“Metals conduct electricity as they have free electrons that act as charge carriers. If the bonds were not equidistant, the electron would be bound to the two atoms with the shortest bond length. Thats why diamond are bad conductor electricity. Why does graphite conduct electricity? It displays properties of both metals, and nonmetals. As we know carbon has four valence electrons, and one remaining electron of carbon is delocalized and move to free across the lattice to conduct electricity. Yes, graphite can conduct electricity in liquid state. “Metals conduct electricity as they have free electrons that act as charge carriers. It’s one of the most commonly used materials on the planet – found in everything from pencils to nuclear reactors – but why does graphite conduct electricity? In graphite, the carbon atoms are joined together and arranged in layers. Graphite forms multiple layers of hexagonal planar carbon atoms attached to it. It’s one of the most commonly used materials on the planet – found in everything from pencils to nuclear reactors – but why does graphite conduct electricity? Science journals have been running out of superlatives for this wondrous stuff: it's just about the lightest, strongest, thinnest, best heat- and electricity- conducting material ever discovered. Graphite forms layers of a hexagonal arrangement of atoms and each carbon atom form a covalent bond with three other carbon atoms, and therefore each carbon atom has one non-bonded electron which becomes delocalized and responsible for conducting electricity. In diamond the bonds are sp and the atoms form tetrahedra with each bound to four nearest neighbors. It is chemically specified as a native element. The specific gravity of this element is found around 2.1 to 2.3. This is also true if you remove the light bulb. So guys, if you have any questions, you can leave a question in the comment section. Graphite has delocalised electrons, just like metals. graphite can conduct electricity when molten because of the free … Graphite can conduct electricity due to the vast electron delocalization (delocalized electrons are electrons in a molecule, ion or solid metal that are not associated with a single atom or one covalent bond) within the carbon layers (a phenomenon called aromaticity).These valence electrons are free to move, so are able to conduct electricity. And similarly, these series keep on in continuous form forming a planar hexagonal structure. Comments (1) Report plz mark as brainliest Log in to add a comment Suhaniv Ambitious; Yes! Graphite can conduct electricity due to the vast electron delocalization (delocalized electrons are electrons in a molecule, ion or solid metal that are not associated with a single atom or one covalent bond) within the carbon layers (a phenomenon called aromaticity). If we talk about the lattice structure of diamond, carbon atoms form a three-dimensional network resulting in a tetrahedral structure. Just look at the below image for better understanding of the structure of graphite. As mentioned before, graphite is composed of layers of carbon atoms, and this single layer of carbon atoms is actually what we often hear about "graphene". Save my name, email, and website in this browser for the next time I comment. Graphite conducts electricity because it possesses delocalized electrons in its structure. The calculated resistivity of pure graphite is calculated as 1.38 * 10^-5 µΩ/m. It is a mineral of carbon that is formed under high pressure and temperature in the earth’s crust. And these layers are loosely connected to each other. The fourth electron between the layers is delocalised. Here's everything you need to know about graphite. Required fields are marked *. Watch Queue Queue The density of this element is around 2.2 gm/cm3. Although diamond is also an allotrope of carbon, it does not conduct electricity because the four electrons of each carbon atom are localized in pure covalent bonds with the four nearest neighboring atoms. Graphite is structured into planes with tightly bound atoms. Each carbon atom is connected to its adjacent three carbon atoms. HCl Lewis Structure, Molecular Geometry, and Hybridization, CH2O Lewis Structure, Molecular Geometry, and Hybridization, PCl5 Lewis Structure, Molecular Geometry, Hybridization, and MO Diagram. Whereas in diamond, they have no free mobile electron. In the automobile industry, it is used in brake linings and brake shoes. It will also not burn out when you place a light bulb between the graphite and the source of … The graphite acts as a path for the electrical energy. The important factor responsible for the electrical conductivity of an element is the presence of mobile electrons that move across it to flow the electric current. Last updated Oct 24 2016. Graphite is a good conductor of electricity because its electrons are delocalized or free to move around. The elements that have delocalized electrons can conduct electricity and the type of conductor depends on the ease of electrons to flow across. Graphite can conduct electricity because of the delocalised (free) electrons in its structure. This video is unavailable. Each of