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LNgo 1G
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Postby LNgo 1G » Thu Nov 07, 2019 6:52 pm

When drawing the Lewis structure for a radical molecule, how do you know which atom the single lone electron belongs to?

Posts: 95
Joined: Wed Sep 11, 2019 12:17 am

Re: Radicals

Postby BNgo_2L » Thu Nov 07, 2019 7:02 pm

Typically radicals are formed by breaking bonds, so wherever the bond is broken is where the single lone electron will be. Other than that, I think they're usually placed at the central atom, such as in methyl and hydroxyl.

Ryan Narisma 4G
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Joined: Fri Aug 30, 2019 12:18 am

Re: Radicals

Postby Ryan Narisma 4G » Thu Nov 07, 2019 7:04 pm

Hi LNgo 14A! I think it would make sense if the single electron was on the more electronegative atom. Because it's more electronegative, the atom will want to take as many electrons as possible and this single electron is no exception. I'm not sure, but I hope this helps explain it!

Lauren Sanchez 3D
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Joined: Sat Aug 24, 2019 12:17 am

Re: Radicals

Postby Lauren Sanchez 3D » Thu Nov 07, 2019 10:18 pm

Are there atoms that commonly are radicals? Or can any atom be a radical?

Manav Govil 1B
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Re: Radicals

Postby Manav Govil 1B » Fri Nov 08, 2019 1:32 pm

This is more of an organic chemistry topic when you have to draw resonance structures regarding radical molecules. In orgo, the radical is most commonly found on the C, but in general, any atom can exhibit a radical. Radicals are notable when they appear on structures that should have their octet filled but are just one electron short - hence them being unstable and radical.

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Re: Radicals

Postby Naren_Ramesh_4F » Sun Nov 10, 2019 5:31 pm

How do you know if something is a biradical molecule though? The adding valence electrons to get an odd number doesn't exactly work with biradicals right?

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