Why does graphite conduct electricity

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.

Diamond Structure and bonding Diamond is a giant covalent structure in which: each carbon atom is joined to four other carbon atoms by strong covalent bonds the carbon atoms form a regular tetrahedral network structure there are no free electrons Carbon atoms in diamond form a tetrahedral arrangement Properties and uses The rigid network of carbon atoms, held together by strong covalent bonds, makes diamond very hard.

Graphite Structure and bonding Graphite has a giant covalent structure in which: each carbon atom forms three covalent bonds with other carbon atoms the carbon atoms form layers of hexagonal rings there are no covalent bonds between the layers there is one non-bonded - or delocalised - electron from each atom Dotted lines represent the weak forces between the layers in graphite Properties and uses Graphite has delocalised electrons, just like metals.

Question Explain why diamond does not conduct electricity and why graphite does conduct electricity. 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. Nagwa uses cookies to ensure you get the best experience on our website.

Learn more about our Privacy Policy. In short: graphite trumps diamond. Her current research focuses on building materials to be used in the safe operation of nuclear reactors. Writing about everything from cosmology to anthropology, he specialises in the latest psychology and neuroscience discoveries.

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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. Why does Diamond not conduct electricity? The geometrical structure of Graphite If we talk about the structure of Graphite, the carbon atoms are connected to each other in a hexagonal trend. The hexagonal rings having carbon atoms connected have the bond length of around 1.

These layers can also slide over each other due to which graphite becomes slippery. The crystal class of graphite is classified as Dihexagonal dipyramidal. Just look at the below image for better understanding of the structure of graphite Physical properties of Graphite Graphite has a grayish-black appearance and is a soft slippery element.

The boiling point of graphite is calculated as around degrees Celcius or Kelvin. Graphite is insoluble in water or any other solvents because of the strong bond within the graphite element however soluble in warm chlorosulfuric acid and molten nickel. Graphite is a very good conductor of electricity because of the presence of the delocalized electron. The density of this element is around 2. It has an opaque surface and metallic luster.

It has its density lower than that of diamond due to extra space present between layers in graphite. Chemical properties of Graphite The hybridization of graphite is sp2 s orbital combines with p-orbitals.

The bond angle formed between the carbon atoms is degrees. The molecular geometry of the graphite molecule is a trigonal planar. The specific gravity of this element is found around 2.