How the same carbon atom can build both a diamond and pencil lead
In short: Explore how the arrangement of atoms determines the physical world. This video explains the distinct structures of diamond and graphite, revealing why one is the world's hardest material while the other is soft enough to write with.
Carbon atoms can form different structural versions called allotropes. In diamond, each carbon atom bonds to four others in a rigid 3D lattice, creating a giant covalent structure that is exceptionally strong and has a high melting point. Because there are no free electrons, diamond cannot conduct electricity.
Graphite differs significantly; its atoms bond to only three others in hexagonal rings. This creates layers held together by weak forces, allowing them to slide over one another. However, because electrons are delocalised between these layers, graphite can conduct heat and electricity. The video also introduces graphene as a single layer of graphite and mentions fullerenes. Understanding these structures explains why identical elements can exhibit opposite physical properties based solely on their geometry.
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Sources
- Summary by Intellect · source: GCSE Chemistry - Diamond & Graphite - Structure | Properties (2027/28 exams)
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