Electrolytes versus Non-electrolytes

Why are we always advised to consume sports drinks after an intense workout? This is because sports drinks contain a high concentration of electrolytes which are essential for the healthy functioning of our body. During an intense exercise, electrolytes like Na⁺ or  K⁺ are rapidly lost from the body via sweat. Therefore, consuming sports drinks are ideal because they contain many electrolytes necessary for the healthy functioning of cells and tissues, including but not limited to Sodium, Potassium, Chloride, Calcium, Sulfates. 
Therefore, electrolytes refer to ionic compounds/ions thats can conduct electricity in the molten state or an aqueous solution, and are themselves decomposed in the process. 

(Above: Fig 4.4 showing how strong electrolytes in an electrolytic set-up conducts an electric current which lights up the bulb). 

Ionic Compounds in the solid state cannot be considered an electrolyte as they cannot conduct electricity. This is because they exist as a giant ionic lattice of oppositely charged ions held together by strong electrostatic forces of attraction. For instance, in the ionic compound Magnesium Oxide, the Mg²⁺ and O^2- ions are held together closely due this strong electrostatic force of attraction.








 In the molten state, the ionic compound has been liquefied by the intense heat applied to the object. As heating the object increases its kinetic energy, the ions vibrate and the rigid ionic structure breaks down to a less-ordered state and is liquefied. As such, the ions can now move freely with electricity and conduct an electric current. Ionic compounds in aqueous solutions can be considered electrolytes. When ionic compounds are in water, they dissociate into their ions. Since there is presence of free moving ions, an electric current can be conducted. Electrolytes can be further classified into strong or weak, which is determined by how much of the ionic compound dissociates into its ions. Therefore, we cannot claim that substances with a greater mole are better electrolytes because not all of the ionic compound might dissociate into its ions.

Non-electrolytes, on the other hand are unable to ionize when in molten or aqueous state. As there are no mobile ions or delocalised electrons in solution, non-electrolytes cannot produce an electric current. Examples of non-electrolytes include organic compounds with hydroxylic groups like alcohol, carbon disulphide, and glucose solution. 






Other than the fact that one can conduct electricity and the other cant, electrolytes contain free moving ions in molten or aqueous solution while non-electrolytes do not.