The structure of diamond is such that each carbon atom forms 4 covalent bonds with other carbon atoms. The carbon atoms are positioned around each other in a tetrahedral arrangement, and the network of carbon atoms extends almost unbroken throughout the whole structure, giving diamond a crystalline structure. Most of the diamonds used around the world have been mined from the Earth's crust. Artificial diamonds can be made by heating other forms of carbon under high pressure, though they are typically too small for jewelry but can be used for drill tips.
Physical Properties of Diamond
- High melting & boiling points, similar to graphite, due to the same reason
- Hardness: diamond cannot be easily scratched because of its difficult-to-break network of strong covalent bonds
- Does not conduct electricity: all of the 4 outer electrons on every carbon atom are involved in covalent bonding, leaving no free electrons available to carry electric current
- Good conductor of heat
Chemical Properties of Diamond
The chemical formula of diamond is C, and it is not a good conductor of electricity owing to its strong covalent bonds.
Uses of Diamond
The properties of diamond, specifically its hardness and ability to conduct heat, make it useful in various industrial applications, including cutting, grinding, and drilling. Additionally, diamonds are also used in jewelry.
Allotropes of Carbon
Diamond and graphite are two well-known allotropes of carbon, with distinct differences in their physical and chemical properties. Whereas diamond has a crystalline structure and is extremely hard, graphite has a layered structure and is relatively soft and slippery.
When comparing the properties of diamond and graphite, it is essential to note that they exhibit differences in hardness, electrical conductivity, and uses, all stemming from their unique structures and bonding between carbon atoms.
In conclusion, the properties of diamond and graphite, including their physical and chemical properties, make them valuable in various applications, highlighting the significance of their unique structures and bonding arrangements.
