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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.
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What type of bond does diamond graphite and buckminsterfullerene have - Single Double or Triple?
Diamond and Graphite both have single covalent bonds whereas Buckminsterfullerene has double covalent bonds.
Calculate c-c bond length in Graphite?
The carbon-carbon bond length in graphite is around 1.42 Å (angstroms), which is shorter than the typical C-C single bond length of about 1.54 Å. This shorter bond length in graphite is due to the strong delocalization of electrons in the hexagonal layers of carbon atoms.
What type of bonding is graphite?
Graphite consists of covalent bonding within the layers of carbon atoms, while the layers are held together by weak van der Waals forces.
Why does carbon graphite conduct electricity and carbon diamond doesn't?
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.
What are 3 forms of carbon?
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.
Can carbon bond with other carbons?
Yes, it can bond with other cabons . For example, a diamond, graphite (in pencils) and charcoal.
What type of bonding graphite?
Graphite is made of pure carbon atoms. The bond between the C atoms is called a covalent bond.
What type of bond does diamond graphite and buckminsterfullerene have - Single Double or Triple?
Diamond and Graphite both have single covalent bonds whereas Buckminsterfullerene has double covalent bonds.
Calculate c-c bond length in Graphite?
The carbon-carbon bond length in graphite is around 1.42 Å (angstroms), which is shorter than the typical C-C single bond length of about 1.54 Å. This shorter bond length in graphite is due to the strong delocalization of electrons in the hexagonal layers of carbon atoms.
The carbon atoms in graphite and the carbon atoms in diamond have different?
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.
What type of bonding is OF?
Graphite is made of pure carbon atoms. The bond between the C atoms is called a covalent bond.
Which carbon allotrope have double bond?
graphite
What type of bonding is graphite?
Graphite consists of covalent bonding within the layers of carbon atoms, while the layers are held together by weak van der Waals forces.
Why does carbon graphite conduct electricity and carbon diamond doesn't?
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.
Differnce between diamond and graphite?
diamonds form a 3 dimensional latice. they also have have four bonds per atom. This makes a very strong material. graphite forms a 2 dimensional latice. it has 3 bonds per atoms (the fourth bond is added to the other three making partial double bonds). it forms sheets. it has excellent 2-d strength: it is what is used in carbon fibers. it also is an excellent lubricant because the sheets slide on one another. fullerenes are like graphite, but the small sheets are wrapped up into small balls or tubes. this gives them 3 d strength on a nano scale. But they lack large scale 3d properties
Why diamond does not conduct electricity but graphite does.?
Both diamond and graphite are bonded covalently and most covalent substances will not conduct electricity. Diamond contains entirely carbon-carbon single bonds and so the electrons basically stay between two atoms. Graphite is sometime represented as having alternate signal and double bond but this is not quite accurate. There are no definite single and double bonds but rather bonds that are in between. This property is called resonance. Because of this resonance the electrons are delocalized; they are not tied down to any pair of atoms and are free to move thought the structure.
How can diamond and graphite be made out of same substance and be so different?
They are so different because of the way the carbon atoms bond to each other. Graphite has layers of very strong bonds, but the layers are very weakly bonded to each other. Diamonds are so strong because all of its carbon atoms are uniformly bonded to one another.
