chapter 15 conjugated systems, orbital symmetry, and ultraviolet spectroscopy jo blackburn richland...
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Chapter 15Conjugated Systems, Orbital Symmetry, and
Ultraviolet Spectroscopy
Jo BlackburnRichland College, Dallas, TX
Dallas County Community College District2003,Prentice Hall
Organic Chemistry, 5th EditionL. G. Wade, Jr.
Chaper 15 2
Definitions
• Conjugated double bonds are separated by one single bond. Example: 1,3-pentadiene.
• Isolated double bonds are separated by two or more single bonds. 1,4-pentadiene.
• Cumulated double bonds are on adjacent carbons. Example: 1,2-pentadiene. =>
Chaper 15 3
Resonance Energy
• Heat of hydrogenation for trans-1,3-pentadiene is less than expected.
H for 1-pentene is 30.0 kcal/mol and for trans-2-pentene is 27.4 kcal/mol, so expect 57.4 kcal for trans-1,3-pentadiene.
• Actual H is 53.7 kcal, so the conjugated diene is more stable.
• Difference, (57.4 – 53.7) 3.7 kcal/mol, is the resonance energy. =>
Chaper 15 4
Relative Stabilities
twice 1-pentene
more substituted
=>
Chaper 15 5
Structure of 1,3-Butadiene• Most stable conformation is planar.
• Single bond is shorter than 1.54 Å.
• Electrons are delocalized over molecule.
=>
Chaper 15 6
Constructing Molecular Orbitals
• Pi molecular orbitals are the sideways overlap of p orbitals.
• p orbitals have 2 lobes. Plus (+) and minus (-) indicate the opposite phases of the wave function, not electrical charge.
• When lobes overlap constructively, (+ and +, or - and -) a bonding MO is formed.
• When + and - lobes overlap, waves cancel out and a node forms; antibonding MO. =>
Chaper 15 7
1 MO for 1,3-Butadiene
• Lowest energy.• All bonding
interactions.• Electrons are
delocalized over four nuclei.
=>
Chaper 15 8
2 MO for 1,3-Butadiene
• 2 bonding interactions
• 1 antibonding interaction
• A bonding MO
=>
Chaper 15 9
3* MO for 1,3-Butadiene
• Antibonding MO
• Empty at ground state
• Two nodes =>
Chaper 15 10
4* MO for 1,3-Butadiene
• All antibonding interactions.
• Highest energy.
• Vacant at ground state.
=>
Chaper 15 11
MO Energy Diagram
The average energy of electrons is lower in the conjugated compound.
=>
Chaper 15 12
Conformations of 1,3-Butadiene
• s-trans conformer is more stable than the s-cis by 2.3 kcal.
• Easily interconvert at room temperature.
HH
H
H
H
H
s-trans s-cis
H
H
H
H
HH
=>
Chaper 15 13
Allylic Cations• Carbon adjacent to C=C is allylic.
• Allylic cation is stabilized by resonance.
• Stability of 1 allylic 2 carbocation.
• Stability of 2 allylic 3 carbocation.
H2C C
H
CH2+
H2C C
H
CH2
+
=>
Chaper 15 14
1,2- and 1,4-Additionto Conjugated Dienes
• Electrophilic addition to the double bond produces the most stable intermediate.
• For conjugated dienes, the intermediate is a resonance stabilized allylic cation.
• Nucleophile adds to either carbon 2 or 4, both of which have the delocalized positive charge. =>
Chaper 15 15
Addition of HBr
H2C C
H
C
H
CH2H
+
H3C C
H
C
H
CH2+
H3C C
H
C
H
CH2+
Br_
Br_
H3C C
H
C
H
CH2
Br
H3C C
H
C
H
CH2
Br
1,2-addition product 1,4-addition product
=>
Chaper 15 16
Kinetic vs. Thermodynamic Control
Major product at 40C
Major product at -80C
=>
Chaper 15 17
Allylic Radicals
• Stabilized by resonance.
• Radical stabilities: 1 < 2 < 3 < 1 allylic.
