Question 1

The ________ quantum number is the quantum number which describes the orientation of the orbital in space.

Accepted Answer

A)  principal 
B)  angular momentum 
C)  magnetic 
D)  spin 
A)  principal 
B)  angular momentum 
C)  magnetic 
D)  spin

Question 2

The orbital diagram for a ground-state nitrogen atom is

Accepted Answer

A)  A 
B)  B 
C)  C 
D)  D 
E)  E 
A)  A 
B)  B 
C)  C 
D)  D 
E)  E

Question 3

What is the electron configuration for tungsten?

Accepted Answer

A)  1s22s22p63s23p64s23d104p65s24d105p66s24f145d6 
B)  1s22s22p63s23p64s23d104p65s24d105p66s14f145d5 
C)  1s22s22p63s23p64s23d104p65s24d105p66s24f145d4 
D)  1s22s22p63s23p64s23d104p65s24d105p66s24f145d7 
E)  1s22s22p63s23p54s23d104p65s24d105p66s24f145d7 
A)  1s22s22p63s23p64s23d104p65s24d105p66s24f145d6 
B)  1s22s22p63s23p64s23d104p65s24d105p66s14f145d5 
C)  1s22s22p63s23p64s23d104p65s24d105p66s24f145d4 
D)  1s22s22p63s23p64s23d104p65s24d105p66s24f145d7 
E)  1s22s22p63s23p54s23d104p65s24d105p66s24f145d7

Question 4

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; c = 3.00 × 108 m/s)

Accepted Answer

A)  2.06 × 106 s-1 
B)  2.74 × 106 s-1 
C)  6.17 × 1014 s-1  
D)  8.23 × 1014 s-1 
E)  > 1015 s-1 
A)  2.06 × 106 s-1 
B)  2.74 × 106 s-1 
C)  6.17 × 1014 s-1  
D)  8.23 × 1014 s-1 
E)  > 1015 s-1

Question 5

Calculate the energy, in joules, required to excite a hydrogen atom by causing an electronic transition from the n = 1 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)  2.07 × 10-29 J 
B)  2.19 × 105 J 
C)  2.04 × 10-18 J 
D)  3.27 × 10-17 J 
E)  2.25 × 10-18 J 
A)  2.07 × 10-29 J 
B)  2.19 × 105 J 
C)  2.04 × 10-18 J 
D)  3.27 × 10-17 J 
E)  2.25 × 10-18 J

Question 6

A 6.0-gram champagne cork is shot out of an opened champagne bottle and traveled at a speed of 65 km/hour. Calculate the de Broglie wavelength (in meters) of the cork.

Accepted Answer

A)  6.1 × 10-33 m 
B)  1.7 × 10-36 m 
C)  6.1 × 10-36 m 
D)  1.7 × 10-33 m 
E)  5.5 × 10-20 m 
A)  6.1 × 10-33 m 
B)  1.7 × 10-36 m 
C)  6.1 × 10-36 m 
D)  1.7 × 10-33 m 
E)  5.5 × 10-20 m

Question 7

Which of the following is a correct set of quantum numbers for an electron in a 3d orbital?

Accepted Answer

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

Question 8

What is the energy in joules of a mole of photons associated with visible light of wavelength 486 nm? (c = 3.00 × 108 m/s; h = 6.63 × 10-34 J • s; NA = 6.022 × 1023 moles-1)

Accepted Answer

A)  6.46 × 10-16 J 
B)  6.46 × 10-25 J 
C)  2.46 × 10-4 J 
D)  12.4 kJ 
E)  246 kJ 
A)  6.46 × 10-16 J 
B)  6.46 × 10-25 J 
C)  2.46 × 10-4 J 
D)  12.4 kJ 
E)  246 kJ

Question 9

What is the wavelength of radiation that has a frequency of 6.912 × 1014 s-1? (c = 3.00 × 108 m/s)

Accepted Answer

A)  1.447 × 10-15 nm 
B)  4.337 × 102 nm 
C)  2.304 × 106 nm 
D)  2.074 × 1023 nm 
E)  4.337 × 10-7 nm 
A)  1.447 × 10-15 nm 
B)  4.337 × 102 nm 
C)  2.304 × 106 nm 
D)  2.074 × 1023 nm 
E)  4.337 × 10-7 nm

Question 10

What type of configuration specifies the arrangement of electrons in the orbitals of an atom?

Accepted Answer

A)  Heisenberg configuration 
B)  Nuclear configuration 
C)  Atomic configuration 
D)  Proton configuration 
E)  Electron configuration 
A)  Heisenberg configuration 
B)  Nuclear configuration 
C)  Atomic configuration 
D)  Proton configuration 
E)  Electron configuration

Question 11

If n = 2 then l = 0, -1, and 1.

Accepted Answer

A) True 
 B)False

Question 12

The following combination of quantum numbers is not allowed. Correct this set of quantum numbers by changing only one quantum number, and write in an appropriate corrected value. n = 2, l = 2, ml = 2; Corrected: ________ = _____

Accepted Answer

Question 13

How many electrons are in the 4p orbitals of selenium?

Accepted Answer

A)  0 
B)  2 
C)  4 
D)  5 
E)  6 
A)  0 
B)  2 
C)  4 
D)  5 
E)  6

Question 14

Electrons will not pair in degenerate orbitals if an empty orbital is available and, according to Hund's rule, the degenerate orbitals must all contain one electron before any of them can contain two electrons.

