Chemistry- Atompic Spectroscopy
Category: Science > Chemistry
Asked by: chemstudent3625-ga
List Price: $3.00
13 Sep 2006 21:30 PDT
Expires: 14 Sep 2006 13:30 PDT
Question ID: 765148
What is the electron energy level transition that produces an energy of 4.84 x 10e-19 J? (For hydrogen-like particles, n2 is 2 and n1 can be 3, 4, 5, or 6 for wavelengths in the visible region of the spectrum
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Re: Chemistry- Atompic Spectroscopy
From: fsmth-ga on 14 Sep 2006 05:00 PDT
For Hydrogen ,when n2=1 ,E2=-13.6eV and 4.84 x 10e-19 J=3.025eV ( 1eV=1.6x10e-19J, eV=electron-volt) if n2=2 ,E2=-13.6eV/4=-3.4eV we can got an equation A: 3.025eV= E1-E2=-13.6eV/(n1 x n1) -(-3.4eV) so n1=6 but if the nuclear charge number ?we usually use Z to symbolize it?? 1? the energy of each electron energy level should be multiplied by Z ?so the equation A must be changed? 3.025ev? Z x E1?Z x E2.
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