Solid NaCl
* Electrical Conductivity: Non-conducting
* Explanation: In its solid state, NaCl exists as a crystalline lattice. The sodium (Na+) and chloride (Cl-) ions are held in a rigid, ordered arrangement. While the ions are charged, they are fixed in their positions and cannot move freely. Without the ability for ions to move, there is no flow of electrical current.
Molten NaCl
* Electrical Conductivity: Conducting
* Explanation: When NaCl is heated to its melting point, the ionic bonds break down, and the ions become mobile. These free-moving ions can now carry an electric current. The molten salt acts as an electrolyte, conducting electricity through the movement of ions.
Aqueous Solution of NaCl
* Electrical Conductivity: Conducting
* Explanation: When NaCl dissolves in water, the ionic bonds break, and the Na+ and Cl- ions become surrounded by water molecules. These hydrated ions can move freely throughout the solution, allowing for the conduction of electricity. The water acts as a solvent, facilitating the movement of ions and creating an electrolytic solution.
Key Points:
* Ionic Compounds: The ability of ionic compounds to conduct electricity depends on the mobility of their ions.
* Electrolytes: Solutions that conduct electricity due to the presence of free-moving ions are called electrolytes.
* Solubility: The ability of an ionic compound to dissolve in a solvent (like water) is crucial for its electrical conductivity in solution.
