Deck 32: Electromagnetic Waves Optics

Question 1

Quantum numbers: An electron in a hydrogen atom is in the n = 7 shell. How many possible values of the orbital quantum number l could it have?

A) 6
B) 7
C) 15
D) 33
E) 98

Answer 1

7

Question 2

Quantum numbers: For each value of the principal quantum number n, what are the possible values of the electron spin quantum number m_s? (There may be more than one correct choice.)

A) 0
B) +1/2
C) -1/2
D) +3/2
E) -3/2

Answer 2

+1/2
-1/2

Question 3

Multielectron atoms: An electron initially in a 4p state decays to a lower energy state. Which energy state is forbidden?

A) 3d
B) 2p
C) 2s
D) 1s

Answer 3

2p

Question 4

Quantum numbers: If the principal quantum number of an electron is n = 5, which one of the following is NOT an allowed magnetic quantum number m_l for the electron?

A) 0
B) 2
C) 3
D) 4
E) 5

Question 5

Quantum numbers: If the orbital quantum number is l = 4, which one of the following is a possible value for the principal quantum number n?

A) 1
B) 2
C) 3
D) 4
E) 8

Question 6

Hydrogen atom: 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
E) -68 eV

Question 7

Quantum numbers: An electron in a hydrogen atom has orbital quantum number l = 7. How many possible values of the magnetic quantum number m_l could it have?

A) 6
B) 7
C) 15
D) 33
E) 98

Question 8

Multielectron atoms: Which of the following electron transitions is forbidden?

A) 3s → 2p
B) 3d → 2p
C) 3d → 1s
D) 4p → 1s

Question 9

Lasers: Which of the following are characteristics of laser light? (There may be more than one correct choice.)

A) It is coherent.
B) It is produced by an inverted population of atoms.
C) It contains a full spectrum of wavelengths.

Question 10

Multielectron atoms: What element has a K_α line with wavelength 1.46 × 10^-11 m?

A) Zirconium
B) Niobium
C) Uranium
D) Protactinium

Question 11

Quantum numbers: If an electron has spin quantum number m_s = - , what is the possible value for the orbital quantum number l of the electron?

A) 0
B) 1
C) 2
D) 11
E) All of the above numbers are possible.

Question 12

Hydrogen atom: What is the minimum speed needed by a ground-state hydrogen atom for its kinetic energy to be enough to ionize the atom in a collision? (1 eV = 1.60 × 10^-19 J, m_h ≈ m_proton = 1.67 × 10^-27 kg)

A) 44.2 km/s
B) 21.7 km/s
C) 66.5 km/s
D) 113 km/s
E) 51.0 km/s

Question 13

Zeeman effect: Electrons in the presence of a magnetic field transition from 4p energy states to 3d states. How many different spectral lines could be observed from these transitions?

A) one
B) two
C) three
D) five

Question 14

Quantum numbers: An electron in a hydrogen atom has principal quantum number n = 4. How many possible values of the orbital quantum number l could it have?

A) 8
B) 9
C) 3
D) 4
E) 10

Question 15

Hydrogen atom: The normalized wave function for a hydrogen atom in the 1s state is given by ψ(r) = e^-r/α₀ where α₀ is the Bohr radius, which is equal to 5.29 × 10^-11 m. What is the probability of finding the electron at a distance greater than 7.8 α₀ from the proton?

A) 2.3 × 10^-5
B) 1.2 × 10^-5
C) 1.7 × 10^-5
D) 4.6 × 10^-5
E) 3.5 × 10^-5

Question 16

Hydrogen atom: How fast must a hydrogen atom be traveling for its kinetic energy to be just enough to excite the ground-state atom to its first excited state in a collision? (1 eV = 1.60 × 10^-19 J, m_h ≈ m_proton = 1.67 × 10^-27 kg)

A) 44.2 km/s
B) 21.7 km/s
C) 66.5 km/s
D) 113 km/s
E) 51.0 km/s

Question 17

Quantum numbers: In the ground state, the quantum numbers (n, l, m_l, m_s) for hydrogen are, respectively

A) 1, 1, 1, 1.
B) 1, 0, 0, 0.
C) 1, 0, 0, ± .
D) 1, 1, 1, ± .
E) 1, 1, 0, ±

Question 18

Hydrogen atom: What is the energy of an incident photon that is just enough to excite a hydrogen atom from its ground state to its n = 4 state?

A) 12.75 eV
B) 10.20 eV
C) 3.40 eV
D) 0.85 eV

Question 19

Quantum numbers: An electron in a hydrogen atom has orbital quantum number l = 4. How many possible values of the magnetic quantum number m_l could it have?

