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.
Some differences between diamond and graphite:
- different crystalline lattice
- different aspect
- graphite is a good electrical conductor, graphite not
- diamond has a very good thermal conductivity
- the density of diamond is approx. 3,5 g/cm2 and the density of graphite is 2,15+/- 0,o7 g/cm2
- the Mohs hardness of diamond is 10; the Mohs hardness of graphite is between 1 and 2
Diamonds are formed at much higher pressure deep inside the Earth.
Diamond and graphite are different structural forms of carbon.
The difference is simple; they have different atomic structures, or their atoms are arranged differently.
Yes. Diamond is isometric, graphite is hexagonal.
what is graphite
Elemental minerals and regular minerals have properties like hardness due to their atomic arrangement and crystalline structures. Graphite, for instance, is composed of the same element (carbon) as diamond is. The difference lies in the arrangement of the carbon atoms.
A polymorph is defined as same composition, different chemical structures. Quartz, cristobalite, and tridymite are examples of polymorph because they are three different minerals with the same chemical composition. Graphite and diamond are also good examples of polymorphism. They both contain carbon atoms, but they have extremely different properties because of the condition in which they formed. Diamond forms where extreme pressures and temperatures produce its compact structure. On the other hand, graphite forms under comparatively low pressures and it has weekly bonded carbon sheets that create its greasy feel. The difference in conditions makes diamond much harder than graphite and graphite much more useful as a lubricant.
Yes, carbon.supplement. when an element exists in two or more forms, these forms are known as an allotrope. Carbon has three allotropes, graphite, diamond, and ordinary carbon.
graphite has hexagonal crystals and diamond tetrahedron
difference between diamond graphite and fullrene
Diamonds are very hard, and graphite is very soft.
There is none, diamond has about 60 bonds of graphite inside of it.
This explanation is not correct.
Diamond and graphite have different structures which account for their different properties. Graphite is arranged into sheets which are easily removed. Diamond, on the other hand, is a network solid that has very strong bonds and intermolecular forces holding it together.
Diamond and graphite are both pure carbon but graphite's atoms attach to three other carbon atoms and are connected in plates that are parallel to eachother. Diamond's atoms attach to four other carbon atoms in a crystal form, and graphite is a lot softer than diamond.
The crystalline structure of graphite and diamond are the cause of these properties.
Yes, diamond and graphite are isotopes of carbon as they are both entirely made of carbon. However they have very different structures resulting in their different properties.
carbon rod, graphite, diamond.
there are no elements which show exact properties but... 1) Luster : Graphite and iodine 2) Liquid metals : Bromine, Mercury 3) Thermal conductivity : Diamond 4) Electric " " : Graphite 5) Non metals which are hard : Graphite and Diamond
Diamond and graphite are allot-ropes of each other. Diamond has a tetrahedral structure where as graphite has an hexagonal arrangement. Both are made of carbon atoms entirely. Diamond is used in jewelry etc. where as graphite is used as in batteries , lubricants etc.