Net Ionic Equations - AP Chemistry

An equation showing only the species that change during the reaction. Shows only species that actually react or are produced.

$Fe^{3+} + 3OH^- \rightarrow Fe(OH)_3$. Iron hydroxide forms as an insoluble precipitate.

No net ionic equation; no ions in the reaction. No ionic compounds are involved in this decomposition.

$Ag^+ + Cl^- \rightarrow AgCl$. Shows formation of insoluble silver chloride precipitate.

$CaCO_3$ is the precipitate. Calcium carbonate is insoluble in water.

$Na^+$ and $NO_3^-$ are spectator ions. These ions don't participate in the precipitation.

$Mg(OH)_2$ is the precipitate. Magnesium hydroxide is insoluble in water.

$Ba^{2+} + SO_4^{2-} \rightarrow BaSO_4$. Formation of insoluble barium sulfate from ionic reactants.

$S^{2-} + 2H^+ \rightarrow H_2S$. Sulfide ion is protonated by acid to form gas.

$Zn + 2H^+ \rightarrow Zn^{2+} + H_2$. Metal displacement reaction producing hydrogen gas.

$Pb^{2+} + 2Cl^- \rightarrow PbCl_2$. Lead chloride forms as an insoluble precipitate.

Spectator ions. They remain unchanged and don't participate in the reaction.

No net ionic equation; no ions in the reaction. No ionic compounds are involved in this decomposition.

$Ba^{2+} + SO_4^{2-} \rightarrow BaSO_4$. Formation of insoluble barium sulfate from ionic reactants.

An equation showing only the species that change during the reaction. Shows only species that actually react or are produced.

$Fe^{3+} + 3OH^- \rightarrow Fe(OH)_3$. Iron hydroxide forms as an insoluble precipitate.

$CO_3^{2-} + 2H^+ \rightarrow CO_2 + H_2O$. Carbonate ion reacts with acid to produce gas.

All ions present in the reaction, including spectator ions. Shows both reacting and non-reacting ions in solution.

$3Ba^{2+} + 3SO_4^{2-} \rightarrow 3BaSO_4$. Three equivalents of precipitation reaction occur.

A reaction where an acid and a base react to form water and a salt. Proton transfer from acid to base forms neutral products.

$CO_3^{2-} + 2H^+ \rightarrow CO_2 + H_2O$. Carbonate reacts with acid to produce gas and water.

$H^+ + OH^- \rightarrow H_2O$. Shows only the acid-base neutralization, omitting spectators.

No precipitate; only water forms. This is an acid-base reaction, not precipitation.

$2H^+ + 2OH^- \rightarrow 2H_2O$. Diprotic acid neutralized by two hydroxide ions.

$Cu^{2+} + 2OH^- \rightarrow Cu(OH)_2$. Hydroxide ions precipitate copper as insoluble hydroxide.

A reaction where an insoluble solid forms and separates from solution. Soluble salts combine to form an insoluble product.

$Mg + 2H^+ \rightarrow Mg^{2+} + H_2$. Active metal displaces hydrogen from acid.

$Na^+$ and $Cl^-$ are spectator ions. These ions remain in solution and don't react.

$Na^+$ and $NO_3^-$ are spectator ions. These ions appear unchanged on both sides of the equation.