The binding energy of a hydrogen atom in the ground state is $13.6 \ eV$. The energies required to remove an electron from the first three energy levels of the hydrogen atom are,respectively,(in $eV$):

The ionisation energy of a hydrogen atom is $13.6 \, eV$. Following Bohr's theory,the energy corresponding to a transition between the $3^{rd}$ and the $4^{th}$ orbit is.....$eV$.

The energy required to remove an electron in a hydrogen atom from $n = 10$ state is (in $\text{ eV}$)

The wavelength of the radiation emitted is $\lambda_0$ when an electron jumps from the second excited state to the first excited state of a hydrogen atom. If the electron jumps from the third excited state to the second orbit of the hydrogen atom,the wavelength of the radiation emitted will be $\frac{20}{x} \lambda_0$. The value of $x$ is $........$

The diagram shows the energy levels for an electron in a certain atom. Which transition shown represents the emission of a photon with maximum wavelength?

As the quantum number $n$ increases,the difference in energy between consecutive energy levels