Solid NaCl (Table Salt)
* Conductivity: Non-conducting
* Explanation: In solid NaCl, the sodium (Na+) and chloride (Cl-) ions are arranged in a tightly packed, crystalline lattice. These ions are fixed in their positions and cannot move freely. While the ions carry a charge, their immobility prevents the flow of electricity.
Molten NaCl
* Conductivity: Conducting
* Explanation: When NaCl is melted, the ionic bonds holding the lattice together break. This allows the Na+ and Cl- ions to move freely throughout the liquid. Now that the charged particles can move, they can carry an electrical current.
Aqueous Solution of NaCl
* Conductivity: Conducting
* Explanation: When NaCl dissolves in water, it dissociates into Na+ and Cl- ions. These ions become surrounded by water molecules (hydration), allowing them to move freely throughout the solution. This mobility of charged particles makes the solution electrically conductive.
In summary:
* Solid: Ions are fixed, no free movement, no conductivity.
* Molten: Ions are free to move, conductivity is present.
* Aqueous: Ions are free to move in solution, conductivity is present.
