Question 1

Which element is most likely to form an ion with a charge of 2+?

Accepted Answer

A)  K 
B)  Al 
C)  F 
D)  S 
E)  Mg 
A)  K 
B)  Al 
C)  F 
D)  S 
E)  Mg E

Question 2

How many electrons in an atom can have the quantum numbers n = 3, l = 2?

Accepted Answer

A)  18 
B)  32 
C)  2 
D)  6 
E)  10 
A)  18 
B)  32 
C)  2 
D)  6 
E)  10 E

Question 3

How many electrons can be described by the quantum numbers n = 4, l = 4, ml = 0?

Accepted Answer

A)  14 
B)  6 
C)  10 
D)  0 
E)  2 
A)  14 
B)  6 
C)  10 
D)  0 
E)  2 D

Question 4

Which atomic species, in its ground state, has six unpaired electrons?

Accepted Answer

A)  O 
B)  Fe 
C)  Cs 
D)  Dy 
E)  Mo 
A)  O 
B)  Fe 
C)  Cs 
D)  Dy 
E)  Mo

Question 5

The number of unpaired electrons in the outer subshell of a Cl atom is

Accepted Answer

A)  0 
B)  1 
C)  3 
D)  2 
E)  none of these 
A)  0 
B)  1 
C)  3 
D)  2 
E)  none of these

Question 6

Consider the following portion of the energy-level diagram for hydrogen:  
-For which of the following transitions does the light emitted have the longest wavelength?

Accepted Answer

A)  n = 2 to n = 1 
B)  n = 4 to n = 1 
C)  n = 3 to n = 2 
D)  n = 4 to n = 2 
E)  n = 4 to n = 3 
A)  n = 2 to n = 1 
B)  n = 4 to n = 1 
C)  n = 3 to n = 2 
D)  n = 4 to n = 2 
E)  n = 4 to n = 3

Question 7

The ionization energy for a hydrogen atom is 1.31 *106 J/mol. What is the ionization energy for He+?

Accepted Answer

A)  2.18 *10-18 J/mol 
B)  1.31 * 106 J/mol 
C)  5.25* 106 J/mol 
D)  8.72 * 10-18 J/mol 
E)  2.63 *106 J/mol 
A)  2.18 *10-18 J/mol 
B)  1.31 * 106 J/mol 
C)  5.25* 106 J/mol 
D)  8.72 * 10-18 J/mol 
E)  2.63 *106 J/mol

Question 8

Which of the following is not determined by the principal quantum number, n, of the electron in a hydrogen atom?

Accepted Answer

A)  the minimum wavelength of the light needed to remove the electron from the atom. 
B)  the energy of the electron 
C)  the shape of the corresponding atomic orbital(s) 
D)  the size of the corresponding atomic orbital(s) 
E)  All of the above are determined by n. 
A)  the minimum wavelength of the light needed to remove the electron from the atom. 
B)  the energy of the electron 
C)  the shape of the corresponding atomic orbital(s) 
D)  the size of the corresponding atomic orbital(s) 
E)  All of the above are determined by n.

Question 9

The ionization energies, in kcalories, for Mg and Ca are   
A) Indicate the reasons for the relatively high third ionization energy for magnesium.
B) Indicate the reasons for the difference between the first ionization energies for Mg and Ca.
C) Predict the third ionization energy for calcium.

Accepted Answer

A) See Section 12.15 of Zumdah

Question 10

The wavelength of light associated with the n = 2 to n = 1 electron transition in the hydrogen spectrum is 1.216 * 10-7 m. By what coefficient should this wavelength be multiplied to obtain the wavelength associated with the same electron transition in the Li2+ ion?

Accepted Answer

A)  1 
B)  1/3 
C)  1/4 
D)  1/7 
E)  1/9 
A)  1 
B)  1/3 
C)  1/4 
D)  1/7 
E)  1/9

Question 11

How many electrons can be described by the quantum number n = 3?

Accepted Answer

A)  32 
B)  2 
C)  18 
D)  8 
E)  10 
A)  32 
B)  2 
C)  18 
D)  8 
E)  10

Question 12

How many electrons can be described by the quantum numbers n = 4, l = 3, ml = 0?

Accepted Answer

A)  2 
B)  10 
C)  6 
D)  0 
E)  14 
A)  2 
B)  10 
C)  6 
D)  0 
E)  14

Question 13

Which of the following is a reasonable criticism of the Bohr model of the atom?

