Question

Which of the following is correct regarding diborane $\left(B_2{H}_6\right)$ ?

• A. It has three centred two electron bond
• B. Terminal $H-B-H$ bond angle is ${90}^{\circ }$
• C. Both Boron atoms are $s{p}^2$ hybridised
• D. All hydrogens in $B_2{H}_6$ lie in the same plane

Answer 1

The correct option is A It has three centred two electron bond

Three centered two electron bond is present in diborane, $B_2{H}_6$.
It has two 3- centred 2 electron bond, each one consisting of the two boron atoms and a hydrogen atom sharing two electrons.

Boron is $s{p}^3$ hybridised.
The terminal $H-B-H$ bond angle is nearly ${120}^{\circ }$.
All hydrogens in $B_2{H}_6$ are not in the same plane. Two boron atoms and the four terminal hydrogen atoms of the molecule are in the same plane and the bridging hydrogen atoms lie above and below this plane.
Hence (a) is correct.