Oxygen

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605379296
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Joined: Sat Aug 17, 2019 12:16 am

Oxygen

Postby 605379296 » Thu Nov 07, 2019 7:53 pm

Why does Oxygen have a low first ionization energy?

Sukanya Mohapatra 2G
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Re: Oxygen

Postby Sukanya Mohapatra 2G » Thu Nov 07, 2019 7:55 pm

This is because of an electron being added to an already half full orbital in oxygen, which results in electron-electron repulsion,lowering the ionization energy.

Haley Chun 4H
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Joined: Sat Aug 17, 2019 12:18 am

Re: Oxygen

Postby Haley Chun 4H » Thu Nov 07, 2019 8:30 pm

Oxygen also has 4 electrons in the 2p orbital, yet it would rather have a half-full shell. Thus, it would be easier to remove the 4th electron.

Victoria Otuya 4F
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Re: Oxygen

Postby Victoria Otuya 4F » Thu Nov 07, 2019 9:10 pm

what about the ionization energy of nitrogen? Is It greater than oxygen?

Amanda Ung 4D
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Re: Oxygen

Postby Amanda Ung 4D » Sun Nov 10, 2019 4:40 pm

Victoria Otuya 4F wrote:what about the ionization energy of nitrogen? Is It greater than oxygen?

Yes because nitrogens subshells are completely half filled which is more stable than oxygen which has 1 pair and 2 lone electrons. The electron electron repulsion of oxygen’s orbital causes it to have a lower ionization energy than nitrogen

pmokh14B
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Re: Oxygen

Postby pmokh14B » Sun Nov 10, 2019 4:48 pm

The first electron being removed from oxygen comes out of a full orbital. The electron-electron repulsion of the two e- decreases the magnitude of the force of the nucleus these electrons experience, decreasing the energy necessary to remove them from the atom.

Dan M -3E
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Re: Oxygen

Postby Dan M -3E » Sun Nov 10, 2019 4:54 pm

Yeah this was a tricky question on the midterm but because of the extra (4th) electron in the 2p subshell, oxygen has a slightly lower IE than nitrogen.

William Francis 2E
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Re: Oxygen

Postby William Francis 2E » Sun Nov 10, 2019 5:02 pm

Oxygen's electron configuration is 1s2 2s2 2p4. Since a p subshell houses three orbitals that can contain up to 6 electrons, a p subshell containing 3 electrons is considered half full with one electron in each orbital (as per Hund's Rule). Half full subshells can be somewhat desirable for atoms (although having full shells is preferable of course).

Oduwole 1E
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Re: Oxygen

Postby Oduwole 1E » Sun Nov 10, 2019 6:08 pm

Victoria Otuya 4F wrote:what about the ionization energy of nitrogen? Is It greater than oxygen?


Nitrogen has a higher ionization energy, because it will take more energy to remove one electron from nitrogen than from oxygen. This is because nitrogen's 2p orbital is half filled, while oxygen's is partially (4/6) filled. Half-filled is more stable than partially filled, so it is easier to remove an electron from oxygen.


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