General Chemistry, 11e (Petrucci)
Chapter 8 Electrons in Atoms
1) The symbol “n” in the Bohr theory of atomic structure refers to the number of electrons in an orbit.
2) The symbol “n” in the Bohr theory of atomic structure refers to the orbit in which an electron is found.
3) The Bohr theory explains that an emission spectral line is due to an interaction between electrons in
atoms.
4) The Bohr theory explains that an emission spectral line is due to an electron losing energy and
changing orbits.
5) The Bohr theory explains that an emission spectral line is due to an electron losing energy but keeping
the same values of its four quantum numbers.
6) When an electron goes from a high energy state to a low one, another electron goes from a low energy
state to a high one.
7) When an electron in an atom goes from a high energy state to a low one, light is given off.
8) Four of the 3d orbitals are alike except for the orientation with respect to the axes.
9) The following orbitals are placed in the correct filling order:
4f, 5d, 6s, 6p.
10) The following orbitals are placed in the correct filling order:
6s, 4f, 5d, 6p.
11) Light passing through a transparent medium has a wavelength of 466 nm and a frequency of 6.20 ×
1014 s-1. What is the speed of the light in the medium?
A) 2.89 × 108 m/s
B) 2.89 × 1017 m/s
C) 1.33 × 1012 m/s
D) 1.33 × 1021 m/s
E) 7.52 × 10–22 m/s
12) What is the frequency of radiation with a wavelength of 440. nm?
A) 6.81 × 1014 s–1
B) 6.81 × 105 s–1
C) 1.51 × 10–27 s–1
D) 4.95 × 10–12 s–1
E) 2.02 × 10–11 s–1
13) What is the frequency associated with radiation of 4.59 × 10-8 cm wavelength?
A) 6.54 × 1017 s–1
B) 6.54 × 1015 s–1
C) 1.53 × 10-8 s–1
D) 13.8 s–1
E) 2.18 × 107 s–1
14) What is the wavelength in nm associated with radiation of frequency 2.8 × 1013 s-1?
A) 840 nm
B) 2.8 × 104 nm
C) 299 nm
D) 9.3 × 104 nm
E) 1.1 × 104 nm
15) Frequency and wavelength are related by the equation:
A) λ = c ∙ v
B) λ = c/v
C) v = λ/c
D) λ = v/c
E) c = λ/v
16) Choose the INCORRECT statement concerning electromagnetic radiation.
A) Infrared light has a longer wavelength than ultraviolet light.
B) The greater the frequency of the electromagnetic radiation, the greater the energy of the radiation.
C) A photon with a wavelength of 5000 angstroms has one-half as much energy as a photon with a
wavelength of 2500 angstroms.
D) The speed of ultraviolet light rays is faster than X-rays in a vacuum.
E) Electromagnetic radiation is energy transmission in which electric and magnetic fields are propagated
as waves.
17) The relationship between the frequency of light and the energy of the light was postulated by:
A) Max Planck
B) Johann Balmer
C) Johannes Rydberg
D) Albert Einstein
E) Robert Bunsen
18) A radiation detector exposed to sunlight records the energy falling on a given area per unit time. If
such a detector has a reading of 0.698 cal cm-2 min-1, how many photons of sunlight are striking each
cm2 in one minute? Assume the average wavelength of sunlight is 460. nm. (4.184 J = 1 calorie)
A) 1.62 × 1018 photons
B) 4.32 × 1019 photons
C) 6.76 × 1018 photons
D) 2.31 × 1018 photons
E) 9.63 × 1019 photons
19) A radiation detector exposed to sunlight records the energy falling on a given area per unit time. If
such a detector has a reading of 0.430 cal cm-2 min-1, how many photons of sunlight are striking each
cm2 in one minute? Assume the average wavelength of sunlight is 460. nm. (4.184 J = 1 calorie)
A) 2.02 × 107 photons
B) 8.46 × 107 photons
C) 4.17 × 1018 photons
D) 1.02 × 1027 photons
E) 4.25 × 1027 photons
20) Use Planck’s equation to determine the energy, in J/photon, of radiation of frequency 5.8 × 1015 s-1.
