© 2015 pearson education, inc. clicker questions chapter 6 barbara mowery york college
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© 2015 Pearson Education, Inc.
Clicker Questions
Chapter 6
Barbara Mowery
York College
© 2015 Pearson Education, Inc.
The wavelength of a photon multiplied by its frequency equals
a. c, the speed of light.
b. h, Planck’s constant.
c. Avogadro’s Number.
d. 4.184.
© 2015 Pearson Education, Inc.
The wavelength of a photon multiplied by its frequency equals
a. c, the speed of light.
b. h, Planck’s constant.
c. Avogadro’s Number.
d. 4.184.
© 2015 Pearson Education, Inc.
The energy of a photon divided by its frequency equals
a. c, the speed of light.
b. h, Planck’s constant.
c. Avogadro’s Number.
d. 4.184.
© 2015 Pearson Education, Inc.
The energy of a photon divided by its frequency equals
a. c, the speed of light.
b. h, Planck’s constant.
c. Avogadro’s Number.
d. 4.184.
© 2015 Pearson Education, Inc.
The “rainbow of colors” produced by sunlight striking a prism is called
a. a continuous spectrum.
b. monochromatic light.
c. a line spectrum.
d. a Balmer series.
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The “rainbow of colors” produced by sunlight striking a prism is called
a. a continuous spectrum.
b. monochromatic light.
c. a line spectrum.
d. a Balmer series.
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The lowest energy state of a hydrogen atom is called its _______ state.
a. bottom
b. ground
c. fundamental
d. original
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The lowest energy state of a hydrogen atom is called its _______ state.
a. bottom
b. ground
c. fundamental
d. original
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When an electron moves from the n = 3 orbit to the n = 2 orbit of a hydrogen atom, what wavelength of light is emitted?
a. 410 nm
b. 434 nm
c. 486 nm
d. 656 nm
© 2015 Pearson Education, Inc.
When an electron moves from the n = 3 orbit to the n = 2 orbit of a hydrogen atom, what wavelength of light is emitted?
a. 410 nm
b. 434 nm
c. 486 nm
d. 656 nm
© 2015 Pearson Education, Inc.
When an electron moves from the n = 4 orbit to the n = 2 orbit of a hydrogen atom, what wavelength of light is emitted?
a. 410 nm
b. 434 nm
c. 486 nm
d. 656 nm
© 2015 Pearson Education, Inc.
When an electron moves from the n = 4 orbit to the n = 2 orbit of a hydrogen atom, what wavelength of light is emitted?
a. 410 nm
b. 434 nm
c. 486 nm
d. 656 nm
© 2015 Pearson Education, Inc.
“It is impossible to simultaneously know both the position and the momentum of an electron in an atom” is
a. Hund’s rule.
b. deBroglie’s hypothesis.
c. Pauli’s exclusion principle.
d. Heisenberg’s uncertainty principle.
© 2015 Pearson Education, Inc.
“It is impossible to simultaneously know both the position and the momentum of an electron in an atom” is
a. Hund’s rule.
b. deBroglie’s hypothesis.
c. Pauli’s exclusion principle.
d. Heisenberg’s uncertainty principle.
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“No two electrons in an atom may have the same values for all four quantum numbers” is
a. Hund’s rule.
b. deBroglie’s hypothesis.
c. Pauli’s exclusion principle.
d. Heisenberg’s uncertainty principle.
© 2015 Pearson Education, Inc.
“No two electrons in an atom may have the same values for all four quantum numbers” is
a. Hund’s rule.
b. deBroglie’s hypothesis.
c. Pauli’s exclusion principle.
d. Heisenberg’s uncertainty principle.
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The line spectrum of hydrogen includes lines at 447, 502, 587, and 668 nm. The line at ___ nm represents the most energetic transition.
a. 447 b. 502
c. 587 d. 668
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The line spectrum of hydrogen includes lines at 447, 502, 587, and 668 nm. The line at ___ nm represents the most energetic transition.
a. 447 b. 502
c. 587 d. 668
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Which sequence lists types of electromagnetic energy in order of increasing energy?
a. microwave, IR, visible, UV
b. IR, microwave, UV, visible
c. UV, visible, IR, microwave
d. visible, UV, microwave, IR
© 2015 Pearson Education, Inc.
