37. What is the wavelength of an electron traveling at 7.59% of the speed of light?
()
A)
B)
C)
D)
E)
38. If the location of a particular electron can be measured only to a precision of 0.011 nm, what
is the minimum uncertainty in the electron’s velocity? (
)
A)
B)
C)
D)
E)
39. If the x-component of the velocity of an electron can be measured only to a precision of
, what is the minimum uncertainty of the position of the electron in the x-
direction? ( )
A)
B)
C)
D)
E)
40. Which of the following statements is a valid conclusion from the Heisenberg uncertainty
principle?
A)
The square of the wave function is proportional to the probability of finding a
particle in space.
B)
Particles can exhibit wavelike behavior.
C)
The orbits proposed by Bohr’s model of the atom are correct.
D)
An electron in a 2p orbital is always closer to the nucleus than an electron in a 3p
orbital.
E)
The act of measuring a particle’s position changes its momentum, and vice versa.
41. Which of the following statements is incorrect concerning the wave function?
A)
The wave function of a particle is a solution to the Schrödinger equation.
B)
For an electron in an atom, the square of the wave function decreases rapidly as the
distance from the nucleus increases.
C)
The square of the wave function is proportional to the probability of finding the
particle in a region of space.
D)
The value of the wave function gives the location of the particle.
E)
The wave function for an electron in an atom is called an atomic orbital.
42. The square of the wave function, 2, of an electron in an atom
A)
is inversely proportional to the distance between the electron and the nucleus.
B)
specifies the momentum of the electron.
C)
describes the energy of the electron.
D)
is proportional to the velocity of the electron.
E)
gives the probability of finding the electron in a region of space.
43. A radial probability plot for an electron in an atom, like that shown below,
A)
specifies the probable speed of the electron at a given radius from the nucleus.
B)
specifies the probable momentum of the electron at a given radius from the
nucleus.
C)
describes the probable energy of the electron at a given radius from the nucleus.
D)
gives the probability of finding one electron near another at a given radius from the
nucleus.
E)
gives the probability of finding the electron at a given radius from the nucleus.
44. The number of orbitals having a given value of l is equal to
A)
2n + 1.
B)
2l + 1.
C)
n + ml.
D)
2ml + 1.
E)
l + ml.
45. Which quantum number distinguishes the different shapes of the orbitals?
A)
n
B)
ml
C)
l
D)
ms
E)
any of these
46. The angular momentum quantum number is best associated with the
A)
shape of the orbital.
B)
number of orbitals in a subshell.
C)
energy of the orbital.
D)
orientation in space of an orbital.
E)
none of the above
47. Which of the following sets of quantum numbers (n, l, ml, ms) refers to a 3d orbital?
A)
2 1 0 +
B)
5 4 3 +
C)
4 2 1 –
D)
4 3 1 –
E)
3 2 1 –
48. What is the value of the angular momentum quantum number for an electron in a 5d orbital?
A)
0
B)
4
C)
1
D)
2
E)
3
49. A possible value of the magnetic quantum number ml for a 5p electron is
A)
1.
B)
–4.
C)
–5.
D)
6.
E)
3.
50. All the following statements about the quantum numbers are true except
A)
ml has 2l + 1 possible values.
B)
n may take integral values from 1 to .
C)
ml may take integral values of +l to –l, including zero.
D)
l may take integral values from 1 to n – 1.
E)
ms may take only the values of and .
51. How many values are there for the magnetic quantum number when the value of the angular
momentum quantum number is 4?
A)
14
B)
9
C)
1
D)
4
E)
15
52. An orbital with the quantum numbers may be found in which subshell?
A)
3f
B)
3d
C)
3p
D)
3g
E)
3s
53. What is the value of the principal quantum number for an electron in a 1s orbital?
A)
–1
B)
C)
1
D)
E)
0
54. What is the value of the spin quantum number for an electron in a 3p orbital?
A)
3
B)
1
C)
either or
D)
E)
55. Which of the following subshells does not exist?
A)
6g
B)
3f
C)
3p
D)
2s
E)
4d
56. The number of orbitals in a p subshell is
A)
3.
B)
1.
C)
7.
D)
2.
E)
5.
57. Which of the following sets of quantum numbers (n, l, ml, ms) is not permissible?
A)
3 3 –3 +
1
2
B)
2 1 –1 +
1
2
C)
1 0 0 +
1
2
D)
3 2 –2 –
E)
4 0 0 –
Test Bank General Chemistry, 10th edition 18
58. Which of the following combinations of quantum numbers is permissible?
A)
n = 1, l = 2, ml = 0, ms =
B)
n = 3, l = 2, ml = 1, ms =
C)
n = 3, l = 3, ml = 1, ms =
D)
n = 2, l = 1, ml = –1, ms = 0
E)
n = 4, l = 3, ml = 4, ms =
59. Which of the following statements is incorrect?
A)
The set of quantum numbers n = 3, l = 2, ml = 0, ms = is not permitted because
ml = 0.
B)
The set of quantum numbers n = 2, l = 2, ml = 1, ms = is not permitted because n
= l.
C)
The set of quantum numbers n = 3, l = 2, ml = 1, ms = is permitted.
D)
The set of quantum numbers n = 3, l = 2, ml = 3, ms = is not permitted because
ml exceeds l.
E)
The set of quantum numbers n = 4, l = 3, ml = –1, ms = 0 is not permitted because
ms = 0.
60. Which of the following statements is incorrect?
A)
The n = 3 shell has three p orbitals.
B)
Every p subshell has three orbital.
C)
The n = 4 shell has seven f orbitals.
D)
An s orbital has a spherical shape.
E)
The n = 2 shell has five d orbitals.
61. How many p orbitals are in the n = 4 shell?
A)
1
B)
8
C)
7
D)
5
E)
3
62. How many orbitals have the set of quantum numbers ?
A)
5
B)
9
C)
7
D)
1
E)
3
63. Which orbital or orbitals is/are specified by the set of quantum numbers n= 4 and l= 3?
A)
4f
B)
3d
C)
1s
D)
2p
E)
4s
64. What is the total number of orbitals found in the n = 4 shell?
A)
16
B)
4
C)
20
D)
24
E)
15
Test Bank General Chemistry, 10th edition 20
65. Which of the following is a representation of a 3dxz orbital?
A)
B)
C)
D)
E)
66. Which of the following is a representation of a orbital?
A)
B)
C)
D)
E)
67. Which hydrogen atom orbital has an energy essentially identical to a 3d orbital?
A)
5d
B)
4p
C)
1s
D)
2s
E)
3p