Answered: What is the transition in hydrogen that…

Chemistry In Focus

7th Edition

ISBN:9781337399692

Author:Tro, Nivaldo J.

Publisher:Tro, Nivaldo J.

Chapter7: Light And Color

Section: Chapter Questions

Problem 30E: Arrange the following three frequencies of light in order of increasing energy per photon:...

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Similar questions

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.)
6.86 An excited He+ ion returns to the ground state by emitting a series of three photons, with wavelengths of 26 nm, 469 nm, and 1014 nm. The process is represented in the energy level diagram below. Which arrow (A, B, or C) in the diagram represents the 1014-nm light?
Helium absorbs light at 587.6 nm. What is the frequency of this light?
Which photons contain more energy, X-ray photons with a frequency of 31017 Hz or ultraviolet photons with a frequency of 21015 Hz? X-ray photons Ultraviolet photons Neither. They both contain the same energy per photon.
A ruby laser puts out a pulse of red light at a wavelength of 694 nm. (The ruby laser is described in the essay on p 226.) If a pulse delivers 1.05 105 watts of power for 280 s, how many photons are there in this pulse? (1 watt = 1 J/s.)
The lasers used in supermarket scanners emit red light at a wavelength of 633 nm. Compact disc players use lasers that emit light (that is not visible) at 840 nm. Which photonsthose emitted by supermarket scanners or compact disc (CD) playerscontain more energy per photon? Supermarket scanners CD players They both contain the same amount of energy per photon.
An atom in its ground state absorbs a photon (photon 1), then quickly emits another photon (photon 2). One of these photons corresponds to ultraviolet radiation, whereas the other one corresponds to red light. Explain what is happening. Which electromagnetic radiation, ultraviolet or red light, is associated with the emitted photon (photon 2)?
Radio waves in the AM region have frequencies in the range 530 to 1700 kilocycles per second (530 to 1700 kHz). Calculate the wavelength corresponding to a radio wave of frequency 1.460 106/s (that is, 1460 kHz).
Microwaves have frequencies in the range 109 to 1012/s (cycles per second), equivalent to between 1 gigahertz and 1 terahertz. What is the wavelength of microwave radiation whose frequency is 1.395 1010/s?
Of the following possible transitions of an electron in a hydrogen atom, which emits light of the highest energy? a Transition from the n = 1 to the n = 3 level b Transition from the n = 1 to the n = 2 level c Transition from the n = 3 to the n = 1 level d Transition from the n = 2 to the n = 1 level e Transition from the n = 5 to the n = 4 level
6.85 The visible lines in the hydrogen atom emission spectrum arise from transitions with a final state with n = 2. In what spectral region should we expect to find transitions that have a final state of n = 1 ? Explain your reasoning using an energy level diagram similar to the one in Problem 6.26.
Given the following energy level diagram for an atom that contains an electron in the n = 3 level, answer the following questions. a Which transition of the electron will emit light of the lowest frequency? b Using only those levels depicted in the diagram, which transition of the electron would require the highest-frequency light? c If the transition from the n = 3 level to the n = 1 level emits green light, what color light is absorbed when an electron makes the transition from the n = 1 to n = 3 level?

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	4 → 2
	5 → 2
	3 → 2

What is the transition in hydrogen that emits light of 486 nm? Question 11 options: 4 → 2 5 → 2 3 → 2