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Postby Shanzey » Sun Nov 03, 2019 1:25 pm

When drawing a radical, do we put the radical on the atom that is less electronegative, since it does not pull electrons towards it as strongly?

Kate Osborne 1H
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Re: Radicals

Postby Kate Osborne 1H » Sun Nov 03, 2019 2:51 pm

In the example Dr. Lavelle gave in class, the carbon held the unpaired electron rather than the hydrogen because carbon only contributed to three bons and as such it has one electron left.

Natalie Wang 1B
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Re: Radicals

Postby Natalie Wang 1B » Sun Nov 03, 2019 6:51 pm

For most molecules, the atom that gets the extra electron is the one that that already has other lone pairs. Of course, for problem 5a from Focus 2C, there is a molecule that is ClO. The extra electron is put onto Cl. I think it is likely because Cl is more electronegative. But also, it makes Cl's formal charge 0.

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Re: Radicals

Postby AryaG_4C » Sun Nov 03, 2019 7:08 pm

Usually it is put on the element thats more electronegative.

Kavee Dodampahala 4E
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Re: Radicals

Postby Kavee Dodampahala 4E » Sun Nov 03, 2019 8:54 pm

Can someone explain why the more electronegative element gets the radical? In my mind, it would make more sense for the less electronegative one to have it.

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Re: Radicals

Postby ATingin_3I » Sun Nov 03, 2019 11:23 pm

What purpose does the radical serve? And how do we know when there is a radical present?

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