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Postby ChristianM3F » Thu Dec 05, 2019 3:58 pm

Wait, so could someone please explain to me how BF3 would be a Lewis acid? Would the boron take in the electron pair, even though it'd take on a negative charge..?

Indy Bui 1l
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Re: 6A13b

Postby Indy Bui 1l » Thu Dec 05, 2019 4:01 pm

Boron is relatively electropositive and especially when it is bounded to fluorine, the negative charge is further distributed away from Boron. This allows it to want to accept an electron pair, making it a Lewis acid.

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Re: 6A13b

Postby McKenna_4A » Thu Dec 05, 2019 4:03 pm

Yes. Boron often draws an electron pair when it already has 3 bonds. Also, the 3 Fs are very electronegative and will delocalize this negative charge. Because it's accepting a lone pair, it's a Lewis Acid.

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