The elements that have delocalized electrons can conduct electricity and the type of conductor depends on the ease of electrons to flow across. The element that possesses low resistance to electrons to flow is a good conductor whereas the elements that possess greater resistance are classified as a bad conductor.
Usually the elements. And the elements that do not have any delocalized electrons present to move are classified as insulators because there are no electrons present to flow current across it. Examples of such elements are plastic, wood, etc.
In Graphite, due to the presence of a delocalized electron of a carbon atom, it can move freely across it. And on applying a potential difference across graphite, the electric current flows through it. The resistance also plays an important role in determining the type of conductor. The calculated resistivity of pure graphite is calculated as 1.
Graphite is also used as dominant anode material in lithium-ion batteries due to its ability to intercalate lithium ions without significant damage from swelling. Resistance is the measure of obstacle offered to the flow of electrons that conducts the electricity. Resistance is usually generated by the heat caused when kernels collide to each other when electrons move fastly across it when voltage is applied across that element.
Diamond is a bad conductor of electricity because it does not have any delocalized electron like graphite. However graphite and diamond both are allotropes of carbon having the same composition but different structures. Free electrons are carriers of electric current. It is not possible for an element to exhibit electrical conductance without free ions or electrons.
If we talk about the lattice structure of diamond, carbon atoms form a three-dimensional network resulting in a tetrahedral structure. Each carbon atom forms a covalent bond with four other adjacent carbon atoms.
Hence all four vacant electrons take participate in the covalent bond leaving behind no free electrons. Whereas in graphite each carbon atom is bonded to three carbon atoms leaving behind one free electron to conduct electricity.
Graphite is a good conductor whereas diamond is an insulator. This explains why diamond does not conduct electricity. The bonding also explains the hardness of diamond and its high melting point. Significant quantities of energy would be needed to separate atoms so strongly bonded together. Graphite contains layers of carbon atoms. Graphite is black, shiny and opaque. It is not transparent. It is also a very slippery material. It is used in pencil leads because layers easily slide onto the paper, leaving a black mark.
This makes graphite slippery, so it is useful as a lubricant. Explain why diamond does not conduct electricity and why graphite does conduct electricity. Diamond does not conduct electricity because it has no charged particles that are free to move.
Graphite does conduct electricity because it has delocalised electrons which move between the layers. Diamond and graphite Diamond and graphite are different forms of the element carbon. The reason graphite can conduct electricity is because there are delocalized electrons that are mobile across the layers. This is the same reason why metals can conduct. When metallic atoms come together they sacrifice their valence electrons to a sea of delocalized electrons that can move between the ions.
Therefore, the feature of graphite responsible for its electrical conductivity is its delocalized electrons. The presence of strong covalent bonds, weak interlayer interactions, or a high sublimating temperature have no direct impact on electrical conductivity.
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