Sample Test Questions

Sample Test Questions
Chapter 1, Chemistry: Methods and Measurement
1. Name the branch of science that involves the study of matter and the changes it
undergoes.
Ans. chemistry
2. What do we call anything that has mass and occupies space?
Ans. matter
3. What is meant by the term "scientific law"?
Ans. a summary of a large amount of scientific information
4. What word means the application of scientific principles to meeting human needs?
Ans. technology
5. What is a hypothesis?
Ans. an attempt to explain an observation in a common-sense way
6. When does a hypothesis attain the status of a theory?
Ans. when sufficient experiments have been performed to confirm that the hypothesis is
correct
7. What does the prefix "centi-" mean?
Ans. 10-2 or 0.01
8. 1 microgram is equivalent to how many grams?
Ans. 1 x10-6 g
9. How many centimeters correspond to 15.68 kilometers?
Ans. 1.568 x 106 cm
10. How many pounds are represented by 764.6 mg? [Use: 1 pound = 454 g]
Ans. 1.684 x 10-3 pounds
11. A typical aspirin tablet contains 5.00 grains of pure aspirin analgesic
compound. The rest of the tablet is starch. How many aspirin tablets
can be made from 100.0 g of pure aspirin? [Use: 1.00 g = 15.4 grains]
Ans. 308
12. A patient weighs 146 pounds and is to receive a drug at a dosage of
45.0 mg per kg of body weight. The drug is supplied as a solution that
contains 25.0 mg of drug per mL of solution. How many mL of the drug
should the patient receive? [Use: 1 pound = 454 g]
Ans. 119 mL
13. If a person smokes 10.0 packs of cigarettes a week and each cigarette
contains 5.00 mg of tar, how many weeks will she have to smoke to
inhale 0.250 pounds of tar? [Use: 20 cigarettes = 1 pack and 1 pound =
454 g]
Ans. 114 weeks
14. The cost of a drug is 125 francs per gram. What is the cost in dollars
per ounce? [Use: $1 = 6.25 francs and 1 ounce = 28.4 g]
Ans. $568/ounce
15. If one atom of carbon-14 weighs 14.0 atomic mass units and one atomic
mass unit is equal to 1.66 x10-24 grams, what is the mass of 250.0
atoms of carbon-14 in grams?
Ans. 5.81 x10-21 g
16. A patient needs 0.300 g of a solid drug preparation per day. How many
10.0 mg tablets must be given to the patient per day?
Ans. 30.0 tablets
17. When the value of an experimental quantity or measurement (e.g. the
mass of a tablet) is reported, it should consist of two parts. What are they?
Ans. number and units
18. What do we call a basic quantity of mass, volume, time, etc.?
Ans. unit
19. What is defined as the difference between the true value and our
measurement of that value?
Ans. error
20. In one sentence, define the word "accuracy"
Ans. the agreement between the true value and the measured value of a
quantity
21. What do we call the degree of agreement between replicate measurements
of the same quantity?
Ans. precision
22. What do we call the degree of doubt in a single measurement?
Ans. uncertainty
23. Express the number 0.000327730 to three significant figures using
scientific notation.
Ans. 3.28 x10-4
24. How many significant figures are in the number 5.0630 x 104?
Ans. 5
25. Write the number 3,000 using scientific notation and the proper number
of significant digits.
Ans. 3 x 103
26. Write the number 0.00946 using scientific notation and the proper
number of significant digits.
Ans. 9.46 x10-3
27. Provide the answer to the following problem using scientific notation
and the proper number of significant digits:
(6.00 x10-2)(3.00 x10-4) = ?
Ans. 1.80 x 10-5
28. Provide the answer to the following problem using scientific notation
and the proper number of significant digits:
(4.3169 x104)/(2.02 x103) = ?
Ans. 2.14 x101
29. Provide the answer to the following problem using the proper number of
significant digits: 0.004 + 26.59 + 3.2 = ?
Ans. 29.8
30. What is meant by the word "mass"?
Ans. the quantity of matter in a sample measured comparing to a standard wieght
31. What instrument is used to measure the mass of an object?
Ans. a balance
32. What commonly used mass unit is approximately the same as the mass of
one hydrogen atom?
Ans. atomic mass unit
33. What experimental quantity gives the force resulting from the pull of
gravity upon an object?
Ans. weight
34. What is the basic unit of volume in the metric system?
Ans. liter
35. List four different forms of energy, other than kinetic energy or
potential energy
Ans. any four of heat, light, electrical, mechanical, chemical
36. What Fahrenheit temperature corresponds to -168.7◦C?
Ans. -271.7◦F
37. What form of energy is usually absorbed or liberated during chemical
reactions?
