Question 1

Calculate the wavelength in meters of light absorbed by an electron in an atom of hydrogen as it moves from n = 3 to n = 6.

Accepted Answer

A)  1.09 × 10-6 m 
B)  8.22 × 10-7 m 
C)  3.28 × 10-6 m 
D)  1.83 × 10-7 m 
E)  1.65 × 10-11 m 
A)  1.09 × 10-6 m 
B)  8.22 × 10-7 m 
C)  3.28 × 10-6 m 
D)  1.83 × 10-7 m 
E)  1.65 × 10-11 m A

Question 2

What is the frequency associated with radiation of 4.59 × 10-8 cm wavelength?

Accepted Answer

A)  6.54 × 1017 s-1 
B)  6.54 × 1015 s-1 
C)  1.53 × 10-8 s-1 
D)  13.8 s-1 
E)  2.18 × 107 s-1 
A)  6.54 × 1017 s-1 
B)  6.54 × 1015 s-1 
C)  1.53 × 10-8 s-1 
D)  13.8 s-1 
E)  2.18 × 107 s-1 A

Question 3

The quantum numbers of the last electron of barium are ________.

Accepted Answer

A)  n = 6, ℓ = 0, mℓ = 1, ms = 1 
B)  n = 5, ℓ = 0, mℓ = 0, ms = 1/2 
C)  n = 6, ℓ = 0, mℓ = 1, ms = 1/2 
D)  n = 6, ℓ = 1, mℓ = 0, ms = 1/2 
E)  n = 6, ℓ = 0, mℓ = 0, ms = 1/2 
A)  n = 6, ℓ = 0, mℓ = 1, ms = 1 
B)  n = 5, ℓ = 0, mℓ = 0, ms = 1/2 
C)  n = 6, ℓ = 0, mℓ = 1, ms = 1/2 
D)  n = 6, ℓ = 1, mℓ = 0, ms = 1/2 
E)  n = 6, ℓ = 0, mℓ = 0, ms = 1/2 E

Question 4

Which of the following statements about the electron spin quantum number is FALSE?

Accepted Answer

A)  ms denotes the spin quantum number. 
B)  The value of the spin quantum number can be +1/2 or -1/2. 
C)  The value of the spin quantum number does not depend on other quantum numbers. 
D)  The value of the spin quantum number can be indicated by arrows to the right and to the left. 
E)  The spin quantum number is an indication that electrons generate a magnetic field. 
A)  ms denotes the spin quantum number. 
B)  The value of the spin quantum number can be +1/2 or -1/2. 
C)  The value of the spin quantum number does not depend on other quantum numbers. 
D)  The value of the spin quantum number can be indicated by arrows to the right and to the left. 
E)  The spin quantum number is an indication that electrons generate a magnetic field.

Question 5

Calculate the energy in kJ/mol of light with a wavelength of 360 nm.

Accepted Answer

A)  5.52 × 10-22 kJ/mol 
B)  5.52 × 10-19 kJ/mol 
C)  332 kJ/mol 
D)  6.63 × 103 kJ/mol 
E)  0.332 kJ/mol 
A)  5.52 × 10-22 kJ/mol 
B)  5.52 × 10-19 kJ/mol 
C)  332 kJ/mol 
D)  6.63 × 103 kJ/mol 
E)  0.332 kJ/mol

Question 6

Use Planck's equation to determine the wavelength, in nm, of radiation with 200.0 kJ/mol of energy.

Accepted Answer

A)  167 nm 
B)  598 nm 
C)  5.98 × 105 nm 
D)  1.67 × 105 nm 
E)  242 nm 
A)  167 nm 
B)  598 nm 
C)  5.98 × 105 nm 
D)  1.67 × 105 nm 
E)  242 nm

Question 7

What is the energy in joules of the 656 nm spectral line of hydrogen?

