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2. Rank the following three transitions in the hydrogen atom in terms of lowest to highest wave- length, energy, and frequency: 6 → 5, 3 → 1, 7-→ 3. Note that the energy levels in Figure 2.2 are shown schematically, so you must calculate the energy difference between any two levels in order to answer this question. Show all calculations below or on the following page. Wavelength: Energy: Frequency:

2. Rank the following three transitions in the hydrogen atom in terms of lowest to highest wave- length, energy, and frequency: 6 → 5, 3 → 1, 7-→ 3. Note that the energy levels in Figure 2.2 are shown schematically, so you must calculate the energy difference between any two levels in order to answer this question. Show all calculations below or on the following page. Wavelength: Energy: Frequency:

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter7: Quantum Theory Of The Atom
Section: Chapter Questions
Problem 7.47QP: A particular transition of the rubidium atom emits light whose frequency is 3.84 1014 Hz. (Hz is...
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Ultraviolet Visible Infrared 5 1 4-1 3 1 2 1 4. 3 and corresponding wavelengths in the The emission spectrum then consists of discrete lines rather than a continuum in which light is emitted at all frequencies. Many such electronic transitions take place with emission of light in the visible region of wavelength 370-700 nm; these transitions can be observed with relatively sp set of "orbits" is not equal). The wavelength of light in the electromagnetic spectrum corr sponding to changes in electronic states in h drogen were described empirically by Rydbe according to the formula: simple equipment and the human eye. It is also possible to examine changes in energy states of 1. R. 1. 1. H. n=5 n=4 Lyman series n=3 6-1 High energy n=2 6 2 5+2 Balmer 4 2 series n=1 H. 3 2 OHayden-McNeil, LLC n-2 6 3 Low energy n=3 Paschen series n=4 Figure 2.2 Transitions in the hydrogen atom (shown schematically-not to scale)
Transcribed Image Text:Ultraviolet Visible Infrared 5 1 4-1 3 1 2 1 4. 3 and corresponding wavelengths in the The emission spectrum then consists of discrete lines rather than a continuum in which light is emitted at all frequencies. Many such electronic transitions take place with emission of light in the visible region of wavelength 370-700 nm; these transitions can be observed with relatively sp set of "orbits" is not equal). The wavelength of light in the electromagnetic spectrum corr sponding to changes in electronic states in h drogen were described empirically by Rydbe according to the formula: simple equipment and the human eye. It is also possible to examine changes in energy states of 1. R. 1. 1. H. n=5 n=4 Lyman series n=3 6-1 High energy n=2 6 2 5+2 Balmer 4 2 series n=1 H. 3 2 OHayden-McNeil, LLC n-2 6 3 Low energy n=3 Paschen series n=4 Figure 2.2 Transitions in the hydrogen atom (shown schematically-not to scale)
2. Rank the following three transitions in the hydrogen atom in terms of lowest to highest wave- length, energy, and frequency: 6→ 5, 3 → 1, 7 → 3. Note that the energy levels in Figure 2.2 are shown schematically, so you must calculate the energy difference between any two levels in order to answer this question. Show all calculations below or on the following page. Wavelength: Energy: Frequency:
Transcribed Image Text:2. Rank the following three transitions in the hydrogen atom in terms of lowest to highest wave- length, energy, and frequency: 6→ 5, 3 → 1, 7 → 3. Note that the energy levels in Figure 2.2 are shown schematically, so you must calculate the energy difference between any two levels in order to answer this question. Show all calculations below or on the following page. Wavelength: Energy: Frequency:
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