Concept explainers
(a)
Interpretation:
The bond order of each carbon-carbon bond in the allyl cation is to be calculated.
Concept introduction:
Resonance structure is a blend of two or more Lewis structures. Resonance structures are represented by a double headed arrow between the structures. Two resonance structures are possible for the allyl cation.
(b)
Interpretation:
The positive charge which resides on each carbon of the allyl cation is to be calculated.
Concept introduction:
Resonance structure is a blend of two or more Lewis structures. Resonance structures are represented by a double headed arrow between the structures. Two resonance structures are possible for the allyl cation.
(c)
Interpretation:
The reason as to why the structure on the right is not a reasonable resonance structure is to be explained.
Concept introduction:
Resonance structure is a blend of two or more Lewis structures. Resonance structures are represented by a double headed arrow between the structures. Two resonance structures are possible for the allyl cation.
Want to see the full answer?
Check out a sample textbook solutionChapter 1 Solutions
Organic Chemistry
- The structure of pyridine is When a proton becomes bonded to the nitrogen atom by way of its unshared electron pair, the result is _____________________________arrow_forwardDo any of the atoms in an ibuprofen molecule have a nonzero formal charge?arrow_forwardThe Lewis structure of acetone is Circling the carbonyl carbon, i.e., the carbon atom attached to oxygen, and its octet gives Circling the oxygen atom and its octet gives Thus, atoms share electrons in making bonds, and a pair of electrons may be included in the octet of two different atoms. When computing the formal charge on an atom, the number of electrons that belong to that atom is compared with the number of electrons the atom would have in the unbonded and neutral state. If the two numbers are the same, the formal charge on the atom is zero. In a Lewis structure both electrons in an unshared pair belong to the atom, and one of every pair of shared (bonding) electrons belongs to the atom.arrow_forward
- The cyclohexane carboxylate anion has a Lewis structure Pushing a pair of unshared electrons away from the negatively charged oxygen atom and, at the same time, pushing a pair of pi electrons toward the other oxygen will generate a second resonance structure. Thus,arrow_forwardGiven the following electro negativities C=2.5N=3.0S=2.6 what is the central atom in CNS-?arrow_forwardIn each of the following Lewis diagrams, Z represents a main-group element. Name the group to which Z belongs in each case and give an example of such a compound or ion that actually exists.arrow_forward
- In each of the following molecules, a central atom is surrounded by a total of three atoms or unshared electron pairs: SnCl2, BCl3, SO2. In which of these molecules would you expect the bond angle to be less than 120? Explain your reasoning.arrow_forwardHow many possible resonance structures can you have in total for the nitrite ion.arrow_forwardWhat is the formal charge of the nitrogen in the following molecule?arrow_forward
- Shown here is a Lewis structure for the chlorite ion, ClO2–, that obeys the octet rule, showing all non-zero formal charges. How many resonance structures for ClO2– that obey the octet are possible? Note: Options 2 and 3 are marked wrongarrow_forwardWhat is the method of calculating the formal charge on any atom?arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning