Deck 8: The Quantum Mechanical Atom

Question 1

The frequency of an electromagnetic wave is

A)the number of complete oscillations or cycles over a distance of one meter.
B)the number of complete oscillations or cycles in a one second time interval.
C)the distance between successive maxima in the wave in one complete cycle.
D)the number of complete oscillations or cycles over a distance of one centimeter.
E)the distance between successive nodes in the wave.

Answer 1

the number of complete oscillations or cycles in a one second time interval.

Question 2

The wavelength of an electromagnetic wave is

A)the number of complete oscillations or cycles over a distance of one meter.
B)the number of complete oscillations or cycles in a one second time interval.
C)the distance between successive maxima in the wave.
D)the number of complete oscillations or cycles over a distance of one centimeter.
E)the distance between a minimum and the nearest maximum in the oscillation.

Answer 2

the distance between successive maxima in the wave.

Question 3

What is the wavelength of electromagnetic radiation which has a frequency of 5.732 × 10¹⁴ s^-1?

A)1.718 × 10²³ m
B)1.912 × 10⁶ m
C)5.234 × 10^-7 m
D)523.4 m
E)5.819 × 10^-15 nm

Answer 3

5.234 × 10^-7 m

Question 4

What is the wavelength of electromagnetic radiation which has a frequency of 4.464 × 10¹⁴ s^-1?

A)1.338 ×10²³ m
B)1.489 × 10^-6 m
C)4.716 × 10⁷ nm
D)6.720 × 10² nm
E)7.472 × 10^-15 nm

Question 5

What is the wavelength of electromagnetic radiation which has a frequency of 3.818 × 10¹⁴ s^-1?

A)1145 nm
B)1.274 × 10^-1 nm
C)1.274 × 10^-7 m
D)7.858 × 10^-7 nm
E)7.858 × 10^-7 m

Question 6

What is the wavelength of electromagnetic radiation which has a frequency of 6.282 × 10¹⁴ s^-1?

A)1.883 × 10²³ m
B)2.095 × 10⁶ m
C)4.776 × 10^-7 m
D)4.776 × 10^-7 nm
E)530.9 nm

Question 7

Calculate the frequency of visible light having a wavelength of 464.1 nm.

A)139.1 s^-1
B)1.548 × 10^-6 s^-1
C)1.548 × 10^-15 s^-1
D)6.464 × 10¹⁴ s^-1
E)6.464 × 10⁵ s^-1

Question 8

Calculate the frequency of visible light having a wavelength of 589.3 nm.

A)176.7 s^-1
B)1.966 × 10^-15 s^-1
C)1.391 × 10^-11 s^-1
D)5.091 × 10¹⁴ s^-1
E)5.660 × 10³ s^-1

Question 9

A police radar unit is operating on a frequency of 9.527 gigahertz. What is the wavelength of the radiation being employed?

A)314.9 nm
B)314.9 m
C)3.149 cm
D)314.9 cm
E)31.78 m

Question 10

Calculate the frequency of visible light having a wavelength of 568.8 nm.

A)170.5 s^-1
B)1.897 × 10⁶ s^-1
C)1.897 × 10¹⁵ s^-1
D)5.274 × 10^-9 s^-1
E)5.274 × 10¹⁴ s^-1

Question 11

Calculate the frequency of visible light having a wavelength of 25.3 cm.

A)8.44 × 10^-8 s^-1
B)1.19 × 10⁹ s^-1
C)1.19 × 10⁷ s^-1
D)7.58 × 10⁹ s^-1
E)7.58 × 10⁷ s^-1

Question 12

Which one of the following types of radiation has the lowest frequency?

A)radio waves
B)infrared radiation
C)microwave radiation
D)X-rays
E)ultraviolet rays

Question 13

Which radiation has the lowest frequency?

A)gamma rays
B)infrared radiation
C)microwave radiation
D)visible light rays
E)ultraviolet rays

Question 14

Which radiation has the highest frequency?

