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Chemistry
Q:
Which orbital-filling diagram represents the ground state of vanadium?
A) B) C) D)
Q:
Which orbital-filling diagram represents the ground state of oxygen?
A) B) C) D)
Q:
Which orbital-filling diagram violates Hund's rule?
A) B) C) D)
Q:
Which orbital-filling diagram violates the Pauli exclusion principle?
A) B) C) D)
Q:
Which grouping of elements, indicated by letter on the periodic table above, represents the s-block elements?
A) A
B) B
C) C
D) D
Q:
Which grouping of elements, indicated by letter on the periodic table above, represents the p-block elements?
A) A
B) B
C) C
D) D
Q:
Which grouping of elements, indicated by letter on the periodic table above, represents the d-block elements?
A) A
B) B
C) C
D) D
Q:
Which grouping of elements, indicated by letter on the periodic table above, represents the f-block elements?
A) A
B) B
C) C
D) D
Q:
Which groups of elements, indicated by letter on the periodic table, have two unpaired p electrons in their valence shell? A) A and B
B) A and C
C) B and C
D) B and D
Q:
Which group of elements, indicated by letter on the periodic table, has electrons with the ground-state valence-shell electron configuration ns2 np4? A) A
B) B
C) C
D) D
Q:
Which period of elements, indicated by letter on the periodic table, has electrons whose highest principal quantum number n is 5? A) A
B) B
C) C
D) D
Q:
Which element, indicated by letter on the periodic table above, has the ground-state electron configuration [Ar]4s2 3d2?
A) A
B) B
C) C
D) D
Q:
Which element, indicated by letter on the periodic table above, contains three f electrons?
A) A
B) B
C) C
D) D
Q:
What is the ground-state valence-shell electron configuration of the group of elements indicated by the shaded portion of the periodic table? A) ns2
B) ns2np2
C) ns2(n-1)d2
D) ns2(n-2)f2
Q:
What is the ground-state valence-shell electron configuration of the group of elements indicated by the shaded portion of the periodic table? A) ns2
B) ns2np2
C) ns2(n-1)d2
D) ns2(n-2)f2
Q:
What is the ground-state valence-shell electron configuration of the group of elements indicated by the shaded portion of the periodic table? A) ns2
B) ns2np2
C) ns2(n-1)d2
D) ns2(n-2)f2
Q:
For the fourth-shell orbital shown below, what are the principal quantum number, n, and the angular momentum quantum number, l? A) n = 4 and l = 0
B) n = 4 and l = 1
C) n = 4 and l = 2
D) n = 4 and l = 3
Q:
For the fourth-shell orbital shown below, what are the principal quantum number, n, and the angular momentum quantum number, l? A) n = 4 and l = 0
B) n = 4 and l = 1
C) n = 4 and l = 2
D) n = 4 and l = 3
Q:
For the fourth-shell orbital shown below, what are the principal quantum number, n, and the angular momentum quantum number, l? A) n = 4 and l = 0
B) n = 4 and l = 1
C) n = 4 and l = 2
D) n = 4 and l = 3
Q:
For the fourth-shell orbital shown below, what are the principal quantum number, n, and the angular momentum quantum number, l? A) n = 4 and l = 0
B) n = 4 and l = 1
C) n = 4 and l = 2
D) n = 4 and l = 3
Q:
Which of the above fourth-shell orbitals is a 4dyz orbital?
A) orbital (a)
B) orbital (b)
C) orbital (c)
D) orbital (d)
Q:
Which of the above fourth-shell orbitals is a 4dx2-y2 orbital?
A) orbital (a)
B) orbital (b)
C) orbital (c)
D) orbital (d)
Q:
Which of the above fourth-shell orbitals is a 4py orbital?
A) orbital (a)
B) orbital (b)
C) orbital (c)
D) orbital (d)
Q:
Which of the above fourth-shell orbitals is a 4pz orbital?
A) orbital (a)
B) orbital (b)
C) orbital (c)
D) orbital (d)
Q:
If wave (a) represents green light, wave (b) might represent
A) blue light.
B) red light.
C) ultraviolet radiation.
