Name _______________________________ Date __________________
SOL Ch.2
1.
The atomic mass of each element
is based on the relative mass of
which element?
A
B
C
D
oxygen - 16
hydrogen - 1
carbon - 12
nitrogen - 14
2.
4.
The elements: B, Si, As, and Te
would be best classified as:
H
He
Li
Be
B
C
N
O
F
Ne
Na
Mg
Al
Si
P
S
Cl
Ar
K
Ca
Ga
Ge
As
Se
Br
Kr
Rb
Ba
Te
I
Xe
Sc
Zn
Which is a subatomic but NOT a
nuclear particle?
A
B
C
D
electron
element
neutron
proton
3.
Rutherford designed an
experiment in which he shot a
beam of alpha particles through
some gold foil, see below.
gold foil
deflected
particle
A
B
C
D
nonmetals.
metals.
semi-metals or metalloids.
transition metals.
5.
The atomic number of carbon is
6. For the element carbon, the
atomic number of a neutral atom
always equals:
A
B
C
D
the number of protons.
the number of electrons.
the atomic mass.
both A and B.
6.
Which of the following is a
chemical property?
A
B
C
D
boiling point
ability to bond with another element
solubility
melting point
beam of alpha
particles
deflected
particle
atom
deflected
particle
nucleus of
atom
What did his results show?
A
B
C
D
Gold is porous.
Electrons are negatively charged.
Atoms contain a dense nucleus.
Atoms have a positive charge.
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SOL Ch.2
7.
Study the following section of a
table showing the periodicity of
atomic radii. What trends can be
deduced about atomic radii?
K
Ca
0.174
4 0.203
1+
0.133
0.144
2+
0.099
Rb
5 0.216
Cs
Ba
0.135
B
C
D
6+
0.052
Nb
Mo
0.134
0.129
5+
A
B
C
D
D
0.134
W
0.130
5+
0.068
6+
0.068
They decrease within each period
(series) and increase across
periods.
They increase within each period
(series) and decrease across
periods.
They decrease within each period
(series) and decrease across
periods.
They decrease within each period
(series) and decrease across
periods.
How many sublevels would there
be in an energy level with a
principal quantum number of 2?
1
2
3
4
B
6+
10. The atomic mass is derived from
the combined mass of the:
A
B
C
D
neutrons, protons, and electrons.
the protons and electrons.
the protons and neutrons.
the neutrons and electrons.
11. Which is true about electrons
and protons?
A
B
C
D
8.
C
0.062
Ta
4+
0.084
A
5+
Hf
3+
0.115
0.04
0.069
0.144
0.169
0.117
4+
0.087
La
2+
1+
A
3+
Of the following atomic models
pictured below, which one is
most accepted today?
Cr
0.122
Zr
0.145
0.093
0.198
0.169
Y
2+
V
4+
0.064
0.162
0.113
6 0.235
3+
Sr
1+
Ti
0.132
0.081
0.192
0.148
Sc
9.
They have similar masses.
They are both nuclear particles.
They are combined to form atomic
mass.
Their opposite charges cause them
to be attracted each other.
12. Which of the following elements
belong to the noble-gas family
(group)?
A
B
C
D
oxygen, nitrogen, hydrogen
fluorine, chlorine, bromine
neon, argon, krypton
xenon, oxygen, hydrogen
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SOL Ch.2
13. Each element in a period (series)
has one more _______ than the
element before it.
A
B
C
D
neutron
proton
nucleus
oxidation number
16. A student measured the mass of
a strip of magnesium ribbon as
2.3 g. She heated the magnesium
at a very high temperature, then
weighed the sample again. This
time she measured the sample to
be 2.8 g. She also noticed a white
powder on the metal. The
reaction was:
14. Electronegativity involves the
difference in attraction of atoms
for electrons in a bond. Which of
the following bond pairs would
have the greatest
electronegativity difference?
