Which statement is true about the cathode in electrochemical cells?

In an electrochemical cell, the cathode is defined as the electrode where reduction occurs. Reduction is the gain of electrons, and during this process, the species being reduced accepts electrons from the external circuit. This distinction is critical because it helps in understanding the overall functioning of both galvanic (spontaneous) and electrolytic (non-spontaneous) cells.

When the cell operates, electrons flow from the anode, where oxidation takes place, to the cathode. This flow of electrons is what enables the cathode to facilitate the reduction reaction that is vital for the electrochemical process.

The other statements do not accurately describe the role of the cathode. While it indeed contributes to the production of electricity in galvanic cells, not all cathodes generate electricity under every condition (as seen in electrolytic cells). Additionally, the cathode is typically connected to the negative terminal of a battery in galvanic cells, countering the assertion that it connects to the positive terminal. Recognizing the cathode's role is fundamental to understanding the reversal of reactions in electrochemical processes and maintaining clarity about how these cells function.