Question 1

No two electrons can have the same four quantum numbers. 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 2

Calculate the wavelength (in nm) of the red light emitted by a neon sign with a frequency of 4.74 × 1014 Hz.

Accepted Answer

A)  633 nm 
B)  158 nm 
C)  142 nm 
D)  704 nm 
E)  466 nm 
A)  633 nm 
B)  158 nm 
C)  142 nm 
D)  704 nm 
E)  466 nm

Question 3

Calculate the wavelength of light associated with the transition from n = 1 to n = 3 in the hydrogen atom.

Accepted Answer

A)  103 nm 
B)  155 nm 
C)  646 nm 
D)  971 nm 
E)  136 nm 
A)  103 nm 
B)  155 nm 
C)  646 nm 
D)  971 nm 
E)  136 nm

Question 4

Define diffraction.

Accepted Answer

When a wave encounters an obst

Question 5

An electron ends in orbital n = 4 after a hydrogen atom absorbs a photon with a wavelength of 486 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 6

What is the maximum number of p orbitals that are possible in the same level?

Accepted Answer

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

Question 7

Determine the energy change associated with the transition from n = 2 to n = 5 in the hydrogen atom.

Accepted Answer

A)  -2.18 × 10-19 J 
B)  +6.54 × 10-19 J 
C)  +4.58 × 10-19 J 
D)  -1.53 × 10-19 J 
E)  +3.76 × 10-19 J 
A)  -2.18 × 10-19 J 
B)  +6.54 × 10-19 J 
C)  +4.58 × 10-19 J 
D)  -1.53 × 10-19 J 
E)  +3.76 × 10-19 J

Question 8

Calculate the orbital for the hydrogen atom that contains an electron with an energy of -4.45 × 10-20 J.

Accepted Answer

A)  n = 5 
B)  n = 4 
C)  n = 1 
D)  n = 3 
E)  n = 7 
A)  n = 5 
B)  n = 4 
C)  n = 1 
D)  n = 3 
E)  n = 7

Question 9

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

Accepted Answer

A)  1.75 ×   
B)  5.71 ×   
C)  1.58 ×   
D)  1.58 ×   
E)  5.71 ×   
A)  1.75 ×   
B)  5.71 ×   
C)  1.58 ×   
D)  1.58 ×   
E)  5.71 ×

Question 10

Identify the numbers for ml for a d orbital.

Accepted Answer

A)  0, 1, 2, 3, 4 
B)  1, 2, 3, 4, 5 
C)  1, 2, 3 
D)  -2, -1, 0, 1, 2 
A)  0, 1, 2, 3, 4 
B)  1, 2, 3, 4, 5 
C)  1, 2, 3 
D)  -2, -1, 0, 1, 2

Question 11

For hydrogen, what is the wavelength of the photon emitted when an electron drops from a 4d orbital to a 2p orbital in a hydrogen atom? The Rydberg constant is 1.097 × 10-2 nm-1.

Accepted Answer

A)  656.3 nm 
B)  486.2 nm 
C)  364.6 nm 
D)  2.057 × 10-3 nm 
A)  656.3 nm 
B)  486.2 nm 
C)  364.6 nm 
D)  2.057 × 10-3 nm

Question 12

Determine the mass of a ball with a velocity of 35.1 m s-1 and a wavelength of 8.92 × 10-34 m.

Accepted Answer

A)  26.0 g 
B)  594 g 
C)  2.08 g 
D)  47.3 g 
E)  21.2 g 
A)  26.0 g 
B)  594 g 
C)  2.08 g 
D)  47.3 g 
E)  21.2 g

Question 13

Place the following types of electromagnetic radiation in order of increasing wavelength. ultraviolet light gamma rays radio waves

Accepted Answer

A)  gamma rays < radio waves < ultraviolet light 
B)  radio waves < ultraviolet light < gamma rays 
C)  radio waves < gamma rays < ultraviolet light 
D)  ultraviolet light < gamma rays < radio waves 
E)  gamma rays < ultraviolet light < radio waves 
A)  gamma rays < radio waves < ultraviolet light 
B)  radio waves < ultraviolet light < gamma rays 
C)  radio waves < gamma rays < ultraviolet light 
D)  ultraviolet light < gamma rays < radio waves 
E)  gamma rays < ultraviolet light < radio waves

Question 14

Identify the correct values for a 1s 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 = 0, 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 = 0, ml = 0 
E)  n = 4, l = -1, ml = -2

Question 15

On the electromagnetic spectrum, visible light is immediately between two other wavelengths. Name them.

Accepted Answer

A)  infrared and X-ray 
B)  radio and microwave 
C)  gamma ray and ultraviolet 
D)  microwave and X-ray 
E)  infrared and ultraviolet 
A)  infrared and X-ray 
B)  radio and microwave 
C)  gamma ray and ultraviolet 
D)  microwave and X-ray 
E)  infrared and ultraviolet

Question 16

Which of the following colours of electromagnetic radiation has the shortest wavelength?

