The Metal Reactivity Series
The reactivity series ranks metals according to their tendency to lose electrons and form positive cations. A more reactive metal displaces a less reactive metal from its aqueous salt solution.
Reactivity Series
Displacement Reactions
A more reactive metal displaces a less reactive one from its salt solution:
Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s)
Zinc is above copper in the reactivity series, so it displaces copper from the solution. Iron placed in CuSO4 would also work, but copper in ZnSO4 would not react.
Predicting Fe + Pb(NO₃)₂ Reaction
Problem: Does iron react with lead(II) nitrate solution?
Solution: Iron (\(\text{Fe}\)) is above lead (\(\text{Pb}\)) in the reactivity series → Fe is a stronger reducing agent → Displacement occurs:
\[\text{Fe}(\text{s}) + \text{Pb}^{2+}(\text{aq}) \rightarrow \text{Fe}^{2+}(\text{aq}) + \text{Pb}(\text{s})\]Linking Reactivity to Standard Potentials
Link the reactivity series directly to standard electrode potentials: the higher the metal is in the reactivity series, the more negative its \(E^\circ\) value.
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