Deck 7: The Quantum-Mechanical Model of the Atom

Question 1

Identify the colour that has a wavelength of 460 nm.

A) blue
B) green
C) red
D) yellow

Answer 1

blue

Question 2

Which of the following visible colours of light has the highest frequency?

A) green
B) red
C) blue
D) yellow
E) orange

Answer 2

blue

Question 3

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

Answer 3

infrared and ultraviolet

Question 4

The number of cycles that pass through a stationary point per unit time is called ________.

A) wavelength
B) amplitude
C) frequency
D) area
E) median

Question 5

Place the following types of electromagnetic radiation in order of increasing wavelength. ultraviolet light gamma rays radio waves

A) gamma rays < radio waves < ultraviolet light
B) radio waves < ultraviolet light < gamma rays
C) radio waves < gamma rays < ultraviolet light
D) ultraviolet light < gamma rays < radio waves
E) gamma rays < ultraviolet light < radio waves

Question 6

Which of the following visible colours of light has the longest wavelength?

A) blue
B) green
C) yellow
D) red
E) violet

Question 7

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

A) blue
B) violet
C) orange
D) green
E) yellow

Question 8

Place the following types of electromagnetic radiation in order of decreasing energy. ultraviolet light radio waves microwaves

A) radio waves > microwaves > ultraviolet light
B) ultraviolet light > microwaves > radio waves
C) radio waves > ultraviolet light > microwaves
D) ultraviolet light > radio waves > microwaves
E) microwaves > radio waves > ultraviolet light

Question 9

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

Question 10

Which of the following occurs as the energy of a photon increases?

A) The frequency decreases.
B) The speed increases.
C) The wavelength increases.
D) The wavelength gets shorter.

Question 11

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

Question 12

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

A) yellow
B) blue
C) orange
D) green
E) purple

Question 13

Food can be cooked by ________ radiation.

A) ultraviolet
B) gamma
C) microwave
D) X-ray
E) radio

Question 14

Calculate the frequency of the red light emitted by a neon sign with a wavelength of 659.9 nm.

A) 2.20 × 10¹⁴ s^-1
B) 1.98 × 10¹⁴ s^-1
C) 4.55 × 10¹⁴ s^-1
D) 5.05 × 10¹⁴ s^-1
E) 3.32 × 10¹⁴ s^-1

Question 15

A sunburn is caused by overexposure to ________ radiation.

A) ultraviolet
B) gamma
C) microwave
D) X-ray
E) radio

Question 16

Identify the colour that has a wavelength of 700 nm.

A) blue
B) green
C) red
D) yellow

Question 17

Which of the following occurs 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 occurs as the wavelength of a photon increases.

Question 18

Calculate the wavelength (in nm) of the red light emitted by a neon sign with a frequency of 4.74 × 10¹⁴ Hz.

A) 633 nm
B) 158 nm
C) 142 nm
D) 704 nm
E) 466 nm

Question 19

The vertical height of a wave is called ________.

A) wavelength
B) amplitude
C) frequency
D) area
E) median

Question 20

Place the following types of electromagnetic radiation in order of increasing frequency. visible light microwaves X-rays

A) microwaves < visible light < X-rays
B) X-rays < visible light < microwaves
C) microwaves < X-rays < visible light
D) X-rays < microwaves < visible light
E) visible light < X-rays < microwaves

Question 21

Calculate the energy of the red light emitted by a neon atom with a wavelength of 703 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

Question 22

Which of the following transitions (in a hydrogen atom) represent absorption of the smallest frequency photon?

A) n = 5 to n = 6
B) n = 5 to n = 4
C) n = 4 to n = 1
D) n = 1 to n = 3
E) n = 1 to n = 2

Question 23

Which of the following transitions (in a hydrogen atom) represent emission of the longest wavelength photon?

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

Question 24

Which of the following transitions represent the emission of a photon with the largest energy?

A) n = 2 to n = 1
B) n = 3 to n = 1
C) n = 6 to n = 3
D) n = 1 to n = 4
E) n = 2 to n = 5

Question 25

Calculate the frequency of the green light emitted by a hydrogen atom with a wavelength of 486.1 nm.

