Chemistry worksheet demonstrating ionic bonding through Lewis dot diagrams for 12 different compounds.

The image you've uploaded is a completed worksheet titled "WS 1-Ionic Bonding – KEY", which shows dot diagrams (Lewis structures) for various ionic compounds. The task was to draw the electron dot diagrams for each element in the compound and show how electrons are transferred to form ions, resulting in ionic bonds.

Let me explain how these diagrams work and verify each one with correct reasoning:

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🔹 Concept: Ionic Bonding

Ionic bonding occurs when electrons are transferred from a metal (which loses electrons to form a cation) to a nonmetal (which gains electrons to form an anion). This results in electrostatic attraction between oppositely charged ions.

We use Lewis dot diagrams to represent valence electrons:
- Dots around the element symbol represent valence electrons.
- Arrows show electron transfer.
- Ions are shown with charges after the transfer.

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✔ Let's go through each compound:

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#### 1. NaCl
- Na: 1 valence electron → loses 1 e⁻ → becomes Na⁺
- Cl: 7 valence electrons → gains 1 e⁻ → becomes Cl⁻
- Electron transfers from Na to Cl.
✔ Correct

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#### 2. CaO
- Ca: 2 valence electrons → loses 2 e⁻ → Ca²⁺
- O: 6 valence electrons → gains 2 e⁻ → O²⁻
✔ Correct

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#### 3. AlN
- Al: 3 valence electrons → loses 3 e⁻ → Al³⁺
- N: 5 valence electrons → gains 3 e⁻ → N³⁻
✔ Correct

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#### 4. MgS
- Mg: 2 valence electrons → loses 2 e⁻ → Mg²⁺
- S: 6 valence electrons → gains 2 e⁻ → S²⁻
✔ Correct

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#### 5. FeCl₂
- Fe: Iron can have multiple charges; here it's Fe²⁺ (iron(II))
- Cl: Each Cl gains 1 e⁻ → Cl⁻
- Two Cl atoms accept 2 electrons from Fe
✔ Correct (assuming Fe²⁺)

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#### 6. CoF₃
- Co: Cobalt forms Co³⁺ here
- F: Each F gains 1 e⁻ → F⁻
- Three F atoms gain 3 electrons from Co
✔ Correct

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#### 7. Li₂O
- Li: 1 valence e⁻ per atom → each loses 1 e⁻ → Li⁺
- O: 6 valence e⁻ → gains 2 e⁻ → O²⁻
- Two Li atoms donate 1 e⁻ each → total 2 e⁻ to O
✔ Correct

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#### 8. Ag₃P
- Ag: Silver typically forms Ag⁺
- P: Phosphorus gains 3 e⁻ → P³⁻
- Three Ag atoms each lose 1 e⁻ → total 3 e⁻ to P
✔ Correct

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#### 9. Ba₃N₂
- Ba: Barium forms Ba²⁺ (loses 2 e⁻)
- N: Nitrogen gains 3 e⁻ → N³⁻
- To balance: 3 Ba²⁺ = +6 charge; 2 N³⁻ = -6 charge
- So, 3 Ba atoms lose 2 e⁻ each → 6 e⁻ total
- 2 N atoms gain 3 e⁻ each → 6 e⁻ total
✔ Correct

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#### 10. Al₂O₃
- Al: 3 valence e⁻ → Al³⁺
- O: 6 valence e⁻ → O²⁻
- 2 Al atoms lose 3 e⁻ each → 6 e⁻ total
- 3 O atoms gain 2 e⁻ each → 6 e⁻ total
✔ Correct

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#### 11. ZnI₂
- Zn: Zinc forms Zn²⁺
- I: Iodine gains 1 e⁻ → I⁻
- One Zn loses 2 e⁻ → two I atoms each gain 1 e⁻
✔ Correct

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#### 12. Au₂S₃
- Au: Gold can be Au³⁺ here
- S: Sulfur gains 2 e⁻ → S²⁻
- 2 Au atoms → each loses 3 e⁻ → 6 e⁻ total
- 3 S atoms → each gains 2 e⁻ → 6 e⁻ total
✔ Correct

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✔ Summary of Key Points:

- Metals lose electrons (form positive ions).
- Nonmetals gain electrons (form negative ions).
- Total electrons lost = total electrons gained.
- Charges must balance in the final compound.

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📌 Final Note:

All the diagrams in your image are correctly drawn and reflect proper electron transfer and ion formation for each ionic compound. The red writing shows the ions formed and their charges, while blue shows the electron transfer via arrows.

This worksheet is a perfect example of how to visualize ionic bonding using Lewis dot structures.

Let me know if you'd like this converted into a printable format or want explanations for any specific compound!