Net Ionic Equation Chemistry Example 1

Follow the full solution, then compare it with the other examples linked below.

Example 1

easy
Explain the difference between a molecular equation, a complete ionic equation, and a net ionic equation. Use the reaction of NaCl(aq)+AgNO3(aq)\text{NaCl(aq)} + \text{AgNO}_3\text{(aq)} as an example.

Solution

  1. 1
    Molecular equation shows all species as complete formulas: NaCl(aq)+AgNO3(aq)→AgCl(s)+NaNO3(aq)\text{NaCl(aq)} + \text{AgNO}_3\text{(aq)} \rightarrow \text{AgCl(s)} + \text{NaNO}_3\text{(aq)}.
  2. 2
    Complete ionic equation splits all aqueous ionic compounds into their ions: Na+(aq)+Cl−(aq)+Ag+(aq)+NO3−(aq)→AgCl(s)+Na+(aq)+NO3−(aq)\text{Na}^+\text{(aq)} + \text{Cl}^-\text{(aq)} + \text{Ag}^+\text{(aq)} + \text{NO}_3^-\text{(aq)} \rightarrow \text{AgCl(s)} + \text{Na}^+\text{(aq)} + \text{NO}_3^-\text{(aq)}.
  3. 3
    Net ionic equation removes spectator ions (Na+\text{Na}^+ and NO3−\text{NO}_3^-) that appear unchanged on both sides: Ag+(aq)+Cl−(aq)→AgCl(s)\text{Ag}^+\text{(aq)} + \text{Cl}^-\text{(aq)} \rightarrow \text{AgCl(s)}.

Answer

Ag+(aq)+Cl−(aq)→AgCl(s)\text{Ag}^+\text{(aq)} + \text{Cl}^-\text{(aq)} \rightarrow \text{AgCl(s)}
The net ionic equation shows only the species that actually participate in the chemical change. Spectator ions are present in solution but do not undergo any change — they merely 'watch' the reaction.

About Net Ionic Equation

A simplified chemical equation that shows only the ions and molecules directly involved in a chemical reaction, with all spectator ions (those unchanged on both.

Learn more about Net Ionic Equation →

More Net Ionic Equation Examples

Example 2 medium

Write the net ionic equation for the reaction between [formula] and [formula].

Example 3 medium

Write the net ionic equation for the neutralization of hydrochloric acid with sodium hydroxide: [for

Example 4 hard

Write the net ionic equation for the reaction: [formula]. Identify all spectator ions.

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