In the galvanic series, the more active metals:

The correct answer indicates that more active metals will corrode if connected to a less active metal. In the galvanic series, metals are categorized based on their electrochemical activity, with more active metals being those that are more prone to oxidation and corrosion. When a more active metal is in contact with a less active (or noble) metal in an electrolyte, a galvanic cell is formed, leading to increased corrosion of the more active metal.

This occurs due to the potential difference between the metals; the more active metal acts as an anode and undergoes oxidation, while the less active metal serves as a cathode, experiencing a reduction reaction. Hence, under these conditions, the more active metal will tend to lose electrons and corrode more quickly than it would if it were not in contact with the less active metal.

Furthermore, the choice suggesting that more active metals are more cathodic or that they will not corrode in contact with a less active metal does not align with the principles behind galvanic corrosion. More active metals are inherently more susceptible to corrosion, especially when they are electrically connected to a more noble metal, leading to their deterioration over time.