Write Lewis structures that obey the octet rule for the following species. Assign the formal charge for each central atom. a. \(\mathrm{POCl}_{3} \quad\) c. \(\mathrm{ClO}_{4}^{-} \quad\) $\mathrm{e} \cdot \mathrm{SO}_{2} \mathrm{Cl}_{2} \quad\( g. \)\mathrm{ClO}_{3}^{-}$ b. \(\mathrm{SO}_{4}^{2-} \quad\) d. \(\mathrm{PO}_{4}^{3-} \quad\) f. \(\mathrm{XeO}_{4} \quad\) h. \(\mathrm{NO}_{4}^{3-}\)

To draw the Lewis structures for each species, start by identifying the central atom, then arrange the other atoms around it. Next, count the total number of valence electrons for all atoms, and then place lone pair electrons around the bonded atoms to achieve an octet configuration (or where it's allowed, a double or triple bond) for each atom. a. \(\mathrm{POCl}_{3}\) The central atom is P, and the total valence electrons are 5 (for P) + 3*7 (for Cl) = 26. The Lewis structure is: O || P-Cl |\ | Cl-Cl b. \(\mathrm{SO}_{4}^{2-}\) The central atom is S, and the total valence electrons are 6 (for S) + 4*6 (for O) + 2 (charge) = 32. The Lewis structure is: O- | S=O | O- c. \(\mathrm{ClO}_{4}^{-}\) The central atom is Cl, and the total valence electrons are 7 (for Cl) + 4*6 (for O) +1 (charge) = 32. The Lewis structure is: O- | Cl=O | O- d. \(\mathrm{PO}_{4}^{3-}\) The central atom is P, and the total valence electrons are 5 (for P) + 4*6 (for O) + 3 (charge) = 32. The Lewis structure is: O- | P=O | O- e. \(\mathrm{SO}_{2} \mathrm{Cl}_{2}\) The central atom is S, and the total valence electrons are 6 (for S) + 2*6 (for O) + 2*7 (for Cl) = 32. The Lewis structure is: O Cl || | S-Cl | O f. \(\mathrm{XeO}_{4}\) The central atom is Xe, and the total valence electrons are 8 (for Xe) + 4*6 (for O) = 32. The Lewis structure is: O || Xe=O || O g. \(\mathrm{ClO}_{3}^{-}\) The central atom is Cl, and the total valence electrons are 7 (for Cl) + 3*6 (for O) + 1 (charge) = 26. The Lewis structure is: O- | Cl=O | O- h. \(\mathrm{NO}_{4}^{3-}\) The central atom is N, and the total valence electrons are 5 (for N) + 4*6 (for O) + 3 (charge) = 32. The Lewis structure is: O- | N=O | O-

To calculate the formal charge of the central atom in each species, use the formula: Formal Charge = Valence Electrons - (0.5 * Bonding Electrons) - Non-bonding Electrons. a. Formal Charge for P: 5 - (0.5 * 8) - 0 = +1 b. Formal Charge for S: 6 - (0.5 * 12) - 0 = 0 c. Formal Charge for Cl: 7 - (0.5 * 12) - 0 = -1 d. Formal Charge for P: 5 - (0.5 * 12) - 0 = -1 e. Formal Charge for S: 6 - (0.5 * 12) - 2 = 0 f. Formal Charge for Xe: 8 - (0.5 * 16) - 0 = 0 g. Formal Charge for Cl: 7 - (0.5 * 10) - 0 = -1 h. Formal Charge for N: 5 - (0.5 * 12) - 0 = -1 Summary: a. P in \(\mathrm{POCl}_{3}\) has a formal charge of +1 b. S in \(\mathrm{SO}_{4}^{2-}\) has a formal charge of 0 c. Cl in \(\mathrm{ClO}_{4}^{-}\) has a formal charge of -1 d. P in \(\mathrm{PO}_{4}^{3-}\) has a formal charge of -1 e. S in \(\mathrm{SO}_{2} \mathrm{Cl}_{2}\) has a formal charge of 0 f. Xe in \(\mathrm{XeO}_{4}\) has a formal charge of 0 g. Cl in \(\mathrm{ClO}_{3}^{-}\) has a formal charge of -1 h. N in \(\mathrm{NO}_{4}^{3-}\) has a formal charge of -1