• Substitution at the allylic position competes with addition to double bond.
• To encourage substitution, use a low concentration of reagent with light, heat, or peroxides to initiate free radical formation. =>
Chaper 15 18
Allylic Bromination
BrH
HHH
H
H
H
H
H
H
+ HBr
Br Br Br Br
H
HBrH
H
H
H
Br+ Br
=>
Br2hBr2
Chaper 15 19
Bromination Using NBS• N-Bromosuccinimide (NBS) provides a
low, constant concentration of Br2.
• NBS reacts with the HBr by-product to produce Br2 and prevent HBr addition.
=>
N Br
O
O
+ HBr N H
O
O
+ Br2
Chaper 15 20
MO’s for the Allylic System
=>
Chaper 15 21
SN2 Reactions of Allylic Halides and Tosylates
=>
Chaper 15 22
Diels-Alder Reaction• Otto Diels, Kurt Alder; Nobel prize, 1950
• Produces cyclohexene ring
• Diene + alkene or alkyne with electron-withdrawing group (dienophile)
C
C
H H
H W
C
C
H
H
W
H
=>
Chaper 15 23
Examples of Diels-Alder Reactions
=>
+
OC
OCH3
C
C
CO OCH3
CC
O
OCH3
COCH3
OC
H3C
H3C
NC
CH
CHH
+
H3C
H3C
C
C
H
C N
H
H
diene dienophile Diels-Alder adduct
Chaper 15 24
Stereochemical Requirements
• Diene must be in s-cis conformation.• Diene’s C1 and C4 p orbitals must
overlap with dienophile’s p orbitals to form new sigma bonds.
• Both sigma bonds are on same face of the diene: syn stereochemistry.
=>
Chaper 15 25
Concerted Mechanism
=>
Chaper 15 26
Endo RuleThe p orbitals of the electron-withdrawing
groups on the dienophile have a secondary overlap with the p orbitals of C2 and C3 in the diene.
=>
Chaper 15 27
RegiospecificityThe 6-membered ring product of the
Diels-Alder reaction will have electron-donating and electron-withdrawing groups 1,2 or 1,4 but not 1,3.
D
C
C
H W
H H
W
D
D C
C
H W
H H D
W
WD
not
=>
Chaper 15 28
Symmetry-Allowed Reaction
• Diene contributes electrons from its highest energy occupied orbital (HOMO).
• Dienophile receives electrons in its lowest energy unoccupied orbital (LUMO).
=>
Chaper 15 29
“Forbidden” Cycloaddition
[2 + 2] cycloaddition of two ethylenes to form cyclobutene has anti-bonding overlap of HOMO and LUMO
=>
Chaper 15 30
Photochemical Induction
Absorption of correct energy photon will promote an electron to an energy level that was previously unoccupied.
=>
Chaper 15 31
[2 + 2] Cycloaddition
Photochemically allowed, but thermally forbidden.
=>
Chaper 15 32
Ultraviolet Spectroscopy
• 200-400 nm photons excite electrons from a bonding orbital to a * antibonding orbital.
• Conjugated dienes have MO’s that are closer in energy.
• A compound that has a longer chain of conjugated double bonds absorbs light at a longer wavelength. =>
Chaper 15 33
=>
* for ethylene
and butadiene
Chaper 15 34
Obtaining a UV Spectrum
• The spectrometer measures the intensity of a reference beam through solvent only (Ir) and the intensity of a beam through a solution of the sample (Is).
• Absorbance is the log of the ratio
• Graph is absorbance vs. wavelength. =>
II
s
r
Chaper 15 35
The UV Spectrum• Usually shows broad peaks.
• Read max from the graph.
• Absorbance, A, follows Beer’s Law: A = cl where is the molar absorptivity, c is the sample concentration in moles per liter, and l is the length of the light path in centimeters.
Chaper 15 36
UV Spectrum of Isoprene
=>
Chaper 15 37
Sample UV Absorptions
=>
Chaper 15 38
Woodward-Fieser Rules
=>
Chaper 15 39
End of Chapter 15
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