Graphite and Diamond are different because they have different structures. Both have Giant Covalent Structures, resulting in very high melting temperatures. However each carbon atom in Diamond has 4 covalent bonds with other Carbons, making it extremely strong and hard.
Do diamond and graphite have the same structure?
Graphite and diamond are two of the most interesting minerals. They are identical chemically – both are composed of carbon (C), but physically, they are very different. Minerals which have the same chemistry but different crystal structures are called polymorphs.
How do the different properties of diamond and graphite depend on their structures?
Since molecules are closely packed they have high density. Because of the large gap between the molecules, they have low density. Since there is no free carbon atom, the diamond does not conduct electricity. Because of the presence of free carbon atom in graphite they can conduct electricity.
Why do diamond and graphite have different properties though they both are made of carbon only explain your answer?
While there are strong covalent bonds between carbon atoms in each layer, there are only weak forces between layers. This allows layers of carbon to slide over each other in graphite. … In this rigid network atoms cannot move. This explains why diamonds are so hard and have such a high melting point.
Why are diamonds more expensive than graphite?
Also, as a result of the rarity, a Diamond is far more expensive than Graphite. … In Diamonds, the atoms are carefully packed with together with each atom connected to various other carbon atoms as compared to Graphite where the bonds in between the layers are weak.
Which is harder graphite or diamond?
We also all know that carbon is present in both diamond and graphite. Diamond is harder than graphite because each of its carbon atoms form four covalent bonds in a tetrahedral structure and also due to the presence of strong covalent bonds in it.
What are 3 differences between diamond and graphite?
2) It has a planar geometry. 3) In diamond, each carbon atom is sp3 hybridized and is bonded to four other carbon atoms through a sigma bond. 3) In graphite, each carbon atom is sp2 hybridized and is bonded to three other carbon atoms through a sigma bond while the fourth electron forms a Π-bond.
Why is graphite softer than diamond?
This means that each carbon atom has a ‘spare’ electron (as carbon has four outer electrons) which is delocalised between layers of carbon atoms. These layers can slide over each other, so graphite is much softer than diamond. … This conductivity makes graphite useful as electrodes for electrolysis .
What is graphite and diamond structure?
Structure and bonding
each carbon atom is joined to three other carbon atoms by covalent bonds. the carbon atoms form layers with a hexagonal arrangement of atoms.
What’s harder than diamond?
Moissanite, a naturally occurring silicon-carbide, is almost as hard as diamond. It is a rare mineral, discovered by the French chemist Henri Moissan in 1893 while examining rock samples from a meteor crater located in Canyon Diablo, Arizona. Hexagonal boron-nitride is 18% harder than diamond.
Why is diamond a poor conductor of electricity?
In a graphite molecule, one valence electron of each carbon atom remains free, Thus making graphite a good conductor of electricity. Whereas in diamond, they have no free mobile electron. Hence there won’t be flow of electrons That is the reason behind diamond are bad conductor electricity.
What is the relationship between diamond and graphite?
Diamond and graphite are both allotropes of carbon. Allotropes are basically different forms of the same element. The only difference is the structure and arrangement of how the carbon atoms are oriented.
Why are pencils so cheap?
Because the graphite core (commonly called “lead”, though it contains no lead at all) is not high-grade pure graphite, it is very inexpensive.
Can you turn graphite into diamond?
Graphite and diamond are two forms of the same chemical element, carbon. … One way to turn graphite into diamond is by applying pressure. However, since graphite is the most stable form of carbon under normal conditions, it takes approximately 150,000 times the atmospheric pressure at the Earth’s surface to do so.
How much is graphite worth?
Prices for graphite globally by flake grade 2011-2020
In 2016, the price for large graphite flakes is expected to reach 996 U.S. dollars per metric ton. Until 2020, the price for this flake grade was expected to increase to 1,165 dollars per metric ton. Graphite prices depend on two factors – flake size and purity.