Chemistry - PERIODIC TABLE Question with Solution | TestHub

Solution:

Statement-1: O⁺ ($1s^{2}2s^{2}2p^3$) has a stable half-filled p-orbital, making it harder to remove the second electron than from N⁺ ($1s^{2}2s^{2}2p^2$). Thus, the second ionization enthalpy of Oxygen is greater than Nitrogen. This statement is TRUE.

Statement-2: Na⁺ ($1s^{2}2s^{2}2p^6$) has a stable noble gas configuration, requiring very high energy to remove an electron. Ne ($1s^{2}2s^{2}2p^6$) also has a stable noble gas configuration. The second ionization enthalpy of sodium (removing an electron from Na⁺) is greater than the first ionization enthalpy of Neon (removing an electron from Ne). This statement is TRUE.

Both statements are true.

The final answer is A