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The type of hybridisation of boron in diborane is
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The correct answer is:
$s p^3-$ hybridisation
Boron has three valence electrons, so it is supposed to make 3 bonds in a molecule with hybridization, $\mathrm{sp}^2$ as only $\mathrm{s}$ and two p orbitals are used in hybridization and last p orbitalis vacant.
But diborane, $\mathrm{B}_2 \mathrm{H}_6$ contains two electrons each, three centred bonds. Each Boron atom is in a link with four hydrogen atoms. This makes tetrahedral geometry.
Hence, each Boron atom is $\mathrm{sp}^3$ - hybridized. The correct option is $3$.
But diborane, $\mathrm{B}_2 \mathrm{H}_6$ contains two electrons each, three centred bonds. Each Boron atom is in a link with four hydrogen atoms. This makes tetrahedral geometry.
Hence, each Boron atom is $\mathrm{sp}^3$ - hybridized. The correct option is $3$.
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