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***Your Practice questions must be submitted at the beginning of class before the exam and be Entirely complete for
credit. To get full extra credit over 90% of questions need to be correct (Partial credit given for anything else).
Unit 2 Practice Exam
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
____
____
1. It has been observed that when wooden splints are soaked in different metal salt solutions and then placed
in a Bunsen burner flame, they give a certain color flame. Which of the following provides an explanation of
what is taking place?
a. The metal electrons are being transferred to the methane gas. Since each metal has a
different number of electrons, this causes the flame to be a certain color.
b. The flame is the same color as the salt solution being investigated.
c. Metal electrons that are excited will emit colored light when they fall to a lower energy
level.
d. Metal electrons give off light when excited to a higher energy level.
2. A wooden splint soaked with potassium chloride solution produces a purple color when placed in the flame
of a Bunsen burner. The Bunsen burner provides the:
a. energy to move electrons in the metal ion to a higher energy level.
b. energy for combustion.
c. energy to move electrons in the metal ion to a lower energy level.
d. energy to move electrons in the nonmetal ion to a lower energy level.
3. The atomic mass unit is defined as exactly 1/12 the mass of which atom?
a.
c.
Mg
Mg
b.
C
d.
C
____
4 Which subatomic particles have a mass of about 1 atomic mass unit each?
a. electron and positron
c. neutron and positron
b. proton and neutron
d. proton and electron
____
5. How do the charge and mass of an electron compare to the charge and mass of a proton?
a. An electron has the opposite charge and a smaller mass than a proton.
b. An electron has the opposite charge and the same mass as a proton.
c. An electron has the same charge and the same mass as a proton.
d. An electron has the same charge, but a smaller mass than a proton.
____
6. What is the total number of protons contained in the nucleus of a carbon-14 atom?
a. 12
c. 6
b. 14
d. 8
____
7. Experiments performed to show the structure of atoms led scientists to make what conclusion about an
atom?
a. The positive charge is evenly distributed throughout the entire volume of the atom.
b. The volume is mainly unoccupied.
c. The mass is evenly distributed throughout the entire volume of the atom.
d. The negative charge is mainly concentrated at the nucleus of the atom.
____
8. What are the charge and mass of a proton?
a. charge of +1 and mass of 1 amu
b. charge of -1 and mass of 1 amu
c. charge of -1 and mass of 1/1836 amu
d. charge of +1 and mass of 1/1836 amu
____
9. Rutherford conducted an experiment in which he bombarded thin sheets of gold foil with alpha particles.
What were the conclusions from his experiment?
a. The atom has a large, dense negatively charged nucleus.
b. The atom has a large, dense positively charged nucleus.
c. The atom is mostly empty space and has a small, positively charged nucleus.
d. The atom is mostly empty space and has a small, negatively charged nucleus.
____ 10. Rutherford's experiment with gold foil indicated that atoms:
a. contain a negatively charged, dense center.
b. contain a positively charged, dense center.
c. usually have a uniform distribution of positive charge.
d. usually have a uniform distribution of negative charge.
____ 11. The element chlorine has an atomic number of 17. How many electrons does chlorine have?
a. 7
c. 42
b. 35
d. 17
____ 12. Which colored light would have the longest wavelength?
a. yellow
c. green
b. blue
d. red
____ 13. Which colored light would have the highest frequency?
a. red
c. yellow
b. blue
d. green
____ 14. When an electron in an atom moves from a lower energy state to a higher energy state, the electron will:
a. only release energy.
c. only absorb energy.
b. neither absorb nor release energy.
d. both absorb and release energy.
____ 15. The nucleus of which atom contains 48 neutrons?
a.
c.
Rb
b.
Ti
d.
S
Cd
____ 16. The nucleus of which atom contains 26 neutrons?
a.
c.
S
b.
____
d.
