Precipitation reactions involve double replacement (metathesis) processes in aqueous solution where two soluble salts exchange partners to form at least one insoluble product (the precipitate) and a soluble salt. The key types of chemical equations used to describe these reactions are:

• Molecular (overall) equation: Displays all reactants and products as complete formulas, showing the stoichiometry of the reaction in its simplest whole-number form.
  Example: CaCl2(aq) + Na2SO4(aq) → CaSO4(s) + 2 NaCl(aq)

• Complete ionic equation: Breaks all soluble strong electrolytes into their constituent ions, while precipitates and weak electrolytes remain as formulas.
  Example: Ca2+(aq) + 2 Cl−(aq) + 2 Na+(aq) + SO42−(aq) → CaSO4(s) + 2 Na+(aq) + 2 Cl−(aq)

• Net ionic equation: Cancels spectator ions (ions that appear on both sides) to show only the species that form the precipitate.
  Example: Ca2+(aq) + SO42−(aq) → CaSO4(s)

These classifications align with standard teaching resources on aqueous precipitation chemistry. If you have specific reactions you’d like categorized (molecular, complete ionic, or net ionic), share them and they’ll be identified accordingly.