The ratio of the wavelengths of radiation emitted when an electron in the hydrogen atom jumps from the $4^{th}$ orbit to the $2^{nd}$ orbit and from the $3^{rd}$ orbit to the $2^{nd}$ orbit is:

The frequencies for the series limit of the Balmer and Paschen series are $v_1$ and $v_3$ respectively. If the frequency of the first line of the Balmer series is $v_2$,then the relation between $v_1, v_2,$ and $v_3$ is:

If an electron in a hydrogen atom jumps from the $3^{rd}$ orbit to the $2^{nd}$ orbit,it emits a photon of wavelength $\lambda$. When it jumps from the $4^{th}$ orbit to the $3^{rd}$ orbit,the corresponding wavelength of the photon will be

Every series of the hydrogen spectrum has an upper and lower limit in wavelength. The spectral series which has an upper limit of wavelength equal to $18752 \mathring{A}$ is:
(Rydberg constant $R = 1.097 \times 10^7 \ m^{-1}$)

In the spectrum of the hydrogen atom,the ratio of the longest wavelength in the Lyman series to the longest wavelength in the Balmer series is

Ratio of the wavelengths of the first line of the Lyman series and the first line of the Balmer series is