Graphite does not have a defined melting point; instead, it sublimates, which means it transitions directly from a solid to a gas without passing through a liquid phase. This sublimation occurs at extremely high temperatures, typically around 3600°C (6512°F) under standard atmospheric pressure.
The reason graphite does not melt is due to its unique crystalline structure. Graphite is composed of carbon atoms arranged in hexagonal sheets stacked on top of each other with weak van der Waals forces between the layers. This structure allows the layers to slide over each other easily, giving graphite its characteristic softness and lubricity. When heated, these layers vibrate more intensely until they eventually overcome the weak interlayer forces and break free, transitioning directly into a gaseous state.
This property of graphite makes it extremely useful in high-temperature applications. It can withstand temperatures up to 5000°F (2760°C) without melting or chemically decomposing, which is why it is commonly used in furnaces, crucibles for melting metals, and as heating elements in high-temperature processes. Its thermal stability, resistance to thermal shock, and inertness to most chemicals further enhance its suitability for these applications.
In summary, graphite's unique structure and properties prevent it from melting and instead cause it to sublime at very high temperatures, making it a valuable material in extreme thermal environments.
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