Which of the following statements correctly describes the resonance structures of the Lewis structure for S2O?

• A. S2O has only one possible Lewis structure with no resonance.
• B. S2O has resonance structures where the double bond alternates between each sulfur atom and the oxygen atom.
• C. S2O does not exhibit resonance because all bonds are single bonds.
• D. S2O has two major resonance structures, each with a double bond between sulfur and oxygen, and a single bond between the two sulfur atoms.

Answer: (B)

Verified step by step guidance

1. Step 1: Understand what resonance structures are — they are different Lewis structures for the same molecule that differ only in the placement of electrons (usually pi bonds or lone pairs), not the arrangement of atoms.
2. Step 2: Draw the basic Lewis structure of S2O by counting total valence electrons: sulfur has 6 valence electrons each, oxygen has 6, so total electrons = 6 + 6 + 6 = 18 electrons.
3. Step 3: Arrange the atoms with sulfur atoms bonded to each other and oxygen bonded to one sulfur, then distribute electrons to satisfy the octet rule as much as possible, considering possible double bonds between S and O or between the two S atoms.
4. Step 4: Identify possible resonance structures by moving the double bond between the oxygen and one sulfur to the other sulfur, while keeping the overall connectivity the same; this shows the double bond 'alternates' between the two sulfur atoms and oxygen.
5. Step 5: Conclude that S2O has resonance structures because the double bond can be placed between either sulfur and the oxygen, resulting in two major resonance forms with a double bond between S and O and a single bond between the two sulfur atoms.