What is the ratio of the total energy of an electron in a hydrogen atom in the first excited state to that in the third excited state?

How much energy is needed to release the electron from the second excited state in the hydrogen atom (in $eV$)?

In a hydrogen atom, the energy of an electron in the first and third orbits is $E_1$ and $E_3$ respectively. If $E_3 = x E_1$, then the value of $x$ will be:

An electron in a hydrogen atom first jumps from the third excited state to the second excited state and then from the second excited state to the first excited state. The ratio of the wavelengths $\lambda_1 : \lambda_2$ emitted in the two cases is

Which of the following transitions in a hydrogen atom emits photons of the highest frequency? ($n=$ principal quantum number)

If the binding energy of the electron in a hydrogen atom is $13.6 \ eV$,then the energy required to remove the electron from the first excited state of $Li^{2+}$ is: (in $eV$)