g) Draw the Lewis structure for SO_(3) and determine the formal charge for each atom . Which is the preferred Lewis structure?

To draw the Lewis structure for (sulfur trioxide), we need to follow these steps:1. Count the total number of valence electrons in the molecule: - Sulfur (S) has 6 valence electrons. - Oxygen (O) has 6 valence electrons, and there are 3 oxygen atoms. - Total valence electrons = 6 (S) + 3 × 6 (O) = 6 + 18 = 24 valence electrons.2. Determine the central atom: - Sulfur (S) is the central atom since it is less electronegative than oxygen.3. Draw the skeletal structure: - Place the sulfur atom in the center and arrange the three oxygen atoms around it.4. Distribute the valence electrons: - Form single bonds between the sulfur and each oxygen atom. - Distribute the remaining electrons to complete the octets of the oxygen atoms.5. Check the formal charges: - Calculate the formal charge for each atom using the formula: Formal charge = Valence electrons - Non-bonding electrons - Bonding electrons/2.The Lewis structure for is:``` O |S - O | O```The formal charges for each atom are:- Sulfur (S): 0- Oxygen (O): 0The preferred Lewis structure is the one with no formal charges, which is the structure shown above.