Chemistry: The Central Science, 13e (Brown et al.)
Chapter 1 Introduction: Matter and Measurement
1.1 Multiple-Choice Questions
1) What is the physical state in which matter has no specific shape but does have a specific volume?
A) gas
B) solid
C) liquid
D) salts
E) ice
2) The law of constant composition applies to ________.
A) solutions
B) heterogeneous mixtures
C) compounds
D) homogeneous mixtures
E) solids
3) A combination of sand, salt, and water is an example of a ________.
A) homogeneous mixture
B) heterogeneous mixture
C) compound
D) pure substance
E) solid
4) A small amount of salt dissolved in water is an example of a ________.
A) homogeneous mixture
B) heterogeneous mixture
C) compound
D) pure substance
E) solid
5) Which one of the following has the element name and symbol correctly matched?
A) S, sodium
B) Tn, tin
C) Fe, iron
D) N, neon
E) B, bromine
6) Which one of the following elements has a symbol that is not derived from its foreign name?
A) tin
B) aluminum
C) mercury
D) copper
E) lead
7) Which one of the following is often easily separated into its components by simple techniques such as
filtering or decanting?
A) heterogeneous mixture
B) compounds
C) homogeneous mixture
D) elements
E) solutions
8) Which states of matter are significantly compressible?
A) gases only
B) liquids only
C) solids only
D) liquids and gases
E) solids and liquids
9) For which of the following can the composition vary?
A) pure substance
B) element
C) both homogeneous and heterogeneous mixtures
D) homogeneous mixture
E) heterogeneous mixture
10) If matter is uniform throughout and cannot be separated into other substances by physical means, it is
________.
A) a compound
B) either an element or a compound
C) a homogeneous mixture
D) a heterogeneous mixture
E) an element
11) An element cannot ________.
A) be part of a heterogeneous mixture
B) be part of a homogeneous mixture
C) be separated into other substances by chemical means
D) interact with other elements to form compounds
E) be a pure substance
12) Homogeneous mixtures are also known as ________.
A) solids
B) compounds
C) elements
D) substances
E) solutions
13) The law of constant composition says ________.
A) that the composition of a compound is always the same
B) that all substances have the same composition
C) that the composition of an element is always the same
D) that the composition of a homogeneous mixture is always the same
E) that the composition of a heterogeneous mixture is always the same
14) Which of the following is an illustration of the law of constant composition?
A) Water boils at 100 °C at 1 atm pressure.
B) Water is 11% hydrogen and 89% oxygen by mass.
C) Water can be separated into other substances by a chemical process.
D) Water and salt have different boiling points.
E) Water is a compound.
15) In the following list, only ________ is not an example of a chemical reaction.
A) dissolution of a penny in nitric acid
B) the condensation of water vapor
C) a burning candle
D) the formation of polyethylene from ethylene
E) the rusting of iron
16) Gases and liquids share the property of ________.
A) compressibility
B) definite volume
C) incompressibility
D) indefinite shape
E) definite shape
17) Of the following, only ________ is a chemical reaction.
A) melting of lead
B) dissolving sugar in water
C) tarnishing of silver
D) crushing of stone
E) dropping a penny into a glass of water
18) Which one of the following is not an intensive property?
A) density
B) temperature
C) melting point
D) mass
E) boiling point
19) Which one of the following is an intensive property?
A) mass
B) temperature
C) heat content
D) volume
E) amount
20) Of the following, only ________ is an extensive property.
A) density
B) volume
C) boiling point
D) freezing point
E) temperature
21) Which of the following are chemical processes?
1. rusting of a nail
2. freezing of water
3. decomposition of water into hydrogen and oxygen gases
4. compression of oxygen gas
A) 2, 3, 4
B) 1, 3, 4
C) 1, 3
D) 1, 2
E) 1, 4
22) In the following list, only ________ is not an example of a chemical reaction.
A) burning a plastic water bottle
B) the production of hydrogen gas from water
C) the tarnishing of a copper penny
D) chopping a log into sawdust
E) charging a cellular phone
23) Of the following, ________ is the largest mass.
A) 25 kg
B) 2.5 × 10-2 mg
C) 2.5 × 1015 pg
D) 2.5 × 109 fg
E) 2.5 × 1010 ng
24) Which one of the following is the highest temperature?
A) 38 °C
B) 96 °F
C) 302 K
D) none of the above
E) the freezing point of water
25) Which of the following is (are) the lowest temperature?
A) The freezing point of water
B) 5 °C
C) 30 °F
D) 280 K
E) A and D
26) Which one of the following is true about the liter?
A) It is the SI base unit for volume.
B) It is equivalent to a cubic decimeter.
C) It is slightly smaller than a quart.
D) It contains 106 cubic centimeters.
E) It is slightly smaller than a gallon.
27) Of the objects below, ________ is the most dense.
A) an object with a volume of 2.5 L and a mass of 12.5 kg
B) an object with a volume of 139 mL and a mass of 93 g
C) an object with a volume of 0.00212 m3 and a mass of 4.22 × 104 mg
D) an object with a volume of 3.91 × 10-24 nm3 and a mass of 7.93 × 10-1 ng
E) an object with a volume of 13 dm3 and a mass of 1.29 × 103 g
28) Which calculation clearly shows a conversion between temperatures in degrees Celsius, °C, and
temperature in Kelvins, K?