A)blue visible light
B)radio waves
C)infrared radiation
D)microwave radiation
E)red visible light

Question 15

Which radiation has the highest frequency?

A)X-rays
B)ultraviolet rays
C)radio waves
D)microwave radiation
E)infrared radiation

Question 16

Which radiation has the shortest wavelength?

A)radio waves
B)infrared radiation
C)microwave radiation
D)ultraviolet rays
E)X-rays

Question 17

Which radiation has the shortest wavelength?

A)gamma rays
B)infrared radiation
C)microwave radiation
D)ultraviolet rays
E)visible light rays

Question 18

Which radiation has the shortest wavelength?

A)FM radio waves
B)infrared radiation
C)microwave radiation
D)ultraviolet rays
E)visible light rays

Question 19

Which radiation has the longest wavelength?

A)gamma rays
B)green visible light rays
C)red visible light rays
D)ultraviolet rays
E)X-rays

Question 20

Which radiation has the longest wavelength?

A)gamma rays
B)infrared radiation
C)microwave radiation
D)ultraviolet rays
E)red visible light rays

Question 21

Which radiation has the longest wavelength?

A)infrared radiation
B)radio waves
C)microwave radiation
D)ultraviolet rays
E)X-rays

Question 22

What is the energy of one photon of microwave radiation with a wavelength of 0.158 m?

A)1.26 × 10^-24 J
B)3.14 × 10^-26 J
C)3.19 × 10²⁵ J
D)3.49 × 10^-43 J
E)7.15 × 10⁴⁰ J

Question 23

What is the energy of one photon of visible radiation with a wavelength of 464.1 nm?

A)1.03 × 10^-48 J
B)2.10 × 10³⁵ J
C)2.34 × 10¹¹ J
D)4.28 × 10^-19 J
E)4.28 × 10^-12 J

Question 24

What is the energy of one mole of photons of visible light having a wavelength of 486.1 nm?

A)12.4 kJ
B)2.46 × 10^-4 J
C)2.46 × 10⁵ J
D)6.17 × 10¹⁴ J
E)8.776.2 × 10²⁵ J

Question 25

The photoelectric effect

A)describes the interaction of light with a photograph.
B)describes how electrons interact with each other.
C)is the process in which electrons are ejected from certain material by photons.
D)is the process of light being emitted from an electrical wire.
E)describes the interactions of photons with a pane of glass.

Question 26

What is the energy of one mole of photons of visible light having a wavelength of 4.89 × 10² nm?

A)1.48 × 10⁴² J
B)1.95 × 10^-16 J
C)2.45 × 10⁵ J
D)3.24 × 10^-40 J
E)4.06 × 10^-19 J

Question 27

What is the energy of one mole of photons associated with radiation that has a frequency of 6.336 × 10¹⁵ Hz?

A)2.528 × 10⁶ J
B)3.882 × 10¹⁴ J
C)3.955 × 10^-7 J
D)4.198 × 10^-18 J
E)6.298 × 10^-26 J

Question 28

What is the energy of one mole of photons associated with radiation that has a frequency of 3.818 × 10¹⁵ Hz?

A)1.045 × 10^-25 J
B)1.524 × 10⁶ J
C)2.530 × 10^-18 J
D)6.564 × 10^-7 J
E)9.568 × 10²⁴ J

Question 29

What is the wavelength of radiation which has an energy of 3.371 × 10^-19 joules per photon?

A)655.9 nm
B)152.5 nm
C)170.0 nm
D)589.3 nm
E)745.1 nm

Question 30

What is the wavelength of radiation which has an energy of 216.1 kJ per mole of photons?

A)655.9 nm
B)546.1 nm
C)108.8 nm
D)589.3 nm
E)977.7 nm

Question 31

What is the frequency of radiation which has an energy of 3.371 × 10^-19 joules per photon?

A)1.697 × 10¹⁵ s^-1
B)5.893 × 10^-7 s^-1
C)5.087 × 10¹⁴ s^-1
D)1.966 × 10^-15 s^-1
E)6.626 × 10^-34 s^-1

Question 32

What is the frequency of radiation which has an energy of 216.1 kJ per mole of photons?Hint: Pay careful attention to your units. 1 kJ = 1000 J.