Ti
Rb
Cd
17 Which subatomic particle is found in the nucleus of all isotopes of hydrogen?
a. neutron
c. electron
b. proton
d. positron
____ 18. What is the total number of protons and neutrons in an atom of
a. 37
c. 86
b. 123
d. 49
____
19 Which atoms are isotopes of the same element?
a.
c.
Z and Z25
b.
d.
Z and Z
Z
and
Z
Z
and
Z
Rb ?
____ 20. In which two atoms do both nuclides contain the same number of neutrons?
a.
c.
Mg and Mg
Cu and Zn6
b.
C
and O
d.
Ne
and
Ar
____ 21. An atom contains 22 neutrons and 40 nucleons. What is the total number of protons in the atom?
a. 62
c. 18
b. 40
d. 22
____ 22. Which of the following is a characteristic of the strong nuclear force?
a. The strong nuclear force is always repulsive.
b. The strong nuclear force always acts between proton and electrons.
c. The strong nuclear force is very strong at large distances.
d. The strong nuclear force always acts between nucleons.
____ 23. A radioactive isotope used for human medical diagnosis should have which of the following characteristics?
a. long half-life and fast elimination from the body
b. long half-life and slow elimination from the body
c. short half-life and fast elimination from the body
d. short half-life and slow elimination from the body
____ 24. Which type of radiation is most similar to high energy X-rays?
a. neutron
c. beta
b. alpha
d. gamma
____
25 Which type of radiation has zero mass and zero charge?
a. beta
c. alpha
b. gamma
d. neutron
____ 26.
The diagram below represents radiation passing through an electric field. The arrow labeled A
most likely represents:
a. a positron.
b. gamma radiation.
c. an alpha particle.
d. an electron.
____ 27. When an alpha particle is emitted by an atom, what happens to the atomic number of the atom?
a. The atomic number will increase by 4.
c. The atomic number will decrease by 2.
b. The atomic number will increase by 2.
d. The atomic number will decrease by 4.
____ 28. Given the reaction.
C
--> N
+
e .
Which type of decay is represented by this reaction?
a. beta decay
c. gamma decay
b. alpha decay
d. neutron decay
____ 29. Given the reaction.
Ra
X is most likely which type of particle?
a. alpha
b. beta

Rn
+ X,
c. neutron
d. gamma
____ 30. Which type of radiation continues in a straight line when passed through an electric field?
a. alpha
c. proton
b. beta
d. gamma
____ 31. In a fusion reaction, reacting nuclei must collide. Why are collisions between the nuclei difficult to achieve?
a. Nuclei are oppositely charged and repel each other.
b. Nuclei are oppositely charged and attract each other.
c. Nuclei are negatively charged and repel each other.
d. Nuclei are positively charged and repel each other.
____ 32. Which reaction best illustrates the process of fusion?
a.
Ra  Rn + He
b. H + H  He
c.
d.
N
U
+ n  C
+ n 
+ H
Br
+
La
+3 n
____ 33. During a fission reaction, which type of particle is captured by a nucleus?
a. proton
c. neutron
b. deuteron
d. electron
____ 34. The diagram below represents a nuclear reaction in which a neutron bombards a heavy nucleus. Which type
of reaction does the diagram illustrate?
a. alpha decay
b. fusion
c. fission
d. beta decay
____ 35. In which reaction is mass converted to energy by the process of fission?
a. N + n
C + H
b.
____
H + H
c.
U
d.
Ra
He
+ n
Br
Rn
+
La
+3 n
+ He
37 Given the nuclear equation.
N
What does the letter X represent?
a. a beta particle
b. a triton
+X
O
+ H
c. a deuteron
d. an alpha particle
____ 38. In the reaction
Be + X
what does the letter X most likely represent?
Li + He ,
a.
H
c.
b.
e
d.
e
n
____ 39. What part of an atom is bombarded with accelerated particles to bring about artificial transmutation?
a. occupied sublevels
c. nucleus
b. valence shell
d. inner principal energy levels
____ 40. Use the data table below to determine the average atomic mass of the naturally occurring isotopes of
copper.
