Why Graphite Conducts Electricity, but Diamond does not?
In the case of diamond, each carbon atom in a single crystal is covalently bound to four other carbon atoms, forming the four corners of a regular tetrahedron. There are no free electrons available due to the four covalent bonds with each carbon atom. Diamond is a poor conductor of electricity due to the lack of free electrons within its crystalline structure.
Every carbon atom in a single crystal of graphite is covalently bonded to three other carbon atoms. Due to the fact that each carbon atom has four valence electrons, one valence electron is left free for each carbon atom. By applying electric potential, these free electrons can be easily made to flow within the crystalline structure of graphite. As a result, graphite is an excellent electrical conductor.
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Carbon
Carbon is a chemical element with the symbol C and atomic number 6. The name of Carbon is derived from the Latin word Carbo meaning ‘coal’. Carbon is a nonmetallic and tetravalent atom, i.e. it forms four covalent bonds with other atoms. Carbon accounts for only about 0.025% of the Earth’s crust. Carbon is the 15th most abundant element in the Earth’s crust and, by mass, the fourth most abundant element in the universe.
In this article, we will learn about, Carbon the properties of carbon, its uses of carbon, and others in detail.
Table of Content
- What is Carbon?
- Properties of Carbon
- Allotropes of Carbon
- Uses of Carbon
- Biological Role of Carbon
- Occurrence of Carbon