Which of the following correctly matches each element with the Lewis dot symbol for its most stable ion: sodium, oxygen, calcium, and chlorine?

• A. Na: [Na]^0, O: [O]^-, Ca: [Ca]^+, Cl: [Cl]^0
• B. Na: [Na]^+, O: [O]^-, Ca: [Ca]^+, Cl: [Cl]^+
• C. Na: [Na]^-, O: [O]^+, Ca: [Ca]^+, Cl: [Cl]^+
• D. Na: [Na]^+, O: [O]^2-, Ca: [Ca]^2+, Cl: [Cl]^-

Answer: (D)

Verified step by step guidance

1. Identify the most stable ion charge for each element by considering their position in the periodic table and common oxidation states: Sodium (Na) typically loses one electron to form Na⁺, Oxygen (O) typically gains two electrons to form O²⁻, Calcium (Ca) typically loses two electrons to form Ca²⁺, and Chlorine (Cl) typically gains one electron to form Cl⁻.
2. Write the Lewis dot symbol for each ion by placing the element symbol inside brackets and indicating the charge as a superscript outside the brackets. For example, for sodium ion, write \([\mathrm{Na}]^{+}\) to show it has lost one electron.
3. For oxygen ion, since it gains two electrons, write \([\mathrm{O}]^{2-}\), showing the extra electrons as a 2- charge outside the brackets.
4. For calcium ion, which loses two electrons, write \([\mathrm{Ca}]^{2+}\), indicating the 2+ charge outside the brackets.
5. For chlorine ion, which gains one electron, write \([\mathrm{Cl}]^{-}\), indicating the single negative charge outside the brackets.