Lewis structure of SO2

[Qinyan Feng 1H]

Hi

For the lewis structure of SO2, does the S form double bonds with both O atoms, or it forms a double bond with one O atom and a single bond with another atom? I think they are resonance structures right? I just wonder which form will be dominant.

Thank you!

[Josephine B 3L]

Hi!

Yes, those are resonance structures and I'm pretty sure that S forms a double bond with each of the Os and the last lone pair goes on the S because it can expand its octet. This one is dominant because it allows both of the oxygen atoms to have a formal charge of zero (oxygens have a formal charge of zero when they have two bonded pairs and two lone pairs FC of oxygen= V-L-B/2 = 6 - 4 - 4/2 = 0 when double bond and two lone pairs).

Hope this helps!

[Raizel Ferrer 1H]

Yes, they are resonance structures! To find which resonance structure is more dominant is which structure has the least formal charge. The lower energy the structure is, the more stable it is and the more it contributes to the resonance structure.

[Sanskriti Balaji 1J]

Hi! Either structure works for SO2 since it has resonance! To figure out the dominant structure, you would have to find the formal charge of each structure using this formula: (Valence Electrons) - (Lone Pairs + Bonded Pairs/2)!

[605721741]

The lewis structure of SO2 is just like CO2!

[Aneesha_Nema_3C]

Both structures are resonance structures, and we would need to look a the formal charges on all of the atoms to see which would be the dominant structure. If S is double bonded to both atoms, then the formal charges of all of the atoms are 0, and sulfur is able to have an expanded octet, which allows this to be viable.

[Alyssa Gutierrez 3A]

In order to have a stable molecule, we would need to make sure that the formal charge is 0 or matches the overall charge of the molecule. In this case, by having a double bond between the Oxygens, they will have a formal charge of 0. The extra electrons will be given to S, since it is also able to have an expanded octet.

[Alyssa Gutierrez 3A]

In order to have a stable molecule, we would need to make sure that the formal charge is 0 or matches the overall charge of the molecule. In this case, by having a double bond between the Oxygens, they will have a formal charge of 0. The extra electrons will be given to S, since it is also able to have an expanded octet.

[Ashrita Singh 2F]

It has two double bonds, as O typically forms double bonds when in lewis structures. The formal charge for the arrangement with double bonds is also lower, meaning that it is more stable.

[Brooklyn Burgess 3L]

How do you know how to create the lewis structure for more complex molecules such as CH3COOH?

[cnyland]

SO2 and CO2 have same!