Chemistry: A Molecular Approach, 3e (Tro)
Chapter 7 The Quantum-Mechanical Model of the Atom
Multiple Choice Questions
1) The vertical height of a wave is called
A) wavelength
B) amplitude
C) frequency
D) area
E) median
2) The number of cycles that pass through a stationary point is called
A) wavelength
B) amplitude
C) frequency
D) area
E) median
3) The distance between adjacent crests is called
A) wavelength
B) amplitude
C) frequency
D) area
E) median
4) On the electromagnetic spectrum, visible light is immediately between two other wavelengths. Name
them.
A) infrared and x-ray
B) radio and microwave
C) gamma ray and ultraviolet
D) microwave and x-ray
E) infrared and ultraviolet
5) Which of the following visible colors of light has the highest frequency?
A) green
B) red
C) blue
D) yellow
E) orange
6) Which of the following visible colors of light has the longest wavelength?
A) blue
B) green
C) yellow
D) red
E) violet
7) Which of the following colors of electromagnetic radiation has the shortest wavelength?
A) blue
B) violet
C) orange
D) green
E) yellow
8) Which of the following types of electromagnetic radiation has the lowest frequency?
A) yellow
B) blue
C) orange
D) green
E) purple
9) A sunburn is caused by overexposure to ________ radiation.
A) ultraviolet
B) gamma
C) microwave
D) x-ray
E) radio
10) ________ are used to image bones and internal organs.
A) Ultraviolet light
B) Gamma rays
C) Microwaves
D) X-rays
E) Radio waves
11) Food can be cooked by ________ radiation.
A) ultraviolet
B) gamma
C) microwave
D) x-ray
E) radio
12) When waves of equal amplitude from two sources are out of phase when they interact, it is called
________.
A) destructive interference
B) diffraction
C) constructive interference
D) effusion
E) amplitude
13) When waves of equal amplitude from two sources are in phase when they interact, it is called
________.
A) destructive interference
B) diffraction
C) constructive interference
D) effusion
E) amplitude
14) When a wave encounters an obstacle or a slit that is comparable in size to its wavelength, it bends
around it. This characteristic is called ________.
A) destructive interference
B) diffraction
C) constructive interference
D) effusion
E) amplitude
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15) Calculate the wavelength (in nm) of the blue light emitted by a mercury lamp with a frequency of
6.88 × 1014 Hz.
A) 229 nm
B) 436 nm
C) 206 nm
D) 485 nm
E) 675 nm
16) Which of the following occur as the energy of a photon increases?
A) the frequency decreases.
B) the speed increases.
C) the wavelength increases
D) the wavelength gets shorter.
E) None of the above occur as the energy of a photon increases.
17) Which of the following occur as the wavelength of a photon increases?
A) the frequency decreases
B) the energy increases
C) the speed decreases
D) Planck’s constant decreases
E) None of the above occur as the wavelength of a photon increases.
18) Calculate the energy of the green light emitted, per photon, by a mercury lamp with a frequency of
5.49 × 1014 Hz.
A) 2.75 × 10-19 J
B) 3.64 × 10-19 J
C) 5.46 × 10-19 J
D) 1.83 × 10-19 J
E) 4.68 × 10-19 J
19) Calculate the energy of the orange light emitted, per photon, by a neon sign with a frequency of 4.89
× 1014 Hz.
A) 3.09 × 10-19 J
B) 6.14 × 10-19 J
C) 3.24 × 10-19 J
D) 1.63 × 10-19 J
E) 5.11 × 10-19 J
20) Calculate the frequency of the green light emitted by a hydrogen atom with a wavelength of 486.1
5
nm.
A) 1.46 × 1014 s-1
B) 6.86 × 1014 s-1
C) 4.33 × 1014 s-1
D) 6.17 × 1014 s-1
E) 1.62 × 1014 s-1
21) Calculate the energy of the red light emitted by a neon atom with a wavelength of 703.2 nm.
A) 3.54 × 10-19 J
B) 4.27 × 10-19 J
C) 2.34 × 10-19 J
D) 6.45 × 10-19 J
E) 2.83 × 10-19 J
22) Calculate the energy of the violet light emitted by a hydrogen atom with a wavelength of 410.1 nm.
A) 4.85 × 10-19 J
B) 2.06 × 10-19 J
C) 1.23 × 10-19 J
D) 8.13 × 10-19 J
E) 5.27 x 10-19 J
23) How many photons are contained in a flash of green light (525 nm) that contains 189 kJ of energy?
