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Another example is that nitrogen's electron affinity is lower than carbon's and that Neon's is not only lower than fluorine's, but is actually lower than lithium's.These exceptions are also due to electron configurations!
Another one is in ionization energy! Generally as you move across a period, the ionization energy should increase. However, the exception is that if there are e- in the same orbital, for atoms right next to each other on the periodic table, it would be easier to remove e- in the same orbital because electrons don't like to share orbitals. If in different orbitals it may be more difficult to remove e- even if elements are in the increasing order across the period.
This isn't a trend but I think a good exceptions to remember when doing electron configuration are chromium, copper, molybdenum and silver such that a half or full d orbital is more stable than being partially filled, so an electron from the 4s/5s orbitals rise to a 3d/4d orbital.
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