The difference in the wavelength between the maximum and minimum of Balmer series [Use $R_{H} = 1 \times 10^7 \ m^{-1}$]. (in $Å$)

In the given figure,the energy levels of a hydrogen atom have been shown along with some transitions marked $A, B, C, D$ and $E$. The transitions $A, B$ and $C$ respectively represent:

If $\Delta \lambda_L$ is the difference between the shortest and longest wavelengths of the Lyman series and $\Delta \lambda_B$ is the difference between the shortest and longest wavelengths of the Balmer series,then $\frac{\Delta \lambda_B}{\Delta \lambda_L} = $

When an electron in a hydrogen atom jumps from the fourth Bohr orbit to the second Bohr orbit,we get the:

$A$ hydrogen atom is excited from the ground state to the energy level $n = 3$. According to Bohr's model,the number of spectral lines emitted is:

What is the shortest wavelength present in the Paschen series of spectral lines (in $;nm$)?