What is the Difference Between Carbon and Graphite?

Carbon and graphite are related substances, as graphite is an allotrope of carbon. An allotrope refers to a pure element that exists in more than one structural form. The main differences between carbon and graphite are:

1. Structure: Carbon is a non-metal that occurs in different structures called allotropes, such as diamond, charcoal, and graphite. Graphite, on the other hand, has a unique structure with layers of carbon atoms, where each carbon atom is attached to three other carbon atoms via covalent bonds, resulting in a planar carbon layer.
2. Electrical Conductivity: Graphite can conduct electricity due to the presence of an electron cloud formed by the remaining electron of each carbon atom. Other allotropes of carbon, such as diamond and charcoal, cannot conduct electricity.
3. Appearance: Carbon is a dark substance, while graphite is silver/gray in appearance. Graphite is also more crystalline than carbon, which results in a softer material.
4. Uses: Carbon has numerous industrial and biological applications, whereas graphite is primarily used as a pigment, molding agent in glass manufacturing, and as an electron moderator in nuclear reactors.

In summary, carbon is a chemical element, while graphite is an allotrope of carbon with a unique structure and properties, such as the ability to conduct electricity.

Comparative Table: Carbon vs Graphite

Carbon and graphite are related substances, with graphite being an allotrope of carbon. Here is a table highlighting the differences between carbon and graphite:

In summary, carbon is a chemical element that can exist in various structures, including graphite, while graphite is an allotrope of carbon with a unique structure and the ability to conduct electricity.