Question 1

An electron in a 3p orbital could have a value of 2 for its angular momentum quantum number (l).

Accepted Answer

A) True 
 B)False

Question 2

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

Question 3

Which of the following, if any, is the proper rank the following types of electromagnetic radiation from lowest energy to highest energy

Accepted Answer

A)  Radio waves < microwaves < visible < infrared < ultraviolet < gamma rays 
B)  Microwaves < visible < ultraviolet < gamma rays < radio waves < infrared 
C)  Microwaves < radio waves < infrared < visible < ultraviolet < gamma rays 
D)  Radio waves < microwaves < infrared < visible < ultraviolet < gamma rays 
E)  None of the above 
A)  Radio waves < microwaves < visible < infrared < ultraviolet < gamma rays 
B)  Microwaves < visible < ultraviolet < gamma rays < radio waves < infrared 
C)  Microwaves < radio waves < infrared < visible < ultraviolet < gamma rays 
D)  Radio waves < microwaves < infrared < visible < ultraviolet < gamma rays 
E)  None of the above

Question 4

What is the wavelength (nm) for a photon of light with an energy of 3.20 x 10-19 J/photon

Accepted Answer

A)  621 nm 
B)  631 nm 
C)  641 nm 
D)  651 nm 
E)  None of the above 
A)  621 nm 
B)  631 nm 
C)  641 nm 
D)  651 nm 
E)  None of the above

Question 5

The colors of the visible spectrum are blue, green, orange, red, violet, and yellow. Of these colors, ______ has the least energy.

Accepted Answer

A)  Red 
B)  Yellow 
C)  Green 
D)  Indigo 
E)  Violet 
A)  Red 
B)  Yellow 
C)  Green 
D)  Indigo 
E)  Violet

Question 6

Which element has the following ground-state electron configuration
[Xe]6s24f145d4

Accepted Answer

A)  W 
B)  Pm 
C)  Mo 
D)  Np 
E)  Re 
A)  W 
B)  Pm 
C)  Mo 
D)  Np 
E)  Re

Question 7

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

Question 8

"No two electrons in an atom can have the same four quantum numbers" is a statement of

Accepted Answer

A)  the Pauli exclusion principle. 
B)  Bohr's equation. 
C)  Hund's rule. 
D)  de Broglie's relation. 
E)  Dalton's atomic theory. 
A)  the Pauli exclusion principle. 
B)  Bohr's equation. 
C)  Hund's rule. 
D)  de Broglie's relation. 
E)  Dalton's atomic theory.

Question 9

What is the wavelength of radiation that has a frequency of 3.4 x 1011 s -1

Accepted Answer

A)  8.8 x 10-4 nm 
B)  8.8 x 105 nm 
C)  8.8 x 10-13 nm 
D)  1.0 x 1011 nm 
E)  1.0 x 10-9 nm 
A)  8.8 x 10-4 nm 
B)  8.8 x 105 nm 
C)  8.8 x 10-13 nm 
D)  1.0 x 1011 nm 
E)  1.0 x 10-9 nm

Question 10

The longest wavelength of light that causes electrons to be ejected from the surface of a copper plate is 243 nm. What is the maximum velocity of the electrons ejected when light of wavelength 200. nm shines on a copper plate

Accepted Answer

A)  1.97 * 104 m/s 
B)  4.67 * 104 m/s 
C)  6.22 * 105 m/s 
D)  1.34 * 106 m/s 
E)  1.48 * 106 m/s 
A)  1.97 * 104 m/s 
B)  4.67 * 104 m/s 
C)  6.22 * 105 m/s 
D)  1.34 * 106 m/s 
E)  1.48 * 106 m/s

Question 11

How many unpaired electrons does an atom of carbon have in its ground state

Accepted Answer

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

Question 12

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

Accepted Answer

A)  antimony 
B)  germanium 
C)  indium 
D)  lead 
E)  tin 
A)  antimony 
B)  germanium 
C)  indium 
D)  lead 
E)  tin

Question 13

List the following sets of quantum numbers in order of increasing energy: 
I. n = 4, l = 0, ml = 0, ms = -1/2
II. n = 4, l = 2, ml = -1, ms = -1/2
III. n = 5, l = 0, ml = 0, ms = +1/2

Accepted Answer

A)  I < II < III 
B)  II < III < I 
C)  III < II < I 
D)  I < III < II 
E)  III < I < II 
A)  I < II < III 
B)  II < III < I 
C)  III < II < I 
D)  I < III < II 
E)  III < I < II

Question 14

The bonds of oxygen molecules are broken by sunlight. The minimum energy required to break the oxygen-oxygen bond is 495 kJ/mol. What is the wavelength of sunlight that can cause this bond breakage

Accepted Answer

A)  212 nm 
B)  222 nm 
C)  221 nm 
D)  242 nm 
E)  None of the above 
A)  212 nm 
B)  222 nm 
C)  221 nm 
D)  242 nm 
E)  None of the above

Question 15

A ground-state chromium atom has how many unpaired electrons

Accepted Answer

A)  1 
B)  2 
C)  4 
D)  5 
E)  6 
A)  1 
B)  2 
C)  4 
D)  5 
E)  6

Question 16

An electron loses energy in the transition from a 4f subshell to a 6s subshell.

