![]() This arrangement is shown in the figure below. By taking advantage of the Sulfur atom’s expanded octet, we can accommodate two double bonds. However, in theory, we’d need the formal charges to be as close to zero as possible. Either of the Oxygen atoms can take part in the double bond formation with the central Sulfur atom. The formal charges from the above table are represented graphically below. It is determined such that the elemental charge on each atom is closest to zero.įC = Valence Electrons – Non-bonding electrons – (Bonding electrons ÷ 2) To verify the stability of this Lewis structure, we can calculate its formal charges.įormal charges for an element/structure help determine its most stable Lewis Structure state. This double bond meets the sulfur atom’s octet requirements, seemingly giving us our SO 2 Lewis structure. We form a double bond between one of the oxygen atoms and the central sulfur atom to address this. The two oxygen atoms’ octet requirements have been met however, this is not the case for Sulfur. This arrangement leaves us with a lone pair on the central sulfur atom, as shown below. The remaining valence electrons are then used to fill the outermost shells of the Oxygen atoms on the outside. From the 18 valence electrons available, four are used to form covalent bonds between Sulfur and Oxygen atoms. The two oxygen atoms are arranged adjacent to the central sulfur atom. Sulfur is the least electronegative atom in the compound and will act as the central atom. Now that we’ve calculated the number of valence electrons available to us, we move on towards building up the Lewis structure for SO 2. Thus, the total number of valence electrons available to form is given by:Ħ + 12 = 18 valence electrons. Therefore, the two Oxygen atoms present contribute 6 x 2 = 12 valence electrons. Oxygen’s electronic configuration is 1s 2 2s 2 2p 4. Oxygen has six valence electrons (group 6) and has a valency of -2. Therefore, the Sulfur atom contributes 6 x 1 = 6 valence electrons Sulfur is in group 6(Chalcogens) of the periodic table with the electronic configuration 3s☣p⁴. There are two oxygen atoms and one sulfur atom present in SO 2. As such, they can potentially break free to take part in bond formation and exchanges.Įach constituent atom in the compound contributes a set amount of valence electrons to the overall structure. They are found in the atom’s outermost shell, where the force of attraction from the nucleus is the weakest. These valence electrons act as the building blocks of the structure. To form the Lewis structure of Sulfur Dioxide, we need first to determine the number of valence electrons available. ![]()
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