A) 4
B) 10
C) 5
D) 9
E) 3

Question 20

Quantum numbers: Consider the four quantum numbers of an electron in an atom, n, l, m_l, and m_s. The energy of an electron in an isolated atom depends on

A) n only.
B) n and l only.
C) n, l, and m_l only.
D) l, m_l, and m_s only.
E) all four quantum numbers.

Question 21

Hydrogen atom: What is the radius of the smallest electron orbit in a singly-ionized helium atom?

A) 1.32 × 10^-11 m
B) 2.65 × 10^-11 m
C) 5.29 × 10^-11 m
D) 1.06 × 10^-10 m

Question 22

Multielectron atoms: The only VALID electron state and shell designation among the following is

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

Question 23

Multielectron atoms: 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. A magnetic field is applied, defining the z-axis along the field. Which of the following sets of angles are possible angles between the magnetic field and the orbital angular momentum?

A) 45°
B) 90°
C) 45°, 90°
D) 45°, 135°
E) 45°, 90°, 135°

Question 24

Multielectron atoms: Consider the n = 9 shell.
(a) What is the largest value of the orbital quantum number, l, in this shell?
(b) How many electrons can be placed in this shell?

Question 25

Multielectron atoms: An atom with 5 electrons is in its ground state. How many electrons are in its outermost shell?

Question 26

Multielectron atoms: What is the electron configuration for ground state Li, which has 3 electrons?

A) 1s³
B) 1s¹2s²
C) 1s²2s¹
D) 1s²1p¹
E) 1s¹1p²

Question 27

Multielectron atoms: How many electrons can be found with principal quantum number in a suitably heavy atom?

A) 18
B) 6
C) 20
D) 9

Question 28

Angular momentum: The magnitude of the orbital angular momentum L of an electron in a certain atom is equal to 3.464ħ. What is the orbital quantum number l of the electron?

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

Question 29

Angular momentum: The magnitude of the orbital angular momentum L of an electron in a certain atom is equal to 3.464ħ. Which of the following angles could NOT be the angle between the orbital angular momentum vector of the electron and an arbitrary z-direction?

A) 107°
B) 90.0°
C) 73.2°
D) 54.7°
E) 0.00°

Question 30

Multielectron atoms: The only INVALID electron state and shell designation among the following is

A) 1s, K.
B) 2s, L.
C) 2d, L.
D) 3s, M.
E) 3d, M.

Question 31

Multielectron atoms: 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 L of the atom?

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

Question 32

Multielectron atoms: The correct ground state electron configuration of boron, which has 5 electrons, is

A) 1s²2s²2p.
B) 1s²2s²2p³.
C) 1s²1p²2s.
D) 1s²2p²3s.
E) 1s²2p³.

Question 33

Multielectron atoms: A neutral atom has an electron configuration of 1s²2s²2p⁶3s²3p². How many protons does it have in its nucleus?

A) 5
B) 11
C) 14
D) 20
E) 26

Question 34

Angular momentum: The magnitude of the orbital angular momentum L of an electron in a certain atom is equal to 3.464ħ. Which one of the following numbers could be the principal quantum number n of the electron?

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

Question 35

Multielectron atoms: How many electrons does it take to fill the d subshell?

A) 10
B) 6
C) 14
D) 4
E) 8

Question 36

Multielectron atoms: How many possible sets of quantum numbers (electron states) are there in the 5f subshell?

A) 2
B) 6
C) 8
D) 10
E) 14

Question 37

Angular momentum: What is the greatest magnitude of the orbital angular momentum L for an electron in a state with principal quantum number

A) 4.47
B) 4.90
C) 5
D) 5.48

Question 38

Angular momentum: What is the greatest total angular momentum J for an electron in the n = 2 shell?

A) 1.9ħ
B) 2.5ħ
C) 0.50ħ
D) 3.5ħ
E) 1.5ħ

Question 39

Hydrogen atom: A muonic hydrogen atom is a proton orbited by a muon (a particle with the same charge as an electron and 207 times its mass) in which the mass of the muon is significant relative to the mass of the proton. What would be the radius of the smallest muon orbit in a muonic hydrogen atom?

A) 1.03 × 10^-8 m
B) 1.10 × 10^-8 m
C) 2.56 × 10^-13 m
D) 2.84 × 10^-13 m
E) 5.29 × 10^-11 m

Question 40

Hydrogen atom: Doubly-ionized lithium is a hydrogen-like ion, in which the nucleus with charge 3e is orbited by a single electron. What wavelength light would be emitted from Li⁺⁺ as the electron dropped from the n = 4 to the n = 3 orbit?

