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Hint: The carbon atoms in a diamond are linked to four other carbon atoms through a single bond. There is a definite three dimensional geometry holding them together.
Complete step by step solution: We know that diamond is the purest form of carbon and it exists as a three-dimensional network solid. It occurs in nature and can also be prepared artificially but because of high cost and poor quality diamonds are seldom made artificially. It is an allotrope of carbon just like graphite and coal. Allotropes are compounds which are chemically similar but significantly vary from each other in their physical properties.
The self-linking property of carbon, which is also known as self-catenation, is shown to the greatest extent in diamond. There is no specific rule defining the number of carbon atoms in a diamond; it just depends directly on the size of the diamond.
In diamond, carbon is \[s{{p}^{3}}\]-hybridized, which means it has a tetrahedral geometry. Each carbon atom is tetrahedrally linked to four other neighboring carbon atoms through four strong $C-C$ , \[s{{p}^{3}}-s{{p}^{3}}\] bonds. This network extends in three dimensions.
Since diamond exists as a three dimensional network solid, it is the hardest substance known with high density and melting point.
Since all the electrons are firmly held in the single bonds between the carbon atoms, there are no free electrons in a diamond crystal. Therefore, diamond is a bad conductor of electricity. However, it has the highest thermal conductivity of any known substance.
Also, because of its high refractive index, diamond can reflect and refract light. It is, therefore, a transparent substance.
Note: Other than being used as an ornamental material, because of its hardness, diamond is used for cutting glass, making bores for rock drilling and for making abrasives.
They are also used for drawing thin wires from metals using a tool called Dies. The need for high pressure demands something very strong and diamonds are the first choice.
Complete step by step solution: We know that diamond is the purest form of carbon and it exists as a three-dimensional network solid. It occurs in nature and can also be prepared artificially but because of high cost and poor quality diamonds are seldom made artificially. It is an allotrope of carbon just like graphite and coal. Allotropes are compounds which are chemically similar but significantly vary from each other in their physical properties.
The self-linking property of carbon, which is also known as self-catenation, is shown to the greatest extent in diamond. There is no specific rule defining the number of carbon atoms in a diamond; it just depends directly on the size of the diamond.
In diamond, carbon is \[s{{p}^{3}}\]-hybridized, which means it has a tetrahedral geometry. Each carbon atom is tetrahedrally linked to four other neighboring carbon atoms through four strong $C-C$ , \[s{{p}^{3}}-s{{p}^{3}}\] bonds. This network extends in three dimensions.
Since diamond exists as a three dimensional network solid, it is the hardest substance known with high density and melting point.
Since all the electrons are firmly held in the single bonds between the carbon atoms, there are no free electrons in a diamond crystal. Therefore, diamond is a bad conductor of electricity. However, it has the highest thermal conductivity of any known substance.
Also, because of its high refractive index, diamond can reflect and refract light. It is, therefore, a transparent substance.
Note: Other than being used as an ornamental material, because of its hardness, diamond is used for cutting glass, making bores for rock drilling and for making abrasives.
They are also used for drawing thin wires from metals using a tool called Dies. The need for high pressure demands something very strong and diamonds are the first choice.
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