Ionization energy

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LeAirraBullingor2k
Posts: 77
Joined: Wed Mar 13, 2019 12:15 am

Ionization energy

Postby LeAirraBullingor2k » Mon Nov 11, 2019 4:05 pm

Why does Oxygen have a lower ionization energy than Nitrogen?

Nicholas Chin 1G
Posts: 100
Joined: Thu Jul 11, 2019 12:17 am

Re: Ionization energy

Postby Nicholas Chin 1G » Mon Nov 11, 2019 4:08 pm

Because nitrogen has 3 parallel spin electrons in separate orbitals in the 2p subshell, while Oxygen has 3 parallel spin electrons and one antiparallel electron in the same orbital. Because of electron-electron repulsion and the fact that having a half-full 2p subshell is more stable, it is easier (requires less energy) to remove the electron in oxygen than in nitrogen.

WUng_1D
Posts: 50
Joined: Sat Aug 24, 2019 12:16 am

Re: Ionization energy

Postby WUng_1D » Mon Nov 11, 2019 4:48 pm

I like to think of it as oxygen is more willing to give up its electrons in order to attain a half full shell of electrons which is why it will require less energy to remove the electron.

PriscillaLi_3G
Posts: 63
Joined: Fri Sep 27, 2019 12:30 am

Re: Ionization energy

Postby PriscillaLi_3G » Mon Nov 11, 2019 5:27 pm

Nitrogen has a half-full shell, which is more stable, so it would be harder to remove an electron, thus increasing the ionization energy. In addition, the 4th electron in the oxygen atom has an electron-electron repulsion with the other electron in the orbital, thus making it easier to remove the electron, which lowers the ionization energy.

005162902
Posts: 102
Joined: Wed Sep 18, 2019 12:15 am

Re: Ionization energy

Postby 005162902 » Mon Nov 11, 2019 7:15 pm

oxygen is more likely to lose one electron to get a half-full shell, which is more stable than having 6 valence. Nitrogen is already half full so will likely keep its electrons. This gives O a lower Ionization energy

Sofia Q
Posts: 49
Joined: Sat Aug 17, 2019 12:15 am

Re: Ionization energy

Postby Sofia Q » Mon Nov 11, 2019 7:21 pm

by looking at the periodic table one would assume nitrogen to be less electronegative than oxygen following the trend on the periodic table, but that in fact due to the symmetry that the nitrogen atom has in the 2p subshell(compared to that of oxygen), more clearly seen in a arrow diagram, gives it a higher electronegativity than oxygen despite having one more electron!

ramiro_romero
Posts: 90
Joined: Sat Sep 07, 2019 12:16 am

Re: Ionization energy

Postby ramiro_romero » Tue Nov 12, 2019 9:03 pm

From periodic trends, it can be incorrectly assumed that Oxygen has a higher ionization energy than Nitrogen. However, Oxygen wants a full shell so is more willing to give up its electrons (requiring less energy to its electrons and therefore giving Oxygen a lower ionization energy than Nitrogen).


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