Which of the following metals is likely to sacrifice and corrode?

The correct response identifies more positive metals as likely candidates to corrode and sacrifice in a galvanic environment. This behavior is best understood through the principles of electrochemistry, particularly the galvanic series, which ranks metals based on their electrochemical potential.

Positive metals, such as noble metals, tend to have a higher reduction potential, meaning they are less willing to oxidize and therefore can act as cathodes in an electrochemical cell. When placed in contact with less noble (more negative) metals, the more positive metals can become galvanically protected while the less positive metals will oxidize, losing electrons and corroding over time.

In contrast, more negative metals possess a greater tendency to oxidize and thus are more likely to act as anodes. Neutral metals do not have marked tendencies towards either oxidation or reduction, while less reactive metals are typically less inclined to undergo corrosion than their more reactive counterparts. This distinction is crucial in applications involving corrosion prevention, material selection, and designing for durability in engineering projects.