Why do ionic compounds conduct electricity when they are melted or dissolved in water?
When melted the ions of which the compound is composed are free to move; the positive ion goes toward the negative electrode and the negative ion goes toward the positive electrode. In solution, the crystal structure is destroyed and the ions are free to move about in the solvent.
Ionic compounds conduct electricity when they are melted or dissolved in water because they consist of positive and negative ions that are free to move. This movement of ions allows the flow of electric charge through the substance. Here's a more detailed explanation of why this occurs:
When an ionic compound, such as sodium chloride (NaCl), is dissolved in water, it dissociates into its constituent ions: Na+ and Cl-. Each of these ions carries an electric charge. The positive sodium ions are attracted to the negative electrode (anode), and the negative chloride ions are attracted to the positive electrode (cathode) when an external electric field is applied.
In a similar way, when an ionic compound is melted, the solid lattice structure breaks down, and the ions become free to move. These mobile ions then allow the flow of electric current through the molten substance.
Overall, the movement of ions in the molten or aqueous state enables the carrying of electric charge, leading to the conductivity of electricity. It is important to note that ionic compounds do not conduct electricity in their solid state since the ions are fixed in position and cannot move freely.