Which of the following statements correctly compares the first ( _i H₁ ) and second ( _i H₂ ) ionization enthalpies of Nitrogen ( N ) and Oxygen ( O )?

Step-by-step solution

For the first ionization enthalpy ( _i H₁ ), we consider the neutral atoms: N : 1s^2 2s^2 2p^3 O : 1s^2 2s^2 2p^4 Nitrogen has a stable half-filled 2p subshell, making it harder to remove an electron compared to Oxygen. Thus, _i H₁( N ) > _i H₁( O ) . For the second ionization enthalpy ( _i H₂ ), we consider the monocations: N ^+: 1s^2 2s^2 2p^2 O ^+: 1s^2 2s^2 2p^3 Now, the O ^+ ion has the stable half-filled 2p subshell. Removing a second electron from Oxygen requires breaking this stable configuration, which req