(a) Diborane

$\mathrm{B}_{2} \mathrm{H}_{6}$ is a compound that does not have an electron. $\mathrm{B}_{2} \mathrm{H}_{6}$ just has 12 electrons $-6 \mathrm{e}^{-}$of $6 \mathrm{H}$ molecules and $3 \mathrm{e}^{-}$of $2 \mathrm{~B}$ iotas each. So none of the boron molecules has any electrons left subsequent to being blended in with $3 \mathrm{H}$ particles. $\mathrm{X}$-beam diffraction studies showed the diborane structure as:

Two boron and four-terminal molecules of hydrogen $\left(\mathrm{H}_{\mathrm{t}}\right)$ lie one way, while the other two connecting particles of hydrogen $\left(\mathrm{H}_{\mathrm{b}}\right)$ are in the surface opposite to the plane of boron iotas. Once, of the two molecules of hydrogen spanning, one particle of $\mathrm{H}$ lies over the plane, and the other beneath the plane. The terminal bonds are standard twocentre two-electron $\left(2 c-2 e^{-}\right)$bonds, while the two bridgings $(B-H-B)$ bonds are three-focus two-electron (3c $\left.- 2 \mathrm{e}^{-}\right)$bonds.

(b) Boric corrosive

Boric corrosive is organized in a layered structure. Each planar unit $\mathrm{BO}_{3}$ is associated by molecules $\mathrm{H}$ to one another. The $\mathrm{H}$ molecules structure a covalent bond with a $\mathrm{BO}_{3}$ unit while another $\mathrm{BO}_{3}$ unit frames a hydrogen bond. The dabbed lines, in the given figure, address hydrogen bonds.