Question 1

The ground-state electron configuration of Cr, Mo, and Ag are exceptions to the Aufbau principle. Which of the following is the electron configuration for Mo?

Accepted Answer

A)  [Kr]5s14d5
B)  [Kr]5s24d4
C)  [Xe]6s25d4
D)  [Ar]4s24d4
E)  [Kr]5s24d6F) B) and E)
G) All of the above

Question 2

A photovoltaic cell converts light into electrical energy. Suppose a certain photovoltaic cell is only 63.5% efficient, in other words, that 63.5% of the light energy is ultimately recovered. If the energy output of this cell is used to heat water, how many 520 nm photons must be absorbed by the photovoltaic cell in order to heat 10.0 g of water from 20.0°C to 30.0°?

Accepted Answer

1.72 * 10<...

Question 3

The electron in a hydrogen atom falls from an excited energy level to the ground state in two steps, causing the emission of photons with wavelengths of 1870 and 102.5 nm. What is the quantum number of the initial excited energy level from which the electron falls?

Accepted Answer

A)  2
B)  3
C)  4
D)  6
E)  8F) A) and C)
G) A) and E)

Question 4

Calculate the wavelength associated with a 20Ne+ ion moving at a velocity of 2.0 * 105 m/s. The atomic mass of Ne-20 is 19.992 amu.

Accepted Answer

A)  1.0 * 10-13 m
B)  1.0 * 10-16 m
C)  1.0 * 10-18 m
D)  9.7 * 1012 m
E)  2.0 * 10-13 cmF) None of the above
G) A) and E)

Question 5

Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level. Recall that for hydrogen En = -2.18 * 10 -18 J(1/n2)

Accepted Answer

A)  3.08 * 1015 /s
B)  1.03 * 108 /s
C)  2.06 * 1014 /s
D)  1.35 * 10-51 /s
E)  8.22 * 1014 /sF) A) and E)
G) A) and C)

Question 6

A ground-state atom of iron has ___ unpaired electrons and is _____.

Accepted Answer

A)  0, diamagnetic
B)  6, diamagnetic
C)  3, paramagnetic
D)  5, paramagnetic
E)  4, paramagneticF) B) and E)
G) A) and B)

Question 7

Which of the following is the electron configuration of an excited state of a copper atom?

Accepted Answer

A)  [Ar]4s23d9
B)  [Ar]4s13d10
C)  [Ar]4s13d8
D)  [Ar]4s23d8
E)  [Ar]4s03d10F) A) and E)
G) A) and B)

Question 8

What is the binding energy (in J/mol or kJ/mol) of an electron in a metal whose threshold frequency for photoelectrons is 2.50 * 1014 /s?

Accepted Answer

A)  99.7 kJ/mol
B)  1.66 * 10-19 J/mol
C)  2.75 * 10-43 J/mol
D)  7.22 * 1017 kJ/mol
E)  1.20 * 10-6 J/molF) A) and B)
G) B) and D)

Question 9

The orbital diagram for a ground-state nitrogen atom is

Accepted Answer

A)   
B)   
C)   
D)   E) A) and D)
F) B) and D)

Question 10

The electron configuration of a ground-state Co atom is

Accepted Answer

A)  [Ar]4s23d7.
B)  1s22s22p63s23d9.
C)  [Ne]3s23d7.
D)  [Ar]4s13d5.
E)  [Ar]4s24d7.F) A) and B)
G) A) and C)

Question 11

Which of the following is the electron configuration of an excited state of an iron atom?

Accepted Answer

A)  [Ar]4s23d7
B)  [Ar]4s23d6
C)  [Ar]4s23d8
D)  [Ar]4s13d7
E)  [Ar]4s13d5F) B) and D)
G) A) and B)

Question 12

According to de Broglie's equation, the wavelength associated with the motion of a particle increases as the particle mass decreases.

Accepted Answer

A) True 
 B)False

Question 13

If we take away two electrons from the outer shell of calcium, it would have the same electron configuration as what element?

Accepted Answer

The answer of If we take away two electrons from...

Question 14

Calculate the wavelength of a neutron that has a velocity of 250 cm/s. (The mass of a neutron = 1.675 * 10-24 g; h = 6.626 * 10-34 J.s)

Accepted Answer

A)  16 pm
B)  0.016 nm
C)  0.16 nm
D)  160 nm
E)  1.6 * 10-4 mF) A) and E)
G) A) and B)

Question 15

Which one of the following sets of quantum numbers is not possible?