Atom
Atomic mass
Relative
(amu)
abundance (%)
Copper-63
62.93
69.1
Copper-65
64.93
30.9
a. 64.4 amu
b. 63.9 amu
c. 64.8 amu
d. 63.6 amu
____ 41. Which statement is true of the strong nuclear force?
a. It acts over very great distances.
b. It holds protons and neutrons together.
c. It is much weaker than gravitational forces.
d. It repels neutral charges.
____
42 If each atom of element D has 3 mass units and each atom of element E has 5 mass units, a chemical
molecule composed of one atom each of D and E has
a. 15 mass units.
c. 35 mass units.
b. 2 mass units.
d. 8 mass units.
____ 43. A certain compound is composed of elements G and H. It always has the same mass ratio of G to H because
a. all atoms have the same mass.
c. G and H have characteristic masses.
b. any excess of G or H will be destroyed.
d. G and H have identical masses.
____ 44. According to Dalton's atomic theory, atoms
a. are destroyed in chemical reactions.
b. can be divided.
c. of each element are identical in size, mass, and other properties.
d. of different elements cannot combine.
____ 45. Which of the following is NOT part of Dalton's atomic theory?
a. Atoms cannot be divided, created, or destroyed.
b. The number of protons in an atom is its atomic number.
c. In chemical reactions, atoms are combined, separated, or rearranged.
d. All matter is composed of extremely small particles called atoms.
____ 46. According to Dalton's atomic theory, atoms
a.
b.
c.
d.
of different elements combine in simple whole-number ratios to form compounds.
can be divided into protons, neutrons, and electrons.
of all elements are identical in size and mass.
can be destroyed in chemical reactions.
____ 47. Dalton's atomic theory did NOT explain the law of
a. whole-number ratios.
c. conservation of mass.
b. definite proportions.
d. conservation of energy.
____ 48. The law of definite proportions
a. contradicted Dalton's atomic theory.
b. was explained by Dalton's atomic theory.
c. replaced the law of conservation of mass.
d. assumes that atoms of all elements are identical.
____ 49. Dalton's atomic theory helped to explain the law of conservation of mass because it stated that atoms
a. could not combine.
c. all had the same mass.
b. could not be created or destroyed.
d. were invisible.
____ 50. Which concept in Dalton's atomic theory has been modified?
a. All matter is composed of atoms.
b. Atoms of different elements have different properties and masses.
c. Atoms can combine in chemical reactions.
d. Atoms cannot be divided.
____ 51. In a glass tube, electrical current passes from the negative electrode, called the ____, to the other electrode.
a. cathode
c. electron
b. anode
d. millikan
____
52 The rays produced in a cathode tube in early experiments were
a. unaffected by a magnetic field.
c. found to carry a positive charge.
b. deflected away from a negative plate.
d. striking the cathode.
____ 53. Experiments with cathode rays led to the discovery of the
a. proton.
c. neutron.
b. nucleus.
d. electron.
____54 .Millikan's experiments
a. demonstrated that the electron carried no charge.
b. demonstrated that the electron carried the smallest possible positive charge.
c. measured the charge on the electron.
d. demonstrated that the electron was massless.
____
55 The deflection of cathode rays in Thomson's experiments was evidence of the ____ nature of electrons.
a. wave
c. particle
b. charged
d. spinning
____ 56. Who discovered the nucleus by bombarding gold foil with positively charged particles and noting that some
particles were widely deflected?
a. Rutherford
c. Chadwick
b. Dalton
d. Bohr
____ 57. In Rutherford's experiments, very few positively charged particles
a. were slightly deflected as they passed through the metal.
b. were greatly deflected back from the metal.
c. passed straight through the metal.
d. combined with the metal.
____ 58. In Rutherford's experiments, positively charged particles
a. passed through a tube containing gas.
c. collided with electrons.
b. were used to bombard a cathode plate.
d. were used to bombard thin metal foil.
