Draw three resonance structures for the sulfine molecule, \(\mathrm{H}_{2} \mathrm{CSO}\). Do not consider ring structures.

First, a Lewis structure needs to be drawn for the sulfine molecule, H2CSO. One can start by putting Sulfur (S) at the center, being the least electronegative atom and having the capability to form more bonds, then arrange Carbon (C) and Oxygen (O) around it. Next is to connect Hydrogen (H) atoms to the Carbon (C) since Hydrogen can only form one bond.

Remembering each bond represents two shared electrons and that the sum of the valence electrons for H2CSO is 18, arrange the remaining electrons so that every atom follows the octet rule - having eight electrons in its outer shell. Carbon will form a double bond with Sulphur. Distribute the remaining electrons equally between Sulphur and Oxygen.The initial Lewis structure should look like this:H-C=S=O (Sulphur and Oxygen both have two lone pairs of electrons)

Now to generate resonance structures, the idea is to shift electrons not atoms. The two electrons can be moved to form a double bond between Sulphur and Oxygen and that would break the π bond between Carbon and Sulphur moving two electrons down to Sulphur and forming a lone pair.The first resonance structure is: H2C-S=OFor the second resonance structure, the opposite can be done by forming a double bond between Carbon and Sulphur which breaks the π bond between Sulphur and Oxygen moving two electrons down to Oxygen and forming a lone pair. The second resonance structure is: H2C=S-OFor the third resonance structure, a lone pair of electrons from Oxygen can form a double bond with Sulphur, breaking the π bond between Sulphur and Carbon and moving two electrons down to Sulphur. The third resonance structure is: H2C-S=O