Ans. heat
38. In the swinging of a pendulum, what two forms of energy are constantly
being interconverted?
Ans. kinetic energy and potential energy
39. What kind of energy is stored or the result of position or composition?
Ans. potential energy
40. What do we call the experimental quantity which gives the number of
particles of a substance (or their mass) contained per unit volume?
Ans. concentration
41. The density of an object is the ratio of its _______ to its _______.
Ans. mass; volume
42. If we assume the density of blood is 1.060 g/mL, what is the mass of
6.56 pints of blood in grams? [Use: 1 L = 2.113 pints]
Ans. 3.29 x 103 g
43. A solid that had a mass of 189.6 g was found to have the following
measurements: length = 9.80 cm; width = 46.6 mm; height = 0.111 m. What
is its density in g/mL?
Ans. 0.374 g/mL
44. When a large object fell into a "full" swimming pool, it displaced 32.0
gallons of water. The density of the object is 1.65 g/mL. What is the
object's weight in pounds? Remember that any fully immersed object
displaces its own volume. [Use: 454 g = 1 pound; 1 L = 1.06 quarts]
Ans. 439 pounds
45. What is the branch of chemistry that is being applied in measuring the
concentration of an air pollutant?
A. analytical chemistry
B. biochemistry
C. inorganic chemistry
D. organic chemistry
E. physical chemistry
Ans. A
46. What do we call a statement of observed behavior for which no
exceptions have been found?
A. hypothesis
B. theory
C. law
D. model
E. result
Ans. C
47. The speed of light is 186,000 miles per second. What is its speed in
centimeters per second?
[Use: 5280 feet = 1 mile; 12 inches = 1 foot; 2.54 cm = 1 inch]
A. 3.01 x1011 cm/s
B. 3.01 x1010 cm/s
C. 6.06 x1012 cm/s
D. 3 x1011 cm/s
E. 2.99 x1010 cm/s
Ans. E
48. 1 kilometer equals how many millimeters?
A. 10-6 B. 10-3 C. 103 D. 104 E. 106
Ans. E
49. Round off 0.052018 to three significant figures.
A. 0.05
B. 0.052
C. 0.0520
D. 0.05201
E. 0.05202
Ans. C
50. Select the answer which best expresses the result of the following
calculation: 1.86 + 246.4 – 79.9208 = ?
A. 168
B. 168.3
C. 168.34
D. 168.339
E. 168.3392
Ans. B
51. The appropriate number of significant figures to be used in expressing
the result of 51.6 / 3.1416 is
A. 1 B. 2 C. 3 D. 4 E. 5
Ans. C
52. What Celsius temperature corresponds to -4.6◦F?
A. –20◦C
B. –20.3◦C
C. –23.0◦C
D. –10.9◦C
E. –68.4◦C
Ans. B
53. What Fahrenheit temperature corresponds to -40.0◦C?
A. –8◦F
B. 16.8◦F
C. –36.9◦F
D. –40.0◦F
E. –1.94◦F
Ans. D
54. What Kelvin temperature corresponds to 98.6◦F?
A. 310K
B. 310.0K
C. 31.00K
D. 132.0K
E. 199K
Ans. B
55. Which temperature scale does not use a degree sign?
A. Celsius
B. Kelvin
C. Centigrade
D. Fahrenheit
E. Absolute zero
Ans. B
56. If the density of carbon tetrachloride is 1.59 g/mL, what is the
volume, in L, of 4.21 kg of carbon tetrachloride?
A. 0.149 L
B. 0.378 L
C. 2.65 L
D. 6.69 L
E. 6690 L
Ans. C
57. What is the specific gravity of an object that weighs 13.35 g and has a volume of
25.00 mL? The density of water under the same conditions is
0.980 g/mL.
A. 1.335
B. 0.545 g/mL
C. 1.335 mL
D. 0.545
E. 0.980
Ans. D
58. T F Organic chemistry is the study of those chemical processes that
are found in living systems.
Ans. F
59. T F Hypotheses are not acceptable in the scientific method.
Ans. F
60. T F In the scientific method, a hypothesis carries more weight than a
theory.
Ans. F
61. T F Each piece of data is the individual result of a single
measurement.
Ans. T
62. T F The presence of some error is a natural consequence of any
measurement.
Ans. T
63. T F Errors which are scattered equally above and below the correct
value are called systematic errors.
Ans. F
64. T F It is possible for a set of measurements to be precise yet
inaccurate.