____ 59 .In Rutherford's experiments, most of the particles
a. bounced back.
c. were absorbed by the foil.
b. passed through the foil.
d. combined with the foil.
____60.Because most particles fired at metal foil passed straight through, Rutherford concluded that
a. atoms were mostly empty space.
c. electrons formed the nucleus.
b. atoms contained no charged particles.
d. atoms were indivisible.
____ 61 . Because a few positively charged particles bounced back from the foil, Rutherford concluded that such
particles were
a. striking electrons.
b. indivisible.
c. repelled by densely packed regions of positive charge.
d. magnetic.
____
62 Rutherford's experiments led to the discovery of the
a. electron.
c. nucleus.
b. cathode ray.
d. neutron.
____ 63. Rutherford's experimental results led him to conclude that atoms contain massive central regions that have
a. a positive charge.
c. no charge.
b. a negative charge.
d. both protons and electrons.
____ 64. Rutherford fired positively charged particles at metal foil and concluded that most of the mass of an atom
was
a. in the electrons.
c. evenly spread throughout the atom.
b. concentrated in the nucleus.
d. in rings around the atom.
____ 65. What did Rutherford conclude about the structure of the atom?
a. An atom is indivisible.
b. Electrons make up the center of an atom.
c. An atom carries a positive charge.
d. An atom contains a small, dense, positively charged central region.
____ 66. The nucleus of an atom has all of the following characteristics EXCEPT that it
a. is positively charged.
c. contains nearly all of the atom's mass.
b. is very dense.
d. contains nearly all of the atom's volume.
____
____
67 The mass of a neutron is
a. about the same as that of a proton.
b. about the same as that of an electron.
c. double that of a proton.
d. double that of an electron.
68 The nucleus of most atoms is composed of
a. tightly packed protons.
b. tightly packed neutrons.
c. tightly packed protons and neutrons.
d. loosely connected protons and electrons.
____ 68. Protons within a nucleus are attracted to each other by
a. nuclear forces.
c. their energy levels.
b. opposite charges.
d. electron repulsion.
____ 69. An atom is electrically neutral because
a. neutrons balance the protons and electrons.
b. nuclear forces stabilize the charges.
c. the numbers of protons and electrons are equal.
d. the numbers of protons and neutrons are equal.
____ 70. Isotopes of an element contain different numbers of
a. electrons.
c. neutrons.
b. protons.
d. nuclides.
____ 71. Until the early 1600s scientists theorized that if two objects were dropped, the heavier object would fall
faster. Galileo disagreed with this theory and suggested that all objects should fall at the same rate
regardless of mass. What should the scientific community have done with the suggestion made by
Galileo?
a. Use Galileo’s new theory and discard the
old theory.
b. Design a series of experiments to test
each of the theories.
c. Ignore the suggestion from Galileo since it
contradicted the old theory.
d. Find a compromise to combine the
fundamental parts of each of the
theories.
____72 Some materials give off light when struck by certain kinds of radiant energy. While studying this phenomenon in
1895, Roentgen discovered a new kind of radiation that he named X-rays. What is one
characteristic of X-rays?
.
a. X-rays are generally considered to be a
c. X-rays are a type of high-energy
type of particle radiation.
electromagnetic radiation.
b. X-rays are a type of non-ionizing
d. Unlike other forms of radiation, X-ray
radiation.
waves can be seen by the human eye
____ 73. Use the following table to answer the question
Isotope
Carbon-12
Carbon-13
Carbon-14
Mass Number
12
13
14
Carbon has three isotopes, carbon-12, carbon-13, and carbon-14. What is different about these three
isotopes?
a.
b.
The atomic number
The number of protons
c.
d.
