Why do BF3 and NH3 bond together to form BF3NH3 if boron only needs 6 valence electrons? If boron is happy with 6, then why would it create a double covalent bond with nitrogen that has a lone pair of electrons?

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Why do BF3 and NH3 bond together to form BF3NH3 if boron only needs 6 valence electrons? If boron is happy with 6, then why would it create a double covalent bond with nitrogen that has a lone pair of electrons?

Chemistry
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I think Boron is an exception, it has an empty p orbital that can accept electrons.
Boron is also a strong Lewis acid meaning that it can accept a pair of electrons in what's known as a coordinate covalent bond
The bond happens when both the electrons come from the same atom, in this case nitrogen.

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it doesn't create a double bond with nitrogen, it's a single bond. It's all about that empty p orbital though |dw:1435764939354:dw|
Oh so when they bond, nitrogen donates one electron to boron and because now they have opposite charges they are attracted to each other similar to how an ionic bond is formed?
@coltonpalmer an ionic bond is when there's a transfer of electrons, electrostatic attraction; this case is different because it's not an ionic bond but rather a coordinate covalent bond, note "covalent". The issue here is that boron is one of those exceptions, but the best way to think of it is as a Lewis acid; Lewis base pair where the electrons are coming from the nitrogen. Boron is a bit funny because it's one of those exceptions. A Lewis acid by definition is an atom that can accept a pair of electrons.
But I guess you could think of it that way just remember that it's not ionic.
ok thank you :) @Photon336 @aaronq
The charges are formal charges, not ionic.

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