Boron fluoride exists as BF_{3} but boron hydride doesn’t exist as BH_3. Give reason. In which form does it exist? Explain its structure.

Answers (1)

The lone pair of electrons in Boron fluoride form a pπ- pπ bonds and accept electrons to reduce the deficiency of them. Thereby reducing the ability of Boron to accept electrons and not becoming a Lewis Acid but instead increasing stability.

 

In BH_3 hydrogen has a lone pair. It therefore, cannot fulfil the deficiency of boron to dimerise to form B_{2}H_{6} which is in the shape of a banana.

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