Concept explainers
Interpretation:
More stable contributing structure for each of the given structures is to be written, curved arrows are to be used which shows the transformation of the original Lewis formula to the new one and formal charges are to be specified.
Concept introduction:
The resonance structure with the greater number of covalent bonds contributes more to the resonance hybrid provided the octet rule is not exceeded for second-row elements.
A Lewis structure can have more than one structure; they are called resonating structures.
The movement of a pair of electrons is shown by curved arrows.
the structure in which the negative charge is present on the most electronegative atom and the positive charge is present on the least electronegative element is known as the major resonance contributor.
The species having the smallest separation of oppositely charged atoms is the major contributor.
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Organic Chemistry
- Draw the resonance structures for the following: ) Please use curved arrows to show how you push the electron(s), and add formal charges.arrow_forwardCalculate the formal charge for each atom that is not carbon or hydrogen in the following molecules.arrow_forwardDraw resonance structures for the following compound:Add curved arrow(s) to show resonance using one of the five patterns, and modify the second structure given to draw the new resonance structure. Include relevant formal charges in your structure. Use the + and - tools to add/remove charges to an atom, and use the single bond tool to add/remove double bonds.arrow_forward
- Draw in any lone pairs that are missing on the oxygen/nitrogen atoms and determine if there is a formal charge on those atoms.arrow_forwardAdd curved arrows to show how the first resonance structure can be converted to the second.arrow_forwardDraw the curved arrows to show the resonance structure for the following molecules. ( there are 3 molecules )arrow_forward
- In the following structures, write if necessary the formal charge that it must have. If you shouldn't have a load, please note that you don't have a load.arrow_forwardAll presented compounds contain oxygen atom in their structure. What is the formal charge on oxygen atom in each compound? PLEASE SOLVE FOR G, H, and I.arrow_forwardDraw the resonance structure for the following molecule: Just started with resonance, where would the arrows go? I'm unsure of this problem.arrow_forward
- Show the other two resonance structures of the following molecule (show the curved arrows). Indicate the major contributor. Draw the resonance hybrid.arrow_forwardWrite resonance structure for each of the following compounds and formal charges where appropriate. Which one most to hybrid? Explain.arrow_forwardEthanol, , is a compound in which the formal charge on all the atoms is zero. Under certain conditions the bond can be broken so that both electrons remain with the oxygen atom. The products are In this structure the oxygen owns one electron from shared pair and two electrons from each of unshared pairs. The total number of electrons belonging to oxygen is Oxygen is a Group element. The formal charge on the oxygen atom is . The correct Lewis structure for the ethoxide ion is Note that the other fragment, the proton, leaves with a formal charge of +1.arrow_forward
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning