Download Chapter 7 Homework questions

Chapter 7 Homework questions
21. Consider the colors of the visible spectrum.
(a) What colors of light involve less energy than green light?
(b) Which color of light has photons of greater energy, yellow or blue?
25. Violet light has a wavelength of about 410 nm. What is its frequency?
Calculate the energy of one photon of violet light.
What is the energy of 1.0 mol of violet photons?
Compare the energy of photons of violet light with those of red light. Which is more
energetic and by what factor?
29. Place the following types of radiation in order of increasing energy per photon:
(a) Radar signals
(b) Radiation within a microwave oven
(c) Gamma rays from a nuclear reaction (d) Red light from a neon sign
(e) Ultraviolet radiation from a sun lamp
31. You are an engineer designing a switch that works by the photoelectric effect. The
metal you wish to use in your device requires 6.7 X 10-19 J/atom to remove an electron.
Will the switch work if the light falling on the metal has a wavelength of 540 nm or
greater? Why or why not?
33. The most prominent line in the spectrum of neon is found at 865.438 nm. Other lines
are located at 837.761 nm, 878.062 nm, 878.375 nm, and 1885.387 nm.
(a) In what region of the electromagnetic spectrum are these lines found?
(b) Are any of these lines found in the spectrum of neon shown in Figure 7.9?
What color or colors are these lines?
(c) Which of these lines represents the most energetic light?
(d) What is the frequency of the most prominent line?
What is the energy of one photon with this wavelength?
39. Consider only transitions involving the n = 1 through n = 5 energy levels for the H
atom (where the line spacing is very approximate) .
_____ n=5
_____ n=4
(a) How many emission lines are possible, considering
only the five quantum levels?
_____ n=3
(b) Photons of the highest frequency are emitted in a transition from the level with n = ___ to a level with n =___
_____
n=2
_____
n=1
(c) The emission line having the longest wavelength
corresponds to a transition from the level with n = __ to
the level with n =_____
42. An electron moves with a velocity of 2.5 X 108 cm/s. What is its wavelength?
46. Quantum numbers:
(a) When n = 4, what are the possible values of l?
(b) When e is 2, what are the possible values of ml?
(c) For a 4s orbital, what are the possible values of n, l, and ml?
(d) For a 4f orbital, what are the possible values of n, l, and ml?
49. A possible excited state for the H atom has an electron in a 5d orbital. List all possible
sets of quantum numbers n, e, and me for this electron.
52. Explain briefly why each of the following is not a possible set of quantum numbers
for an electron in an atom.
(a) n = 2, l = 2, ml = 0
(b) n = 3, l = 0, ml = -2
(c) n = 6, l = 0, ml = 1
55. What is the maximum number of orbitals that can be identified by each of the
following sets of quantum numbers? When "none" is the correct answer, explain your
reasoning.
(a) n = 4, l = 3
(c) n = 5
(b) n = 2, l = 2
(d) n = 3, l = 1, ml= -1
61. A given orbital has a magnetic quantum number of ml = -1.
This could not be a (an)
(a) f orbital
(c) p orbital
(b) d orbital
(d) s orbital