Reactivity series is a list of metals ordered according to their reactivity. Hydrogen is commonly included in a reactivity series as a reference middle point. A more reactive metal displaces a less reactive metal in its salt solution unless the more reactive metal reacts with water in a solution. For example, iron chloride solution reacts with zinc to produce iron and a zinc chloride solution. Copper nitrate solution reacts with zinc to produce copper and zinc nitrate.

FeCl₂ + Zn → Fe + ZnCl₂
Zn + Cu(NO₃)₂ → Zn(NO₃)₂ + Cu

Unreactive metals are commonly found as pure metals. Other more reactive metals are found naturally in their ores and need to be processed to get pure elements. The most unreactive metals can be simply heated to extract them from their ores, for example, 2Ag₂O → 4Ag + O₂. Heating an ore with carbon can be used to extract other metals that are less reactive than carbon, for example, C + 2FeO → CO₂ + 2Fe. Alternatively, electrolysis can be used to extract metals from metal compounds. During the reduction of metal oxides, metal oxides lose oxygen and are reduced to pure metals.

Reactivity series can help determine if metals react with cold water, diluted acids or just oxygen. Reactive metals tend to form positive ions in many of these reactions. Unreactive metals are less likely to react with the aforementioned compounds to form positive ions.

The most reactive metals react with water to produce metal hydroxides and hydrogen. For example:
2K + 2H₂O → 2KOH + H₂

Some metals react with acids to displace hydrogen forming metal salts and hydrogen. For example:
Mg + 2HCl → MgCl₂ + H₂

During reactions with oxygen metals are oxidised to produce metal oxides. For example:
4Na + O₂ → 2Na₂O

The most reactive metals react with water to produce metal hydroxides and hydrogen.

2Li + 2H₂O → 2LiOH + H₂

A more reactive metal displaces a less reactive metal in its salt solution unless the more reactive metal reacts with water in a solution. Since sodium reacts vigorously with water, sodium does not displace iron in an iron chloride solution.

Sodium reacts with water in the solution.

Reactive metals tend to form positive ions in many of these reactions. Unreactive metals are less likely to react with the aforementioned compounds to form positive ions.

The tendency to form positive ions decrease with a decreasing reactivity of metals.

A more reactive metal displaces a less reactive metal in its salt solution unless the more reactive metal reacts with water in a solution.

2Al + 3FeCl₂ → 2AlCl₃ + 3Fe

During reactions with oxygen metals are oxidised to produce metal oxides.

magnesium oxide