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In my discussion, we saw how Be has a larger ionization energy than B even though B is farther to the right than Be because B has 1 electron in the 2p-orbital while Be has a full 2s-orbital. The same was true for N having a larger ionization energy than O because of its half full 2p-orbital. How do these exceptions in trends relate to electronegativity and electron affinity? are there any other exceptions to trends in electronegativity or electron affinity?
Expanding off of the previous answer, an exception for electron affinity is that the electron affinity of carbon is higher than that of nitrogen. This is because the addition of an electron to carbon makes the shell half-filled, which is much more favorable compared to nitrogen having an electron added to its half-filled shell. This exception follows the same logic as the ionization energy one.
When the element has full orbital or half full orbital structure, their structure is so stable that it is difficult for them to lose electrons, which means that it would require more energy to move one electron away from them, thus making their ionization energy higher.
I believe for atomic radius, the element going up and down matters more because when you go down a group, there are additional shells added. For ionization energy and electron affinity, there are less obvious trends.
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