Graphite is soft and good conductor of electricity explain

Why can graphite conduct electricity but diamond can not?

graphite is soft and good conductor of electricity explain

Which Metals Conduct Electricity The Best? - Metal Supermarkets

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Graphite is a good conductor of electricity because its electrons are delocalized or free to move around. Graphite is structured into planes with tightly bound atoms. There is a great deal of distance between planes, and they are bonded weakly together, allowing the electrons to move around. Because graphite is such a great conductor, it is used in electrical cells. It is also found in motor oil and pencils. Because graphite is soft, it is combined with clay, and baked, and hardened before being inserted into wood for pencils. Graphite is made up of bonded carbon atoms.

In part a ii , majority of the candidates could not state the type of bond present in diamond and graphite as covalent, only a few could. In part a iii , majority of the candidates could not explain correctly why diamond is hard, and graphite soft. In part b , majority of the candidates stated the different conditions under which carbon burns in air to form two gaseous products. They equally wrote and balanced the equation for the formation of each product, and named the product formed under each condition. However, some of the candidates wrote the equations, but could not state the conditions. In part c , only few candidates could write the equation for the reaction between excess lead trioxonitrate V solution and sodium chloride.

Explain the difference in properties of diamond and graphite on the basis of their structures. The following are the differences in the properties of diamond and graphite based on their structures -. In diamond there is a three dimensional network of strong covalent bonds. This makes diamond extremely hard. Because of hardness, diamond is used in making cutting and grinding tools. On the other hand, in graphite there are flat layers of carbon atoms. This makes graphite extremely soft and slippery.

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The carbon atoms are bonded differently in each substance. Graphite is a good conductor of electricity because its electrons are high boiling and melting points, while the weak bonds make graphite soft and flexible. 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. Since electrical conductivity relies on the flow of free electrons, diamond is not a good conductor.



What Makes Graphite A Good Conductor Of Electricity

Last updated: December 1, I f the 20th century was the age of plastics , the 21st century seems set to become the age of graphene a recently discovered material made from honeycomb sheets of carbon just one atom thick.

Graphite is soft and good conductor of electricity. why?

Diamond and graphite are both allotropes of carbon; they are both made entirely of the same element carbon but they differ in the way that the atoms bond with each other and arrange themselves in a structure. Each carbon atom has 4 electrons in its outer shell that it can share with other atoms in order to form 4 covalent bonds. Diamond is a giant covalent structure; each valence electron outer shell electron of every carbon atom forms a covalent bond, which means that there are no free electrons. Since electrical conductivity relies on the flow of free electrons, diamond is not a good conductor. Graphite on the other hand, although also only made up of carbon atoms, is the only non-metal that can conduct electricity. This is because only 3 of the available valence electrons form covalent bonds leaving 1 spare electron, which then becomes delocalised.

Structure Of Diamond And Graphite

Why Is Graphite a Good Conductor of Electricity?

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Graphite is a soft lubricant and a good conductor of electricity because their electrons are delocalised and free to move. These free electrons.
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