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How do I find the initial energy of an electron given the wavelength and the final energy

An electron jumps to the n = 4 level of a hydrogen atom after absorbing a photon of wavelength 1875 nm. What energy level did the electron move from? I haven't found equations for how to to find the energy absourbtion, just emission. I know that the values are negative when the electron is jumping up to a level, but I don't know how to proceed in terms of what equation to use or how to solve.

chemtopper Tue, 09/26/2017 - 00:12

Energy absorbed and emitted are same if the energy levels are same .Use same equation and only take care of final state and initial sate of energy levels .

Detla E = -RH [1/ n(f)^2  - 1/n(i)^2]

for absortion this value  is positive.

Calculate E using plancks equation