Accepted Answer

A) True 
 B)False

Question 17

A possible set of quantum numbers to describe an electron in a 4s subshell is

Accepted Answer

A)  n = 4, l = 0, ml = 1 , ms = +1/2 
B)  n = 4, l = 0, ml = 0, ms = - 1/2 
C)  n = 4, l = 1, ml = 1, ms = +1/2 
D)  n = 3, l = 1, ml = 1, ms = - 1/2 
E)  n = 3, l = 0, ml = 0, ms = +1/2 
A)  n = 4, l = 0, ml = 1 , ms = +1/2 
B)  n = 4, l = 0, ml = 0, ms = - 1/2 
C)  n = 4, l = 1, ml = 1, ms = +1/2 
D)  n = 3, l = 1, ml = 1, ms = - 1/2 
E)  n = 3, l = 0, ml = 0, ms = +1/2

Question 18

Which one of the following sets of quantum numbers is not possible $\begin{array}{lccc}
~~~~~\text { n } & l & \mathrm{~m}_{l} & \mathrm{~m}_{5} \
\text { A. } 4 & 3 & -2 & +1 / 2 \
\text { B. } 3 & 2 & -3 & -1 / 2 \
\text { C. } 3 & 0 & 0 & +1 / 2 \
\text { D. } 4 & 1 & 1 & -1 / 2 \
\text { E. } 2 & 0 & 0 & +1 / 2
\end{array}$

Accepted Answer

The answer of Which one of the following sets of...

Question 19

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]5s24d6 
A)  [Kr]5s14d5 
B)  [Kr]5s24d4 
C)  [Xe]6s25d4 
D)  [Ar]4s24d4 
E)  [Kr]5s24d6

Question 20

What is the total number of electrons possible in the 2p orbitals

Accepted Answer

A)  3 
B)  6 
C)  10 
D)  Since it depends on the particular atom that has the 2p orbital this cannot be answered without more information. 
E)  None of the above 
A)  3 
B)  6 
C)  10 
D)  Since it depends on the particular atom that has the 2p orbital this cannot be answered without more information. 
E)  None of the above

Exam 7: Quantum Theory and the Electronic Structure of Atoms

An electron in a 3p orbital could have a value of 2 for its angular momentum quantum number (l).

The electron configuration of a ground-state Co atom is

Which of the following, if any, is the proper rank the following types of electromagnetic radiation from lowest energy to highest energy

What is the wavelength (nm) for a photon of light with an energy of 3.20 x 10-19 J/photon

The colors of the visible spectrum are blue, green, orange, red, violet, and yellow. Of these colors, ______ has the least energy.

Which element has the following ground-state electron configuration [Xe]6s24f145d4

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).

"No two electrons in an atom can have the same four quantum numbers" is a statement of

What is the wavelength of radiation that has a frequency of 3.4 x 1011 s -1

The longest wavelength of light that causes electrons to be ejected from the surface of a copper plate is 243 nm. What is the maximum velocity of the electrons ejected when light of wavelength 200. nm shines on a copper plate

How many unpaired electrons does an atom of carbon have in its ground state

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

List the following sets of quantum numbers in order of increasing energy: I. n = 4, l = 0, ml = 0, ms = -1/2 II. n = 4, l = 2, ml = -1, ms = -1/2 III. n = 5, l = 0, ml = 0, ms = +1/2

The bonds of oxygen molecules are broken by sunlight. The minimum energy required to break the oxygen-oxygen bond is 495 kJ/mol. What is the wavelength of sunlight that can cause this bond breakage

A ground-state chromium atom has how many unpaired electrons

An electron loses energy in the transition from a 4f subshell to a 6s subshell.

A possible set of quantum numbers to describe an electron in a 4s subshell is

Which one of the following sets of quantum numbers is not possible \nobreakspace\nobreakspace\nobreakspace\nobreakspace\nobreakspace n l A. 4 3 -2 +1/2 B. 3 2 -3 -1/2 C. 3 0 0 +1/2 D. 4 1 1 -1/2 E. 2 0 0 +1/2

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

What is the total number of electrons possible in the 2p orbitals

Chemistry: The Study of Change

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Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Gases

Thermochemistry

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

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Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

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Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metals Chemistry and Coordination Compounds

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What is the wavelength (nm) for a photon of light with an energy of 3.20 x 10^-19 J/photon

Which element has the following ground-state electron configuration [Xe]6s²4f¹⁴5d⁴

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).

What is the wavelength of radiation that has a frequency of 3.4 x 10¹¹ s ^-1

List the following sets of quantum numbers in order of increasing energy: I. n = 4, l = 0, m_l = 0, m_s = -1/2 II. n = 4, l = 2, m_l = -1, m_s = -1/2 III. n = 5, l = 0, m_l = 0, m_s = +1/2