Ionization Energy: P vs P

[405513470]

Here are the given facts:
P's first ionization energy:1011, P's second ionization energy:1903
S's first ionization energy:1000, S's second ionization energy:2251
According to the exception rule of ionization energy and group 15, Phosphorus should have a higher ionization energy than Sulfur. Why is phosphorus"s second ionization energy lower than that of sulfur? Does that mean that the exception only apply to the first ionization energy?

[Chem_Mod]

Yes, the exception only applies to the first ionization energy. The exception occurs because in Group 16, one of the electrons is sharing an orbital with the other. The electron repulsions make it easier to remove this first electron. There are no electron repulsion forces to take into account for the second and beyond ionization energies

[905715668]

The exception is because Phosphorus has a 1/2 full p-orbital (3 electrons). Because atoms gravitate toward having 1/2 full or completely full shells, it is hard for Phosphorus to lose its first electron. This does not apply to the second ionization energy because, to personify the example, once phosphorus looses it's 1/2 full shell it doesn't care that much about loosing more electrons on top of that.