C
d. –34 C
49. Which of the following equalities is NOT correct? Use the table on page 74 in your textbook to help you.
a. 100 cg = 1 g
c. 1 cm = 1 mL
b. 1000 mm = 1 m
d. 10 kg = 1 g
50. Density is found by dividing ____.
a. mass by volume
c. mass by area
b. volume by mass
d. area by mass
51. What is the density of an object having a mass of 8.0 g and a volume of 25 cm ?
a. 0.32 g/cm
c. 3.1 g/cm
b. 2.0 g/cm
d. 200 g/cm
52. If a liter of water is heated from 20 C to 50 C, what happens to its volume?
a. The volume decreases.
____
b. The volume increases.
c. The volume first increases, then decreases.
d. The volume first decreases, then increases.
53. If the temperature of a piece of steel decreases, what happens to its density?
a. The density decreases.
b. The density increases.
c. The density does not change.
d. The density first increases, then decreases.
Short Answer
54. The following length measurements were taken by students using several different measuring devices. Find the average of
the measurements. Make sure that your answer has the correct number of significant figures.
10.05 cm, 10.1 cm, 9.741 cm, 10.6 cm, 10.5 cm
55. Round off the measurement 0.003 095 5 m to three significant figures.
56. What is the sum of 2.7 g and 2.47 g expressed in the correct number of significant digits?
57. What is the sum of 6.210 L and 3 L expressed in the correct number of significant digits?
58. What is the product of the number 1000 and the measurement 0.003 57 m expressed in the correct number of significant
digits?
59. The mass of the electron is 9.109 39
10
kg. Express the mass of the electron to 1, 2, 3, and 4 significant figures.
60. Perform the following operation: 3.43 cm
figures.
5.2 cm. Make sure that your answer has the correct number of significant
61. What is the temperature 128 K expressed in degrees Celsius?
62. What is the density of an object having a mass of 4.0 g and a volume of 39.0 cubic centimeters?
63. A cube of a gold-colored metal with a volume of 59 cm has a mass of 980 g. The density of pure gold is 19.3 g/cm . Is
the metal pure gold? Show calculations to justify your answer.
Numeric Response
64. How many steps are involved in solving numeric problems?
Essay
65. Describe the rules that are used to determine the number of significant figures in the results of addition, subtraction,
multiplication, and division.
66. Explain the difference between mass and weight. Provide an example to illustrate the distinction.
67. You are given a jar containing a mixture of three different solid substances. The particles of each substance are larger than
0.5 cm in diameter. All you know about the substances is that each is a pure metal. Describe a method for determining the