A) 5.67 × 1023 photons
B) 2.01 × 1024 photons
C) 1.25 × 1031 photons
D) 4.99 × 1023 photons
E) 7.99 × 1030 photons
24) Determine the shortest frequency of light required to remove an electron from a sample of Ti metal,
if the binding energy of titanium is 3.14 × 103 kJ/mol.
A) 7.87 x 1015 Hz
B) 4.74 x 1015 Hz
C) 2.11 x 1015 Hz
D) 1.27 x 1015 Hz
E) 6.19 x 1015 Hz
25) What total energy (in kJ) is contained in 1.0 mol of photons, all with a frequency of 2.75 × 1014 Hz?
A) 182 kJ
B) 219 kJ
C) 457 kJ
D) 326 kJ
E) 110 kJ
26) Determine the longest wavelength of light required to remove an electron from a sample of
potassium metal, if the binding energy for an electron in K is 1.76 × 103 kJ/mol.
A) 147 nm
B) 68.0 nm
C) 113 nm
D) 885 nm
E) 387 nm
27) Identify the color of a flame test for potassium.
A) violet
B) red
C) white
D) yellow
E) blue
28) Identify the color of a flame test for sodium.
A) violet
B) red
C) white
D) yellow
E) blue
29) Identify the color of a flame test for lithium.
A) violet
B) red
C) white
D) yellow
E) blue
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30) Which of the following statements is TRUE?
A) The emission spectrum of a particular element is always the same and can be used to identify the
element.
B) Part of the Bohr model proposed that electrons in the hydrogen atom are located in “stationary states”
or particular orbits around the nucleus.
C) The uncertainty principle states that we can never know both the exact location and speed of an
electron.
D) An orbital is the volume in which we are most likely to find an electron.
E) All of the above are true.
31) Calculate the wavelength of an electron (m = 9.11 × 10-28 g) moving at 3.66 × 106 m/s.
A) 1.99 × 10-10 m
B) 5.03 × 10-10 m
C) 1.81 × 10-10 m
D) 5.52 × 10-9 m
E) 2.76 × 10-9 m
32) Calculate the wavelength of a baseball (m = 155 g) moving at 32.5 m/s.
A) 7.60 × 10-36 m
B) 1.32 × 10-34 m
C) 2.15 × 10-32 m
D) 2.68 × 10-34 m
E) 3.57 × 10-32 m
33) Determine the velocity of a medicine ball (m = 10.0 kg) with a wavelength of 1.33 × 10-35 m.
A) 8.81 m/s
B) 12.3 m/s
C) 2.21 m/s
D) 4.98 m/s
E) 6.44 m/s
34) Determine the mass of a ball with a wavelength of 3.45 x 10-34 m and a velocity of 6.55 m/s.
A) 0.293 g
B) 12.6 g
C) 293 g
D) 346 g
E) 3.41 g
35) It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the
ionization energy for an atom of hydrogen, making the assumption that ionization is the transition from
n = 1 to n = ∞.
A) -2.18 × 10-18 J
B) +2.18 × 10-18 J
C) +4.59 × 10-18 J
D) -4.59 × 10-18 J
E) +4.36 x 10-18 J
36) For n = 3, what are the possible sublevels?
A) 0
B) 0, 1
C) 0, 1, 2
D) 0, 1, 2, 3
37) What are the possible orbitals for n = 3?
A) s, p, d
B) s, p, d, f
C) s
D) s, p
38) What value of l is represented by a d orbital?
A) 1
B) 2
C) 0
D) 3
39) What value of l is represented by a f orbital?
A) 1
B) 2
C) 0
D) 3
40) How many orbitals are contained in the third principal level (n = 3) of a given atom?
A) 9
B) 3
C) 18
D) 7
E) 5
41) How many sublevels are contained in the second shell (n = 2) of a given atom?
A) 1
B) 2
C) 9
D) 4
E) 3
42) Which of the following statements is TRUE?
A) We can sometimes know the exact location and speed of an electron at the same time.
B) All orbitals in a given atom are roughly the same size.
C) Since electrons have mass, we must always consider them to have particle properties and never
wavelike properties.
D) Atoms are roughly spherical because when all of the different shaped orbitals are overlapped, they
take on a spherical shape.
E) All of the above are true.
43) Which of the following quantum numbers describes the shape of an orbital?
A) principal quantum number
B) magnetic quantum number
C) spin quantum number
D) Schrödinger quantum number
E) angular momentum quantum number
44) Which of the following quantum numbers describes the orientation of an orbital?
