These electrons are free to move between the layers in graphite, so graphite can conduct electricity. There is a great deal of distance between planes, and they are bonded weakly together, allowing the electrons to move around.
These valence electrons are free to …

Question #114085.

Why does graphite conduct electricity while diamond does not even if both of them are forms of carbon? Graphite is a good conductor of electricity because its electrons are delocalized or free to move around. Graphite is a mineral whose molecular structure is made up of carbon atoms.


This makes graphite useful for electrodes in batteries and for … The honeycomb layout of the stacked carbon atoms of graphite leaves a single electron unbound in each hexagon. Last updated Oct 24 2016. The resistance also plays an important role in determining the type of conductor. In graphite, one of the outer electrons of the carbon atom is not involved in the crystal bonding of the solid. Vote for this answer . Because of its ability to conduct electricity and withstand heat, graphite is used in making electrodes, as lubricant for machines, and in nuclear reactors to absorb neutrons. Uses of Graphite. Originally posted Apr 13 2010 4:43 AM. How does graphite conduct electricity? Graphite can conduct electricity because of the delocalised (free) electrons in its structure. In graphite, the carbon atom is connected to three adjacent carbon atoms due to which one electron remains free which is responsible for conducting electricity. Graphite is structured into planes with tightly bound atoms. Graphite can conduct electricity due to the vast electron delocalization within the carbon layers (a phenomenon called aromaticity). Because the structure of the metal and its free valence electrons has a lot to do with how well it conducts electricity, some metals are better than it than others. star_gazer 18 year member 5236 replies Answer has 9 votes.

star_gazer Answer has 9 votes Currently Best Answer. Why Graphite Conduct Electricity? Graphite on the other hand, although also only made up of carbon atoms, is the only non-metal that can conduct electricity.

Graphite conducts electricity because it possesses delocalized electrons in its structure.

Graphite is a good conductor of electricity because it contains delocalized electrons which are carriers of electrical current. Asked by prince1239. This is because only 3 of the available valence electrons form covalent bonds leaving 1 spare electron, which then becomes delocalised. In Graphite, due to the presence of a delocalized electron of a carbon atom, it can move freely across it. A carbon atom can bind up to 4 other atoms around it (it has 4 electrons in its outer-most shell which it can share with other atoms to form bonds). Currently voted the best answer. Why Diamond is not a good conductor of electricity? Unlike oil or grease, graphite is stable and can withstand … Graphite is used as lubricant in machines, which have to be operated at high temperatures, because oil or grease vaporizes immediately at high temperatures. While nearly all metals and graphite can conduct electricity, some have a better atomical structure for doing so. The structure of graphite is very unlike any other substances.

Each of these electrons is free to move within the structure, enabling electrical conduction. And on applying a potential difference across graphite, the electric current flows through it. However, in diamond, all 4 outer electrons on each carbon atom are used in covalent bonding, so there are no delocalised electrons.

That electron is somewhat free to move, and graphite therefore can conduct an electrical current, but it conducts much more poorly than metals. Why can graphite conduct electricity?


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