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(C) The energy of an electron in the $n$-th orbit of a hydrogen atom is given by $E_n = -13.6/n^2 \ eV$.For the transition from the second orbit $(n_2

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Ultraviolet

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(C) The energy of an electron in the $n$-th orbit of a hydrogen atom is given by $E_n = -13.6/n^2 \ eV$.For the transition from the second orbit $(n_2 = 2)$ to the first orbit $(n_1 = 1)$,the energy of the emitted photon is $\Delta E = E_2 - E_1 = -13.6(1/2^2 - 1/1^2) = -13.6(1/4 - 1) = -13.6(-3/4) = 10.2 \ eV$.This transition corresponds to the first line of the Lyman series.The Lyman series of the hydrogen spectrum lies in the ultraviolet region of the electromagnetic spectrum.

If the electron in a hydrogen atom transits from the second orbit to the first orbit,in what region would the emitted radiation be?

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