Astronomers have detected hydrogen atoms in interstellar space in the n=732 energy level. Suppose an atom in this excited state emits of a photon and undergoes a transition from n=732 to n=632. How much energy does the atom lose as a result of this transition? what is the frequemcy of this radiation? In which spectral region does this radiation lie?
Chemistry - DrBob222, Thursday, November 29, 2012 at 11:40pm
1/wavelength = R*(1/632^2 - 1/732^2)
R = 1.09737E7
Wavelength is in meters.
c = frequency x wavelength
I don't have a chart showing energy regarding spectral region but you can find one by looking google.