Deck 29: Atoms and Molecules

Question 1

Which of the following values can be taken by the electron spin quantum number, m_s?

A) ±1/2
B) 0
C) ±1
D) ±2
E) ±3

Answer 1

A

Question 2

The principal quantum number n can have any integer value ranging from

A) -∞ to +∞.
B) 0 to ∞.
C) 1 to ∞.
D) 1 to 100.

Answer 2

C

Question 3

Which of the following statements are true for the Bohr model of the atom? (There could be more than one correct choice.)

A) The spacing between all the electron shells is the same.
B) The energy difference between all the electron shells is the same.
C) As we look at higher and higher electron shells, they get closer and closer together, but the difference in energy between them gets greater and greater.
D) As we look at higher and higher electron shells, they get farther and farther apart, but the difference in energy between them gets smaller and smaller.
E) There is no general pattern in the spacing of the shells or their energy differences.

Answer 3

D

Question 4

The Lyman series is formed by electron transitions in hydrogen that

A) end on the n = 1 shell.
B) begin on the n = 1 shell.
C) end on the n = 2 shell.
D) begin on the n = 2 shell.
E) are between the n = 1 and n = 3 shells.

Question 5

The orbital angular momentum quantum number can take which of the following values for any given value of the principal quantum number, n?

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

Question 6

According to the quantum mechanical model of the hydrogen atom, if the orbital angular momentum quantum number is ℓ, there will be how many permitted magnetic quantum numbers?

A) ℓ/2
B) 2ℓ
C) 2ℓ + 1
D) 2ℓ - 1
E) 3ℓ

Question 7

The energy difference between adjacent orbit radii in a hydrogen atom

A) increases with increasing values of n.
B) decreases with increasing values of n.
C) remains constant for all values of n.
D) varies randomly with increasing values of n.

Question 8

The distance between adjacent orbits in a hydrogen atom

A) increases with increasing values of n.
B) decreases with increasing values of n.
C) remains constant for all values of n.
D) varies randomly with increasing values of n.

Question 9

To which of the following values of n does the shortest wavelength in the Balmer series correspond?

A) 3
B) 5
C) 7
D) 1
E) ∞ (very large)

Question 10

Hydrogen atoms can emit four spectral lines with visible colors from red to violet. These four visible lines emitted by hydrogen atoms are produced by electrons

A) that start in the n = 2 level.
B) that end up in the n = 2 level.
C) that end up in the n = 3 level.
D) that end up in the ground state.
E) that start in the ground state.

Question 11

When an electron jumps from an orbit where n = 4 to one where n = 2

A) a photon is emitted.
B) a photon is absorbed.
C) two photons are emitted.
D) two photons are absorbed.
E) None of the given answers are correct.

Question 12

If a hydrogen atom originally in a state with principal quantum number n is excited to state n' = 2n, then

A) its radius and binding energy will double.
B) its radius will quadruple and the binding energy will double.
C) its radius will double and the binding energy will quadruple.
D) its radius will quadruple and the binding energy will be reduced by a factor of four.
E) its radius and binding energy will quadruple.

Question 13

To which of the following values of n does the longest wavelength in the Balmer series correspond?

A) 3
B) 5
C) 1
D) 7
E) ∞ (very large)

Question 14

According to Pauli's exclusion principle, how many electrons in an atom may have a particular set of quantum numbers?

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

Question 15

According to the quantum mechanical model of the hydrogen atom, if the principal quantum number is n, how many different orbital angular momentum quantum numbers are permitted?

A) n/2
B) n
C) 2n
D) 3n
E) 4n

Question 16

The orbital angular momentum quantum number ℓ can have any integer value ranging from

A) 0 to n.
B) 0 to (n-1).
C) 1 to n.
D) 1 to (n+1).
E) -n to n.

Question 17

The figure shows part of the energy level diagram of a certain atom. The energy spacing between levels 1 and 2 is twice that between 2 and 3. If an electron makes a transition from level 3 to level 2, the radiation of wavelength λ is emitted. What possible radiation wavelengths might be produced by other transitions between the three energy levels?

