[Solved] Why Can Graphite Conduct Electricity?

Answer: Graphite is a form of carbon. It consists of sheets of carbon atoms arranged in layers. The reason for the good electrical conductivity is due to the structure of graphite. In fact, each carbon atom is bonded into its layer with three strong covalent bonds; this leaves each atom with a spare electron, which together form a delocalized sea of electrons loosely bonding the layers together.

Why can graphite conduct electricity and not a diamond?

The answer to your question is because of the size and structure of the carbon atoms. In diamond, each carbon atom is bonded to four other atoms, and all the valence electrons are used up in bonding to other carbon atoms. In graphite, each carbon atom is only bonded to three other atoms. The remaining valence electrons can be used for conducting electricity.

In order for a material to conduct electricity well, it must have free electrons that move easily from one atom to another. This allows them to carry a current through a wire or circuit. There are many different ways in which materials can be arranged so that they have free electrons that can conduct electricity well, but these arrangements are not always easy to find.

Which best explains why graphite conducts electricity?

The key to why graphite is a good conductor is that it has high electron mobility. There are two factors that determine this:

1) The number of covalent bonds per carbon atom.

The more covalent bonds there are, the easier it is for electrons to move around. In graphite each Carbon atom forms three covalent bonds, this means that one electron per carbon atom is delocalized. The delocalized electrons can therefore carry the charge throughout the structure, meaning graphite can conduct electricity.

2) The size of the structure.

The bigger the structure, the easier it is for electrons to move around inside it. Graphite has a very large structure (2D sheets), meaning that electrons can move around easily through these sheets.

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