A) K = °C + 273.15
B) K = 273.15 – °C
C) K = [°C – 32] / 1.8
D) K = [°C + 32] × 1.8
E) K = °C
29) You have to calculate the mass of a 30.0 mL liquid sample with density of 1.52 g/mL, but you have
forgotten the formula. Which way of reasoning would help you in finding the correct mass?
A) If 1 mL of a liquid has the mass of 1.52 g, then 30.0 mL has the mass of __________ g.
B) If 1.52 mL of a liquid has the mass of 1 g, then 30.0 mL has the mass of __________ g.
30) You have to calculate the volume of a gas sample with mass of 1.000 × 103 g and density of 1.027 g/L,
but you have forgotten the formula. Which way of reasoning would help you in finding the correct mass?
A) If 1.027 g of a gas takes up a volume of 1 L, then 1.000 × 103 g of the same gas takes up a volume of
__________.
B) If 1.027 L of gas has a mass of 1 g, then __________ L has the mass of 1.000 × 103 g.
31) Osmium has a density of 22.6 g/cm3. What volume (in cm3) would be occupied by a 21.8 g sample of
osmium?
A) 0.965
B) 1.04
C) 493
D) 2.03 × 10-3
E) 2.03 × 103
32) Iron has a density of 7.9 g/cm3. What is the mass of a cube of iron with the length of one side equal to
55.0 mm?
A) 2.1 × 104 g
B) 4.3 × 102 g
C) 1.3 × 103 g
D) 1.4 g
E) 2.3 × 10-2 g
33) Precision refers to ________.
A) how close a measured number is to other measured numbers
B) how close a measured number is to the true value
C) how close a measured number is to the calculated value
D) how close a measured number is to zero
E) how close a measured number is to infinity
34) Accuracy refers to ________.
A) how close a measured number is to zero
B) how close a measured number is to the calculated value
C) how close a measured number is to other measured numbers
D) how close a measured number is to the true value
E) how close a measured number is to infinity
35) Which of the following has the same number of significant figures as the number 1.00310?
A) 1 × 106
B) 199.791
C) 8.66
D) 5.119
E) 100
36) Acceleration due to gravity of a free–falling object is 9.8 m/s2. Express this in millimeters/millisecond2.
A) 9.8 × 10-9
B) 9.8 × 103
C) 9.8 × 10-6
D) 9.8 × 106
E) 9.8 × 10-3
37) If an object is accelerating at a rate of 25 m/s2, how long (in seconds) will it take to reach a speed of
550 m/s? (Assume an initial velocity of zero.)
A) 22
B) 1.4 × 104
C) 0.045
D) 1.2 × 104
E) 2.3 × 102
38) If an object is accelerating at a rate of 25 m/s2, how fast will it be moving (in m/s) after 1.50 min?
(Assume an initial velocity of zero.)
A) 17
B) 3.6
C) 38
D) 2.3 × 103
E) 0.060
11
39) A wooden object has a mass of 10.782 g and occupies a volume of 13.72 mL. What is the density of the
object determined to an appropriate number of significant figures?
A) 8 × 10-1 g/mL
B) 7.9 × 10-1 g/mL
C) 7.86 × 10-1 g/mL
D) 7.859 × 10-1 g/mL
E) 7.8586 × 10-1 g/mL
40) Expressing a number in scientific notation ________.
A) changes its value
B) removes ambiguity as to the significant figures
C) removes significant zeros
D) allows to increase the number’s precision
E) all of the above
41) The number with the most significant zeros is ________.
A) 0.00002510
B) 0.02500001
C) 250000001
D) 2.501 × 10-7
E) 2.5100000
42) How many significant figures should be retained in the result of the following calculation?
12.00000 × 0.9893 + 13.00335 × 0.0107
A) 2
B) 3
C) 4
D) 5
E) 6
43) In which one of the following numbers are all of the zeros significant?
A) 100.090090
B) 0.143290
C) 0.05843
D) 0.1000
E) 00.0030020
44) Which of the following is not an exact number?
A) the number of seconds in a year
B) the number of millimeters in a kilometer
C) the number of liters in a gallon
D) the number of centimeters in an inch
E) the number of grams in a kilogram
45) Round the number 0.007222 to three significant figures.
A) 0.007
B) 0.00722
C) 0.0072
D) 0.00723
E) 0.007225
46) Round the number 3456.5 to two significant figures.
A) 3400.0
B) 3400
C) 3000
D) 3500
E) 3000.0
13
47) One angstrom, symbolized Å, is 10–10 m. 1 cm3 = ________ Å3.
A) 1024
B) 10–24
C) 1030
D) 10–30
E) 10-9
1.2 Bimodal Questions
1) Solids have a ________ shape and are not appreciably ________.
A) definite, compressible
B) definite, incompressible
C) indefinite, compressible
D) indefinite, incompressible
E) sharp, convertible
2) ________ is the chemical symbol for elemental sodium.
