Forming and Naming Binary Ionic Compounds Practice Worksheet ... - Free Printable

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🔹 Part 1: Identify Charges and Name Ions

> List the charges the following elements would have as ions. Tell whether they are anions or cations, and name them.

| Element | Ion | Charge | Cation/Anion | Name |
|--------|-----|--------|--------------|------|
| Ca | Ca²⁺ | +2 | Cation | Calcium ion |
| Cl | Cl⁻ | -1 | Anion | Chloride ion |
| Al | Al³⁺ | +3 | Cation | Aluminum ion |
| O | O²⁻ | -2 | Anion | Oxide ion |

✔ Explanation:
- Metals (like Ca, Al) lose electrons → form cations (positive ions).
- Nonmetals (like Cl, O) gain electrons → form anions (negative ions).
- The charge is based on typical group trends:
- Ca (Group 2): loses 2 e⁻ → Ca²⁺
- Cl (Group 17): gains 1 e⁻ → Cl⁻
- Al (Group 13): loses 3 e⁻ → Al³⁺
- O (Group 16): gains 2 e⁻ → O²⁻

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🔹 Part 2: How many electrons does the neutral atom gain or lose when each ion forms?

| Ion | Electrons gained or lost |
|-----|--------------------------|
| Li⁺ | Loses 1 electron |
| Mg²⁺ | Loses 2 electrons |
| F⁻ | Gains 1 electron |
| S²⁻ | Gains 2 electrons |
| Ca²⁺ | Loses 2 electrons |
| N³⁻ | Gains 3 electrons |

✔ Explanation:
- Positive ions (cations): lose electrons.
- Negative ions (anions): gain electrons.
- The magnitude of the charge tells how many electrons were transferred.

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🔹 Part 3: Write the equation for formation of ions

These are electron transfer reactions:

1. Li → Li⁺ + e⁻
Lithium loses one electron to form a +1 ion.

2. Na → Na⁺ + e⁻
Sodium loses one electron.

3. Mg → Mg²⁺ + 2e⁻
Magnesium loses two electrons.

4. Al → Al³⁺ + 3e⁻
Aluminum loses three electrons.

5. O + 2e⁻ → O²⁻
Oxygen gains two electrons.

6. N + 3e⁻ → N³⁻
Nitrogen gains three electrons.

7. S + 2e⁻ → S²⁻
Sulfur gains two electrons.

8. Cl + e⁻ → Cl⁻
Chlorine gains one electron.

✔ Explanation:
- Metals lose electrons (oxidation).
- Nonmetals gain electrons (reduction).

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🔹 Part 4: Fill in the chart for binary ionic compounds

Let’s complete this table using standard rules:

| Compound Formula | Cation | Anion | Formula | Total Charge | Compound Name |
|------------------|--------|-------|---------|---------------|----------------|
| magnesium bromide | Mg²⁺ | Br⁻ | MgBr₂ | 0 | Magnesium bromide |
| sodium oxide | Na⁺ | O²⁻ | Na₂O | 0 | Sodium oxide |
| potassium chloride | K⁺ | Cl⁻ | KCl | 0 | Potassium chloride |
| calcium sulfide | Ca²⁺ | S²⁻ | CaS | 0 | Calcium sulfide |
| barium iodide | Ba²⁺ | I⁻ | BaI₂ | 0 | Barium iodide |
| aluminum oxide | Al³⁺ | O²⁻ | Al₂O₃ | 0 | Aluminum oxide |
| lithium nitride | Li⁺ | N³⁻ | Li₃N | 0 | Lithium nitride |
| cesium chloride | Cs⁺ | Cl⁻ | CsCl | 0 | Cesium chloride |
| gallium sulfide | Ga³⁺ | S²⁻ | Ga₂S₃ | 0 | Gallium sulfide |
| aluminum iodide | Al³⁺ | I⁻ | AlI₃ | 0 | Aluminum iodide |
| calcium fluoride | Ca²⁺ | F⁻ | CaF₂ | 0 | Calcium fluoride |
| germanium sulfide | Ge⁴⁺ | S²⁻ | GeS₂ | 0 | Germanium sulfide |
| strontium oxide | Sr²⁺ | O²⁻ | SrO | 0 | Strontium oxide |

✔ How to determine formulas:
- Balance charges so total positive = total negative.
- Example: Al³⁺ and O²⁻ → need 2 Al³⁺ (total +6) and 3 O²⁻ (total -6) → Al₂O₃.

✔ Naming Rules:
- Metal name first, then nonmetal root + *-ide*.
- No prefixes used (unlike covalent compounds).

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✔ Summary of Key Concepts

1. Cations: Positively charged ions (metals lose electrons).
2. Anions: Negatively charged ions (nonmetals gain electrons).
3. Electron Transfer: Number of electrons lost/gained equals the charge.
4. Binary Ionic Compound Formation:
- Combine metal and nonmetal.
- Use charges to balance formula.
- Name: [Metal] + [Nonmetal root] + *-ide*.

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