Why are covalent compounds generally poor conductors of electricity?

Question

Answer

Covalent compound do not form ions. Thus, no carrier of charge is present.

Answer

Covalent compounds are generally poor conductors of electricity because covalent compounds are formed by sharing of electrons. So free ion will not form.So covalent compounds do not conduct electricity.

Answer

Covalent compounds are generally poor conductor of electricity because there are no ions to move the electrical charges .

Answer

H

Answer

Introduction:
Covalent compounds are formed by the sharing of electrons between atoms. They have a distinct molecular structure and are characterized by their low melting and boiling points. One of the key properties of covalent compounds is their poor conductivity of electricity. This can be explained by considering the nature of covalent bonding and the behavior of electrons in these compounds.

Explanation:
1. Covalent bonding:
- Covalent compounds are formed when two or more non-metal atoms share electrons in order to achieve a stable electron configuration.
- The shared electrons are attracted to the nuclei of both atoms, creating a strong bond between them.
- This shared electron pair forms a localized bond between the atoms, resulting in the formation of a molecule.

2. Lack of free electrons:
- In covalent compounds, electrons are tightly held within the shared pairs and are not free to move around.
- Unlike metallic compounds, which have a 'sea of delocalized electrons,' covalent compounds do not have any free or mobile electrons.
- As a result, there are no charged particles (either positive or negative) that can move through the compound to conduct electricity.

3. Absence of ions:
- Covalent compounds do not dissociate into ions in solution or when melted, unlike ionic compounds.
- In ionic compounds, the dissociated ions are responsible for conducting electricity.
- In covalent compounds, the sharing of electrons is localized between the bonded atoms, and there are no free ions that can carry an electric charge.

4. Insulating properties:
- The lack of mobile charged particles makes covalent compounds poor conductors of electricity.
- These compounds are generally insulators or have very low conductivity.
- Examples of covalent compounds with insulating properties include water (H2O) and methane (CH4).

Conclusion:
Covalent compounds are generally poor conductors of electricity due to the absence of free or mobile charged particles. The tightly held shared electrons and the absence of dissociated ions prevent the flow of electric current through these compounds. It is important to note that there are exceptions to this rule, such as certain covalent compounds that can conduct electricity when they undergo chemical reactions or are exposed to specific conditions.

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