Net Ionic Equation Worksheet Answers | Study notes Chemistry | Docsity - Free Printable

Problem Overview:

The task involves writing balanced molecular, complete ionic, and net ionic equations for two chemical reactions. The reactions are:
1. Sodium chloride (NaCl) and silver nitrate (AgNO₃)
2. Sodium hydroxide (NaOH) and iron(II) carbonate (FeCO₃)

We will solve each reaction step by step.

---

Reaction 1: Sodium Chloride (NaCl) and Silver Nitrate (AgNO₃)

#### Step 1: Molecular Equation
Sodium chloride (NaCl) reacts with silver nitrate (AgNO₃) to form silver chloride (AgCl), which is insoluble in water (a precipitate), and sodium nitrate (NaNO₃).

- Balanced molecular equation:
\[
\text{NaCl}_{(aq)} + \text{AgNO}_3{}_{(aq)} \rightarrow \text{AgCl}_{(s)} + \text{NaNO}_3{}_{(aq)}
\]

#### Step 2: Complete Ionic Equation
In the complete ionic equation, all soluble ionic compounds are written as their dissociated ions. Insoluble compounds (precipitates) remain as molecules.

- Dissociation of NaCl:
\[
\text{NaCl}_{(aq)} \rightarrow \text{Na}^+{}_{(aq)} + \text{Cl}^-{}_{(aq)}
\]
- Dissociation of AgNO₃:
\[
\text{AgNO}_3{}_{(aq)} \rightarrow \text{Ag}^+{}_{(aq)} + \text{NO}_3^-{}_{(aq)}
\]
- Dissociation of NaNO₃ (soluble):
\[
\text{NaNO}_3{}_{(aq)} \rightarrow \text{Na}^+{}_{(aq)} + \text{NO}_3^-{}_{(aq)}
\]

Putting it together:
\[
\text{Na}^+{}_{(aq)} + \text{Cl}^-{}_{(aq)} + \text{Ag}^+{}_{(aq)} + \text{NO}_3^-{}_{(aq)} \rightarrow \text{AgCl}_{(s)} + \text{Na}^+{}_{(aq)} + \text{NO}_3^-{}_{(aq)}
\]

#### Step 3: Net Ionic Equation
The net ionic equation is obtained by eliminating spectator ions (ions that appear on both sides of the equation). Here, \(\text{Na}^+\) and \(\text{NO}_3^-\) are spectator ions.

Removing spectator ions:
\[
\text{Cl}^-{}_{(aq)} + \text{Ag}^+{}_{(aq)} \rightarrow \text{AgCl}_{(s)}
\]

#### Particulate Drawing
For the particulate drawing, represent atoms as small circles:
- \(\text{Cl}^-\): One circle labeled "Cl" with a negative charge.
- \(\text{Ag}^+\): One circle labeled "Ag" with a positive charge.
- \(\text{AgCl}\): A pair of circles labeled "Ag" and "Cl" bonded together, representing the solid precipitate.

---

Reaction 2: Sodium Hydroxide (NaOH) and Iron(II) Carbonate (FeCO₃)

#### Step 1: Molecular Equation
Sodium hydroxide (NaOH) reacts with iron(II) carbonate (FeCO₃). However, FeCO₃ is already an insoluble salt, so no reaction occurs between these two substances in aqueous solution. Therefore, the molecular equation is:

\[
\text{No reaction}
\]

#### Step 2: Complete Ionic Equation
Since there is no reaction, there is no complete ionic equation to write.

#### Step 3: Net Ionic Equation
Similarly, since there is no reaction, there is no net ionic equation to write.

#### Particulate Drawing
For the particulate drawing, represent atoms as small circles:
- \(\text{NaOH}\): One \(\text{Na}^+\) ion and one \(\text{OH}^-\) ion.
- \(\text{FeCO}_3\): Represented as a solid compound with \(\text{Fe}^{2+}\) and \(\text{CO}_3^{2-}\) ions bonded together.

---

Final Answers

#### Reaction 1: Sodium Chloride and Silver Nitrate
1. Molecular Equation:
\[
\boxed{\text{NaCl}_{(aq)} + \text{AgNO}_3{}_{(aq)} \rightarrow \text{AgCl}_{(s)} + \text{NaNO}_3{}_{(aq)}}
\]
2. Complete Ionic Equation:
\[
\boxed{\text{Na}^+{}_{(aq)} + \text{Cl}^-{}_{(aq)} + \text{Ag}^+{}_{(aq)} + \text{NO}_3^-{}_{(aq)} \rightarrow \text{AgCl}_{(s)} + \text{Na}^+{}_{(aq)} + \text{NO}_3^-{}_{(aq)}}
\]
3. Net Ionic Equation:
\[
\boxed{\text{Cl}^-{}_{(aq)} + \text{Ag}^+{}_{(aq)} \rightarrow \text{AgCl}_{(s)}}
\]

#### Reaction 2: Sodium Hydroxide and Iron(II) Carbonate
1. Molecular Equation:
\[
\boxed{\text{No reaction}}
\]
2. Complete Ionic Equation:
\[
\boxed{\text{No reaction}}
\]
3. Net Ionic Equation:
\[
\boxed{\text{No reaction}}
\]

---

Boxed Final Answer

\[
\boxed{
\begin{aligned}
&\text{Reaction 1:} \\
&\text{Molecular Equation: } \text{NaCl}_{(aq)} + \text{AgNO}_3{}_{(aq)} \rightarrow \text{AgCl}_{(s)} + \text{NaNO}_3{}_{(aq)} \\
&\text{Complete Ionic Equation: } \text{Na}^+{}_{(aq)} + \text{Cl}^-{}_{(aq)} + \text{Ag}^+{}_{(aq)} + \text{NO}_3^-{}_{(aq)} \rightarrow \text{AgCl}_{(s)} + \text{Na}^+{}_{(aq)} + \text{NO}_3^-{}_{(aq)} \\
&\text{Net Ionic Equation: } \text{Cl}^-{}_{(aq)} + \text{Ag}^+{}_{(aq)} \rightarrow \text{AgCl}_{(s)} \\
\\
&\text{Reaction 2:} \\
&\text{Molecular Equation: } \text{No reaction} \\
&\text{Complete Ionic Equation: } \text{No reaction} \\
&\text{Net Ionic Equation: } \text{No reaction}
\end{aligned}
}
\]