(a) Describe the molecule xenon trioxide, \(\mathrm{XeO}_{3}\), using four possible Lewis structures, one each with zero, one, two, or three \(\mathrm{Xe}-\mathrm{O}\) double bonds. \((\mathbf{b})\) Do any of these resonance structures satisfy the octet rule for every atom in the molecule? (c) Do any of the four Lewis structures have multiple resonance structures? If so, how many resonance structures do you find? (d) Which of the Lewis structures in part (a) yields the most favorable formal charges for the molecule?

We will begin by creating four Lewis structures with zero, one, two, or three Xe–O double bonds. (a) For each structure, start with the central atom, \(Xe\), and add \(O\) atoms with appropriate numbers of double bonds: 1. 0 double bonds: All Xe–O bonds are single. 2. 1 double bond: Two Xe–O bonds are single, and one is a double bond. 3. 2 double bonds: One Xe–O bond is single, and two are double bonds. 4. 3 double bonds: All Xe–O bonds are double. Don't forget to add lone pairs to ensure each atom reaches its octet.

(b) Now, we'll examine each structure and see if it satisfies the octet rule: 1. 0 double bonds: Xe has 3 single bonds and 2 lone pairs (10 electrons in total), O atoms have 2 lone pairs each (8 electrons for each O atom). This structure does not satisfy the octet rule for the Xe atom. 2. 1 double bond: Xe has 2 single bonds, 1 double bond, and 1 lone pair (9 electrons in total), O atoms have 2 lone pairs each (8 electrons for each O atom). This structure does not satisfy the octet rule for the Xe atom. 3. 2 double bonds: Xe has 1 single bond, 2 double bonds, and no lone pair (8 electrons in total), O atoms have 2 lone pairs each (8 electrons for each O atom). This structure satisfies the octet rule for all atoms. 4. 3 double bonds: Xe has 3 double bonds and no lone pair (6 electrons in total), O atoms have 2 lone pairs each (8 electrons for each O atom). This structure does not satisfy the octet rule for the Xe atom.

(c) The structure with 2 double bonds between Xe and O atoms can have resonance structures. The resonance can occur by moving one of the double bonds to the other single bond in the structure. There are three possible resonance structures for this molecule.

(d) The Lewis structure with 2 double bonds between Xe and O atoms is the most favorable because it satisfies the octet rule for all atoms. Moreover, the formal charges on the atoms in this structure are more favorable compared to other possible structures: - Xe has a formal charge of 0. - Double-bonded O atoms have a formal charge of 0. - The single-bonded O atom has a formal charge of -1. This Lewis structure with 2 double bonds and its resonance structures best represent the molecule xenon trioxide.