Molten sodium chloride conducts electricity due to the presence of

Options

A. Free electrons
B. Free ions
C. Free molecules
D. Atoms of sodium and chlorine

Answer

To solve the question "Molten sodium chloride conducts electricity due to the presence of", we will analyze the properties of sodium chloride in different states and how they relate to electrical conductivity.

### Step-by-Step Solution:

1. **Understanding Sodium Chloride (NaCl):**
Sodium chloride is an ionic compound composed of sodium ions (Na⁺) and chloride ions (Cl⁻). In its solid state, these ions are arranged in a rigid lattice structure.

**Hint:** Remember that ionic compounds consist of positively and negatively charged ions.

2. **Solid State of Sodium Chloride:**
In solid sodium chloride, the ions are fixed in place within the crystal lattice and cannot move freely. This immobility of ions means that solid NaCl does not conduct electricity.

**Hint:** Think about what happens to the ions in a solid structure compared to a liquid.

3. **Molten State of Sodium Chloride:**
When sodium chloride is heated to its melting point, it becomes molten (liquid). In this molten state, the rigid lattice breaks down, allowing the ions to move freely.

**Hint:** Consider what happens to the structure of a solid when it is heated.

4. **Ionic Dissociation:**
In the molten state, sodium chloride dissociates into its constituent ions: Na⁺ and Cl⁻. These free-moving ions are essential for conducting electricity.

**Hint:** Recall that electrical conductivity in ionic compounds is due to the movement of charged particles.

5. **Conductivity of Molten Sodium Chloride:**
The presence of free-moving ions (Na⁺ and Cl⁻) in molten sodium chloride allows it to conduct electricity. When an electric potential is applied, these ions can migrate towards the electrodes, facilitating the flow of electric current.

**Hint:** Think about how charges need to move to create an electric current.

### Final Answer:
Molten sodium chloride conducts electricity due to the presence of free-moving ions (Na⁺ and Cl⁻).