A student mixes aqueous solutions of lead(II) nitrate, \(\text{Pb(NO}_3)_2\text{(aq)}\), and potassium iodide, \(\text{KI(aq)}\). A precipitate of lead(II) iodide, \(\text{PbI}_2\text{(s)}\), forms according to the balanced net ionic equation below.

\[\text{Pb}^{2+}\text{(aq)} + 2\,\text{I}^-\text{(aq)} \rightarrow \text{PbI}_2\text{(s)}\]

The diagram below represents the aqueous mixture immediately upon mixing but before any reaction occurs, containing \(3\) \(\text{Pb}^{2+}\) ions, \(4\) \(\text{I}^-\) ions, \(4\) \(\text{K}^+\) ions, and \(6\) \(\text{NO}_3^-\) ions (solvent water molecules are omitted for clarity). Assuming the reaction proceeds to completion, which of the following particulate diagrams best represents the contents of the container at the end of the reaction?