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Hi! I am having a bit of trouble doing 1A.15 in the textbook. I know I need to use -hR/n^2, find the change in E, and that n initial is equal to 2 because the wavelength, 102.6 nm is in the ultraviolet spectrum. I am unsure of how to put it all together. Here is the question: In the ultraviolet spectrum of atomic hydrogen, a line is observed at 102.6 nm. Determine the values of n for the initial and final energy levels of the electron during the emission of energy that leads to this spectral line.
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