Identify the correct statements regarding structure of diborane:
(This question has multiple correct options)
A. There are two bridging hydrogen atoms
B. Each boron atom forms four bonds
C. The hydrogen atoms are not in the same plane
D. Each boron atom is in \[s{{p}^{3}}\] hybridized state

Hint: Diborane has bridge bonding and it has \[3C-2{{e}^{-}}\] bond. The Boron element has \[1{{s}^{2}}2{{s}^{2}}2{{p}^{1}}\] configuration and its valency is 3. Configuration of boron in borane is \[s{{p}^{2}}\].

Step by step solution:
Diborane is formed by dimerisation of borane:
\[B{{H}_{3}}\xrightarrow{Dimerisation}{{B}_{2}}{{H}_{6}}\]
Diborane has non-planar structure.


“A” is correct, because in diborane there are 6 hydrogen atoms in which 2 hydrogens are bridged and the other 4 are in the same plane.

“B” is correct, because each boron forms four bonds, two bonds with two bridged hydrogen (\[3C-2{{e}^{-}}\]) and two bonds (\[2C-2{{e}^{-}}\]) with the same planar hydrogen.

“C” is correct, because 4 hydrogens are in the same plane and two bridged hydrogens are there to reduce the bond pair – bond pair repulsion.

“D” is correct, because this molecule has a total 12 valance electrons, 3 from boron and 6 from hydrogen. Here, 8 e- are used in normal \[2C-2{{e}^{-}}\] bonds and other 4valence electrons are shared by remaining 2 hydrogens and borons for making banana bonds. Each atom contributes one orbital to form \[3C-2{{e}^{-}}\] bond. Boron uses its vacant p orbital, so its configuration is \[s{{p}^{3}}\].

Note: \[3C-2{{e}^{-}}\] bond is also known as banana bond/p-seudo bond/tau bond. It is a non-planar structure, which we can understand from the configuration of boron (\[s{{p}^{3}}\]). Banana bonds are covalent in nature, so there are 2 electrons which are shared by 3 centres.