Which sequence lists types of electromagnetic energy in order of increasing energy?
a. microwave, IR, visible, UV
b. IR, microwave, UV, visible
c. UV, visible, IR, microwave
d. visible, UV, microwave, IR
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n and l are the principal and angular momentum quantum numbers. When n = 3, the allowed values of l are
a. 1, 2, and 3.
b. 1 and 2.
c. 0, 1, 2, and 3.
d. 0, 1, and 2.
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n and l are the principal and angular momentum quantum numbers. When n = 3, the allowed values of l are
a. 1, 2, and 3.
b. 1 and 2.
c. 0, 1, 2, and 3.
d. 0, 1, and 2.
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Which set of quantum numbers correctly describes an electron in the outermost orbital of a sulfur atom?
a. n = 3, l = 2, ml = –2
b. n = 2, l = 1, ml = –1
c. n = 2, l = 0, ml = 0
d. n = 3, l = 1, ml = –1
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Which set of quantum numbers correctly describes an electron in the outermost orbital of a sulfur atom?
a. n = 3, l = 2, ml = –2
b. n = 2, l = 1, ml = –1
c. n = 2, l = 0, ml = 0
d. n = 3, l = 1, ml = –1
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Which set of values is not correct for an electron occupying a 4d orbital?
a. n = 4, l = 2, ml = 0
b. n = 4, l = 2, ml = –1/2
c. n = 3, l = 4, ml = 1
d. n = 3, l = 1, ml = 1
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Which set of values is not correct for an electron occupying a 4d orbital?
a. n = 4, l = 2, ml = 0
b. n = 4, l = 2, ml = –1/2
c. n = 3, l = 4, ml = 1
d. n = 3, l = 1, ml = 1
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The only allowed values for the spin magnetic quantum number are
a. 0 and 1.
b. 0 and +1/2.
c. +1/2 and 1.
d. +1/2 and –1/2.
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The only allowed values for the spin magnetic quantum number are
a. 0 and 1.
b. 0 and +1/2.
c. +1/2 and 1.
d. +1/2 and –1/2.
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s orbitals are shaped like
a. four-leaf clovers.
b. dumbbells.
c. spheres.
d. triangles.
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s orbitals are shaped like
a. four-leaf clovers.
b. dumbbells.
c. spheres.
d. triangles.
© 2015 Pearson Education, Inc.
p orbitals are shaped like
a. four-leaf clovers.
b. dumbbells.
c. spheres.
d. triangles.
© 2015 Pearson Education, Inc.
p orbitals are shaped like
a. four-leaf clovers.
b. dumbbells.
c. spheres.
d. triangles.
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At a node, the probability of finding an electron is ___ %.
a. 0
b. 1
c. 50
d. 100
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At a node, the probability of finding an electron is ___ %.
a. 0
b. 1
c. 50
d. 100
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The electron configuration of a carbon atom is
a. [He]2s22p6.
b. [He]2s22p4.
c. [He]2s22p2.
d. [He]2s2.
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The electron configuration of a carbon atom is
a. [He]2s22p6.
b. [He]2s22p4.
c. [He]2s22p2.
d. [He]2s2.
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The electron configuration of a germanium atom is
a. [Ar]4s24p2.
b. [Ar]4s23d104p2.
c. [Kr]4s23d104p2.
d. [Kr]4s23d104p2.
© 2015 Pearson Education, Inc.
The electron configuration of a germanium atom is
a. [Ar]4s24p2.
b. [Ar]4s23d104p2.
c. [Kr]4s23d104p2.
d. [Kr]4s23d104p2.
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The electron configuration of a copper atom is
a. [Ar]4s23d9.
b. [Ar]4s13d10.
c. [Ar]4s23d10.
d. [Ar]4s23d7.
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The electron configuration of a copper atom is
a. [Ar]4s23d9.
b. [Ar]4s13d10.
c. [Ar]4s23d10.
d. [Ar]4s23d7.
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The valence electron configuration of elements in column 6A(16) of the Periodic Table is
a. np6.
b. ns0np6.
c. ns2np4.
d. impossible to predict because each element is unique.
© 2015 Pearson Education, Inc.
The valence electron configuration of elements in column 6A(16) of the Periodic Table is
a. np6.
b. ns0np6.
c. ns2np4.
d. impossible to predict becauseeach element is unique.