A) 3.8 × 10–18 J
B) 1.7 × 1024 J
C) 5.8 × 10–25 J
D) 1.7 × 10–16 J
E) 5.2 × 10-8 J
21) Calculate the energy in kJ/mol of light with a wavelength of 360 nm.
A) 5.52 × 10–22 kJ/mol
B) 5.52 × 10–19 kJ/mol
C) 332 kJ/mol
D) 6.63 × 103 kJ/mol
E) 0.332 kJ/mol
22) How many photons of light with frequency 5.50 × 1015 Hz are required to provide 1 kJ of energy?
A) 3.64 × 10–18 photons
B) 2.74 × 1020 photons
C) 4.56 × 10-4 photons
D) 1.65 × 1044 photons
E) 3.64 × 10–16 photons
23) The existence of discrete (quantized) energy levels in an atom may be inferred from:
A) diffraction of electrons by crystals
B) X-ray diffraction by crystals
C) atomic line spectra
D) experiments on the photoelectric effect
E) visible spectrum
24) The photoelectric effect:
A) was discovered by Max Planck
B) describes the phenomenon of producing light by shining a beam of electrons by on any metal surface
C) contradicted the view that light energy was dependent upon intensity only
D) is not the same principle used in modern electric eyes and solar calculators
E) results in a beam of electrons which increases in number, but not velocity, as the wavelength of
incident light decreases
25) The mathematical equation deduced by Johann Balmer and subsequently rewritten in another form
by Johannes Rydberg gives us:
A) the relationship between wavelengths of spectral lines and the electrons’ energies responsible for them
B) the relationship between wavelength and frequency of spectral lines
C) the relationship between frequencies of spectral lines and the energy values associated with them
D) a model for finding the limited numbers of wavelengths associated with atomic spectral lines
E) an explanation for the continuous range of energy values associated with atomic spectra
26) The symbol “n” in the Bohr theory of atomic structure refers to:
A) the energy of the electrons
B) the total energy of the atom
C) the number of electrons in an orbit
D) the orbit in which an electron is found
E) the number of orbits in an atom
27) For the Bohr hydrogen atom determine the energy level corresponding to n = 3.
A) 7.26 × 10–19 J
B) 7.36 × 10–35 J
C) -2.42 × 10–19 J
D) 3.33 × 107 J
E) 1.96 × 10–17 J
28) Which statement regarding the wave function as suggested by Erwin Schrodinger is INCORRECT?
A) It is the lowest energy value of a particle.
B) It’s value can be zero.
C) It is denoted by psi (Ψ).
D) Zero-point energy corresponds to n = 1.
E) The zero-point energy is an allowable value of the energy of the particle.
29) What is the energy in joules of the 656 nm spectral line of hydrogen?
A) 4.35 × 10-31 J
B) 3.03 × 10-19 J
C) 1.30 × 10-22 J
D) 3.03 × 10-28 J
E) 1.45 × 10-48 J
30) What is the energy in joules of the 434 nm spectral line of hydrogen?
A) 1.53 × 10-27 J
B) 4.58 × 10-28 J
C) 1.04 × 1048 J
D) 4.58 × 10-19 J
E) 9.59 × 10-49 J
31) What is the energy in joules of a mole of photons with the energy of the 434 nm spectral line of
hydrogen?
A) 2.76 × 105 J
B) 9.21 × 10–4 J
C) 2.76 × 10–4 J
D) 5.78 × 10-25 J
E) 434 J
32) The Bohr theory explains that an emission spectral line is:
A) due to an electron losing energy but keeping the same values of its four quantum numbers
B) due to an electron losing energy and changing orbits
C) due to an interaction between electrons in two different principal orbits
D) due to an electron gaining energy and changing orbits
E) due to an increase in the principal quantum number n of an electron
33) When an electron in an atom goes from a high energy state to a low one, what occurs?
A) Another electron goes from a low energy state to a high one.
B) The atom moves faster.
C) Light is given off.
D) Light is absorbed.
E) This process is not possible.
34) Calculate the wavelength in meters of light absorbed by an electron in an atom of hydrogen as it
moves that makes a transition from n = 3 to n = 6.