Accepted Answer

A)  4.35 × 10-31 J 
B)  3.03 × 10-19 J 
C)  1.30 × 10-22 J 
D)  3.03 × 10-28 J 
E)  1.45 × 10-48 J 
A)  4.35 × 10-31 J 
B)  3.03 × 10-19 J 
C)  1.30 × 10-22 J 
D)  3.03 × 10-28 J 
E)  1.45 × 10-48 J

Question 8

The ground state electron configuration for antimony is ________.

Accepted Answer

A)  [Kr] 5s25d105p3 
B)  [Kr] 4s24d105p3 
C)  [Xe] 5s24d105p2 
D)  [Kr] 4d105s25p3 
E)  [Xe] 5s25d105p3 
A)  [Kr] 5s25d105p3 
B)  [Kr] 4s24d105p3 
C)  [Xe] 5s24d105p2 
D)  [Kr] 4d105s25p3 
E)  [Xe] 5s25d105p3

Question 9

Arrange the following in order of increasing ENERGY: UV radiation, visible radiation, X-rays, and microwaves.

Accepted Answer

A)  X-rays < microwave < UV < visible 
B)  X-ray < microwave < visible < UV 
C)  microwave < visible < UV < X-rays 
D)  visible < UV < X-rays < microwave 
E)  UV < X-rays < microwave < visible 
A)  X-rays < microwave < UV < visible 
B)  X-ray < microwave < visible < UV 
C)  microwave < visible < UV < X-rays 
D)  visible < UV < X-rays < microwave 
E)  UV < X-rays < microwave < visible

Question 10

Exceptions to ________ are represented by chromium and copper in the 4th row of the periodic table.

Accepted Answer

A)  the Aufbau Principle 
B)  Hund's Rule 
C)  the Bohr Theory 
D)  the Heisenberg Principle 
E)  the Pauli Exclusion Principle 
A)  the Aufbau Principle 
B)  Hund's Rule 
C)  the Bohr Theory 
D)  the Heisenberg Principle 
E)  the Pauli Exclusion Principle

Question 11

What is the total number of orbitals possible for n = 3?

Accepted Answer

A)  9 
B)  6 
C)  5 
D)  3 
E)  11 
A)  9 
B)  6 
C)  5 
D)  3 
E)  11

Question 12

The fact that the valence orbital configuration of nitrogen in the ground state is 2s2, 2px12py12pz1 is an illustration of:

Accepted Answer

A)  the Bohr Theory 
B)  Hund's Rule 
C)  the Aufbau Principle 
D)  the Pauli Exclusion Principle 
E)  the Heisenberg Uncertainty Principle 
A)  the Bohr Theory 
B)  Hund's Rule 
C)  the Aufbau Principle 
D)  the Pauli Exclusion Principle 
E)  the Heisenberg Uncertainty Principle

Question 13

Which two orbitals are located between the axes of a coordinate system and not along the axes?

Accepted Answer

A)  dxy, py 
B)  dyz, px 
C)  dx2-y2, pz 
D)  dxy, dz2 
E)  dxy, dyz 
A)  dxy, py 
B)  dyz, px 
C)  dx2-y2, pz 
D)  dxy, dz2 
E)  dxy, dyz

Question 14

What is the wavelength of a bullet that is 0.450 g traveling at 2000. m/s?

Accepted Answer

A)  2000. m 
B)  2.94 × 10-24 m 
C)  7.36 × 10-34 m 
D)  7.36 × 10-37 m 
E)  1.49 × 10-40 m 
A)  2000. m 
B)  2.94 × 10-24 m 
C)  7.36 × 10-34 m 
D)  7.36 × 10-37 m 
E)  1.49 × 10-40 m

Question 15

Calculate the wavelength, in nm, of the first line of the Balmer series. The constant for Balmer's equation is 3.2881 × 1015 s-1.