Accepted Answer

A) True 
 B)False

Question 15

What element is represented by the electron configuration 1s22s22p63s23p64s23d104p65s14d10?

Accepted Answer

A)  Ag 
B)  Rb 
C)  Cd 
D)  Sr 
E)  Cu 
A)  Ag 
B)  Rb 
C)  Cd 
D)  Sr 
E)  Cu

The ________ quantum number is the quantum number which describes the orientation of the orbital in space.

The orbital diagram for a ground-state nitrogen atom is

What is the electron configuration for tungsten?

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; c = 3.00 × 10⁸m/s)

Calculate the energy, in joules, required to excite a hydrogen atom by causing an electronic transition from the n = 1 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).

A 6.0-gram champagne cork is shot out of an opened champagne bottle and traveled at a speed of 65 km/hour. Calculate the de Broglie wavelength (in meters) of the cork.

Which of the following is a correct set of quantum numbers for an electron in a 3d orbital?

What is the energy in joules of a mole of photons associated with visible light of wavelength 486 nm? (c = 3.00 × 10⁸m/s; h = 6.63 × 10^-34 J • s; N_A = 6.022 × 10²³ moles^-1)

What is the wavelength of radiation that has a frequency of 6.912 × 10¹⁴ s^-1? (c = 3.00 × 10⁸m/s)

What type of configuration specifies the arrangement of electrons in the orbitals of an atom?

If n = 2 then l = 0, -1, and 1.

The following combination of quantum numbers is not allowed. Correct this set of quantum numbers by changing only one quantum number, and write in an appropriate corrected value. n = 2, l = 2, m_l = 2; Corrected: ____ = _

How many electrons are in the 4p orbitals of selenium?

Electrons will not pair in degenerate orbitals if an empty orbital is available and, according to Hund's rule, the degenerate orbitals must all contain one electron before any of them can contain two electrons.

What element is represented by the electron configuration 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s¹4d¹⁰?

Chemistry: the Central Science

Atoms, Molecules, and Ions

Stoichiometry: Ratios of Combination

Reactions in Aqueous Solutions

Thermochemistry

Electron Configuration and the Periodic Table

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Bonding Theories

Gases

Intermolecular Forces and the Physical Properties of Liquids and Solids

Modern Materials

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy, Free Energy, and Equilibrium

Electrochemistry

Nuclear Chemistry

Environmental Chemistry

Coordination Chemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Organic Chemistry

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Exam 6: Quantum Theory and the Electronic Structure of Atoms

The ________ quantum number is the quantum number which describes the orientation of the orbital in space.

The orbital diagram for a ground-state nitrogen atom is

What is the electron configuration for tungsten?

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; c = 3.00 × 108 m/s)

Calculate the energy, in joules, required to excite a hydrogen atom by causing an electronic transition from the n = 1 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).

A 6.0-gram champagne cork is shot out of an opened champagne bottle and traveled at a speed of 65 km/hour. Calculate the de Broglie wavelength (in meters) of the cork.

Which of the following is a correct set of quantum numbers for an electron in a 3d orbital?

What is the energy in joules of a mole of photons associated with visible light of wavelength 486 nm? (c = 3.00 × 108 m/s; h = 6.63 × 10-34 J • s; NA = 6.022 × 1023 moles-1)

What is the wavelength of radiation that has a frequency of 6.912 × 1014 s-1? (c = 3.00 × 108 m/s)

What type of configuration specifies the arrangement of electrons in the orbitals of an atom?

If n = 2 then l = 0, -1, and 1.

The following combination of quantum numbers is not allowed. Correct this set of quantum numbers by changing only one quantum number, and write in an appropriate corrected value. n = 2, l = 2, ml = 2; Corrected: ________ = _____

How many electrons are in the 4p orbitals of selenium?

Electrons will not pair in degenerate orbitals if an empty orbital is available and, according to Hund's rule, the degenerate orbitals must all contain one electron before any of them can contain two electrons.

What element is represented by the electron configuration 1s22s22p63s23p64s23d104p65s14d10?

Chemistry: the Central Science

Atoms, Molecules, and Ions

Stoichiometry: Ratios of Combination

Reactions in Aqueous Solutions

Thermochemistry

Electron Configuration and the Periodic Table

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Bonding Theories

Gases

Intermolecular Forces and the Physical Properties of Liquids and Solids

Modern Materials

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy, Free Energy, and Equilibrium

Electrochemistry

Nuclear Chemistry

Environmental Chemistry

Coordination Chemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Organic Chemistry

Filters

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; c = 3.00 × 10⁸m/s)

Calculate the energy, in joules, required to excite a hydrogen atom by causing an electronic transition from the n = 1 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).

What is the energy in joules of a mole of photons associated with visible light of wavelength 486 nm? (c = 3.00 × 10⁸m/s; h = 6.63 × 10^-34 J • s; N_A = 6.022 × 10²³ moles^-1)

What is the wavelength of radiation that has a frequency of 6.912 × 10¹⁴ s^-1? (c = 3.00 × 10⁸m/s)

The following combination of quantum numbers is not allowed. Correct this set of quantum numbers by changing only one quantum number, and write in an appropriate corrected value. n = 2, l = 2, m_l = 2; Corrected: ____ = _

What element is represented by the electron configuration 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s¹4d¹⁰?