Magnesium, aluminium and zinc can react with water, but the reaction is usually very slow unless the metal samples are specially prepared to remove the surface layer of oxide which protects the rest of the metal. There is some ambiguity at the borderlines between the groups. Metals in the middle of the reactivity series, such as iron, will react with acids such as sulfuric acid (but not water at normal temperatures) to give hydrogen and a metal salt, such as iron(II) sulfate:įe (s) + H 2SO 4 (l) → FeSO 4 (aq) + H 2 (g) The most reactive metals, such as sodium, will react with cold water to produce hydrogen and the metal hydroxide:Ģ Na (s) + 2 H 2O (l) →2 NaOH (aq) + H 2 (g) There is no unique and fully consistent way to define the reactivity series, but it is common to use the three types of reaction listed below, many of which can be performed in a high-school laboratory (at least as demonstrations).
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