Ionization energy is defined as the minimum energy required to remove an electron from the ground state (n0) to infinity (n∞). Determine the wavelength of radiation required to ionize the hydrogen electron from the n = 2 energy level. Calculate the energy (Joules) associated with this photon. (1 cm-1 = 1.986 x 10-23 J)

do I use E = -RH / n^2 ?

I don't know why I'm given the cm to J conversion, or why they ask for the wavelength first.

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  1. I would do it the other way around.
    delta E = 2.180 x 10^-18 J*[(1/n1^2)-(1/n2^2)]. With the Balmer series, n1 is 2 and n2 is infinity.
    Then delta E = hc/wavelength.
    The reason reciprocal cm is given (cm^-1) is because wave number = 1/wavelength and many spectroscopists prefer to use wave number instead of wavelength. Also, if you use the Rydberg constant, then
    1/wavelength = R[(1/N1^2) - (1/N2^2)] and you don't need to convert to wavelength first to get energy in joules.

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  2. ok so 1/lambda = (2.18e-19) (.25 - 0)
    1/lambda = 5.45e-19

    then i set up a proportion to convert it into joules?

    1 cm-1/1.986e-23 joules = 5.45e-19 cm-1/x

    I got x = 1.082e-41 joules and that it so not right..

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  3. thank you i got it now!!

    thanks so much for your help!!

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