Net Ionic Equations

Net Ionic Equation A simplified chemical equation that only shows the ions that participate in the reaction, removing spectator ions.

Spectator Ions Ions that do not change during a reaction and appear on both sides of the equation.

Steps to Writing a Net Ionic Equation 1. Write the full balanced equation. 2. Break all aqueous (aq) compounds into ions. 3. Identify and remove spectator ions. 4. Write the remaining reacting ions as the net ionic equation.

Example of a Full Reaction (AgNO₃ + NaCl) AgNO₃ (aq) + NaCl (aq) → AgCl (s) + NaNO₃ (aq)

Example of a Complete Ionic Equation Ag⁺ (aq) + NO₃⁻ (aq) + Na⁺ (aq) + Cl⁻ (aq) → AgCl (s) + Na⁺ (aq) + NO₃⁻ (aq)

Spectator Ions in AgNO₃ + NaCl Na⁺ (aq) and NO₃⁻ (aq), because they appear on both sides and don’t participate in the reaction.

Net Ionic Equation for AgNO₃ + NaCl Ag⁺ (aq) + Cl⁻ (aq) → AgCl (s)

Why Use Net Ionic Equations? 1. Simplifies reactions by removing unnecessary ions. 2. Helps predict precipitate formation. 3. Shows how ions interact in solution.