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(a) sp (b) sp2(c) sp3(d) dsp2
Asked by Neelima Last Modified
Answer Boron has three valence electrons so it is supposed to make three bonds in a molecule with hybridisation sp2 as only s and two p orbitals are used in hybridisation because last p orbital is vacant.
But the case of diborane is different. In diborane bonding of B atom with H and other B is different. Is has two three-centre 2-electron bonds, each one consisting of the two boron atoms and a hydrogen atom sharing two electrons.
The molecule has a total of 12 valence electrons, three from each boron atom and one from each hydrogen atom. In this molecule, each of the two boron atoms will be bonded to two hydrogen atoms via covalent bonds. These bonds will use up 8 of the 12 valence electrons.
The other four valence electrons will be shared by the remaining two hydrogen atoms and by the boron atoms, each particle contributing one orbital to the formation of the 3-centre 2-electron bond. Such a relationship is called the banana bond.
Vishaka Bhutia
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