What is the Difference Between Diamond Graphite and Fullerene?

Diamond, graphite, and fullerene are allotropes of carbon, meaning they are different forms of the same element. They have distinct structures and properties due to the different arrangements of carbon atoms in their structures.

• Diamond:
• Giant macromolecular structure.
• Diamond cubic crystal structure.
• Each carbon atom is attached to four other carbon atoms in a tetrahedral arrangement.
• Covalent bonding.
• No delocalized electrons.
• Bond angles of 109°.
• Hardest naturally occurring material on Earth.
• Graphite:
• Layered structure of hexagonal rings.
• Hexagonal crystal structure.
• Each carbon atom is attached to three other carbon atoms.
• Covalent bonding and London dispersion forces.
• Delocalized electrons.
• Bond angles of 120°.
• Electrical conductor.
• Fullerene:
• Spheres made of atoms arranged in hexagons.
• Large spheroidal molecule structure.
• Each carbon atom is attached to three other carbon atoms.
• Covalent bonding and London dispersion forces.
• Delocalized electrons.
• Bond angles between 109° and 120°.

In summary, the key difference between diamond, graphite, and fullerene is their structure, bonding, and properties, which arise from the distinct arrangements of carbon atoms in their respective structures.

Comparative Table: Diamond Graphite vs Fullerene

Diamond, graphite, and fullerene are all allotropes of carbon, meaning they have the same chemical composition but different arrangements of atoms. Here is a comparison of their structures and properties:

In summary, diamond has a three-dimensional covalent network structure, graphite has layers of hexagonally arranged carbon atoms bonded covalently within each layer, and fullerene has a hollow, cage-like structure made up of 60 carbon atoms. The different arrangements of carbon atoms in these allotropes lead to unique properties and applications based on their structure and bonding.