A) 16.9 µm
B) 1.88 µm
C) 470 nm
D) 208 nm

Question 41

Zeeman effect: The energy of an electron in the p-level of an atom is changed in the presence of a magnetic field of magnitude 4.6 T. What is the difference between the largest and smallest possible energies? (Bohr magneton = μ_B = 9.27 × 10^-24 J/T)

Question 42

Lasers: A collection of atoms has 20% of the sample in a state above the ground state. If these emit coherent radiation, what is the wavelength of the laser light produced? (c = 3.00 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s, 1 eV = 1.60 × 10^-19 J)

A) 210 nm
B) 91 nm
C) 340 nm
D) 34 nm

Question 43

Lasers: How many photons per second emerge from a laser of power with wavelength (c = 3.00 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s)

A) 6.09 × 10¹⁵ photons/s
B) 5.03 × 10¹² photons/s
C) 3.07 × 10¹⁵ photons/s
D) 3.07 × 10¹³ photons/s

Question 44

Zeeman effect: An s state (l = 0) energy level is split into two levels by an applied magnetic field. A photon of microwave radiation having frequency 60 GHz induces a transition between the two levels. What is the magnitude of the applied magnetic field? (h = 6.626 × 10^-34 J ∙ s, Bohr magneton = μ_B = 9.27 × 10^-24 J/T)

A) 2.1 T
B) 0.34 T
C) 1.2 T
D) 2.8 T
E) 13 T

Question 45

Multielectron atoms: What is the correct electronic configuration for ground state carbon, which has 6 electrons?

A) 1s²2s²2p²
B) 1s¹2p¹
C) 1s¹2s²2p¹
D) 1s¹2s¹2p¹
E) 1s²2s²2p⁴

Question 46

Zeeman effect: An alkali metal atom is in the ground state. The orbital angular momentum equals zero and the spin angular momentum is entirely due to the single valence electron. A magnetic field is applied that splits the ground state energy level into two levels, 65 μeV apart.A photon, absorbed by the atom, induces a transition between the two levels. What is the wavelength of the photon? (c = 3.00 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s, Bohr magneton = μ_B = 9.27 × 10^-24 J/T, 1 eV = 1.60 × 10^-19 J)

A) 19 mm
B) 25 mm
C) 31 mm
D) 38 mm
E) 41 mm

Question 47

Zeeman effect: An atom in a state with its orbital quantum number l = 1 decays to its ground state (with l = 0). A photon of wavelength 630.000 nm is emitted in the process. When the same process takes place in the presence of an intense magnetic field, the following change in the spectrum is observed. With the magnetic field present, one of the emitted lines observed now has a wavelength of 630.030 nm. Which of the following wavelengths would you expect to be also present?

A) 629.970 nm
B) 630.060 nm
C) 630.090 nm
D) 630.120 nm
E) 629.910 nm

Question 48

Lasers: The wavelength of a ruby laser is 694.3 nm. What is the energy difference between the two energy states involved in laser action? (c = 2.9979 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s, 1 eV = 1.6022 × 10^-19 J)

A) 1.537 eV
B) 1.646 eV
C) 1.786 eV
D) 1.812 eV
E) 3.572 eV

Question 49

Multielectron atoms: What is the correct electronic configuration for the ground state sodium atom, which has 11 electrons?

A) 1s¹2s²3p⁶2s²
B) 1s²2s¹3p⁶2s²
C) 1s¹2s²2p⁶
D) 1s²2s²2p⁶3s²
E) 1s²2s²2p⁶3s¹

Question 50

Lasers: You need 14 W of infrared laser light power with wavelength 1270 nm to bore a hole in a diamond. How many downward atomic transitions per second must occur in the laser if all of them result in light directed onto the diamond? (c = 3.00 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s)

A) 8.9 × 10¹⁹
B) 8.9 × 10¹⁸
C) 5.9 × 10¹⁹
D) 2.7 × 10¹⁸

Question 51

Zeeman effect: An alkali metal atom is in the ground state. The orbital angular momentum equals zero and the spin angular momentum is entirely due to the single valence electron. A magnetic field is applied that splits the ground state energy level into two levels, 27 μeV apart. What is the strength of the applied magnetic field? (h = 6.626 × 10^-34 J ∙ s, Bohr magneton = μ_B = 9.27 × 10^-24 J/T, 1 eV = 1.60 × 10^-19 J)

A) 0.23 T
B) 0.18 T
C) 0.29 T
D) 0.34 T
E) 0.40 T

Question 52

Multielectron atoms: What is the wavelength of the K_α line for Mercury?

A) 1.94 × 10^-11 m
B) 5.38 × 10^-12 m
C) 1.85 × 10^-11 m
D) 3.02 × 10^-12 m

Question 53

Lasers: In a ruby laser, an electron jumps from a higher energy level to a lower one. If the energy difference between the two levels is 1.8 eV, what is the wavelength of the emitted photon? (c = 3.00 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s, 1 eV = 1.60 × 10^-19 J)

A) 350 nm
B) 470 nm
C) 650 nm
D) 690 nm
E) 960 nm