The number of neutrons
The number of electrons
____74 .It is more difficult to remove a proton from an atom than an electron. Which of the following forces must be
overcome to remove a proton from an atom?
a. Centrifugal force
b. Electromagnetic force
c. Gravitational force
d. Strong force
____ 75. Alpha and beta particles can be given off during the radioactive decay of an unstable nucleus. Which of the
following correctly describes alpha and beta particles
a. An alpha particle has a negative charge
c. A beta particle has a negative charge and
and is heavier than the positively charged
is heavier than the positively charged
beta particle.
alpha particle
b. An alpha particle has a positive charge
d. A beta particle has a positive charge and
and is heavier than the negatively
is heavier than the negatively charged
charged beta particle.
alpha particle
____76.
Uranium (U) and thorium (Th) decay naturally through a series of steps to produce a stable isotope of lead.
The atomic number of thorium is 90. It produces protactinium (Pa) with an atomic number of 91. What is
the missing decay particle in the nuclear reaction below?
234
90 Th
a. An alpha particle
b. A beta particle
?4?
234
91 Pa
+ ?
c. A gamma ray
d. An X-ray
____ 77.
A scientist analyzes a sample of the fossilized remains of a fern leaf and determines that about 12.5 billion
atoms of carbon-14 are present. The same size sample of a living fern leaf is found to contain 50.0 billion
atoms. The half-life of carbon-14 is 5730 years. What is the approximate age of the fossilized fern?
a.
b.
1,432 years
2,865 years
c. 5,730 years
d. 11,460 years
____ 78. Elements have both physical and chemical properties that help to identify them. Some elements can be
drawn into wires and have a shiny surface. Which of the following correctly matches these two
properties to the type of property and the class of element?
a. Physical – a nonmetal
b. Physical – a metal
c. Chemical – a nonmetal
d. Chemical – a meta
____ 79. In the wave-mechanical model of the atom, orbitals are regions of the most probable locations of
a. protons
c. neutrons
b. positrons
d. electrons
____
80 Which phrase describes an atom?
a.
a positively charged electron cloud
c. a negatively charged electron cloud
surrounding a positively charged nucleus
surrounding a positively charged nucleus
b. a positively charged electron cloud
d. a negatively charged electron cloud
surrounding a negatively charged nucleus
surrounding a negatively charged nucleus
____ 81. Which total mass is the smallest?
a.
the mass of 2 electrons
b. the mass of 2 neutrons
c. the mass of 1 electron plus the mass of 1
proton
d. the mass of 1 neutron plus the mass of
1 electron
____ 82. Chlorine-37 can be represented as
a.
c.
b.
d.
____ 83. Which list of formulas represents compounds, only?
a.
c.
b.
d.
____ 84. What can be determined if only the atomic number of an atom is known?
a. the total number of neutrons in the atom, c. the total number of protons and the total
only
number of neutrons in the atom
b. the total number of protons in the atom,
only
d. the total number of protons and the total
number of electrons in the atom
____ 85. The diagram below represents the bright-line spectra of four elements and a bright-line spectrum produced
by a mixture of two of these elements.
Which
two elements are in this mixture?
a. barium and hydrogen
b. helium and hydrogen
c. barium and lithium
d. helium and lithium
____ 86. The table below gives information about the nucleus of each of four atoms.
How many different elements are represented by the nuclei in the table?
a. 1
c. 3
b. 2
d. 4
____
87 "Orbitals of equal energy are each occupied by one electron before any is occupied by a second electron,
and all electrons in singly occupied orbitals must have the same spin" is a statement of
a. the Pauli exclusion principle.
c. the quantum effect.
b. the Aufbau principle.
d. Hund's rule.
____ 88. The statement that no two electrons in the same atom can have the same four quantum numbers is
a. the Pauli exclusion principle.
c. Bohr's law.
b. Hund's rule.
d. the Aufbau principle.
____ 89. The sequence in which energy sublevels are filled is specified by
a. the Pauli exclusion principle.
c. Lyman's series.
b. the orbital rule.
d. the Aufbau principle.
____ 90. The Pauli exclusion principle states that no two electrons in the same atom can
a. occupy the same orbital.
c. have the same set of quantum numbers.
b. have the same spin quantum numbers.
d. be at the same main energy level.
