Why graphite is chemically reactive than diamond?

Density: Graphite’s specific gravity is 2.3, which makes it lighter than diamond. Chemical activity: it is slightly more reactive than diamond. This is because the reactants are able to penetrate between the hexagonal layers of carbon atoms in graphite.

Why are diamonds not reactive?

It does not conduct electricity. Every atom in a diamond is bonded to its neighbours by four strong covalent bonds, leaving no free electrons and no ions .

Is graphite chemically different from diamond?

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.

Why is graphite stronger than diamond?

The sheets of carbon become bonded by weaker intermolecular forces. It is because of these weak intermolecular forces that the layersof graphite can slide over eachother, making the overall substance a lot weaker than diamond.

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Which graphite is more reactive?

Carbon and its compounds | Exercise

Q6) With reference to the structure of the two crystalline allotropes of carbon, state why diamond is inert or unreactive while graphite is comparably more reactive. … Graphite has an open structure which makes it more prone to chemical attack.

Do diamonds decay into graphite?

Diamonds degrade to graphite, because graphite is a lower-energy configuration under typical conditions. … The degradation of diamond to graphite is a simple case of the atoms internally rearranging and relaxing to a lower energy state. This process requires no chemical reaction with an external material.

Is Liquid diamond possible?

Can diamond be in a liquid state? – Quora. No, diamond is a crystalline form of carbon, diamonds can melt at high temperature (3000–5000 kelvin depending on pressure) they are then no longer diamonds but liquid carbon. The liquid carbon must be kept well away from oxygen of course.

Why is diamond different from graphite?

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. On the other hand, each carbon in graphite is bonded to three carbons, and therefore graphite is formed in layers.

What are the main two difference between graphite and diamond?

Explain the difference in properties of diamond and graphite on the basis of their structures.

DIAMOND GRAPHITE
1) It has a crystalline structure. 1) It has a layered structure.
2) It is made up of tetrahedral units. 2) It has a planar geometry.
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Why do diamond and graphite differ in their properties?

The differing properties of carbon and diamond arise from their distinct crystal structures. In a diamond, the carbon atoms are arranged tetrahedrally. … This accounts for diamond’s hardness, extraordinary strength and durability and gives diamond a higher density than graphite (3.514 grams per cubic centimeter).

Why is graphite weaker than diamond?

Graphite. Graphite is a form of carbon in which the carbon atoms form covalent bonds with three other carbon atoms. … These layers can slide over each other, so graphite is much softer than diamond.

Why does graphite have weak intermolecular forces?

Each carbon atom in graphite is bonded to three other carbon atoms. These carbon atoms are linked by covalent bonds – which are very strong. Graphite is arranged in sheet like structures and between each layer there are Van der Waals intermolecular forces which are weak in comparison to the covalent bonds.

Why is graphite an electrical conductor but diamond is not?

Graphite can conduct electricity because of the delocalised (free) electrons in its structure. These arise because each carbon atom is only bonded to 3 other carbon atoms. … However, in diamond, all 4 outer electrons on each carbon atom are used in covalent bonding, so there are no delocalised electrons.

Are Diamonds highly reactive?

1. Diamond is unreactive while graphite is highly reactive in comparison to it. … In diamond each carbon has sp3 hybridisation and no free electrons are present.

Are Diamonds reactive?

Chemical stability

At room temperature, diamonds do not react with any chemical reagents including strong acids and bases.

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Which is the most reactive allotrope of phosphorus?

White phosphorus is most reactive of all the allotropes of phosphorus because it is unstable due to the angular strain on P4 molecule with the bond angle of 60°.