Accepted Answer

A)  It shows the electrons to exist outside of the nucleus. 
B)  It does not adequately predict the ionization energy of the first-energy-level electrons for elements other than hydrogen. 
C)  It makes no attempt to explain why the negative electron does not eventually fall into the positive nucleus. 
D)  It does not adequately predict the ionization energy of the valence electron(s) for elements other than hydrogen. 
E)  It does not adequately predict the line spectrum of hydrogen. 
A)  It shows the electrons to exist outside of the nucleus. 
B)  It does not adequately predict the ionization energy of the first-energy-level electrons for elements other than hydrogen. 
C)  It makes no attempt to explain why the negative electron does not eventually fall into the positive nucleus. 
D)  It does not adequately predict the ionization energy of the valence electron(s) for elements other than hydrogen. 
E)  It does not adequately predict the line spectrum of hydrogen.

Question 14

What is the electron configuration for the chromium atom?

Accepted Answer

A)  [Kr] 4s13d5 
B)  [Ar] 4s23d4 
C)  [Kr] 4s23d4 
D)  [Ar] 4s13d5 
E)  none of these 
A)  [Kr] 4s13d5 
B)  [Ar] 4s23d4 
C)  [Kr] 4s23d4 
D)  [Ar] 4s13d5 
E)  none of these

Question 15

Sodium losing an electron is an ________ process, and fluorine losing an electron is an _______ process.

Accepted Answer

A)  exothermic, endothermic 
B)  endothermic, exothermic 
C)  exothermic, exothermic 
D)  More information is needed. 
E)  endothermic, endothermic 
A)  exothermic, endothermic 
B)  endothermic, exothermic 
C)  exothermic, exothermic 
D)  More information is needed. 
E)  endothermic, endothermic

Question 16

What value is the closest estimate of Zeff  for a valence electron of the calcium atom?

Accepted Answer

A)  20 
B)  40 
C)  2 
D)  6 
E)  1 
A)  20 
B)  40 
C)  2 
D)  6 
E)  1

Question 17

Which orbital has the highest energy in the rubidium atom?

Accepted Answer

A)  4p 
B)  4s 
C)  5s 
D)  1s 
E)  4d 
A)  4p 
B)  4s 
C)  5s 
D)  1s 
E)  4d

Question 18

Write the electron configuration for the following:
-Cu

Accepted Answer

1s²2s²2p⁶3s²3p

Question 19

Four electrons are confined to a one-dimensional box 5.64 * 10-10 m long. If two electrons can occupy each allowed energy level, calculate the wavelength of electromagnetic radiation necessary to promote the highest-energy electron into the first excited state.

Accepted Answer

The answer of Four electrons are confined to a one-dimensional...

Question 20

Place the elements C, N, and O in order of increasing ionization energy.

Accepted Answer

A)  N, O, C 
B)  C, N, O 
C)  O, N, C 
D)  C, O, N 
E)  none of these 
A)  N, O, C 
B)  C, N, O 
C)  O, N, C 
D)  C, O, N 
E)  none of these

Which element is most likely to form an ion with a charge of 2+?

How many electrons in an atom can have the quantum numbers n = 3, l = 2?

How many electrons can be described by the quantum numbers n = 4, l = 4, m_l = 0?

Which atomic species, in its ground state, has six unpaired electrons?

The number of unpaired electrons in the outer subshell of a Cl atom is

Consider the following portion of the energy-level diagram for hydrogen: -For which of the following transitions does the light emitted have the longest wavelength?

The ionization energy for a hydrogen atom is 1.31 *10⁶ J/mol. What is the ionization energy for He⁺?

Which of the following is not determined by the principal quantum number, n, of the electron in a hydrogen atom?

The ionization energies, in kcalories, for Mg and Ca are A) Indicate the reasons for the relatively high third ionization energy for magnesium. B) Indicate the reasons for the difference between the first ionization energies for Mg and Ca. C) Predict the third ionization energy for calcium.

The wavelength of light associated with the n = 2 to n = 1 electron transition in the hydrogen spectrum is 1.216 * 10^-⁷ m. By what coefficient should this wavelength be multiplied to obtain the wavelength associated with the same electron transition in the Li²⁺ ion?

How many electrons can be described by the quantum number n = 3?

