Which of the following statements correctly describes the Lewis dot structure of the BrO4^- ion?

• A. Bromine is the central atom, surrounded by four oxygen atoms, each connected by single bonds; the negative charge is delocalized over all oxygens.
• B. Bromine is the central atom, surrounded by three oxygen atoms, each connected by single bonds; the negative charge is on the bromine atom.
• C. Bromine is the central atom, surrounded by four oxygen atoms, each connected by double bonds; the negative charge is on the bromine atom.
• D. Bromine is the central atom, surrounded by four oxygen atoms, with three double bonds and one single bond; the negative charge is located on the singly bonded oxygen.

Answer: (D)

Verified step by step guidance

1. Identify the central atom in the BrO4^- ion. Since bromine is less electronegative than oxygen, bromine will be the central atom surrounded by four oxygen atoms.
2. Determine the total number of valence electrons available. Bromine has 7 valence electrons, each oxygen has 6, and there is an extra electron due to the negative charge, so total electrons = 7 + (4 × 6) + 1.
3. Distribute electrons to form bonds between bromine and each oxygen atom. Start by placing single bonds between bromine and each oxygen, using 2 electrons per bond.
4. Complete the octets of the oxygen atoms by adding lone pairs, then use any remaining electrons to form double bonds as needed to satisfy the octet rule and minimize formal charges.
5. Assign the negative charge to the oxygen atom that is singly bonded to bromine, as this oxygen will have an extra lone pair, making it the site of the negative charge in the Lewis structure.