GCSE Chemistry (AQA)

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Ionic Equations

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Chemical changes Reactivity of metals

Ionic Equations

9:28 Oxidation and Reduction of Metals
Spec 4.4.1.4
Previous Electrons: Oxidation & Reduction Next H+ Concentration and pH
  • Ionic compounds dissolve in water, separating into ions surrounded by water molecules.
  • Water consists of H2O molecules with oxygen covalently bonded to two hydrogen atoms.
  • Silver nitrate is an ionic compound with positively charged silver ions and negatively charged nitrate ions.
  • When dissolved, silver and nitrate ions are surrounded by water molecules, forming aqueous silver nitrate.
  • In reactions with aqueous ionic compounds, not all ions react; water molecules typically aren't involved.
  • Adding potassium bromide to the solution introduces positive potassium and negative bromide ions.
  • Bromide and silver ions bond to form solid silver bromide, which precipitates out of the solution.
  • Remaining potassium and nitrate ions are dissolved in water, forming aqueous potassium nitrate.
  • Spectator ions, like potassium and nitrate, do not react and remain unchanged.
  • Ionic equations focus on ions that react, excluding spectator ions.
  • Writing ionic equations involves separating aqueous ionic compounds into ions.
  • In exams, balanced non-ionic equations are provided for writing ionic equations.
  • Example: Silver nitrate and potassium bromide react to form silver bromide and potassium nitrate.
  • Spectator ions are identified and removed to focus on reacting ions.
  • Example: Aluminum and copper chloride reaction involves electron transfer, not just ion formation.

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