📘 IB Understanding
A more reactive metal can displace a less reactive metal from a solution of its salt. The reactivity series ranks metals in order of their tendency to lose electrons (act as reducing agents).
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.
Worked Example
Q: Will lead(II) nitrate react with iron?
Iron is above lead in the reactivity series, so iron will displace lead:
Fe(s) + Pb(NO3)2(aq) → Fe(NO3)2(aq) + Pb(s)
Yes, the reaction will occur spontaneously.
⚠️ Exam Tip
The reactivity series is directly linked to standard electrode potentials. The most reactive metals have the most negative E° values.
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