Ans. T
65. T F The number 0.068 has 3 significant figures.
Ans. F
66. T F The terms mass and weight are identical.
Ans. F
67. T F Mass is the force resulting from the pull of gravity upon an
object.
Ans. F
68. T F Equal masses of glass and steel at the same temperature will
generally have different heat energies.
Ans. T
69. T F Energy may be defined as the heat content of an object.
Ans. F
70. T F One Calorie is the amount of energy needed to raise the
temperature of one gram of water one degree Celsius.
Ans. T
71. T F Density and specific gravity can be expressed in the same units.
Ans. F
Chapter 2, The Composition and Structure of the Atom
1. In which state does matter have a definite shape and volume?
Ans. solid
2. In which state of matter are forces between particles least dominant?
Ans. gas
3. What kind of change does not alter the composition or identity of the
substance undergoing the change?
Ans. physical
4. Conversion of ice to liquid water or liquid water to steam is an
example of what kind of change?
Ans. physical
5. In one sentence, explain clearly what is meant by a "chemical change".
Ans. A chemical change results in different substance(s) from those
initially present.
6. What type of change is represented by the decay of a fallen tree?
Ans. chemical
7. Give an example of a chemical property of iron metal.
Ans. its tendency to form rust when exposed to the atmosphere
8. What do we call the starting and final materials in a chemical
reaction?
Ans. reactants and products
9. What type of property of matter is independent of the quantity of the
substance?
Ans. intensive
10. What word is used to describe properties of a substance that depend on
the quantity of substance? Give two examples of such properties.
Ans. extensive; mass, volume and others
11. What is meant in chemistry by the term "pure substance"?
Ans. The substance consists of only one component; it has a fixed
composition throughout.
12. What are two kinds of pure substance?
Ans. elements and compounds
13. Explain what is meant in chemistry by the word "compound".
Ans. a pure substance consisting of two or more elements chemically combined
in a definite ratio
14. What are the two classes of mixtures?
Ans. homogeneous and heterogeneous
15. Give an example of a heterogeneous mixture.
Ans. concrete, salt and pepper, smoky air and others
16. What kind of mixture is a solution of alcohol and water?
Ans. homogeneous
17. Which of the following terms are appropriate in describing an apple?
pure substance; element; compound; mixture; homogeneous; heterogeneous
Ans. mixture; heterogeneous
18. List the three primary particles found in an atom.
Ans. proton, electron, and neutron
19. What quantity does the mass number minus the atomic number represent?
Ans. number of neutrons
20. In a neutral atom, what number of particles is equal to the number of
protons?
Ans. number of electrons
21. Given that He helium has an isotope predict the number of electrons 42,
in a helium atom.
Ans. 2
22. How many neutrons are present in an atom of the isotope 3 7
Li?
Ans. 4
23. What is the value of the mass number in the isotope 53
131I?
Ans. 131
24. What is the term for atoms of the same element having different masses
due to a different number of neutrons?
Ans. isotopes
25. What is the process by which certain isotopes emit particles and
release large amounts of energy?
Ans. radioactive decay
26. What do we call electrically charged particles that result from the
gain of one or more electrons by a parent atom?
Ans. anions
27. Dalton proposed that all atoms of an element have identical properties.
Briefly, explain why this proposal is invalid.
Ans. Isotopes of an element have different properties, particularly their
mass.
28. J. J. Thomson in 1897 announced that cathode rays consisted of a stream
of _______.
Ans. electrons
29. In one sentence, state Rutherford's important contribution to our
knowledge of atomic structure.
Ans. He concluded that atoms have a small, heavy, positively charged nucleus
surrounded largely by empty space, occupied by electrons.
General, Organic, and Biochemistry, 3/e Page 9
30. A more general term for "light" is _______ _______ (two words).
Ans. electromagnetic radiation
31. What word means the study of wavelengths of light emitted and absorbed
by atoms?
Ans. spectroscopy
32. In Bohr's model of the hydrogen atom, what is an "orbit"?
Ans. An orbit is a circular path followed by the electron.
33. In Bohr's theory of the atom, what is the number n (n = 1, 2, 3, 4)
called?
Ans. quantum number
34. In one sentence, explain the meaning/consequences of Heisenberg's
Uncertainty Principle.
Ans. It is impossible to know the exact position and momentum of a particle,
such as an electron in an atom.
35. In modern atomic theory, Bohr's orbits are replaced by atomic orbitals.
What is an atomic orbital?
Ans. It is a region of space where an electron is likely to be found; or, an
electron "cloud".
