What is the difference between carbon graphite and graphite?
because carbon graphite had carbon but graphite does not have carbon
Graphite and diamond are allotropes of carbon. In other words they're both carbon in different "forms" this difference is represented in thevaryingstructures of the atoms. Specifically, graphite is aspecific structure (layers of atoms) and diamond is formed by face-centered cubic crystals disposed in a diamond type lattice.
Graphite and diamonds are both network covalent carbon chains. The only difference is the structure of each. Graphite is very soft and is used as a lubricant, due to the fact that its carbon atoms are bonded together in layers which slide apart easily. Diamond, however, is very abrasive, because its carbons are all bonded to each other in a very rigid fashion.
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.
actually graphite , diamond, fullerene are allotrope of carbon. so they are made of the same atom. but the difference is that the bond between atoms is different for diamond ,graphite .etc. for example in graphite, atoms are arranged in a flat manner,in diamond it is a cone model, in buckminsterfullerene it is sphere shaped.
Both graphite and diamonds are both made up of carbon and their chemistry is one of the most important similarities that they have. Due to the fact that these minerals are highly solid and have a high melting point makes it very difficult to burn. Even though both of these minerals are chemically the same in composition, they are different in physical form and in other aspects. Even a non- expert can tell the difference…
The difference between graphite and diamond is in the three-dimensional arrangement of the carbon atoms in the material. Graphite is made of flat sheets of carbon atoms in a hexagonal arrangement. The sheets stack one over the other, with only weak interactions between sheets. Diamond is not arranged in sheets; instead, each carbon atom is connected to four others in a tetrahedral arrangement. It turns out that this arrangement is not as different from the…