Final answer:
The Lewis structures for CO2, SO2, NO3-, and O3 involve illustrating the valence electrons and bonding among atoms, with resonance structures shown for SO2, NO3-, and O3 to depict electron delocalization.
Step-by-step explanation:
The question pertains to the construction of Lewis electron dot structures for several molecules and ions, including resonance structures where applicable. These structures are a visual representation of the valence electrons around atoms, illustrating how the atoms in a molecule are bonded together.
- CO2: Carbon dioxide is a linear molecule with carbon in the center and double bonds to each oxygen atom. There are no resonance structures for CO2 as all the atoms have full octets with the existing double bonds.
- SO2: Sulfur dioxide has a bent V-shaped structure. It has resonance structures due to the ability to form double bonds with either oxygen atom, resulting in two possible structures with a single and a double bond to sulfur, alternating between the two oxygen atoms.
- NO3-: The nitrate ion has three resonance structures, each with a different nitrogen to oxygen double bond, while the other two nitrogen-oxygen bonds are single. This delocalization of the double bond is represented by resonance structures.
- O3: Ozone has a bent structure and contains two resonance forms, with a single double bond alternating between the left and the right oxygen atom.
Resonance structures are an important concept in chemistry to understand the distribution of electrons in molecules or ions where the electrons can be delocalized. It represents different possible structures that collectively describe the full electronic structure of the molecule or ion.