Chemistry - Are there any major exceptions when comparing electron affinity?

This exception rule is actually orbital filling rule. For two electrons to be in same orbital they need to have different spins (Pauli exclusion principal). This electron pairing requires additional energy and thus it is easier to add electrons if there are free orbitals. When element has a half-filled p sublevel all 3 orbitals have one electron and pairing takes place (difference between energy levels of 2p and 3s is greater than electron pairing energy).

Electron pairing effects have significant impact to physical properties of coordination complexes (like color and magnetic properties).