Multiple Choice
Identify the
choice that best completes the statement or answers the question.
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1.
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The sample below contains the
mass for the stable isotopes of an element. Calculate the average atomic mass
| Isotope | Mass | Percent Abundance | | Isotop 1 | 84.92 amu | 72.15% | | Isotope 2 | 86.91 amu | 27.85% | | | |
a. | 85.47
amu | c. | 85.13
amu | b. | 86.49 amu | d. | 86.21 amu |
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2.
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Which of the following would
have the greatest electronegativity?
a. | Fluorine | c. | Beryllium | b. | Sulfur | d. | Potassium |
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3.
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Name the only element that is
consider a metalloid
a. | Silicon | c. | Hydrogen | b. | Sulfur | d. | Nitrogen |
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4.
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Which of the following would
have the greatest ionization energy?
a. | Francium | c. | Helium | b. | Calcium | d. | Chlorine |
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5.
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Which of the following factors contributes to the increase in atomic size within
a group on the periodic table?
a. | more energy levels as you go down a group | b. | an increase in
number of protons | c. | an increase in size of the
nucleus | d. | fewer electrons in the highest occupied energy level |
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6.
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Which family correctly
represents the elements in Group 1 on the periodic table?
a. | Transition
metals | c. | Alkali
metals | b. | Lanthanide metals | d. | Actinide series |
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7.
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How many electrons are in a
Cd3+
ion?
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8.
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How many neutrons would  have?
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9.
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The energy that is pulling on an electron in order to share that electron with
aothern element is called the
a. | ionization energy | c. | atomic radius | b. | electron affinity | d. | electronegativity |
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10.
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What is the mass number of a
carbon isotope that has 6 protons, 6 electrons, and 8 neutrons?
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11.
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Which of the following processes does NOT involve a change in chemical
properties?
a. | burning | c. | boiling | b. | rusting | d. | fermenting |
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12.
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What is the element with the lowest electronegativity value?
a. | calcium | c. | Hydrogen | b. | cesium | d. | fluorine |
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13.
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The average atomic mass of an element depends upon the ____.
a. | mass and relative abundance of each isotope of that element | b. | mass of each isotope
of that element | c. | mass of each electron in that element | d. | relative abundance of protons in that
element |
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14.
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Which of the following is true about subatomic particles?
a. | Electrons are negatively charged and are the heaviest subatomic
particle. | b. | Protons are positively charged and the lightest subatomic
particle. | c. | The mass of a neutron equals the mass of a proton. | d. | Neutrons have no
charge and are the lightest subatomic particle. |
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15.
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How many protons does an atom
of Potassium (K) have?
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16.
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Which of the following factors contributes to the increase in ionization energy
from left to right across a period?
a. | an increase in the shielding effect | b. | fewer electrons in the highest occupied energy
level | c. | an increase in the volume of the atom | d. | an increase in the number of
protons |
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17.
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A chemical change occurs when a piece of wood ____.
a. | decays | c. | is split | b. | is cut | d. | is painted |
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18.
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As the atomic number increases
within a group of elements, the atomic radius usually--
a. | remains the
same | c. | decreases, then
increases | b. | increases | d. | decreases |
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19.
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The energy required to remove an electron from an element is called the
a. | ionization energy | c. | electron affinity | b. | atomic radius | d. | electronegativity |
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20.
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Which family of elements has
properties of both Metals and Non-metals?
a. | Metalloids | c. | Lanthanide Series | b. | Transition metals | d. | Alkaline Earth Metals |
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21.
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Helium and Hydrogen in their
gas states are less dense than air. Why is helium used to inflate balloons rather than
hydrogen?
a. | Hydrogen has a higher atomic number
than Helium | c. | Hydrogen is not a
gas | b. | Like the others in its group, helium is an unreactive
gas | d. | Hydrogen is too light and will leak out of the
balloon
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22.
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An isotope of mercury has 80
protons and 120 neutrons. What is the mass number of this isotope?
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23.
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Sodium, mercury, argon, and
neon are used in the production of lamps. There are fewer safety guidelines regarding the handling of
neon and argon than for mercury and sodium. Which of the following best describes the elements within
the group of the periodic table that contains neon and argon gas?
a. | Gaseous at room temperature and
highly reactive with metals | c. | Solid at room temperature and mostly unreactive with strong
acids | b. | Gaseous at room temperature and unreactive
| d. | Solid at room temperature and mildly reactive with strong
acids |
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