Hybridisation of boron in diborane is

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(C) In diborane $(B_2H_6)$, each boron atom is bonded to four hydrogen atoms (two terminal and two bridging). To accommodate these four bonds, the bor

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$sp^3$

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(C) In diborane $(B_2H_6)$, each boron atom is bonded to four hydrogen atoms (two terminal and two bridging). To accommodate these four bonds, the boron atom undergoes $sp^3$ hybridisation. Three of the $sp^3$ hybrid orbitals contain one electron each, while one is empty. The two terminal $B-H$ bonds are normal covalent bonds, while the two bridging $B-H-B$ bonds are three-center two-electron $(3c-2e)$ bonds, often referred to as banana bonds. Therefore, the hybridisation of boron in diborane is $sp^3$.

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