Covalent Compounds are Generally Poor Conductors of Electricity. Why

Covalent Compounds are Generally Poor Conductors of Electricity. Why?

Because electrons are necessary for the flow of electricity through any substance, and because ions are responsible for the formation of electrons, if a compound is able to form ions, then it is also able to conduct electricity; however, in order for metals to be involved in the bond, the compound must first conduct electricity.

The presence of free electrons in a material is necessary for the generation of electricity inside that substance. Ions are responsible for the formation of electrons, which are the fundamental building blocks for the ability of any substance to conduct electricity.

Ionic bonds, covalent bonds, and coordinate bonds are the three types of bonds that may be formed between two atoms, as is well known. Covalent bonds are the most common type. And since we have been provided substances with covalent bonds, we now know that covalent bonds are the bonds established between two non-metal atoms, whether they are the same or different.

 If this is the case, then the breaking of the covalent link will not result in the creation of ions. Ions are produced whenever an existing ionic connection is broken. These ions are able to do so when they are in an aqueous or molten condition; however, the covalent bond only comprises non-metals, and non-metals are unable to carry electricity or heat.

As an illustration, there are two different chemicals known as sodium chloride and carbon dioxide. The dissociation of sodium chloride results in the creation of sodium ions and chloride ions. On the other hand, the dissociation of carbon dioxide results in the synthesis of carbon monoxide and oxygen gas. Ions, and only ions, are capable of conducting electricity; carbon monoxide and oxygen gas are unable to do so.