Question

Structure of diborane, preparation of biborane ,orbital structure of diborane and properties of diborane

Answer 1

The structure of Diborane molecule consists of four hydrogen atoms and that of two boron atoms coming on the same plane. In between these planes, there are said to be two dividing atoms of hydrogen.

The boron atom is known to be sp3 hybridized and has four hybrid orbitals. From these four hybrid orbitals, three of the orbitals have one electron each, and of which one is an empty orbital. The two electrons of the hybrid orbitals in each of the boron atoms form 2 bonds with the 1s hydrogen atoms. The two atoms of boron left with that of each unpaired electron orbital and empty orbital forms the two bridging (B–H–B) bonds with that of the two 1s hydrogen atoms, is also called as the banana bond.

Properties Of Diborane

Some of the physical and chemical properties of Diborane are as below:

Diborane is said to be a colourless and highly flammable type of gas at the room temperatures. At the high concentrations, it ignites rapidly in the presence of moist air at the room temperature.

It is said to have a boiling point of about 180 K and is a toxic gas.

It releases a huge amount of energy when burnt in the presence of oxygen.

Diborane readily hydrolyzes in water to give hydrogen gas and boric acid.

Most of the diborane are known to be flammable in air.

Uses And Applications Of Diborane

Diborane as a chemical substance has many numbers of applications in various fields, of which some are given below:

Diborane is used as a rocket propellant.

It is utilized in the manufacture of borophosphosilicate which is a form of glass.

In most of the chemical reactions, it is employed as reducing agent.

Diborane is used as a catalyst and rubber vulcanizer in the polymerization reactions.

It is even used as a doping agent in the manufacturing of semiconductor devices.

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Answer 2

Preparation of Diborane:—

$\longrightarrow$The simplest boron hydride known as Diborane. It is prepared by treating boron trifluoride with LiAlH4 in diethyl ether.

$\sf{4BF_{3}+3LiAlH_{4}\longrightarrow\:2B_{2}H_{6}+3LiF+3AlF_{3}}$

$\longrightarrow$A convenient laboratory method for the preparation of Diborane involves the Oxidation of sodium borohydride with iodine.

$\sf{2NaBH_{4}+I_{2}\longrightarrow\:,B_{2}H_{6}+2NaI+H_{2}}$

$\longrightarrow$ Diborane is produced on an industrial scale by reaction of BF3 with sodium hydride.

$\sf{2BF_{3}+6NaH\longrightarrow\:B_{2}H_{6}+6NaF}$

Properties of Diborane:—

$\longrightarrow$ Diborane is colorless.

$\longrightarrow$ It a highly to toxic gas with boiling point of 180 K.

$\longrightarrow$ It catches fire spontaneously upon exposure to air.

$\longrightarrow$ It burns in oxygen releasing an enormous amount of energy.

$\longrightarrow$ Diborane are readily hydrolyzed by water to give boric acid.

$\sf{B_{2}H_{6}+6H_{2}O\longrightarrow\:2B(OH)_{3}+6H_{2}}$