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why does boron triflouride behave as a Lewis acid?

why does boron triflouride behave as a Lewis acid?

Grade:Upto college level

2 Answers

Suraj Prasad IIT Patna
askIITians Faculty 286 Points
6 years ago
because Boron here can accept electrons in vacant p- orbitals....
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Raheema Javed
156 Points
6 years ago
Boron only has 3 valence electrons (ns2 np1). So, with three flourine's attached, you'll form a covalent compound by sharing electrons. The compound now has 6 electrons, and it needs to have 8 (octet rule, though there are exceptions for some atoms). Anyhow, it can accept two more electrons to fill its octet.

Lewis Acid = Donate H, Accept e-

Lewis Base = Accept H, Donate e-

So, BF3 is a Lewis Acid. I think when a Lewis Base donates two electrons to the compound, it is called a "coordinate covalent bond." If the base is removed from the acid, it will take its two electrons with it.

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