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Posted by on Thursday, November 29, 2012 at 11:11pm.

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 - , 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.

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