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I think you mean nitrogen and oxygen? That is one of the exceptions to the ionization energies increasing from left to right, because oxygen is in group 16 and nitrogen is in group 15. This is because the electron configuration of nitrogen is more stable, because all of the p orbitals only have one electron in each subshell while oxygen has paired electrons in one of the p orbitals. This makes oxygen more willing to give up an electron than nitrogen.
Emmaraf 3K wrote:Are you referring to a specific question? Looking at a chart online for ionization energies, it says the ionization energy for sulfur is less than oxygen.
Here is the chart they were referring to. It may help to have a visual to better understand the concept:
Down a group there is a greater distance between the nucleus and electrons of an atom because of added energy shells, so because sulphur's electrons are further away from its nucleus than oxygen, it will take less energy to remove an electron from sulphur. The farther an electron is from its nucleus, the easier it is to remove the electron.
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