Accepted Answer

A)  18.3 nm 
B)  656 nm 
C)  547 nm 
D)  152 nm 
E)  252 nm 
A)  18.3 nm 
B)  656 nm 
C)  547 nm 
D)  152 nm 
E)  252 nm

Question 16

The photoelectric effect:

Accepted Answer

A)  was discovered by Max Planck 
B)  describes the phenomenon of producing light by shining a beam of electrons by on any metal surface 
C)  contradicted the view that light energy was dependent upon intensity only 
D)  is not the same principle used in modern electric eyes and solar calculators 
E)  results in a beam of electrons which increases in number, but not velocity, as the wavelength of incident light decreases 
A)  was discovered by Max Planck 
B)  describes the phenomenon of producing light by shining a beam of electrons by on any metal surface 
C)  contradicted the view that light energy was dependent upon intensity only 
D)  is not the same principle used in modern electric eyes and solar calculators 
E)  results in a beam of electrons which increases in number, but not velocity, as the wavelength of incident light decreases

Question 17

When an electron goes from a high energy state to a low one, another electron goes from a low energy state to a high one.

Accepted Answer

A) True 
 B)False

Question 18

Give the appropriate values of n and ℓ for the orbital designation 3p.

Accepted Answer

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

Question 19

What is the orbital designation for the quantum numbers n = 2, ℓ = 1?

Accepted Answer

A)  3s 
B)  2s 
C)  2d 
D)  2p 
E)  3p 
A)  3s 
B)  2s 
C)  2d 
D)  2p 
E)  3p

Question 20

What is the energy in joules of the 434 nm spectral line of hydrogen?

Accepted Answer

A)  1.53 × 10-27 J 
B)  4.58 × 10-28 J 
C)  1.04 × 1048 J 
D)  4.58 × 10-19 J 
E)  9.59 × 10-49 J 
A)  1.53 × 10-27 J 
B)  4.58 × 10-28 J 
C)  1.04 × 1048 J 
D)  4.58 × 10-19 J 
E)  9.59 × 10-49 J

Exam 8: Electrons in Atoms

Calculate the wavelength in meters of light absorbed by an electron in an atom of hydrogen as it moves from n = 3 to n = 6.

What is the frequency associated with radiation of 4.59 × 10-8 cm wavelength?

The quantum numbers of the last electron of barium are ________.

Which of the following statements about the electron spin quantum number is FALSE?

Calculate the energy in kJ/mol of light with a wavelength of 360 nm.

Use Planck's equation to determine the wavelength, in nm, of radiation with 200.0 kJ/mol of energy.

What is the energy in joules of the 656 nm spectral line of hydrogen?

The ground state electron configuration for antimony is ________.

Arrange the following in order of increasing ENERGY: UV radiation, visible radiation, X-rays, and microwaves.

Exceptions to ________ are represented by chromium and copper in the 4th row of the periodic table.

What is the total number of orbitals possible for n = 3?

The fact that the valence orbital configuration of nitrogen in the ground state is 2s2, 2px12py12pz1 is an illustration of:

Which two orbitals are located between the axes of a coordinate system and not along the axes?

What is the wavelength of a bullet that is 0.450 g traveling at 2000. m/s?

Calculate the wavelength, in nm, of the first line of the Balmer series. The constant for Balmer's equation is 3.2881 × 1015 s-1.

The photoelectric effect:

When an electron goes from a high energy state to a low one, another electron goes from a low energy state to a high one.

Give the appropriate values of n and ℓ for the orbital designation 3p.

What is the orbital designation for the quantum numbers n = 2, ℓ = 1?

What is the energy in joules of the 434 nm spectral line of hydrogen?

Matter - Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Additional Aspects

Intermolecular Forces: Liquids and Solids

Solutions and Their Physical Properties

Chemical Kinetics

Principles of Chemical Equilibrium

Acids and Bases

Additional Aspects of Acid-Base Equilibria

Solubility and Complex-Ion Equilibria

Spontaneous Change: Entropy and Free Energy

Electrochemistry

Main Group Elements I: Groups 1, 2, 13, and 14

Main Group Elements II: Groups 18, 17, 16, 15, and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry 1-41

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

Filters

What is the frequency associated with radiation of 4.59 × 10^-8 cm wavelength?

Calculate the wavelength, in nm, of the first line of the Balmer series. The constant for Balmer's equation is 3.2881 × 10¹⁵ s-1.