Activity Series Calculator

The activity series ranks metals by their tendency to lose electrons (oxidize) and enter solution as ions. More active metals higher on the list will displace less active metals from their compounds in aqueous solution. A metal can only displace another metal that sits below it in the series.

The standard series from most to least active: Li > K > Ca > Na > Mg > Al > Zn > Cr > Fe > Ni > Sn > Pb > (H) > Cu > Hg > Ag > Pt > Au

The hydrogen entry is the dividing line for acid reactions. Metals above hydrogen will dissolve in hydrochloric or dilute sulfuric acid, releasing hydrogen gas. Metals below hydrogen do not react with most acids.

Single displacement reactions follow this pattern: A + BX → AX + B, where A is the more active metal displacing B from its compound BX. The driving force is the difference in reduction potentials between the two metals — the greater the gap, the more thermodynamically favored the reaction.

Zinc displacing copper from copper sulfate is a classic demonstration: Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s). You can watch the blue color of the copper solution fade as metallic copper plates out on the zinc surface.

A few practical notes. Aluminum sits high on the series, yet a piece of aluminum left in air does not vigorously react because it instantly forms a dense Al2O3 oxide layer that blocks further attack. Similarly, lead’s low reactivity relative to its position makes it useful in acid storage batteries. The activity series predicts thermodynamic feasibility — kinetic factors (oxide coatings, passivation) can prevent a reaction that is theoretically possible.

This tool uses the standard electrochemical series for 14 common metals, not including hydrogen.