identities of the metals that make up the mixture. Assume that each metal is a different color, so you can tell one from the
others.
Chapter 1 & 3 Review Worksheeet
Answer Section
MATCHING
1. ANS:
OBJ:
2. ANS:
OBJ:
3. ANS:
OBJ:
4. ANS:
OBJ:
5. ANS:
OBJ:
6. ANS:
OBJ:
7. ANS:
OBJ:
8. ANS:
OBJ:
H
3.1.2
G
3.1.2
F
3.1.3
E
3.2.1
A
3.2.1
B
3.2.1
D
3.2.2
C
3.2.2
PTS:
1
DIF:
L1
REF:
p. 64
PTS:
1
DIF:
L1
REF:
p. 64
PTS:
1
DIF:
L1
REF:
p. 66
PTS:
1
DIF:
L1
REF:
p. 76
PTS:
1
DIF:
L1
REF:
p. 77
PTS:
1
DIF:
L1
REF:
p. 77
PTS:
1
DIF:
L1
REF:
p. 76
PTS:
1
DIF:
L1
REF:
p. 76
PTS:
1
DIF:
L2
REF:
p. 7
PTS:
1
DIF:
L2
REF:
p. 20 | p. 21
PTS:
1
DIF:
L1
REF:
p. 23
PTS:
1
DIF:
L1
REF:
p. 23
PTS:
1
DIF:
L2
REF:
p. 22
PTS:
1
DIF:
L2
REF:
p. 22
PTS:
1
DIF:
L2
REF:
p. 24
PTS:
1
DIF:
L2
REF:
p. 28
PTS:
1
DIF:
L2
REF:
p. 29
PTS:
1
DIF:
L1
REF:
p. 63
PTS:
1
DIF:
L1
REF:
p. 63
PTS:
1
DIF:
L1
REF:
p. 64
PTS:
1
DIF:
L1
REF:
p. 66
PTS:
1
DIF:
L2
REF:
p. 64
PTS:
1
DIF:
L2
REF:
p. 64
PTS:
1
DIF:
L2
REF:
p. 64
PTS:
1
DIF:
L2
REF:
p. 66
MULTIPLE CHOICE
9. ANS:
OBJ:
10. ANS:
OBJ:
11. ANS:
OBJ:
12. ANS:
OBJ:
13. ANS:
OBJ:
14. ANS:
OBJ:
15. ANS:
OBJ:
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OBJ:
17. ANS:
OBJ:
18. ANS:
OBJ:
19. ANS:
OBJ:
20. ANS:
OBJ:
21. ANS:
OBJ:
22. ANS:
OBJ:
23. ANS:
OBJ:
24. ANS:
OBJ:
25. ANS:
B
1.1.1
A
1.3.1
A
1.3.2
B
1.3.2
C
1.3.2
D
1.3.2
C
1.3.3
C
1.4.1
C
1.4.2
D
3.1.1
A
3.1.1
B
3.1.2
C
3.1.2
D
3.1.2
C
3.1.2
B
3.1.2
C
OBJ:
26. ANS:
OBJ:
27. ANS:
OBJ:
28. ANS:
OBJ:
29. ANS:
OBJ:
30. ANS:
OBJ:
31. ANS:
OBJ:
32. ANS:
OBJ:
33. ANS:
OBJ:
34. ANS:
OBJ:
35. ANS:
OBJ:
36. ANS:
OBJ:
37. ANS:
OBJ:
38. ANS:
OBJ:
39. ANS:
OBJ:
40. ANS:
OBJ:
41. ANS:
OBJ:
42. ANS:
OBJ:
43. ANS:
OBJ:
44. ANS:
OBJ:
45. ANS:
OBJ:
46. ANS:
OBJ:
47. ANS:
OBJ:
48. ANS:
OBJ:
49. ANS:
OBJ:
50. ANS:
OBJ:
51. ANS:
OBJ:
52. ANS:
OBJ:
53. ANS:
OBJ:
3.1.2
C
3.1.3
A
3.1.3
B
3.1.3
D
3.1.3
C
3.1.3
B
3.1.3
B
3.1.3
B
3.1.3
A
3.1.3
D
3.1.3
C
3.2.1
D
3.2.1
D
3.2.1
A
3.2.1
D
3.2.1
B
3.2.1
D
3.2.1
D
3.2.1
B
3.2.1
B
3.2.2
C
3.2.3
C
3.2.3
D
3.2.3
D
3.3.2
A
3.4.1
A
3.4.1
B
3.4.2
B
3.4.2
PTS:
1
DIF:
L1
REF:
p. 66
PTS:
1
DIF:
L1
REF:
p. 66
PTS:
1
DIF:
L1
REF:
p. 66
PTS:
1
DIF:
L1
REF:
p. 66
PTS:
1
DIF:
L1
REF:
p. 68
PTS:
1
DIF:
L1
REF:
p. 68 | p. 70
PTS:
1
DIF:
L1
REF:
p. 68 | p. 71
PTS:
1
DIF:
L2
REF:
p. 66 | p. 68
PTS:
1
DIF:
L2
REF:
p. 66 | p. 68
PTS:
1
DIF:
L2
REF:
p. 68 | p. 71
PTS:
1
DIF:
L1
REF:
p. 74
PTS:
1
DIF:
L1
REF:
p. 74
PTS:
1
DIF:
L1
REF:
p. 73
PTS:
1
DIF:
L1
REF:
p. 74 | p. 75
PTS:
1
DIF:
L1
REF:
p. 76
PTS:
1
DIF:
L1
REF:
p. 77
PTS:
1
DIF:
L1
REF:
p. 77
PTS:
1
DIF:
L1
REF:
p. 77
PTS:
1
DIF:
L2
REF:
p. 74 | p. 76
PTS:
1
DIF:
L2
REF:
p. 76
PTS:
1
DIF:
L1
REF:
p. 77 | p. 78
PTS:
1
DIF:
L1
REF:
p. 77 | p. 78
PTS:
1
DIF:
L2
REF:
p. 77 | p. 78
PTS:
1
DIF:
L2
REF:
p. 84
PTS:
1
DIF:
L1
REF:
p. 90 | p. 91
PTS:
1
DIF:
