I was working on this question:
"An excited hydrogen atom emits light with a frequency of 1/14 x 10^14 Hz to reach the energy level n=4. In what principle quantum level did the electron begin?"
I thought that atoms only emit light when they're moving down quantum levels by emitting a photon, but this is saying that the atom is emitting light but also is "excited" which would indicate that it's moving up energy levels. I feel like this question is contradicting itself, but maybe I'm just confused.
Please let me know what you guys think and if anyone gets an answer please let me know so we can compare!
emitting light and changing energy levels
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Re: emitting light and changing energy levels
Postby Arielle Sass 2A » Wed Dec 09, 2020 10:03 am
Hi,
I think an "excited" electron means one that is already in the "excited" state, as in it is at a higher energy level n than it originally was, before it absorbed any light. So when the excited atom emits light, the electron moves back down to a lower energy level and becomes, at least partially, "un"-excited.
I don't have the answer but when doing the calculations, I would set n=4 as the final energy level and solve for initial.
I think an "excited" electron means one that is already in the "excited" state, as in it is at a higher energy level n than it originally was, before it absorbed any light. So when the excited atom emits light, the electron moves back down to a lower energy level and becomes, at least partially, "un"-excited.
I don't have the answer but when doing the calculations, I would set n=4 as the final energy level and solve for initial.
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