Question

Why are these 2 statements false? Could anyone explain it?

I.	It takes less energy to add an electron to nitrogen than to carbon because nitrogen will be closer to achieving a noble gas configuration.
II.	It takes more energy to add an electron to fluorine than to oxygen because the radius of fluorine is smaller and more repulsion would occur in the p-orbitals.

Answer 1

I) Since N has half-filled p-sub shell, it is more stable.

   So it is harder to add extra electron to N.

Hence, It takes more energy to add an electron to nitrogen.

If we add an electron to Carbon, it will give half-filled p-subshell which is more stable.

Hence, It takes less energy to add an electron to carbon than to nitrogen.

II)   Electron affinity of oxygen = - 142 kJ/mol

     Electron affinity of fluorine = - 328 kJ/mol

      Due to more electronegativity of Fluorine, more repulsion would occur in the p-orbitals