Question 1

Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error.

Accepted Answer

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

Question 2

When filling degenerate orbitals, electrons fill them singly first, with parallel spins. What is this known as?

Accepted Answer

A)  Pauli exclusion principle 
B)  Hund's rule 
C)  aufbau principle 
D)  Heisenberg uncertainty principle 
A)  Pauli exclusion principle 
B)  Hund's rule 
C)  aufbau principle 
D)  Heisenberg uncertainty principle

Question 3

Why do atoms only emit certain wavelengths of light when they are excited? (Why do line spectra exist?)

Accepted Answer

The energies of atoms are quantized. Whe

Question 4

Choose the valence orbital diagram that represents the ground state of Se2⁻.

Accepted Answer

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

Question 5

An FM radio station broadcasts electromagnetic radiation at a frequency of 100.5 MHz. The wavelength of this radiation is ________ m.

Accepted Answer

A)  3.015 ×   
B)  3.015 ×   
C)  0.3350 
D)  2.985 ×   
E)  2.985 
A)  3.015 ×   
B)  3.015 ×   
C)  0.3350 
D)  2.985 ×   
E)  2.985

Question 6

Choose the ground-state electron configuration for Cr3⁺.

Accepted Answer

A)  [Ar]4s13d2 
B)  [Ar] 
C)  [Ar]4s23d6 
D)  [Ar]3d3 
E)  [Ar]4s23d1 
A)  [Ar]4s13d2 
B)  [Ar] 
C)  [Ar]4s23d6 
D)  [Ar]3d3 
E)  [Ar]4s23d1

Question 7

What total energy (in kJ) is contained in 1.0 mol of photons, all with a frequency of 2.75 × 1014 Hz?

Accepted Answer

A)  182 kJ 
B)  219 kJ 
C)  457 kJ 
D)  326 kJ 
E)  110 kJ 
A)  182 kJ 
B)  219 kJ 
C)  457 kJ 
D)  326 kJ 
E)  110 kJ

Question 8

If two electrons in the same atom have the same value of l, they are ________.

Accepted Answer

A)  in the same sublevel, but not necessarily in the same level 
B)  in the same level, but in different sublevels 
C)  in the same orbital 
D)  in different levels and in different shaped orbitals 
E)  None of the above. 
A)  in the same sublevel, but not necessarily in the same level 
B)  in the same level, but in different sublevels 
C)  in the same orbital 
D)  in different levels and in different shaped orbitals 
E)  None of the above.

Question 9

Which of the following statements is TRUE?

Accepted Answer

A)  We can sometimes know the exact location and speed of an electron at the same time. 
B)  All orbitals in a given atom are roughly the same size. 
C)  Since electrons have mass, we must always consider them to have particle properties and never wavelike properties. 
D)  Atoms are roughly spherical because when all of the different shaped orbitals are overlapped, they take on a spherical shape. 
A)  We can sometimes know the exact location and speed of an electron at the same time. 
B)  All orbitals in a given atom are roughly the same size. 
C)  Since electrons have mass, we must always consider them to have particle properties and never wavelike properties. 
D)  Atoms are roughly spherical because when all of the different shaped orbitals are overlapped, they take on a spherical shape.

Question 10

Each of the following sets of quantum numbers is supposed to specify an orbital. Which of the following sets of quantum numbers contains an error?

Accepted Answer

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

Question 11

How many different values of l are possible in the third principal level?

Accepted Answer

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

Question 12

Calculate the energy of the green light emitted, per photon, by a mercury lamp with a frequency of 5.49 × 1014 Hz.

Accepted Answer

A)  2.75 × 10-19 J 
B)  3.64 × 10-19 J 
C)  5.46 × 10-19 J 
D)  1.83 × 10-19 J 
E)  4.68 × 10-19 J 
A)  2.75 × 10-19 J 
B)  3.64 × 10-19 J 
C)  5.46 × 10-19 J 
D)  1.83 × 10-19 J 
E)  4.68 × 10-19 J

Question 13

Choose the valence orbital diagram that represents the ground state of Zn.