A) S
B) W
C) So
D) Na
E) Sn
3) If matter is uniform throughout and cannot be separated into other substances by physical processes,
but can be decomposed into other substances by chemical processes, it is called a(n) ________.
A) heterogeneous mixture
B) element
C) homogeneous mixture
D) compound
E) mixture of elements
4) A separation process that depends on differing abilities of substances to form gases is called ________.
A) filtration
B) solvation
C) distillation
D) chromatography
E) All of the above are correct.
5) The initial or tentative explanation of an observation is called a(n) ________.
A) law
B) theory
C) hypothesis
D) experiment
E) test
6) A concise verbal statement or mathematical equation that summarizes a broad variety of observations
and experiences is called a(n) ________.
A) law
B) theory
C) hypothesis
D) experiment
E) test
7) The SI unit for mass is ________.
A) kilogram
B) gram
C) pound
D) troy ounce
E) none of the above
8) A one degree of temperature difference is the smallest on the ________ temperature scale.
A) Kelvin
B) Celsius
C) Fahrenheit
D) Kelvin and Celsius
E) Fahrenheit and Celsius
9) ________ is the abbreviation for the prefix mega-.
A) k
B) m
C) M
D) n
E) d
10) ________ is the abbreviation for the prefix milli-.
A) k
B) m
C) M
D) n
E) d
11) A common English set of units for expressing velocity is miles/hour. The SI unit for velocity is
________.
A) km/hr
B) km/s
C) m/hr
D) m/s
E) cm/s
12) The density of a gold nugget is 19.3 g/cm3. If the volume of the gold nugget is 0.00369 L, the mass of
the nugget is ________ g.
A) 71.2
B) 0.191
C) 19.3
D) 5.23
E) none of the above
13) The length of the side of a cube having a density of 12.6 g/ml and a mass of 7.65 g is ________ cm.
A) 3.20
B) 0.847
C) 1.02
D) 0.584
E) 1.32
14) The unit of force in the English measurement system is
s
ft lb
2
•
. The SI unit of force is the Newton,
which is ________ in base SI units.
A)
s
cm g
2
•
B)
hr
m kg
2
•
C)
s
m kg
2
•
D)
s
m g
2
•
E)
s
cm g •
15) Momentum is defined as the product of mass and velocity. The SI unit for momentum is ________.
A)
s
m kg •
B)
hr
m kg •
C)
s
m g •
D)
s
km g •
E)
hr
km kg •
16) The SI unit of temperature is ________.
A) K
B) °C
C) °F
D) t
E) T
17) The freezing point of water at 1 atm pressure is ________.
A) 0 °F
B) 0 K
C) 0 °C
D) -273 °C
E) -32 °F
18) A temperature of ________ K is the same as 63 °F.
A) 17
B) 276
C) 290
D) 29
E) 336
19) 1 nanometer = ________ picometers
A) 1000
B) 0.1
C) 0.01
D) 1
E) 10
20) 1 picometer = ________ centimeters
A) 1 × 1010
B) 1 × 10–10
C) 1 × 108
D) 1 × 10-8
E) 1 × 10–12
21) 1 kilogram = ________ milligrams
A) 1 × 10-6
B) 1,000
C) 10,000
D) 1,000,000
E) none of the above
22) “Absolute zero” refers to ________.
A) 0 Kelvin
B) 0° Fahrenheit
C) 0° Celsius
D) °C + 9/5(°F – 32)
E) 273.15 °C
23) The density (in g/cm3) of a gold nugget that has a volume of 1.68 cm3 and a mass of 32.4 g is
________.
A) 0.0519
B) 19.3
C) 54.4
D) 0.0184
E) 32.4
24) A certain liquid has a density of 2.67 g/cm3. 1340 g of this liquid would occupy a volume of
________ L.
A) 1.99 × 10-3
B) 50.2
C) 3.58
D) 35.8
E) 0.502
25) A certain liquid has a density of 2.67 g/cm3. 30.5 mL of this liquid would have a mass of ________ Kg.
A) 81.4
B) 11.4
C) 0.0875
D) 0.0814
E) 0.0114
26) Osmium has a density of 22.6 g/cm3. The mass of a block of osmium that measures 1.01 cm × 0.233 cm
× 0.648 cm is ________ g.
A) 6.75 × 10-3
B) 3.45
C) 148
D) 6.75 × 103
E) 34.5
27) 3.337 g/cm3 = ________ kg/m3
A) 3.337 × 10-9
B) 3.337 × 10-5
C) 3337
D) 0.3337
E) 333.7
28) One side of a cube measures 1.55 m. The volume of this cube is ________ cm3.
A) 2.40 × 104
B) 3.72 × 106
C) 2.40
D) 3.72
E) 155
29) The length of the side of a cube (in cm) having a volume of 44.4 L is ________.
A) 875
B) 35.4
C) 6.66
D) 66.6
E) 0.354
30) 45 m/s = ________ km/hr
A) 2.7
B) 0.045
C) 1.6 × 102
D) 2.7 × 103
E) 1.6 × 105