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

The short version of the answer to the question is: a) \(\mathrm{POCl}_{3}\): Lewis structure: [P](=O)(-Cl)3, Formal charge of \(P\) = 0. b) \(\mathrm{SO}_{4}^{2-}\): Lewis structure: [S](=O)4 with two resonance structures, Formal charge of \(S\) = 0. c) \(\mathrm{ClO}_{4}^{-}\): Lewis structure: [Cl](=O)4, Formal charge of \(Cl\) = 0. d) \(\mathrm{PO}_{4}^{3-}\): Lewis structure: [P](=O)4 with three resonance structures, Formal charge of \(P\) = 0. e) \(\mathrm{SO}_{2}\mathrm{Cl}_{2}\): Lewis structure: [S](=O)2(-Cl)2, Formal charge of \(S\) = 0. f) \(\mathrm{XeO}_{4}\): Lewis structure: [Xe](=O)4, Formal charge of \(Xe\) = 0. g) \(\mathrm{ClO}_{3}^{-}\): Lewis structure: [Cl](=O)3(-O), Formal charge of \(Cl\) = 0. h) \(\mathrm{NO}_{4}^{3-}\): Lewis structure: [N](=O)4, Formal charge of \(N\) = +1.