The energy required for the ionization of an | vedclass

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(C) The ionization energy $(IE)$ of an atom is the minimum energy required to remove an electron from a given state to infinity $(n = \infty)$.
For a

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$ < 13.6$

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(C) The ionization energy $(IE)$ of an atom is the minimum energy required to remove an electron from a given state to infinity $(n = \infty)$.
For a hydrogen atom,the energy of an electron in the $n^{th}$ orbit is given by $E_n = -\frac{13.6}{n^2} \ eV$.
The ionization energy required from the $n^{th}$ state is $IE_n = E_{\infty} - E_n = 0 - (-\frac{13.6}{n^2}) = \frac{13.6}{n^2} \ eV$.
For the ground state $(n=1)$,$IE_1 = 13.6 \ eV$.
For any excited state $(n > 1)$,the value of $n^2$ is greater than $1$.
Therefore,$IE_n = \frac{13.6}{n^2} < 13.6 \ eV$ for all $n > 1$.

The energy required for the ionization of an excited hydrogen atom would be (in $eV$)-

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