Which of the following best describes the Lewis dot structure for the HO2^- ion?

• A. The central oxygen atom is bonded to a hydrogen atom and another oxygen atom, with one single bond and one double bond, and the negative charge is located on the terminal oxygen.
• B. The central oxygen atom is bonded to two hydrogen atoms, and the negative charge is on the central oxygen.
• C. The hydrogen atom is bonded to both oxygen atoms, and the negative charge is shared equally between the two oxygens.
• D. Both oxygen atoms are double-bonded to each other, and the hydrogen atom is attached to one oxygen, with the negative charge on the hydrogen.

Answer: (A)

Verified step by step guidance

1. Identify the atoms present in the HO2^- ion: one hydrogen (H), two oxygens (O), and an overall negative charge (-1).
2. Determine the central atom, which is typically the least electronegative atom that can form multiple bonds; here, oxygen is the central atom bonded to hydrogen and the other oxygen.
3. Calculate the total number of valence electrons: oxygen has 6 valence electrons each, hydrogen has 1, and add 1 extra electron for the negative charge, so total electrons = 6 + 6 + 1 + 1 = 14 electrons.
4. Arrange the atoms with the central oxygen bonded to hydrogen and the other oxygen, then distribute the 14 valence electrons to satisfy the octet rule for oxygen atoms and duet for hydrogen, considering single and double bonds as needed.
5. Assign formal charges to each atom to find the most stable Lewis structure, ensuring the negative charge is located on the terminal oxygen atom, which is more electronegative and can better accommodate the extra electron.