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(B) The electronic configuration of the given elements is:$Ne: [He] 2s^2 2p^6$$He: 1s^2$$Be: 1s^2 2s^2$$N: [He] 2s^2 2p^3$Ionization Potential $(I.P.)

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$He$

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(B) The electronic configuration of the given elements is:$Ne: [He] 2s^2 2p^6$$He: 1s^2$$Be: 1s^2 2s^2$$N: [He] 2s^2 2p^3$Ionization Potential $(I.P.)$ increases across a period and decreases down a group.Among the given elements,$He$ is the smallest atom and its electron is removed from the $1s$ orbital,which is closest to the nucleus.Due to the high effective nuclear charge and the proximity of the $1s$ electrons to the nucleus,$He$ has the highest $I.P.$ value among all elements in the periodic table.

Element having highest $I.P.$ value is

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Triad-$I$ $[N^{3-}, O^{2-}, Na^{+}]$
Triad-$II$ $[N^{+}, C^{+}, O^{+}]$
Choose the species of lowest $IP$ from triad-$I$ and highest $IP$ from triad-$II$ respectively.

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