Through appropriate experiments, we could expand the...

Through appropriate experiments, we could expand the activity series in Table 4.6 to include additional metals. If aluminum is oxidized by $V^{3+}$ but aluminum does not reduce $\mathrm{Sc}^{3+}$, where would you place vanadium and scandium in the activity series? Which metal would you test to firmly establish scandium's position?

Key Concepts

Standard Reduction Potentials

Standard reduction potentials quantitatively measure a species’ tendency to gain electrons. In the context of the activity series, a metal with a more negative reduction potential is more easily oxidized and is placed higher in reactivity, while a metal with a more positive potential is less reactive. This concept underpins the order of metals in the activity series.

Experimental Determination of Metal Reactivity

To firmly establish a metal's position within the activity series, one conducts controlled displacement experiments using metal ions with known reactivity. By comparing reactions—such as a metal's ability (or inability) to reduce another metal’s ion—researchers can determine its relative position in the series. Testing a metal whose position is well established, such as magnesium, against the metal of interest provides a firm benchmark.

Activity Series of Metals

The activity series is a ranking of metals (and some nonmetals) according to their relative reactivities, especially their tendency to lose electrons (oxidize). Metals higher in the series react more readily and can displace metals that appear lower in the series during redox (displacement) reactions.

Metal Displacement (Redox) Reactions

These reactions involve a more reactive metal donating electrons to reduce the ions of a less reactive metal, causing deposition of the less reactive metal and oxidation of the more reactive one. Such reactions are key for experimentally determining the relative reactivities of metals by observing whether one metal can displace another from its compound.

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