Accepted Answer

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

Question 14

Calculate the energy change associated with the transition from n = 4 to n = 1 in the hydrogen atom.

Accepted Answer

A)  +4.89 × 10-18 J 
B)  +1.64 × 10-18 J 
C)  -6.12 × 10-18 J 
D)  +3.55 × 10-18 J 
E)  -2.04 × 10-18 J 
A)  +4.89 × 10-18 J 
B)  +1.64 × 10-18 J 
C)  -6.12 × 10-18 J 
D)  +3.55 × 10-18 J 
E)  -2.04 × 10-18 J

Question 15

Choose the valence orbital diagram that represents the ground state of Sr2⁺.

Accepted Answer

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

Question 16

Identify the colour of a flame test for potassium.

Accepted Answer

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

Question 17

An electron initially in the n = 5 orbital of a hydrogen atom emits a photon with a wavelength of 1284 nm. Calculate the final orbital, nf.

Accepted Answer

A)  1 
B)  3 
C)  2 
D)  6 
E)  4 
A)  1 
B)  3 
C)  2 
D)  6 
E)  4

Question 18

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. 
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.

Question 19

How many orbitals are there in the fourth shell?

Accepted Answer

A)  3 
B)  4 
C)  6 
D)  16 
A)  3 
B)  4 
C)  6 
D)  16

Question 20

Identify the ground-state electron configuration for Rb⁺.

Accepted Answer

A)  [Ar]4s24p6 
B)  [Kr]5s1 
C)  [Ar]4s23d104p6 
D)  [Kr]5s2 
E)  [Kr]5s24d2 
A)  [Ar]4s24p6 
B)  [Kr]5s1 
C)  [Ar]4s23d104p6 
D)  [Kr]5s2 
E)  [Kr]5s24d2

Exam 7: The Quantum-Mechanical Model of the Atom

Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error.

When filling degenerate orbitals, electrons fill them singly first, with parallel spins. What is this known as?

Why do atoms only emit certain wavelengths of light when they are excited? (Why do line spectra exist?)

Choose the valence orbital diagram that represents the ground state of Se2⁻.

An FM radio station broadcasts electromagnetic radiation at a frequency of 100.5 MHz. The wavelength of this radiation is ________ m.

Choose the ground-state electron configuration for Cr3⁺.

What total energy (in kJ) is contained in 1.0 mol of photons, all with a frequency of 2.75 × 1014 Hz?

If two electrons in the same atom have the same value of l, they are ________.

Which of the following statements is TRUE?

Each of the following sets of quantum numbers is supposed to specify an orbital. Which of the following sets of quantum numbers contains an error?

How many different values of l are possible in the third principal level?

Calculate the energy of the green light emitted, per photon, by a mercury lamp with a frequency of 5.49 × 1014 Hz.

Choose the valence orbital diagram that represents the ground state of Zn.

Calculate the energy change associated with the transition from n = 4 to n = 1 in the hydrogen atom.

Choose the valence orbital diagram that represents the ground state of Sr2⁺.

Identify the colour of a flame test for potassium.

An electron initially in the n = 5 orbital of a hydrogen atom emits a photon with a wavelength of 1284 nm. Calculate the final orbital, nf.

Which of the following statements is TRUE?

How many orbitals are there in the fourth shell?

Identify the ground-state electron configuration for Rb⁺.

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 Metallurgy

Transition Metals and Coordination Compounds

Filters

Choose the valence orbital diagram that represents the ground state of Se²⁻.

Choose the ground-state electron configuration for Cr³⁺.

What total energy (in kJ) is contained in 1.0 mol of photons, all with a frequency of 2.75 × 10¹⁴ Hz?

Calculate the energy of the green light emitted, per photon, by a mercury lamp with a frequency of 5.49 × 10¹⁴ Hz.

Choose the valence orbital diagram that represents the ground state of Sr²^⁺.

An electron initially in the n = 5 orbital of a hydrogen atom emits a photon with a wavelength of 1284 nm. Calculate the final orbital, n_f.