Uses Of Diamond And Graphite In Chemistry

Graphite has a giant covalent structure in which.

Uses of diamond and graphite in chemistry.

Graphite is mostly used for refractory battery steel expanded graphite brake linings foundry facings and lubricants. Diamonds usually have eight sides forming double pyramids. The dispersion of graphite in oil is known as oil dag and in water is known as aqua dag. Graphite has a lower density than diamond.

This is because of the relatively large amount of space that is wasted between the sheets. Diamond has a tetrahedral structure where as graphite has an hexagonal arrangement. These minerals in general are known to be as polymorphs having the same type of chemistry but of the various crystalline structures. These minerals chemically consist of carbon atoms with different physical properties.

This lesson describes the relationship between the structure and function of the giant covalent substances graphite and diamond. Diamond is a solid form of pure carbon with its atoms arranged in a crystal. The low density 2 26 g cm 3 of graphite is due to large distance between different layers of carbon atoms. Graphite is used as lubricant either as a powder or as a dispersion in oil or water.

Graphene a naturally occurring ingredient in graphite has unique physical properties and is one of the strongest known substances. Some have six sides and they form cubes. Both are made of carbon atoms entirely. Attractions between solvent molecules.

Diamond and graphite both are known as the allotropes of carbon. The rigid network of carbon atoms held together by strong covalent bonds makes diamond very hard. Makes diamond useful for cutting tools such as diamond tipped glass cutters and oil rig drills. When you use a pencil sheets are rubbed off and stick to the paper.

The chemical properties of synthetic and natural diamonds are the same. Carbon atoms in diamond form a tetrahedral arrangement properties and uses. Graphite is insoluble in water and organic solvents for the same reason that diamond is insoluble. The two most common allotropes of pure carbon are diamond and graphite in graphite the bonds are sp 2 orbital hybrids and the atoms form in planes with each bound to three nearest neighbors 120 degrees apart.

Diamond and graphite are allot ropes of each other. Mixed with clay it is used in lead pencils. Graphite is a stable form of naturally occurring carbon also known as plumbago blacklead or mineral carbon. Diamonds so prepared are called synthetic or artificial diamonds.