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Postby KDang_1D » Mon Nov 04, 2019 3:39 pm

Why can't the molecule be drawn Cl-C-O-Cl rather than centered around C? The formal charges would all be 0 instead of +1/-1.

Brian Tangsombatvisit 1C
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Re: 2B.1b

Postby Brian Tangsombatvisit 1C » Mon Nov 04, 2019 4:44 pm

The structure that you have drawn has formal charges of 0 on the Cl and O, however the C has a formal charge of +2 since it only has 2 bonds. It also shows 26 valence electrons instead of 24.

In order for the formal charges on all the elements to be 0, Carbon must be placed in the middle and have a double bond with oxygen. This would satisfy the HONC 1234 rule where carbon gets 4 bonds and oxygen gets 2.

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Re: 2B.1b

Postby Mashkinadze_1D » Tue Nov 05, 2019 1:19 am

In general dont forget that we draw the structure around the least electronegative element. In this case it is carbon and therefore for this reason it will be the structure we draw around. Generally, carbon likes to form four bonds and the other three elements will allow it to bond this way with a double bond if necessary. The majority of organic compounds will maintain carbon as the central atom.

Minh Ngo 4G
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Re: 2B.1b

Postby Minh Ngo 4G » Tue Nov 05, 2019 1:30 am

Most of the time, C should have 4 bonds around it since it's most stable that way. Also, since C also is your central atom. In addition if you draw C in the middle with one side double bond to O and two sides, each bond with one Cl, everything's formal charge would be 0.

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