Concept explainers
Interpretation:
The fact that whether the given structures are resonance contributors of a single species or depict different substances is to be determined and the reason due to which the structures that are not resonance contributors is to be given.
Concept introduction:
According to the resonance concept, Lewis formulas that have different distribution of electrons in their structure can be written for a single molecule. Lewis formulas that confer to a resonance hybrid can be made easier to understand by using curved arrows to represent the delocalized electrons.
Each structure contributing to resonance must have an equal total number of valence electrons and the same value of net charge. Among the various Lewis formulas written for a molecule, the formal charges on individual atoms may vary. Each structure contributing to resonance must have the same number of unshared electrons.
When two or more structures satisfy the octet rule, the major contributor structure is the one with the smallest separation of oppositely charged atoms. The contributor structure with the least number of formal charges is more stable.
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Organic Chemistry - Standalone book
- Can you please explain why N-acetylamino group, -NHC(O)CH3, has a positive σ − value (0.47) but a negative σ + value (−0.6) using resonance structures.arrow_forwardSpecify whether the two structures are resonance contributors to the same resonance hybrid. Be sure to explain your reasoning. If yes, be sure to specify which is preferred and why. H2C=NH2arrow_forwardProvide the following 2 resonance structures and indicate whether or not they're major or minorarrow_forward
- For each example, specify whether the two structures are resonance contributors to the same resonance hybrid.arrow_forwardI am unsure of how to draw all the available resonance structures for these structures. Could anyone help please? Thank you.arrow_forwardHow is the resonance form of Acid Orange, drawn below, obtained? Redraw the molecule and show all arrows in your rationale. NaO3S HN-N=arrow_forward
- 3. Which of the following molecules are conjugated? For those which are conjugated, write a resonance structure.arrow_forwardDraw all the resonance contributors for the following molecule. Based on your resonance structures, which atoms are most electron deficient? Please re-draw the molecule and label these electron deficient molecules with "S+"- thus indicating it carries a partial positive charge.arrow_forward2. For the following ion, (1) draw important resonant forms to show delocalization of charge. Indicate the major resonance form(s), and justify your answerfs); (2) use a formal charge calculation to show why the ion shown below has a negative charge. NHarrow_forward
- Is the following true or false? Resonance is a useful tool to analyse intermediates, but cannot be used to examine starting materials or products.arrow_forward4. (i) On the structure below, add all missing lone pairs of electrons, assuming that all of the formal charges are correct. (ii) Draw line-angle structures for all resonance forms (including minor, but still significant) using appropriate notation, including double-headed resonance arrows and curved arrows for electrons. (Hint: Draw two more) (iii) Rank the three structures from most =1 to least =3 important.arrow_forwardConsider Lewis formulas A, B, and C:(a) Are A, B, and C constitutional isomers, or are they resonance contributors? (b) Which have a negatively charged carbon? (c) Which have a positively charged carbon? (d) Which have a positively charged nitrogen? (e) Which have a negatively charged nitrogen? (f) What is the net charge on each? (g) Which is a more stable structure, A or B? Why? (h) Which is a more stable structure, B or C? Why? (i) What is the CNN geometry in each according to VSEPR?arrow_forward
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning