Question

Predict and explain which of the following systems are electrically conducting: (a) solid NaCl, (b) molten NaCl, (c) an aqueous solution of NaCl.

Answer 1

Molten NaCl and an aqueous solution of NaCl are electrically conducting, while solid NaCl is not.

Step-by-step explanation:

The systems that are electrically conducting are:

• (b) molten NaCl: When NaCl is melted, the crystal lattice breaks apart, allowing the ions to move freely and conduct electricity.
• (c) an aqueous solution of NaCl: When NaCl is dissolved in water, the crystal lattice also breaks apart, and the individual positive and negative ions can move, conducting electricity.

The system that is not electrically conducting is:

• (a) solid NaCl: In the solid state, the crystal lattice of NaCl is too rigid to allow the ions to move and conduct

Answer 2

Solid NaCl does not conduct electricity due to its rigid crystal lattice. Both molten NaCl and an aqueous solution of NaCl conduct electricity because they allow free movement of ions, which carry the current.

Step-by-step explanation:

To predict and explain the electrical conductivity of different states of NaCl (sodium chloride), we should consider the following: electrolytic reactions and the movement of ions.

(a) Solid NaCl does not conduct electricity because the ions are held in a rigid crystal lattice and are not free to move. As a result, there are no mobile charged particles to carry the current.

(b) Molten NaCl does conduct electricity because the ionic solid has melted, meaning the ions are now free to move and carry the electrical current.

(c) An aqueous solution of NaCl conducts electricity because the NaCl has dissolved, releasing free cations and anions that can move and thus carry the current.