Question

Why are carbon compounds poor conductors of electricity? Write the name and structure of a saturated compound in which the carbon atoms are arranged in a ring. Give the number of single bonds present in this compound.

Answer 1

Hint: Try to recall that carbon compounds and most hydrocarbons are poor electrical conductors because the covalent bonds in most carbon compounds don’t really support ionic or metallic conduction. Now, by using this you can easily answer the given question.

Complete step by step solution:
* It is known to you that carbon compounds are mostly poor conductors of electricity. Some, such as oils and waxes, are actually excellent insulators.
* This happens because atoms of carbon do not have free electrons in the conduction band. Therefore, they do not conduct well at room temperature.
* But, if the temperature is increased, more electrons acquire energy and start contributing to the conduction of electricity.
* The name of a saturated compound in which the carbon atoms are arranged in a ring is fullerenes.
* Of all the fullerenes, $C_{60}$ is most stable. It looks like a soccer ball and is sometimes called a bucky ball. It contains 20 six-membered rings and 12 five-membered rings.
* Six-membered rings are fused both to other six-membered rings and five-membered rings, but the five-membered rings are connected only to six-membered rings.
* The total number of single bonds present in $C_{60}$ is 60.

Note:
* It should be remembered to you that in $C_{60}$_, each carbon atom forms three sigma bonds with other three carbon atoms. The remaining one electron of each carbon is delocalized in molecular orbital which, in turn, gives aromatic character to the molecule.
* Also, you should remember that fullerene can react with alkali metals to form solids which behave as a superconductor.