The hybrid state of B-atom in boron-hydride is sp², while in its dimer it has sp³ hybrid state because :

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$B_{2} H_{6}$ is an electron rich compound

one of the empty orbitals of boron takes part in hybridisation

overlapping between s and p-orbitals of H and B forms $π$ -bond

$B_{2} H_{6}$ is less stable than ${BH}_{3}$

answer is A.

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Detailed Solution

Because it has three valence electrons, the element borax should make three bonds in a molecule (sp²) during hybridization because only the s and p orbitals are used, leaving the final p orbital unoccupied.
The diborane, on the other hand, contains two electrons per bond and three centre bonds. Each boron atom is joined by four hydrogen atoms. This leads to tetrahedral geometry.
As a result, every boron atom is sp³hybridized.

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