Carbon atoms in graphite are covalently bonded to form flat atomic layers arranged in an ordered hexagonal lattice. Each carbon atom tightly connects with three neighboring carbon atoms within the same plane, constructing stable two-dimensional planar networks. This distinctive atomic layout lays the fundamental foundation for graphite’s characteristic performance, including excellent electrical conductivity and outstanding self-lubricating capability. Without this hexagonal planar structure, graphite would not possess the comprehensive physical and chemical properties that distinguish it from other carbon materials.
These planar carbon layers stack upon one another to form bulk graphite. Adjacent layers are only bound by weak van der Waals intermolecular forces instead of firm covalent bonds. The weak bonding allows the atomic sheets to slide smoothly relative to each other under external force. This unique structural feature delivers good flexibility and machinability, supporting widespread utilization across metallurgy, new energy, machinery manufacturing and many other industrial sectors.
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