L2
REF:
p. 90 | p. 91
PTS:
1
DIF:
L1
REF:
p. 91
PTS:
1
DIF:
L1
REF:
p. 91
SHORT ANSWER
54. ANS:
Average = (10.05 + 10.1 + 9.741 + 10.6 + 10.5) / 5 = 10.2 cm
PTS: 1
55. ANS:
0.003 10 m
DIF:
L2
REF:
p. 68 | p. 71
OBJ:
3.1.3
PTS: 1
56. ANS:
5.2 g
DIF:
L2
REF:
p. 68
OBJ:
3.1.3
PTS: 1
57. ANS:
9L
DIF:
L2
REF:
p. 63 | p. 70
OBJ:
3.1.3
PTS: 1
58. ANS:
3.57 m
DIF:
L2
REF:
p. 63 | p. 70
OBJ:
3.1.3
PTS: 1
59. ANS:
one: 9 10
DIF:
L2
REF:
p. 68 | p. 71
OBJ:
3.1.3
kg; two: 9.1
PTS: 1
DIF:
60. ANS:
3.43 cm 5.2 cm = 18 cm
10
kg; three: 9.11
L2
10
kg; four: 9.109
10
REF:
p. 63 | p. 71
OBJ:
3.1.3
REF:
p. 68 | p. 71
OBJ:
3.1.3
PTS: 1
DIF: L2
REF: p. 77 | p. 78
62. ANS:
Density = mass/volume = 4.0 g/39.0 cm = 0.10 g/cm
OBJ:
3.2.3
PTS: 1
DIF: L2
63. ANS:
No; mass/volume = 980 g/59 cm = 17 g/cm
PTS: 1
DIF: L2
61. ANS:
C = K – 273 = 128 – 273 = –145 C
PTS:
1
REF:
p. 91
OBJ:
3.4.1
DIF:
L3
REF:
p. 90 | p. 91
OBJ:
3.4.1
DIF:
L1
REF:
p. 29
OBJ:
1.4.2
kg
NUMERIC RESPONSE
64. ANS: 3
PTS:
1
ESSAY
65. ANS:
The answer of an addition or subtraction can have no more digits to the right of the decimal point than are contained in
the measurement with the least number of digits to the right of the decimal point. The answer of a multiplication or
division can have no more significant figures than the measurement having the least number of significant figures. For
multiplication and division, the position of the decimal point has nothing to do with the number of significant figures.
PTS:
1
DIF:
L3
REF:
p. 70
OBJ:
3.1.3
66. ANS:
Mass is a measure of the quantity of matter in an object. Weight is a measure of the strength of the pull of a gravitational
force (usually Earth's) on an object. The weight of an object changes, however, with the object's distance from the center
of the gravitational field it is in. The mass of a person is exactly the same whether the person is on Earth or on the moon.
The weight of that person will be much less on the moon than on Earth because the gravitational pull of the moon is much
less than that of Earth.
PTS: 1
DIF: L3
REF: p. 78
OBJ: 3.2.2
67. ANS:
Each substance is a pure metal, so they should be identifiable by determining their densities. Separate the solids by color
into three separate batches. Determine the mass of each metal using a balance. Determine the volume of each metal as
follows. Immerse each metal in a measured volume of a suitable liquid in a graduated cylinder. Measure the volume of
the liquid plus the metal. Calculate the difference between the volume of the liquid plus the metal and the liquid by itself.
To calculate the density, divide the mass of each metal by its volume. Compare the density and color of each metal to the
density and color listed in reference books.
PTS:
1
DIF:
L3
REF:
p. 90
OBJ:
3.4.1