Electron affinity increases in the periods across the p block. An exception to this trend occurs between groups 14 and 15.
Ex: compare the the EA's of C ([He]2s2 2p2) and N ([He]2s2 2p3). Adding an electron to a C atom gives a half-filled p sublevel. This occurs much more easily than forcing an electron to pair with another electron in an orbital of the already half filled p sub level of a N atom.
Could someone please explain this? What's so important about the half filled p sublevel and wouldnt forcing an electron to pair with another electron in an orbital of the already half filled p sub level of a N atom make the atom gain an electron?
Ex: compare the the EA's of C ([He]2s2 2p2) and N ([He]2s2 2p3). Adding an electron to a C atom gives a half-filled p sublevel. This occurs much more easily than forcing an electron to pair with another electron in an orbital of the already half filled p sub level of a N atom.
Could someone please explain this? What's so important about the half filled p sublevel and wouldnt forcing an electron to pair with another electron in an orbital of the already half filled p sub level of a N atom make the atom gain an electron?