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I am confused, how can hydrogen produce emission lines in the visible light region? the only excitation that can happen to hydrogen is from energy level 1 to any other energy level, all of that correspond to ultraviolet range.

This can happen if the electron of the hydrogen atom can be excited from energy level 1 to 2 then instantly from 2 to any other level. But, I read before that the electron can't have double excitation.

Also, this can happen if the hydrogen is ionised, then the free electron is the one which produced the visible light spectrum.

What is right?

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    $\begingroup$ The "production" of light happens when an electron de-excites. It emits a photon. Upon excitation, it absorbs a photon. $\endgroup$
    – Peeyush Kushwaha
    Commented Mar 21, 2016 at 20:51
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    $\begingroup$ So visible light is produced when electrons come from a higher level of excitation down to level 2. See Balmer Series on wikipedia $\endgroup$
    – Peeyush Kushwaha
    Commented Mar 21, 2016 at 20:57
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    $\begingroup$ Your assertion that "the energy of the emitted photon is the same as the absorbed one" is misleading. The electron may be excited from 1 to 3, then de-excited from 3 to 2 (giving off red) and then from 2 to 1. $\endgroup$
    – Peeyush Kushwaha
    Commented Mar 21, 2016 at 21:04
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    $\begingroup$ hyperphysics.phy-astr.gsu.edu/hbase/hyde.html#c4 $\endgroup$
    – Gert
    Commented Mar 21, 2016 at 22:01
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    $\begingroup$ Only the excitations of ground state hydrogen are restricted to the ultraviolet. Likewise de-excitation ending in the ground state *are in the ultraviolet. $\endgroup$
    – dmckee --- ex-moderator kitten
    Commented Mar 21, 2016 at 22:21

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