Nomenclature Worksheet 4: Ionic Compounds Containing Transition Metals - a table with 16 entries for naming and writing formulas of ionic compounds involving transition metals.

Here’s the completed table with explanations for each compound. We’ll use standard ionic compound naming rules: name = cation + anion, and formula = balance charges to make neutral compound.

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✔ Completed Table:

| # | Name of Ionic Compound | Formula of Ionic Compound |
|---|--------------------------------|---------------------------|
| 1 | Copper (II) sulfate | CuSO₄ |
| 2 | Copper (I) oxide | Cu₂O |
| 3 | Chromium (III) cyanide | Cr(CN)₃ |
| 4 | Cobalt (II) hydroxide | Co(OH)₂ |
| 5 | Silver bromide | AgBr |
| 6 | Zinc nitrate | Zn(NO₃)₂ |
| 7 | Iron (III) acetate | Fe(C₂H₃O₂)₃ or Fe(CH₃COO)₃ |
| 8 | Lead (IV) sulfate | Pb(SO₄)₂ |
| 9 | Iron (II) chloride | FeCl₂ |
|10 | Lead (II) sulfite | PbSO₃ |
|11 | Cobalt (III) carbonate | Co₂(CO₃)₃ |
|12 | Silver nitrate | AgNO₃ |
|13 | Zinc cyanide | Zn(CN)₂ |
|14 | Copper (I) chlorate | CuClO₃ |
|15 | Chromium (III) hydroxide | Cr(OH)₃ |
|16 | Mercury (I) oxide | Hg₂O |

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## 🔍 Detailed Explanations:

1. Copper (II) sulfate

- Cu²⁺ and SO₄²⁻ → charges cancel directly → CuSO₄

2. Copper (I) oxide

- Cu⁺ and O²⁻ → need 2 Cu⁺ to balance 1 O²⁻ → Cu₂O

3. Chromium (III) cyanide

- Cr³⁺ and CN⁻ → need 3 CN⁻ to balance Cr³⁺ → Cr(CN)₃

4. Cobalt (II) hydroxide

- Co²⁺ and OH⁻ → need 2 OH⁻ → Co(OH)₂

5. Silver bromide

- Ag⁺ and Br⁻ → 1:1 ratio → AgBr

6. Zinc nitrate

- Zn²⁺ and NO₃⁻ → need 2 NO₃⁻ → Zn(NO₃)₂

7. Iron (III) acetate

- Fe³⁺ and CH₃COO⁻ (acetate, C₂H₃O₂⁻) → need 3 acetates → Fe(C₂H₃O₂)₃

8. Lead (IV) sulfate

- Pb⁴⁺ and SO₄²⁻ → need 2 SO₄²⁻ to balance Pb⁴⁺ → Pb(SO₄)₂

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9. FeCl₂ → Iron (II) chloride

- Fe²⁺ and Cl⁻ → 2 Cl⁻ needed → name: Iron (II) chloride

10. PbSO₃ → Lead (II) sulfite

- Pb²⁺ and SO₃²⁻ → 1:1 → name: Lead (II) sulfite
*(Note: Pb can have multiple charges, but here charge is +2 to balance SO₃²⁻)*

11. Co₂(CO₃)₃ → Cobalt (III) carbonate

- Two Co ions, three CO₃²⁻ → total anion charge = 3 × (-2) = -6 → each Co must be +3 → Cobalt (III) carbonate

12. AgNO₃ → Silver nitrate

- Ag⁺ and NO₃⁻ → 1:1 → Silver nitrate (silver only has +1 charge)

13. Zn(CN)₂ → Zinc cyanide

- Zn²⁺ and CN⁻ → two CN⁻ → Zinc cyanide

14. CuClO₃ → Copper (I) chlorate

- ClO₃⁻ is -1, so Cu must be +1 → Copper (I) chlorate

15. Cr(OH)₃ → Chromium (III) hydroxide

- Three OH⁻ = -3, so Cr = +3 → Chromium (III) hydroxide

16. Hg₂O → Mercury (I) oxide

- Hg₂²⁺ (mercury(I) is diatomic ion) and O²⁻ → 1:1 → Mercury (I) oxide
*(Important: Mercury(I) is Hg₂²⁺, not Hg⁺)*

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## 📝 Key Rules Used:
- Charge Balance: Total positive charge = total negative charge.
- Roman numerals: Used for transition metals with variable charge (e.g., Fe, Cu, Cr, Co, Pb, Hg).
- Polyatomic ions: Memorize common ones (SO₄²⁻, NO₃⁻, OH⁻, CN⁻, CO₃²⁻, ClO₃⁻, etc.).
- Mercury(I): Always Hg₂²⁺ — never Hg⁺ alone.

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✔ All formulas and names are now correctly matched based on ionic charge balancing and standard nomenclature rules.