Multiple Choice
Which element is the best reducing agent?
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16. Oxidation and Reduction
Spontaneous Redox Reactions
Multiple Choice
Suppose you wanted to cause Ni2+ ions to come out of solution as solid Ni. Which metal could you use to accomplish this?
A
Au
B
Sn
C
Mn
D
Ag
E
Cu
Verified step by step guidance1
Understand the concept of reduction potential: Metals can cause ions to come out of solution based on their reduction potential. A metal with a lower reduction potential can reduce ions of a metal with a higher reduction potential.
Identify the reduction potential of Ni2+ ions: Nickel ions (Ni2+) have a specific reduction potential, which can be found in standard reduction potential tables.
Compare reduction potentials: Look up the reduction potentials for each of the metals listed (Au, Sn, Mn, Ag, Cu) and compare them to the reduction potential of Ni2+.
Determine which metal can reduce Ni2+: The metal that has a lower reduction potential than Ni2+ can donate electrons to Ni2+ ions, causing them to be reduced to solid Ni.
Select the appropriate metal: Based on the comparison, identify which metal has a lower reduction potential than Ni2+ and can therefore cause Ni2+ ions to come out of solution as solid Ni.
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