Which of the following statements correctly describes the Lewis dot structure of the perchlorate ion, ClO_4^-?

• A. Chlorine is surrounded by four oxygen atoms, each connected by a single bond, and all oxygens have three lone pairs.
• B. Chlorine is bonded to two oxygen atoms with single bonds and two with double bonds; the negative charge is on a doubly bonded oxygen.
• C. Chlorine is at the center, bonded to four oxygen atoms with one double bond and three single bonds; the negative charge is located on one of the singly bonded oxygens.
• D. Chlorine is bonded to four oxygen atoms, each with a double bond, and the negative charge is delocalized over all oxygens.

Answer: (C)

Verified step by step guidance

1. Step 1: Identify the central atom and the total number of valence electrons. Chlorine (Cl) is the central atom, and each oxygen (O) atom contributes 6 valence electrons. The perchlorate ion (ClO_4^-) has an extra electron due to the negative charge, so add 1 more electron to the total count.
2. Step 2: Draw a skeletal structure with chlorine in the center bonded to four oxygen atoms. Initially, connect each oxygen to chlorine with a single bond.
3. Step 3: Distribute the remaining valence electrons to complete the octets of the oxygen atoms first, placing lone pairs on each oxygen to satisfy the octet rule.
4. Step 4: Check the formal charges on each atom. To minimize formal charges, convert some of the oxygen-chlorine single bonds into double bonds by sharing lone pairs from oxygen with chlorine, keeping in mind that chlorine can have an expanded octet.
5. Step 5: Determine the resonance structures and the location of the negative charge. The most stable Lewis structure has chlorine bonded to four oxygens with one double bond and three single bonds, with the negative charge localized on one of the singly bonded oxygens.