A
B
C
D
A
B
C
D
17. Study the diagram of the
hydrogen spectrum below. Such
bright-line emission spectra are
evidence that electrons:
F-CI
Cl-Cl
Mg-Cl
H-Mg
a chemical change.
a physical change.
a decomposition reaction.
an error of the student.
Violet
410.1 nm
15. What is the oxidation number for
the polyatomic ion in this
compound?
Red
656.2 nm
Blue-violet Green
434.0 nm
486.1 nm
KMnO4
400
A
B
C
D
+1
–1
+4
–4
450
500
550
Hydrogen Spectrum
A
B
C
D
600
650 700
nm
are in constant motion.
have a great deal of energy.
accept and give up only discrete
packets of energy.
are very unstable.
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12
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SOL Ch.2
18. Consider the following entry for
magnesium taken from the
periodic table.
24.305
+2
21. J.J. Thompson used a cathoderay tube to study the effect of an
electrostatic field on a stream of
electrons. Study the diagram
below and identify the stream of
electrons.
Mg
Source of
Electricity
Plate A
Magnesium
12
I
[Ne]3s2
The number 12 represents:
A
B
C
D
the atomic mass number.
the atomic number.
the oxidation number.
the number of neutrons.
Anode (+)
III
Fluorescent screen
II
Cathode (-)
Plate B
IV
A
B
C
D
I
II
III
IV
19. The mass number is derived
from:
22. From the diagram we can
conclude that:
A
A
B
C
D
the average of all magnesium
atoms.
various isotopes of magnesium.
a random assignment of mass.
its nuclear decay.
B
C
D
20. Elements that are in the same
family (group) share the same:
A
B
C
D
atomic mass.
atomic number.
number of valence electrons.
number of neutrons.
Plate A has a negative charge and
plate B has a positive charge.
Plate A has a positive charge and
plate B has a negative charge.
Plate A and plate B have positive
charges.
Plate A and plate B have negative
charges
23. A typical period (series) on the
periodic table begins with ______
on the left and ends with _______
on the right.
A
B
C
D
metals, nonmetals
transition metals, semi-metals
nonmetals, metals
gases, solids
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SOL Ch.2
24. Consider the diagram of a single
helium atom below. (The diagram
is not to scale.) The line segement that best identifies the
atomic radius is:
C
A
A
B
C
D
–
+ n
n +
–
E
D
B
BC
AC
BD
AE
25. Which of the following electron
configurations represents an
element in an excited state?
A
B
C
D
1s22s22p53s1
1s22s22p63s2
1s22s22p6
1s22s22p63s1
26. Which of the following is NOT a
chemical change?
A
B
C
D
frying an egg
souring of milk
burning of wood
dissolving sugar in water
27. The scientist who used the
quantum theory and explained
the hydrogen spectrum using the
planetary model was:
A
B
C
D
Mendeleev.
Planck.
Rutherford.
Bohr.
28. Which electron configuration
represents Boron, atomic
number = 5?
A
B
C
D
1s22s22p1
1s22s2
1s22s22p63s1
1s22s22p63s23p64s23d3
29. Atoms of the same element
which have different mass
numbers as a result of having
different numbers of neutrons
are called:
A
B
C
D
isomers.
isotopes.
ions.
isoelectronic species.
30. Millikan measured the charge of
an electron in his:
A
B
C
D
cathode-ray tube.
plum pudding model.
oil-drop experiment.
gold foil experiment.
31. The following elements belong to
which family (group): Li, Na, K,
Rb, Cs, Fr?
A
B
C
D
halogens
alkali metals
alkaline earth metals
metalloids
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14
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SOL Ch.2
32.
One of the periodic properties
involves the amount of energy
required to remove the most loosely
held electron from the outer energy
level of the atom (in the gas phase).
This property is known as:
A
B
C
D
electronegativity.
atomic radius.
ionization energy.
ionic radius.
