GCSE Chemistry (AQA)

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Reacting Metals with Water and Acids

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Chemical changes Reactivity of metals

Reacting Metals with Water and Acids

4:26 Metal Reactivity, Oxidation, and Extraction
Spec 4.4.1.2
Previous The Reactivity Series Next Extraction of Metals
  • Metals react with water to form a metal hydroxide and hydrogen gas.
  • Example: Magnesium metal added to water produces bubbles of hydrogen gas.
  • More reactive metals have more vigorous reactions.
  • Reactions of metals with water can be used to place them in the reactivity series.
  • Potassium reacts vigorously with a lilac flame, placing it at the top of the reactivity series.
  • Copper does not react with water, placing it at the bottom of the series.
  • Metals become less reactive as you go down the reactivity series.
  • Zinc and iron usually have no reaction with water, making it difficult to differentiate between them.
  • Reactions with dilute acids can also determine metal reactivity.
  • Metals react with dilute acids to form a salt and hydrogen gas (MASH acronym).
  • Example: Lithium metal added to hydrochloric acid forms lithium chloride and hydrogen gas.
  • More reactive metals have more vigorous reactions with acids.
  • Reactions with acids can also place metals in the reactivity series.
  • Zinc reacts more intensely with dilute acids than iron, which reacts more intensely than copper.
  • Experimental results can deduce the reactivity of unknown metals.
  • Example: Metal Z reacts fast with water, making it the most reactive; Metal X fizzes with acid, making it more reactive than Metal Y.
  • Order of reactivity: Z, X, Y.

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