Deck 7: Quantum Theory and Atomic Structure

Question 1

In the Bohr model of the hydrogen atom, the electron moves in a circular path which Bohr referred to as an orbital.

Answer 1

False

Question 2

Continuous spectra are characteristic of heated solids.

Answer 2

True

Question 3

A wave function for an electron is called an atomic orbital.

Answer 3

True

Question 4

In the Rydberg equation, for a fixed value of n₁, the longest wavelength line has n₂ = ∞.

Question 5

Who developed an empirical equation from which the wavelengths of lines in the spectrum of hydrogen atoms can be calculated?

A)Planck
B)de Broglie
C)Bohr
D)Rutherford
E)Rydberg

Question 6

Which scientist first proposed that the electron in the hydrogen atom can have only certain energies?

A)Planck
B)Einstein
C)Bohr
D)Rydberg
E)Heisenberg

Question 7

Who was the first scientist to propose that the atom had a dense nucleus that occupied only a small fraction of the volume of the atom?

A)Planck
B)Bohr
C)Rydberg
D)Rutherford
E)Thomson

Question 8

The Rydberg equation, giving the wavelengths of lines in the spectrum of the hydrogen atom, was obtained by assuming that energy is quantized.

Question 9

Continuous spectra are characteristic of molecules in the gas phase.

Question 10

Line spectra are characteristic of atoms in the gas phase.

Question 11

Other factors being constant, a heavy object will have a longer de Broglie wavelength than a light object.

Question 12

Which scientist demonstrated that photons transferred momentum during collisions with matter?

A)Bohr
B)de Broglie
C)Planck
D)Compton
E)Billiard

Question 13

The Rydberg equation is an example of an empirical equation.

Question 14

Who proposed a model that successfully explained the photoelectric effect?

A)Planck
B)Einstein
C)Compton
D)Rydberg
E)Bohr

Question 15

The energy of a photon is directly proportional to the wavelength of the radiation.

Question 16

In the quantum mechanical treatment of the hydrogen atom, the probability of finding an electron at any point is proportional to the wave function Ψ.

Question 17

In the quantum mechanical treatment of the hydrogen atom, the energy depends on the principal quantum number n but not on the values of l or m_l.

Question 18

As the frequency of electromagnetic radiation increases, its wavelength also increases.

Question 19

Which scientist first proposed that particles of matter could have wave properties?

A)Einstein
B)Planck
C)de Broglie
D)Compton
E)Heisenberg

Question 20

Who was the first scientist to propose that an object could emit only certain amounts of energy?

A)Planck
B)Einstein
C)Bohr
D)Rydberg
E)de Broglie

Question 21

Which of the following frequencies of electromagnetic radiation has the shortest wavelength?

A)1 kilohertz
B)1 terahertz
C)1 dekahertz
D)1 gigahertz
E)1 megahertz

Question 22

Electromagnetic radiation of 500 nm wavelength lies in the __________ region of the spectrum.

A)infrared
B)visible
C)ultraviolet
D)X-ray
E)γ-ray

Question 23

Contact lenses can focus light due to the __________ of the waves.

A)diffraction
B)reflection
C)refraction
D)dispersion
E)interference

Question 24

Infrared radiation from the sun has a wavelength of 6200 nm. Calculate the energy of one photon of that radiation.

A)4.l × 10 ⁻³⁹ J
B)4.l × 10 ⁻³⁰ J
C)3.2 × 10 ⁻²⁹ J
D)3.2 × 10 ⁻²⁶ J
E)between 10 ⁻²⁰ and 10 ⁻¹⁹ J

Question 25

The interference pattern seen when light passes through narrow, closely spaced slits, is due to

A)diffraction.
B)reflection.
C)refraction.
D)dispersion.
E)deflection.

Question 26

Green light has a wavelength of 5200 Å. Calculate the energy of one photon of green light.

A)3.4 × 10 ⁻⁴⁰ J
B)3.4 × 10 ⁻³⁰ J
C)3.8 × 10 ⁻²⁹ J
D)3.4 × 10 ⁻²⁷ J
E)3.8 × 10 ⁻¹⁹ J

Question 27

Select the arrangement of electromagnetic radiation which starts with the lowest energy and increases to greatest energy.

A)radio, infrared, ultraviolet, gamma rays
B)radio, ultraviolet, infrared, gamma rays
C)gamma rays, infrared, radio, ultraviolet
D)gamma rays, ultraviolet, infrared, radio
E)infrared, ultraviolet, radio, gamma rays

Question 28

A photon has an energy of 5.53 × 10⁻¹⁷ J. What is its frequency in s⁻¹ ?

