The sheets are not connected through covalent bonds their atoms interact via London dispersion forces.

However, these sheets interact with each other weakly.

It could also mean that the carbon sheets are very powerfully bonded.

Graphene layers are singular sheets of carbon atoms, and the ring arrays are organised in large sheets. Each carbon atom is connected with other carbon atoms in this type of molecular orbital model.Carbon atoms arranged in these rings are in an sp² hybridised state.An endless sequence of fused benzene rings could be used to make layers of linked rings.These hexagonal rings are connected at their edges. Graphite has layers of carbon arranged in hexagonal rings along with six members.The graphite structure is a trigonal planar, and the atoms have a bond angle of 120° between them. Molecular Geometry of GraphiteĪs we know, the hybridisation of graphite is an sp² hybridisation. This weak force could be the reason that graphite is highly anisotropic, with mechanical, electrical, and thermal properties that are very dissimilar within in-plane and out-of-plane directions. Graphite has different properties as the layers have a weak force between them. The hybridised carbon atoms thus formed are put together in several layers, and in those layers, they are arranged in a hexagonal arrangement.The structure made by these atoms is a trigonal planar geometry and the C-C-C bond formed has a 120° angle.These newly formed orbitals connect each atom of carbon to the other three atoms by a covalent bond.

Carbon has a general electronic configuration of (1s 2, 2s 2, 2p 2 ) thereby spreading the four valence electrons in the s and p orbitals. In sp² hybridisation, one s orbital and two p orbitals combine to form three sp² orbitals. The Hybridisation of GraphiteĬarbon atoms undergo sp² hybridisation to form graphite. Carbon atoms undergo sp² hybridisation to form graphite. Graphite has layers of atoms of carbon that are put together in six-membered hexagonal rings. Hybridisation is when two or more atomic orbitals are combined to form a new hybridised orbital. The process of hybridisation of carbon forms graphite. It is because of the arrangement of carbon atoms in the molecule. Both are pure carbon, but still, they have different properties. Graphite is soft, opaque, and can conduct electricity on the other hand, diamond is hard, transparent, and cannot conduct electricity. Carbon has different allotropes, such as graphite and diamond.

Carbon atoms in graphite