![]() Using this formula, you will find out that when there are four single bonds in this molecule, each Oxygen atom has a charge of -1, and the Sulphur atom has a charge of -2. You can either use our Formal charge calculator to find the charges on the atoms or use the following formula:į.C = Valence electrons – Nonbonding pairs of electrons * ½ bonding pairs of electrons Now doing this, you might wonder that this is the correct way to present the Lewis Structure, but it is suggested to calculate the formal charges to do so. Start putting these electrons around the Oxygen atom, as Sulphur has shared four electrons with the Oxygen atoms. Placing four single bonds will use eight valence electrons out of 32, which means we are only left with 24 valence electrons now. So place a pair of electrons between each Oxygen and Sulphur atom to show a single bond. Now that you have the arrangement of the atoms in the molecule, we can look at the bonding of atoms.Īs mentioned above, each atom will try to have eight valence electrons in its outer shell to attain a stable structure. So place a Sulfur atom in the center and Oxygen atoms around it. ![]() So as a result of this Sulphur atom will take the central position, and all the Oxygen atoms are arranged around it. In SO42-, if you compare the electronegativities of Sulphur and Oxygen atoms, Oxygen is more electronegative than Sulphur atoms. This doesn’t apply to Hydrogen atoms, as these atoms never take the central position. To determine which atom takes the central atom, always remember that the less electronegative atom takes the central position, and more electronegative atoms are arranged around it. Here as we already have the total number of valence electrons, we can start by determining the central atom.
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