Multiple Choice
Identify the
letter of the choice that best completes the statement or answers the question.
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1.
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How
many valence electrons are in an atom of phosphorus?
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2.
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How
many valence electrons are in an atom of magnesium?
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3.
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How
many valence electrons does a helium atom have?
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4.
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How
many valence electrons are in a silicon atom?
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5.
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What
is the name given to the electrons in the highest occupied energy level of an atom? a. | orbital
electrons | c. | anions | b. | valence electrons | d. | cations | | | | |
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6.
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How
does calcium obey the octet rule when reacting to form compounds? a. | It gains
electrons. | b. | It gives up electrons. | c. | It does not
change its number of electrons. | d. | Calcium does not obey the octet rule. | | |
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7.
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What
is the maximum charge an ion is likely to have?
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8.
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What
is the electron configuration of the calcium ion?
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9.
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What
is the electron configuration of the gallium ion?
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10.
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What
is the charge on the strontium ion? a. | 2– | c. | 1 | b. | 1– | d. | 2 | | | | |
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11.
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The
octet rule states that, in chemical compounds, atoms tend to have ____. a. | the electron
configuration of a noble gas | b. | more protons than electrons | c. | eight electrons
in their principal energy level | d. | more electrons than protons | | |
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12.
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How
many electrons does barium have to give up to achieve a noble-gas electron
configuration?
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13.
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What
is the formula of the ion formed when potassium achieves noble-gas electron
configuration?
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14.
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Which
of the following elements does NOT form an ion with a charge of 1 ? a. | fluorine | c. | potassium | b. | hydrogen | d. | sodium | | | | |
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15.
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How
many electrons does nitrogen gain in order to achieve a noble-gas electron
configuration?
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16.
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What
is the formula of the ion formed when phosphorus achieves a noble-gas electron
configuration?
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17.
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How
does oxygen obey the octet rule when reacting to form compounds? a. | It gains
electrons. | b. | It gives up electrons. | c. | It does not
change its number of electrons. | d. | Oxygen does not obey the octet rule. | | |
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18.
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The
electron configuration of a fluoride ion, F , is
____. a. | | c. | | b. | the same as that of a neon atom | d. | the same as that of a potassium ion | | | | |
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19.
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What
is the electron configuration of the oxide ion (O )? a. | | c. | 1s 2s | b. | | d. | | | | | |
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20.
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What
is the electron configuration of the iodide ion?
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21.
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When
Group 2A elements form ions, they ____. a. | lose two protons | c. | lose two electrons | b. | gain two
protons | d. | gain two
electrons | | | | |
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22.
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What
is the correct name for the N ion? a. | nitrate
ion | c. | nitride
ion | b. | nitrogen
ion | d. | nitrite
ion | | | | |
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23.
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When
naming a transition metal ion that can have more than one common ionic charge, the numerical value of
the charge is indicated by a ____. a. | prefix | c. | Roman numeral following the name | b. | suffix | d. | superscript
after the name | | | | |
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24.
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Aluminum is a group 3A metal. Which ion does A1 typically form?
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25.
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The
nonmetals in Groups 6A and 7A ____. a. | lose electrons when they form ions | b. | have a numerical
charge that is found by subtracting 8 from the group number | c. | all have ions
with a –1 charge | d. | end in -ate | | |
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