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Chapter 8: Electrons in Atoms
1, 4, 5, 11, 15, 19, 22, 25, 29, 39, 40, 50, 51, 57, 58, 59, 60, 71, 75, 82,
85 – 88, 101 , 123, 124, 126
Electromagnetic Radiation
1.” A hypothetical electromagnetic wave is pictured here. What is the wavelength of this
radiation?
4.” The most intense line in the cerium spectrum is at 418.7 nm.
(a) Determine the frequency of the radiation producing this line.
(b) In what part of the electromagnetic spectrum does this line occur?
(c) Is it visible to the eye? If so, what color is it? If not, is this line at higher or lower energy than
visible light?
5.” Without doing detailed calculations , determine which of the following wavelengths
represents light of the highest frequency:
(a)
(b) 1.13 mm;
(c) 860 Å;
(d)

Chapter 8 2
Atomic Spectra
11.” Use Planck's equation (8.3) to determine
(a) the energy, in joules per photon, of radiation of frequency
(b) the energy, in kilojoules per mole, of radiation of frequency
15.” Calculate the wavelengths, in nanometers, of the first four lines of the Balmer series of
the hydrogen spectrum, starting with the longest wavelength component.
Quantum Theory
19.” A certain radiation has a wavelength of 474 nm. What is the energy, in joules, of
(a) one photon;
(b) a mole of photons of this radiation?

Chapter 8 3