Chemistry worksheet titled 'Ionic & Covalent Compound Naming Race' featuring a table where students identify compound types and write formulas.

Task Overview:

The task requires identifying whether each compound is ionic or covalent and writing the correct chemical formula for each compound. Let's solve this step by step.

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Key Concepts:

1. Ionic Compounds:
- Formed between a metal and a nonmetal (or a polyatomic ion).
- Typically involve electrostatic forces.
- Examples: Sodium chloride (NaCl), Calcium bromate (Ca(BrO₃)₂).

2. Covalent Compounds:
- Formed between two nonmetals.
- Involve sharing of electrons.
- Examples: Water (H₂O), Carbon dioxide (CO₂).

3. Rules for Naming and Formula Writing:
- Ionic Compounds:
- Use Roman numerals for transition metals to indicate their charge.
- Polyatomic ions have specific names and formulas (e.g., chlorite = ClO₂⁻, permanganate = MnO₄⁻).
- Covalent Compounds:
- Use prefixes to indicate the number of atoms of each element (e.g., di-, tri-, tetra-).
- The ending "-ide" is used for binary compounds.

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Solution:

#### Step 1: Identify Ionic or Covalent
We will analyze each compound based on its composition (metal/nonmetal) and naming conventions.

#### Step 2: Write Correct Chemical Formulas
For each compound, we will ensure the formula adheres to the rules of ionic or covalent bonding.

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Compound Analysis and Solutions:

#### 1. Copper (II) Chlorite
- Type: Ionic (copper is a metal, and chlorite is a polyatomic ion).
- Formula: Cu(ClO₂)₂ (Corrected from Cu(ClO)).
- Copper (Cu²⁺) has a +2 charge.
- Chlorite (ClO₂⁻) has a -1 charge.
- To balance charges: 1 Cu²⁺ and 2 ClO₂⁻.

#### 2. Sodium Hydroxide
- Type: Ionic (sodium is a metal, and hydroxide is a polyatomic ion).
- Formula: NaOH (Correct).
- Sodium (Na⁺) has a +1 charge.
- Hydroxide (OH⁻) has a -1 charge.
- Charges are already balanced.

#### 3. Nitrogen Dioxide
- Type: Covalent (both nitrogen and oxygen are nonmetals).
- Formula: NO₂ (Correct).
- No need for balancing charges in covalent compounds.

#### 4. Cobalt (III) Oxalate
- Type: Ionic (cobalt is a metal, and oxalate is a polyatomic ion).
- Formula: Co₂(C₂O₄)₃ (Corrected from Co₂(C₂O₄)₃).
- Cobalt (Co³⁺) has a +3 charge.
- Oxalate (C₂O₄²⁻) has a -2 charge.
- To balance charges: 2 Co³⁺ and 3 C₂O₄²⁻.

#### 5. Ammonium Sulfide
- Type: Ionic (ammonium is a polyatomic cation, and sulfide is a polyatomic anion).
- Formula: (NH₄)₂S (Corrected from (NH₄)₂S).
- Ammonium (NH₄⁺) has a +1 charge.
- Sulfide (S²⁻) has a -2 charge.
- To balance charges: 2 NH₄⁺ and 1 S²⁻.

#### 6. Aluminum Cyanide
- Type: Ionic (aluminum is a metal, and cyanide is a polyatomic ion).
- Formula: Al(CN)₃ (Corrected from Al(CN)₃).
- Aluminum (Al³⁺) has a +3 charge.
- Cyanide (CN⁻) has a -1 charge.
- To balance charges: 1 Al³⁺ and 3 CN⁻.

#### 7. Carbon Disulfide
- Type: Covalent (both carbon and sulfur are nonmetals).
- Formula: CS₂ (Correct).
- No need for balancing charges in covalent compounds.

#### 8. Tetraphosphorous Pentoxide
- Type: Covalent (both phosphorus and oxygen are nonmetals).
- Formula: P₄O₁₀ (Corrected from P₄O₅).
- The name indicates 4 phosphorus atoms and 10 oxygen atoms.

#### 9. Potassium Permanganate
- Type: Ionic (potassium is a metal, and permanganate is a polyatomic ion).
- Formula: KMnO₄ (Correct).
- Potassium (K⁺) has a +1 charge.
- Permanganate (MnO₄⁻) has a -1 charge.
- Charges are already balanced.

#### 10. Manganese (III) Chloride
- Type: Ionic (manganese is a metal, and chloride is a polyatomic ion).
- Formula: MnCl₃ (Correct).
- Manganese (Mn³⁺) has a +3 charge.
- Chloride (Cl⁻) has a -1 charge.
- To balance charges: 1 Mn³⁺ and 3 Cl⁻.

#### 11. Calcium Bromate
- Type: Ionic (calcium is a metal, and bromate is a polyatomic ion).
- Formula: Ca(BrO₃)₂ (Correct).
- Calcium (Ca²⁺) has a +2 charge.
- Bromate (BrO₃⁻) has a -1 charge.
- To balance charges: 1 Ca²⁺ and 2 BrO₃⁻.

#### 12. Carbon Monoxide
- Type: Covalent (both carbon and oxygen are nonmetals).
- Formula: CO (Correct).
- No need for balancing charges in covalent compounds.

