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Yes, ionic compounds can only conduct electricity when molten or dissolved.
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In Which state do ionic compounds and covalent compounds conduct electricity?
Ionic compounds conduct electricity in molten state (melted) or when dissolved in a solution. Covalent compounds do not conduct electricity. Period.
Why is a melted ionic compound a good conductor of electric current but the a solid ionic compound is a poor conductor of electric current?
Upon melting, the ions are free to move and conduct electricity.
Why ionic compound are called good electrolytes?
Even insoluble ionic compounds such as CaCO 3 are electrolytes because they can conduct a current in the molten (melted) state.
Why are ionic compounds good conductors when they are melted?
Ionic compounds are good conductors of electricity when they are melted because the molecules in the compound are spread out further and can create more friction therefore creating an electric current
Why can ionic substances conduct electricity when melted?
Molten ionic compounds form a liquid that contains positive and negative ions and these conduct electricity. Cations move to the cathode, anions to anode. Not that someionic compounds decompose when melted.
How does electric conductivity of ionic compounds change when they are melted or dissolved in water?
Melting or dissolving ionic compounds increases the electrical conductivity. This is because there are free mobile charged ions that can move in the electric field and conduct current.
How does the electrical conductivity of ionic compounds change when they are melted or dissolve in water?
Melting or dissolving ionic compounds increases the electrical conductivity. This is because there are free mobile charged ions that can move in the electric field and conduct current.
What do you call compounds that conduct electric currents when dissolved or melted?
When dissolved or melted you would call them ionic. However you cannot then be absolutely certain that the solid is a straight forward ionic solid!
In Which state do ionic compounds and covalent compounds conduct electricity?
Ionic compounds conduct electricity in molten state (melted) or when dissolved in a solution. Covalent compounds do not conduct electricity. Period.
Why is a melted ionic compound a good conductor of electric current but the a solid ionic compound is a poor conductor of electric current?
Upon melting, the ions are free to move and conduct electricity.
Why is a melted ionic compound is a good conductor of electric current but a solid ionic compound is a poor conductor of electric current?
Upon melting, the ions are free to move and conduct electricity.
What do you call compounds that conduct electricity when dissolved or melted?
Electrolytes
Do aqueous solutions of ionic compounds conduct electricity?
When sodium chloride is melted, the orderly crystal structure breaks down. If a voltage is applied across this molten mass, cations migrate freely to one electrode and anions migrate to the other. This movement of ions allows electric current to flow between the electrodes through an external wire. For a similar reason, ionic compounds also conduct electric current if they are dissolved in water. When dissolved, the ions are free to move about in the solution.
When can ionic compound conduct electric?
An ionic compound can conduct electricity when it is in solution or melted.
Why ionic compound are called good electrolytes?
Even insoluble ionic compounds such as CaCO 3 are electrolytes because they can conduct a current in the molten (melted) state.
Why are ionic compounds good conductors when they are melted?
Ionic compounds are good conductors of electricity when they are melted because the molecules in the compound are spread out further and can create more friction therefore creating an electric current
Why can ionic substances conduct electricity when melted?
Molten ionic compounds form a liquid that contains positive and negative ions and these conduct electricity. Cations move to the cathode, anions to anode. Not that someionic compounds decompose when melted.
