Table of Contents
- 1 Why does graphite conducts electricity but not diamond Class 10?
- 2 Why is diamond not electrically conductive?
- 3 What are the difference between diamond and graphite?
- 4 Why is graphite The only non-metal that conducts electricity?
- 5 Why diamond is a non conductor and graphite is fairly a good conductor?
- 6 What is the relationship between graphite and diamond?
- 7 What makes a diamond different from a graphite?
- 8 How are electrons used to conduct electricity in graphite?
Why does graphite conducts electricity but not diamond Class 10?
Answer: It is because of free electron in graphite. Explanation: Graphite is a good conductor of electricity as each carbon atom is linked to three of its neighbouring carbon atoms. But diamond do not contain any free electon and all electrons are covalently bonded.
Why is diamond not electrically conductive?
Diamond is a form of carbon in which each carbon atom is joined to four other carbon atoms, forming a giant covalent structure. It does not conduct electricity as there are no delocalised electrons in the structure.
Why does graphite can conduct electricity?
Graphite has delocalised electrons, just like metals. These electrons are free to move between the layers in graphite, so graphite can conduct electricity. The forces between the layers in graphite are weak.
Why is graphite a good conductor of electricity but diamond is non conductor of electricity D state any two uses of graphite?
(c) Graphite is a good conductor of electricity because of free electrons presence in the graphite crystal. But there will be no free electrons in the diamond crystals, so there will not be any conductance of electricity. (d) Graphite is used for making leads for pencils and used as lubricants.
What are the difference 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. |
Why is graphite The only non-metal that conducts electricity?
In graphite each carbon is bonded to three other carbon atoms hence leaving behind a free electron. Due to the presence of this one delocalised electron, graphite is a good conductor of electricity. However, graphite is the only non-metal that can conduct electricity.
Is graphite electrically conductive?
Graphite is an electrical conductor, hence useful in such applications as arc lamp electrodes. It can conduct electricity due to the vast electron delocalization within the carbon layers (a phenomenon called aromaticity). These valence electrons are free to move, so are able to conduct electricity.
Why diamond is hard and graphite is soft?
The carbon atoms in graphite appear to bond with weaker intermolecular forces, allowing the layers to move over one another. The weak intermolecular forces are known as the weak Van der Waals forces. Therefore, diamond is hard but graphite is soft and slippery even though both have carbon present in them.
Why diamond is a non conductor and graphite is fairly a good conductor?
Further there is no free electron in the carbon tetrahedra so that diamond do not conduct electricity. Graphite is a good conductor of electricity. Its structure is the main reason for this property. Each carbon atom in graphite is directly linked to only three carbon atoms through covalent bonds.
What is the relationship between graphite and diamond?
In diamond the atoms are arranged in a three dimensional lattice, while in graphite they are joined together in an array of planar six membered rings, arranged in layers. The diamond is very hard while the possible movement of the layers in graphite makes it into an excellent lubricant.
What is the cause of difference between diamond and graphite?
Answer: The difference in properties of diamond and graphite on the basis of their structures is listed below. In diamond, strong three-dimensional networks are formed due to the presence of covalent bonds. Graphites are formed due to the weak van der Waals force of attraction.
Why diamond is so hard while it is a non metal?
Answer Expert Verified. The hardness of diamond comes due to the tetrahedral structure of diamond!! Carbon element is a non metal and even though diamond in the hardest substance known,it is an allotrope of carbon and thus is A NON METAL!!
What makes a diamond different from a graphite?
However, in a diamond there are no free electrons as four outermost electrons of a carbon atom in a diamond are covalently bonded to four other carbon atoms whereas in graphite each carbon atom is only covalently bonded to three other carbon atoms leaving free electrons to conduct electricity.
How are electrons used to conduct electricity in graphite?
In diamond, each carbon atom uses all four of its valence electrons to bond with neighboring atoms. That doesn’t leave any electrons free for conducting electricity. But in graphite, each carbon atom is only bonded to three other atoms, leaving one valence electron free to carry an electric current.
What makes a diamond able to conduct electricity?
A material’s ability to conduct electricity is determined by the number and mobility of its free electrons. In diamond, each carbon atom uses all four of its valence electrons to bond with neighboring atoms.
Which is more conductive, graphene or diamond?
Graphite is simply stacking graphene parties in the same building, one on top of the next. Each one is relatively free to come and go as they please, hence why diamond is more robust. The free electrons of graphene/graphite provide the conductivity.