Matching
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Match each item with the correct statement below. a. | atomic
orbital | d. | ground
state | b. | aufbau principle | e. | Pauli exclusion principle | c. | electron
configuration | f. | Heisenberg
uncertainty principle | | | | |
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1.
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region of high probability of finding an electron
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2.
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lowest energy level
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3.
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tendency of electrons to enter orbitals of lowest energy first
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4.
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arrangement of electrons around atomic nucleus
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5.
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each
orbital has at most two electrons
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Multiple Choice
Identify the
letter of the choice that best completes the statement or answers the question.
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6.
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In
Bohr's model of the atom, where are the electrons and protons located? a. | The electrons
move around the protons, which are at the center of the atom. | b. | The electrons
and protons move throughout the atom. | c. | The electrons occupy fixed positions around the protons, which
are at the center of the atom. | d. | The electrons and protons are located throughout the atom, but
they are not free to move. | | |
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7.
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The
principal quantum number indicates what property of an electron? a. | position | c. | energy
level | b. | speed | d. | electron cloud shape | | | | |
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8.
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How
many energy sublevels are in the second principal energy level?
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9.
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What
is the maximum number of f orbitals in any single energy level in an atom?
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10.
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What
is the maximum number of d orbitals in a principal energy level?
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11.
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What
is the maximum number of orbitals in the p sublevel?
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12.
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What
is the maximum number of electrons in the second principal energy level?
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13.
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When
an electron moves from a lower to a higher energy level, the electron ____. a. | always doubles
its energy | b. | absorbs a continuously variable amount of
energy | c. | absorbs a quantum of energy | d. | moves closer to
the nucleus | | |
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14.
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If
the spin of one electron in an orbital is clockwise, what is the spin of the other electron in that
orbital? a. | zero | c. | counterclockwise | b. | clockwise | d. | both clockwise and counterclockwise | | | | |
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15.
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What
types of atomic orbitals are in the third principal energy level? a. | s and
p only | c. | s, p, and
d only | b. | p and d only | d. | s, p, d, and f | | | | |
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16.
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What
is the electron configuration of potassium?
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17.
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If
three electrons are available to fill three empty 2p atomic orbitals, how will the electrons
be distributed in the three orbitals? a. | one electron in each orbital | b. | two electrons in
one orbital, one in another, none in the third | c. | three in one
orbital, none in the other two | d. | Three electrons cannot fill three empty 2p atomic
orbitals. | | |
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18.
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How
many unpaired electrons are in a sulfur atom (atomic number 16)?
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19.
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Emission of light from an atom occurs when an electron ____. a. | drops from a
higher to a lower energy level | b. | jumps from a lower to a higher energy
level | c. | moves within its atomic orbital | d. | falls into the
nucleus | | |
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20.
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Which
of the following quantum leaps would be associated with the greatest energy of emitted
light? a. | n = 5 to n =
1 | c. | n = 2 to n =
5 | b. | n = 4 to n =
5 | d. | n = 5 to n =
4 | | | | |
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21.
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Which
scientist developed the quantum mechanical model of the atom? a. | Albert
Einstein | c. | Niels
Bohr | b. | Erwin
Schrodinger | d. | Ernest
Rutherford | | | | |
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Short Answer
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22.
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Give
the electron configuration for a neutral atom of chlorine.
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23.
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Give
the electron configuration for a neutral atom of selenium.
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24.
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Write
the electron configuration for chromium.
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Essay
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25.
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Describe the shapes and relative energies of the s, p, d, and f atomic
orbitals.
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26.
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Explain why the 4s sublevel fills before the 3d sublevel begins to fill
as electrons are added.
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