Boron Trifluoride class example

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juliefilice 4A
Posts: 31
Joined: Fri Sep 28, 2018 12:27 am

Boron Trifluoride class example

Postby juliefilice 4A » Thu Nov 01, 2018 3:27 pm

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?

505095972
Posts: 69
Joined: Fri Sep 28, 2018 12:17 am

Re: Boron Trifluoride class example

Postby 505095972 » Thu Nov 01, 2018 4:24 pm

Fluorine is really unstable when it has a positive charge, so much so that I don't really think it ever happens. So it is a bad thing because it just isn't realistic or really possible.

Sofia Ban
Posts: 80
Joined: Fri Sep 28, 2018 12:25 am

Re: Boron Trifluoride class example

Postby Sofia Ban » Thu Nov 01, 2018 4:36 pm

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.

Kelly Hollman
Posts: 33
Joined: Fri Sep 28, 2018 12:27 am

Re: Boron Trifluoride class example

Postby Kelly Hollman » Fri Nov 02, 2018 2:41 pm

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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