D) X-rays.
Q:
Wave (b) has the
A) higher amplitude and greater intensity than wave (a).
B) higher amplitude and weaker intensity than wave (a).
C) lower amplitude and greater intensity than wave (a).
D) lower amplitude and weaker intensity than wave (a).
Q:
Wave (b) has the
A) higher frequency and higher energy than wave (a).
B) higher frequency and lower energy than wave (a).
C) lower frequency and higher energy than wave (a).
D) lower frequency and lower energy than wave (a).
Q:
Wave (a) has the
A) longer wavelength and higher frequency than wave (b).
B) longer wavelength and lower frequency than wave (b).
C) shorter wavelength and higher frequency than wave (b).
D) shorter wavelength and lower frequency than wave (b).
Q:
Wave (a) has the
A) longer wavelength and higher energy than wave (b).
B) longer wavelength and lower energy than wave (b).
C) shorter wavelength and higher energy than wave (b).
D) shorter wavelength and lower energy than wave (b).
Q:
Which atom in each group (I and II) has the smallest atomic radius?
(I) Sr, Zr, I (II) N, P, As
A) Sr; N
B) Sr; As
C) I; N
D) I; As
Q:
Of the following, which atom has the smallest atomic radius?
A) Mg
B) S
C) Sr
D) Te
Q:
Of the following, which atom has the largest atomic radius?
A) Na
B) Cl
C) K
D) Br
Q:
A neutral sulfur atom has how many valance electrons?
A) 2
B) 4
C) 6
D) 16
Q:
The element In has how many valence electrons?
A) 1
B) 2
C) 3
D) 13
Q:
The element Mn has how many valence electrons?
A) 2
B) 5
C) 7
D) 25
Q:
Which of the following have the same number of valence electrons?
A) K, As, Br
B) B, Si, As
C) N, As, Bi
D) He, Ne, F
Q:
Which of the following have their valence electrons in the same shell?
A) K, As, Br
B) B, Si, As
C) N, As, Bi
D) He, Ne, F
Q:
List all the elements that have a ground-state configuration with five unpaired electrons in the 3d subshell.
A) Mn, Fe, Co, Cu, and Zn
B) Cr and Mn
C) Cr
D) Mn
Q:
Which have the largest number of unpaired electrons in p orbitals in their ground-state electron configurations?
A) N, P, As
B) F, Cl, Br
C) Ne, Ar, Kr
D) Te, I, Xe
Q:
How many unpaired electrons are in an atom of Co in its ground state?
A) 1
B) 2
C) 3
D) 7
Q:
Which element has the ground-state electron configuration [Xe]6s25d14f7?
A) Pt
B) Eu
C) Gd
D) Tb
Q:
What is the ground-state electron configuration of tellurium?
A) [Kr]4d105s25p4
B) [Kr]5s25p65d8
C) [Kr]5s25p4
D) [Kr]4f144d105s25p4
Q:
What is the ground-state electron configuration of Co?
A) [Ar]3d9
B) [Ar]4s13d8
C) [Ar]4s23d7
D) [Ar]4s24p64d1
Q:
What is the general valence-electron ground-state electron configuration for neutral alkaline earth metals?
A) ns1
B) ns2
C) 1s22s1
D) 1s22s2
Q:
Molybdenum has an anomalous electron configuration. Write the electron configuration of Mo using shorthand notation.
A) [Kr] 5s0 4d6
B) [Kr] 5s0 4d0 5p6
C) [Kr] 5s1 4d5
D) [Kr] 5s2 4d4
Q:
Which of the following elements would you predict to have an anomalous electron configuration?
A) Ag
B) Ce
C) Se
D) Sr
Q:
Which of the following represent electron configurations that are allowed but do not represent ground-state configurations?
(A) [Ne]3s13p5 (B) [Kr]4d125s25p3 (C) [Ar]3d104s24p2
A) only (A)
B) only (B)
C) (A) and (B)
D) (B) and (C)
Q:
The symbol [Kr] represents
A) 4s24p6.
B) 1s22s22p63s23p64s24p6.
C) 1s22s22p63s23p63d104s24p6.
