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Boron compounds behave as Lewis acid because of their
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electron deficient in nature
Boron compounds are often employed as Lewis acids due to strong electrophilic nature granted by a vacant $p$-orbital into which electrons can be received. It behaves as Lewis acid as its number of valence shell electrons is 3 . Thus, its octet is incomplete.
e.g. $\mathrm{B}_2 \mathrm{H}_6$ (electron deficient compounds)
$$
\mathrm{B}(Z=5)=[\mathrm{He}] 2 s^2 2 p^1
$$
$\Rightarrow$ Total 5 electrons (incomplete octet)
e.g. $\mathrm{B}_2 \mathrm{H}_6$ (electron deficient compounds)
$$
\mathrm{B}(Z=5)=[\mathrm{He}] 2 s^2 2 p^1
$$
$\Rightarrow$ Total 5 electrons (incomplete octet)
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