A) magnetic quantum number
B) principal quantum number
C) angular momentum quantum number
D) spin quantum number
E) Schrödinger quantum number
45) Which of the following quantum numbers describes the size and energy of an orbital?
A) magnetic quantum number
B) principal quantum number
C) angular momentum quantum number
D) spin quantum number
E) Schrödinger quantum number
46) How many different values of l are possible in the third principal level?
A) 1
B) 2
C) 3
D) 0
E) 4
47) If two electrons in the same atom have the same value of “l“, they are
A) in the same sublevel, but not necessarily in the same level.
B) in the same level, but different sublevel.
C) in the same orbital.
D) in different levels and in different shaped orbitals.
E) none of the above.
48) Determine the energy change associated with the transition from n = 2 to n = 5 in the hydrogen
atom.
A) -2.18 × 10-19 J
B) +6.54 × 10-19 J
C) +4.58 × 10-19 J
D) -1.53 × 10-19 J
E) +3.76 × 10-19 J
49) Determine the energy change associated with the transition from n = 3 to n = 2 in the hydrogen
atom.
A) +3.03 × 10-19 J
B) -1.82 × 10-19 J
C) +5.51 × 10-19 J
D) -3.03 × 10-19 J
E) +2.69 × 10-19 J
50) Calculate the energy change associated with the transition from n = 4 to n = 1 in the hydrogen atom.
A) +4.89 × 10-18 J
B) +1.64 × 10-18 J
C) -6.12 × 10-18 J
D) +3.55 × 10-18 J
E) -2.04 × 10-18 J
51) Which of the following statements is TRUE?
A) The principal quantum number (n) describes the shape of an orbital.
B) The angular momentum quantum number (l) describes the the size and energy associated with an
orbital.
C) The magnetic quantum number (ml) describes the orientation of the orbital.
D) An orbital is the path that an electron follows during its movement in an atom.
E) All of the above are true.
52) It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the
ionization energy (in kJ) for a mole of hydrogen atoms, making the assumption that ionization is the
transition from n = 1 to n = ∞.
A) 7.62 × 103 kJ
B) 2.76 × 103 kJ
C) 1.31 × 103 kJ
D) 3.62 × 103 kJ
E) 5.33 × 103 kJ
53) Calculate the wavelength of light associated with the transition from n = 1 to n = 3 in the hydrogen
atom.
A) 103 nm
B) 155 nm
C) 646 nm
D) 971 nm
E) 136 nm
54) Calculate the frequency of light associated with the transition from n = 2 to n = 3 in the hydrogen
atom.
A) 2.19 × 1014 s-1
B) 5.59 × 1014 s-1
C) 4.57 × 1014 s-1
D) 1.79 × 1014 s-1
E) 3.28 × 1014 s-1
55) Determine the end (final) value of n in a hydrogen atom transition, if the electron starts in n = 4 and
the atom emits a photon of light with a wavelength of 486 nm.
A) 1
B) 5
C) 3
D) 4
E) 2
56) Determine the end (final) value of n in a hydrogen atom transition, if the electron starts in n = 2 and
the atom absorbs a photon of light with a frequency of 4.57 × 1014 Hz.
A) 3
B) 1
C) 4
D) 6
E) 7
57) Determine the end (final) value of n in a hydrogen atom transition, if the electron starts in n = 1 and
the atom absorbs a photon of light with an energy of 2.044 × 10-18 J.
A) 3
B) 4
C) 2
D) 5
E) 6
58) Give the numbers for ml for an s orbital.
A) 0
B) -1, 0, 1
C) 0, 1
D) 1
59) Give the numbers for ml for a d orbital.
A) 0, 1, 2
B) -1, 0, 1
C) 1, 2, 3
D) -2, -1, 0, 1, 2
60) Give the numbers for ml for a p orbital.
A) 0, 1
B) -1, 0, 1
C) 1, 2
D) -2, -1, 0, 1, 2
61) Give the numbers for ml for an f orbital.
A) 0, 1, 2, 3
B) 1, 2, 3, 4
C) -3, -2, -1, 0, 1, 2, 3
D) -2, -1, 0, 1, 2
62) Describe the shape of a p orbital.
A) spherical
B) dumbbell shaped
C) three balls
D) four balls
E) eight balls
63) Describe the shape of a s orbital.
A) spherical
B) dumbbell shaped
C) three balls
D) four balls
E) eight balls
64) What is the maximum number of s orbitals that are possible?
A) 1
B) 3
C) 7
D) 5
E) 9