____ 91. In the ground state, the 3d and 4s sublevels of the chromium atom (atomic number 24) may be represented
as
a. 3d6 4s1.
c. 3d5 4s1.
b. 3d4 4s2.
d. 4s2 3d4.
____ 92. The element with electron configuration 1s2 2s2 2p6 3s2 3p2 is
a. Mg (Z = 12).
c. S (Z = 16).
b. C (Z = 6).
d. Si (Z = 14).
____ 93. The electron configuration for the carbon atom (C) is 1s2 2s2 2p2. The atomic number of carbon is
a. 3.
c. 11.
b. 6.
d. 12.
____ 94. The electron notation for aluminum (atomic number 13) is
a. 1s2 2s2 2p3 3s2 3p3 3d1.
c. 1s2 2s2 2p6 3s2 3p1.
b. 1s2 2s2 2p6 3s2 2d1.
____
d. 1s2 2s2 2p9.
95 If the s and p sublevels of the highest main energy level of an atom are filled, how many electrons are in the
main energy level?
a. 2
c. 16
b. 8
d. 32
____ 96. If an element has an octet of electrons in its highest main energy level, there are ____ electrons in this level.
a. 2
c. 10
b. 8
d. 32
97. Use the electron configuration for nitrogen, 1s2 2s2 2p3, to state how many electrons are in each main
energy level.
98. Write the electron configuration for beryllium, atomic number 4.
99. Write the electron configuration for argon, atomic number 18.
100. Use the figure above. Which element has the following electron configuration: [Ar] 4s2 3d10 4p5?
101. Use the figure above. Which element has the following electron configuration: [Kr] 5s2 4d10 5p3?
102. Use the figure above and the symbols for the noble gases to write the electron configuration for strontium.
103. Refer to the figure above and draw the orbital diagram for calcium.
104. Refer to the figure above and draw the orbital diagram for carbon.
105. Write the electron configuration of the figure above.
106. Which of the illustrations above represents a fission reaction?
a. A
b. B
106. . In nuclear chemistry, an atom is a(n)
a. nuclide.
c. C
d. D
c. nucleus.
b. nucleon.
d. alpha particle.
107. . A nuclide is
a. an atom with a specific number of protons.
b. an atom with a specific number of neutrons.
c. an atom with a specific number of protons and neutrons.
d. a mass number divided by an atomic number.
108. A nuclide is identified by
a. the number of protons in its nucleus.
b. the number of neutrons in its nucleus.
c. the number of protons and neutrons in its nucleus.
d. None of the above
109. . A nuclide is represented by
a. the symbol of the element with a superscript indicating its mass number and a subscript
indicating its atomic number.
b. the symbol of the element with a superscript indicating its atomic number and a subscript
indicating its mass number.
c. the full name of the element with a hyphen and the mass number.
d. Both a and c
110. . What does the 4 in
represent?
a. the mass number
b. the atomic number
c. the number of protons
d. the number of neutrons
111. . What does the 101 in
a. the mass number
b. the atomic number
c. the nuclide number
d. the number of neutrons
represent?
113. What does the 218 in polonium-218 represent?
a. the mass number
b. the atomic number
c. the mass defect
d. the neutron number
114. . Mass defect is the difference between the mass of
a. a nucleus and its atom.
b. a neutron and a proton.
c. an atom and the sum of the masses of its nucleons.
d. an atom and the sum of the masses of its constituent particles.
115. The mass defect of a nuclide represents its
a. atomic mass.
b. binding energy.
c. energy of chemical reaction.
d. mass number.
116. Which of the following is the correct relationship between mass and energy?
a. E = mc2
c. E2 = mc
b. E = mc
d. E = m2c
117.
Element
name
Atomic
number
Mass number
Number of
protons
Number of
electrons
Zinc
Number of
neutrons
38
7
26
11
13
24
30
3
Physicist’s
notation