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I understand why oxygen is the exception to the trend of ionization energy and why it's lower. However, I want to clarify why other Group 16 elements (Sulfur, Selenium, etc.) don't have a lower ionization energy like oxygen? Or hold on, do they?
Yes, I think the other Group 16 elements are also exceptions to the trend and have lower ionization energies, since they all have 4 electrons in their outermost p orbitals. This makes them have more repulsive interactions, so it takes less energy to remove an electron.
The other group 16 elements that follow this trend include O, S, and Se. The other group 16 elements get too large for the ionization energy to reflect this change going down. This photo shows the energies of the first ionization energy.
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