Which of the following best describes the Lewis dot structure for the hypochlorite ion, ClO^-?

• A. Chlorine is triple-bonded to oxygen, with one lone pair on chlorine, one lone pair on oxygen, and an overall negative charge.
• B. Chlorine is single-bonded to oxygen, with two lone pairs on chlorine, three lone pairs on oxygen, and no overall charge.
• C. Chlorine is single-bonded to oxygen, with three lone pairs on chlorine, three lone pairs on oxygen, and an overall negative charge.
• D. Chlorine is double-bonded to oxygen, with two lone pairs on chlorine, two lone pairs on oxygen, and an overall negative charge.

Answer: (C)

Verified step by step guidance

1. Step 1: Determine the total number of valence electrons for the hypochlorite ion (ClO⁻). Chlorine (Cl) has 7 valence electrons, oxygen (O) has 6 valence electrons, and the negative charge adds 1 extra electron. So, total valence electrons = 7 + 6 + 1 = 14 electrons.
2. Step 2: Draw a skeletal structure with chlorine and oxygen connected by a single bond initially. This single bond accounts for 2 electrons, so subtract these from the total valence electrons: 14 - 2 = 12 electrons remaining to be placed as lone pairs.
3. Step 3: Distribute the remaining 12 electrons as lone pairs to satisfy the octet rule for both atoms. Start by placing lone pairs on oxygen to complete its octet, then place the remaining electrons on chlorine.
4. Step 4: Check the formal charges on each atom to ensure the most stable Lewis structure. Formal charge is calculated by: \(\text{Formal Charge} = \text{Valence Electrons} - \text{Nonbonding Electrons} - \frac{1}{2} \times \text{Bonding Electrons}\). Adjust bonding (single, double, or triple bonds) if necessary to minimize formal charges.
5. Step 5: Confirm that the overall charge of the ion is -1 by summing the formal charges of chlorine and oxygen. The correct Lewis structure will have chlorine single-bonded to oxygen, three lone pairs on chlorine, three lone pairs on oxygen, and an overall negative charge.