Question 1

How many electrons will fit into a 4f subshell?

Accepted Answer

A)  3 
B)  4 
C)  7 
D)  14 
A)  3 
B)  4 
C)  7 
D)  14

Question 2

Given that the energy levels of the hydrogen atom are given by En = $\frac { \text { Rch } } { n ^ { 2 } }$ , 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?

Accepted Answer

Question 3

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

Accepted Answer

A)  3 
B)  5 
C)  7 
D)  1 
E)  ∞ (very large) 
A)  3 
B)  5 
C)  7 
D)  1 
E)  ∞ (very large)

Question 4

What is the longest wavelength in the Paschen series?

Accepted Answer

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

Question 5

How many values of the magnetic quantum number, mℓ, are possible if the orbital angular momentum quantum number is ℓ = 2?

Accepted Answer

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

Question 6

What is the energy of the photon emitted when an electron drops from the n = 20 state to the n = 7 state in a hydrogen atom?

Accepted Answer

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

Question 7

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?

Accepted Answer

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

Question 8

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

Accepted Answer

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. 
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 9

What is the shortest wavelength in the Paschen series?

Accepted Answer

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

Question 10

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

Accepted Answer

A)  ±1/2 
B)  0 
C)  ±1 
D)  ±2 
E)  ±3 
A)  ±1/2 
B)  0 
C)  ±1 
D)  ±2 
E)  ±3

Question 11

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

Accepted Answer

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

Question 12

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

Accepted Answer

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

Question 13

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)

Accepted Answer

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

Question 14

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)

Accepted Answer

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

Question 15

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)

Accepted Answer

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

Question 16

How many unique quantum states correspond to the lowest possible energy level of an electron in the hydrogen atom?

Accepted Answer

A)  3 
B)  0 
C)  1 
D)  4 
E)  2 
A)  3 
B)  0 
C)  1 
D)  4 
E)  2

Question 17

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?

Accepted Answer

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

Question 18

One of the emission lines described by the original version of Balmer's formula has wavelength $377 \mathrm {~nm}$ What is the value of n in Balmer's formula that gives this emission line?

Accepted Answer

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

Question 19

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?

Accepted Answer

A)  1.0 $\frac { h } { 2 \pi }$ 
B)  1.2 $\frac { h } { 2 \pi }$ 
C)  1.4 $\frac { h } { 2 \pi }$ 
D)  1.7 $\frac { h } { 2 \pi }$ 
E)  2.0 $\frac { h } { 2 \pi }$ 
A)  1.0 $\frac { h } { 2 \pi }$ 
B)  1.2 $\frac { h } { 2 \pi }$ 
C)  1.4 $\frac { h } { 2 \pi }$ 
D)  1.7 $\frac { h } { 2 \pi }$ 
E)  2.0 $\frac { h } { 2 \pi }$

Question 20

What is the shortest wavelength in the Balmer series?

Accepted Answer

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

Exam 29: Atoms and Molecules

How many electrons will fit into a 4f subshell?

Given that the energy levels of the hydrogen atom are given by En = Rch n2\frac { \text { Rch } } { n ^ { 2 } }n2 Rch ​ , 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?

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

What is the longest wavelength in the Paschen series?

How many values of the magnetic quantum number, mℓ, are possible if the orbital angular momentum quantum number is ℓ = 2?

What is the energy of the photon emitted when an electron drops from the n = 20 state to the n = 7 state in a hydrogen atom?

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?

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

What is the shortest wavelength in the Paschen series?

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

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

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

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)

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)

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)

How many unique quantum states correspond to the lowest possible energy level of an electron in the hydrogen atom?

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?

One of the emission lines described by the original version of Balmer's formula has wavelength 377 nm377 \mathrm {~nm}377 nm What is the value of n in Balmer's formula that gives this emission line?

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?

What is the shortest wavelength in the Balmer series?

Representing Motion

Motion in One Dimension

Vectors and Motion in Two Dimensions

Forces and Newtons Laws of Motion

Applying Newtons Laws

Gravity

Rotational Motion

Equilibrium Ad Elasticity

Momentum

Energy and Work

Using Energy

Thermal Properties of Matter

Fluids

Oscillations

Traveling Waves and Sound

Superposition and Standing Waves

Wave Optics

Ray Optics

Optical Instruments

Electric Fields and Forces

Electric Potential

Current and Resistance

Circuits

Magnetic Fields and Forces

EM Induction and Em Waves

AC Electricity

Relativity

Quantum Physics

Nuclear Physics

Filters

Given that the energy levels of the hydrogen atom are given by E_n = $\frac { \text { Rch } } { n ^ { 2 } }$ , 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?

How many values of the magnetic quantum number, m_ℓ, are possible if the orbital angular momentum quantum number is ℓ = 2?

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

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

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^-19J)

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^-19J)

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^-19J)

One of the emission lines described by the original version of Balmer's formula has wavelength $377 \mathrm {~nm}$ What is the value of n in Balmer's formula that gives this emission line?