(40) GCSE Chemistry Revision "Graphite"

Overview of Graphite

• Graphite is a form of carbon, classified as a giant covalent molecule.

Properties of Graphite

Key Properties

• Soft and Slippery: Graphite has a unique structure that allows its layers to slide over one another, making it useful as a lubricant in machinery.

• High Melting and Boiling Points: The presence of strong covalent bonds requires a significant amount of energy to break, leading to high melting and boiling points.

• Good Conductors of Electricity and Heat: The movement of delocalized electrons within graphite enables it to conduct both electricity and thermal energy effectively.

Structure of Graphite

• Covalent Bonds Formation: In graphite, each carbon atom forms covalent bonds with three other carbon atoms.

• Hexagonal Rings: Carbon atoms are arranged in hexagonal rings of six atoms. These rings are stacked in layers.

• Layered Arrangement: There are no covalent bonds between the layers, allowing them to slide easily, contributing to the softness and lubricating properties of graphite.

Delocalized Electrons

• Electron Configuration: Each carbon atom in graphite has one electron that is not involved in covalent bonding, resulting in delocalized electrons that can move freely.

• Conductivity Comparison: Similar to metals, the mobility of delocalized electrons in graphite facilitates the conduction of electricity and heat, even though graphite is not a metal.

Summary of Comparison with Diamond

• In contrast to diamond, which is very hard due to a higher number of covalent bonds and cannot conduct electricity, graphite's structure provides it with unique properties such as softness, gleaming conductivity, and high thermal stability.