Worksheet on ionic bonds and naming ionic compounds for chemistry education.

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Part 1: Fill in the Blanks

Here are the completed sentences with explanations:

1. Ionic bonds form between ___ and ___.
→ Metals and nonmetals
*Explanation:* Ionic bonds occur when electrons are transferred from a metal (which loses electrons) to a nonmetal (which gains electrons).

2. In naming simple ionic compounds, the ___ is always first, the ___ second (e.g., sodium chloride).
→ Cation (positive ion) is always first, anion (negative ion) is second.
*Example:* Sodium (Na⁺) is the cation; chloride (Cl⁻) is the anion → Sodium chloride.

3. Ionic compounds dissolve easily in ___ and other polar solvents.
→ Water
*Explanation:* Water is a polar solvent that can stabilize ions through hydration, allowing ionic compounds to dissolve.

4. In solution, ionic compounds exist as ___ .
→ Ions
*Explanation:* When dissolved, ionic compounds dissociate into their respective positive and negative ions.

5. Ionic compounds tend to form ___ with ___ melting temperatures.
→ Crystals with high melting temperatures.
*Explanation:* The strong electrostatic forces between ions require a lot of energy to break, resulting in high melting points.

6. When writing formulas for ionic compounds:
- Write the cation first and the anion second.
- Use subscripts to indicate the number of atoms of each type present in the compound.
- No prefixes are used.
- Change the ending of the anion name to -ide to stay consistent.

*Example:* Na⁺ and Cl⁻ → NaCl (sodium chloride)

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Part 2: Complete the Table

We need to fill in the following columns:
- Number of valence electrons
- # of electrons gained or lost (or to be gained/lost)
- Charge (Oxidation Number)

Let’s go element by element:

| Element | Valence Electrons | Electrons Gained/Lost | Charge (Oxidation Number) |
|-------------|-------------------|------------------------|----------------------------|
| Sodium | 1 | Loses 1 | +1 |
| Chlorine | 7 | Gains 1 | -1 |
| Beryllium | 2 | Loses 2 | +2 |
| Fluorine | 7 | Gains 1 | -1 |
| Lithium | 1 | Loses 1 | +1 |
| Oxygen | 6 | Gains 2 | -2 |
| Potassium | 1 | Loses 1 | +1 |
| Magnesium | 2 | Loses 2 | +2 |
| Phosphorus | 5 | Gains 3 | -3 |
| Aluminum | 3 | Loses 3 | +3 |

#### Explanations:

- Sodium (Na): Group 1 → 1 valence electron → loses 1 → +1
- Chlorine (Cl): Group 17 → 7 valence electrons → gains 1 → -1
- Beryllium (Be): Group 2 → 2 valence electrons → loses 2 → +2
- Fluorine (F): Group 17 → 7 valence electrons → gains 1 → -1
- Lithium (Li): Group 1 → 1 valence electron → loses 1 → +1
- Oxygen (O): Group 16 → 6 valence electrons → gains 2 → -2
- Potassium (K): Group 1 → 1 valence electron → loses 1 → +1
- Magnesium (Mg): Group 2 → 2 valence electrons → loses 2 → +2
- Phosphorus (P): Group 15 → 5 valence electrons → gains 3 to complete octet → -3
- Aluminum (Al): Group 13 → 3 valence electrons → loses 3 → +3

> Note: These charges are typical for forming ionic compounds. Phosphorus can have multiple oxidation states, but in ionic compounds like phosphides, it commonly forms P³⁻.

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✔ Final Answer Summary:

#### Fill-in-the-blank Answers:
1. Metals, nonmetals
2. Cation, anion
3. Water
4. Ions
5. Crystals, high
6. Cation, anion; subscripts; ending; -ide

#### Completed Table:

| Element | Valence Electrons | Electrons Gained/Lost | Charge (Oxidation Number) |
|-------------|-------------------|------------------------|----------------------------|
| Sodium | 1 | Loses 1 | +1 |
| Chlorine | 7 | Gains 1 | -1 |
| Beryllium | 2 | Loses 2 | +2 |
| Fluorine | 7 | Gains 1 | -1 |
| Lithium | 1 | Loses 1 | +1 |
| Oxygen | 6 | Gains 2 | -2 |
| Potassium | 1 | Loses 1 | +1 |
| Magnesium | 2 | Loses 2 | +2 |
| Phosphorus | 5 | Gains 3 | -3 |
| Aluminum | 3 | Loses 3 | +3 |

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Let me know if you'd like help writing formulas for ionic compounds using this data!