A)615.9 × 10¹⁴ s^-1
B)1.624 × 10¹⁴ s^-1
C)1.058 × 10^-10 s^-1
D)5.416 × 10¹⁴ s^-1
E)3.588 × 10^-19 s^-1

Question 33

What is the energy of one mole of photons whose wavelength is 5.461 × 10² nm?Hint: Pay careful attention to your units. 1 m = 10^{9 nm.}

A)2.191 × 10^-4 J
B)2.437 × 10^-12 J
C)2.191 × 10⁵ J
D)1.376 × 10⁶ J
E)4.06 × 10^-19 J

Question 34

Which statement is true?

A)The line spectra of elements are the same provided they belong to the same family.
B)The line spectra of elements are the same provided they belong to the same family and are combined with oxygen.
C)The line spectra of elements are the same provided they belong to the same family and are in the same physical state.
D)The line spectra of elements can be used for separation of elements from mixtures.
E)The line spectra of elements can be used to identify the elements.

Question 35

Which statement is true?

A)The line spectra of atoms consist of a series of white lines superimposed on a colorful background.
B)The line spectra of atoms consist of a series of white lines superimposed on a dark background.
C)The line spectra of atoms consist of a series of colorful lines superimposed on a dark background.
D)The line spectra of atoms consist of a series of dark lines superimposed on a white background.
E)The line spectra of atoms consist of a series of dark lines superimposed on a colorful background.

Question 36

The definite energies associated with specific wavelengths in the emission spectrum of atomic hydrogen suggest that

A)electrons have a smaller rest mass than photons.
B)photons have a smaller rest mass than electrons.
C)energy states of the electron in the hydrogen atom are quantized.
D)atomic hydrogen is more stable and has a lower potential energy than molecular hydrogen.
E)the potential energy of electrons in the atom can have any arbitrary value over a period of time, but the kinetic energy may only have certain specific values.

Question 37

Calculate the wavelength of the spectral line in the spectrum of hydrogen for which n₁ = 1 and n₂ = 3.Hint: Use the Rydberg equation to solve.

A)277 nm
B)103 nm
C)345 nm
D)397 nm
E)489 nm

Question 38

Calculate the wavelength of the spectral line in the spectrum of hydrogen for which n₁ = 2 and n₂ = 4.Hint: Use the Rydberg equation to solve.

A)207 nm
B)365 nm
C)486 nm
D)274 nm
E)131 nm

Question 39

Calculate the wavelength of the spectral line in the spectrum of hydrogen for which n₁ = 4 and n₂ = 7.Hint: Use the Rydberg equation to solve.

A)2.17 × 10^-6 m
B)2.17 × 10^-4 m
C)4.62 × 10³ m
D)8.51 × 10^-5 m
E)8.51 × 10^-7 m

Question 40

Which statement is true concerning the spectrum of hydrogen obtained from a gas discharge tube?

A)A photon is absorbed as the electron goes from a state with a higher energy to one with a lower energy.
B)An electron is absorbed as the electron goes from a state with a lower energy to one with a higher energy.
C)A photon is emitted as the electron goes from a state with a higher energy to one with a lower energy.
D)A photon is emitted as the electron goes from a state with a lower energy to one with a higher energy.
E)An electron is emitted as the photon goes from a state with a higher energy to one with a lower energy.

Question 41

Which statement is true concerning Bohr's model of the atom?

A)The model accounted for the absorption spectra of atoms but not for the emission spectra.
B)The model could account for the emission spectrum of hydrogen and for the Rydberg equation.
C)The model was based on the wave properties of the electron.
D)The model accounted for the emission spectra of atoms, but not for the absorption spectra.
E)The model was generally successful for all atoms to which it was applied.

Question 42

Which statement about a hydrogen atom is false?