A) both λ/2 and λ/3
B) only λ/2
C) both 2λ and 3λ
D) only 2λ

Question 18

The Paschen series is formed by electron transitions that

A) end on the n = 1 shell.
B) begin on the n = 1 shell.
C) end on the n = 2 shell.
D) begin on the n = 3 shell.
E) end on the n = 3 shell.

Question 19

The Balmer series is formed by electron transitions in hydrogen that

A) end on the n = 1 shell.
B) begin on the n = 1 shell.
C) end on the n = 2 shell.
D) begin on the n = 2 shell.
E) are between the n = 1 and n = 3 shells.

Question 20

A hydrogen atom is in the 6h state. What is the principal quantum number.

A) 0
B) 3
C) 5
D) 6
E) 7

Question 21

The magnetic quantum number m₁ can have any integer value ranging from

A) -n to +n.
B) -ℓ to +ℓ.
C) 0 to n.
D) 0 to ℓ.
E) 0 to (n-1)

Question 22

What is the wavelength in the Balmer series for n = 15?

A) 277.1 nm
B) 371.1 nm
C) 188.6 nm
D) 656 nm
E) 754.2 nm

Question 23

If ℓ = 4, which one of the following is a possible quantum number for n?

A) 0
B) 2
C) 3
D) 4
E) 8

Question 24

What is the value of n in the Balmer series for which the wavelength is 410.2 nm.

A) 4
B) 5
C) 6
D) 7
E) 9

Question 25

If n = 5, which one of the following is not an allowed magnetic quantum number m₁?

A) 0
B) 2
C) 4
D) 5

Question 26

The elements in the periodic table that have completely filled shells or subshells are referred to as

A) noble gases.
B) halogens.
C) alkali metals.
D) transition elements.

Question 27

What value of n corresponds to a wavelength of 91.7 nm in the Lyman series?

A) 1
B) 3
C) 5
D) 9
E) 13

Question 28

One of the emission lines described by the original version of Balmer's formula has wavelength What is the value of n in Balmer's formula that gives this emission line?

A) 11
B) 12
C) 13
D) 14

Question 29

In its ground state, the quantum numbers (n, ℓ, m₁, m_s) for hydrogen are, respectively,

A) 1, 1, 1, 1.
B) 1, 0, 0, 0.
C) 1, 0, 0, ±1/2.
D) 1, 1, 1, ±1/2.

Question 30

What is the longest wavelength in the Paschen series?

A) 2.01 nm
B) 2.01 μm
C) 365 nm
D) 1.88 nm
E) 1.88 μm

Question 31

Consider ground-state helium having two electrons in orbit. If one of the electrons has quantum numbers (n, ℓl, m₁, m_s) of 1, 0, 0, -1/2 respectively, the quantum numbers for the other electron will be

A) 1, 1, 0, -1/2.
B) 1, 0, 0, +1/2.
C) 1, 1, 1, +1/2.
D) none of the given answers.

Question 32

What is the longest wavelength in the Lyman Series?

A) 45.60 nm
B) 91.20 nm
C) 121.5 nm
D) 240.1 nm
E) 365 nm

Question 33

The value of a wavelength in the Balmer series is 372.1 nm. What is the corresponding value of n?

A) 6
B) 3
C) 9
D) 10
E) 14

Question 34

What value of n corresponds to a wavelength of 922.7 nm in the Paschen series?

A) 3
B) 5
C) 7
D) 9
E) 15

Question 35

What is the longest wavelength in the Balmer series?

A) 240 nm
B) 328 nm
C) 365 nm
D) 656 nm
E) 820 nm

Question 36

What is the shortest wavelength of the Lyman series?

A) 91.16 nm
B) 45.60 nm
C) 121.5 nm
D) 204.1 nm
E) 365 nm

Question 37

What is the shortest wavelength in the Paschen series?

