Chemistry – Atoms, elements and compounds - Giant covalent structures | e-Consult
Atoms, elements and compounds - Giant covalent structures (1 questions)
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| Feature | Graphite | Diamond |
| Structure | Layered, hexagonal rings | Giant covalent, tetrahedral arrangement |
| Bonding | Covalent within layers, weak van der Waals forces between layers | Strong covalent bonds throughout |
| Hardness | Soft | Very Hard |
| Electrical Conductivity | Conducts electricity | Does not conduct electricity |
| Uses | Lubricant, electrode | Cutting tools, abrasives |
The difference in structure and bonding directly explains the different uses. Graphite's layered structure and weak interlayer forces allow the layers to easily slide past each other, making it a lubricant. The delocalised electrons within the layers enable electrical conductivity, making it useful as an electrode. Diamond's strong, three-dimensional covalent network results in exceptional hardness, making it ideal for cutting and abrasive applications. The lack of delocalised electrons prevents electrical conductivity.