Practice midterm 6d

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Fiona Grant 1I
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Joined: Fri Apr 06, 2018 11:03 am

Practice midterm 6d

Postby Fiona Grant 1I » Sat May 05, 2018 3:06 pm

The question asks us to rank C,N,O, and F in order of increasing ionization energies. I know that the solution is C < O < N < F, however I expected the answer to be C < N < O < F because the ionization energy increases across a period. We talked about how this is an exception during the review session, but I am still confused about the reason why O and N are flipped.

Natalie Noble 1G
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Re: Practice midterm 6d

Postby Natalie Noble 1G » Sat May 05, 2018 3:07 pm

C < O < N < F

The reason the N and O breaks the ionization trend is because N is more stable dues to half shell stability. N has one electron in all three orbitals, which gives it slightly more stability making the ionization energy higher as it is more difficult to remove an electron. (while O has 4 electrons and does not have the same stability granted by a half shell)

Bianca Nguyen 1B
Posts: 36
Joined: Fri Apr 06, 2018 11:04 am

Re: Practice midterm 6d

Postby Bianca Nguyen 1B » Sat May 05, 2018 3:12 pm

O and N are flipped because of half-shell stability. N does not want to lose an electron because all of its p orbitals are filled with an electron and they are parallel to each other. It is easier to remove an electron from O because it will have half-shell stability when you remove an electron. I’m not great at explaining this, but hopefully it makes sense


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