Concept explainers
Interpretation: Whether the cation given below gives two resonance structures or not should be determined.
Concept introduction: Lewis structure is a representation of molecules in which dots are shown to represent unshared electrons and lines are shown to represent bonds. These lines and dots represent distribution of electrons in the molecule.
When one single structure is unable to describe all the properties of a single-molecule, a phenomenon called resonance comes into play. This arises when two or more than two Lewis structures are possible for one molecule. All such structures are called resonating structures and have same placement of atoms in them but these have different locations of bond pairs and lone pairs. The resonating structures are inter-convertible with each other. The resultant of all the resonating or contributing structures is called the resonance hybrid.
Rules to form resonance structure are as follows:
1. Use arrow types 1 and 2 for the resonance structure of anions in the movement of negative charge.
2. Use only arrow type 3 to move a positive charge for the resonance structure of cations.
3. The sigma bond should not be broken. Any atom must not move from its place and total number of electrons must be the same in all resonance structures.
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Organic Chemistry: A Guided Inquiry
- The instructions are to draw the resonance hybrid structure of the molecule on the left. My answer is circled , which is wrong. Can someone explain why?arrow_forwardOne of the orbital interactions we did not consider in this chapter is that between an s AO from one atom and a p AO from another atom in the fashion shown. These orbitals will not interact while in this orientation. Explain why.arrow_forwardConsider the resonance scheme shown below. Select the correct answer from the list below. t an arrow incorrectly starts at the positive charge the charge on the carbons needs to be negative This mechanism is free of errors. the charge on the carbons is not positivearrow_forward
- (e) Chemical bonds can also be classified as single or number of according to thearrow_forwardExamine the molecule below, and select the statements that apply. If it can lose H ', draw its conjugate base. If it can gain H', draw its conjugate acid. Show all lone pairs and non-zero formal charges. O This molecule will not lose an H" O This molecule will not gain an H" O This molecule could lose an H". Its conjugate base is: O This molecule could gain an H". Its conjugate acid is:arrow_forwardPlease explain the R clockwise to S in your answerarrow_forward
- a model of each molecule shown above: Is the molecule in the left box the same moleculeas the molecule in the right box? Use your models to answer the question, and recall that...arrow_forwardDescribe with words how you would draw the curved arrow(s) to get to the more stable resonance form for the left-hand pair. Be sure to include how many curved arrows are needed and what atom (or bond) the electrons are coming from or going to. Do the same for the resonance pair on the right-hand side. more stable more stablearrow_forwardSee image belowarrow_forward
- Please solve correctly.arrow_forwardIn the molecule shown label the indicated bonds with either their hybridization (sp,sp2,sp3) or the type of bond present (sigma, pi )arrow_forwardanswer 3 and 5. PLS MAKE IT LIKE THIS WAY SO THAT I UNDERSTAND IT IONIC YES OR NO POLAR YES OR NO NON POLAR YES OR NO IMF EXIST IS..... NO EXPLANATION NEEDED.arrow_forward
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning