## Midterm Review Problem 10 d

Kallista McCarty 1C
Posts: 212
Joined: Wed Sep 18, 2019 12:18 am

### Midterm Review Problem 10 d

Rank the following in order of increasing ionization energies: C N O F

I thought the answer would be C<N<O<F, but the key said C<O<N<F can someone please explain this?

AlyshaP_2B
Posts: 112
Joined: Wed Sep 18, 2019 12:19 am

### Re: Midterm Review Problem 10 d

Oxygen has a lower ionization energy than Nitrogen because of the 4th electron joining. Having 2 electrons in the same orbital increases the electron repulsion, making Oxygen more likely to want to give up an electron.

Michelle N - 2C
Posts: 117
Joined: Wed Sep 18, 2019 12:19 am

### Re: Midterm Review Problem 10 d

Oh.. yep. Definitely wrote something completely different.

Is oxygen the only exception from this trend then? Asking for future reference and learning.

Michelle Chan 1J
Posts: 50
Joined: Thu Jul 25, 2019 12:16 am

### Re: Midterm Review Problem 10 d

If you draw out the three orbitals, N is more stable because they are each filled with one e-, thus O would want to lose one to become more stable.

MTanikella_1K
Posts: 110
Joined: Sat Jul 20, 2019 12:16 am

### Re: Midterm Review Problem 10 d

Oxygen is an exception to the trend because it is easier for oxygen to give up an electron to have a more stable configuration than it is for nitrogen to give up an electron. This is because nitrogen has three electrons in the p orbital, which is relatively more stable than the four electrons oxygen has in the p orbital.

RichBollini4G
Posts: 100
Joined: Wed Sep 18, 2019 12:18 am

### Re: Midterm Review Problem 10 d

MTanikella_1C wrote:Oxygen is an exception to the trend because it is easier for oxygen to give up an electron to have a more stable configuration than it is for nitrogen to give up an electron. This is because nitrogen has three electrons in the p orbital, which is relatively more stable than the four electrons oxygen has in the p orbital.