Choose te correct Lewis Dot diagram for NaCl; ~Na: Cl 1+ Na’ :C Na: 8 Cl Na: 9: 3a
The Correct Answer and Explanation is:
✅ Correct Lewis Dot Diagram for NaCl:
Na⁺ :Cl⁻
This is typically shown as:
- Na⁺ (no dots, as it lost its one valence electron)
- :Cl⁻ (eight valence electrons—4 pairs—around the Cl atom, representing a full octet)
🧠 Explanation
Sodium chloride (NaCl) is an ionic compound formed by the transfer of electrons between a metal (sodium, Na) and a non-metal (chlorine, Cl).
1. Understanding Valence Electrons:
- Sodium (Na) is in Group 1 of the periodic table, meaning it has 1 valence electron.
- Chlorine (Cl) is in Group 17 (halogens) and has 7 valence electrons.
2. How the Ionic Bond Forms:
- Sodium readily loses its single valence electron to achieve the stable noble gas configuration of neon (Ne). When it loses this electron, it becomes a positively charged ion (Na⁺).
- Chlorine needs one more electron to complete its octet and become like argon (Ar). When it gains one electron, it becomes a negatively charged ion (Cl⁻).
3. Lewis Dot Diagrams:
- In a Lewis Dot Diagram, we represent valence electrons as dots around the element symbol.
- For Na⁺, it has lost its only valence electron, so we write Na⁺ with no dots.
- For Cl⁻, it gains one electron to have 8 total. This is shown with 4 pairs of dots around the symbol, and it’s written as [ :Cl: ]⁻ or :Cl⁻, indicating a full octet.
4. Key Points:
- The resulting electrostatic attraction between Na⁺ and Cl⁻ is what forms the ionic bond.
- Lewis Dot Diagrams for ionic compounds do not show a shared pair of electrons (unlike covalent bonds), but rather complete transfer.
- Therefore, the correct representation is Na⁺ :Cl⁻, with Na having no dots and Cl having a full octet.
This diagram clearly represents the ionic nature of the bond and follows the octet rule, making it the correct choice.
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