A)3.66 × 10 ⁻⁵⁰ s ⁻¹
B)1.20 × 10 ⁻¹⁷ s ⁻¹
C)3.59 × 10 ⁻⁹ s ⁻¹
D)2.78 × 10 ⁸ s ⁻¹
E)8.35 × 10 ¹⁶ s ⁻¹

Question 29

An infrared wave has a wavelength of 6.5 × 10⁻⁴ cm. What is this distance in angstroms, Å?

A)6.5 × 10 ⁻⁴ Å
B)2.2 × 10 ⁻⁴ Å
C)4.6 × 10 ³ Å
D)6.5 × 10 ⁴ Å
E)6.5 × 10 ⁶ Å

Question 30

If the energy of a photon is 1.32 × 10⁻¹⁸ J, what is its wavelength in nm?

A)1.50 × 10 ⁻⁷ nm
B)150 nm
C)1.99 × 10 ¹⁵ nm
D)1.99 × 10 ²⁴ nm
E)None of these choices are correct.

Question 31

The AM station KBOR plays your favorite music from the 20s and 30s at 1290 kHz. Find the wavelength of these waves.

A)4.30 × 10 ⁻² m
B)0.144 m
C)6.94 m
D)232 m
E)> 10 ³ m

Question 32

Which word best describes the phenomenon which gives rise to a rainbow?

A)Reflection
B)Dispersion
C)Diffraction
D)Interference
E)Deflection

Question 33

A radio wave has a frequency of 8.6 × 10⁸ Hz. What is the energy of one photon of this radiation?

A)7.7 × 10 ⁻⁴³ J
B)2.3 × 10 ⁻³⁴ J
C)5.7 × 10 ⁻²⁵ J
D)1.7 × 10 ⁻¹⁶ J
E)> 10 ⁻¹⁵ J

Question 34

A modern compact fluorescent lamp contains 1.4 mg of mercury. If each mercury atom in the lamp were to emit a single photon of wavelength 254 nm, how many joules of energy would be emitted?

A)7.8 × 10 ⁻¹⁹ J
B)3.3 J
C)6.6 × 10 ² J
D)3.3 × 10 ³ J
E)4.2 × 10 ¹⁸ J

Question 35

The FM station KDUL broadcasts music at 99.1 MHz. Find the wavelength of these waves.

A)1.88 × 10 ⁻² m
B)0.330 m
C)3.03 m
D)5.33 × 10 ² m
E)> 10 ³ m

Question 36

Select the arrangement of electromagnetic radiation which starts with the lowest energy and increases to greatest energy.

A)radio, visible, infrared, ultraviolet
B)infrared, visible, ultraviolet, microwave
C)visible, ultraviolet, infrared, gamma rays
D)X-radiation, visible, infrared, microwave
E)microwave, infrared, visible, ultraviolet

Question 37

Who proposed the principle that states that one cannot simultaneously know the exact position and velocity of a particle?

A)Einstein
B)Planck
C)Heisenberg
D)Compton
E)de Broglie

Question 38

Interference of light waves

A)separates light into its component colors.
B)creates a pattern of light and dark regions.
C)focuses a broad beam of light into a point.
D)bends light as it passes the edge of an object.
E)creates a laser beam.

Question 39

Electromagnetic radiation can be specified by its wavelength (λ), its frequency (υ) or its period (τ). The period τ is the time it takes one complete wavelength to pass a point in space. Based on this information, what is the mathematical relationship between υ and τ?

A)υ = 1/τ
B)υ= τ
C)τ = υ/ с
D)с = τ × υ
E)τ = с/υ

Question 40

Select the arrangement of electromagnetic radiation which starts with the lowest wavelength and increases greatest wavelength.

A)radio, infrared, ultraviolet, gamma rays
B)radio, ultraviolet, infrared, gamma rays
C)gamma rays, radio, ultraviolet, infrared
D)gamma rays, infrared, radio, ultraviolet
E)gamma rays, ultraviolet, infrared, radio

Question 41

Excited hydrogen atoms radiate energy in the

A)infrared region only.
B)visible region only.
C)ultraviolet region only.
D)visible and ultraviolet regions only.
E)infrared, visible, and ultraviolet regions.

Question 42

In the photoelectric effect, a photon with an energy of 5.3 × 10⁻¹⁹ J strikes an electron in a metal. Of this energy, 3.6 × 10⁻¹⁹ J is the minimum energy required for the electron to escape from the metal. The remaining energy appears as kinetic energy of the photoelectron. What is the velocity of the photoelectron, assuming it was initially at rest?

