1.A) Draw all resonance structures for this compound (where all atoms have afilled valence shell). Show accurate electron pushing arrows.B) Assign all non-zero formal charges and show on each drawing.N=-CH22. A. Draw all resonance structures for the following compound (for moststructures, all atoms except one in each case should have a full valence shell. In onestructure, all atoms should have a full valence shell). Show any non-zero formalcharges and all electron pushing arrows.B. Circle the most important resonance structure for this compound. Noexplanation is required.

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Answered: 1. A) Draw all resonance structures for…

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter2: Lewis Structures

Section: Chapter Questions

Problem 17E

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Q4. Draw all the resonance contributing structures for each of the molecules or ions below. Be sure to include the curved arrows that indicate which pairs of electrons are moving in going from one resonance structure to the next. Be certain to show all valence electrons and all formal charges. a) CH3NO2 b) CH3CH=CHCH2
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3. The following shows all resonance structures for the following molecule. a. Draw in all implied lone pairs. b. Draw in curved arrows that show the flow of electrons, making sure the arrows show the precise starting point and destination of the electrons. Label each arrow as: lp →→→л (p=lone pair) c. d. Rank the resonance structures from most stable to least based on the number of formal charges and atoms that lack an octet of electrons. ol-of-o. B A D d-d-d-o E C F G
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In the following Lewis structure of [(CH3)2OH]*, every atom, bond and lone pair is positioned. To complete the structure, drag the formal charge tags to the appropriate atom(s). Each marker may be used more than once, or not at all. If an atom has a formal charge of zero, do not drag a tag to it. When you drag the marker in, place the little crosshairs in the upper left corner of the marker directly over the atom(s) in question (not above them). H. H-C Н-С-О-С-Н C-H H HH 2- II 2-
) Draw a Lewis structure the molecule or ion below. Draw any resonance structures. Determine the formal charges on atoms in each of your resonance structures. Based on this, determine which resonance structure(s) are most important. Circle the most important contributor(s) to the resonance hybrid. If they are all equivalent, circle them all. COFCl
A) 1) One of the following four structural formulas is not a permissible resonance contributor which one? Why? на HC на a) b) NFO c) H₂C HC H.C H₂C ks 2) Using curved arrows, show the electron movement that connects the three resonance contributors. لوج شركة السار NFO
5. Assign the appropriate formal charge to the indicated atoms. Here, lone pairs are shown for learning and clarity. In other words, consider the structure as drawn. In the future, only the charge will be drawn. Н NH2 Н .N'
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3. For each molecule below, draw two additional resonance reasonable structures. Be show sure to show how the resonance structures are related using formal arrow pushing. Rank the resonance structures from most stable to least stable (if they are the same stability rank them the same). Finally, draw the hybrid. ΝΗ G yg
1. Draw all the important resonance structures for the following ion showing all lone pairs of electrons, formal charges and double bonds. Show the electron flow by using arrows for full credit.) མ་
Q3. Circle the following pairs of structures that do not constitute resonance structures. H3C.CH3 H3C-N-CH3 a) b) H,C=C=CH2 H3C-CECH c) d) H3C CH2 H3C FCH2 OH e) H3C CH3 H,CCH2

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