A) 410.2 nm
B) 410.2 μm
C) 365 nm
D) 820.4 nm
E) 820.4 μm

Question 38

The electron spin quantum number can have values of

A) -1/2, -1, 0, +1, +1/2.
B) -1/2, -1, +1, +1/2.
C) -1/2, 0, +1/2.
D) -1/2, +1/2.
E) only +1/2.

Question 39

What is the shortest wavelength in the Balmer series?

A) 328 nm
B) 365 nm
C) 456 nm
D) 656 nm
E) 820 nm

Question 40

What is the atomic number of a neutral atom that has an electron configuration of 1s² 2s² 2p⁶ 3s² 3p²?

A) 5
B) 11
C) 14
D) 20

Question 41

A hydrogen atom makes a downward transition from the state to the state. Find the wavelength of the emitted photon. (c = 3.00 × 10⁸ m/s, 1 eV = 1.60 × 10^-19 J, h = 6.626 × 10^-34 J ∙ s)

A) 2.56 μm
B) 1.54 μm
C) 2.05 μm
D) 3.07 μm

Question 42

What is the energy of the photon emitted when an electron drops from the state to the state in a hydrogen atom?

A) 0.244 eV
B) 0.264 eV
C) 0.283 eV
D) 0.303 eV

Question 43

The shortest wavelength of a photon that can be emitted by a hydrogen atom, for which the initial state is is closest to which one of the following values?

A) 92 nm
B) 82 nm
C) 72 nm
D) 62 nm
E) 52 nm

Question 44

In a hydrogen atom, the electron makes a transition from the n = 8 to the n = 3 state. The wavelength of the emitted photon is closest to which one of the following values? (c = 3.00 × 10⁸ m/s, 1 eV = 1.60 × 10^-19 J, h = 6.626 × 10^-34 J ∙ s)

A) 9.57 × 10^-7 m
B) 1.13 × 10^-6 m
C) 3.12 × 10^-7 m
D) 4.52 × 10^-6 m
E) 6.34 × 10^-7 m

Question 45

Given that the binding energy of the hydrogen atom in its ground state is -13.6 eV, what is the energy when it is in the n = 5 state?

A) 2.72 eV
B) -2.72 eV
C) 0.544 eV
D) -0.544 eV

Question 46

The longest wavelength of a photon that can be emitted by a hydrogen atom, for which the initial state is n = 3, is closest to which one of the following values? (c = 3.00 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s, 1 eV = 1.60 × 10^-19 J)

A) 550 nm
B) 575 nm
C) 600 nm
D) 625 nm
E) 658 nm

Question 47

Given that the energy levels of the hydrogen atom are given by E_n = , where R = 1.097 × 10⁷ m^-1, what wavelength photon is emitted when the atom undergoes a transition from the n = 4 to the n = 6 level?

Question 48

A hydrogen atom is excited to the n = 9 level. Its decay to the n = 6 level detected in a photographic plate. What is the frequency of the light photographed? (1 eV = 1.60 × 10^-19 J, h = 6.626 × 10^-34 J ∙ s)

A) 5.08 × 10¹³ Hz
B) 5910 Hz
C) 5910 nm
D) 3.28 × 10^-9 km

Question 49

A hydrogen atom is excited to the n = 11 level. Its decay to the n = 7 level is detected in a photographic plate. What is the wavelength of the light photographed? (c = 3.00 × 10⁸ m/s, 1 eV = 1.60 × 10^-19 J, h = 6.626 × 10^-34 J ∙ s)

A) 7510 nm
B) 4670 nm
C) 12,400 nm
D) 4380 nm

Question 50

The longest wavelength photon that can be emitted by a hydrogen atom, for which the final state is is closest to which one of the following values? (c = 3.0 × 10⁸ m/s,

A) 39,000 nm
B) 22,000 nm
C) 7400 nm
D) 16,000 nm
E) 28,000 nm

Question 51

What is the energy required to remove the electron from a hydrogen atom in the n = 11 state?