A) 1.462 × 10¹⁴ s^-1
B) 6.868 × 10¹⁴ s^-1
C) 4.332 × 10¹⁴ s^-1
D) 6.172 × 10¹⁴ s^-1
E) 1.626 × 10¹⁴ s^-1

Question 26

Calculate the wavelength of light absorbed by a hydrogen atom when an electron undergoes an n = 2 to n = 4 transmission.

A) 433.9 nm
B) 410.0 nm
C) 1093 nm
D) 486.0 nm
E) 3295 nm

Question 27

How much energy (in kJ) do 3.0 moles of photons, all with a wavelength of 655 nm, contain?

A) 183 kJ
B) 303 kJ
C) 394 kJ
D) 548 kJ
E) 254 kJ

Question 28

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

Question 29

How many photons are contained in a burst of yellow light (589 nm) from a sodium lamp that contains 609 kJ of energy?

A) 3.37 × 10¹⁹ photons
B) 3.06 × 10³⁰ photons
C) 1.80 × 10²⁴ photons
D) 4.03 × 10²⁸ photons
E) 2.48 × 10²⁵ photons

Question 30

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

Question 31

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 potassium metal is 1.76 × 10³ kJ mol^-1.

A) 147 nm
B) 68.0 nm
C) 113 nm
D) 885 nm
E) 387 nm

Question 32

Identify the colour of a flame test for sodium.

A) violet
B) red
C) white
D) yellow
E) blue

Question 33

Calculate the energy of the violet light emitted by a hydrogen atom with a wavelength of 410 nm.

A) 4.84 × 10^-19 J
B) 2.06 × 10^-19 J
C) 1.23 × 10^-19 J
D) 8.13 × 10^-19 J
E) 5.27 × 10^-19 J

Question 34

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

Question 35

Calculate the wavelength of light emitted from a hydrogen atom when an electron undergoes an n = 8 to n = 4 transmission.

A) 1940 nm
B) 2620 nm
C) 1.245 × 10³ nm
D) 3.178 × 10³ nm
E) 714.8 nm

Question 36

Identify the colour of a flame test for potassium.

A) violet
B) red
C) white
D) yellow
E) blue

Question 37

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 × 10^-18 J

Question 38

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^-1.

A) 7.87 × 10¹⁵ Hz
B) 4.74 × 10¹⁵ Hz
C) 2.11 × 10¹⁵ Hz
D) 1.27 × 10¹⁵ Hz
E) 6.19 × 10¹⁵ Hz

Question 39

Choose the transition (in a hydrogen atom) below which represents the absorption of the shortest wavelength photon.

A) n = 1 to n = 2
B) n = 2 to n = 3
C) n = 4 to n = 5
D) n = 6 to n = 3
E) n = 3 to n = 1

Question 40

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

Question 41

Determine the velocity of a marble (mass = 8.66 g) with a wavelength of 3.46 × 10^-33 m.

A) 45.2 m s^-1
B) 11.3 m s^-1
C) 22.1 m s^-1
D) 38.8 m s^-1
E) 52.9 m s^-1

Question 42

An electron initially in the n = 5 orbital of a hydrogen atom emits a photon with a wavelength of 1284 nm. Calculate the final orbital, n_f.

A) 1
B) 3
C) 2
D) 6
E) 4

Question 43

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

Question 44

An electron ends in orbital n = 4 after a hydrogen atom emits a photon with a wavelength of 2165 nm. Calculate the initial orbital, n_i.

A) 6
B) 7
C) 1
D) 3
E) 2

Question 45

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

Question 46

An electron ends in orbital n = 3 after a hydrogen atom emits a photon with a wavelength of 1093 nm. Calculate the initial orbital, n_i.

A) 1
B) 5
C) 2
D) 3
E) 6

Question 47

Calculate the energy associated with an n = 2 to n = 5 transmission in a hydrogen atom.

A) 9.176 × 10^-20 J
B) 1.977 × 10^-19 J
C) 5.005 × 10^-19 J
D) 4.844 × 10^-19 J
E) 4.578 × 10^-19 J

Question 48

An electron ends in orbital n = 4 after a hydrogen atom absorbs a photon with a wavelength of 486 nm. Calculate the initial orbital, n_i.

A) 1
B) 5
C) 2
D) 3
E) 6

Question 49

An electron initially in the n = 2 orbital of a hydrogen atom absorbs a photon with a wavelength of 656 nm. Calculate the final orbital, n_f.

