## Going from Spectroscopic line to Energy levels

H-Atom ($E_{n}=-\frac{hR}{n^{2}}$)

monikac4k
Posts: 56
Joined: Fri Sep 28, 2018 12:25 am

### Going from Spectroscopic line to Energy levels

Hi, I am a bit confused with the idea of taking the length of the spectroscopic line and working backwards to find the beginning and ending energy levels of the electron. This confusion comes from problem 15 in chapter 1 of the 6th edition textbook. However, I want to understand this type of problem conceptually instead of understanding how to work through this exact problem. Thanks for the help!

Yousif Jafar 1G
Posts: 59
Joined: Thu May 10, 2018 3:00 am

### Re: Going from Spectroscopic line to Energy levels

So conceptually, this problem is similar to the graphs that Dr. Lavelle showed us in class. When the wavelength is shorter, so UV waves, the electron is falling from an elevated state to n=1. However when you go to a larger wavelength, visible light (400nm-700nm), the electron is falling from an elevated state to n=2. Because the problem gives you wavelength is 102.6 nm, you know that it is in the UV spectra (Lyman series) so therefore n=1 and then you do the conversions using the equations given to us E= hv and c= lambda v.

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