In order to write the complete ionic equation for a reaction, we first need a specific chemical reaction to work with. However, I can illustrate the process using a common example: the reaction of sodium chloride (NaCl) with silver nitrate (AgNO₃) in aqueous solution.
Step 1: The Balanced Molecular Equation
The balanced molecular equation for the reaction is:
\[ \text{NaCl (aq)} + \text{AgNO}_3 \text{ (aq)} \rightarrow \text{NaNO}_3 \text{ (aq)} + \text{AgCl (s)} \]
Step 2: Writing the Complete Ionic Equation
Next, we'll break down the soluble ionic compounds into their constituent ions:
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Reactants:
- NaCl (aq) dissociates into Na⁺ (aq) and Cl⁻ (aq)
- AgNO₃ (aq) dissociates into Ag⁺ (aq) and NO₃⁻ (aq)
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Products:
- NaNO₃ (aq) dissociates into Na⁺ (aq) and NO₃⁻ (aq)
- AgCl is insoluble and does not dissociate, remaining as AgCl (s)
The complete ionic equation is:
\[ \text{Na}^+ \text{(aq)} + \text{Cl}^- \text{(aq)} + \text{Ag}^+ \text{(aq)} + \text{NO}_3^- \text{(aq)} \rightarrow \text{Na}^+ \text{(aq)} + \text{NO}_3^- \text{(aq)} + \text{AgCl (s)} \]
Step 3: Writing the Net Ionic Equation
In the complete ionic equation, the sodium ions (Na⁺) and nitrate ions (NO₃⁻) appear on both sides of the equation and can be removed as they are spectator ions. The net ionic equation, which shows only the species that participate in forming the precipitate, is:
\[ \text{Ag}^+ \text{(aq)} + \text{Cl}^- \text{(aq)} \rightarrow \text{AgCl (s)} \]
Summary
In this example:
- Dissociated molecules included NaCl (dissociating into Na⁺ and Cl⁻) and AgNO₃ (dissociating into Ag⁺ and NO₃⁻).
- The insoluble product formed was AgCl, which did not dissociate.
If you have a different reaction in mind, please specify, and I can help with that!
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