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Why does boron trifluoride behave as a Lewis acid ?

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The B atoms in `BF_(3)` has only 6 electrons in the valence shell and needs two more electrons to complete its octet. Therefore, it easily accepts a pair of electrons from nucleophiles such as `F^(-), (C_(2)H_(5))_(2)O, RCH_(2)OH`, etc. and thus behaves as a Lewis acid.

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