The hydrogen spectrum consists of several spectral lines in Lyman series ( $\mathrm{L}_1, \mathrm{~L

Question

The hydrogen spectrum consists of several spectral lines in Lyman series ( $\mathrm{L}_1, \mathrm{~L}_2$, $\mathrm{L}_3 \ldots ; \mathrm{L}_1$ has lowest energy among Lyman series). Similarly it consists of several spectral lines in Balmer series $\left(\mathrm{B}_1, \mathrm{~B}_2, \mathrm{~B}_3 \ldots ; \mathrm{B}_1ight.$ has lowest energy among Balmer lines). The energy of $\mathrm{L}_1$ is $x$ times the energy of $\mathrm{B}_1$. The value of $x$ is $\_\_\_\_$ $	imes 10^{-1}$ . (Nearest integer)

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See detailed solution for explanation.