Ionization Energy

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Layal Suboh 1I
Posts: 61
Joined: Fri Sep 28, 2018 12:23 am

Ionization Energy

Postby Layal Suboh 1I » Wed Oct 24, 2018 10:35 pm

Why does sulfur have a higher ionization energy than oxygen?

Emmaraf 1K
Posts: 94
Joined: Sat Oct 20, 2018 12:16 am

Re: Ionization Energy

Postby Emmaraf 1K » Wed Oct 24, 2018 11:28 pm

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.

Sabrina Ryu 3L
Posts: 30
Joined: Fri Sep 28, 2018 12:26 am

Re: Ionization Energy

Postby Sabrina Ryu 3L » Thu Oct 25, 2018 1:04 am

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.

Kevin ODonnell 2B
Posts: 62
Joined: Fri Sep 28, 2018 12:24 am

Re: Ionization Energy

Postby Kevin ODonnell 2B » Thu Oct 25, 2018 11:09 am

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:
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Mallory_Podosin_1H
Posts: 31
Joined: Fri Sep 28, 2018 12:15 am

Re: Ionization Energy

Postby Mallory_Podosin_1H » Thu Oct 25, 2018 9:35 pm

I was wondering the same thing... maybe just an exception??

Charles Gu 1D
Posts: 60
Joined: Fri Sep 28, 2018 12:16 am

Re: Ionization Energy

Postby Charles Gu 1D » Fri Oct 26, 2018 11:25 am

Sulfur has less ionization energy than oxygen since its valence electrons are at a higher orbital and since the distance is farther, it would be easier to remove an electron due to shielding.

Rosha Mamita 2H
Posts: 63
Joined: Fri Sep 28, 2018 12:19 am

Re: Ionization Energy

Postby Rosha Mamita 2H » Fri Oct 26, 2018 3:32 pm

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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