Chemistry – Physical chemistry | e-Consult
Physical chemistry (1 questions)
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Diamond: Diamond has a giant covalent structure where each carbon atom is covalently bonded to four other carbon atoms in a tetrahedral arrangement. This results in a strong, rigid, and three-dimensional network of covalent bonds.
Graphite: Graphite also consists of carbon atoms, but the carbon atoms are arranged in layers. Within each layer, the carbon atoms are covalently bonded in a hexagonal lattice. However, the layers are held together by weak van der Waals forces.
Comparison of Physical Properties:
- Hardness: Diamond is extremely hard due to its strong covalent network. Graphite is soft and can be easily powdered.
- Melting Point: Diamond has a very high melting point due to the strong covalent bonds. Graphite has a much lower melting point.
- Electrical Conductivity: Diamond is an electrical insulator because there are no free electrons. Graphite is a good conductor of electricity because the delocalised electrons in the layers can move freely.
- Chemical Reactivity: Diamond is chemically very inert. Graphite is more reactive and can be oxidised at high temperatures.
Bonding Types: Diamond exhibits strong covalent bonding, while graphite exhibits strong covalent bonding within the layers and weak van der Waals forces between the layers.