36. Which state of matter has no definite shape or volume?
A. liquid B. solid C. vapor D. steam E. gas
Ans. E
37. Which of the following is NOT a physical property of matter?
A. odor
B. compressibility
C. flash point
D. melting point
E. color
Ans. C
38. What kind of change does NOT alter the composition or identity of the
substance undergoing the change?
A. molecular
B. endothermic
C. exothermic
D. physical
E. chemical
Ans. D
39. What kind of change always results in the formation of new materials?
A. molecular
B. exothermic
C. endothermic
D. physical
E. chemical
Ans. E
40. Which of the following is a chemical property?
A. flammability
B. color
C. hardness
D. odor
E. taste
Ans. A
41. Which one of the following is an example of an extensive property?
A. density
B. specific gravity
C. mass
D. hardness
E. boiling temperature
Ans. C
42. Which one of the following is an example of a pure substance?
A. ethyl alcohol
B. sugar water
C. salt and pepper
D. milk
E. sand
Ans. A
43. Air is a/an
A. element
B. compound
C. mixture
D. molecule
E. pure substance
Ans. C
44. What type of mixture is represented by a collection of salt and pepper?
A. atoms
B. molecules
C. solution
D. heterogeneous
E. homogeneous
Ans. D
45. What kind(s) of particles can be found in the nucleus of an atom?
A. protons
B. neutrons
C. electrons
D. protons and electrons
E. protons and neutrons
Ans. E
46. The total mass of the protons in any neutral atom is about _______
times the total mass of electrons in the atom.
A. 0.0005 B. 0.3 C. 1 D. 2 E. 2000
Ans. E
47. What is the quantity represented by the mass number (Z) minus the atomic
number?
A. number of atoms
B. number of neutrons
C. number of electrons
D. number of protons
E. number of particles in the nucleus
Ans. B
48. Which isotope of hydrogen has two neutrons?
A. hydrogen-1
B. hydrogen-2
C. hydrogen-3
D. deuterium
E. H2
Ans. C
49. Which of the following accounts for the fact that chlorine has an
atomic mass of 35.45 amu rather than a whole number?
A. isotopes
B. electrons
C. protons
D. radioactivity
E. isomers
Ans. A
50. Who discovered that cathode rays consist of a stream of negative
particles, electrons?
A. Crookes
B. Thomson
C. Geiger
D. Rutherford
E. Bohr
51. Who discovered the existence of the atomic nucleus?
A. Crookes
B. Thomson
C. Geiger
D. Rutherford
E. Bohr
Ans. D
52. In Rutherford &Geiger's experiment which led to the discovery of the atomic
nucleus, what type of particle or ray was fired at the gold foil
target?
A. alpha
B. beta
C. gamma
D. neutrons
E. cathode rays
Ans. A
53. Which of the following statements relating to Bohr's model of the
hydrogen atom, is incorrect?
A. The lowest energy orbit has quantum number n = 1
B. The highest energy orbits are furthest from the nucleus
C. In a transition from the n = 3 to the n = 1 level, light is emitted
D. Energy differences between energy levels can be calculated from the
wavelengths of the light absorbed or emitted
E. The greater the energy difference between two levels, the longer the
wavelength of the light absorbed or emitted
Ans. E
54. Who proposed that electrons could behave like waves, as well as like
particles?
A. Thomson
B. Rutherford
C. Bohr
D. de Broglie
E. Heisenberg
Ans. D
55. T F The term "solution" refers only to homogeneous mixtures of
liquids.
Ans. F
56. T F In the cal Calcium atom represented by the symbol , 60Ca, calcium-60, there are
40 protons, 20 neutrons and 20 electrons.
Ans. T
57. T F According to modern atomic theory, all atoms of a particular element have
identical physical properties.
Ans. F
58. T F According to modern atomic theory, an atom cannot be created, divided,
destroyed or converted to any other type of atom.
Ans. F
59. T F The atomic number of an ion tells us the number of protons that are present.
Ans. T
60. T F If an atom gains one electron, it becomes a cation.
Ans. F
61. T F The first experimentally based theory of atomic structure was
proposed by John Dalton.
Ans. T
62. T F J. J. Thomson was the first to state that an atom is mostly empty space.
Ans. F
63. T F Short wavelengths of electromagnetic radiation have more energy than long
wavelengths.
Ans. T
64. T F Rutherford was the first to use the term "orbit" to explain the fixed energy levels
of electrons.
Ans. F
65. T F Niels Bohr developed a theory which accounted for the lines in the visible
region of the hydrogen spectrum.
Ans. T