Question 1

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

Accepted Answer

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.F) A) and E)
G) None of the above

Question 2

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

Accepted Answer

A)   Einstein
B)   Planck
C)   Heisenberg
D)   Compton
E)   de BroglieF) A) and B)
G) None of the above

Question 3

The following combinations of quantum numbers are not allowed.

Accepted Answer

a. n = 3
b...

Question 4

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

Accepted Answer

A)   1.88 × 10-2 m
B)   0.330 m
C)   3.03 m
D)   5.33 × 102 m
E)   > 103 mF) All of the above
G) B) and D)

Question 5

Use the Bohr equation to calculate the energy of
a. the largest energy absorption or emission process involving the n = 2 state of the hydrogen atom.
b. the smallest energy absorption or emission process involving the n = 2 state of the hydrogen atom.

Accepted Answer

a. 1.64 × 10^-18 J (n = ...

Question 6

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

Accepted Answer

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 & ml) .
E)   the principal, angular momentum and magnetic quantum numbers.F) C) and E)
G) A) and E)

Question 7

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

Accepted Answer

A)   one
B)   two
C)   three
D)   four
E)   fiveF) B) and C)
G) None of the above

Question 8

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)

Accepted Answer

A)   2.056 × 106 s-1
B)   2.742 × 106 s-1
C)   6.165 × 1014 s-1
D)   8.226 × 1014 s-1
E)   > 1015 s-1F) C) and D)
G) A) and D)

Question 9

Platinum, which is widely used as a catalyst, has a work function  (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?

Accepted Answer

A)   2.196 × 10-7 m
B)   4.553 × 10-6 m
C)   5.654 × 102 m
D)   1.370 × 1015 m
E)   > 106 mF) B) and C)
G) A) and E)

Question 10

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?

Accepted Answer

A)   n = 1
B)   n = 2
C)   n = 3
D)   n = 4
E)   n = 5F) All of the above
G) A) and E)

Question 11

Atomic orbitals developed using quantum mechanics

Accepted Answer

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.F) C) and D)
G) B) and E)

Question 12

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

Accepted Answer

A)   Planck
B)   Einstein
C)   Bohr
D)   Rydberg
E)   de BroglieF) B) and D)
G) C) and D)

Question 13

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

Accepted Answer

The answer of In the quantum mechanical treatment of the...

Question 14

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

Accepted Answer

A) True 
 B)False

Question 15

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

Accepted Answer

A)   Planck
B)   de Broglie
C)   Bohr
D)   Rutherford
E)   RydbergF) A) and D)
G) A) and B)

Question 16

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?

Accepted Answer

A)   7.8 × 10-19 J
B)   3.3 J
C)   6.6 × 102 J
D)   3.3 × 103 J
E)   4.2 × 1018 JF) A) and C)
G) B) and D)

Question 17

a. Use Bohr's equation to calculate how much energy (in J) is needed to promote an electron from the H-atom ground state to the n = 4 level.
b. If a photon provides the energy in (a), what is its wavelength in nm?

Accepted Answer

a. 2.04 × ...

Question 18

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

Accepted Answer

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, ultravioletF) A) and E)
G) A) and D)

Question 19

a. Calculate the momentum of a photon of green light, wavelength 515 nm.
b. If this photon is traveling in a vacuum, what is its "mass"?

Accepted Answer

a. 1.29 × ...

Question 20

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

Accepted Answer

A)   n = 3 l = 1 ml = 2
B)   n = 1 l = 3 ml = 3
C)   n = 3 l = 2 ml = 1
D)   n = 3 l = 1 ml = -1
E)   n = 3 l = 0 ml = 1F) A) and E)
G) A) and D)

Exam 7: Quantum Theory and Atomic Structure

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

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

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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)

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Use the Bohr equation to calculate the energy of a. the largest energy absorption or emission process involving the n = 2 state of the hydrogen atom. b. the smallest energy absorption or emission process involving the n = 2 state of the hydrogen atom.

Correct Answerverifieda. 1.64 × 10-18 J (n = ...View AnswerShow Answer

a. Use Bohr's equation to calculate how much energy (in J) is needed to promote an electron from the H-atom ground state to the n = 4 level. b. If a photon provides the energy in (a), what is its wavelength in nm?

Correct Answerverifieda. 2.04 × ...View AnswerShow Answer

a. Calculate the momentum of a photon of green light, wavelength 515 nm. b. If this photon is traveling in a vacuum, what is its "mass"?

Correct Answerverifieda. 1.29 × ...View AnswerShow Answer

Atomic orbitals developed using quantum mechanics

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Platinum, which is widely used as a catalyst, has a work function  (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?

Correct AnswerverifiedShow Answer

The following combinations of quantum numbers are not allowed.

Correct Answerverifieda. n = 3b...View AnswerShow Answer

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

Correct AnswerverifiedShow Answer

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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)

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a. 1.64 × 10^-18 J (n = ...
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a. 2.04 × ...
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a. 1.29 × ...
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Platinum, which is widely used as a catalyst, has a work function  (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?

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a. n = 3
b...
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