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(a) Draw the resonance forms for SO2 (bonded O—S—O)(b)

Organic Chemistry | 8th Edition | ISBN: 9780321768414 | Authors: L.G. Wade Jr ISBN: 9780321768414 33

Solution for problem 20SP Chapter 1

Organic Chemistry | 8th Edition

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Organic Chemistry | 8th Edition | ISBN: 9780321768414 | Authors: L.G. Wade Jr

Organic Chemistry | 8th Edition

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Problem 20SP

Problem 20SP

(a) Draw the resonance forms for SO2 (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.

Step-by-Step Solution:

Problem 20SP

(a) Draw the resonance forms for SO2 (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.

                                              Step by step solution

Step 1 of 3

a)

The Lewis structure of  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 pair 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.

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Therefore, possible resonance structures are as follows.

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Step 2 of 3

Chapter 1, Problem 20SP is Solved
Step 3 of 3

Textbook: Organic Chemistry
Edition: 8
Author: L.G. Wade Jr
ISBN: 9780321768414

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(a) Draw the resonance forms for SO2 (bonded O—S—O)(b)