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What differences can you think of between the photon and the electron? |
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2 | |
The photon and the neutrino both have neither charge nor mass. What are the differences between them? |
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3 | |
(a) Compare the evidence for the wave nature of light with the evidence for its particle nature. (b) Why do you think the wave nature of light was established long before its particle nature? |
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4 | |
A certain metal surface emits electrons when light is shone on it. (a) How can the number of electrons per second be increased? (b) How can the energies of the electrons be increased? |
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5 | |
Energy is carried in light by means of separate photons, yet even the faintest light we can see does not appear as a series of flashes. Explain. |
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6 | |
How does the speed of a photon compare with the speed of an em wave? |
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7 | |
When the speed of the electrons that strike a metal surface is increased, what happens to the speed, energy, and number per second of the x-ray photons that are emitted? |
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8 | |
If Planck's constant were smaller than it is, would quantum phenomena be more or less conspicuous than they are now? |
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9 | |
How does the speed of a matter wave compare with the speed of an em wave? |
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10 | |
The uncertainty principle applies to all bodies, yet its consequences are significant only for such extremely small particles as electrons, protons, and neutrons. Explain. |
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11 | |
Must a particle have an electric charge in order for matter waves to be associated with its motion? |
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12 | |
What kind of experiment might you use to distinguish between a gamma ray of wavelength 10-11 m and an electron whose de Broglie wavelength is also 10-11 m? |
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13 | |
A photon and a proton have the same wavelength. How does the photon's energy compare with the proton's kinetic energy? |
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14 | |
A proton and an electron have the same de Broglie wavelength. How do their speeds compare? |
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15 | |
What kind of spectrum is observed in (a) light from the hot filament of a lightbulb; (b) light from a sodium-vapor highway lamp; (c) light from a lightbulb surrounded by cool sodium vapor? |
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16 | |
How are the Bohr and Rutherford models of the hydrogen atom related? In the Bohr model, why is the electron pictured as revolving around the nucleus? |
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17 | |
In the Bohr model of the atom, the electron is in constant motion. How can such an electron have a negative amount of energy? |
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18 | |
Why does the hydrogen spectrum contain many lines, even though the hydrogen atom has only a single electron? |
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19 | |
Why is the Bohr theory incompatible with the uncertainty principle? |
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20 | |
On the basis of the Bohr model of the atom, explain why the absorption lines in the spectrum of hydrogen have the same wavelengths as some of the emission lines of the same element. |
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21 | |
(a) What is meant by the ground state of an atom? (b) What is the quantum number of the ground state of a hydrogen atom in the Bohr model? |
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22 | |
What is coherent light? Is the light from a lightbulb coherent? The light from the sun? |
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23 | |
What is a metastable atomic state? |
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24 | |
How is quantum mechanics related to Newtonian Mechanics? |
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25 | |
In what way does light from a laser differ from light from other sources? |
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26 | |
Why is the optical length of a laser so important? |
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27 | |
The Bohr theory permits us to visualize the structure of the atom, whereas quantum mechanics is very complex and concerned with such ideas as wave functions and probabilities. What reasons would lead to the replacement of the Bohr theory by quantum mechanics? |
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28 | |
What physical quantities are governed by the quantum numbers of an atomic electron? |
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29 | |
Under what circumstances do electrons exhibit spin? |
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30 | |
Under what circumstances can two electrons share the same probability cloud in an atom? |
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