Question

why does BF3 behaves as lewis acid?

Answer 1

the reason behind it is simple...
The boron in BF3 is electron poor and has an empty orbital, So it can accept a pair of electrons, making it a Lewis Acid.

Answer 2

$BF_3$ acts as Lewis acid

• The substance which can accept the electron pair donated by the Lewis base, they are termed as Lewis acid.
• $BF_3$ is a compound which is made up of two atoms namely boron and fluorine.
• The atomic number of boron is 5 and its electronic setup is 2, 3. Its valency is 3 and Flourine (2,7) valency is 1.
• Consequently, by imparting 1 electron to every fluorine molecule, boron has 3 sigma bonds around it which means that each boron atom is surrounded by 6 electrons.
• To have the steady octet setup Boron needs 2 additional electrons.
• Since boron can accept a couple of electrons from Lewis base, it is considered as Lewis acid.

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