Question 1

Give the ground-state electron configuration for Cd+2.

Accepted Answer

Question 2

Which of the following occurs as the energy of a photon increases?

Accepted Answer

A) The frequency decreases. 
B) The speed increases. 
C) The wavelength increases. 
D) The wavelength gets shorter. 
E) None of the above occurs as the energy of a photon increases. 
A) The frequency decreases. 
B) The speed increases. 
C) The wavelength increases. 
D) The wavelength gets shorter. 
E) None of the above occurs as the energy of a photon increases.

Question 3

Identify the colour of a flame test for sodium.

Accepted Answer

A) violet 
B) red 
C) white 
D) yellow 
E) blue 
A) violet 
B) red 
C) white 
D) yellow 
E) blue

Question 4

Identify the ground-state electron configuration for Se2⁻.

Accepted Answer

A) [Ar]4s23d104p4 
B) [Ar]4s23d104p2 
C) [Ar]4s24p6 
D) [Ar]4s23d104p6 
E) [Ar]4s23d84p6 
A) [Ar]4s23d104p4 
B) [Ar]4s23d104p2 
C) [Ar]4s24p6 
D) [Ar]4s23d104p6 
E) [Ar]4s23d84p6

Question 5

Give the number of core electrons for Br-.

Accepted Answer

A) 35 
B) 18 
C) 30 
D) 40 
E) 28 
A) 35 
B) 18 
C) 30 
D) 40 
E) 28

Question 6

Identify the set of four quantum numbers that could represent the last electron added (using the aufbau principle)to the Cl atom.

Accepted Answer

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

Question 7

What is the maximum number of f orbitals that are possible?

Accepted Answer

A) 1 
B) 3 
C) 7 
D) 5 
E) 9 
A) 1 
B) 3 
C) 7 
D) 5 
E) 9

Question 8

An electron ends in orbital n = 3 after a hydrogen atom emits a photon with a wavelength of 1093 nm. Calculate the initial orbital, ni.

Accepted Answer

A) 1 
B) 5 
C) 2 
D) 3 
E) 6 
A) 1 
B) 5 
C) 2 
D) 3 
E) 6

Question 9

For a hydrogen atom, which electronic transition would result in the emission of a photon with the highest energy?

Accepted Answer

A) 2s → 3p 
B) 2p → 6d 
C) 6p → 4s 
D) 7f → 5d 
A) 2s → 3p 
B) 2p → 6d 
C) 6p → 4s 
D) 7f → 5d

Question 10

When waves of equal amplitude from two sources are out of phase when they interact, it is called

Accepted Answer

A) destructive interference. 
B) diffraction. 
C) constructive interference. 
D) effusion. 
E) amplitude. 
A) destructive interference. 
B) diffraction. 
C) constructive interference. 
D) effusion. 
E) amplitude.

Question 11

Which of the following quantum numbers describes the shape of an orbital?

Accepted Answer

A) principal quantum number 
B) magnetic quantum number 
C) spin quantum number 
D) Schrödinger quantum number 
E) angular momentum quantum number 
A) principal quantum number 
B) magnetic quantum number 
C) spin quantum number 
D) Schrödinger quantum number 
E) angular momentum quantum number

Question 12

Give all possible values of l for a 3 sublevel.

Accepted Answer

A) 0 
B) 1, 2 
C) 0, 1, 2 
D) -1, 0, 1 
E) 0, 1, 2, 3 
A) 0 
B) 1, 2 
C) 0, 1, 2 
D) -1, 0, 1 
E) 0, 1, 2, 3

Question 13

Electromagnetic radiation with a wavelength of 525 nm appears as green light to the human eye. The energy of one photon of this light is ________ J.

Accepted Answer

A) 1.04 × 10-31 
B) 3.79 × 10-28 
C) 3.79 × 10-19 
D) 1.04 × 10-22 
E) 2.64 × 1018 
A) 1.04 × 10-31 
B) 3.79 × 10-28 
C) 3.79 × 10-19 
D) 1.04 × 10-22 
E) 2.64 × 1018

Question 14

Match the following.

-2

Accepted Answer

A) number of unpaired electrons in Zn2+ 
B) number of unpaired electrons in Ti2+ 
A) number of unpaired electrons in Zn2+ 
B) number of unpaired electrons in Ti2+

Question 15

Calculate the energy of an electron in the orbital n = 6 of a hydrogen atom.

