Matching
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Match each item with the correct statement below. A | electronegativity | D | period | B | ionization energy | E | transition metal | C | atomic
radius | F | group |
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1
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ability of an atom to attract electrons when the atom is in a compound
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2
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vertical column in the periodic table
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3
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horizontal row in the periodic table
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4
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energy required to remove an electron from an atom
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5
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one-half the distance between the nuclei of two atoms when the atoms are
joined
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6
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type of element characterized by the presence of electrons in the d
orbital
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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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Use the following passage and table to answer the
following 2 questions
A student studying electron configurations in atoms created Table 1 in
order to summarize the various facts she learned about principal energy levels, energy sublevels, and
orbitals.
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7
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What is the maximum number of electrons that can be
contained in the third energy level?
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8
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Based on
Table 1 what is the relationship between the principal energy level number (n)
and the number of energy sublevels that the principal energy level
contains?
A | There is no clear
relationship. | B | They are the
same. | C | The number of orbitals is greater than the principal
energy level number (n). | D | The maximum number
of electrons equals 2n2 - 1 |
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9
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What element has the e- configuration
[Ne]3s23p5?
A | Chlorine | C | Sulfur | B | Neon | D | Oxygen |
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10
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An orbital that could never exist according to the quantum or
wave-mechanical description of the atom is
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11
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As you move down the periodic table from carbon through lead, atomic
radii
A | generally increase. | C | do not change. | B | generally decrease. | D | vary
unpredictably. |
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12
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A spherical electron cloud surrounding an atomic nucleus would best
represent
A | an s orbital. | C | a combination of px and py
orbitals. | B | a px orbital. | D | a combination of an s and a
px orbital. |
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13
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The atomic emission spectra of a sodium atom on Earth and of a sodium atom in
the sun would be ____.
A | the same | B | different from each other | C | the same as those of
several other elements | D | the same as each other only in the ultraviolet
range |
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14
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How does the energy of an electron change when the electron moves closer to the
nucleus?
A | It decreases. | C | It stays the same. | B | It increases. | D | It doubles. |
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15
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In the Bohr model of the atom, an electron in an orbit has a fixed ____.
A | position | C | energy | B | color | D | size |
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16
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In a row/period in the periodic table, as you move across and as the atomic
number increases, the atomic radius generally
A | decreases. | C | increases. | B | remains constant. | D | becomes
unmeasurable. |
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17
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How are the frequency and wavelength of light related?
A | They are inversely proportional to each other. | B | Frequency equals
wavelength divided by the speed of light. | C | Wavelength is determined by dividing frequency
by the speed of light. | D | They are directly proportional to each
other. |
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18
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Electrons are elevated from the ground state to the excited state by:
A | the absorption of energy | C | the release of
energy | B | the loss of mass | D | the destruction of energy |
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19
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Which of the following subshells CANNOT exist in an
atom?
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20
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If the s and p orbitals of the highest main energy level of an atom are filled
with electrons, the atom has a(n)
A | electron pair. | C | ellipsoid. | B | octet. | D | circle. |
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21
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The elements of the Noble Gas family, except for Helium, have an outer shell (s
and p) of:
A | 6 electrons | C | 2 electrons | B | 8 electrons | D | 18 electrons |
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22
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According to Bohr, electrons cannot reside at ____ in the figure above.
A | point A | C | point C | B | point B | D | point D |
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23
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Which of the following groups of atoms have the
same outermost electron configurations but with different (principal) energy
levels?
A | N, O, F, Ne | C | Ca, Ge,
Sr, In | B | S, Cl, Ar, K | D | O, S, Se,
Te |
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24
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A student drew the following electron box diagram for an atom of sodium in the
ground state.  Which of the following statements is true? A | The student’s diagram is correct. | B | The student’s
diagram is incorrect because it shows an incorrect number of electron. | C | The student’s
diagram is incorrect because the arrows that represent the electrons should have opposite
spins. | D | The student’s diagram violates the law of conservation of
mass. |
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25
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Which of the following electron configurations is most likely to result in an
element that is relatively inactive?
A | a half-filled energy sublevel | B | a filled energy sublevel | C | one empty and one
filled energy sublevel | D | a filled highest occupied principal energy
level |
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26
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What element is displayed in the above electron orbital diagram?
A | Nitrogen | C | Oxygen | B | Carbon | D | None of these |
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27
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The shape (not the size) of an electron cloud is determined by the
electron's ____.
A | energy sublevel (s, p, d, & f) | C | speed | B | diet | D | principal quantum number |
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28
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The element that has the greatest electronegativity is
A | oxygen. | C | chlorine. | B | sodium. | D | fluorine. |
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29
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Bohr's theory helped explain why
A | electrons have negative charge. | B | most of the mass of the atom is in the
nucleus. | C | excited atoms give off certain colors of light. | D | atoms combine to form
molecules. |
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30
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The atomic sublevel with the next highest energy after 4s is
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31
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The elements on the modern periodic table are organized by increasing:
A | atomic number | C | ionization energy | B | atomic mass | D | size |
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32
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Write the ground-state electron conguration of a
lead atom.
A | [Xe]
6s1 5d54f146p6 7s2 | C | [Xe] 6s1 5d10 4f14 6p3 | B | [Xe] 6s2
5d10 4f14 6p2 | D | [Xe]
6p4 4f14 5d10 |
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33
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In a given atom, how many electrons can occupy the
3d set of orbitals?
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34
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The letter designations for the first four sublevels with the number of
electrons that can be accommodated in each sublevel are
A | s:1, p:3, d:10, and f:14. | C | s:2, p:6, d:10,
and f:14. | B | s:1, p:3, d:5, and f:7. | D | s:1, p:2, d:3, and
f:4. |
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35
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When a salt such as sodium chloride is exposed to a flame, the visible light
given off is the result of:
A | ground state electrons moving to higher energy levels | C | excited electrons returning to the
ground state | B | nuclear decay | D | gamma radiation |
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36
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Which of the following is the correct orbital notation for the element oxygen
(O, atomic #8)?
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37
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What is the shape of the 3p atomic orbital?
A | sphere | C | bar | B | dumbbell | D | two perpendicular
dumbbells |
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38
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Which element is predicted to have the ground-state
electron conguration [He] 2s2?
A | beryllium | C |
boron | B | lithium | D | carbon |
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39
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Given the representation of a chlorine atom, which circle might be a chloride
ion, Cl-?
A | Circle A | C | Circle C | B | Circle B | D | Circle D |
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40
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The number of orbitals for the d sublevel is
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41
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The number of electrons in the highest energy level of the argon atom (atomic
number 18) is
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42
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In the alkaline-earth group, atoms with the smallest radii
A | are the most reactive. | C | are all gases. | B | have the largest volume. | D | have the highest ionization
energies. |
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43
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 The "up" and "down"
arrows in electron orbital notation, such as is shown here, depict: A | electrons and protons attracting each other | C | protons and neutrons in
orbitals | B | oppositely charged electrons | D | electrons with opposite spins |
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44
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Cations have a ______________ charge and are ______________ than the atoms from
which they formed.
A | positive/larger | C | negative/larger | B | negative/smaller | D | positive/smaller |
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45
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Which of the following is NOT a valid electron
configuration?
A | 1s22s22p63s23p64s1
| C |
1s22s22p62d103s23p64s2
| B | 1s22s22p63s23p64s23d5
| D |
1s22s22p63s23p6 |
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