Complete ionic equation and net ionic equation for 2 K3PO4 + 3 Fe(NO3)2 --> 6 KNO3 + Fe3(PO4)2

To write the complete ionic equation, we need to first identify all the strong electrolytes and write them as ions. The compounds that are strong electrolytes and dissociate completely in solution are K3PO4, Fe(NO3)2, and KNO3.

The complete ionic equation is:

2 K⁺ + 3 PO₄³⁻ + 3 Fe²⁺ + 6 NO₃⁻ → 6 K⁺ + 6 NO₃⁻ + Fe₃(PO₄)₂

Next, we need to write the net ionic equation by removing the spectator ions, which are the ions that appear on both sides of the equation without taking part in the chemical reaction. In this case, the spectator ions are K⁺ and NO₃⁻.

The net ionic equation is:

3 PO₄³⁻ + 3 Fe²⁺ → Fe₃(PO₄)₂

Therefore, the complete ionic equation is 2 K⁺ + 3 PO₄³⁻ + 3 Fe²⁺ + 6 NO₃⁻ → 6 K⁺ + 6 NO₃⁻ + Fe₃(PO₄)₂, and the net ionic equation is 3 PO₄³⁻ + 3 Fe²⁺ → Fe₃(PO₄)₂.

To write the complete ionic equation and net ionic equation for the given reaction, we need to understand the concept of ionic compounds and how they dissociate in a solution.

Step 1: Write the balanced equation
The balanced equation for the given reaction is already provided:
2 K3PO4 + 3 Fe(NO3)2 → 6 KNO3 + Fe3(PO4)2

Step 2: Write the complete ionic equation
In the complete ionic equation, we will separate all the soluble ionic compounds into their respective ions.
2 K3PO4 (aq) + 3 Fe(NO3)2 (aq) → 6 KNO3 (aq) + Fe3(PO4)2 (s)

Now let's break down the soluble compounds into their respective ions:
2 K+ (aq) + 6 PO4^3- (aq) + 3 Fe2+ (aq) + 6 NO3- (aq) → 6 K+ (aq) + 6 NO3- (aq) + Fe3(PO4)2 (s)

Step 3: Write the net ionic equation
In the net ionic equation, we remove the spectator ions (ions that appear on both sides of the equation and do not directly participate in the reaction).
The spectator ions in this reaction are the potassium ions (K+) and the nitrate ions (NO3-), which are present on both sides of the equation. Therefore, they can be removed.

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

So, the complete ionic equation for the reaction is 2 K3PO4 (aq) + 3 Fe(NO3)2 (aq) → 6 KNO3 (aq) + Fe3(PO4)2 (s), and the net ionic equation is 6 PO4^3- (aq) + 3 Fe^2+ (aq) → Fe3(PO4)2 (s).

We have a problem here. You have Fe^2+ on the left and Fe^3+ on the right which means Fe has been oxidized. But there is no reduction. You can't have oxidation without reduction. I expect you meant Fe(NO3)3 on the left