How many electrons can be described by the quantum numbers n = 4, l = 3, m_l = 0?

Which of the following is a reasonable criticism of the Bohr model of the atom?

What is the electron configuration for the chromium atom?

Sodium losing an electron is an __ process, and fluorine losing an electron is an _ process.

What value is the closest estimate of Z_eff for a valence electron of the calcium atom?

Which orbital has the highest energy in the rubidium atom?

Write the electron configuration for the following: -Cu

Four electrons are confined to a one-dimensional box 5.64 * 10^-10 m long. If two electrons can occupy each allowed energy level, calculate the wavelength of electromagnetic radiation necessary to promote the highest-energy electron into the first excited state.

Place the elements C, N, and O in order of increasing ionization energy.

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Spontaneity, Entropy, and Free Energy

Electrochemistry

Bonding: General Concepts

Covalent Bonding: Orbitals

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Exam 12: Quantum Mechanics and Atomic Theory

Which element is most likely to form an ion with a charge of 2+?

How many electrons in an atom can have the quantum numbers n = 3, l = 2?

How many electrons can be described by the quantum numbers n = 4, l = 4, ml = 0?

Which atomic species, in its ground state, has six unpaired electrons?

The number of unpaired electrons in the outer subshell of a Cl atom is

Consider the following portion of the energy-level diagram for hydrogen: -For which of the following transitions does the light emitted have the longest wavelength?

The ionization energy for a hydrogen atom is 1.31 *106 J/mol. What is the ionization energy for He+?

Which of the following is not determined by the principal quantum number, n, of the electron in a hydrogen atom?

The ionization energies, in kcalories, for Mg and Ca are A) Indicate the reasons for the relatively high third ionization energy for magnesium. B) Indicate the reasons for the difference between the first ionization energies for Mg and Ca. C) Predict the third ionization energy for calcium.

The wavelength of light associated with the n = 2 to n = 1 electron transition in the hydrogen spectrum is 1.216 * 10-7 m. By what coefficient should this wavelength be multiplied to obtain the wavelength associated with the same electron transition in the Li2+ ion?

How many electrons can be described by the quantum number n = 3?

How many electrons can be described by the quantum numbers n = 4, l = 3, ml = 0?

Which of the following is a reasonable criticism of the Bohr model of the atom?

What is the electron configuration for the chromium atom?

Sodium losing an electron is an ________ process, and fluorine losing an electron is an _______ process.

What value is the closest estimate of Zeff for a valence electron of the calcium atom?

Which orbital has the highest energy in the rubidium atom?

Write the electron configuration for the following: -Cu

Four electrons are confined to a one-dimensional box 5.64 * 10-10 m long. If two electrons can occupy each allowed energy level, calculate the wavelength of electromagnetic radiation necessary to promote the highest-energy electron into the first excited state.

Place the elements C, N, and O in order of increasing ionization energy.

Atoms, Molecules, and Ions

Stoichiometry

Chemical Reactions and Solutions Stoichiometry

Gases

Chemical Equilibrium

Acids and Bases

Applications of Aqueous Equilibria

Energy, Enthalpy, and Thermochemistry

Spontaneity, Entropy, and Free Energy

Electrochemistry

Bonding: General Concepts

Covalent Bonding: Orbitals

Chemical Kinetics

Liquids and Solids

Properties of Solutions

The Representative Elements

Transition Metals and Coordination Chemistry

The Nucleus: a Chemists View

Organic and Biochemical Molecules

Filters

How many electrons can be described by the quantum numbers n = 4, l = 4, m_l = 0?

The ionization energy for a hydrogen atom is 1.31 *10⁶ J/mol. What is the ionization energy for He⁺?

The wavelength of light associated with the n = 2 to n = 1 electron transition in the hydrogen spectrum is 1.216 * 10^-⁷ m. By what coefficient should this wavelength be multiplied to obtain the wavelength associated with the same electron transition in the Li²⁺ ion?

How many electrons can be described by the quantum numbers n = 4, l = 3, m_l = 0?

Sodium losing an electron is an __ process, and fluorine losing an electron is an _ process.

What value is the closest estimate of Z_eff for a valence electron of the calcium atom?

Four electrons are confined to a one-dimensional box 5.64 * 10^-10 m long. If two electrons can occupy each allowed energy level, calculate the wavelength of electromagnetic radiation necessary to promote the highest-energy electron into the first excited state.