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).

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They help visualize the arrangement of electrons and the connectivity of atoms, allowing chemists to predict molecular geometry and reactivity. Each dot represents a valence electron, while lines indicate covalent bonds between atoms.

Formal charge is a concept used to determine the distribution of electrons in a molecule. It is calculated by taking the number of valence electrons of an atom, subtracting the number of non-bonding electrons, and half the number of bonding electrons. This helps in assessing the most stable Lewis structure, as structures with formal charges closest to zero are generally preferred.

Resonance structures are different Lewis structures that represent the same molecule but differ in the arrangement of electrons. They are used when a single Lewis structure cannot accurately depict the electron distribution. The actual structure of the molecule is a hybrid of these resonance forms, which helps explain properties such as bond lengths and strengths that are intermediate between those predicted by individual structures.