4.73

$sp, sp^{2}, sp^{3}, dsp^{3}, d^{2}sp^{3}$

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daisyjimenezt
Posts: 30
Joined: Fri Sep 28, 2018 12:26 am

4.73

The question in the textbook is Identify each as a radical or not: [CH3+; CH4; CH3-; CH2; CH2 2+; CH2 2-]
and the answer was that none of them were radicals but i dont understand why if some of them have lone pairs??

Becky Belisle 1A
Posts: 81
Joined: Fri Sep 28, 2018 12:18 am

Re: 4.73

They have to have unpaired electrons not lone pairs.

Grace Kim 1J
Posts: 60
Joined: Fri Sep 28, 2018 12:18 am
Been upvoted: 1 time

Re: 4.73

After drawing the lewis structures, all of them have paired electrons, meaning they are diamagnetic. Radicals are an atom, molecule, or ion that has an unpaired valence electron. Therefore, none of the structures in the problem are radicals.

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