What is the structural difference between graphite and diamond?

The difference between the structural properties of diamond and graphite is that; four other carbon atoms are bond with each carbon atom in diamond, while in graphite, three other atoms are bond with each carbon atom. Due to this, graphite is made in the form of layers, while diamonds are more of a tetrahedral structure. Graphite is used as a lubricant due to this property that it possesses; the atoms can slide easily over another because they are structured in the form of layers.

In addition, graphite is also a bad or weak conductor of electricity, while a diamond is a good or strong conductor of electricity. Also, the diamond possesses stronger intramolecular bond compared to graphite. Diamond is very strong; it has more strength than graphite. It is used for cutting, drilling, etc. and making such drilling and cutting machines. Diamond has a higher boiling point than graphite. Both diamond and graphite are allotropes of carbon, but with different atomic structures.

Graphite and diamonds are both carbon-based allotropes, and both use covalent bonds, but there are substantial differences between the two. Diamonds are hard and durable. They require quite a bit more work to break them down, as the bonds are stronger. The boiling point for a diamond is much higher than that of graphite. Diamonds are used for a large number of things, including drill bits, and jewelry.

Graphite, on the other hand, is not as strong as a diamond. Instead of a harder substance, it can be broken down easier, as it only has three covalent bonds, not four. The atoms move quite a bit more comfortable in graphite, and the boiling point to break it down is not major.

The molecular bonds of graphite are finer, which makes it a better lubricant, than that of a diamond. In addition to being used used as a lubricant, some of the primary uses for graphite are electrical, pencils, and clay.