How can graphite and diamond be so different?

When you look at graphite and diamond, it is hard to imagine that they are identical chemically, for they are so different physically. Graphite is opaque and metallic- to earthy-looking, while diamonds are transparent and brilliant. Another important physical difference is their hardness.

What are 3 differences between diamond and graphite?

For example, Graphite and diamond are two different allotropes of carbon.

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.

How can graphite and diamond be so different if they are both composed of pure carbon?

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.

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How do diamond and graphite differ in their structure?

Diamond: each carbon atom bonds to 4 other carbon atoms, WHILST, Graphite: each carbon atom bonds to 3 other carbon atoms. Thus, diamond bears more of a tetrahedral structure, whereas graphite takes the form of layers.

What are 5 differences between diamond and graphite?

Difference between diamond and graphite.

The p-Block Elements.

Diamond Graphite
4. It has huge three dimensional network structure. 4. It has two dimensional sheet like structure.
5. It does not possess any lustre 5. It a has metallic lustre.
6. It a has very high melting point. 6. It has low metling point.

What are the similarity and difference between diamond and graphite?

Diamond has a tetrahedral structure and is the hardest material known to man. There are strong covalent bonds between carbon atoms and each carbon atom is bonded to 4 other carbon atoms. Graphite has a hexagonal layered structure and each carbon is bonded via strong covalent bonds to 3 other carbon atoms.

Why do diamond and graphite have different physical properties even though they are both composed entirely of the element carbon?

Why do diamond and graphite have different physical properties, even though they are both composed entirely of the element carbon? … The minerals have different arrangements of carbon atoms.

Why is diamond hard and graphite not note that diamond and graphite are both composed of carbon atoms?

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.

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Why are graphite and diamond so different in their appearance hardness and usage if both minerals have the same composition of carbon?

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).

How does diamond and graphite differ in physical properties Class 10?

In diamond one carbon atom is bonded with four other carbon atoms with strong covalent bond so it is hard while in case of graphite each carbon forms two strong bonds with other two carbon atoms and one weak bond is formed with third carbon atom and forms hexagonal rings which slide over each other so it is soft.

How does diamond and graphite differ in terms of electrical conductivity and hardness?

Graphite, for example, has a melting point of more than 3,600°C. Variable electrical conductivity – diamond does not conduct electricity, whereas graphite contains free electrons so it does conduct electricity. Silicon is a semi-conductor – it is midway between non-conductive and conductive.