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Electrical conductivity of graphite

The fact that Graphite is electrically conductive results from its atomic structure. Each carbon atom in a graphite crystal has four valence electrons, also called outer electrons, which can form bonds with neighboring atoms. However, only three of the four valence electrons enter into a bond, while the fourth electron remains freely mobile and thus allows electricity to be conducted. Graphite has a layer structure. In each layer, each carbon atom is bound to three others. This results in a two-dimensional network of hexagons. There are strong bonds within each layer, but the bonds are very weak between the different layers. Thus, the layers can easily be shifted against each other and even separated. This structure is why Graphite is very soft and even used as a lubricant. But Graphite also has other special properties: Graphite is a naturally occurring modification of carbon (chemical formula: C). Its atoms arrange themselves in the hexagonal pattern, which is typical for carbon, and thus form a hexagonal layered lattice. Graphite gets its typical grey color from its opaque grey to black crystals. While diamond, another carbon modification, is the hardest naturally occurring material in the world, with a value of 10 on the Mohs hardness scale, Graphite is one of the softest, with a value of 1-2. The different properties of graphite and diamond result from their structure: If you are looking for high quality, high purity, and cost-effective Graphite, or if you require the latest price of Graphite, please feel free to email contact mis-asia.

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