A bar of strontium metal is immersed in a 1.0 M copper(ll) nitrate solution. write the net ionic. I have the molecular formula written out but im not sure how to write the net ionic for this single displacement reaction
Separate the molecular equation into ions using the following rules.
1. If the substance is soluble, show the ions with (aq) after + and - ions.
2. If a gas so that as a molecule and write (g) after it.
3. If a solid, show it as the molecule and write (s) after it.
4. If a weakly ionized material (i.e., such as H2O), write it as the molecule and (l) after it. What you will have here is the full ionic equation.
Then cancel anything on the reactant side that is the same thing on the product side. What's left is the net ionic equation.
If you have trouble, post your full molecular equation.
To write the net ionic equation for a single displacement reaction, you need to first write the balanced molecular equation and then convert it into an ionic equation.
Here is the balanced molecular equation for the reaction:
Sr(s) + Cu(NO3)2(aq) -> Cu(s) + Sr(NO3)2(aq)
Now, let's convert this into an ionic equation by representing the soluble ionic compounds as dissociated ions:
Sr(s) + Cu^2+(aq) + 2NO3^-(aq) -> Cu(s) + Sr^2+(aq) + 2NO3^-(aq)
Note that the nitrate ion (NO3-) remains unchanged on both sides of the equation. Now, we can cancel out the spectator ions, which are the ions that appear on both sides of the equation and do not participate in the reaction. In this case, the nitrate ions (NO3-) are spectator ions, so we can eliminate them:
Sr(s) + Cu^2+(aq) -> Cu(s) + Sr^2+(aq)
Finally, we can write the net ionic equation by removing the spectator ions from the ionic equation:
Sr(s) + Cu^2+(aq) -> Cu(s) + Sr^2+(aq)
So, the net ionic equation for the given single displacement reaction is Sr(s) + Cu^2+(aq) -> Cu(s) + Sr^2+(aq).