Sulfur dioxide resonance structures

Resonance forms do not imply different kinds of molecules with electrons shifting eternally between them. There is only one type of S02 molecule its structure is intermediate between those of the two resonance forms drawn for sulfur dioxide. 

For sulfur dioxide, with resonating Lewis structure... 

I. Some of the pollutants in the atmosphere are ozone, sulfur dioxide, and sulfur trioxide. Draw Lewis structures for these three molecules. Show all resonance structures. 

You can draw resonance structures for sulfur dioxide, SO2, a chemical that can add to air pollution. 

Another molecule that has resonance structures is sulfur dioxide, SO2, shown in Figure 13. Sulfur dioxide released into the atmosphere is partly responsible for acid precipitation. The actual structure of SO2 is an average, or a resonance hybrid, of the two structures. Although you draw the structures as if the bonds change places again and again, the bonds do not in fact move back and forth. The actual bonding is a mixture of the two extremes represented by each of the Lewis structures. 

Draw two resonance structures for the sulfur dioxide molecule, SO2. 

Draw three resonance structures of sulfur dioxide (SO2). Indicate the most plausible structure(s). Hint See Example 9.11.)... 

Use Lewis formulas to depict the resonance structures of the following species from the valence bond point of view, and then sketch MOs for the delocalized tt systems (a) SO2, sulfur dioxide (b) O3 ozone (c) HC02, formate ion (H is bonded to C). 

Sulfur dioxide is produced by volcanic activity and the burning of snlfnr-containing coal. Once in the atmosphere, the SO2 is converted to SO3, which combines with water forming sulfuric acid, H2SO4, a component of acid rain. Draw two resonance structures for sulfur dioxide. 

Sulfur trioxide is produced from the catalytic oxidation of the dioxide. Its trigonal planar structure requires three resonance structures to describe. The very short S-0 bond distances seem to indicate that there are strong dir-fm interactions in addition to the expected delocalized fnr bonds. It is a powerful oxidizing agent. Although selenium and tellurium are less stable in the +6 oxidation state than is sulfur, both Se03 and Te03 can be prepared. 

By analog with sulfur dioxide, sulfur trioxide requires four resonance structures to fully describe the very strong S-O bonds that characterize this oxide. Draw four possible resonance structures and assign formal charges to all the atoms in each one. Describe the role of both tr- tr and dir-pir bonding in these structures. 

In a multiple covalent bond, all electrons in the bond are confined to the region between the bonded atoms, and together constitute one group of electrons. Let us test this idea by predicting the molecular geometry of sulfur dioxide. S is the central atom, and the total number of valence electrons is 3 X 6 = 18. The Lewis structure is the resonance hybrid of the three contributing structures shown below. 

---