33. The effective distance between
the nucleus of the atom and its
valence shell, when the atom has
formed a covalent bond by the
sharing of electrons, is known
as:
A
B
C
D
shielding effect.
electronegativity.
atomic radius.
Ionization.
34. Consider the following covalent
compounds. What is the
apparent charge on nitrogen in
the compound dinitrogen
trioxide?
A
B
C
D
Formula
Name
N2O
NO
N2O3
NO2
N2O5
dinitrogen monoxide
nitrogen monoxide
dinitrogen trioxide
nitrogen dioxide
dinitrogen pentoxide
35. Which of the physical properties
would NOT be considered an
intensive property?
A
B
C
D
density
volume
melting point
specific gravity
36. What is the name of the theory
that energy is absorbed or
radiated in definite or discrete
units?
A
B
C
D
quantum mechanics
relativity
energy polarization
conservation of energy
37. Which of the following is the best
approximation of the mass of an
electron?
A
B
C
D
9.07 x 10 -28 g
1.00 g
4.2 g
1.0 amu
38. The modern standard for atomic
mass is based on the mass of a
certain isotope of carbon. Which
is it?
A
B
C
D
carbon-10
carbon-14
carbon-12
carbon-6
+1
+2
+3
+4
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15
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SOL Ch.2
39. Which experiment was helpful in
determining the charge of a
proton?
43. The atom’s energy changes
when it gains an extra electron is
known as:
A
B
C
D
A
B
C
D
cathode-ray tube
oil drop
gold foil
fractional distillation
40. Originally, Mendeleev arranged
the families (columns) in the
periodic table according to:
A
B
C
D
alphabetic order.
atomic number.
atomic mass.
similar properties.
41. Why did Mendeleev's original
arrangement of the periodic table
NOT work perfectly in describing
the properties of the elements?
A
B
C
D
He should have used atomic mass
instead.
He should have used atomic
number instead.
He should have used the number of
neutrons in each atom instead.
He put the noble gasses in the
wrong position in his table.
42. Each period (series) in the
periodic table ends with:
A
B
C
D
alkali metals.
semi-metals.
halogens.
noble gases.
electronegativity.
electron affinity.
ionization energy.
atomic radius.
44. Regarding the configuration of
electrons, there is a rule that the
more we know about the location
of an electron, the less we can
know about its velocity (and vice
versa). This rule is known as:
A
B
C
D
the uncertainty principle.
the theory of relativity.
quantum mechanics.
the Pauli exclusion principle.
45. Which property cannot be
observed without the production
of new substances?
A
B
C
D
Chemical
Physical
Intensive
Extensive
46. Niels Bohr’s atomic model was
different from the charge cloud
because it showed:
A
B
C
D
the paths of electrons.
the exact location of electrons.
electron configurations.
that electrons have no mass.
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SOL Ch.2
47. An atom with 3 neutrons, 2
protons, and 2 electrons would
have the mass of:
A
B
C
D
52. Rutherford’s alpha-particle
experiment, pictured below,
helped support what idea about
electrons?
2 amu.
5 amu.
7 amu.
4 amu.
48. The following are all examples of
what?
beam of alpha particles
radioactive
substance
baryons, mesons, leptons,
omegas, and quarks
circular ZnS-coated
fluorescent screen
gold foil
A
B
C
D
elements
constants
subatomic particles
families (groups) on the periodic
table
49. In its "normal" state, an atom is:
A
B
C
D
electrically positive.
electrically neutral.
electrically negative.
excited.
50. Which of the following is
considered a transition metal?
A
B
C
D
magnesium
titanium
sodium
gold
51. Which of the following is NOT a
physical change?
A
B
C
D
melting wax
burning a peanut
dissolving NaCl in water
condensation
A
B
C
D
Electrons have mass.
Electrons have a negative charge.
The charge of an electron is 1.
atoms have a dense nucleus.
53. If the nucleus of a atom were the
size of a dime, the entire atom
would be the size of a:
A
B
C
D
pea.
basketball.
house.
football stadium.