Accepted Answer

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

Question 16

A ground-state chromium atom has how many unpaired electrons?

Accepted Answer

A)  1
B)  2
C)  4
D)  5
E)  6F) A) and B)
G) A) and C)

Question 17

Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 6 to the n = 3 principal energy level. Recall that for hydrogen En = -2.18 * 10-18 J(1/n2) .

Accepted Answer

A)  1.64 * 1015 /s
B)  9.13 * 1013 /s
C)  3.65 * 1014 /s
D)  1.82 * 10-19 /s
E)  2.74 * 1014/sF) A) and E)
G) All of the above

Question 18

Which ground-state atom has an electron configuration described by the following orbital diagram?

Accepted Answer

A)  phosphorus
B)  germanium
C)  selenium
D)  tellurium
E)  none of theseF) B) and C)
G) A) and D)

Question 19

Calculate the wavelength, in nanometers, of the light emitted by a hydrogen atom when its electron falls from the n = 7 to the n = 4 principal energy level. Recall that the energy levels of the H atom are given by En = -2.18 * 10-18 J(1/n2)

Accepted Answer

A)  4.45 * 10-20 nm
B)  2.16 * 10-6 nm
C)  9.18 * 10-20 nm
D)  1.38 * 1014 nm
E)  2.16 * 103 nmF) D) and E)
G) A) and B)

Question 20

A photon is roughly 1800 times more massive than an electron. If a proton and an electron have the same kinetic energy,

Accepted Answer

A)  the wavelength of the photon will be about 1800 times longer than the wavelength of the electron.
B)  the wavelength of the photon will be about  times longer than the wavelength of the electron.
C)  the wavelength of the photon will be roughly equal to the wavelength of the electron.
D)  the wavelength of the electron will be about  times longer than the wavelength of the photon.
E)  the wavelength of the electron will be about 1800 times longer than the wavelength of the photon.F) B) and D)
G) B) and C)

Exam 7: The Electronic Structure of Atoms

A ground-state chromium atom has how many unpaired electrons?

Correct Answer
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If we take away two electrons from the outer shell of calcium, it would have the same electron configuration as what element?

Correct Answer
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Which one of the following sets of quantum numbers is not possible?

Correct Answer
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Which of the following is the electron configuration of an excited state of an iron atom?

Correct Answer
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The orbital diagram for a ground-state nitrogen atom is

Correct Answer
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The electron in a hydrogen atom falls from an excited energy level to the ground state in two steps, causing the emission of photons with wavelengths of 1870 and 102.5 nm. What is the quantum number of the initial excited energy level from which the electron falls?

Correct Answer
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The ground-state electron configuration of Cr, Mo, and Ag are exceptions to the Aufbau principle. Which of the following is the electron configuration for Mo?

Correct Answer
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Calculate the wavelength of a neutron that has a velocity of 250 cm/s. (The mass of a neutron = 1.675 * 10^-24 g; h = 6.626 * 10^-34 J.s)

Correct Answer
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Correct Answer
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1.72 * 10<...
View Answer

A ground-state atom of iron has _ unpaired electrons and is ___.

Correct Answer
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Which ground-state atom has an electron configuration described by the following orbital diagram?

Correct Answer
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A photon is roughly 1800 times more massive than an electron. If a proton and an electron have the same kinetic energy,

Correct Answer
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Calculate the wavelength associated with a ²⁰Ne⁺ ion moving at a velocity of 2.0 * 10⁵ m/s. The atomic mass of Ne-20 is 19.992 amu.

Correct Answer
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Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level. Recall that for hydrogen E_n = -2.18 * 10^-18 J(1/n²)

Correct Answer
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According to de Broglie's equation, the wavelength associated with the motion of a particle increases as the particle mass decreases.

Correct Answer
verified

The electron configuration of a ground-state Co atom is

Correct Answer
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Which of the following is the electron configuration of an excited state of a copper atom?

Correct Answer
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What is the binding energy (in J/mol or kJ/mol) of an electron in a metal whose threshold frequency for photoelectrons is 2.50 * 10¹⁴/s?

Correct Answer
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Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 6 to the n = 3 principal energy level. Recall that for hydrogen E_n = -2.18 * 10^-18 J(1/n²) .

Correct Answer
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Calculate the wavelength, in nanometers, of the light emitted by a hydrogen atom when its electron falls from the n = 7 to the n = 4 principal energy level. Recall that the energy levels of the H atom are given by E_n = -2.18 * 10^-18 J(1/n²)

Correct Answer
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Exam 7: The Electronic Structure of Atoms

A ground-state chromium atom has how many unpaired electrons?

