Worksheet on ionic bonding showing how metals and non-metals form compounds by transferring electrons, illustrated with atomic diagrams and a magnet symbolizing attraction between ions.

Let's solve the worksheet on Ionic Bonding step by step and fill in all the blanks with correct answers. This is a great educational resource for understanding how ionic bonds form between metals and non-metals.

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✔ Completed Worksheet with Explanations

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#### Main Paragraph:
> Metals and non-metals react together to form ionic compounds. They are held together by ionic bonds. Ionic bonding is a force of electrostatic attraction between two oppositely charged atoms (called ions). An atom becomes charged by either donating or accepting valence electrons from another atom. A valence electron is one from the outermost shell of the atom.

- Ionic: Metals and non-metals form ionic compounds.
- Electrostatic: The force between oppositely charged ions.
- Oppositely charged: One ion positive, one negative.
- Ions: Charged atoms.
- Valence: Electrons in the outer shell that can be transferred.
- Outermost: Valence electrons are in the highest energy level.

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> If an atom loses an electron, it becomes positively charged. This is then called a cation. Metals always donate electrons. If an atom accepts an electron, it becomes negatively charged. This is called an anion. Non-metals always accept electrons.

- Loses: Losing electrons → positive charge.
- Cation: Positively charged ion.
- Metals: Tend to lose electrons (low ionization energy).
- Negatively: Gaining electrons → negative charge.
- Anion: Negatively charged ion.

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> Atoms do this in order to become ‘stable’. A stable atom is one which has obtained a full outer shell of electrons.

- Stable: Atoms aim for noble gas configuration (octet rule).
- Full outer shell: Usually 8 electrons (except H and He).

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🔬 How do we know which atoms donate and which accept electrons?

#### Left Box – Sodium (Na):
> Sodium has one lone electron in the outer shell. It is easiest for this atom to lose one electron than to try and find seven more to fill the outer shell.

- Sodium (Na) has atomic number 11 → Electron config: 2,8,1 → 1 valence electron.
- Easier to lose 1 electron than gain 7.

> All metals donate electrons and therefore become cations.

- Metals tend to lose electrons → form cations.

#### Right Box – Chlorine (Cl):
> Chlorine has seven electrons in its outer shell. Therefore, it is easiest for Chlorine to gain one electron than to try and donate seven.

- Chlorine (Cl) has atomic number 17 → Electron config: 2,8,7 → 7 valence electrons.
- Needs only 1 more to complete octet.

> All non-metals accept electrons and therefore become anions.

- Non-metals gain electrons → form anions.

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🧪 Final Answer Summary:

| Blank | Answer |
|------|--------|
| 1. Metals and non-metals form ___ compounds | ionic |
| 2. Force of ___ attraction | electrostatic |
| 3. Between two ___ atoms | oppositely charged |
| 4. Called ___ | ions |
| 5. Donating or accepting ___ electrons | valence |
| 6. From the ___ shell | outermost |
| 7. If an atom ___ an electron | loses |
| 8. Called a ___ | cation |
| 9. ___ always donate electrons | Metals |
| 10. Becomes ___ charged | negatively |
| 11. Called an ___ | anion |
| 12. To become ___ | stable |
| 13. Has obtained a ___ ___ ___ of electrons | full outer shell |
| 14. Sodium has ___ lone electron | one |
| 15. To ___ one electron | lose |
| 16. All ___ donate electrons | metals |
| 17. Chlorine has ___ electrons | seven |
| 18. To ___ one electron | gain |
| 19. All ___ accept electrons | non-metals |

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💡 Key Concept Recap:

- Ionic Bonding: Transfer of electrons from metal to non-metal.
- Metal → Loses e⁻ → Cation (+)
- Non-metal → Gains e⁻ → Anion (–)
- Electrostatic attraction holds them together.
- Both achieve stable electron configurations (like noble gases).

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✔ Example: Sodium Chloride (NaCl)
- Na loses 1 e⁻ → Na⁺
- Cl gains 1 e⁻ → Cl⁻
- Na⁺ and Cl⁻ attract → ionic bond

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This worksheet teaches the fundamental principles of ionic bonding, using clear visuals and logical progression. Great job on creating or using this! Let me know if you'd like a printable version or quiz based on it.