A)Atoms undergo the same specific energy changes.
B)When an excited atom loses energy, only a specific amount can be lost.
C)When an atom is supplied with energy, an electron drops from a higher energy level to a lower energy level.
D)When an electron drops back to a lower energy level, energy equal to the difference between the two levels is released and emitted as a photon.
E)The statements above are all true.

Question 43

Which statement is true of Bohr's equation, E = -b/n²?

A)E represents the energy of the proton.
B)b represents the energy of an excited electron.
C)The negative sign in the equation suggests that any electron with a finite value of n has a lower energy than an unbound electron.
D)The possible values of n are any real number
E)Each orbit is identified by its unique values for b and n.

Question 44

Calculate the energy required to excite a hydrogen atom by causing an electronic transition from the energy level with n = 1 to the level with n = 4. Recall that the quantized energies of the levels in the hydrogen atom are given by:

A)2.02 × 10^-29 J
B)2.04 × 10^-18 J
C)2.19 × 10⁵ J
D)2.25 × 10^-18 J
E)3.27 × 10^-17 J

Question 45

A hydrogen atom starts in the n = 1 energy level. What energy level would the atom end up in if it were to absorb 2.093 × 10^-18 J of energy?Hint: Make sure to convert energy to wavelength for your calculations.

A)n = 2
B)n = 3
C)n = 4
D)n = 5
E)n = 6

Question 46

Calculate the wavelength, in nanometers, of light emitted by a hydrogen atom when the electron falls from an n = 7 energy level to an n = 4 energy level. Recall that the quantized energies of the levels in the hydrogen atom are given by:

A)4.45 × 10^-20 nm
B)8.51 × 10² nm
C)2.17 × 10³ nm
D)1.38 × 10¹⁴ nm
E)2.16 × 10³ nm

Question 47

The de Broglie relationship provides a link between which two properties of the electron?

A)the mass and the charge
B)the mass and the energy
C)its energy and its charge
D)the orbit and its wavelike movements
E)its wave and particle properties

Question 48

Calculate the wavelength of a particle of mass 1.00 kg traveling at 1.00 km per hour.

A)101 m
B)3.45 × 10^-19 m
C)7.20 × 10^-29 m
D)2.38 × 10^-33 m
E)6.25 × 10^--34 m

Question 49

Calculate the wavelength of an electron (mass = 9.109 × 10^-31 kg)traveling at4.38 × 10⁶ m/s.

A)101 pm
B)166 pm
C)720 pm
D)298 pm
E)435 pm

Question 50

Calculate the wavelength of a hydrogen atom (mass = 1.674 × 10^-27 kg)traveling at7.88 × 10⁴ m/s.

A)3.12 × 10^-2 m
B)3.12 × 10^-56 m
C)2.12 × 10^-32 m
D)5.02 × 10^-12 m
E)1.32 × 10^-22 m

Question 51

Calculate the wavelength of a helium atom (mass = 6.65 × 10^-27 kg)traveling at 1.25 km/s.

A)79.7 nm
B)79.7 pm
C)8.31 × 10^-27 m
D)1.25 × 10¹⁰ m
E)831 pm

Question 52

The first description of the electron in the hydrogen atom by application of the wave nature of matter was presented by

A)Louis de Broglie.
B)Werner von Heisenberg.
C)Wolfgang Pauli.
D)Ernest Rutherford.
E)Erwin Schrödinger.

Question 53

The letter designation for the subshell in an atom is based on

A)the value of the secondary quantum number, l.
B)the value of the principal quantum number, n.
C)the value of the magnetic quantum number, m_l.
D)the value of the spin quantum number, m_s.
E)the transverse polarization of the optical emission from the H atom.

Question 54

The three quantum numbers which characterize the solutions to Schrodinger's equation, describing the behavior of the electron in the H atom are usually designated as

A)
B)
C)
D)
E)

Question 55

All orbitals with the same value of the principal quantum number are said to belong to the same

A)shell.
B)subshell.
C)group.
D)period.
E)class.

Question 56

All orbitals with the same value of the principal quantum number and the secondary quantum number are said to belong to the same

A)shell.
B)subshell.
C)group.
D)period.
E)class.