D) 1s22s22p63s23p63d104s24p64d10.
Q:
Which has the highest Zeff for its valence electrons?
A) Na
B) K
C) Si
D) Cl
Q:
For a multielectron atom, a 3s orbital lies lower in energy than a 3p orbital because
A) a 3p orbital has more nodal surfaces than a 3s orbital.
B) other electrons more effectively shield electrons in the 3s orbital from the nucleus.
C) other electrons more effectively shield electrons in the 3p orbital from the nucleus.
D) there are more p orbitals than s orbitals in a given shell.
Q:
Within a given shell of a multielectron atom, the lower l for an orbital, the
A) higher the orbital energy and the higher Zeff for the electron.
B) higher the orbital energy and the lower Zeff for the electron.
C) lower the orbital energy and the higher Zeff for the electron.
D) lower the orbital energy and the lower Zeff for the electron.
Q:
Which statement is false?
A) For any atom, the 4s orbital lies lower in energy than the 5s orbital.
B) For a hydrogen atom, a 4s orbital, a 4p orbital, and a 4d orbital all have the same energy.
C) The 4s orbital lies lower in energy than the 3d orbital for atoms K, Ca, Sc, and Ti.
D) The 4s orbital lies lower in energy than the 3d orbital for Cu and Fe2+.
Q:
Which of the following represent electron configurations that violate the Pauli exclusion principle?
(A) [Ne]3s13p5 (B) [Kr]4d125s25p3 (C) [Ar]3d104s24p2
A) only (A)
B) only (B)
C) (A) and (B)
D) (B) and (C)
Q:
The first vibrational level for NaH lies at 1.154 10-20 J and the second vibrational level lies at 3.406 10-20 J. What is the frequency of the photon emitted when a molecule of NaH drops from the second vibrational level to the first vibrational level?
A) 1.742 1013 Hz
B) 3.399 1013 Hz
C) 5.140 1013 Hz
D) 6.882 1013 Hz
Q:
The absorption of a photon of wavelength 4.67 10-6 m is necessary for a CO molecule to pass from the lowest vibrational energy level to the next highest vibrational level. If this higher vibrational level has an energy of 6.41 10-20 J, what is the energy of the lowest vibrational level?h = 6.626 10-34 J sA) 1.60 10-20 JB) 2.15 10-20 JC) 3.20 10-20 JD) 4.26 10-20 J
Q:
The absorption of light of frequency 1.16 1011 Hz is required for CO molecules to go from the lowest rotational energy level to the next highest rotational energy level. Determine the energy for this transition in kJ/mol. h = 6.626 10-34 J sA) 7.69 10-23 kJ/molB) 0.0463 kJ/molC) 46.3 kJ/molD) 949 kJ/mol
Q:
Molecular vibrational energy transitions are observed in the infrared, molecular rotational transitions in the microwave, and electronic transitions in the ultraviolet-visible range. Which transitions require the most energy and which the least energy?
A) Electronic transitions require the least energy and vibrational transitions the most.
B) Rotational transitions require the least energy and electronic transitions the most.
C) Vibrational transitions require the least energy and electronic transitions the most.
D) Vibrational transitions require the least energy and rotational transitions the most.
Q:
For hydrogen, what is the wavelength of the photon emitted when an electron drops from a 4d orbital to a 2p orbital in a hydrogen atom? The Rydberg constant is 1.097 10-2 nm-1.
A) 656.3 nm
B) 486.2 nm
C) 364.6 nm
D) 2.057 10-3 nm
Q:
What is the first ionization energy for a hydrogen atom in the ground state? The Rydberg constant is
1.097 10-2 nm-1.
A) 7.27 10-36 J
B) 1.63 10-27 J
C) 2.18 10-18 J
D) 0.00823 J
Q:
The Balmer-Rydberg equation can be extended to ions with only one electron, such as He+. In that case it has the form: 1/ = Z2R(1/m2 - 1/n2), where Z is the atomic number. What is the energy of the photon required to promote an electron in He+ from a 1s orbital to a 2p orbital?A) (3/4)hcRB) 3hcRC) 4hcRD) 12hcR
Q:
For a hydrogen atom, which electronic transition would result in the emission of a photon with the highest energy?A) 2s -> 3pB) 3p -> 6dC) 4p -> 2sD) 5f -> 3d
Q:
Which of the following is true? The probability density
A) for all s orbitals is independent of direction from the nucleus.