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

Question 50

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

Question 51

How much energy (in kJ) is required to ionize 2.78 moles of hydrogen atoms?

A) 2.74 × 10³ kJ
B) 4.72 × 10³ kJ
C) 1.66 × 10³ kJ
D) 3.65 × 10³ kJ
E) 5.89 × 10³ kJ

Question 52

Calculate the wavelength of an electron (m = 9.11 × 10^-28 g) moving at 3.66 × 10⁶ m s^-1.

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

Question 53

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

Question 54

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

Question 55

Calculate the wavelength of a baseball (m = 155 g) moving at 32.5 m s^-1.

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

Question 56

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

Question 57

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

Question 58

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

Question 59

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

Question 60

Calculate the final orbital, n_f, of an electron in a hydrogen atom that starts at orbital n = 4 and undergoes an energy transition of -1.06 × 10^-19 J.

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

Question 61

Calculate the de Broglie wavelength of a pen with a mass of 14.28 g travelling at 16.3 m s^-1.

A) 1.76 × 10^-31 m
B) 6.43 × 10^-37 m
C) 2.85 × 10^-33 m
D) 8.19 × 10^-32 m
E) 5.30 × 10^-34 m

Question 62

Calculate the orbital for the hydrogen atom that contains an electron with an energy of -2.42 × 10^-19 J.

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

Question 63

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.

Question 64

Calculate the orbital for the hydrogen atom that contains an electron with an energy of -4.45 × 10^-20 J.

A) n = 5
B) n = 4
C) n = 1
D) n = 3
E) n = 7

Question 65

Calculate the de Broglie wavelength of an egg with a mass of 60 g travelling at 32.18 m s^-1.

A) 5.0 × 10^-34 m
B) 2.8 × 10^-34 m
C) 4.9 × 10^-34 m
D) 1.2 × 10^-34 m
E) 3.4 × 10^-34 m

Question 66

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^-1
B) 12.3 m s^-1
C) 2.21 m s^-1
D) 4.98 m s^-1
E) 6.44 m s^-1

Question 67

Determine the mass of a ball with a wavelength of 3.45 × 10^-34 m and a velocity of 6.55 m s^-1.

A) 0.293 g
B) 12.6 g
C) 293 g
D) 346 g
E) 3.41 g

Question 68

Calculate the mass of a pickup truck travelling at 100.0 km h^-1 and a de Broglie wavelength of 1.24 × 10^-38 m.

A) 1924 kg
B) 1134 kg
C) 2347 kg
D) 2841 kg
E) 941.6 kg

Question 69

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

Question 70

Calculate the velocity of a pickup truck with a de Broglie wavelength of 1.27 × 10^-38 m and a mass of 2347 kg.

A) 88 km h^-1
B) 62.1 km h^-1
C) 94 km h^-1
D) 80.0 km h^-1
E) 106 km h^-1

Question 71

What are the possible orbitals for n = 3?

A) s, p, d
B) s, p, d, f
C) s
D) s, p

Question 72

Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error.

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

Question 73

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

Question 74

Calculate the energy of an electron in the orbital n = 5 of a hydrogen atom.

A) -1.08 × 10^-19 J
B) 8.72 × 10^-20 J
C) 1.08 × 10^-19 J
D) -8.72 × 10^-20 J
E) -7.21 × 10^-20 J

Question 75

For n = 3, what are the possible sublevels?

A) 0
B) 0, 1
C) 0, 1, 2
D) 0, 1,2, 3

Question 76

What value of l is represented by a d orbital?

A) 1
B) 2
C) 0
D) 3

Question 77

Determine the mass of a ball with a velocity of 35.1 m s^-1 and a wavelength of 8.92 × 10^-34 m.

A) 26.0 g
B) 594 g
C) 2.08 g
D) 47.3 g
E) 21.2 g

Question 78

Calculate the energy of an electron in the orbital n = 6 of a hydrogen atom.

A) 3.19 × 10^-20 J
B) 4.18 × 10^-20 J
C) -6.06 × 10^-20 J
D) -7.80 × 10^-20 J
E) -8.62 × 10^-20 J

Question 79

Each of the following sets of quantum numbers is supposed to specify an orbital. Which of the following sets of quantum numbers contains an error?

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

Question 80

Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error.

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