Suggested problems Chapter 7
7.19
Consider two beams of the same yellow light. Imagine that one beam has its wavelength doubled; the other has
its frequency doubled. Which of these beams is then in the ultraviolet region?
7.27
Given the following energy diagram for an atom that contains an electron in the n = 3 level, answer the following
questions.
n=5
n=4
Energy (E)
n=3
n=2
n=1
a. Which transition of the electron will emit the lowest frequency light?
b. Using only those levels depicted in the diagram, which transition of the electron would require the highest
frequency light?
c. If the transition from the n = 3 level to the n = 1 level emits green light, what color light is absorbed when an
electron makes the transition from the n = 1 to n = 3 level?
7.29
Radio waves in the AM region have frequencies in the range 550 to 1600 kilocycles per second (550 to 1600
kHz). Calculate the wavelength corresponding to a radio wave of frequency 1.365 x 106/s (that is, 1365 kHz).
7.31
Light with a wavelength of 478 nm lies in the blue region of the visible spectrum. Calculate the frequency if this
light.
7.33
At its closest approach, Mars is 156 million km from Earth. How long would it take to send a radio message from
a space probe of Mars to Earth when the planets are at this closest distance?
7.37
What is the energy of a photon corresponding to radio waves of frequency 1.365 x 106/s?
7.39
The green line in the atomic spectrum of thallium has a wavelength of 535 nm. Calculate the energy of a photon
of this light.
7.41
A particular transition of the rubidium atom emits light whose frequency is 3.84 x 1014 Hz. Is this light in the
visible spectrum? If so, what is the color of the light?
7.57
If the n quantum number of an atomic orbital is 4, what are the possible values of 𝑙 ? If the quantum 𝑙 number is
3, what are the possible values of 𝑚𝑙 ?
7.59
How many subshells are there in the M shell? How many orbitals are there in the f subshell?
7.61
Give the notation (using letter designations for 𝑙) for the subshells denoted by the following quantum numbers?
a.
b.
c.
d.
7.63
𝑛 = 1, 𝑙
𝑛 = 1, 𝑙
𝑛 = 3, 𝑙
𝑛 = 0, 𝑙
𝑛 = 2, 𝑙
= 0, 𝑚𝑙
= 3, 𝑚𝑙
= 2, 𝑚𝑙
= 1, 𝑚𝑙
= 1, 𝑚𝑙
= 0, 𝑚𝑠 = +1
= +3, 𝑚𝑠 = +1/2
= +3, 𝑚𝑠 = −1/2
= 0, 𝑚𝑠 = +1/2
= +1, 𝑚𝑠 = +3/2
What is the number of different orbitals in each of the following subshells?
a. 3d
7.85
=2
=4
=3
=1
Explain why each of the following sets of quantum numbers would not be permissible for an electron, according
to the rules for quantum numbers.
a.
b.
c.
d.
e.
7.81
𝑛 = 6, 𝑙
𝑛 = 5, 𝑙
𝑛 = 4, 𝑙
𝑛 = 6, 𝑙
b. 4f
c. 4p
5s
The energy required to dissociate the Cl2 molecule to Cl atoms is 239 kJ/mol Cl2. If the dissociation of a Cl2
molecule were accomplished by the absorption of a single photon whose energy was exactly the quantity
required, what would be its wavelength (in meters).