Free Printable Chemical Bonding Worksheets - Free Printable

Let's solve this Chemical Bonding and Intermolecular Forces Worksheet step by step.

We need to determine the type of bond present in each compound: Ionic, Polar Covalent, or Non-polar Covalent.

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🔍 Guidelines for Determining Bond Type:

1. Ionic Bond: Typically between a metal and a non-metal with a large electronegativity difference (> ~1.7–2.0).
2. Polar Covalent Bond: Between two non-metals with a moderate electronegativity difference (0.4–1.7).
3. Non-polar Covalent Bond: Between two identical atoms or atoms with very small electronegativity difference (< 0.4).

> Note: The bond type refers to the type of bonding within the molecule, not necessarily the overall molecular polarity.

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Now, let’s go through each compound:

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1. NH₃ (Ammonia)

- Nitrogen (N) and Hydrogen (H): both non-metals.
- Electronegativity: N = 3.0, H = 2.1 → ΔEN = 0.9 → Polar covalent.
✔ Polar Covalent Bond

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2. F₂ (Fluorine gas)

- Two identical fluorine atoms.
- ΔEN = 0 → Non-polar covalent.
✔ Non-polar Covalent Bond

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3. NO (Nitric oxide)

- Nitrogen and Oxygen: both non-metals.
- Electronegativity: O = 3.5, N = 3.0 → ΔEN = 0.5 → Polar covalent.
✔ Polar Covalent Bond

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4. HCl (Hydrogen chloride)

- H and Cl: both non-metals.
- Electronegativity: Cl = 3.0, H = 2.1 → ΔEN = 0.9 → Polar covalent.
✔ Polar Covalent Bond

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5. NaCl (Sodium chloride)

- Sodium (Na, metal) and Chlorine (Cl, non-metal).
- ΔEN ≈ 3.0 → Ionic bond.
✔ Ionic Bond

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6. CH₃Cl (Chloromethane)

- C and H: ΔEN = 0.4 → weakly polar, but mostly covalent.
- C and Cl: ΔEN = 3.0 - 2.5 = 0.5 → Polar covalent.
- Overall: Contains polar covalent bonds (especially C–Cl).
✔ Polar Covalent Bond

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7. I₂ (Iodine)

- Two identical iodine atoms.
- ΔEN = 0 → Non-polar covalent.
✔ Non-polar Covalent Bond

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8. KF (Potassium fluoride)

- K (metal), F (non-metal).
- ΔEN ≈ 3.0 → Ionic bond.
✔ Ionic Bond

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9. NO (again) – same as #3

✔ Polar Covalent Bond

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10. CaCl₂ (Calcium chloride)

- Ca (metal), Cl (non-metal).
- ΔEN large → Ionic bond.
✔ Ionic Bond

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11. CH₃OH (Methanol)

- Contains C–H, C–O, O–H bonds.
- C–O: ΔEN = 1.0 → polar covalent.
- O–H: ΔEN = 1.4 → polar covalent.
✔ Polar Covalent Bond

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12. H₂O (Water)

- O and H: ΔEN = 1.4 → Polar covalent.
✔ Polar Covalent Bond

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13. PCl₃ (Phosphorus trichloride)

- P and Cl: both non-metals.
- ΔEN = 3.0 – 2.2 = 0.8 → Polar covalent.
✔ Polar Covalent Bond

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14. CH₄ (Methane)

- C and H: ΔEN = 0.4 → Non-polar covalent (very small difference).
- Although individual bonds are slightly polar, due to symmetry, molecule is non-polar.
- But the question asks about bond type, not molecular polarity.
- Since ΔEN < 0.5, it's considered non-polar covalent.
✔ Non-polar Covalent Bond

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15. O₂ (Oxygen gas)

- Two identical oxygen atoms.
- ΔEN = 0 → Non-polar covalent.
✔ Non-polar Covalent Bond

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✔ Final Answer Table:

| Name of the Compound | Ionic Bond | Polar Covalent Bond | Non-polar Covalent Bond |
|----------------------|------------|-----------------------|--------------------------|
| NH₃ | | ✔ | |
| F₂ | | | ✔ |
| NO | | ✔ | |
| HCl | | ✔ | |
| NaCl | ✔ | | |
| CH₃Cl | | ✔ | |
| I₂ | | | ✔ |
| KF | ✔ | | |
| NO | | ✔ | |
| CaCl₂ | ✔ | | |
| CH₃OH | | ✔ | |
| H₂O | | ✔ | |
| PCl₃ | | ✔ | |
| CH₄ | | | ✔ |
| O₂ | | | ✔ |

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📝 Summary:

- Ionic Bonds: NaCl, KF, CaCl₂
- Polar Covalent Bonds: NH₃, NO, HCl, CH₃Cl, CH₃OH, H₂O, PCl₃
- Non-polar Covalent Bonds: F₂, I₂, CH₄, O₂

> Note: Some compounds like CH₄ have polar bonds (C–H) but are non-polar molecules due to symmetry. However, since the question asks about bond type, we classify based on electronegativity differences.

✔ This table correctly reflects the type of chemical bond formed in each compound.

Let me know if you'd like an explanation of intermolecular forces too!