Which of the following statements correctly describes the Lewis dot structure of the BrO2^- ion?

• A. Bromine is the central atom, bonded to two oxygen atoms, with no lone pairs on bromine and a total of 16 valence electrons.
• B. Oxygen is the central atom, bonded to two bromine atoms, with a total of 18 valence electrons.
• C. Bromine is the central atom, bonded to two oxygen atoms, with two lone pairs on bromine and a total of 20 valence electrons.
• D. Bromine is the central atom, bonded to two oxygen atoms, with one lone pair on bromine and a total of 18 valence electrons.

Answer: (D)

Verified step by step guidance

1. Identify the atoms involved in the BrO2^- ion: one bromine (Br) atom and two oxygen (O) atoms, with an overall negative charge of -1.
2. Determine the total number of valence electrons: bromine has 7 valence electrons, each oxygen has 6 valence electrons, and the extra negative charge adds 1 more electron. Calculate total valence electrons as \$7 + 2 \times 6 + 1 = 20$ electrons.
3. Choose the central atom: bromine is less electronegative than oxygen, so bromine is the central atom bonded to two oxygen atoms.
4. Draw single bonds between bromine and each oxygen atom, using 2 electrons per bond, and then distribute the remaining electrons to satisfy the octet rule for each atom, including lone pairs on bromine and oxygen atoms.
5. Count the total electrons used in the structure and verify the number of lone pairs on bromine and oxygen atoms, ensuring the total valence electrons equal 20 and that the formal charges are minimized to confirm the correct Lewis structure.