The figure shows an energy level diagram for the hydrogen atom. Several transitions are marked as I, II, III, …….  . The diagram is only indicative and not to scale. Which of the following statements are correct ?

The jump of electron from n=2 to any higher orbit happens due to absorption of Balmer series photon.

$\frac{hc}{\lambda }=13.6\left(\frac{1}{n_1^2}-\frac{1}{n_2^2}\right)$

Put ${\mathrm{n}}_1=2 \mathrm{and} {\mathrm{n}}_2=4$, we get $\mathrm{\lambda }=486\mathrm{nm}$

Transition IV will occur when a hydrogen atom is irradiated with radiation of  wavelength 656 nm.

$\frac{hc}{\lambda }=13.6\left(\frac{1}{n_1^2}-\frac{1}{n_2^2}\right)$

Put ${\mathrm{n}}_1=2 \mathrm{and} {\mathrm{n}}_2=3$, we get $\mathrm{\lambda }=656\mathrm{nm}$

Transition IV will emit the longest wavelength line in the visible portion of the  hydrogen spectrum.