Structure and Properties of Carbon Allotropes: Diamond and Graphite

Introduction to Allotropes

• Definition: Allotropes are different structural forms of the same element in the same physical state.
• Carbon Allotropes: In solid state, carbon exists as diamond, graphite, fullerenes, etc.
• Upcoming Topics: Graphene and fullerenes will be discussed in the next video.

Diamond

• Structure:
  • Giant covalent structure.
  • Carbon atoms are covalently bonded to four other carbon atoms (maximum bonding capacity for carbon).
  • Forms a regular 3D pattern.
• Properties:
  • Very strong and high melting point due to strong covalent bonds.
  • Does not conduct electricity as there are no free electrons or ions.

Graphite

• Structure:
  • Giant covalent structure.
  • Each carbon atom is bonded to three other carbon atoms.
  • Atoms form hexagons that create large flat sheets.
  • Layers are stacked and held weakly, allowing them to slide over each other.
• Properties:
  • Softer than diamond due to weak interlayer forces.
  • High melting point due to strong covalent bonds within layers.
  • Conducts electricity and heat because of delocalized electrons.

Graphene

• Definition: A single layer of graphite.
• Usage: Can be isolated to create other structures like spheres and tubes.

Conclusion

• Recap of the differences in structure and properties between diamond and graphite.
• Mention of future topics on graphene and fullerenes.
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