Hulls of ships and, in general, other parts of boats can be protected using a “sacrificial metal.” Zinc or magnesium may be used for this purpose. The zinc or magnesium piece is placed in direct contact with the steel hull. Explain the chemical process th

The use of a sacrificial metal such as zinc or magnesium to protect the hull of a ship involves a process called cathodic protection. In this process, the sacrificial metal acts as an anode and is placed in direct contact with the steel hull, which acts as the cathode. When the two metals are in contact with seawater, which acts as an electrolyte, an electrochemical reaction occurs. As a result, the sacrificial metal releases electrons which flow towards the hull, effectively protecting it from corrosion. This happens because the hull has a more negative potential than the sacrificial metal, which creates a natural electrical potential difference between the two metals. In essence, the corrosion that would normally occur on the hull of the ship is redirected to the sacrificial metal, which deteriorates instead. The sacrificial metal is therefore periodically replaced to ensure continued protection. Overall, cathodic protection using a sacrificial metal can effectively prevent the loss of structural integrity of ships and other marine structures due to corrosion, by redirecting the corrosion to a sacrificial metal that can be easily replaced.