Some Important Compounds Of Boron
Chapter Name : The P- Block Elements |
Sub Topic Code : 102_11_11_04_03 |
Topic Name : Some Important Compounds Of Boron |
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Sub Topic Name : Diborane |
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Introduction
• The simplest boron hydride known, is diborane. • It is prepared by treating boron trifluoride with LiAlH4 in diethyl ether. • A convenient laboratory method for the preparation of diborane involves the oxidation of sodium borohydride with iodine. • Diborane is produced on an industrial scale by the reaction of BF3 with sodium hydride. • Diborane is a colourless, highly toxic gas with a b.p. of 180 K. • Diborane catches fire spontaneously upon exposure to air. • It burns in oxygen releasing an enormous amount of energy. • Most of the higher boranes are also spontaneously flammable in air. • Boranes are readily hydrolysed by water to give boric acid. • The structure of diborane has four terminal hydrogen atoms and the two boron atoms lie in one plane.
Pre-Requisites:
Elements, periodic table, Group
Activity:
• Group 13 has aluminium, boron which are important industrial elements.
Real Life Question:
What is boron used for?
Key Words / FlashCards
| Key Words | Definitions (pref. in our own words) |
|---|---|
| P block elements | Have the last electron in the outermost p orbital. |
Learning aids / Gadgets
| Gadgets | How it can be used |
|---|---|
| Boric acid | Used for killing insects. |
Real life uses :
• Diborane is used as a rubber vulcaniser and as a catalyst for hydrocarbon polymerisation.
Places to visit :
Chemistry lab, kitchen.
Practical examples around us
| Examples | Explainations |
|---|---|
| Boric acid | Used for killing insects. |
What you learn in Theory:
• The simplest boron hydride known, is diborane. • It is prepared by treating boron trifluoride with LiAlH4 in diethyl ether. • A convenient laboratory method for the preparation of diborane involves the oxidation of sodium borohydride with iodine. • Diborane is produced on an industrial scale by the reaction of BF3 with sodium hydride. • Diborane is a colourless, highly toxic gas with a B.P. of 180 K. • Diborane catches fire spontaneously upon exposure to air. • It burns in oxygen releasing an enormous amount of energy. • Most of the higher boranes are also spontaneously flammable in air. • Boranes are readily hydrolysed by water to give boric acid. • The structure of diborane has four terminal hydrogen atoms and the two boron atoms lie in one plane.
What you learn in Practice:
• Group 13 has aluminium, boron which are important industrial elements.