Question

Explain the structure of diborane.

Answer 1

Dear student,

● Structure of diborane -

• B-atom in diborane is sp3 hybridized.
• Diborane has 4 normal B-H terminal bonds and two B-H-B bridge bonds in its structure.
• Bridge bonds B-H-B are called as banana bonds.
• 2 B atoms and 4 terminal H atoms lie in same plane while 2 bridge H atoms lie above & below the plane.
• B2H6 molecule has total 8 covalent bonds but only 6 pairs of e-. Hence it is electron deficient.

[Refer to the figure for structure of diborane.]

Hope this helps you...

Answer 2

★ STRUCTURE OF DIBORANE:-

→ In diborane each boron atom undergoes sp3 hybridisation giving four sp3 hybrid orbitals. Out of four hybrid orbital one is vacant.

→ Each boron forms two bond with two hydrogen atoms by overlapping with 1s orbital of hydrogen atom.

→ That is 4B-H bonds in which those hydrogen atoms are called terminal hydrogen.

→ The remaining half filled hybrid orbitals of one boron atoms and the vacant hybrid orbital of second boron atom overlap simultaneously with half filled orbital of hydrogen atom and forms B-H-B bonds. Here hydrogen atoms are called bridged hydrogen.

→ The B-H bond is formed by sharing a pair of electrons so it is called two-centre two electron bonds (2c-2e)

→ In B-H-B bond is formed each bridged hydrogen is bonded to two boron atoms by a pairs of electrons (2e) that is called two electron bond (3c-2e) also known as banana bonds.