* The free metal: This is the most common outcome. The metal ions in the solution migrate towards the negatively charged cathode, where they gain electrons and are reduced to their elemental form. For example, in the electrolysis of copper sulfate (CuSO₄), copper ions (Cu²⁺) are reduced at the cathode to form solid copper metal (Cu).
* Hydrogen gas: If the metal is less reactive than hydrogen, hydrogen ions (H⁺) from the solution will be reduced at the cathode instead of the metal ions. This results in the evolution of hydrogen gas (H₂). For example, in the electrolysis of a solution containing sodium chloride (NaCl), hydrogen gas is produced at the cathode, while sodium ions (Na⁺) remain in solution.
* Other species: Depending on the specific compound and conditions, other species might form at the cathode. These could include:
* Hydrated metal ions: In some cases, metal ions might not be fully reduced to the elemental state but form hydrated metal ions.
* Metallic alloys: If the solution contains multiple metal ions, alloys might form at the cathode.
In summary, the specific product formed at the cathode during electrolysis depends on the relative reactivity of the metal and hydrogen, as well as the specific conditions of the electrolysis.
