The ratio of energies of photons produced due to the transition of an electron of a hydrogen atom from its $(i)$ second to first energy level and $(ii)$ highest energy level to $2^{nd}$ level is respectively: (in $: 1$)

The total energy of an electron in an atom in an orbit is $-3.4 \; eV$. Its kinetic and potential energies are,respectively:

$A$ sample of hydrogen atoms is in an excited state (all the atoms). The photons emitted from this sample are made to pass through a filter through which light having a wavelength greater than $800 \ nm$ can only pass. Only one type of photon is found to pass through the filter. The sample's initial excited state is: [Take $hc = 1240 \ eV \cdot nm$,ground state energy of hydrogen atom = $-13.6 \ eV$.]

The four lowest energy levels of an $H$-atom are shown in the figure. The number of possible emission lines would be

In Bohr's atomic model of hydrogen,let $K$,$P$ and $E$ be the kinetic energy,potential energy and total energy of the electron,respectively. Choose the correct option when the electron undergoes transitions to a higher level.

In a hydrogen atom,the electron is in the $n^{th}$ excited state. It may come down to the second excited state by emitting ten different wavelengths. What is the value of $n$?