Line spectra are due to

The energy of an electron in the $n^{th}$ orbit of a hydrogen atom is expressed as $E_n = \frac{-13.6}{n^2} \, eV$. The shortest and longest wavelengths of the Lyman series will be:

Match List $I$ with List $II$.

List $I$ (Spectral Lines of Hydrogen for transitions from)	List $II$ (Wavelengths $(nm)$)
$A$. $n_2=3$ to $n_1=2$	$I$. $410.2$
$B$. $n_2=4$ to $n_1=2$	$II$. $434.1$
$C$. $n_2=5$ to $n_1=2$	$III$. $656.3$
$D$. $n_2=6$ to $n_1=2$	$IV$. $486.1$

Choose the correct answer from the options given below:

The wavelength of light for the least energetic photons emitted in the Lyman series of the hydrogen spectrum is nearly. [Take $hc = 1240 \text{ eV-nm}$, change in energy of the levels $= 10.2 \text{ eV}$] (in $\text{ nm}$)

In hydrogen spectrum,which of the following spectral series lies in the ultraviolet region?

If the longest wavelength in the ultraviolet region of the hydrogen spectrum is $\lambda_{0}$,then the shortest wavelength in its infrared region is: