1/wavelength = R(1/2^2 - 1/x^2)
R = 1.09737E7
Solve for X.
(NOTE: It may be easier, math wise, to plug in whole numbers, beginning at 3, and see which whole number(3,4,5,6, etc) ends up giving a wavelength of 656E-9m.)
What is the final energy level of an electron that absorbs energy of 656nm if the electron started at the n=2 level of the hydrogen atom?
3 answers
3.03 x 10^-19 J
Is that right?
Is that right?
I didn't interpret the problem that way. I thought the problem was asking us to determine the orbit to which the electron was promoted. It started at n = 2 and I thought it was asking if it was moved to n = 3, n = 4, n= 5, etc. According to my calculations above it will be moved to n = 3.
3.03E-19 J is the energy of the photon of wavelength 656 nm but that isn't the energy level of the n = 3 orbit.
3.03E-19 J is the energy of the photon of wavelength 656 nm but that isn't the energy level of the n = 3 orbit.
1 answer