Answer:
The structures are shown below.
Explanation:
The disulfur monoxide has molecular formula S₂O, and, to do the Lewis structure, we must write all the elements with their valence electrons. The bonds must be represented by lines.
Both sulfur and oxygen have 6 electrons at their valence shell, thus they must have to win 2 electrons to be stable (octet rule = 8 valence electrons). Thus, there are three possible structures for this molecule, which are called resonance structures. The resonance structures exist at the same time, and the molecule converts itself to be more stable.
The central atom must be one of the sulfur because it can expand the octet and has more than 8 valence electrons (all the elements from period 3 to 7 has this ability). So, the central sulfur can share 2 electrons with the other sulfur and 2 with the oxygen, or one electron with the sulfur and 2 with the oxygen, or 2 electrons with the sulfur and 1 with the oxygen.
The three structures are shown below.
