What do I do when writing the net ionic equation for Magnesium nitrate reacted with sodium chloride?

I've wrote out the molecular equation and the total ionic equation. Everything cancels out....under my total ionic equation do i just write no reaction? |thanks!

You're right. There is no reaction.

When writing the net ionic equation, you need to consider whether there is a reaction or not, based on the information provided.

To write the net ionic equation for the reaction between magnesium nitrate (Mg(NO3)2) and sodium chloride (NaCl), you should first write the balanced molecular equation:

Mg(NO3)2 + 2NaCl -> MgCl2 + 2NaNO3

Next, you can write the balanced total ionic equation, separating all the soluble compounds into their respective ions:

Mg2+ + 2NO3- + 2Na+ + 2Cl- -> Mg2+ + 2Cl- + 2Na+ + 2NO3-

After that, look for any ions that are present on both sides of the equation. In this case, we have Mg2+ and 2Cl-. Since they appear on both sides, we can cancel them out, as they are known as spectator ions.

The resulting net ionic equation for the reaction is:

NO3- + Na+ -> NaNO3

As you can see, the nitrate ion (NO3-) and the sodium ion (Na+) are the only ions involved in the reaction, forming sodium nitrate (NaNO3).

So, in conclusion, there is a net ionic equation for the given reaction, and it does not result in "no reaction."