To calculate the formal charge on the sulfur atom in the compound SO, we need to follow these steps:1. Determine the number of valence electrons for the sulfur atom. Sulfur is in group 16 also known as group 6A of the periodic table, so it has 6 valence electrons.2. Calculate the number of bonding electrons. In SO, sulfur is bonded to three oxygen atoms through double bonds. Each double bond consists of 2 bonding pairs, so there are a total of 6 bonding pairs 3 double bonds x 2 bonding pairs per double bond = 6 bonding pairs . Since each bonding pair consists of 2 electrons, there are 12 bonding electrons 6 bonding pairs x 2 electrons per bonding pair = 12 bonding electrons .3. Calculate the number of non-bonding electrons. In SO, each oxygen atom has two lone pairs of electrons. Since there are three oxygen atoms, there are a total of 6 lone pairs 3 oxygen atoms x 2 lone pairs per oxygen atom = 6 lone pairs . Each lone pair consists of 2 electrons, so there are 12 non-bonding electrons 6 lone pairs x 2 electrons per lone pair = 12 non-bonding electrons .4. Calculate the formal charge on the sulfur atom using the following formula:Formal charge = Number of valence electrons - Number of bonding electrons/2 - Number of non-bonding electrons In this case, the formal charge on the sulfur atom is:Formal charge = 6 - 12/2 - 0 = 6 - 6 - 0 = 0Therefore, the formal charge on the sulfur atom in the compound SO is 0.