these electrons is free to move within the structure, enabling electrical conduction. These valence electrons are free to move, so are able to conduct electricity. Explain why graphite conduct electricity but silicon carbide does not. So diamond has the spacial structure and it is very hard and does not conduct electricity. Graphite conducts electricity due to the ‘spare’ electrons being delocalised between the layers. I f the 20th century was the age of plastics, the 21st century seems set to become the age of graphene —a recently discovered material made from honeycomb sheets of carbon just one atom thick. The molecular geometry of the graphite molecule is a trigonal planar. C60 and graphene are also forms of carbon that possess this electron delocalization. The µΩ/m is referred to as ohms per meter. Yes, graphite is a very good conductor of electricity because of delocalized electrons. It has a pretty high melting point of around 3600°C or 3873.15 Kelvin. So, does graphite conduct electricity? However graphite and diamond both are allotropes of carbon having the same composition but different structures. However, in diamond, all 4 outer electrons on each carbon atom are used in covalent bonding, so there are no delocalised electrons. Yes, graphite is a very good conductor of electricity because of delocalized electrons. These layers are connected by weak van der Waals forces. This conductivity makes graphite useful as electrodes for electrolysis. How does graphite conduct electricity? It in-fact does conduct electricity, molten graphite is a key element in which terrorists use for I.E.D'S it causes a large heat blast when heated with electricity and mixed with different compounds. The most common example is Copper. Answer: the very reason why metals do. Is graphite a good conductor of electricity? Graphite is an interesting material, an allotrope of carbon (as is diamond). . star_gazer 19 year member 5236 replies Answer has 9 … Graphite is used in the manufacturing of pencil lead since the 16th century. It’s one of the most commonly used materials on the planet – … The distance between these layers is around 3.35Ao. Look at the periodic table: graphite is carbon, and carbon is the same group as silicon and germanium, natural semiconductors. The hexagonal rings having carbon atoms connected have the bond length of around 1.42Ao. The U.S. Supreme Court: Who Are the Nine Justices on the Bench Today. Question #114085. 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. So, In this article, I will answer this question and cover the surrounding topics too. The two most common are diamond and graphite (less common ones include buckminsterfullerene). Graphite has properties of both metal and non-metal which make it an interesting element. Graphite carries the properties of metal and non-metal as well that make it a unique element. Thanks 1. They are both soft and malleable, and can conduct electricity. Why does graphite conduct electricity but silicon carbide does not? So, does graphite conduct electricity? Graphite is a layer compound, each layer has fused hexagons of carbon with delocalistion of electrons across the layer (p orbitals). It has an opaque surface and metallic luster. If we talk about the structure of Graphite, the carbon atoms are connected to each other in a hexagonal trend. Free electrons are carriers of electric current. When the battery is placed on the graphite, energy flows from the battery, along the graphite path, through the wires on the light bulb, continuing back to the battery completing the circuit. Graphite can withstand the heat generated by electricity running through its atoms. Why is Graphite Slippery / Used as a lubricant. And on applying a potential difference across graphite, the electric current flows through it. In other hand, carbon atoms in graphite has only 3 bonds and the 3 bonds are in a plane because it is the sp2 hybrid. Can graphite conduct electricity? Diamond and graphite that are allotropes of carbon but differ largely in term of electrical conductivity because diamond does not have delocalized electron responsible for conducting electricity. Graphite and Diamond both are allotropes of Carbon, yet diamond is a bad electrical conductor and graphite is a good conductor of electricity. The honeycomb layout of the stacked carbon atoms of graphite leaves a single electron unbound in each hexagon. And why doesn't diamond do the same? Graphite is a good conductor whereas diamond is an insulator. These electrons are free to move between the layers in graphite, so graphite can conduct electricity. It is a free electron and these free electrons between the layers allows graphite to conduct electricity … (a) In a graphite molecule, one valence electron of each carbon atom remains free, Thus making graphite a good conductor of electricity. Graphite is actually a carbon structure. Graphite is an electrical conductor, hence useful in such applications as arc lamp electrodes. It is used in the electronic industries like in making batteries. Rate! It is also widely used as a lubricant in industrial processes. 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