The activity series of metals ranks metals from most reactive (Li, K, Na) to least reactive (Au, Pt). Use the displacement predictor to determine whether a metal will react with an ionic solution, and see the balanced equation with KaTeX rendering.
Activity Series
Most reactive at top
Displacement Reaction Predictor
Will Metal A displace Metal B from its ionic solution?
Quick Reference
How to Use the Activity Series Reference
The activity series is an empirical ranking of metals based on their reactivity — their tendency to lose electrons and form positive ions. Understanding this series is essential for predicting single displacement (single replacement) reactions.
Step 1: Read the Series
The activity series lists metals from most reactive (lithium at the top) to least reactive (gold at the bottom). Each entry shows the standard reduction potential — the more negative the E° value, the more reactive the metal. Metals with very negative E° (Li, Na, K) readily lose electrons; metals with positive E° (Cu, Ag, Au) resist oxidation.
Step 2: Predict Displacement
Select a metal A and a metal ion solution of B. If A is higher in the series than B, A will displace B from solution (A gets oxidized, B gets reduced). The reaction: A + B^n+(aq) → A^n+(aq) + B(s). If A is lower than B, no reaction occurs.
The Zn + CuSO₄ Classic Experiment
When a zinc strip is placed in copper sulfate solution, the blue color fades and copper metal deposits on the zinc. Zinc (−0.76 V) is higher in the activity series than copper (+0.34 V), so Zn displaces Cu²⁺. The reaction is: Zn(s) + CuSO₄(aq) → ZnSO₄(aq) + Cu(s). The driving force is the 1.10 V difference in reduction potentials.
Reactions with Water and Acids
The series also tells you about reactions with water and acids. Alkali metals (Li, Na, K) react explosively with water: 2Na + 2H₂O → 2NaOH + H₂. Metals above hydrogen but below the alkali metals react with dilute acids to produce H₂ gas: Fe + H₂SO₄ → FeSO₄ + H₂. Copper, silver, and gold are below hydrogen and do not react with dilute HCl or H₂SO₄.
Practical Applications
The activity series explains galvanization (zinc coating protects iron because Zn is more reactive and sacrificially corrodes first), corrosion protection, and battery selection. In electroplating, the metal being plated must be less reactive than the plating metal. In the blast furnace, carbon (like coke) reduces iron ore because carbon is effectively above iron in the series under those conditions.
FAQ
What is the activity series of metals?
The activity series ranks metals from most reactive (top) to least reactive (bottom) based on their tendency to lose electrons and form positive ions. Metals higher in the series can displace metals lower in the series from their solutions.
How do you predict single displacement reactions?
A metal A will displace metal B from solution only if A is higher (more reactive) in the activity series than B. Example: Zn + CuSO₄ → ZnSO₄ + Cu (Zn is more reactive than Cu). If A is below B, no reaction occurs.
Why does zinc displace copper but not vice versa?
Zinc is higher in the activity series than copper — it has a more negative standard reduction potential (Zn: -0.76V vs Cu: +0.34V). Zinc more readily loses electrons (is oxidized), so it can reduce Cu²⁺ ions to Cu metal. Copper cannot reduce Zn²⁺ ions because Cu is less reactive.
Which metals react with water?
Alkali metals (Li, Na, K) and alkaline earth metals (Ca, Ba) react vigorously with water to produce hydrogen gas and metal hydroxides. Magnesium reacts slowly with hot water. Metals below Mg in the series generally do not react with water.
Is this activity series tool free?
Yes, completely free with no signup required. All calculations and lookups run in your browser.
What metals react with acids?
Metals above hydrogen in the activity series react with dilute acids (HCl, H₂SO₄) to produce hydrogen gas and a metal salt. Example: Zn + H₂SO₄ → ZnSO₄ + H₂. Metals below hydrogen (Cu, Ag, Au, Pt) do not react with dilute acids.
What is the relationship between activity series and electrochemical series?
They are essentially the same! The electrochemical series ranks metals by standard reduction potential (E°). More negative E° = more reactive = higher in activity series. The activity series is the qualitative version; the electrochemical series provides quantitative E° values.