Consider the incomplete structure. Add formal charges as necessary to the structure. All unshared valence electrons areshown. Do not alter the structure-just add charges. If you need to revert the drawing palette to the original state, select theMore menu, then select Reset Drawing.Add formal chargesWhat is the net charge on the species?+17L+2 Add formal charges4What is the net charge on the species?O +10 0 0 0 0-20-1+2FeedbackAt least one of the atoms in youranswer is missing a formal charge orshows an incorrect formal charge.These hints may help you identifythe issue and correct it.Oxygen is in group 6A and thus has6 valence electrons per neutral atom.In this structure, however, oxygen isshown with a valence-electron countof 7, so it has excess negative charge.Chlorine is in group 7A and thus has7 valence electrons per neutral atom.In this structure, however, chlorine isshown with a valence-electron countof 4, so it is electron-deficient.

A question based on electronic effects. 2 subdivision questions are given that are to be determined…

Consider the incomplete structure. Add formal charges as necessary to the structure. All unshared valence electrons are shown. Do not alter the structure-just add charges. If you need to revert the drawing palette to the original state, select the More menu, then select Reset Drawing. Add formal charges What is the net charge on the species? O +1 -2 ± 0000 -1 +2

Consider the incomplete structure. Add formal charges as necessary to the structure. All unshared valence electrons are shown. Do not alter the structure-just add charges. If you need to revert the drawing palette to the original state, select the More menu, then select Reset Drawing. Add formal charges What is the net charge on the species? O +1 -2 ± 0000 -1 +2

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter2: Lewis Structures

Section: Chapter Questions

Problem 13CTQ: A complete Lewis structure must show all nonzero formal charges. Complete each of thefollowing Lewis...

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