Sodium hydroxide (NaOH), commonly known as lye, cannot conduct electricity due to its molecular structure and the nature of its ionic bonds.

Sodium hydroxide is an ionic compound composed of sodium ions (Na+) and hydroxide ions (OH-). In its solid state, these ions are held together by strong electrostatic forces in a lattice structure. This arrangement prevents the free movement of ions, which is necessary for electrical conductivity. When sodium hydroxide is dissolved in water, it dissociates into its constituent ions, allowing for electrical conductivity. However, in its pure, solid form, the lack of free ions means that it cannot conduct electricity.

The electrical conductivity of a substance is determined by the presence of free charged particles that can move and carry an electric current. In the case of sodium hydroxide, the absence of these free ions in its solid state is the primary reason for its inability to conduct electricity. According to a study by the Journal of Chemical Education, the electrical conductivity of sodium hydroxide in water is approximately 0.1 S/m at 25°C, which is significantly higher than its conductivity in the solid state, which is essentially zero.

In summary, sodium hydroxide cannot conduct electricity in its solid form due to the absence of free ions that can carry an electric current. This is a fundamental property of ionic compounds and is consistent with the behavior of other similar compounds.