Worksheet for practicing naming and writing formulas of ionic compounds with transition metals.

To solve the problem, we need to fill in the table by converting the names of ionic compounds to their chemical formulas and vice versa. Let's go through each entry step by step.

Part 1: Converting Names to Formulas

#### 1. Copper (II) sulfate
- Copper (II) has a charge of +2: \( \text{Cu}^{2+} \)
- Sulfate ion has a charge of -2: \( \text{SO}_4^{2-} \)
- The charges balance, so the formula is:
\[
\boxed{\text{CuSO}_4}
\]

#### 2. Copper (I) oxide
- Copper (I) has a charge of +1: \( \text{Cu}^+ \)
- Oxide ion has a charge of -2: \( \text{O}^{2-} \)
- To balance the charges, we need 2 copper (I) ions for every 1 oxide ion:
\[
\boxed{\text{Cu}_2\text{O}}
\]

#### 3. Chromium (III) cyanide
- Chromium (III) has a charge of +3: \( \text{Cr}^{3+} \)
- Cyanide ion has a charge of -1: \( \text{CN}^- \)
- To balance the charges, we need 3 cyanide ions for every 1 chromium (III) ion:
\[
\boxed{\text{Cr(CN)}_3}
\]

#### 4. Cobalt (II) hydroxide
- Cobalt (II) has a charge of +2: \( \text{Co}^{2+} \)
- Hydroxide ion has a charge of -1: \( \text{OH}^- \)
- To balance the charges, we need 2 hydroxide ions for every 1 cobalt (II) ion:
\[
\boxed{\text{Co(OH)}_2}
\]

#### 5. Silver bromide
- Silver has a charge of +1: \( \text{Ag}^+ \)
- Bromide ion has a charge of -1: \( \text{Br}^- \)
- The charges balance, so the formula is:
\[
\boxed{\text{AgBr}}
\]

#### 6. Zinc nitrate
- Zinc has a charge of +2: \( \text{Zn}^{2+} \)
- Nitrate ion has a charge of -1: \( \text{NO}_3^- \)
- To balance the charges, we need 2 nitrate ions for every 1 zinc ion:
\[
\boxed{\text{Zn(NO}_3)_2}
\]

#### 7. Iron (III) acetate
- Iron (III) has a charge of +3: \( \text{Fe}^{3+} \)
- Acetate ion has a charge of -1: \( \text{CH}_3\text{COO}^- \)
- To balance the charges, we need 3 acetate ions for every 1 iron (III) ion:
\[
\boxed{\text{Fe(CH}_3\text{COO)}_3}
\]

#### 8. Lead (IV) sulfate
- Lead (IV) has a charge of +4: \( \text{Pb}^{4+} \)
- Sulfate ion has a charge of -2: \( \text{SO}_4^{2-} \)
- To balance the charges, we need 2 sulfate ions for every 1 lead (IV) ion:
\[
\boxed{\text{Pb(SO}_4)_2}
\]

Part 2: Converting Formulas to Names

#### 9. \( \text{FeCl}_2 \)
- Iron (Fe) has a charge of +2 (since it is FeCl₂, not FeCl₃).
- Chloride ion has a charge of -1.
- The name is:
\[
\boxed{\text{Iron (II) chloride}}
\]

#### 10. \( \text{PbSO}_3 \)
- Lead (Pb) has a charge of +2 (since it is PbSO₃, not PbSO₄).
- Sulfite ion has a charge of -2.
- The name is:
\[
\boxed{\text{Lead (II) sulfite}}
\]

#### 11. \( \text{Co}_2(\text{CO}_3)_3 \)
- Cobalt (Co) has a charge of +3 (since there are 2 Co atoms and 3 carbonate ions).
- Carbonate ion has a charge of -2.
- The name is:
\[
\boxed{\text{Cobalt (III) carbonate}}
\]

#### 12. \( \text{AgNO}_3 \)
- Silver (Ag) has a charge of +1.
- Nitrate ion has a charge of -1.
- The name is:
\[
\boxed{\text{Silver nitrate}}
\]

#### 13. \( \text{Zn(CN)}_2 \)
- Zinc (Zn) has a charge of +2.
- Cyanide ion has a charge of -1.
- The name is:
\[
\boxed{\text{Zinc cyanide}}
\]

#### 14. \( \text{CuClO}_3 \)
- Copper (Cu) has a charge of +2.
- Chlorate ion has a charge of -1.
- The name is:
\[
\boxed{\text{Copper (II) chlorate}}
\]

#### 15. \( \text{Cr(OH)}_3 \)
- Chromium (Cr) has a charge of +3.
- Hydroxide ion has a charge of -1.
- The name is:
\[
\boxed{\text{Chromium (III) hydroxide}}
\]

#### 16. \( \text{Hg}_2\text{O} \)
- Mercury (Hg) in this compound forms a dimeric cation \( \text{Hg}_2^{2+} \) with a charge of +2.
- Oxide ion has a charge of -2.
- The name is:
\[
\boxed{\text{Mercury (I) oxide}}
\]

Final Answer:

\[
\boxed{
\begin{array}{|c|c|}
\hline
\text{Name of Ionic Compound} & \text{Formula of Ionic Compound} \\
\hline
1. \text{Copper (II) sulfate} & \text{CuSO}_4 \\
2. \text{Copper (I) oxide} & \text{Cu}_2\text{O} \\
3. \text{Chromium (III) cyanide} & \text{Cr(CN)}_3 \\
4. \text{Cobalt (II) hydroxide} & \text{Co(OH)}_2 \\
5. \text{Silver bromide} & \text{AgBr} \\
6. \text{Zinc nitrate} & \text{Zn(NO}_3)_2 \\
7. \text{Iron (III) acetate} & \text{Fe(CH}_3\text{COO)}_3 \\
8. \text{Lead (IV) sulfate} & \text{Pb(SO}_4)_2 \\
9. & \text{FeCl}_2 \\
10. & \text{PbSO}_3 \\
11. & \text{Co}_2(\text{CO}_3)_3 \\
12. & \text{AgNO}_3 \\
13. & \text{Zn(CN)}_2 \\
14. & \text{CuClO}_3 \\
15. & \text{Cr(OH)}_3 \\
16. & \text{Hg}_2\text{O} \\
\hline
\end{array}
}
\]