Graphite is one of the most chemically resistant materials. At temperatures above 3750 ☌ graphite sublimates even without the presence of oxygen. In an inert gas atmosphere, graphite becomes plastically deformable starting at a temperature of 2500 ☌. Graphite does not have a melting point it changes from the solid state directly into the gaseous state. Graphite has excellent thermal conductivity combined with high temperature resistance. 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. Each carbon atom in a graphite crystal has four valence electrons, also called outer electrons, which can form bonds with neighboring atoms. The fact that graphite is electrically conductive results from its atomic structure. But graphite has other special properties as well: Electrical conductivity of graphite This structure is the reason graphite is very soft and is even used as a lubricant. Thus, the layers can easily be shifted against each other and even separated. Within each layer there are strong bonds, but between the different layers the bonds are very weak. This results in a two-dimensional network of hexagons. In each layer each carbon atom is bound to three others.
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