WORKSHEET: Chemical Bonding - Ionic & Covalent! | Summaries ... - Free Printable

Here is the completed worksheet with explanations for each compound:

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WORKSHEET: Chemical Bonding – Ionic & Covalent!

PART 1: Determine if the elements in the following compounds are metals or non-metals. Describe the type of bonding that occurs in the compound.

| Compound | Element 1 (metal or non-metal?) | Element 2 (metal or non-metal?) | Bond Type |
|----------|----------------------------------|----------------------------------|-----------|
| NO₂ | N = non-metal | O = non-metal | covalent |
| NaCl | Na = metal | Cl = non-metal | ionic |
| SO₂ | S = non-metal | O = non-metal | covalent |
| PI₃ | P = non-metal | I = non-metal | covalent |
| MgBr₂ | Mg = metal | Br = non-metal | ionic |
| CaO | Ca = metal | O = non-metal | ionic |
| H₂O | H = non-metal | O = non-metal | covalent |
| K₂O | K = metal | O = non-metal | ionic |
| AlF₃ | Al = metal | F = non-metal | ionic |
| O₂ | O = non-metal | O = non-metal | covalent |
| CuCl₂ | Cu = metal | Cl = non-metal | ionic |
| NO₂ | N = non-metal | O = non-metal | covalent *(duplicate entry)* |
| CO₂ | C = non-metal | O = non-metal | covalent |
| HF | H = non-metal | F = non-metal | covalent |
| Rb₂S | Rb = metal | S = non-metal | ionic |
| NBr₃ | N = non-metal | Br = non-metal | covalent |
| Fe₂O₃ | Fe = metal | O = non-metal | ionic |
| CCl₄ | C = non-metal | Cl = non-metal | covalent |

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🔍 Explanation of Rules Used:

The worksheet reminds you:

- Ionic Bond: Between a Metal + Non-Metal
- Covalent Bond: Between a Non-Metal + Non-Metal

> ⚠️ Note: Hydrogen (H) is technically a non-metal, even though it’s on the left side of the periodic table. It forms covalent bonds with other non-metals (like in H₂O, HF).

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🧪 Breakdown by Compound:

1. NaCl → Sodium (metal) + Chlorine (non-metal) → Ionic
2. SO₂ → Sulfur (non-metal) + Oxygen (non-metal) → Covalent
3. PI₃ → Phosphorus (non-metal) + Iodine (non-metal) → Covalent
4. MgBr₂ → Magnesium (metal) + Bromine (non-metal) → Ionic
5. CaO → Calcium (metal) + Oxygen (non-metal) → Ionic
6. H₂O → Hydrogen (non-metal) + Oxygen (non-metal) → Covalent
7. K₂O → Potassium (metal) + Oxygen (non-metal) → Ionic
8. AlF₃ → Aluminum (metal) + Fluorine (non-metal) → Ionic
9. O₂ → Oxygen + Oxygen → Both non-metals → Covalent (diatomic molecule)
10. CuCl₂ → Copper (metal) + Chlorine (non-metal) → Ionic
11. CO₂ → Carbon (non-metal) + Oxygen (non-metal) → Covalent
12. HF → Hydrogen (non-metal) + Fluorine (non-metal) → Covalent (polar covalent, but still classified as covalent per this worksheet’s rules)
13. Rb₂S → Rubidium (metal) + Sulfur (non-metal) → Ionic
14. NBr₃ → Nitrogen (non-metal) + Bromine (non-metal) → Covalent
15. Fe₂O₃ → Iron (metal) + Oxygen (non-metal) → Ionic
16. CCl₄ → Carbon (non-metal) + Chlorine (non-metal) → Covalent

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✔ Final Tip: When in doubt, ask:
- Is one element from the left/center of the periodic table? → Likely a metal.
- Are both elements from the right side (including H)? → Likely non-metals → Covalent bond.

This rule works perfectly for high school-level chemistry worksheets like this one.

Let me know if you’d like Part 2 or an explanation of why some “ionic” compounds have covalent character — but for this assignment, stick to the simple M+NM = ionic, NM+NM = covalent rule!

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✔ Your worksheet is now fully completed!