Correct AnswerverifiedShow Answer

If we take away two electrons from the outer shell of calcium, it would have the same electron configuration as what element?

Correct AnswerverifiedShow Answer

Which one of the following sets of quantum numbers is not possible?

Correct AnswerverifiedShow Answer

Which of the following is the electron configuration of an excited state of an iron atom?

Correct AnswerverifiedShow Answer

The orbital diagram for a ground-state nitrogen atom is

Correct AnswerverifiedShow Answer

The electron in a hydrogen atom falls from an excited energy level to the ground state in two steps, causing the emission of photons with wavelengths of 1870 and 102.5 nm. What is the quantum number of the initial excited energy level from which the electron falls?

Correct AnswerverifiedShow Answer

The ground-state electron configuration of Cr, Mo, and Ag are exceptions to the Aufbau principle. Which of the following is the electron configuration for Mo?

Correct AnswerverifiedShow Answer

Calculate the wavelength of a neutron that has a velocity of 250 cm/s. (The mass of a neutron = 1.675 * 10-24 g; h = 6.626 * 10-34 J.s)

Correct AnswerverifiedShow Answer

Correct Answerverified1.72 * 10<...View AnswerShow Answer

A ground-state atom of iron has ___ unpaired electrons and is _____.

Correct AnswerverifiedShow Answer

Which ground-state atom has an electron configuration described by the following orbital diagram?

Correct AnswerverifiedShow Answer

A photon is roughly 1800 times more massive than an electron. If a proton and an electron have the same kinetic energy,

Correct AnswerverifiedShow Answer

Calculate the wavelength associated with a 20Ne+ ion moving at a velocity of 2.0 * 105 m/s. The atomic mass of Ne-20 is 19.992 amu.

Correct AnswerverifiedShow Answer

Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level. Recall that for hydrogen En = -2.18 * 10 -18 J(1/n2)

Correct AnswerverifiedShow Answer

According to de Broglie's equation, the wavelength associated with the motion of a particle increases as the particle mass decreases.

Correct AnswerverifiedShow Answer

The electron configuration of a ground-state Co atom is

Correct AnswerverifiedShow Answer

Which of the following is the electron configuration of an excited state of a copper atom?

Correct AnswerverifiedShow Answer

What is the binding energy (in J/mol or kJ/mol) of an electron in a metal whose threshold frequency for photoelectrons is 2.50 * 1014 /s?

Correct AnswerverifiedShow Answer

Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 6 to the n = 3 principal energy level. Recall that for hydrogen En = -2.18 * 10-18 J(1/n2) .

Correct AnswerverifiedShow Answer

Calculate the wavelength, in nanometers, of the light emitted by a hydrogen atom when its electron falls from the n = 7 to the n = 4 principal energy level. Recall that the energy levels of the H atom are given by En = -2.18 * 10-18 J(1/n2)

Correct AnswerverifiedShow Answer

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
verified

Calculate the wavelength of a neutron that has a velocity of 250 cm/s. (The mass of a neutron = 1.675 * 10^-24 g; h = 6.626 * 10^-34 J.s)

Correct Answer
verified

Correct Answer
verified
1.72 * 10<...
View Answer

A ground-state atom of iron has _ unpaired electrons and is ___.

Correct Answer
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Correct Answer
verified

Correct Answer
verified

Calculate the wavelength associated with a ²⁰Ne⁺ ion moving at a velocity of 2.0 * 10⁵ m/s. The atomic mass of Ne-20 is 19.992 amu.

Correct Answer
verified

Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level. Recall that for hydrogen E_n = -2.18 * 10^-18 J(1/n²)

Correct Answer
verified

Correct Answer
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Correct Answer
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Correct Answer
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What is the binding energy (in J/mol or kJ/mol) of an electron in a metal whose threshold frequency for photoelectrons is 2.50 * 10¹⁴/s?

Correct Answer
verified

Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 6 to the n = 3 principal energy level. Recall that for hydrogen E_n = -2.18 * 10^-18 J(1/n²) .

Correct Answer
verified

Calculate the wavelength, in nanometers, of the light emitted by a hydrogen atom when its electron falls from the n = 7 to the n = 4 principal energy level. Recall that the energy levels of the H atom are given by E_n = -2.18 * 10^-18 J(1/n²)

Correct Answer
verified