Very Short Question and Answers - Reactivity Series of Metals

The Reactivity Series of Metals is a list of metals arranged in order of their decreasing chemical reactivity.

Potassium is at the top (most reactive) and Platinum is at the bottom (least reactive) of the series.

Hydrogen is included for comparison, to help predict whether a metal can displace hydrogen from acids.

Reactivity decreases as you move down the series.

Because they lose their valence electrons very easily, making them highly reactive.

2Na + 2H₂O → 2NaOH + H₂↑

Zinc will react with steam, but not with cold water; copper will not react with either.

Zn(s) + CuSO₄(aq) → ZnSO₄(aq) + Cu(s)

No reaction; iron is less reactive than zinc, so it can't displace zinc.

They are extracted by electrolysis of their molten salts.

Moderately reactive metals like zinc, iron, and lead can be reduced using carbon because they are less reactive than carbon.

Mg + 2HCl → MgCl₂ + H₂↑

No, copper does not react with dilute hydrochloric acid to liberate hydrogen gas because it is less reactive than hydrogen.

Iron is coated with a more reactive metal like zinc (galvanization) to prevent corrosion.

They are very low in the reactivity series, so they do not tarnish or corrode easily.

A more reactive metal displaces a less reactive metal from its salt solution; e.g., iron displaces copper from copper sulphate solution.

Aluminium > Zinc > Iron > Copper

Magnesium displaces iron: Mg(s) + FeSO₄(aq) → MgSO₄(aq) + Fe(s)

They can often be extracted by simple methods, as they occur in native (uncombined) form.

Down the alkali and alkaline earth metal groups, metals become more reactive because their outer electrons are farther from the nucleus and more easily lost.