Asked by Giznelbell
Calculate the wavelength of light emitted when each of the following transitions occur in the hydrogen atom.
(a) n = 5 n = 4
_________nm
(b) n = 5 n = 3
_____________ nm
(c) n = 5 n = 2
__________ nm
Calculate the maximum wavelength of light capable of removing an electron for a hydrogen atom from the energy state characterized by the following.
n = 2
_________nm
n = 4
_______ nm
how do u do this?
(a) n = 5 n = 4
_________nm
(b) n = 5 n = 3
_____________ nm
(c) n = 5 n = 2
__________ nm
Calculate the maximum wavelength of light capable of removing an electron for a hydrogen atom from the energy state characterized by the following.
n = 2
_________nm
n = 4
_______ nm
how do u do this?
Answers
Answered by
bobpursley
http://en.wikipedia.org/wiki/Rydberg_formula
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.