The type of hybridisation of boron in diborane is\

Question

Professor PC Thomas Classes · Answer

(a) : Each ' $B$ ' atom in diborane $\left(B_{2} \mathrm{H}_{6}ight)$ is $s p^{3}$-hybridised. Of the 4 -hybrid orbitals, three have one electron each, while the $4^{	ext {th }}$ is empty. Two orbitals of each form $\sigma$ bonds with two ' $H$ 'atoms, while one of the remaining hybrid orbital (either filled or empty), $1 s$ orbital of ' H ' atom and one of the hybrid orbitals of other ' $B$ ' atom overlap to form three centered two electron bond. So there exists two such type of three centered bonds.\