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Chapter 38: Q 11 (page 1114)
A red laser with a wavelength of 650 nm and a blue laser with a wavelength of 450 nm emit laser beams with the same light power. How do their rates of photon emission compare? Answer this by computing Rred/Rblue.
Rates of photon emission of red and blue laser can be compared as
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The electron interference pattern of Figure 38.12 was made by shooting electrons with of kinetic energy through two slits spaced role="math" localid="1650737433408" apart. The fringes were recorded on a detector behind the slits.
a. What was the speed of the electrons? (The speed is large enough to justify using relativity, but for simplicity do this as a nonrelativistic calculation.)
b. Figure 38.12 is greatly magnified. What was the actual spacing on the detector between adjacent bright fringes?
Potassium and gold cathodes are used in a photoelectric effect experiment. For each cathode, find:
a) The threshold frequency.
b) The threshold wavelength.
c) The maximum photoelectron ejection speed if the light has a wavelength of 220 nm.
d) The stopping potential if the wavelength is 220 nm
In the atom interferometer experiment shown in Figure laser cooling techniques were used to cool a dilute vapor of sodium atoms to a temperature of . The ultracold atoms passed through a series of collimating apertures to form the atomic beam you see circling the figure from the left. The standing light waves were created from a laser beam with a wavelength of
a. What is the rms speed of a sodium atom in a gas at this temperature ?
b. By treating the laser beam as if it were a diffraction grating. cakculate the first-order diffraction angle of a sodium atom traveling with the rms speed of part a.
c. allow far apart are points and if the second sanding wave is from the first?
d. Because interference is observed between the two paths, each individual atom is apparently present at both point and point . Describe, in your own words, what this experiment tells you about the nature of matter.
a. What wavelength photon does a hydrogen atom emit in a transition?
b. What is the difference in the wavelengths emitted in a localid="1650823513478" transition and a transition?
Consider a hydrogen atom in stationary state n.
a. Show that the orbital period of an electron in quantum state n is, and find a numerical value for
b. On average, an atom stays in the n = 2 state for 1.6 ns before undergoing a quantum jump to the n = 1 state. On average, how many revolutions does the electron make before the quantum jump?
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