Question 1

Which of the following visible colours of light has the longest wavelength?

Accepted Answer

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

Question 2

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 3

Which of the following types of electromagnetic radiation has the lowest frequency?

Accepted Answer

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

Question 4

How many subshells are there in the shell with n = 4?

Accepted Answer

A) 3 
B) 4 
C) 6 
D) 18 
A) 3 
B) 4 
C) 6 
D) 18

Question 5

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

Accepted Answer

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

Question 6

Which of the following transitions (in a hydrogen atom)represent absorption of the smallest frequency photon?

Accepted Answer

A) n = 5 to n = 6 
B) n = 5 to n = 4 
C) n = 4 to n = 1 
D) n = 1 to n = 3 
E) n = 1 to n = 2 
A) n = 5 to n = 6 
B) n = 5 to n = 4 
C) n = 4 to n = 1 
D) n = 1 to n = 3 
E) n = 1 to n = 2

Question 7

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 8

Identify the set of four quantum numbers that could represent the electron lost to form the Rb ION from the Rb atom.

Accepted Answer

A) n = 6, l = 0, ml = 0, ms = -   
B) n = 4, l = 1, ml = 1, ms = -   
C) n = 5, l = 1, ml = 0, ms = +   
D) n = 4, l = 1, ml = 0, ms = -   
E) n = 5, l = 0, ml = 0, ms = +   
A) n = 6, l = 0, ml = 0, ms = -   
B) n = 4, l = 1, ml = 1, ms = -   
C) n = 5, l = 1, ml = 0, ms = +   
D) n = 4, l = 1, ml = 0, ms = -   
E) n = 5, l = 0, ml = 0, ms = +

Question 9

Which ion does not have a noble gas configuration in its ground state?

Accepted Answer

A) Sc3+ 
B) Al3+ 
C) Ga3+ 
D) As3- 
A) Sc3+ 
B) Al3+ 
C) Ga3+ 
D) As3-

Question 10

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

Accepted Answer

A) The frequency decreases. 
B) The energy increases. 
C) The speed decreases. 
D) Planck's constant decreases. 
E) None of the above occurs as the wavelength of a photon increases. 
A) The frequency decreases. 
B) The energy increases. 
C) The speed decreases. 
D) Planck's constant decreases. 
E) None of the above occurs as the wavelength of a photon increases.

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

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 13

How much energy (in kJ)is required to ionize 2.78 moles of hydrogen atoms?

Accepted Answer

A) 2.74 × 103 kJ 
B) 4.72 × 103 kJ 
C) 1.66 × 103 kJ 
D) 3.65 × 103 kJ 
E) 5.89 × 103 kJ 
A) 2.74 × 103 kJ 
B) 4.72 × 103 kJ 
C) 1.66 × 103 kJ 
D) 3.65 × 103 kJ 
E) 5.89 × 103 kJ

Question 14

What value of l is represented by a d orbital?

Accepted Answer

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

Question 15

How many photons are contained in a flash of green light (525 nm)that contains 189 kJ of energy?

Accepted Answer

A) 5.67 × 1023 photons 
B) 2.01 × 1024 photons 
C) 1.25 × 1031 photons 
D) 4.99 × 1023 photons 
E) 7.99 × 1030 photons 
A) 5.67 × 1023 photons 
B) 2.01 × 1024 photons 
C) 1.25 × 1031 photons 
D) 4.99 × 1023 photons 
E) 7.99 × 1030 photons

Question 16

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 17

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 18

Match the following.

-n = 2 to n = 3

Accepted Answer

A) 657 nm 
B) 7460 nm 
C) 103 nm 
D) 1280 nm 
E) 122 nm 
A) 657 nm 
B) 7460 nm 
C) 103 nm 
D) 1280 nm 
E) 122 nm

Question 19

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 20

Which of the following quantum numbers describes the size and energy of an orbital?

Accepted Answer

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

Exam 7: The Quantum-Mechanical Model of the Atom

Which of the following visible colours of light has the longest wavelength?

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

Which of the following types of electromagnetic radiation has the lowest frequency?

How many subshells are there in the shell with n = 4?

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

Which of the following transitions (in a hydrogen atom)represent absorption of the smallest frequency photon?

Identify the correct values for a 1s sublevel.

Identify the set of four quantum numbers that could represent the electron lost to form the Rb ION from the Rb atom.

Which ion does not have a noble gas configuration in its ground state?

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

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.

Choose the ground-state electron configuration for Cr3⁺.

How much energy (in kJ)is required to ionize 2.78 moles of hydrogen atoms?

What value of l is represented by a d orbital?

How many photons are contained in a flash of green light (525 nm)that contains 189 kJ of energy?

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

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.

Match the following. -n = 2 to n = 3

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.

Which of the following quantum numbers describes the size and energy of an orbital?

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Filters

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

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.

Choose the ground-state electron configuration for Cr³⁺.

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