What do the terms anode and cathode refer to in an electrochemical cell?

In an electrochemical cell, the terms anode and cathode specifically refer to the positive and negative terminals, respectively. The anode is the electrode where oxidation occurs, meaning it is the site where electrons are released during the electrochemical reaction. Conversely, the cathode is where reduction takes place, which is the site where electrons are accepted. This flow of electrons from the anode to the cathode generates the electric current that can be harnessed for various applications, such as powering a device.

Understanding that anode and cathode designate the roles of the electrodes in the context of electron flow is crucial in electrical theory, as it underpins the functionality of batteries and electrochemical cells. Each terminal has distinct characteristics; the anode is negatively charged in galvanic cells (voltaic cells), while in electrolytic cells, the roles are reversed. This distinction directly correlates to how these devices operate in providing electric energy through chemical reactions.