A) 0.112 eV
B) 1.24 eV
C) 13.5 eV
D) 12.4 eV
E) 0.141 eV

Question 52

Light shines through atomic hydrogen gas that was initially in its ground state. You observe that after awhile much of the hydrogen gas has been excited to its n = 5 state. What wavelength of light entering the gas caused this excitation? (c = 3.00 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s, 1 eV = 1.60 × 10^-19 J)

A) 110 nm
B) 91.4 nm
C) 95.2 nm
D) 2280 nm

Question 53

If a hydrogen atom in the ground state absorbs a photon of energy 12.09 eV, to which state will the electron make a transition?

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

Question 54

What is the ionization energy of the neutral hydrogen atom?

A) 27.2 eV
B) 13.6 eV
C) 6.8 eV
D) none of the given answers

Question 55

The wavelength of a ruby laser is 694.3 nm. What is the energy difference between the two energy states for the transition that produces this light? (c = 3.00 × 10⁸ m/s, 1 eV = 1.60 × 10^-19 J, h = 6.626 × 10^-34 J ∙ s)

A) 1.54 eV
B) 1.65 eV
C) 1.79 eV
D) 1.81 eV

Question 56

What is the energy (in electron-volts) of the n = 3 state of atomic hydrogen?

Question 57

If light excites atomic hydrogen from its lowest energy level to the n = 12 level, what is the energy of the photons of this light?

A) 13.5 eV
B) 32.2 eV
C) 13.6 eV
D) 0.0944 eV
E) 1.13 eV

Question 58

What is the shortest wavelength of a photon that can be emitted by a hydrogen atom, for which the initial state is n = 3? (c = 3.00 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s, 1 eV = 1.60 × 10^-19 J)

A) 822 nm
B) 850 nm
C) 103 nm
D) 91.4 nm
E) 950 nm

Question 59

A hydrogen atom is in its n = 2 excited state when its electron absorbs in an interaction with a photon. What is the energy of the resulting free electron?

A) 6.1 eV
B) 7.9 eV
C) 8.2 eV
D) 9.2 eV

Question 60

Consider the Bohr model for the hydrogen atom. (c = 3.00 × 10⁸ m/s, 1 eV = 1.60 × 10^-19 J, h = 6.626 × 10^-34 J ∙ s)
(a) How much energy (in eV) is needed to cause a transition of an electron from the second excited state to the third excited state?
(b) What wavelength photon just has enough energy to initiate the transition in (a)?

Question 61

A hydrogen atom with a barely bound electron may have an average radius as large as a bacterium, which is a radius of What is the nearest principal quantum number of the atom in this state? The radius for ground state hydrogen is 0.0529 nm.

A) 514
B) 51
C) 16
D) 264,650

Question 62

What is the wavelength of the photon emitted when an electron in a hydrogen atom which is in the initial state n = 8 jumps to the final state n = 2? (c = 3.00 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s, 1 eV = 1.60 × 10^-19 J)

A) 205 nm
B) 104 nm
C) 389 nm
D) 486 nm
E) 610 nm

Question 63

The only valid electron state and shell designation among the following is

A) 1p, K (n = 1) shell.
B) 2s, K (n = 1) shell.
C) 1s, L (n = 2) shell.
D) 2p, L (n = 2) shell.
E) 3f, M (n = 3) shell.

Question 64

An atom has completely filled inner shells and a single valence electron in an excited p state. The filled inner shells have an orbital momentum equal to zero. What is the magnitude of the orbital angular momentum of the atom?

A) 1.0
B) 1.2
C) 1.4
D) 1.7
E) 2.0

Question 65

Write out the electron configuration for the ground state of the phosphorus atom, which has 15 electrons.

