Allotropes Of Carbon
Chapter Name : The P- Block Elements |
Sub Topic Code : 102_11_11_08_01 |
Topic Name : Allotropes Of Carbon |
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Sub Topic Name : Diamond |
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Introduction
• Carbon exhibits many allotropic forms; both crystalline as well as amorphous. • Diamond and graphite are two well-known crystalline forms of carbon. • In 1985, third form of carbon known as fullerenes was discovered by H.W.Kroto, E.Smalley and R.F.Curl. • For this discovery they were awarded the Nobel Prize in 1996. • It has a crystalline lattice. • In diamond each carbon atom undergoes sp3 hybridisation and linked to four other carbon atoms by using hybridised orbitals in tetrahedral fashion. • The C–C bond length is 154 pm. • The structure extends in space and produces a rigid three dimensional network of carbon atoms. • In this structure directional covalent bonds are present throughout the lattice. • It is very difficult to break extended covalent bonding and, therefore, diamond is the hardest substance on the earth. • It is used as an abrasive for sharpening hard tools, in making dyes and in the manufacture of tungsten filaments for electric light bulbs.
Pre-Requisites:
Elements, periodic table, allotrope
Activity:
It is used as an abrasive for sharpening hard tools, in making dyes and in the manufacture of tungsten filaments for electric light bulbs.
Real Life Question:
What is diamond 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 |
|---|---|
| Diamond | Diamond is used to cut glass. |
Real life uses :
• It is used as an abrasive for sharpening hard tools, in making dyes and in the manufacture of tungsten filaments for electric light bulbs.
Places to visit :
Chemistry lab, kitchen.
Practical examples around us
| Examples | Explainations |
|---|---|
| Diamond | It is used as an abrasive for sharpening hard tools, in making dyes and in the manufacture of tungsten filaments for electric light bulbs. |
What you learn in Theory:
• Carbon exhibits many allotropic forms; both crystalline as well as amorphous. • Diamond and graphite are two well-known crystalline forms of carbon. • In 1985, third form of carbon known as fullerenes was discovered by H.W.Kroto, E.Smalley and R.F.Curl. • For this discovery they were awarded the Nobel Prize in 1996. • It has a crystalline lattice. • In diamond each carbon atom undergoes sp3 hybridisation and linked to four other carbon atoms by using hybridised orbitals in tetrahedral fashion. • The C–C bond length is 154 pm. • The structure extends in space and produces a rigid three dimensional network of carbon atoms. • In this structure directional covalent bonds are present throughout the lattice. • It is very difficult to break extended covalent bonding and, therefore, diamond is the hardest substance on the earth. • It is used as an abrasive for sharpening hard tools, in making dyes and in the manufacture of tungsten filaments for electric light bulbs.
What you learn in Practice:
• Diamond is the hardest substance on this earth.