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Rachel Lu_dis1H
Posts: 66
Joined: Fri Sep 29, 2017 7:06 am
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Postby Rachel Lu_dis1H » Sun Oct 29, 2017 1:53 pm

Can someone explain why the ionization energy for oxygen would be lower than that of nitrogen or fluorine?

Danah Albaaj 1I
Posts: 50
Joined: Fri Sep 29, 2017 7:07 am

Re: 2.81

Postby Danah Albaaj 1I » Sun Oct 29, 2017 2:48 pm

Oxygen has a lower ionization energy than nitrogen and fluorine because of the repulsion between its electrons. Nitrogen only has 3 electrons in the 2p-orbital which means each electron is unpaired. Fluorine has 5 electrons in the 2p-orbital meaning only one electron is unpaired, which makes it more difficult to remove an electron. However, oxygen has 4 electrons in the 2p-orbital, meaning that there is one set of paired electrons. The repulsion between the two electrons in the pair makes it much easier to remove an electron from oxygen than nitrogen or fluorine.

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