A) 1.09 × 10-6 m
B) 8.22 × 10-7 m
C) 3.28 × 10-6 m
D) 1.83 × 10-7 m
E) 1.65 × 10–11 m
35) The fact that we cannot simultaneously measure the exact position and precise momentum of an
electron is referred to as:
A) Pauli Exclusion Principle
B) The Aufbau Principle
C) Hund’s Rule
D) The DeBroglie Relationship
E) Heisenberg Uncertainty Principle
36) What is the wavelength associated with electrons traveling at one one-hundredth the speed of light?
A) 243 nm
B) 0.243 nm
C) 412 nm
D) 7.98 × 10-2 nm
E) 12.5 nm
37) What is the wavelength of a ball that is 25.0 g traveling at 40.2 m/s?
A) 6.59 × 10–37 m
B) 6.59 × 10-34 m
C) 1.07 × 10–30 m
D) 4.12 × 10–37 m
E) 2.42 × 10–11 m
38) What is the wavelength of a bullet that is 0.450 g traveling at 2000. m/s?
A) 2000. m
B) 2.94 × 10-24 m
C) 7.36 × 10-34 m
D) 7.36 × 10-37 m
E) 1.49 × 10-40 m
39) Calculate the deBroglie wavelength of a ball of mass 125 grams and velocity 90 m/s.
A) 0.59 m
B) 5.9 × 10–31 m
C) 5.9 × 10–35 m
D) 590 m
E) 1.7 × 1034 m
40) What is the wavelength, in nm, associated with a 2000. kg truck traveling at a speed of 20 m/s, that is,
considering the truck to be a “matter” wave?
A) 1.33 × 10–29 nm
B) 2.65 × 10–29 nm
C) 6.02 × 10–29 nm
D) 7.50 × 103 nm
E) 1.66 × 10–29 nm
41) Which statement regarding the wave function as suggested by Erwin Schrodinger is INCORRECT?
A) It has fluctuating values at all points on the curve.
B) It is a mathematical equation.
C) It is denoted by psi (Ψ).
D) It can describe any particle with wavelike motions.
E) It corresponds to a standing wave within the boundary of the system.
42) An atomic orbital represents:
A) the shape of an atom
B) the repulsion of all the electrons among themselves
C) a fixed path that an electron follows around the nucleus of an atom
D) the region of electron density for a covalent bond
E) the region of high probability for an electron to exist near the nucleus of an atom
43) An atomic orbital:
I) describes a region of high electron density.
II) describes a region in an atom where an electron is likely to be found.
III) is a wave function resulting from specific values assigned to quantum numbers in wave equations.
IV) describes a spherical region around a nucleus where an electron can be found.
A) II only
B) I and II
C) II and III
D) I, II, and III
E) I, II, III, and IV
44) Which of the following is not possible?
A) 2p
B) 4d
C) 5p
D) 3f
E) 2s
45) The possible value(s) of the orbital angular momentum quantum number of a 3p electron are:
A) +1/2, -1/2
B) -1, 0, +1
C) -1
D) 0
E) 1
46) The possible values of the magnetic quantum number, mℓ , of a 3p electron are:
A) 0, 1, 2
B) 2, 1, 0, -1, –2
C) 0
D) -1, 0, +1
E) +1, -1
47) Give the appropriate values of n and ℓ for the orbital designation 3p.
A) n = 3, ℓ = 0
B) n = 1, ℓ = 3
C) n = 3, ℓ = 3
D) n = 3, ℓ = 1
E) n = 3, ℓ = 2
48) Give the appropriate values of n and ℓ for the orbital designation 3s.
A) n = 3, ℓ = 1
B) n = 0, ℓ = 3
C) n = 3, ℓ = 3
D) n = 3, ℓ = 2
E) n = 3, ℓ = 0
49) What is the smallest acceptable value for the missing quantum number?
n = ?, ℓ = 2, mℓ = 0, ms = +1/2
A) 3
B) 2
C) 4
D) 5
E) 1
50) What is the orbital designation for the quantum numbers n = 2, ℓ = 1?
