Final answer:
An electrode is a metal conductor that serves as a terminal in an electrochemical cell; this statement is true. It functions as either the anode or the cathode where oxidation and reduction occur, respectively, facilitating the flow of electric current in processes like electroplating.
Step-by-step explanation:
The statement that an electrode is an electric conductor, usually metal, used as either of the two terminals of an electrically conducting medium is true. Electrodes play a crucial role in electrochemical cells, which are systems that either generate electricity through chemical reactions or use electrical energy to stimulate chemical changes. In these cells, one electrode known as the cathode is where reduction occurs (gain of electrons), while the other electrode known as the anode is where oxidation occurs (loss of electrons).
Electrochemical cells consist of an arrangement where two separate solutions containing an anode and cathode are joined by a salt bridge and a wire that conducts electrons. This setup allows for the flow of electrons from the anode to the cathode, conducting useful work, such as powering devices or electroplating objects for durability and aesthetic qualities. Electrolytes are the medium in which these redox reactions occur as they are substances containing free ions that facilitate the movement of electric current.
In the process of electrolysis, which is crucial for electroplating, a metal object connected to the cathode is immersed in a solution containing metal cations. When the electrolysis is carried out, metal cations are reduced to the elemental metal, creating a thin layer on the object's surface. Thus, electrode functionality is essential in converting chemical energy to electrical energy or vice versa, and in applications like coating materials with metals.