Graphite is a transitional crystal between atomic crystals, metal crystals and molecular crystals. In the crystal, the same layer of carbon atoms are hybridized by SP2 to form a covalent bond. Each carbon atom is connected to the other three carbon atoms. The six carbon atoms form a positive hexagonal ring on the same plane. Essence There is also a P orbit left in the carbon atoms of the same plane. They overlap each other to form the icon π -key electrons can move freely and can be excited in the lattice. Therefore, graphite has metallic luster, which can conduct electricity and heat transfer. Due to the large distance between the layers and the layer, the combination of force (Van Dehua) is small, each layer can slide, so the density of the graphite is smaller than the diamond stone, soft and slippery. [1]

The distance between each layer of the graphite is 3.40å, which is combined with Van Dehua, that is, the molecular crystals between the layers and the layer, and the spacing of the carbon atom in the same network layer is 1.42å. Because the carbon atom on the same plane layer is on the same plane layer The binding between is strong and it is extremely difficult to destroy, so the melting point of graphite is also very high, and the chemical properties are stable. Given its special key way, it cannot be single -considers that it is a single crystal or polycrystal, and now it is generally believed that graphite is a mixed crystal.

Graphite belongs to the hexagonal crystal, with a complete layer -like lapse. The molecular keys are mainly attractive to the molecular keys, so it is naturally floating.