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When talking about Lewis acids and bases, Lavelle drew the Lewis structure for BF3 with Boron only having 6 electrons. He explained this was because making one of the B-F bonds a double bond would give F a + charge. Why would that be a bad thing?
It wouldn't be correct or rather very unlikely (as said by the comment above) because the boron atoms obey a sextet rule. In this compound, the boron atom only has six valence shell electrons, but the octet rule is satisfied by the fluorine atoms around it.
Fluorine needs on electron to fulfill an octet, so taking an electron away from it would be difficult and unlikely. A double bond between B and F would require that positive charge for Fluorine, so in this case, it won't happen.
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