For this we have to consider the reactive series of metals in which metals are arranged according to their reactivity order.
Oxidation of a metal can be defined as ability to lose electrons to become positively charged metal and a metal will lose its electrons by reacting with a metal that is having low chemical reactivity as a higher reactive metal can lose its electrons to a low reactive metal. So here a metal should be one that is more reactive than tin so that it can lose its electrons to tin to become positively charged and less reactive than iron so that it will not give its electrons to iron to become positively charged. If we look into reactive series of metal than we will find that nickel is the example of a metal that is more reactive than tin and less reactive than iron.
Nickel and cadmium is the metal that can be oxidized with a sn2+ solution, but not with a fe2+ solution.
An ionic chemical reaction occurs on the surface of metal in the presence of oxygen.
Metals that can be oxidized in solution must have a weaker oxidizing agent or be less reactive than tin.
With solution, the same metals cannot be oxidized.
Thus, the correct option is Nickel and cadmium.
Learn more about oxidization
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