A) 3s
B) 2s
C) 2d
D) 2p
E) 3p
51) Which of the following orbitals have their lobes aligned along the y axis?
I) dxy
II) dx2-y2
III) py
IV) dyz
A) II and III
B) I and IV
C) I and II
D) II and IV
E) I and III
52) Which of the following orbitals have lobes aligned along the x axis?
A) dxy
B) dx2-y2
C) dxz
D) dyz
E) s
53) Which two orbitals are located between the axes of a coordinate system and not along the axes?
A) dxy, py
B) dyz, px
C) dx2–y2, pz
D) dxy, dz2
E) dxy, dyz
54) Which of the following statements about orbital shapes is NOT true?
A) A 1s orbital is spherical.
B) 2p orbitals have a node at r = 0.
C) There are only two 2p orbitals, each directed along and x or y axis.
D) There are five 3d orbitals.
E) Four of the 3d orbitals are alike except for the orientation with respect to the axes.
55) All of the terms below are quantum numbers EXCEPT:
A) principal
B) magnetic
C) spin
D) valence
E) orbital angular momentum
56) Which of the following statements concerning quantum numbers is NOT correct?
A) “n” relates the most probable distance from the nucleus.
B) “l” denotes geometric shape.
C) “m” denotes orientation of an orbital with respect to the others.
D) The fourth quantum number refers to electron spin.
E) The four quantum numbers are derived from wave mechanics.
57) Which one of the following set of quantum numbers would not be allowed?
A) n = 3, ℓ = 2, mℓ = 1
B) n = 3, ℓ = 0, mℓ = 0
C) n = 3, ℓ = 3, mℓ = 1
D) n = 3, ℓ = 2, mℓ = -1
E) n = 3, ℓ = 1, mℓ = -1
58) Which of the following statements about the electron spin quantum number is FALSE?
A) ms denotes the spin quantum number.
B) The value of the spin quantum number can be +1/2 or -1/2.
C) The value of the spin quantum number does not depend on other quantum numbers.
D) The value of the spin quantum number can be indicated by arrows to the right and to the left.
E) The spin quantum number is an indication that electrons generate a magnetic field.
59) Which of the following statements about electron spin is FALSE?
A) An electron produces a magnetic field.
B) The electron’s magnetic field can be oriented in two directions in the presence of an external magnetic
field.
C) Paired electrons produced no net magnetic field.
D) An experiment with silver atoms passing through a magnetic field seems to prove that electron spin
exists.
E) Electron spin only exists when mℓ = 0.
60) Experimental evidence for electron spin:
A) has not yet been found
B) was provided by Uhlenbeck and Goudsmit in 1925
C) came as the result of an experiment with vaporized silver atoms, which was originally designed for
another purpose
D) is provided each time we make mirror-image molecules, called left and right-handed isomers
E) is not needed because the concept is only for our convenience
61) What is an acceptable value for the missing quantum number?
n = 4, ℓ = 2, mℓ = 0, ms = ?
A) 0
B) +1/2
C) 1
D) 2
E) 3/2
62) Which series below represents the correct order of orbital filling in a multielectron atom?
A) 5d, 4f, 6s, 6p
B) 4f, 6s, 5d, 6p
C) 4f, 5d, 6s, 6p
D) 6s, 4f, 5d, 6p
E) 6s, 6p, 5d, 4s
63) “One places electrons into orbitals one by one from low energy to high energy” is one way of stating
the:
A) Aufbau principle
B) Hund’s Rule
C) Heisenberg Principle
D) Pauli Exclusion Principle
E) Rydberg’s Principle
64) The principle that is based on electrons attempting to be as far apart as possible is the:
A) Heisenberg Principle
B) Pauli Exclusion Principle
C) Bohr Theory
D) Hund’s Rule
E) Aufbau principle
65) Which of the following subshells is correctly designated?
A) 1p5
B) 3s3
C) 3f2
D) 4d11
E) 2p6
66) Exceptions to ________ are represented by chromium and copper in the 4th row of the periodic table.
A) the Aufbau Principle
B) Hund’s Rule
C) the Bohr Theory
D) the Heisenberg Principle
E) the Pauli Exclusion Principle