Which of the following compounds conducts electricity when dissolved in water?

The correct answer is the compound classified as an electrolyte. An electrolyte is a substance that, when dissolved in water, dissociates into ions, which are charged particles that enable the solution to conduct electricity. This ionic dissociation is essential for electrical conductivity, as the movement of these ions through the solution allows for the flow of electric current.

Electrolytes are typically salts, acids, or bases that free up ions in solution. For example, when sodium chloride (table salt) dissolves in water, it breaks apart into sodium ions (Na⁺) and chloride ions (Cl⁻), which can then move freely in the solution, facilitating electrical conduction.

In contrast, solvents such as water are typically the medium in which solutes dissolve but do not themselves contribute to electrical conductivity in terms of ion movement. Solutes can be any substance that is dissolved in a solvent, which can include electrolytes, but not all solutes are electrolytes. Nonelectrolytes, like sugars, do not dissociate into ions in solution, and thus do not conduct electricity. Their molecular structure does not allow for the free movement of charged particles.