Why is the ionization energy for Neon greater than Fluorine?

Neon had a higher proton charge than Fluorine (first I.E increase)

Neon the same radius, due to the same amount of shells, but it is slightly smaller than fluorine due to a higher number of protons in the nucleus attracting the electrons in the outer shells close (Doesn't really affect first I.E.)

Neon also has the same amount of shielding electrons, due to having the same number of sub-shells, therefore this doesn't really affect I.E. either

However the largest factor is that the 2p sub shell in neon is full, whereas in fluorine it is not, a full sub shell means that the atom is more stable therefore ionization energy significantly rises.

Therefore Neon, overall has a larger first ionization energy.

Neon- First I.E.=2080.7

Fluorine-First I.E. =1681.0