54. Aluminum is a:
A
B
C
D
metal.
nonmetal.
metalloid.
noble gas.
Use this diagram of an atom to answer
the next seven questions.
M
L
K
11p
12n
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17
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SOL Ch.2
55. What is the atomic mass of this
element?
A
B
C
D
11 amu
12 amu
23 amu
22 amu
56. Removing one electron from this
atom would:
A
B
C
D
lower the atomic mass.
produce a negative charge.
produce a positive charge.
change the identity of the atom.
57. Adding an additional neutron to
this atom would:
A
B
C
D
change the electrical charge of the
atom.
change the atomic number of the
atom.
change the atomic mass of the
atom.
have no real effect on the atom.
60. The fact that the M-level electron
is held less tightly by the nucleus
than the other electrons is a
result of:
A
B
C
D
shielding effect.
specific gravity.
it is a singleton.
electrostatic forces.
61. What would the oxidation
number of this atom be?
A
B
C
D
+1
+2
–2
–1
Study the following diagram to
answer the next question.
58. The overall charge of this atom
is:
A
B
C
D
59. This element would belong in
which family (group)?
A
B
C
D
A copper spiral, when lowered into
the candle flame, conducts heat away
so rapidly that the flame is cooled
below kindling temperature. As a
result, the flame is extinguished.
positive.
negative.
neutral.
There is insufficient information to
answer the question.
alkali metals
halogens
noble gases
nitrogen family (group)
62. The ability of the copper wire to
transfer heat is NOT:
A
B
C
D
a chemical property.
a physical property.
an intensive property.
a metallic property.
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SOL Ch.2
Use the diagram below to answer the
next question.
Outer Region
66. One atom has 15 protons, 16
neutrons, and 15 electrons.
Another atom has 15 protons, 17
neutrons, and 15 electrons. How
are these two atoms related?
A
B
C
Nucleus (proton)
D
They are isotopes of the same
element.
They are ions of the same element.
They are atoms of different
elements.
They are isotopes of different
elements.
63. The outer region of this atom
represents:
A
B
C
D
an electron cloud.
nuclear decay.
radioactivity.
electromagnetic radiation.
64. The smallest unit of carbon
dioxide is the:
A
B
C
D
atom.
ion.
molecule.
isotope.
65. The atomic number is:
I. the whole number nearest the
mass.
II. the number of protons in a
neutral atom.
III. The number of electrons in a
neutral atom.
IV. the number of neutrons in an
atom.
V. the number of protons and
neutrons in the nucleus of the
atom.
A
B
C
D
67. The atomic number of nickel-60
is:
A
B
C
D
28.
58.
60.
58.7.
68. The number of electrons in
nickel-60 is:
A
B
C
D
28.
31.
59.
60.
69. The number of neutrons in
nickel-60 is:
A
B
C
D
28.
30.
32.
60.
I and V
II only
I and IV
II and III
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SOL Ch.2
70. The atomic number of the
isotope of tin with 68 neutrons is:
A
B
C
D
50.
68.
82.
118.
71. The number of protons in the
isotope of tin with 68 neutrons is:
A
B
C
D
50.
68.
82.
118.
74. How many orbitals per p-energy
sublevel are there?
A
B
C
D
3
5
7
10
75. How many electrons per f-energy
sublevel are there?
A
B
C
D
3
5
7
14
72. When electrons enter orbitals of
equal energy, one electron enters
each orbital until all the orbitals
contain one electron with parallel
spins according to:
A
B
C
D
the Pauli Exclusion Principle.
Hund’s Rule of Maximum
Multiplicity.
The Heisenberg Uncertainty
Principle.
The Aufbau Principle.
73. In the notation 3p5, the number 5
represents the:
A
B
C
D
energy level.
the number of electrons in the
energy level.
the number of electrons in the
energy sublevel.
the number of electrons in the
orbital.
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