Concept explainers
(a)
Interpretation: The missing formal charges in below set of resonance structure should be added. Also, unimportant resonance structure should be determined.
Concept introduction: Lewis structure is representation of molecule 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 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 resonance structure of anions in movement of negative charge.
2. Use only arrow type 3 to move a positive charge for 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 same in all resonance structures.
(b)
Interpretation: The missing formal charges in below set of resonance structure should be added. Also, unimportant resonance structure should be determined.
Concept introduction: Lewis structure is representation of molecule 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 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 resonance structure of anions in movement of negative charge.
2. Use only arrow type 3 to move a positive charge for 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 same in all resonance structures.
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Chapter 5 Solutions
Organic Chemistry: A Guided Inquiry
- Add curved arrows to show how the first resonance structure can be converted into the second.arrow_forward1. A) Draw all resonance structures for this compound (where all atoms have a filled valence shell). Show accurate electron pushing arrows. B) Assign all non-zero formal charges and show on each drawing. N= -CH2 2. A. Draw all resonance structures for the following compound (for most structures, all atoms except one in each case should have a full valence shell. In one structure, all atoms should have a full valence shell). Show any non-zero formal charges and all electron pushing arrows. B. Circle the most important resonance structure for this compound. No explanation is required.arrow_forwardFor the following Structure, a) draw in any missing lone pairs; b) identify and list the resonance patterns (i.e. allylic cation) present. If one pattern shows up more than once, list it multiple times c) draw curved arrows on the initial structure to produce a resonance structure, including formal charge. (hint - use a minimum of curved arrows for each resonance structure). Repeat on the second structure to generate a third structure. Rank the resonance structures in order of decreasing importance: 1 is most important, 2 is second most important, etc... H Pattern 1: Pattern 2: Rank: Pattern 1: Pattern 2: Rank: Pattern 1: Pattern 2: Rank:arrow_forward
- Specify the number of unshared pairs of electrons necessary to complete the valence shell of the labeled atoms, a-c in the following structures. Specify "0" if no pair of electron and that the atoms are NOT labeled in sequence. needs to be added. Notice that formal charges are indicated by or 1. 2. ob d a de C H H H a a b C b ✓Carrow_forwardIn 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-arrow_forwardPlease provide explanationarrow_forward
- This question requires you to show arrow pushing! Draw all lone pairs on the 5) 6 molecule below first and next draw at least six resonance structures upon delocalization of appropriate electrons. show formal charges on each resonance structure NH2arrow_forward11. Add curved arrows to the following structures to show how electron pairs must be moved to interconvert the structures, and locate any formal charges. This is the nitrate ion and it has three resona onance structures (RS). וך- :ó: :0: 1. supply formal charges 1. supply formal charges 2. draw e pushing arrows draw third RS here 2. draw e¯ pushing arrows that make second RS to make third RSarrow_forwardDraw all resonance structures for the following compounds. Include curved www arrows NH₂arrow_forward
- For the following, use curved arrows to show the transformation of one resonance structure into another. Label the major and minor resonance forms (major and minor contributors to the resonance hybrid), and show which ones are of equal energy. Briefly justify your choices. Draw the structure of the resonance hybrid. [re % la] uarrow_forward3. Draw all resonance structures for the following radicals.arrow_forwardThe structure of Vitamin C (ascorbic acid) is shown below. As the name indicates, the molecule is somewhat acidic. Actually, one of the hydrogens on the four OH groups is much more acidic than the other three ones. Which one is the acidic hydrogen? Hints: To find the answer, you will again have to draw some resonance structures of the product formed after loss of H+. Consider the product after the loss of H+ for each of the OH groups. Only two of the OH groups have resonance structures after deprotonation; one of these two groups has a much better resonance structure than the other one (again after deprotonation). Note that the oxygen atom that is part of the five-membered ring has nothing to do with the problem.arrow_forward
Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning