Assertion (A): First ionization energy of O⁺(g) is greater than that of N(g), but the first ionization energy of N⁺(g) is less than N(g). Reason (R): It is easier to remove the fourth 2p electron from

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Assertion (A): First ionization energy of O⁺(g) is greater than that of N(g), but the first ionization energy of N⁺(g) is less than N(g). Reason (R): It is easier to remove the fourth 2p electron from oxygen than it is to remove a 2p electron from nitrogen.

TestHub · Accepted Answer

O⁺ is [He]2s² 2p³, so removing an electron from O⁺ breaks a stable half-filled subshell; therefore, IE(O⁺) is much greater than IE(N). N⁺ is [He]2s² 2p², so IE(N⁺) is lower than IE(N), whose 2p³ subshell is half-filled. Thus, the Assertion is false. The Reason is true because removing the fourth 2p electron from neutral O forms the stable 2p³ configuration, whereas removing one from N breaks it. Answer A.

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