chapter 7 electron delocalization and resonance more about molecular orbital theory
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Chapter 7 Electron Delocalization and Resonance More about Molecular Orbital Theory. Adapted from Irene Lee Case Western Reserve University. Resonance. An intellectual explanation for observed differences in bond lengths and energies. The concept of e- delocalization stability. Lab: - PowerPoint PPT PresentationTRANSCRIPT
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Chapter 7
Electron Delocalization
and Resonance
More about MolecularOrbital Theory
Adapted from Irene LeeCase Western Reserve University
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Resonance
An intellectual explanation for observed differences in bond lengths and energies. The concept of e-
delocalization stability.
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Lab:ModelingExercise
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Pushing electrons:Need doublebonds
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Resonance Energy• A measure of the extra stability a compound gains from having delocalized electrons
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Benzene is stabilized by electron delocalization
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Benzene• A planar molecule
• Has six identical carbon–carbon bonds
• Each electron is shared by all six carbons
• The electrons are delocalized
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Resonance Contributors and the Resonance Hybrid
Resonance contributors are imaginary; the resonance hybrid is a weighted average that
explains experimental observations.
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electrons cannot delocalize in nonplanar molecules
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Drawing Resonance Contributors
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Resonance• Occurs when more than one valid
Lewis structure can be written for a particular molecule.
• These are resonance structures. The actual structure is an average of the resonance structures.
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Resonance: Delocalized Electron-Pairs
Ozone : O3 ...... .
.
O OO ........ ..OO
O..I II
O
O
O
....
.... ..
Resonance Hybrid Structure
One pair of electron’s resonates between the two locations!!
....
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Resonance and Formal Charge
Not as good Better
COO(-1)(0)(+1)COO(0)(0)(0)
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Acetic acid Acetic acid
Complete the Lewis Structure.Complete the Lewis Structure.
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Acetic acidAcetic acid
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Rules for Drawing Resonance Contributors
1. Only electrons move
2. Only electrons and lone-pair electrons move
3. The total number of electrons in the molecule does not change
4. The numbers of paired and unpaired electrons do not change
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The electrons can be moved in one of the following ways:
1. Move electrons toward a positive charge or toward a bond
2. Move lone-pair electrons toward a bond
3. Move a single nonbonding electron toward a bond
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Resonance contributors are obtained by moving electrons toward a positive charge:
CH2CH2CH2CH2CH2CH2δ+δ+δ+δ+
resonance hybrid
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Moving electrons toward a bond
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Moving a nonbonding pair of electrons toward a bond
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Resonance Structures for the Allylic Radical and for the Benzyl Radical
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Note
• Electrons move toward an sp2 carbon but never toward an sp3 carbon
• Electrons are neither added to nor removed from the molecule when resonance contributors are drawn
• Radicals can also have delocalized electrons if the unpaired electron is on a carbon adjacent to an sp2 atom
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The Difference Between Delocalized and Localized Electrons
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Resonance contributors with separated charges are less stable
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Electrons always move toward the more electronegativeatom
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When there is only one way to move the electrons,
because electron delocalization makes a molecule more stable
movement of the electrons away from the more electronegative atom is better than no movement at all
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Features that decrease the predicted stability of a contributing resonance structure …
1. An atom with an incomplete octet
2. A negative charge that is not on the most electronegative atom
3. A positive charge that is not on the most electropositive atom
4. Charge separation
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Summary• The greater the predicted stability of a resonance contributor, the more it contributes to the resonance hybrid
• The greater the number of relatively stable resonance contributors, the greater is the resonance energy
• The more nearly equivalent the resonance contributors, the greater is the resonance energy
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Resonance-Stabilized Cations
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Relative Stabilities of Allylic and Benzylic Cations
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Relative Stabilities of Carbocations
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Relative Stabilities of Radicals
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Some Chemical Consequences of Electron Delocalization
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Why is RCO2H more acidic than ROH?
Electron withdrawal by the double-bonded oxygen decreases the electron density of the negatively charged oxygen, thereby stabilizing the conjugated base (the carboxylate)
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Increased resonance stabilization of the conjugated base
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Account for the Acidity of Phenol by Resonance Stabilization
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Account for the Acidity of Protonated Aniline by Resonance Stabilization
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A Molecular Orbital Description of Stability
• Bonding MO: constructive (in-phase) overlap• Antibonding MO: destructive (out-of-phase) overlap
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The Molecular Orbitals of 1,3-Butadiene
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Symmetry in Molecular Orbitals
1 and 3 in 1,3-butadiene are symmetrical molecular orbitals
2 and 4 in 1,3-butadiene are fully asymmetrical orbitals
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• HOMO = the highest occupied molecular orbital
• LUMO = the lowest unoccupied orbital
• The highest-energy molecular orbital of 1,3-butadiene that contains electrons is 2 (HOMO)
• The lowest-energy molecular orbital of 1,3-butadiene that does not contain electrons is 3 (LUMO)
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Consider the molecular orbitals of 1,4-pentadiene:
This compound has four electrons that are completelyseparated from one another
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The Molecular Orbitals of the Allyl System
No overlap between the p orbitals: the nonbonding MO
2 is the nonbonding MO
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The Molecular Orbitals of 1,3,5-Hexatriene
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Benzene has six molecular orbitals
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Benzene is unusually stable because of large delocalization energies