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(B) Boron compounds are often employed as Lewis acids due to their strong electrophilic nature,which is caused by a vacant $p$-orbital that can accept

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electron deficient nature

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(B) Boron compounds are often employed as Lewis acids due to their strong electrophilic nature,which is caused by a vacant $p$-orbital that can accept electrons.Boron behaves as a Lewis acid because it has only $3$ valence electrons,leaving its octet incomplete.For example,$B_2H_6$ is an electron-deficient compound.The electronic configuration of Boron is $B (Z=5) = [He] 2s^2 2p^1$.This results in a total of $6$ electrons in the valence shell of the central atom in compounds like $BF_3$,which is less than the $8$ required for a complete octet.

Boron compounds behave as Lewis acids because of their

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