Which one of the following has the lowest ion | vedclass

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(B) The ionization energy is the energy required to remove the most loosely bound electron from an isolated gaseous atom.Among the given electronic co

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$1s^2 2s^2 2p^6 3s^1$

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(B) The ionization energy is the energy required to remove the most loosely bound electron from an isolated gaseous atom.Among the given electronic configurations, $1s^2 2s^2 2p^6 3s^1$ represents an alkali metal (Sodium, $Na$).Alkali metals have the largest atomic size in their respective periods and a single electron in their outermost $s$-orbital, making it easiest to remove that electron.Therefore, the configuration $1s^2 2s^2 2p^6 3s^1$ has the lowest ionization energy.

Which one of the following has the lowest ionization energy?

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