From the ground state electronic configuratio | vedclass

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(B) The second ionisation energy $(IE_2)$ is the energy required to remove an electron from a unipositive ion.Option $A$ $(1s^2\,2s^2\,2p^6\,3s^2)$ is

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

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(B) The second ionisation energy $(IE_2)$ is the energy required to remove an electron from a unipositive ion.Option $A$ $(1s^2\,2s^2\,2p^6\,3s^2)$ is Magnesium $(Mg)$. Its $IE_2$ involves removing an electron from $Mg^+$,which is relatively easy.Option $B$ $(1s^2\,2s^2\,2p^6\,3s^1)$ is Sodium $(Na)$. After losing one electron,it attains the stable noble gas configuration $(1s^2\,2s^2\,2p^6)$. Removing the second electron requires breaking this stable octet,resulting in a very high $IE_2$.Option $C$ $(1s^2\,2s^2\,2p^6)$ is Neon $(Ne)$,a noble gas with a very high first ionisation energy.Option $D$ $(1s^2\,2s^2\,2p^5)$ is Fluorine $(F)$.Therefore,alkali metals like Sodium exhibit the highest $IE_2$ because the second electron is removed from a stable noble gas core.

From the ground state electronic configuration of the elements given below,pick the one with the highest value of second ionisation energy.

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