Write Lewis structures for each molecule or ion. Include resonance structures if necessary and assign formal charges to all atoms. If you need to, expand the octet on the central atom to lower formal charge. a. SO4^2- b. HSO4^- c. SO3 d. BrO2^-

Verified step by step guidance

1. <b>Step 1:</b> Determine the total number of valence electrons for each molecule or ion. For ions, adjust the count by adding or subtracting electrons based on the charge.
2. <b>Step 2:</b> Identify the central atom (usually the least electronegative element) and arrange the other atoms around it. Connect each surrounding atom to the central atom with a single bond.
3. <b>Step 3:</b> Distribute the remaining valence electrons as lone pairs to satisfy the octet rule for each atom, starting with the most electronegative atoms. If necessary, expand the octet on the central atom to accommodate extra electrons.
4. <b>Step 4:</b> Check for resonance structures by moving electrons to form double or triple bonds where possible, ensuring that the formal charges are minimized across the structure.
5. <b>Step 5:</b> Calculate the formal charge for each atom using the formula: \( \text{Formal Charge} = \text{Valence Electrons} - \text{Non-bonding Electrons} - \frac{1}{2} \times \text{Bonding Electrons} \). Adjust the structure to minimize formal charges, expanding the octet if necessary.