Chemistry

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?

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  1. 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.)

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  2. 3.03 x 10^-19 J

    Is that right?

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  3. 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.

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