Write the net ionic equation for the following molecular equation.

3FeCl2(aq) + 2(NH4)3PO4(aq) Fe3(PO4)2(s) + 6NH4Cl(aq)

You add the aq.

3Fe^2+ + 6Cl^- + 6NH4^+ + 2PO4^3- ==> Fe3(PO4)2(s) + 6NH4+ + 6Cl^-

Now cancel the ions that are common to both sides; what is left is the net ionic equation.

To write the net ionic equation for the given molecular equation, we first need to start by writing the balanced molecular equation.

The balanced molecular equation is:
3FeCl2(aq) + 2(NH4)3PO4(aq) → Fe3(PO4)2(s) + 6NH4Cl(aq)

To write the net ionic equation, we need to cancel out the spectator ions (ions that do not participate in the reaction) that appear on both sides of the equation.

In this case, the spectator ions are the 6 ammonium ions (NH4+) and 6 chloride ions (Cl-) on the left side of the equation.

The net ionic equation is:
3Fe2+(aq) + 2PO43-(aq) → Fe3(PO4)2(s)

So, the net ionic equation for the given molecular equation is:
3Fe2+(aq) + 2PO43-(aq) → Fe3(PO4)2(s)

To write the net ionic equation for the given molecular equation, you need to first write out the balanced molecular equation and then identify the soluble compounds and the insoluble compound, which will be the precipitate. Then you can write the net ionic equation by eliminating the spectator ions.

Here's how you can do it step by step:

Step 1: Write the balanced molecular equation:
3FeCl2(aq) + 2(NH4)3PO4(aq) → Fe3(PO4)2(s) + 6NH4Cl(aq)

Step 2: Identify the soluble and insoluble compounds:
Soluble compounds include all ions that remain in solution after the reaction. In this case, FeCl2, NH4Cl, and (NH4)3PO4 are soluble.
The insoluble compound is Fe3(PO4)2, which is the precipitate formed.

Step 3: Write the complete ionic equation:
The complete ionic equation includes all the soluble ionic compounds in their fully dissociated form.
3Fe^2+(aq) + 6Cl^-(aq) + 6NH4+(aq) + 2PO4^3-(aq) → Fe3(PO4)2(s) + 6NH4+(aq) + 6Cl^-(aq)

Step 4: Write the net ionic equation:
The net ionic equation is obtained by removing the spectator ions that are present on both sides of the equation. In this case, NH4+ and Cl- are spectator ions.
The remaining ions involved in the reaction are:
Fe^2+(aq) + PO4^3-(aq) → Fe3(PO4)2(s)

Thus, the net ionic equation for the given molecular equation is:
Fe^2+(aq) + PO4^3-(aq) → Fe3(PO4)2(s)