Question

molten (liquid) nacl is represented by the particulate diagram shown above. which of the following indicates whether nacl(l) conducts electricity and best explains why or why not?
a it conducts electricity because na is a metal.
b it conducts electricity because ions are free to move.
c it does not conduct electricity because cl is a nonmetal.
d it does not conduct electricity because there are no free electrons.

Explanation:

Step1: Recall the concept of electrical conductivity in ionic compounds

Ionic compounds conduct electricity when ions are free to move. In solid NaCl, ions are fixed in lattice. In molten (liquid) NaCl, the lattice breaks, and \(Na^{+}\) and \(Cl^{-}\) ions are free to move.

Step2: Analyze each option

• Option A: Incorrect. NaCl is an ionic compound. Conductivity in molten NaCl is due to ions (\(Na^{+}\) and \(Cl^{-}\)), not because Na is a metal (in NaCl, Na is in ionic form \(Na^{+}\), not metallic Na).
• Option B: Correct. Molten NaCl has free - moving \(Na^{+}\) and \(Cl^{-}\) ions. Ions carry electric charge, so it conducts electricity.
• Option C: Incorrect. The conductivity of molten NaCl is not related to Cl being a non - metal. The key is the presence of free - moving ions.
• Option D: Incorrect. Molten NaCl has free - moving ions (\(Na^{+}\) and \(Cl^{-}\)), so it conducts electricity.

Answer:

B. It conducts electricity because ions are free to move.