Does anybody know how to calculate the wavelength and energy of the photon that gives rise to the third line in the Lyman series in the emission spectrum of hydrogen?
Stacey Warren - Expert brainly.com
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you would have to calculate the energy of the proton at ground level and at the 3rd energey level and take the difference.
What grade level of chem is this for? If I'm going to have to do this this year... Wow...
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So , you are saying that first I have to calculate the ground level which is n=1 and then n=3, after that subtract the difference from n=1 with n=3?
I am not sure what grade level is this for, but I have to take 221, 222 and 223 for computer science major.
yes nelly thats how i always do it. then you should be able to calculate wave length from that number.
What confuses me is the numbers on the right where it says -1312kJ, and on n=3 level to the right -146kJ. Do I have to use this numbers?
Thats the part that was confusing me normally the energy of a proton is a very very small number. This may be a case where you are using a different way than I would go about figuring this out. or you are just learning a different methode. I can't read whatever language it's in so your link isn't very helpful for me. I have tried to school myself up on it a little bit and this is the site i was using. http://en.wikipedia.org/wiki/Hydrogen_spectral_series . The strange thing is the page you were looking at has it in KJ and the one i have is in nm. So i'm not really sure whats going on.
hm yes, it is confusing. Thanks anyways for trying.
zbay, does the wavelength occur in region between n=1 and n=3?