The ionization potential or ionization energy of an atom is defined as the energy required to remove an electron from a neutral atom in the gas phase. The first ionization potential is the energy needed to remove the first electron from the atom.

Nitrogen (N) has an electron configuration of $$1s^2 2s^2 2p^3$$, while oxygen (O) has an electron configuration of $$1s^2 2s^2 2p^4$$. Although both elements are in the same period of the periodic table, nitrogen has a half-filled p-orbital, which is a relatively stable configuration compared to the configuration of oxygen. As a result, nitrogen requires more energy to remove one electron compared to oxygen, which would tend to stabilize after losing an electron due to the gain of a half-filled p-orbital configuration.

The first ionization energies for nitrogen and oxygen are indeed different with nitrogen generally having a higher ionization energy. According to experimental data:

• Ionization energy of nitrogen $$N$$ is approximately 14.6 eV.
• Ionization energy of oxygen $$O$$ is approximately 13.6 eV.

Given these values, the correct answer is:
Option A: 14.6, 13.6