Interactive 3D visualization of diamond and graphite
Diamond has a tetrahedral crystal structure where each carbon atom forms four covalent bonds arranged in a tetrahedral geometry (sp³ hybridization). This creates a strong 3D network structure, making diamond extremely hard with a high melting point. Each C-C bond angle is 109.5°.
Graphite consists of layered hexagonal sheets of carbon atoms (sp² hybridization). Within each layer, atoms are strongly bonded in a hexagonal pattern, but layers are held together by weak van der Waals forces, making graphite soft and allowing the layers to slide over each other easily.
Coal has an amorphous (disordered) structure composed of randomly oriented carbon atoms and clusters. Unlike diamond and graphite, coal is not a pure crystalline form—it contains irregular graphite-like fragments, impurities (hydrogen, oxygen, nitrogen, sulfur), and various organic compounds. This disordered structure makes coal less conductive than graphite and much softer than diamond.