The hydrogen spectrum consists of several spectral lines in Lyman series $\left(\mathrm{L}_1, \mathrm{~L}_2, \mathrm{~L}_3 \ldots ; \mathrm{L}_1\right.$ has lowest energy among Lyman series). Similarly it consists of several spectral lines in Balmer series ( $\mathrm{B}_1, \mathrm{~B}_2, \mathrm{~B}_3 \ldots ; \mathrm{B}_1$ has lowest energy among Balmer lines). The energy of $L_1$ is $x$ times the energy of $B_1$. The value of $x$ is $\_\_\_\_$ $\times 10^{-1}$. (Nearest integer)