Final answer:
The metals likely to corrode more in each pair, based on their position in the activity series, are aluminum over copper, silver over gold, zinc over iron, and magnesium over nickel.
Step-by-step explanation:
To determine which member of each pair of metals is more likely to corrode (oxidize), one needs to understand the activity series of metals. The activity series is a list of metals arranged according to their reactivity from highest to lowest. Metals that are higher on the activity series will oxidize more readily than those lower on the list.
Copper vs. Aluminum: Aluminum is more active than copper, making it more likely to corrode.
Silver vs. Gold: Silver is more active than gold and therefore more prone to corrosion.
Zinc vs. Iron: Zinc is more active than iron, so it is more likely to corrode.
Nickel vs. Magnesium: Magnesium is higher on the activity series than nickel, indicating that magnesium is more likely to corrode.
Factors such as the metals' positions in the periodic table, the formation of protective oxide layers, and their standard reduction potentials influence their corrosion resistance. For example, aluminum forms a protective oxide layer which shields it from further corrosion, despite being higher on the activity series compared to iron.