What is the difference between a diamond and graphite?
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.
How are graphite and diamond similar and different?
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 5 differences between diamond and graphite?
Explain the difference in properties of diamond and graphite on the basis of their structures.
| DIAMOND | GRAPHITE |
|---|---|
| 5) It has a rigid covalent bond network which is difficult to break. | 5) It is quite soft and its layers can be separated easily. |
| 6) It acts as an electric insulator. | 6) It is a good conductor of electricity. |
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.
What are 3 differences between diamond and graphite?
(a) Why is graphite a good conductor of electricity but not diamond ?…
| Diamond | Graphite |
|---|---|
| Diamond is the hardest naturally occurring substance. | The graphite is soft and has a greasy touch. |
| Diamond is used in jewelry making, construction and surgery. | Graphite is used in stationary and lubricants. |
What are three differences between diamond and graphite 10?
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. |
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 do diamonds 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.
Why properties of graphite and diamond are different?
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.
What is the reason for the difference in properties between diamond and graphite?
Solution 2 Since diamond exists as a three-dimensional network solid, it is the hardest substance known with high density and high melting point. Whereas in graphite, any two successive layers are held together by weak forces of attraction. This makes graphite soft.
What are the difference between diamond and graphite Class 10?
(a) Write two points of difference in the structures of diamond and graphite….
| DIAMOND | GRAPHITE |
|---|---|
| There is no presence of free carbon atoms in diamonds. | There is presence of free Carbon atoms in graphite. |
| Diamonds do not conduct electricity. | Graphite conducts electricity. |
What are three difference between diamond and graphite?
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. 4) The C-C bond length in the diamond is 154pm.
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.