Question 66

For an electron in the M (n = 3) shell, find (a) the largest possible orbital angular momentum it can have, and (b) the smallest possible orbital angular momentum it can have. Express your answers in SI units, and for each case indicate the subshell (s, p, d, ...) of the electron. (h = 6.626 × 10^-34 J ∙ s)

Question 67

Consider the n = 10 shell.
(a) What is the largest value of the angular momentum quantum number, ℓ, in this shell?
(b) How many electrons can be placed in this shell?

Question 68

An atom with atomic number 6 is in its ground state. How many electrons are in its outermost shell?

Question 69

In a transition from one vibrational state to another, a molecule emits a photon of wavelength 5.56 µm. What is the energy difference between these two states? (c = 3.00 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s, 1 eV = 1.60 × 10^-19 J)

A) 0.223 eV
B) 2.23 MeV
C) 13.6 eV
D) 13.6 MeV
E) 0.223 MeV

Question 70

In making a transition from state n = 1 to state n = 2, the hydrogen atom must

A) absorb a photon of energy 10.2 eV.
B) emit a photon of energy 10.2 eV.
C) absorb a photon of energy 13.58 eV.
D) emit a photon of energy 13.58 eV.

Question 71

What is the wavelength of the emitted photon if an electron in the hydrogen atom makes a transition from the n = 7 state to the n = 2 state? (c = 3.00 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s, 1 eV = 1.60 × 10^-19 J)

A) 199 nm
B) 365 nm
C) 4480 nm
D) 398 nm
E) 796 nm

Question 72

What is the greatest magnitude of the orbital angular momentum L that you can find in a state with

A) 5.48
B) 5.92
C) 6
D) 6.48

Question 73

In the n = 1 state, the energy of the hydrogen atom is -13.6 eV. What is its energy in the n = 2 state?

A) -6.79 eV
B) -4.53 eV
C) -3.40 eV
D) -1.51 eV

Question 74

What is the wavelength of the photon emitted when an electron in a hydrogen atom which is in the initial state n = 4 jumps to the final state n = 2? (c = 3.00 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s, 1 eV = 1.60 × 10^-19 J)

A) 243 nm
B) 486 nm
C) 556 nm
D) 312 nm
E) 609 nm

Question 75

What frequency must a photon have to raise an electron in a hydrogen atom from the n = 2 to the n = 4 state? (h = 6.626 × 10^-34 J ∙ s, 1 eV = 1.60 × 10^-19 J)

A) 3.06 × 10¹⁴ Hz
B) 6.16 × 10¹⁴ Hz
C) 4.11 × 10¹⁴ Hz
D) 5.20 × 10¹⁴ Hz
E) 9.24 × 10¹⁴ Hz

Question 76

The wavelength of the emitted photon if an electron in the hydrogen atom makes a transition from the n = 2 state to the ground state is closest to which of the following values? (c = 3.0 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s, 1 eV = 1.60 × 10^-19 J)

A) 122 nm
B) 203 nm
C) 243 nm
D) 389 nm
E) 411 nm

Question 77

Consider the Bohr model for the hydrogen atom in its second excited state.
(a) Determine the binding energy (eV) of the electron.
(b) What is the radius of the electron orbit, given that r₁ = 0.0529 nm?
(c) How far is it from the next higher excited orbit?

Question 78

Given that the speed of an electron in the ground state of hydrogen is 2190 km/s, what is the speed of an electron in the n = 4 orbit of hydrogen?

A) 547 km/s
B) 31,000 km/s
C) 139 km/s
D) 178 km/s
E) 2180 km/s

Question 79

Calculate the orbital Bohr radius of the excited state in a hydrogen atom.

A) 0.212 nm
B) 0.106 nm
C) 0.170 nm
D) 0.244 nm

Question 80

Radio astronomers often study the radiation emitted by a hydrogen atom from a transition between the two hyperfine levels associated with the ground state. This radiation has a wavelength of 21 cm. What is the energy difference between the hyperfine levels? (1 eV = 1.60 × 10^-19 J)

A) 5.9 × 10^-6 eV
B) 5.9 × 10^-25 J
C) 1.7 × 10^-24 J
D) 4.7 × 10^-25 J