If the electron in a hydrogen atom moves from the ground state orbit to the $5^{\text{th}}$ orbit,then the potential energy of the electron

The following diagram indicates the energy levels of a certain atom. When the system moves from the $2E$ level to the $E$ level, it emits a photon of wavelength $\lambda$. What is the wavelength of the photon produced during its transition from the $\frac{4E}{3}$ level to the $E$ level?

The energy of an electron in the $n^{th}$ orbit of a hydrogen atom is given by $E_n = - \frac{13.6}{n^2} \ eV$. How much energy in $eV$ is required to move an electron from the first orbit to the third orbit?

The total energy of an electron in an orbit of a hydrogen atom is $E$. The potential energy of the electron in the same orbit is:

$A$ photon is emitted in transition from $n = 4$ to $n = 1$ level in a hydrogen atom. The corresponding wavelength for this transition is $......... \, nm$ (given,$h = 4 \times 10^{-15} \, eV \cdot s$ and $c = 3 \times 10^8 \, m/s$):

The energy levels of an electron in an atom are shown. Which transition of the electron represents the emission of a photon with the highest energy?