Diamond and Graphite have 2 different structures, Diamond has a rigid tetrahedral network whereas Graphite has layers which completely changes the properties of both types of carbon.
Basically graphite has free delocalised electrons which means electricity can be conducted, diamond however does not have any delocalised electrons which means it cannot conduct electricity.
Both diamond and graphite are made up of strong covalent bonds which means they both have high melting points. Graphite is soft though because the layers which it is made up of slide, this makes it soft. Diamond is made up of carbon atoms close to each other and in a 3 layered cube shape which is a lot more rigid and this makes it 'the hardest substance on earth'.
Hope this helps, Obrien9
diamond -it has a hard structure and crystals that shine in light and it does not conduct electricity. Graphite -it has sticky structure and has some delocalised electrons so it conducts electricity and has a slippery surface
Three examples of allotropes of carbon are diamond, graphite, and graphene. Diamond consists of a three-dimensional network of carbon atoms, graphite has a layered structure, and graphene is a single layer of carbon atoms arranged in a hexagonal lattice.
Diamond and Graphite are allotropes of Carbon [chemical symbol: C]The chemical symbol of Silicon is Si.
Diamond and graphite are both allotropes of carbon, meaning they are made up of the same element but have different structures. They are similar in that they are both composed of carbon atoms and have high melting points. However, they differ in their physical properties due to their different structures - diamond is the hardest natural substance, while graphite is a good conductor of electricity.
Both diamonds and graphite are allotropes of carbon.
Graphite and diamond are good electricity conductors.
No, carbon in its pure form is not a good conductor of electricity. However, certain forms of carbon like graphene and carbon nanotubes can conduct electricity due to their unique structure and properties.
=>diamond is not conducting electricity and heat. =>it is hardest natural substances known. =>it occurs naturally free state. =>graphite is soft and greasy to touch. =>it doesn't conduct heat an electricity. =>it occurred naturally and manufactured artificially. =>buckminsterfullerene is used in medicines. =>it is used in treatment of cancer.
Graphite and Diamonds are both allotropes of Carbon.
diamond graphite and graphene
Carbon.
No. Both graphite and diamond are allotropes of carbon. They have different molecular structures.
Both diamond and graphite are allotropes of pure carbon.
The three different allotropes of carbon are: -Diamond-Graphite-Buckminsterfullerene
Both diamond and graphite are allotropes of carbon.
they don't conduct electricity: they have no free electrons. graphite, however, made of the same stuff as diamond (carbon) has a different structure, which means that it does have free electrons, and a lot of them. Therefore graphite is a good conductor of electricity.
diamond -it has a hard structure and crystals that shine in light and it does not conduct electricity. Graphite -it has sticky structure and has some delocalised electrons so it conducts electricity and has a slippery surface