The term "anode" refers to an essential component in electrochemical cells, such as batteries and electrolysis systems. A central concept in electrochemistry, an anode is the electrode where electrons flow out of the cell or system during a chemical reaction. It is commonly described as the positively charged (+) electrode.
During discharge, anodes in batteries and other power sources oxidize, releasing electrons into the external circuit. These electron movements create a flow of electric current that powers external devices. In electrolysis, the anode is where an oxidation reaction occurs, producing positively charged ions or cations that migrate towards the cathode (negatively charged electrode).
Anodes are typically made of materials that can easily lose electrons or undergo oxidation, such as metals like zinc, magnesium, or aluminum. To prevent corrosion or damage, anodes are often coated or protected with materials like graphite, platinum, or titanium. In some cases, sacrificial anodes made of more reactive materials are employed to purposely become corroded and protect other parts of a system from being damaged.
The anode's counterpart is the cathode, which is where electrons enter the system or cell, enabling the overall electrochemical reaction to occur. Together, the anode and the cathode maintain the continuous flow of electrons, ions, and chemical reactions necessary for numerous electrochemical processes and devices.
