Boron Hydrides

   Boron forms hydrides of the types B_nH_n+4 and B_nH_n+6 known as boranes. Diborane is the simplest boron hydride which is a dimer of BH₃ .

         Preparation

 (c) In the laboratory, it is prepared by the oxidation of sod. Borohydride with I₂.

         Properties: (a) Since Boron in boranes never complete its octet of electrons hence all boranes are called as electron-deficient compounds or Lewis acids.

         (b) All boranes catch fire in the presence of oxygen to liberate a lot of heat energy. Hence, they can also be used as high energy fuels.

         (c) Boranes are simply hydrolysed by water.

         (d) With carbon monoxide

         (e) The boranes are used for the formation of hydroborates or borohydrides such as LiBH₄ or NaBH₄ , which are extensively used as reducing agents in the organic synthesis.

   Structure of diborane : B₂H₆ has a three centre electon pair bond also called a banana shape bond.

   (a) B - H_t : It is a normal covalent bond (two centre electron pair bond that is 2c - 2e). 

   (b) B-H_b: This is a bond between three atoms, B-H_b-B  (three centre electron pair bond that is 3c-2e)

   The other boron hydrides are B₅H₉, B₄H₁₀, B₅H₁₁ etc.

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