What is the difference between graphite and a diamond?
Diamond and graphite are allotropes of carbon. These have different chemical and physical properties. The main difference between diamond and graphite is that diamond is made out of sp3 hybridized carbon atoms whereas graphite is made out of sp2 hybridized carbon atoms.
What are the main two difference between graphite and diamond?
| Diamond | Graphite |
|---|---|
| Diamond is formed by tetrahedral units in which each carbon atom is sp3 hybridized. | Graphite has a planner geometry in which each carbon atom is sp2 hybridized by forming three sigma and one π−bond. |
| Diamond is an insulator of electricity. | Graphite is a good conductor of electricity. |
What is the difference in bonding between diamond and graphite?
Differences 1. 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. The presence of layers means that atoms can slide over each other easily.
Why do graphite and diamond have different properties?
The way the carbon atoms are arranged in space, however, is different for the three materials, making them allotropes of carbon. The differing properties of carbon and diamond arise from their distinct crystal structures.
Why do diamond and graphite have different hardness?
Rotate the Graphite molecule This allows layers of carbon to slide over each other in graphite. On the other hand, in diamond each carbon atom is the same distance to each of its neighboring carbon atoms. In this rigid network atoms cannot move. This explains why diamonds are so hard and have such a high melting point.
How do diamond and graphite differ in their structure Class 10?
But they differ in their structures. In diamond, all the four valence electrons of carbon atom are involved in the covalent bond formation with the electrons of neighbouring carbon atoms. In graphite, only three electrons participate in the bond formation while the fourth electron is free.
Why diamond and graphite has different physical properties?
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.
Why do graphite and diamond show different properties?
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.