why does boron triflouride behave as a Lewis acid?

Question

Suraj Prasad · Answer

because Boron here can accept electrons in vacant p- orbitals.... &hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;. &hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;. &hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;. &hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;.&hellip;.

Raheema Javed · Answer

Boron only has 3 valence electrons (ns 2 np 1 ). 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, BF 3 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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why does boron triflouride behave as a Lewis acid?

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why does boron triflouride behave as a Lewis acid?

why does boron triflouride behave as a Lewis acid?

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