Graphite does conduct electricity when melted. This is due to its unique crystalline structure, which consists of layers of hexagonally arranged carbon atoms. These layers allow for high thermal and electrical conductivity, even when graphite is in a molten state.
Graphite's electrical conductivity is a result of its crystalline structure, which allows for the easy movement of electrons through the material. This is because the carbon atoms in graphite are arranged in a hexagonal pattern, creating a network of delocalized electrons that can move freely throughout the material. This delocalization of electrons is what allows graphite to conduct electricity, even when it is melted.
In addition to its electrical conductivity, graphite also has high thermal conductivity. This means that it can efficiently transfer heat, making it an ideal material for applications such as crucibles for metallurgical processes and heat exchangers in chemical industries. The high thermal conductivity of graphite is also what allows it to melt metals such as gold, silver, and platinum.
Overall, the unique crystalline structure of graphite, combined with its high thermal and electrical conductivity, make it a versatile material with a wide range of applications. Its ability to conduct electricity even when melted makes it particularly useful in industries that require the melting and processing of metals.
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