greater vel ocity? What is the velocity of the electrons? 4. Titanium ( 6.94 X 1019 J) 10 and silicon (D 7.24 X -19 J surfaces are irradiated with UV radiation with a wavelength of 250 nm. Which surface emits electrons with the longer wavelength? What is the wavelength of the electrons emitted by the titanium surface? 5. Red Lasers The power of a red laser (A = 630 nm) is 1.00 watt (abbreviated W, where 1 W = 1 J/s). How many photons per second does the laser emit? -6. Starlight The energy density of starlight in interstellar space is 1015 J/m3. If the average wavelength of starlight is 500 nm, what is the corresponding density of photons per cubic meter of space?

greater vel ocity? What is the velocity of the electrons? 4. Titanium ( 6.94 X 1019 J) 10 and silicon (D 7.24 X -19 J surfaces are irradiated with UV radiation with a wavelength of 250 nm. Which surface emits electrons with the longer wavelength? What is the wavelength of the electrons emitted by the titanium surface? 5. Red Lasers The power of a red laser (A = 630 nm) is 1.00 watt (abbreviated W, where 1 W = 1 J/s). How many photons per second does the laser emit? -6. Starlight The energy density of starlight in interstellar space is 1015 J/m3. If the average wavelength of starlight is 500 nm, what is the corresponding density of photons per cubic meter of space?

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter6: The Periodic Table And Atomic Structure

Section: Chapter Questions

Problem 6.71PAE: 6.71 Several excited states of the neon atom are important in the operation of a helium-neon laser....

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Similar questions

Imagine a world in which the rule for the l quantum number is that values start with 1 and go up to n. The rules for the n and mi quantum numbers are unchanged from those of our world. Write the quantum numbers for the first two shells (i.e., n = 1 and n = 2).
The root-mean-square speed of an oxygen molecule, O2, at 21C is 479 m/s. Calculate the de Broglie wavelength for an O2 molecule traveling at this speed. How does this wavelength compare with the approximate length of this molecule, which is about 242 pm? (For this comparison, state the wavelength as a percentage of the molecular length.)
A hydrogen atom in the ground stale absorbs a photon whose wavelength is 95.0 nm. The resulting excited atom then emits a photon of 1282 nm. What are the regions of the electromagnetic spectrum for the radiations involved in these transitions? What is the principal quantum number of the final state resulting from the emission from the excited atom?
What type of relationship (direct or inverse) e xists between wavelength, frequency, and photon energy? What does a photon energy unit of a joule equal?
The figure below represents part of the emission spectrum for a one-electron ion in lhe gas phase. All the lines result from electronic transitions from excited states to the n = 3 state. (See Exercise 160.) a. What electronic transitions correspond to lines A and B? b. If the wavelength of line B is 142.5 nm, calculate the wavelength of line A.
What is the de Broglie wavelength of a 149-g baseball traveling at 23.0 m/s (51.4 mph)? Is the wavelength much smaller or much larger than the diameter of an atom (on the order of 100 pm)?
The energy of a photon is 3.05 1019 J. What is the wavelength of the corresponding light? What is the color of this light?
Calculate the wavelength of the Balmer line of the hydrogen spectrum in which the initial n quantum number is 5 and the final n quantum number is 2.
A bright violet line occurs at 435.8 nm in the emission spectrum of mercury vapor. What amount of energy, in joules, must be released by an electron in a mercury atom to produce a photon of this light?
A particular transition of the rubidium atom emits light whose frequency is 3.84 1014 Hz. (Hz is the abbreviation for hertz, which is equivalent to the unit/s, or s1.) Is this light in the visible spectrum? If so, what is the color of the light? (See Figure 7.5.)
6.71 Several excited states of the neon atom are important in the operation of a helium-neon laser. In these excited states, one electron of the neon atom is promoted from the 2p level to a higher energy orbital. An excited neon atom with a 1s22s22p55s1 electron configuration can emit a photon with a wavelength of 3391 nm as it makes a transition to a lower energy state with a 1s22s22p54p1 electron configuration. Other transitions are also possible. If an excited neon atom with a 1s22s22p53p1 electron configuration makes a transition to a lower energy state with a 1s22s22p53p1 electron configuration, it emits a photon with a wavelength of 632.8 nm. Find the wavelength of the photon that would be emitted in a transition from the 1s22s22p54p1 electron configuration to the 1s22s22p53p1 electron configuration. (It should help if you start by drawing an energy-level diagram.)
The wave function for the 2pz, orbital in the hydrogen atom is 2pl=142(za0)3/2e/2cos where a0 is the value for the radius of the first Bohr orbit in meters (5.29 | 1011), is Z(r/a0), r is the value for the distance from the nucleus in meters, and is an angle. Calculate the value of 2pz2 at r = a0 for = 0 (z axis) and for = 90 (xy plane).

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