What is single-metal corrosion technically referred to as?

Single-metal corrosion is most accurately described as electrochemical corrosion. This type of corrosion occurs when a single metal is exposed to an electrolyte, leading to the deterioration of that metal due to electrochemical reactions. This process typically involves the conversion of metal to metal ions, facilitated by the presence of moisture and other electrolytes that can transport ions.

In electrochemical corrosion, the metal acts as an anode, where oxidation takes place, releasing electrons and resulting in the formation of metal ions. These ions then migrate into the solution, leading to the degradation of the metal structure. This type of corrosion can be influenced by factors such as the pH of the electrolyte, temperature, and the presence of different oxidizing agents.

The other options refer to different processes. Bimetallic corrosion involves two dissimilar metals in contact with each other in the presence of an electrolyte, leading to accelerated corrosion of one metal due to galvanic effects. Galvanic corrosion is a specific situation under bimetallic corrosion where a more noble metal protects a less noble one but causes increased corrosion at the anode. Chemical corrosion, on the other hand, typically pertains to the direct reaction of a metal with non-electrolyte chemicals, rather than electrochemical processes.