Question

among the second period elements the actual ionization energies are in the order li<B<Be<C<O<N<F<Ne.

Explain why (ii) O has lower ionization enthalpy than N and F?​

Answer 1

Answer:

cause it needs only 2 electrons for it to complete it's shell

Answer 2

Answer:

Oxygen(8) has a subshell electronic configuration of 1s2 2s2 2p4 while Nitrogen has 1s2 2s2 2p3(7). Nitrogen has more stability than oxygen(due to half filled atomic orbitals). Therefore, high amount of energy is needed to remove an electron in nitrogen than oxygen.

So oxygen has lower ionization than nitrogen.