Which of the following Lewis dot diagrams correctly represents the ionic bond between sodium (Na) and chlorine (Cl)?

• A. Na^{+} ig[ egin{array}{c} ext{Cl} \ ext{:} \ ext{:} \ ext{:} \ ext{:} \ ext{:} \ ext{:} \ ext{:} ig]^{-}
• B. Na ext{:} ext{:} ext{:} ext{:} ext{:} ext{:} ext{:} ext{:} ext{Cl}
• C. Na ig[ ext{Cl} ext{:} ext{:} ext{:} ext{:} ext{:} ext{:} ext{:} ig]
• D. Na^{+} ext{:} ext{:} ext{:} ext{:} ext{:} ext{:} ext{:} ext{:} ext{Cl}^{-}

Answer: (A)

Verified step by step guidance

1. Understand that an ionic bond forms when one atom donates an electron to another, resulting in positively and negatively charged ions.
2. Recognize that sodium (Na) has one valence electron and tends to lose it to achieve a stable electron configuration, becoming Na⁺.
3. Recognize that chlorine (Cl) has seven valence electrons and tends to gain one electron to complete its octet, becoming Cl⁻.
4. Draw the Lewis dot structure for Na⁺ without any valence electrons (since it lost one electron) and for Cl⁻ with eight valence electrons (including the gained electron), typically shown as dots around the Cl symbol enclosed in brackets with a negative charge.
5. Combine these to represent the ionic bond: Na⁺ (no dots) next to [Cl with eight dots]⁻, indicating the transfer of an electron and the resulting charges.