To calculate the formal charge of the central atom sulfur in SF4, we need to follow these steps:1. Determine the number of valence electrons for sulfur S . Sulfur is in group 16, so it has 6 valence electrons.2. Calculate the number of bonding electrons. In SF4, there are 4 single bonds between sulfur and fluorine, so there are 4 x 2 = 8 bonding electrons.3. Calculate the number of non-bonding electrons. Subtract the number of bonding electrons from the total valence electrons: 6 valence electrons - 8 bonding electrons = -2 non-bonding electrons.4. Calculate the formal charge. The formula for formal charge is: Formal Charge = Valence Electrons - Non-bonding Electrons + 1/2 Bonding Electrons . In this case, Formal Charge = 6 - -2 + 1/2 * 8 = 6 - 0 = 0.The formal charge of the central atom sulfur in SF4 is 0.Now, let's check if the molecule is overall neutral or has a partial charge. Fluorine has 7 valence electrons, and each fluorine atom forms a single bond with sulfur. So, the formal charge on each fluorine atom is:Formal Charge = Valence Electrons - Non-bonding Electrons + 1/2 Bonding Electrons Formal Charge = 7 - 6 + 1/2 * 2 = 7 - 7 = 0Each fluorine atom has a formal charge of 0. Since there are 4 fluorine atoms and the sulfur atom also has a formal charge of 0, the overall charge of the SF4 molecule is 0. Therefore, the molecule is overall neutral.