Accepted Answer

A)  blue 
B)  violet 
C)  orange 
D)  green 
E)  yellow 
A)  blue 
B)  violet 
C)  orange 
D)  green 
E)  yellow

Question 17

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 18

Calculate the wavelength (in nm) of the blue light emitted by a mercury lamp with a frequency of 6.88 × 1014 Hz.

Accepted Answer

A)  229 nm 
B)  436 nm 
C)  206 nm 
D)  485 nm 
E)  675 nm 
A)  229 nm 
B)  436 nm 
C)  206 nm 
D)  485 nm 
E)  675 nm

Question 19

Determine the energy change associated with the transition from n = 3 to n = 2 in the hydrogen atom.

Accepted Answer

A)  +3.03 × 10-19 J 
B)  -1.82 × 10-19 J 
C)  +5.51 × 10-19 J 
D)  -3.03 × 10-19 J 
E)  +2.69 × 10-19 J 
A)  +3.03 × 10-19 J 
B)  -1.82 × 10-19 J 
C)  +5.51 × 10-19 J 
D)  -3.03 × 10-19 J 
E)  +2.69 × 10-19 J

Question 20

Calculate the wavelength of an electron (m = 9.11 × 10-28 g) moving at 3.66 × 106 m s-1.

Accepted Answer

A)  1.99 × 10-10 m 
B)  5.03 × 10-10 m 
C)  1.81 × 10-10 m 
D)  5.52 × 10-9 m 
E)  2.76 × 10-9 m 
A)  1.99 × 10-10 m 
B)  5.03 × 10-10 m 
C)  1.81 × 10-10 m 
D)  5.52 × 10-9 m 
E)  2.76 × 10-9 m

Exam 7: The Quantum-Mechanical Model of the Atom

No two electrons can have the same four quantum numbers. What is this known as?

Calculate the wavelength (in nm) of the red light emitted by a neon sign with a frequency of 4.74 × 1014 Hz.

Calculate the wavelength of light associated with the transition from n = 1 to n = 3 in the hydrogen atom.

Define diffraction.

An electron ends in orbital n = 4 after a hydrogen atom absorbs a photon with a wavelength of 486 nm. Calculate the initial orbital, ni.

What is the maximum number of p orbitals that are possible in the same level?

Determine the energy change associated with the transition from n = 2 to n = 5 in the hydrogen atom.

Calculate the orbital for the hydrogen atom that contains an electron with an energy of -4.45 × 10-20 J.

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

Identify the numbers for ml for a d orbital.

For hydrogen, what is the wavelength of the photon emitted when an electron drops from a 4d orbital to a 2p orbital in a hydrogen atom? The Rydberg constant is 1.097 × 10-2 nm-1.

Determine the mass of a ball with a velocity of 35.1 m s-1 and a wavelength of 8.92 × 10-34 m.

Place the following types of electromagnetic radiation in order of increasing wavelength. ultraviolet light gamma rays radio waves

Identify the correct values for a 1s sublevel.

On the electromagnetic spectrum, visible light is immediately between two other wavelengths. Name them.

Which of the following colours of electromagnetic radiation has the shortest wavelength?

Identify the ground-state electron configuration for Se2⁻.

Calculate the wavelength (in nm) of the blue light emitted by a mercury lamp with a frequency of 6.88 × 1014 Hz.

Determine the energy change associated with the transition from n = 3 to n = 2 in the hydrogen atom.

Calculate the wavelength of an electron (m = 9.11 × 10-28 g) moving at 3.66 × 106 m s-1.

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

Calculate the wavelength (in nm) of the red light emitted by a neon sign with a frequency of 4.74 × 10¹⁴ Hz.

An electron ends in orbital n = 4 after a hydrogen atom absorbs a photon with a wavelength of 486 nm. Calculate the initial orbital, n_i.

Calculate the orbital for the hydrogen atom that contains an electron with an energy of -4.45 × 10^-20 J.

Identify the numbers for m_l for a d orbital.

For hydrogen, what is the wavelength of the photon emitted when an electron drops from a 4d orbital to a 2p orbital in a hydrogen atom? The Rydberg constant is 1.097 × 10^-2 nm^-1.

Determine the mass of a ball with a velocity of 35.1 m s^-1 and a wavelength of 8.92 × 10^-34 m.

Identify the ground-state electron configuration for Se²⁻.

Calculate the wavelength (in nm) of the blue light emitted by a mercury lamp with a frequency of 6.88 × 10¹⁴ Hz.

Calculate the wavelength of an electron (m = 9.11 × 10^-28 g) moving at 3.66 × 10⁶ m s^-1.