B) for all s orbitals is independent of distance from the nucleus.
C) is independent of direction from the nucleus for 1s orbitals only.
D) is independent of distance from the nucleus for 1s orbitals only.
Q:
For a particular orbital, as one goes away from the nucleus along the z-axis, the probability density decreases to zero, then increases, and finally decreases without increasing a second time. This is consistent with a
A) 2s orbital.
B) 2pz orbital.
C) 2s or a 2pz orbital.
D) 3s orbital.
Q:
For an orbital, a node is
A) the midpoint of the orbital.
B) a surface inside which there is a 90% chance of finding the electron.
C) a surface where there is a maximum probability of finding the electron.
D) a surface where there is no chance of finding the electron.
Q:
What is the number of spherical nodes in a 4s orbital?
A) zero
B) two
C) three
D) four
Q:
Which orbitals have two nodal planes passing through the nucleus?
A) s
B) p
C) d
D) all in the third shell
Q:
Which orbitals do not have a node at the nucleus?
A) all beyond the first shell
B) all but s
C) none
D) s
Q:
An electron in a 4p orbital can have a wave function with which of the following set of quantum numbers, (n, l, ml, ms)?A) (4, 0, 0, 1/2)B) (4, 1, -1, -1/2)C) (5, 4, 1, -1/2)D) (5, 4, 4, 1/2)
Q:
Which of the following is not a valid set of quantum numbers?
A) n = 2, l = 1, ml = 0, and ms = -1/2
B) n = 2, l = 1, ml = -1, and ms = -1/2
C) n = 3, l = 0, ml = 0, and ms = 1/2
D) n = 3, l = 2, ml = 3, and ms = 1/2
Q:
If the quantum number ms had possible values 1, 2, what would be the maximum number of electrons that be placed in a single orbital?
A) one
B) two
C) three
D) four
Q:
How many electrons can a single orbital hold?
A) 2n
B) 2
C) 2l + 1
D) 8
Q:
How many orbitals are there in the seventh shell?
A) 6
B) 7
C) 21
D) 49
Q:
What are the possible values of n and ml for an electron in a 5d orbital?
A) n = 1, 2, 3, 4, or 5 and ml = 2
B) n = 1, 2, 3, 4, or 5 and ml = -2, -1, 0, +1, or +2
C) n = 5 and ml = 2
D) n = 5 and ml = -2, -1, 0, +1, or +2
Q:
The number of orbitals in a given subshell, such as the 5d subshell, is determined by the number of possible values of
A) n.
B) l.
C) ml.
D) ms.
Q:
How many h orbitals are allowed in a given shell?
A) 5
B) 6
C) 11
D) 13
Q:
The subshell designations follow the alphabet after f. What is the first shell in which an h orbital would be allowed?
A) fifth
B) sixth
C) seventh
D) eighth
Q:
How many subshells are there in the shell with n = 6?
A) 5
B) 6
C) 15
D) 36
Q:
What are the possible values of l if n = 5?
A) 5
B) 0, 1, 2, 3, or 4
C) -4, -3, -2, -1, 0, +1, +2, +3, or +4
D) -5, -4, -3, -2, -1, 0, +1, +2, +3, +4, or +5
Q:
For an electron in a given atom, the larger n, the
A) larger the average distance from the nucleus and the higher the orbital energy.
B) larger the average distance from the nucleus and the lower the orbital energy.
C) smaller the average distance from the nucleus and the higher the orbital energy.
D) smaller the average distance from the nucleus and the lower the orbital energy.
Q:
Which of the following is true?
A) The Bohr atom is the model currently accepted for electrons in atoms.
B) Electrons travel around the nucleus in circular orbits.
C) There is a 5% chance of finding an electron in an atom outside its orbital.
D) The square of the wave function gives the probability of finding the electron.