Worksheet on chemical bonding with electronegativity values and bond type classification.

Absolutely! Let’s solve this worksheet step by step.

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## 🧠 Key Concepts to Remember:

1. Electronegativity (EN): An atom’s ability to attract bonding electrons.
2. Difference in EN (ΔEN) determines bond type:
- ΔEN ≥ 1.7 → Ionic
- 0.4 ≤ ΔEN < 1.7 → Polar Covalent
- ΔEN < 0.4 → Non-polar Covalent

3. Use the provided electronegativity chart to find values for each element.

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## ✔ Step-by-Step Solution:

We’ll go row by row, filling in:

- More electronegative element + its value
- Less electronegative element + its value
- Difference in EN (subtract smaller from larger)
- Bond Type (based on ΔEN)

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1. Sulfur and Hydrogen

- S = 2.5, H = 2.1 → More EN: S (2.5), Less EN: H (2.1)
- ΔEN = 2.5 – 2.1 = 0.4
- Bond Type: Polar Covalent (since 0.4 is the lower limit for polar covalent)

✔ Answer:
- More EN: Sulfur (2.5)
- Less EN: Hydrogen (2.1)
- ΔEN: 0.4
- Bond Type: Polar Covalent

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2. Sulfur and Cesium

- S = 2.5, Cs = 0.8 → More EN: S (2.5), Less EN: Cs (0.8)
- ΔEN = 2.5 – 0.8 = 1.7
- Bond Type: Ionic (exactly 1.7 — threshold for ionic)

✔ Answer:
- More EN: Sulfur (2.5)
- Less EN: Cesium (0.8)
- ΔEN: 1.7
- Bond Type: Ionic

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3. Chlorine and Bromine

- Cl = 3.0, Br = 2.8 → More EN: Cl (3.0), Less EN: Br (2.8)
- ΔEN = 3.0 – 2.8 = 0.2
- Bond Type: Non-polar Covalent

✔ Answer:
- More EN: Chlorine (3.0)
- Less EN: Bromine (2.8)
- ΔEN: 0.2
- Bond Type: Non-polar Covalent

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4. Calcium and Chlorine

- Ca = 1.0, Cl = 3.0 → More EN: Cl (3.0), Less EN: Ca (1.0)
- ΔEN = 3.0 – 1.0 = 2.0
- Bond Type: Ionic

✔ Answer:
- More EN: Chlorine (3.0)
- Less EN: Calcium (1.0)
- ΔEN: 2.0
- Bond Type: Ionic

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5. Oxygen and Hydrogen

- O = 3.5, H = 2.1 → More EN: O (3.5), Less EN: H (2.1)
- ΔEN = 3.5 – 2.1 = 1.4
- Bond Type: Polar Covalent

✔ Answer:
- More EN: Oxygen (3.5)
- Less EN: Hydrogen (2.1)
- ΔEN: 1.4
- Bond Type: Polar Covalent

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6. Nitrogen and Hydrogen

- N = 3.0, H = 2.1 → More EN: N (3.0), Less EN: H (2.1)
- ΔEN = 3.0 – 2.1 = 0.9
- Bond Type: Polar Covalent

✔ Answer:
- More EN: Nitrogen (3.0)
- Less EN: Hydrogen (2.1)
- ΔEN: 0.9
- Bond Type: Polar Covalent

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7. Iodine and Iodine

- I = 2.5, I = 2.5 → More EN: I (2.5), Less EN: I (2.5)
- ΔEN = 2.5 – 2.5 = 0.0
- Bond Type: Non-polar Covalent

✔ Answer:
- More EN: Iodine (2.5)
- Less EN: Iodine (2.5)
- ΔEN: 0.0
- Bond Type: Non-polar Covalent

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8. Copper and Sulfur

- Cu = 1.9, S = 2.5 → More EN: S (2.5), Less EN: Cu (1.9)
- ΔEN = 2.5 – 1.9 = 0.6
- Bond Type: Polar Covalent

✔ Answer:
- More EN: Sulfur (2.5)
- Less EN: Copper (1.9)
- ΔEN: 0.6
- Bond Type: Polar Covalent

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9. Hydrogen and Fluorine

- H = 2.1, F = 4.0 → More EN: F (4.0), Less EN: H (2.1)
- ΔEN = 4.0 – 2.1 = 1.9
- Bond Type: Ionic (some textbooks may call HF “polar covalent” due to molecular nature, but based strictly on ΔEN ≥ 1.7, it’s ionic)

⚠️ *Note: In reality, HF is often classified as polar covalent because it forms molecules, not a lattice. But according to your worksheet’s rule (ΔEN ≥ 1.7 = ionic), we must classify it as ionic.*

✔ Answer:
- More EN: Fluorine (4.0)
- Less EN: Hydrogen (2.1)
- ΔEN: 1.9
- Bond Type: Ionic

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10. Carbon and Oxygen

- C = 2.5, O = 3.5 → More EN: O (3.5), Less EN: C (2.5)
- ΔEN = 3.5 – 2.5 = 1.0
- Bond Type: Polar Covalent

✔ Answer:
- More EN: Oxygen (3.5)
- Less EN: Carbon (2.5)
- ΔEN: 1.0
- Bond Type: Polar Covalent

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## 📋 Final Completed Table:

| Bonding between | More electronegative element and value | Less electronegative element and value | Difference in electronegativity | Bond Type |
|------------------------|----------------------------------------|----------------------------------------|----------------------------------|--------------------|
| Sulfur and Hydrogen | Sulfur (2.5) | Hydrogen (2.1) | 0.4 | Polar Covalent |
| Sulfur and Cesium | Sulfur (2.5) | Cesium (0.8) | 1.7 | Ionic |
| Chlorine and Bromine | Chlorine (3.0) | Bromine (2.8) | 0.2 | Non-polar Covalent |
| Calcium and Chlorine | Chlorine (3.0) | Calcium (1.0) | 2.0 | Ionic |
| Oxygen and Hydrogen | Oxygen (3.5) | Hydrogen (2.1) | 1.4 | Polar Covalent |
| Nitrogen and Hydrogen | Nitrogen (3.0) | Hydrogen (2.1) | 0.9 | Polar Covalent |
| Iodine and Iodine | Iodine (2.5) | Iodine (2.5) | 0.0 | Non-polar Covalent |
| Copper and Sulfur | Sulfur (2.5) | Copper (1.9) | 0.6 | Polar Covalent |
| Hydrogen and Fluorine | Fluorine (4.0) | Hydrogen (2.1) | 1.9 | Ionic |
| Carbon and Oxygen | Oxygen (3.5) | Carbon (2.5) | 1.0 | Polar Covalent |

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## 💡 Extra Tip:

While the worksheet uses strict cutoffs, real chemistry sometimes has exceptions (like HF being polar covalent despite high ΔEN). But for schoolwork, follow the rules given!

Let me know if you want this in printable table format or need explanations for any row! 😊