# Write the complete ionic equation and the net ionic equation for the following reaction....

## Question:

Write the complete ionic equation and the net ionic equation for the following reaction.

{eq}3Cr(C_2H_3O_2)_2 + 2(NH_4)_3P \to 6NH_4C_2H_3O_2 + Cr_3P_2 {/eq}

## Net Ionic Equation:

We can simplify a chemical reaction that occurs in an aqueous solution by omitting the spectator ions. Spectator ions remain dissolved in the solution even after the chemical reaction has occurred. A net ionic equation summarizes the chemical equation in aqueous solution by omitting the spectator ions.

The given balanced molecular equation can be completed by writing the phases of each substance. The reaction is a precipitation reaction as Chromium(III) phosphide is formed. It is the precipitate for the given reaction when mixing the two solutions.

{eq}\rm molecular~equation: 3Cr(C_2H_3O_2)_2(aq) + 2(NH_4)_3P(aq) \to 6NH_4C_2H_3O_2(aq) + Cr_3P_2(s){/eq}

The next step is to separate the chemical equation into their respective ions. In doing so, we get the following complete ionic equation.

{eq}\rm complete~ionic~equation: 3Cr^{3+}(aq) + 2C_2H_3O_2^-(aq) + 6NH_4^+(aq) + 2P^{3-}(aq) \to 6NH_4^+(aq) + 6C_2H_3O_2^-(aq) + Cr_3P_2(s) {/eq}

By removing the acetate and ammonium ions, we obtain the following net ionic equation:

{eq}\rm net~ionic~equation: 3Cr^{3+}(aq) + 2P^{3-}(aq) \to Cr_3P_2(s) {/eq}