Question

explain the structure of diborane?

Answer 1

Well, it has tetrahedral geometry. I am not sure if you're fmiliar with point group, but it's D\(\sf_{2h}\)

Answer 2

If we consider the molecule B2H6 (diborane Figure 1), there are 12 valence electrons at our disposal for
chemical bonding (B has 3, and H has 1, so 2xB + 6xH =12). Each terminal B–H bond is a standard vanilla
two electron bond, and there are four of these, thus accounting for a total of eight
electrons. This leaves a total of four electrons to share between the two bridging H
atoms and the two B atoms. Consequently, two B–H–B bridging bonds are formed,
each of which consists of two electrons (Figure 2), forming what are called threecenter-
two-electron bonds (i.e., 3 atoms share 2 electrons) – sometimes called
‘banana’ bonds, as they are not linear but curved.
Each B atom is, approximately, sp3 hybridized

Answer 3

Uh, that photo doesn't look like diborane.

Answer 4

it is diborane i guess...!!