Graphite has a layered structure where the carbon atoms in each layer are bonded in hexagonal arrays with covalent bonds; the layers are bonded to each other by secondary bonds, that is, Van der Waals interactions. The weak bonds among the layers determine weak shear strength, so that they can slide one each other by applying low force. Hence, graphite is anisotropic, as properties depend on the direction of force application. 

It is a good thermal and electrical conductor along each layer of graphite but not perpendicular to it. The reason for the good electrical conductivity is due to the structure of graphite. In fact, each carbon atom is bonded into its layer with three strong covalent bonds; this leaves each atom with a spare electron, which together form a delocalized sea of electrons loosely bonding the layers together. These delocalized electrons can all move along together on each layer, making graphite a good electrical conductor. 

Natural graphite and artificial graphite have always been the largest negative electrode materials. However, artificial graphite requires high temperature treatment during the production process, which greatly increases its production cost and has an adverse impact on the environment. 

Compared with artificial graphite, natural graphite has many advantages Its low cost, high degree of crystallinity, mature purification, crushing, and classification technology, low charge and discharge voltage platform, and high theoretical specific capacity have laid a good foundation for its application in the lithium-ion battery industry.