Electricity can be defined as charged particles in motion. Using this definition, explain how an aqueous solution of an electrolyte conducts electricity.

To understand the basics of electrolyte conduction, one must first grasp what electrolytes are in the chemical world. Electrolytes are substances that, when dissolved in water or another solvent, separate into ions, becoming capable of conducting electricity. Common electrolytes include general salts, like sodium chloride (table salt), as well as acids such as hydrochloric acid (HCl), and bases like sodium hydroxide (NaOH).

These substances are integral to a plethora of biological processes in the body, such as nerve signal transmission and muscle contractions. In our daily lives, they're found in household items like batteries and sports drinks, highlighting the practical importance of understanding their chemistry.

The dissociation of electrolytes is a fundamental concept when discussing their conductivity. This is the process where solid ionic compounds, upon dissolving in a solvent, separate into individual ions that are each surrounded by solvent molecules. This happens because the polar molecules of the solvent, like water, are attracted to the different charges on the ions. For example,
\[NaCl_{(s)} \rightarrow Na^+_{(aq)} + Cl^-_{(aq)}\]
illustrates how the ionic compound sodium chloride separates into sodium (Na\textsuperscript{+}) and chloride (Cl\textsuperscript{-}) ions when it enters an aqueous solution. This is crucial for conduction as only free-moving charged particles can carry an electrical current.

The principle of conductivity in aqueous solutions is inherently linked to the presence of ions. Not all solutions are conductive; only those that contain free ions can carry an electric charge. It is the movement of these ions, with their positive and negative charges, that allows for the flow of electricity. When an electrolyte such as table salt dissolves in water, it's not the water carrying the charge, but rather the free ions that the salt releases into the solution. The better a solution can release these ions, the higher its conductivity will be. A strong electrolyte like saltwater will have more ions available to conduct electricity, unlike a weak electrolyte, which dissociates partially, providing fewer ions for conduction.

Delving into the realm of physics, the movement of ions is the ultimate reason an electrolyte solution conducts electricity. Each type of ion, whether anion or cation, moves independently in response to an external electrical field. Upon applying a voltage, cations migrate towards the negative electrode (cathode), while anions make their way toward the positive electrode (anode).

The speed at which these ions move can depend on many factors, such as the charge and size of the ions, the viscosity of the solvent, and the strength of the electric field. The coordinated movement of countless ions is what constitutes an electric current through the solution. Fundamentally, without the movement of ions, you would not obtain an electric current; conduction would be impossible. This concept is supremely significant in fields like electrochemistry, where the manipulation of ion movement is central to processes like electrolysis.