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