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How do you solve this problem: "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". I'm not really sure where to start at, thank you!
I think you would start by using the formula "(hc)/wavelength = change in energy" to find the change in the energy since the wavelength is given to you and h and c are constants. Then you would use Rydberg's formula.
The Rydberg formula is just a simplified version of the formula, ΔE=[(-hR)/(N22)-(-hR)/(N12)]=hν. Cancel out and substitute some terms and you should end up with c/(Rλ)=1/n12-1/n22, and it should be pretty clear what the two values of n are.
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