Neon- electron configuration

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Neon- electron configuration

Postby CNourian2H » Sun Oct 20, 2019 9:06 pm

In class, Dr. Lavelle said that elements like Neon are not good at building bonds. Why is this so?

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Re: Neon- electron configuration

Postby charleejohnson1L » Sun Oct 20, 2019 9:07 pm

Elements like neon have a full valence shell and meet the octet rule! They don't really have a need for more electrons, so they're less likely to form bonds. :) I hope this helps!

Harry Zhang 1B
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Re: Neon- electron configuration

Postby Harry Zhang 1B » Sun Oct 20, 2019 9:11 pm

This is so because Neon belongs to what we call the noble gas family in the periodic table(last column) and all the atoms in this family has the same electron configuration in which there is no unpaired electron and a full s and p orbital, which makes them extremely unstable and therefore unreactive.

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Re: Neon- electron configuration

Postby jvera4b » Sun Oct 20, 2019 9:14 pm

Elements like neon meet the octet rule meaning they have eight electron in its valence shell. The octet rule states that all elements want to have eight electrons in their valence shell, so neon and other elements like it aren't as likely to bond with other elements.

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