#### 13. Potassium Oxide
- Type: Ionic (potassium is a metal, and oxide is a polyatomic ion).
- Formula: K₂O (Corrected from K₂O).
- Potassium (K⁺) has a +1 charge.
- Oxide (O²⁻) has a -2 charge.
- To balance charges: 2 K⁺ and 1 O²⁻.

#### 14. Antimony Tribromide
- Type: Ionic (antimony is a metal, and bromide is a polyatomic ion).
- Formula: SbBr₃ (Correct).
- Antimony (Sb³⁺) has a +3 charge.
- Bromide (Br⁻) has a -1 charge.
- To balance charges: 1 Sb³⁺ and 3 Br⁻.

#### 15. Zinc Phosphate
- Type: Ionic (zinc is a metal, and phosphate is a polyatomic ion).
- Formula: Zn₃(PO₄)₂ (Correct).
- Zinc (Zn²⁺) has a +2 charge.
- Phosphate (PO₄³⁻) has a -3 charge.
- To balance charges: 3 Zn²⁺ and 2 PO₄³⁻.

#### 16. Copper (II) Bicarbonate
- Type: Ionic (copper is a metal, and bicarbonate is a polyatomic ion).
- Formula: Cu(HCO₃)₂ (Correct).
- Copper (Cu²⁺) has a +2 charge.
- Bicarbonate (HCO₃⁻) has a -1 charge.
- To balance charges: 1 Cu²⁺ and 2 HCO₃⁻.

#### 17. Dinitrogen Tetroxide
- Type: Covalent (both nitrogen and oxygen are nonmetals).
- Formula: N₂O₄ (Correct).
- No need for balancing charges in covalent compounds.

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Final Answer:

Here is the completed table with the corrected information:

| Compound Name | Type of Compound | Chemical Formula |
|------------------------------|------------------|-------------------|
| 1. Copper (II) Chlorite | Ionic | Cu(ClO₂)₂ |
| 2. Sodium Hydroxide | Ionic | NaOH |
| 3. Nitrogen Dioxide | Covalent | NO₂ |
| 4. Cobalt (III) Oxalate | Ionic | Co₂(C₂O₄)₃ |
| 5. Ammonium Sulfide | Ionic | (NH₄)₂S |
| 6. Aluminum Cyanide | Ionic | Al(CN)₃ |
| 7. Carbon Disulfide | Covalent | CS₂ |
| 8. Tetraphosphorous Pentoxide| Covalent | P₄O₁₀ |
| 9. Potassium Permanganate | Ionic | KMnO₄ |
| 10. Manganese (III) Chloride | Ionic | MnCl₃ |
| 11. Calcium Bromate | Ionic | Ca(BrO₃)₂ |
| 12. Carbon Monoxide | Covalent | CO |
| 13. Potassium Oxide | Ionic | K₂O |
| 14. Antimony Tribromide | Ionic | SbBr₃ |
| 15. Zinc Phosphate | Ionic | Zn₃(PO₄)₂ |
| 16. Copper (II) Bicarbonate | Ionic | Cu(HCO₃)₂ |
| 17. Dinitrogen Tetroxide | Covalent | N₂O₄ |

Final Answer:
\boxed{
\begin{array}{|c|c|c|}
\hline
\text{Compound Name} & \text{Type of Compound} & \text{Chemical Formula} \\
\hline
\text{1. Copper (II) Chlorite} & \text{Ionic} & \text{Cu(ClO₂)₂} \\
\hline
\text{2. Sodium Hydroxide} & \text{Ionic} & \text{NaOH} \\
\hline
\text{3. Nitrogen Dioxide} & \text{Covalent} & \text{NO₂} \\
\hline
\text{4. Cobalt (III) Oxalate} & \text{Ionic} & \text{Co₂(C₂O₄)₃} \\
\hline
\text{5. Ammonium Sulfide} & \text{Ionic} & \text{(NH₄)₂S} \\
\hline
\text{6. Aluminum Cyanide} & \text{Ionic} & \text{Al(CN)₃} \\
\hline
\text{7. Carbon Disulfide} & \text{Covalent} & \text{CS₂} \\
\hline
\text{8. Tetraphosphorous Pentoxide} & \text{Covalent} & \text{P₄O₁₀} \\
\hline
\text{9. Potassium Permanganate} & \text{Ionic} & \text{KMnO₄} \\
\hline
\text{10. Manganese (III) Chloride} & \text{Ionic} & \text{MnCl₃} \\
\hline
\text{11. Calcium Bromate} & \text{Ionic} & \text{Ca(BrO₃)₂} \\
\hline
\text{12. Carbon Monoxide} & \text{Covalent} & \text{CO} \\
\hline
\text{13. Potassium Oxide} & \text{Ionic} & \text{K₂O} \\
\hline
\text{14. Antimony Tribromide} & \text{Ionic} & \text{SbBr₃} \\
\hline
\text{15. Zinc Phosphate} & \text{Ionic} & \text{Zn₃(PO₄)₂} \\
\hline
\text{16. Copper (II) Bicarbonate} & \text{Ionic} & \text{Cu(HCO₃)₂} \\
\hline
\text{17. Dinitrogen Tetroxide} & \text{Covalent} & \text{N₂O₄} \\
\hline
\end{array}
}