Question 57

The notation for the subshell with n = 5 and l = 3 is

A)5d subshell.
B)5p subshell.
C)5f subshell.
D)5g subshell.
E)5s subshell.

Question 58

The notation for the subshell with n = 4 and l = 2 is

A)4d subshell.
B)4p subshell.
C)4f subshell.
D)4s subshell.
E)There is no subshell fitting this description.

Question 59

The notation for the subshell with n = 3 and l = 3 is

A)3d subshell.
B)3f subshell.
C)3p subshell.
D)3s subshell.
E)There is no subshell fitting this description.

Question 60

Which statement correctly summarizes allowed values of quantum numbers in atoms?

A)All of the quantum numbers are allowed to have values which are not integers.
B)Only the principal quantum number is allowed to have values which are not integers.
C)Only the spin quantum numbers are allowed to have values which are not integers.
D)Only the secondary quantum number is allowed to have values which are not integers.
E)No quantum numbers are allowed to have values which are not integers.

Question 61

The Pauli principle states that

A)an electron in an atom can move to another energy level.
B)the energy of an electron has a specific quantum number.
C)the electron trapped in an atom has particle characteristics.
D)no two electrons in the same atom can have the exact same set of quantum numbers.
E)an orbital can hold as many electrons as possible.

Question 62

What is the maximum number of electrons that can fill all the orbitals of an f subshell?

A)6
B)8
C)10
D)12
E)14

Question 63

What is the maximum number of electrons that can fill all the orbitals of a d subshell?

A)6
B)8
C)10
D)12
E)14

Question 64

What is the maximum number of electrons that can fill all the orbitals of a p subshell?

A)2
B)3
C)4
D)6
E)10

Question 65

The number of electrons required to fill all the energy levels for a shell having principal quantum number n is

A)n
B)n+1
C)2n
D)n²
E)2n²

Question 66

Which of the following gives a possible quantum number assignment for the last electron added to the sodium atom when developing the electron configuration using the aufbau principle?

Question 67

Which of the following gives a possible quantum number assignment for the last electron added to the oxygen atom when developing the electron configuration using the aufbau principle?

Question 68

Given the following sets of quantum numbers for n, l, m_l, and m_s, which one of these sets is not possible for an electron in an atom?

Question 69

Given the following sets of quantum numbers for n, l, m_l, and m_s, which one of these sets is not possible for an electron in an atom?

Question 70

Given the following sets of quantum numbers for n, l, m_l, and m_s, which one of these sets is not possible for an electron in an atom?

Question 71

Given the following sets of quantum numbers for n, l, m_l, and m_s,which one of these sets is not possible for an electron in an atom?

Question 72

Given the following sets of quantum numbers for n, l, m_l, and m_s, which one of these sets is not possible for an electron in an atom?

Question 73

Given the following sets of quantum numbers for n, l, m_l, and m_s, which one of these sets is not possible for an electron in an atom?

Question 74

A paramagnetic element is an element

A)that always has an element in an excited state.
B)that is missing electrons.
C)that is attracted to a magnet.
D)that is not attracted to a magnet.
E)that forms a molecule with two atoms.

Question 75

A diamagnetic element is an element

A)that always has an element in an excited state.
B)that is missing electrons.
C)that is attracted to a magnet.
D)that is not attracted to a magnet.
E)that forms a molecule with two atoms.

Question 76

A possible set of quantum numbers for an electron in the partially filled subshell in a gallium atom in its ground state configuration would be

Question 77

A possible set of quantum numbers for an electron in the partially filled subshell in a vanadium atom in its ground state configuration would be

Question 78

A possible set of quantum numbers for an electron in the partially filled subshell in a potassium atom in its ground state configuration would be

Question 79

A possible set of quantum numbers for an electron in the partially filled subshell in a germanium atom in its ground state configuration would be

Question 80

A possible set of quantum numbers for an electron in the partially filled subshell in a technetium atom in its ground state configuration would be