A)3.7 × 10 ¹⁴ m/s
B)3.7 × 10 ¹¹ m/s
C)1.9 × 10 ⁶ m/s
D)6.1 × 10 ⁵ m/s
E)1.7 × 10 ⁻¹⁹ m/s

Question 43

Platinum, which is widely used as a catalyst, has a work functionΦ (the minimum energy needed to eject an electron from the metal surface) of 9.05 × 10⁻¹⁹ J. What is the longest wavelength of light which will cause electrons to be emitted?

A)2.196 × 10 ⁻⁷ m
B)4.553 × 10 ⁻⁶ m
C)5.654 × 10 ² m
D)1.370 × 10 ¹⁵ m
E)> 10 ⁶ m

Question 44

The size of an atomic orbital is associated with

A)the principal quantum number ( n).
B)the angular momentum quantum number ( l).
C)the magnetic quantum number ( m_l)_.
D)the spin quantum number ( m_s)_.
E)the angular momentum and magnetic quantum numbers, together.

Question 45

The Bohr theory of the hydrogen atom predicts the energy difference (in J) between the n = 3 and the n = 5 state to be

A)8.72 × 10 ⁻²⁰ J.
B)1.36 × 10 ⁻¹⁹ J.
C)2.42 × 10 ⁻¹⁹ J.
D)1.55 × 10 ⁻¹⁹ J.
E)1.09 × 10 ⁻¹⁸ J.

Question 46

Use the Rydberg equation to calculate the frequency of a photon absorbed when the hydrogen atom undergoes a transition from n₁ = 2 to n₂ = 4. (R = 1.096776 × 10⁷ m⁻¹)

A)2.056 × 10 ⁶ s ⁻¹
B)2.742 × 10 ⁶ s ⁻¹
C)6.165 × 10 ¹⁴ s ⁻¹
D)8.226 × 10 ¹⁴ s ⁻¹
E)> 10 ¹⁵ s ⁻¹

Question 47

The de Broglie equation predicts that the wavelength (in m) of a proton moving at 1000. m/s is

A)3.96 × 10 ⁻¹⁰ m.
B)3.96 × 10 ⁻⁷ m.
C)2.52 × 10 ⁶ m.
D)2.52 × 10 ⁹ m.
E)> 10 ¹⁰ m.

Question 48

According to the Rydberg equation, the line with the shortest wavelength in the emission spectrum of atomic hydrogen is predicted to lie at a wavelength (in nm) of

A)91.2 nm.
B)1.10 × 10 ⁻² nm.
C)1.10 × 10 ² nm.
D)1.10 × 10 ¹⁶ nm.
E)None of these choices are correct.

Question 49

The ionization energy is the energy needed to remove an electron from an atom. In the Bohr model of the hydrogen atom, this means exciting the electron to the n = ∞ state. What is the ionization energy in kJ/mol, for hydrogen atoms initially in the n = 2 energy level?

A)290 kJ/mol
B)328 kJ/mol
C)656 kJ/mol
D)983 kJ/mol
E)1311 kJ/mol

Question 50

A sprinter must average 24.0 mi/h to win a 100-m dash in 9.30 s. What is his wavelength at this speed if his mass is 84.5 kg?

A)7.29 × 10 ⁻³⁷ m
B)3.26 × 10 ⁻³⁷ m
C)5.08 × 10 ⁻³⁰ m
D)1.34 × 10 ⁻³⁰ m
E)None of these choices are correct.

Question 51

Consider the following adjectives used to describe types of spectrum: continuous, line, atomic, emission and absorption.How many of them are appropriate to describe the spectrum of radiation given off by a black body?

A)None
B)One
C)Two
D)Three
E)Four

Question 52

According to the Rydberg equation, the longest wavelength (in nm) in the series of H-atom lines with n₁ = 3 is

A)1875 nm.
B)1458 nm.
C)820. nm.
D)656 nm.
E)365 nm.

Question 53

Line spectra from all regions of the electromagnetic spectrum, including the Paschen series of infrared lines for hydrogen, are used by astronomers to identify elements present in the atmospheres of stars. Calculate the wavelength of the photon emitted when the hydrogen atom undergoes a transition from n = 5 to n = 3. (R = 1.096776 × 10⁷ m⁻¹)

A)205.1 nm
B)384.6 nm
C)683.8 nm
D)1282 nm
E)> 1500 nm

Question 54

What type of spectrum, if any, would be produced if the light radiated by a heated atomic gas were to be dispersed through a prism?

