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Graphite has delocalised electrons, just like metals. This makes graphite useful for electrodes in batteries and for electrolysis. This means that it is donated to form a common pool of electrons which can flow through the molecule carrying charge and so conducting electricity. The delocalised electrons are free to move through the structure, so graphite can conduct electricity. This delocalised electron is no longer associated with one particular carbon atom and it is able to move freely between the carbon layers of graphite and conduct electricity.Diamond and graphite are both allotropes of carbon; they are both made entirely of the same element (carbon) but they differ in the way that the atoms bond with each other and arrange themselves in a structure.Each carbon atom has 4 electrons in its outer shell that it can share with other atoms in order to form 4 covalent bonds. Have a Free Meeting with one of our hand picked tutors from the UK’s top universitiesGraphite on the other hand, although also only made up of carbon atoms, is the only non-metal that can conduct electricity. Graphite is used as lubricant in machines, which have to be operated at high temperatures, because oil or grease vaporizes immediately at high temperatures. Since electrical conductivity relies on the flow of free electrons, diamond is not a good conductor. Graphite conducts electricity due to the ‘spare’ electrons being delocalised between the layers. Have a Free Meeting with one of our hand picked tutors from the UK’s top universitiesHowever in graphite each carbon atom only bonds to 3 others around it- this means there is an electron spare which becomes 'delocalised'.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).Graphite is a mineral whose molecular structure is made up of carbon atoms.This means that it is donated to form a common pool of electrons which can flow through the molecule carrying charge and so conducting electricity. Diamond is a giant covalent structure; each valence electron (outer shell electron) of every carbon atom forms a covalent bond, which means that there are no free electrons. This is because only 3 of the available valence electrons form covalent bonds leaving 1 spare electron, which then becomes delocalised. This delocalised electron is no longer associated with one particular carbon atom and it is able to move freely between the carbon layers of graphite and conduct electricity. This is because only 3 of the available valence electrons form covalent bonds leaving 1 spare electron, which then becomes delocalised. These electrons are free to move between the layers in graphite, so graphite can conduct electricity. Materials that conduct heat very well also conduct electricity well, because both processes transport energy using electrons. This is where graphene starts to get really interesting! Like graphite, graphene conducts electricity well because it has delocalised electrons that are free to move across its surface. However in graphite each carbon atom only bonds to 3 others around it- this means there is an electron spare which becomes 'delocalised'. Graphite conducts electricity because it is only bonded 3x (meaning there is a delocalised electron to pass the charge) Explain why ionic compounds have a giant structure Ionic compounds have giant structures because the ions keep their charge and attract up to 6 other ions - forming a giant lattice 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.
Graphite has delocalised electrons, just like metals. This makes graphite useful for electrodes in batteries and for electrolysis. This means that it is donated to form a common pool of electrons which can flow through the molecule carrying charge and so conducting electricity. The delocalised electrons are free to move through the structure, so graphite can conduct electricity. This delocalised electron is no longer associated with one particular carbon atom and it is able to move freely between the carbon layers of graphite and conduct electricity.Diamond and graphite are both allotropes of carbon; they are both made entirely of the same element (carbon) but they differ in the way that the atoms bond with each other and arrange themselves in a structure.Each carbon atom has 4 electrons in its outer shell that it can share with other atoms in order to form 4 covalent bonds. Have a Free Meeting with one of our hand picked tutors from the UK’s top universitiesGraphite on the other hand, although also only made up of carbon atoms, is the only non-metal that can conduct electricity. Graphite is used as lubricant in machines, which have to be operated at high temperatures, because oil or grease vaporizes immediately at high temperatures. Since electrical conductivity relies on the flow of free electrons, diamond is not a good conductor. Graphite conducts electricity due to the ‘spare’ electrons being delocalised between the layers. Have a Free Meeting with one of our hand picked tutors from the UK’s top universitiesHowever in graphite each carbon atom only bonds to 3 others around it- this means there is an electron spare which becomes 'delocalised'.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).Graphite is a mineral whose molecular structure is made up of carbon atoms.This means that it is donated to form a common pool of electrons which can flow through the molecule carrying charge and so conducting electricity. Diamond is a giant covalent structure; each valence electron (outer shell electron) of every carbon atom forms a covalent bond, which means that there are no free electrons. This is because only 3 of the available valence electrons form covalent bonds leaving 1 spare electron, which then becomes delocalised. This delocalised electron is no longer associated with one particular carbon atom and it is able to move freely between the carbon layers of graphite and conduct electricity. This is because only 3 of the available valence electrons form covalent bonds leaving 1 spare electron, which then becomes delocalised. These electrons are free to move between the layers in graphite, so graphite can conduct electricity. Materials that conduct heat very well also conduct electricity well, because both processes transport energy using electrons. This is where graphene starts to get really interesting! Like graphite, graphene conducts electricity well because it has delocalised electrons that are free to move across its surface. However in graphite each carbon atom only bonds to 3 others around it- this means there is an electron spare which becomes 'delocalised'. Graphite conducts electricity because it is only bonded 3x (meaning there is a delocalised electron to pass the charge) Explain why ionic compounds have a giant structure Ionic compounds have giant structures because the ions keep their charge and attract up to 6 other ions - forming a giant lattice 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.