Questions: Fill in the name and empirical formula of each ionic compound that could be formed from - cation: Zn^2+, anion: NO2^-, empirical formula: , name of compound: - cation: Cu^2+, anion: ClO^-, empirical formula: , name of compound: - cation: Pb^2+, anion: SO3^2-, empirical formula: , name of compound: - cation: Ba^2+, anion: IO2^-, empirical formula: , name of compound:

Fill in the name and empirical formula of each ionic compound that could be formed from

- cation: Zn^2+, anion: NO2^-, empirical formula: , name of compound:
- cation: Cu^2+, anion: ClO^-, empirical formula: , name of compound:
- cation: Pb^2+, anion: SO3^2-, empirical formula: , name of compound:
- cation: Ba^2+, anion: IO2^-, empirical formula: , name of compound:

Transcript text: Fill in the name and empirical formula of each ionic compound that could be formed from \begin{tabular}{|c|c|c|c|} \hline \multicolumn{4}{|c|}{ some ionic compounds } \\ \hline cation & anion & empirical formula & name of compound \\ \hline $\mathrm{Zn}^{2+}$ & $\mathrm{NO}_{2}^{-}$ & $\square$ & $\square$ \\ \hline $\mathrm{Cu}^{2+}$ & $\mathrm{ClO}^{-}$ & $\square$ & $\square$ \\ \hline $\mathrm{Pb}^{2+}$ & $\mathrm{SO}_{3}^{2-}$ & $\square$ & $\square$ \\ \hline $\mathrm{Ba}^{2+}$ & $\mathrm{IO}_{2}^{-}$ & $\square$ & $\square$ \\ \hline \end{tabular}

Solution

Solution Steps

Step 1: Identify the cation and anion for each compound

We are given pairs of cations and anions. We need to combine them to form neutral ionic compounds.

Step 2: Determine the empirical formula

To form a neutral compound, the total positive charge must equal the total negative charge. We will balance the charges for each pair.

For $\mathrm{Zn}^{2+}$ and $\mathrm{NO}_{2}^{-}$:
- $\mathrm{Zn}^{2+}$ has a charge of +2.
- $\mathrm{NO}_{2}^{-}$ has a charge of -1.
- We need two $\mathrm{NO}_{2}^{-}$ ions to balance one $\mathrm{Zn}^{2+}$ ion.
- Empirical formula: $\mathrm{Zn}(\mathrm{NO}_{2})_{2}$
For $\mathrm{Cu}^{2+}$ and $\mathrm{ClO}^{-}$:
- $\mathrm{Cu}^{2+}$ has a charge of +2.
- $\mathrm{ClO}^{-}$ has a charge of -1.
- We need two $\mathrm{ClO}^{-}$ ions to balance one $\mathrm{Cu}^{2+}$ ion.
- Empirical formula: $\mathrm{Cu}(\mathrm{ClO})_{2}$
For $\mathrm{Pb}^{2+}$ and $\mathrm{SO}_{3}^{2-}$:
- $\mathrm{Pb}^{2+}$ has a charge of +2.
- $\mathrm{SO}_{3}^{2-}$ has a charge of -2.
- One $\mathrm{Pb}^{2+}$ ion balances one $\mathrm{SO}_{3}^{2-}$ ion.
- Empirical formula: $\mathrm{PbSO}_{3}$
For $\mathrm{Ba}^{2+}$ and $\mathrm{IO}_{2}^{-}$:
- $\mathrm{Ba}^{2+}$ has a charge of +2.
- $\mathrm{IO}_{2}^{-}$ has a charge of -1.
- We need two $\mathrm{IO}_{2}^{-}$ ions to balance one $\mathrm{Ba}^{2+}$ ion.
- Empirical formula: $\mathrm{Ba}(\mathrm{IO}_{2})_{2}$

Step 3: Name the compounds

We will use standard naming conventions for ionic compounds.

$\mathrm{Zn}(\mathrm{NO}_{2})_{2}$:
- Name: Zinc nitrite
$\mathrm{Cu}(\mathrm{ClO})_{2}$:
- Name: Copper(I) hypochlorite
$\mathrm{PbSO}_{3}$:
- Name: Lead(II) sulfite
$\mathrm{Ba}(\mathrm{IO}_{2})_{2}$:
- Name: Barium iodite

Final Answer

\[ \begin{array}{|c|c|c|c|} \hline \text{cation} & \text{anion} & \text{empirical formula} & \text{name of compound} \\ \hline \mathrm{Zn}^{2+} & \mathrm{NO}_{2}^{-} & \boxed{\mathrm{Zn}(\mathrm{NO}_{2})_{2}} & \boxed{\text{Zinc nitrite}} \\ \hline \mathrm{Cu}^{2+} & \mathrm{ClO}^{-} & \boxed{\mathrm{Cu}(\mathrm{ClO})_{2}} & \boxed{\text{Copper(I) hypochlorite}} \\ \hline \mathrm{Pb}^{2+} & \mathrm{SO}_{3}^{2-} & \boxed{\mathrm{PbSO}_{3}} & \boxed{\text{Lead(II) sulfite}} \\ \hline \mathrm{Ba}^{2+} & \mathrm{IO}_{2}^{-} & \boxed{\mathrm{Ba}(\mathrm{IO}_{2})_{2}} & \boxed{\text{Barium iodite}} \\ \hline \end{array} \]

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