Complete the exercises below. Write the Lewis structure for each of the following species, and indicate the structure of each: a. SeO₃²⁻; b. S₂Cl₂; c. chlorosulfonic acid, HSO₃Cl (chlorine is bonded to sulfur).

Verified step by step guidance

1. Step 1: Determine the total number of valence electrons for each species. For SeO₃²⁻, calculate the valence electrons from Se and O, and add 2 for the charge. For S₂Cl₂, sum the valence electrons from S and Cl. For HSO₃Cl, sum the valence electrons from H, S, O, and Cl.
2. Step 2: Draw the skeletal structure for each species. For SeO₃²⁻, place Se in the center with O atoms around it. For S₂Cl₂, place the S atoms in the center with Cl atoms bonded to them. For HSO₃Cl, place S in the center with O, Cl, and H atoms bonded to it, ensuring Cl is bonded to S.
3. Step 3: Distribute the valence electrons around the atoms to satisfy the octet rule, starting with the outer atoms. For SeO₃²⁻, distribute electrons to the O atoms first. For S₂Cl₂, distribute electrons to the Cl atoms. For HSO₃Cl, distribute electrons to the O and Cl atoms.
4. Step 4: Check for formal charges and adjust the structure if necessary to minimize them. For SeO₃²⁻, consider forming double bonds between Se and O to reduce formal charges. For S₂Cl₂, ensure the formal charges are minimized. For HSO₃Cl, adjust bonds to minimize formal charges, especially around S.
5. Step 5: Verify that all atoms have complete octets (or duets for hydrogen) and that the total number of electrons used matches the total number of valence electrons calculated in Step 1.