b. Draw the resonance forms for ozone (bonded O–O–O)
c. Sulfur dioxide has one more resonance form than ozone. Explain why this structure is not possible for ozone.

Verified step by step guidance

1. To draw the resonance forms for ozone (O₃), start by considering the Lewis structure. Ozone consists of three oxygen atoms in a bent shape. The central oxygen atom is bonded to the other two oxygen atoms.
2. In the first resonance form, draw a double bond between the central oxygen and one of the terminal oxygens, and a single bond between the central oxygen and the other terminal oxygen. Assign formal charges: the oxygen with the double bond has a formal charge of 0, the central oxygen has a formal charge of +1, and the oxygen with the single bond has a formal charge of -1.
3. In the second resonance form, move the double bond to the other terminal oxygen. This means the double bond is now between the central oxygen and the other terminal oxygen. Reassign the formal charges: the oxygen with the double bond has a formal charge of 0, the central oxygen has a formal charge of +1, and the other terminal oxygen has a formal charge of -1.
4. For sulfur dioxide (SO₂), it has one more resonance form than ozone because sulfur can expand its octet, allowing for additional resonance structures. In SO₂, sulfur can form a double bond with each oxygen atom, resulting in three resonance forms: one with a double bond to one oxygen, one with a double bond to the other oxygen, and one with double bonds to both oxygens.
5. Ozone cannot have a resonance form with double bonds to both terminal oxygens because oxygen cannot expand its octet like sulfur can. Oxygen is limited to an octet configuration, which restricts the number of resonance forms compared to sulfur dioxide.

Key Concepts

Resonance Structures

Resonance structures are different Lewis structures for a molecule that depict the same arrangement of atoms but differ in the placement of electrons. They help illustrate the delocalization of electrons within a molecule, which can stabilize the molecule. Understanding resonance is crucial for predicting molecular behavior and properties.

Ozone Molecular Structure

Ozone (O3) consists of three oxygen atoms bonded in a linear arrangement. The molecule exhibits resonance, with electrons delocalized across the O-O-O bonds. This delocalization results in partial charges and bond lengths that differ from those predicted by a single Lewis structure, making resonance forms essential for accurate representation.

Sulfur Dioxide Resonance

Sulfur dioxide (SO2) has a bent molecular geometry and exhibits resonance with more possible structures than ozone due to the presence of sulfur, which can expand its octet. This allows for additional resonance forms, contributing to the molecule's stability. The difference in resonance forms between SO2 and O3 is due to sulfur's ability to accommodate more electrons than oxygen.