Concept explainers
Interpretation:
An energy diagram for the three molecular orbitals of the cyclopropenyl system is to be drawn. How these three molecular orbitals are occupied in the cyclopropenyl anion, cation and radical is to be indicated. Which among the three is
Concept introduction:
The numberof molecular orbitals formed is equal to the number of orbitals overlapping. The available orbitals are filled by the electrons in the increasing order of their energies.Each moleclar orbital can accommodate two electrons with opposite spin. Electrons occupy the orbitals individually first before they get paired in the same orbital.
The cyclopropenyl cation has two electrons to be filled in molecular orbitals.
The cyclopropenyl radical has three electrons to be filled in molecular orbitals.
The cycloproenyl anion has four electrons to be filled in molecular orbitals.
To draw:
The relative energy levels of the three π molecular orbitals of the cyclopropenyl cation, radical and anion.
To indicate:
How the three π molecular orbitals are filled in cyclopropenyl cation, radical and anion.
To state:
Which of these three are aromatic.
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Chapter 15 Solutions
Organic Chemistry
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- Determine if the following compounds are aromatic, non-aromatic, or anti-aromatic. Show a structure that helps to support your classification. This structure should not just redraw the compound; show lone pairs, resonance, and/or contributing π bonds as part of your explanation.arrow_forwardIn the molecular orbital model of cyclopentadienyl cation, how many pi-electrons are in bonding molecular orbitals? FOUR SEVEN OTWO O SIX O FIVE THREEarrow_forwardCompare the structures of 1,4-pentadiene and divinylamine: 1,4-Pentadiene The first compound does not absorb UV light in the region between 200 and 400 nm. The second compound does absorb light above 200 nm. Using this information, identify the hybridization state of the nitrogen atom in divinylamine. O sp³ hybridized O sp³d hybridized sp² hybridized O sp hybridized N H Divinylamine Justify your answer. The lone pair is a part of the TT system in the second compound. Therefore the compound is conjugated ✓ .As such, the compound absorbs light above 200 nm (UV light). In contrast, 1,4-pentadiene has two double bonds and therefore does not absorb UV light in the region between 200 and 400 nm. 3 isolated cumulated conjugatedarrow_forward
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningOrganic ChemistryChemistryISBN:9781305580350Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. FootePublisher:Cengage Learning