The problem is the following: The energy of the electron in the lowest level of

Question

The problem is the following:

The energy of the electron in the lowest level of the hydrogen atom (n=l) is -2.179x10 -18J. What is the energy of the electron in level n=5? Tries 0/99 The electron in a hydrogen atom moves from level n=4 to level n=5. Is a photon emitted or absorbed? What is the wavelength of the photon? Tries 0/99 An excited hydrogen atom emits a photon with a wavelength of 1094.0 nm. In what region of the spectrum is this photon? What is the frequency of this photon? Tries 0/99 A hydrogen atom in the ground state absorbs a photon of wavelength 93.8 nm. What energy level does the electron reach? This excited atom then emits a photon of wavelength 7458.9 nm. What energy level does the electron fall to? Tries 0/9

Explanation / Answer

1. energy = n^-2 Eo ...where Eo is give. ...so answer -8.7*10^-20 J

2. photon must be absorbed...as e- goes to higher energy orbit..

wavelength = 12400/.306 = 4.05*10^-6 m

3. infrared....c=f w ..so f = 2.74*10^14 sec-

4. delta E = 12400/938 ev = 13.2 ev .... so it goes frm 1 to 6 ....

5. delta E = 12400/74589 = .166 ev ... so it goes frm 6 to 5 ....

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