Chapter 7: Q42E (page 281)
In Appendix G. the operator for the square of the angular momentum is shown to be
Use this to rewrite equation (7-19) as
Chapter 7: Q42E (page 281)
In Appendix G. the operator for the square of the angular momentum is shown to be
Use this to rewrite equation (7-19) as
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Get started for freeThe space between two parallel metal plates is filled with an element in a gaseous stale. Electrons leave one plate at negligible speed and are accelerated toward the other by a potential differenceapplied between the plates. As is increased from 0, the electron current increases more or less linearly, but when reaches 4.9 V , the current drops precipitously. From nearly 0 , it builds again roughly linearly as is increased beyond 4.9 V .
(a) How can the presence of the gas explain these observations?
(b) The Gas emits pure “light” when exceeds 4.9 V . What is its wavelength?
Some degeneracies are easy to understand on the basis of symmetry in the physical situation. Others are surprising, or “accidental”. In the states given in Table 7.1, which degeneracies, if any, would you call accidental and why?
In general, we might say that the wavelengths allowed a bound particle are those of a typical standing wave, , where is the length of its home. Given that , we would have , and the kinetic energy, , would thus be . These are actually the correct infinite well energies, for the argumentis perfectly valid when the potential energy is 0 (inside the well) and is strictly constant. But it is a pretty good guide to how the energies should go in other cases. The length allowed the wave should be roughly the region classically allowed to the particle, which depends on the “height” of the total energy E relative to the potential energy (cf. Figure 4). The “wall” is the classical turning point, where there is nokinetic energy left: . Treating it as essentially a one-dimensional (radial) problem, apply these arguments to the hydrogen atom potential energy (10). Find the location of the classical turning point in terms of E , use twice this distance for (the electron can be on both on sides of the origin), and from this obtain an expression for the expected average kinetic energies in terms of E . For the average potential, use its value at half the distance from the origin to the turning point, again in terms of . Then write out the expected average total energy and solve for E . What do you obtain
for the quantized energies?
The only visible spectral lines of hydrogen are four Balmer series lines noted at the beginning of Section 7.3. We wish to cause hydrogen gas to glow with its characteristic visible colors.
(a) To how high an energy level must the electrons be exited?
(b) Energy is absorbed in collisions with other particles. Assume that after absorbing energy in one collision, an electron jumps down through lower levels so rapidly that it is in the ground state before another collision occurs. If an electron is to be raised to the level found in part (a), how much energy must be available in a single collision?
(c) If such energetic collisions are to be affected simply by heating the gas until the average kinetic energy equals the desired upward energy jump, what temperature would be required? (This explains why heating is an impractical way to observe the hydrogen spectrum. Instead, the atoms are ionized by strong electric fields, as is the air when a static electric spark passes through.)
Doubly ionized lithium, absorbs a photon and jumps from the ground state to its n=2level. What was the wavelength of the photon?
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