Solution Found!
(a) Draw the resonance forms for SO2 (bonded O—S—O)(b)
Chapter 1, Problem 20SP(choose chapter or problem)
(a) Draw the resonance forms for \(\mathrm{SO}_{2}\) (bonded O—S—O)
(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.
Questions & Answers
QUESTION:
(a) Draw the resonance forms for \(\mathrm{SO}_{2}\) (bonded O—S—O)
(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.
ANSWER:
Step 1 of 3
a) The Lewis structure of \(\mathrm{SO}_{2}\) is as follows.
By moving an electron pair in one of the double bonds towards oxygen, the resonance structure for a molecule is drawn, so this creates a lone pair on an oxygen atom that develops a charge of -1. Due to the movement of the electron pair "S" and produces a charge of +1 by losing one electron.
In the above formed resonance structure, lone pairs on negatively charged oxygen move to form a double bond between “S” and “O”. While the lone pair on the existing double bond moves onto “O” as lone pair, this develops a negative charge of -1.
Therefore, possible resonance structures are as follows.
