Graphite is a crystalline form of the element carbon. It is a non-metal and is one of the three familiar naturally occurring forms of carbon, the other two being coal and diamond. Graphite has a layered, planar structure and is a good conductor of electricity due to the delocalized electrons within its layers. It is commonly used as a lubricant, in pencils, and as a moderator in nuclear reactors.
Graphite has a unique structure that consists of layers of carbon atoms arranged in a hexagonal lattice. Within each layer, the carbon atoms are covalently bonded to form strong, stable bonds. However, between the layers, the bonding is much weaker, allowing the layers to slide over each other easily. This property gives graphite its lubricating quality and makes it useful for applications where low friction is desired.
Graphite has several notable physical properties, including:
Graphite has a variety of important uses, including:
To study graphite effectively, it's important to understand its structure, properties, and uses. Here are some key points to focus on:
By mastering these concepts, you will develop a comprehensive understanding of graphite and its significance in various fields.
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