Accepted Answer

A) 3.19 × 10-20 J 
B) 4.18 × 10-20 J 
C) -6.06 × 10-20 J 
D) -7.80 × 10-20 J 
E) -8.62 × 10-20 J 
A) 3.19 × 10-20 J 
B) 4.18 × 10-20 J 
C) -6.06 × 10-20 J 
D) -7.80 × 10-20 J 
E) -8.62 × 10-20 J

Question 16

Identify the correct values for a 2p sublevel.

Accepted Answer

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

Question 17

What are the possible values of n and ml for an electron in a 4d orbital?

Accepted Answer

A) n = 1, 2, 3, or 4 and ml = 2 
B) n = 1, 2, 3, or 4 and ml = -2, -1, 0, +1, or +2 
C) n = 4 and ml = 2 
D) n = 5 and ml = -2, -1, 0, +1, +2 
A) n = 1, 2, 3, or 4 and ml = 2 
B) n = 1, 2, 3, or 4 and ml = -2, -1, 0, +1, or +2 
C) n = 4 and ml = 2 
D) n = 5 and ml = -2, -1, 0, +1, +2

Question 18

Choose the ground-state electron configuration for Zn2⁺.

Accepted Answer

A) [Ar]4s23d8 
B) [Ar]3d10 
C) [Ar]4s23d6 
D) [Ar] 
E) [Ar]3d8 
A) [Ar]4s23d8 
B) [Ar]3d10 
C) [Ar]4s23d6 
D) [Ar] 
E) [Ar]3d8

Question 19

Which of the following statements is TRUE?

Accepted Answer

A) An orbital that penetrates into the region occupied by core electrons is less shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy. 
B) An orbital that penetrates into the region occupied by core electrons is more shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy. 
C) It is possible for two electrons in the same atom to have identical values for all four quantum numbers. 
D) Two electrons in the same orbital can have the same spin. 
E) None of the above is true. 
A) An orbital that penetrates into the region occupied by core electrons is less shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy. 
B) An orbital that penetrates into the region occupied by core electrons is more shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy. 
C) It is possible for two electrons in the same atom to have identical values for all four quantum numbers. 
D) Two electrons in the same orbital can have the same spin. 
E) None of the above is true.

Question 20

Choose the paramagnetic species from below.

Accepted Answer

A) Ca 
B) O2⁻ 
C) Cd2⁺ 
D) Zn 
E) Nb3⁺ 
A) Ca 
B) O2⁻ 
C) Cd2⁺ 
D) Zn 
E) Nb3⁺

Exam 7: The Quantum-Mechanical Model of the Atom

Give the ground-state electron configuration for Cd+2.

Which of the following occurs as the energy of a photon increases?

Identify the colour of a flame test for sodium.

Identify the ground-state electron configuration for Se2⁻.

Give the number of core electrons for Br-.

Identify the set of four quantum numbers that could represent the last electron added (using the aufbau principle)to the Cl atom.

What is the maximum number of f orbitals that are possible?

An electron ends in orbital n = 3 after a hydrogen atom emits a photon with a wavelength of 1093 nm. Calculate the initial orbital, ni.

For a hydrogen atom, which electronic transition would result in the emission of a photon with the highest energy?

When waves of equal amplitude from two sources are out of phase when they interact, it is called

Which of the following quantum numbers describes the shape of an orbital?

Give all possible values of l for a 3 sublevel.

Electromagnetic radiation with a wavelength of 525 nm appears as green light to the human eye. The energy of one photon of this light is ________ J.

Match the following. -2

Calculate the energy of an electron in the orbital n = 6 of a hydrogen atom.

Identify the correct values for a 2p sublevel.

What are the possible values of n and ml for an electron in a 4d orbital?

Choose the ground-state electron configuration for Zn2⁺.

Which of the following statements is TRUE?

Choose the paramagnetic species from below.

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules, Compounds, and Nomenclature

Chemical Reactions and Stoichiometry

Gases

Thermochemistry

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry II: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallury

Transition Metals and Coordination Compounds

Filters

Give the ground-state electron configuration for Cd⁺².

Identify the ground-state electron configuration for Se²⁻.

Give the number of core electrons for Br^-.

An electron ends in orbital n = 3 after a hydrogen atom emits a photon with a wavelength of 1093 nm. Calculate the initial orbital, n_i.

What are the possible values of n and m_l for an electron in a 4d orbital?

Choose the ground-state electron configuration for Zn²⁺.