* No free charges: In covalent compounds, electrons are shared between atoms to form strong covalent bonds. These electrons are tightly bound and are not free to move independently. There are no free ions or electrons to carry an electrical current.
* Neutral molecules: Covalent compounds typically form neutral molecules. Since there's no separation of charge within the molecule, there are no charged particles to transport electricity.
* Weak intermolecular forces: The forces between covalent molecules (like van der Waals forces or hydrogen bonds) are much weaker than the ionic bonds found in ionic compounds. This means the molecules are less likely to break apart into ions that could conduct electricity.
In contrast, ionic solutions conduct electricity well because:
* Free ions: Ionic compounds dissociate in solution, releasing free ions that can move and carry an electric current.
* Charged particles: The presence of charged ions allows for the flow of electricity.
Example:
* Sugar (covalent) in water: Sugar dissolves in water, but the molecules remain intact. The solution does not conduct electricity.
* Salt (ionic) in water: Salt dissolves in water and dissociates into Na+ and Cl- ions. The solution conducts electricity.
In summary: Covalent solutions have poor electrical conductivity because they lack free charges (ions or electrons) to carry an electric current.
