2.67 part B

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Alex Kashou
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Joined: Fri Sep 29, 2017 7:07 am

2.67 part B

Postby Alex Kashou » Mon Oct 23, 2017 9:35 pm

I understand that electron affinity is the energy released when an electron is added to an atom. I also understand the trend that as you go up and to the right of the periodic table electron affinity increased. Therefore, why does Carbon have a higher electron affinity than nitrogen?

Lena Nguyen 2H
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Re: 2.67 part B

Postby Lena Nguyen 2H » Mon Oct 23, 2017 10:27 pm

For carbon and nitrogen, we would need to consider their electron configurations. Adding an electron to carbon would be adding it to an empty p-orbital, but for nitrogen, adding an electron means adding it to a p-orbital with an electron already inside it. This is more difficult because of electron repulsion since both have negative charges. So nitrogen has a lower electron affinity than carbon.

Example 2.4 explains this as well.

Brigitte Phung 1F
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Re: 2.67 part B

Postby Brigitte Phung 1F » Tue Oct 24, 2017 1:21 pm

In Nitrogen, all three orbitals in the p subshell are half-filled with one electron each which makes it more stable than Carbon, which has two half-filled and one empty p-orbital. Thus, Carbon has a higher electron affinity than Nitrogen. Hope this helps!

Ramya Lakkaraju 1B
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Re: 2.67 part B

Postby Ramya Lakkaraju 1B » Thu Oct 26, 2017 8:12 pm

Generally atoms that have half or full orbitals are the most stable so they will not want to add electrons that easily.

Emily Duggan 1F
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Re: 2.67 part B

Postby Emily Duggan 1F » Fri Oct 27, 2017 2:33 pm

does this rule of half-filled being more stable and therefore lower electron affinities apply to the entirety of Group 15 or just nitrogen?


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