Which of the following correctly describes the bonding in the Lewis dot structure of neutral SO_2?

• A. SO_2 has two single bonds between sulfur and each oxygen atom.
• B. SO_2 has two double bonds between sulfur and each oxygen atom.
• C. SO_2 has a triple bond between sulfur and one oxygen atom, and a single bond to the other.
• D. SO_2 has one single bond and one double bond between sulfur and the two oxygen atoms.

Answer: (D)

Verified step by step guidance

1. Step 1: Determine the total number of valence electrons for SO_2. Sulfur (S) has 6 valence electrons, and each oxygen (O) has 6 valence electrons, so total valence electrons = 6 + 2 \times 6 = 18.
2. Step 2: Draw a skeletal structure with sulfur as the central atom bonded to two oxygen atoms. Connect sulfur to each oxygen with a single bond initially, which uses 2 electrons per bond.
3. Step 3: Distribute the remaining electrons to satisfy the octet rule for the oxygen atoms first, placing lone pairs around each oxygen to complete their octets.
4. Step 4: Check the octet of the sulfur atom. If sulfur does not have a complete octet, form double bonds by converting lone pairs from oxygen atoms into bonding pairs between sulfur and oxygen.
5. Step 5: Confirm the formal charges on each atom to ensure the most stable Lewis structure. The best structure minimizes formal charges, which leads to one double bond and one single bond between sulfur and the two oxygen atoms.