Graphite and diamond form a polymorphous mineral series which have identical chemical composition but different structures or shapes. The reason minerals with identical chemical composition can form different structures is due to the physical conditions, in particular temperature and pressure under which they formed.
Graphite has a sheet structure horizontally with weak vertical bonds joining the horizontal sheets. This produces a weak unstable structure. Diamonds on the other hand have a very different structure and form a octahedron structure which is much more compact and denser structure and a much more stable compound which is the result of the extreme pressure during its formation.
Diamond and graphite both are allotropes of carbon. The carbon atoms in both are bonded
to each other by sharing electrons. Diamond is 100% carbon and graphite is 95-97% carbon.
In diamond each carbon atom is bonded to its four adjacent carbon atoms whereas in
graphite each carbon atom is bonded to its three adjacent carbon atoms.
Well, diamonds and graphite are only made of carbon atoms if that helps.
Both of these compounds are made out of the same element, carbon. Both of these compounds are composed of covalent bonds. And they have similar boiling points.
Diamond has a greater density than graphite.
One of them might be denser
Diamond
Graphite is made of pure carbon atoms. The bond between the C atoms is called a covalent bond.
single covalent bond between each carbon.
In graphite which consists of fused hexagons of carbon atoms arranged in sheets there is considerable delocalisation of electrons. In diamond the structure is "3 dimensional" with each atom of carbon tetrahedrally surronded by 4 other carbon atoms. The bonding is covalent and the electrons in each bond are localised.
Different arrangements in allotropes like coal, graphite, diamond or buckmisterfullerenes. Also, the arrangement varies across different compounds containing carbons: cyclic and acyclic hydrocarbons, for example.
No, diamond, an allotrope of carbon, does not have a metallic bond. Carbon, which is the element from which diamond is formed, is a nonmetal.
Yes, it can bond with other cabons . For example, a diamond, graphite (in pencils) and charcoal.
Graphite is made of pure carbon atoms. The bond between the C atoms is called a covalent bond.
Graphite is made of pure carbon atoms. The bond between the C atoms is called a covalent bond.
They have different structures.They are both made up of Carbon (diamond has more Carbon atoms though) but the reason that graphite and diamond are so different in shape, hardness, etc, is due to how it is structured.The carbon atoms themselves are identical, the inter-atom bonding is different.Graphite - carbon atoms bond in flat hexagons that tessellate flat sheets.Diamond - carbon atoms bond in cubes that form a cubic crystal solid.
single covalent bond between each carbon.
In graphite which consists of fused hexagons of carbon atoms arranged in sheets there is considerable delocalisation of electrons. In diamond the structure is "3 dimensional" with each atom of carbon tetrahedrally surronded by 4 other carbon atoms. The bonding is covalent and the electrons in each bond are localised.
Graphite is made of pure carbon atoms. The bond between the C atoms is called a covalent bond.
graphite
Different arrangements in allotropes like coal, graphite, diamond or buckmisterfullerenes. Also, the arrangement varies across different compounds containing carbons: cyclic and acyclic hydrocarbons, for example.
No, diamond, an allotrope of carbon, does not have a metallic bond. Carbon, which is the element from which diamond is formed, is a nonmetal.
Graphite, diamonds, Lonsdaleite, C60 (Buckminsterfullerene), C540 Fullerene, C70 Fullerene, Amorphous carbon, and Single-walled carbon nanotube are all solid allotropes of carbon. Allotropes are different structural forms of the same element.
: Diamond is made up of pure carbon. In the structure of diamond one carbon atom is attached to four other carbon atoms forming a covalent bond. All the electrons of each carbon atom is shared and the octet rule is satisfied. Hence no free electron is left for the conductance of electricity. : In case of graphite the carbon atoms naturally combine covalently with three other carbon atoms so every combined carbon has one unshared or free electron. Now this free electron is responsible for conductance in graphite. : Graphite and metals have free electrons to conduct electricity.