To determine the net ionic equation of the given reaction, we need to follow these steps:
1. Write the full balanced reaction:
[tex]\[ Mg(s) + Zn^{2+} + 2 NO_3^- \rightarrow Mg^{2+} + 2 NO_3^- + Zn(s) \][/tex]
2. Identify the spectator ions:
Spectator ions are ions that do not change during the reaction. Here, the \( NO_3^- \) (nitrate) ions appear on both sides of the equation and do not change their form, so they are spectator ions.
3. Eliminate the spectator ions to find the net ionic equation:
After removing the spectator ions, we focus on the species that undergo a change:
[tex]\[ Mg(s) + Zn^{2+} \rightarrow Mg^{2+} + Zn(s) \][/tex]
This is the net ionic equation because it only includes the species that participate in the reaction, excluding the unchanged spectator ions.
Comparing with the given choices, the correct answer is:
A. \( Mg(s) + Zn^{2+} \rightarrow Mg^{2+} + Zn(s) \)
Hence, the net ionic equation for the given reaction is:
[tex]\[ Mg(s) + Zn^{2+} \rightarrow Mg^{2+} + Zn(s) \][/tex]
