Questions: Write the net ionic equation for the reaction of magnesium metal with aqueous silver nitrate. Include physical states. net ionic equation:

Write the net ionic equation for the reaction of magnesium metal with aqueous silver nitrate. Include physical states.
net ionic equation:

Transcript text: Write the net ionic equation for the reaction of magnesium metal with aqueous silver nitrate. Include physical states. net ionic equation: $\square$

Solution

Solution Steps

Step 1: Write the balanced molecular equation

First, we write the balanced molecular equation for the reaction between magnesium metal and aqueous silver nitrate:

\[ \text{Mg}(s) + 2\text{AgNO}_3(aq) \rightarrow \text{Mg(NO}_3\text{)}_2(aq) + 2\text{Ag}(s) \]

Step 2: Write the complete ionic equation

Next, we write the complete ionic equation by breaking all soluble strong electrolytes (aqueous compounds) into their ions:

\[ \text{Mg}(s) + 2\text{Ag}^+(aq) + 2\text{NO}_3^-(aq) \rightarrow \text{Mg}^{2+}(aq) + 2\text{NO}_3^-(aq) + 2\text{Ag}(s) \]

Step 3: Identify and cancel spectator ions

Spectator ions are ions that appear on both sides of the complete ionic equation and do not participate in the reaction. In this case, the nitrate ions ($\text{NO}_3^-$) are spectator ions:

\[ \text{Mg}(s) + 2\text{Ag}^+(aq) + \cancel{2\text{NO}_3^-(aq)} \rightarrow \text{Mg}^{2+}(aq) + \cancel{2\text{NO}_3^-(aq)} + 2\text{Ag}(s) \]

Step 4: Write the net ionic equation

After canceling the spectator ions, we are left with the net ionic equation:

\[ \text{Mg}(s) + 2\text{Ag}^+(aq) \rightarrow \text{Mg}^{2+}(aq) + 2\text{Ag}(s) \]