With which of the following electronic config | vedclass

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(B) Ionisation enthalpy is the energy required to remove the most loosely bound electron from an isolated gaseous atom.As the principal quantum number

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$1s^2 \ 2s^2 \ 2p^5 \ 3s^1$

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(B) Ionisation enthalpy is the energy required to remove the most loosely bound electron from an isolated gaseous atom.As the principal quantum number $(n)$ increases,the distance of the valence electron from the nucleus increases,leading to a decrease in the effective nuclear charge experienced by the electron.Option $B$ $(1s^2 \ 2s^2 \ 2p^5 \ 3s^1)$ represents an atom with its valence electron in the $n=3$ shell,which is further from the nucleus compared to the electrons in the $n=2$ shell in the other options.Therefore,the electron in the $3s$ orbital is held least tightly,resulting in the lowest ionisation enthalpy.

With which of the following electronic configurations does an atom have the lowest ionisation enthalpy?

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