# Are there any major exceptions when comparing electron affinity?

I was tasked with figuring out whether carbon or nitrogen has a more negative electron affinity value. I initially picked nitrogen, just because nitrogen has a higher $Z_\mathrm{eff}$, creating a larger attraction between electrons and protons, decreasing the radius, causing a higher ionization energy, and therefore decreasing the electron affinity value, but I was actually wrong, and the solutions manual explains it as this:

"As you go from C to N across the Periodic Table you would normally expect N to have the more negative electron affinity. However, N has a half-filled p subshell, which lends it extra stability; therefore, it is harder to add an electron."

Are there any major exceptions to the rules when comparing electron affinity? I'm hesitant to use nitrogen as an exception, because I don't know how far it extends. If nitrogen has a more positive EA than carbon, does that also extend to boron, aluminium, or phosphorus?

I later found that this also applies when comparing silicon and phosphorus. The explanation given was the same.

What exceptions should be noted when comparing electron affinities? Are there any at all? And how far does the exception with atoms with half-filled p subshells extend?

Exceptions abound in electron affinity. Another case is in that of $\ce{F}$ versus that of $\ce{Cl}$. You would think that $\ce{F}$ being far more electronegative, would have the more negative electron affinity, but actually, that is not the case. The small size of $\ce{F}$ makes another electron energetically unfavorable due to electron-electron repulsion. $E\ce{(F)} = -328 kJ/mol$, while $E\ce{(Cl)} = -349 kJ/mol$
In general, exceptions arise when new subshells are being filled/half-filled, or in cases where the atom is too small. In the first case, $\ce{Be}$ and $\ce{Mg}$ are interesting examples: they have a positive electron affinity (just like $\ce{N}$, in fact) because of the energy difference between the s and p subshells. This is no longer the case in $\ce{Ca}$, which as a low-lying 3d orbital; $E\ce{(Ca)}$ is $-2 kJ/mol$.