Question 1

Electromagnetic radiation with a wavelength of 745 nm appears as red light to the human eye.The energy of one photon of this light is ________ J.

Accepted Answer

A)  1.48 × 10-31 
B)  2.67 × 10-28 
C)  2.67 × 10-19 
D)  1.48 × 10-22 
E)  3.75 × 1018 
A)  1.48 × 10-31 
B)  2.67 × 10-28 
C)  2.67 × 10-19 
D)  1.48 × 10-22 
E)  3.75 × 1018

Question 2

What are the possible values of l if n = 4?

Accepted Answer

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

Question 3

Identify the color 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

How much energy (in kJ)do 3.0 moles of photons,all with a wavelength of 670 nm,contain?

Accepted Answer

A)  179 kJ 
B)  358 kJ 
C)  412 kJ 
D)  536 kJ 
E)  242 kJ 
A)  179 kJ 
B)  358 kJ 
C)  412 kJ 
D)  536 kJ 
E)  242 kJ

Question 5

Sketch one of the 3p orbitals below.How are they different from the 2p orbitals?

Accepted Answer

They are larger in s

Question 6

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 different sublevel. 
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 different sublevel. 
C)  in the same orbital. 
D)  in different levels and in different shaped orbitals. 
E)  none of the above.

Question 7

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 8

Calculate the frequency of light associated with the transition from n = 2 to n = 3 in the hydrogen atom.

Accepted Answer

A)  2.19 × 1014 s-1 
B)  5.59 × 1014 s-1 
C)  4.57 × 1014 s-1 
D)  1.79 × 1014 s-1 
E)  3.28 × 1014 s-1 
A)  2.19 × 1014 s-1 
B)  5.59 × 1014 s-1 
C)  4.57 × 1014 s-1 
D)  1.79 × 1014 s-1 
E)  3.28 × 1014 s-1

Question 9

What are the possible orbitals for n = 3?

Accepted Answer

A)  s, p, d 
B)  s, p, d, f 
C)  s 
D)  s, p 
A)  s, p, d 
B)  s, p, d, f 
C)  s 
D)  s, p

Question 10

Identify the color that has a wavelength of 545 nm.

Accepted Answer

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

Question 11

Which of the following colors 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 12

Give an example of a d orbital.

Accepted Answer

The answer of Give an example of a d orbital....

Question 13

Identify the orbital.

Accepted Answer

A)  pz orbital 
B)  dxy orbital 
C)  px orbital 
D)  dyz orbital 
E)  py orbital 
A)  pz orbital 
B)  dxy orbital 
C)  px orbital 
D)  dyz orbital 
E)  py orbital

Question 14

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

Question 15

It is possible to determine the ionization energy for hydrogen using the Bohr equation.Calculate the ionization energy (in kJ)for a mole of hydrogen atoms,making the assumption that ionization is the transition from n = 1 to n = ∞.

Accepted Answer

A)  7.62 × 103 kJ 
B)  2.76 × 103 kJ 
C)  1.31 × 103 kJ 
D)  3.62 × 103 kJ 
E)  5.33 × 103 kJ 
A)  7.62 × 103 kJ 
B)  2.76 × 103 kJ 
C)  1.31 × 103 kJ 
D)  3.62 × 103 kJ 
E)  5.33 × 103 kJ

Question 16

Determine the mass of a ball with a velocity of 45.0 m/s and a wavelength of 8.92 × 10-34 m.

Accepted Answer

A)  33.4 g 
B)  594 g 
C)  2.66 g 
D)  60.6 g 
E)  16.5 g 
A)  33.4 g 
B)  594 g 
C)  2.66 g 
D)  60.6 g 
E)  16.5 g

Question 17

Match between columns
                        Premises: n = 5 to n = 3
n = 2 to n = 3
n = 3 to n = 1
n = 1 to n = 2
n = 6 to n = 5

Accepted Answer

The Answer of 657 nm and 103 nm and 7460 is...

Question 18

Determine the mass of a ball with a wavelength of 3.45 × 10-34 m and a velocity of 6.55 m/s.

Accepted Answer

A)  0.293 g 
B)  12.6 g 
C)  293 g 
D)  346 g 
E)  3.41 g 
A)  0.293 g 
B)  12.6 g 
C)  293 g 
D)  346 g 
E)  3.41 g

Question 19

Identify the color that has a wavelength of 480 nm.

Accepted Answer

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

Question 20

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

Accepted Answer

A)  0 
B)  3 
C)  6 
D)  12 
E)  9 
A)  0 
B)  3 
C)  6 
D)  12 
E)  9

Exam 7: The Quantum-Mechanical Model of the Atom

Electromagnetic radiation with a wavelength of 745 nm appears as red light to the human eye.The energy of one photon of this light is ________ J.

What are the possible values of l if n = 4?

Identify the color of a flame test for sodium.

How much energy (in kJ)do 3.0 moles of photons,all with a wavelength of 670 nm,contain?

Sketch one of the 3p orbitals below.How are they different from the 2p orbitals?

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

What value of l is represented by a d orbital?

Calculate the frequency of light associated with the transition from n = 2 to n = 3 in the hydrogen atom.

What are the possible orbitals for n = 3?

Identify the color that has a wavelength of 545 nm.

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

Give an example of a d orbital.

Identify the orbital.

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

It is possible to determine the ionization energy for hydrogen using the Bohr equation.Calculate the ionization energy (in kJ)for a mole of hydrogen atoms,making the assumption that ionization is the transition from n = 1 to n = ∞.

Determine the mass of a ball with a velocity of 45.0 m/s and a wavelength of 8.92 × 10-34 m.

Determine the mass of a ball with a wavelength of 3.45 × 10-34 m and a velocity of 6.55 m/s.

Identify the color that has a wavelength of 480 nm.

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

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Determine the mass of a ball with a velocity of 45.0 m/s and a wavelength of 8.92 × 10^-34 m.

Determine the mass of a ball with a wavelength of 3.45 × 10^-34m and a velocity of 6.55 m/s.