A)A continuous band of color
B)A continuous band of color with some dark lines (missing wavelengths)
C)Only blue light
D)Only red light
E)Discrete lines of different colors

Question 55

An electron in the n = 6 level emits a photon with a wavelength of 410.2 nm. To what energy level does the electron move?

A)n = 1
B)n = 2
C)n = 3
D)n = 4
E)n = 5

Question 56

For all the allowed vibration(s) (wavelength(s)) of a plucked guitar string, what is the correct relationship between the length of the string, L, and the wavelength, λ?

A)L = λ/2
B)L = λ
C)L = nλ/2 where n is a positive integer
D)L = nλ where n is a positive integer
E)L = 1/λ

Question 57

According to the Heisenberg uncertainty principle, if the uncertainty in the speed of an electron is 3.5 × 10³ m/s, the uncertainty in its position (in m) is at least

A)1.7 × 10 ⁻⁸ m.
B)6.6 × 10 ⁻⁸ m.
C)17 m.
D)66 m.
E)None of these choices are correct.

Question 58

For potassium metal, the work functionΦ (the minimum energy needed to eject an electron from the metal surface) is 3.68 × 10⁻¹⁹ J. Which is the longest wavelength of the following which could excite photoelectrons?

A)550 nm
B)500 nm
C)450 nm
D)400 nm
E)350 nm

Question 59

Consider the following adjectives used to describe types of spectrum: continuous, line, atomic, emission and absorption.How many of them are appropriate to describe the spectrum of radiation absorbed by a sample of mercury vapor?

A)One
B)Two
C)Three
D)Four
E)Five

Question 60

According to the Bohr theory of the hydrogen atom, the minimum energy (in J) needed to ionize a hydrogen atom from the n = 2 state is

A)2.18 × 10 ⁻¹⁸ J.
B)1.64 × 10 ⁻¹⁸ J.
C)5.45 × 10 ⁻¹⁹ J.
D)3.03 × 10 ⁻¹⁹ J.
E)None of these choices are correct.

Question 61

In the quantum mechanical treatment of the hydrogen atom, which one of the following combinations of quantum numbers is not allowed?

A)A
B)B
C)C
D)D
E)E

Question 62

Atomic orbitals developed using quantum mechanics

A)describe regions of space in which one is most likely to find an electron.
B)describe exact paths for electron motion.
C)give a description of the atomic structure which is essentially the same as the Bohr model.
D)allow scientists to calculate an exact volume for the hydrogen atom.
E)are in conflict with the Heisenberg Uncertainty Principle.

Question 63

In an atom, the square of an electron's wave function

A)becomes zero at the nucleus.
B)is smallest near the nucleus.
C)is largest near the nucleus.
D)may be zero at more than one point.
E)tends to infinity at large distances from the nucleus.

Question 64

The shape of an atomic orbital is associated with

A)the principal quantum number ( n).
B)the angular momentum quantum number ( l).
C)the magnetic quantum number ( m_l)_.
D)the spin quantum number ( m_s)_.
E)the magnetic and spin quantum numbers, together.

Question 65

Which one of the following sets of quantum numbers can correctly represent a 3p orbital?

A)n = 3 l = 1 m_l = 2
B)n = 1 l = 3 m_l = 3
C)n = 3 l = 2 m_l = 1
D)n = 3 l = 1 m_l = −1
E)n = 3 l = 0 m_l = 1

Question 66

The orientation in space of an atomic orbital is associated with

A)the principal quantum number ( n).
B)the angular momentum quantum number ( l).
C)the magnetic quantum number ( m_l)_.
D)the spin quantum number ( m_s)_.
E)None of these choices are correct.

Question 67

The energy of an electron in the hydrogen atom is determined by

A)the principal quantum number ( n)only.
B)the angular momentum quantum number ( l)only.
C)the principal and angular momentum quantum numbers ( n & l ).
D)the principal and magnetic quantum numbers ( n & m_l)_.
E)the principal, angular momentum and magnetic quantum numbers.

Question 68

Which of the following is a correct set of quantum numbers for an electron in a 5f orbital?

A)n = 5, l = 3, m_l = +1
B)n = 5, l = 2, m_l = +3
C)n = 4, l = 3, m_l = 0
D)n = 4, l = 2, m_l = +1
E)n = 5, l = 4, m_l = 3

Question 69

Which of the following is a correct set of quantum numbers for an electron in a 3d orbital?

A)n = 3, l = 0, m_l = −1
B)n = 3, l = 1, m_l = +3
C)n = 3, l = 2, m_l = 3
D)n = 3, l = 3, m_l = +2
E)n = 3, l = 2, m_l = −2