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Chapter 11: Radical Reactions 11.1 Radicals – species that contain unpaired electrons
double-headed arrow single-headed
arrow
The movement of a single electron is denoted by a curved single headed arrow (fishhook or hook) – radical reactions.
The movement of an electron pair is denoted by a curved double headed arrow – polar reactions.
Polar reac)on Radical Reac)ons A B
heterolyticA:– + B+ A B A• + B•
homolytic
Structure and geometry of radicals
carbocation – sp2 carboanion – sp3
+
–
radical – sp2 229
R3C-H R3C• + H • BDE
ΔH° H
C
H
HH
H
C
H
HH3C
H3C
C
H
HH3C
H3C
C
H3C
HH3C
H
C
H
HCCH
H
H
H
C
H
H
ΔH° = 435 KJ/mol
410
397
381
ΔH° = 364 KJ/mol
356
The bond dissociation energies (BDEs) reflect the stabilities of the radical products.
Table 6.1, p. 238
230
115
The stability and structure of alkyl radicals parallels those of carbocations:
231
11.2 Common Patterns in Radical Mechanisms
Homolytic cleavage – Coupling (radical combination) Addition to a π-bond – Elimination (β-scission)
232
116
Hydrogen atom abstraction (transfer) Halogen atom abstraction (transfer) Mechanism of free radical reactions have three distinct steps:
1. Initiation (Homolytic cleavage)
2. Propagation (Addition to a π-bond, Elimination, Hydrogen atom abstraction, Halogen abstraction)
3. Termination (Coupling) 233
11.3 Chlorination of Methane Free-radical chain mechanism:
234
117
H
C
H
HHCl2
H
C
H
ClH
+ HCl
Cl2Cl
C
H
ClH
+ HCl
Cl2Cl
C
H
ClCl
+ HCl
Cl2Cl
C
Cl
ClCl
+ HCl
Free radical chlorination is not very useful for making alkyl chlorides due to polychlorination and non-specific chlorination
C-H BDEs (KJ/mol): 431 423 414 377
Radical initiators
Cl Cl RO OR
O
OR
O
RO
BDEs (KJ/mol): 243 159 121
235
11.4 Thermodynamic Considerations for Halogenation Reactions.
X= F ΔH° (KJ/mol) 435 159 456 569 – 431 KJ/mol
X= Cl 435 243 351 431 – 104
X= Br 435 193 293 368 – 33
X= I 435 151 234 297 + 55
H
C
H
HH X X+
H
C
H
XH + H X
Free radical . . . fluorination is so exothermic that it cannot be controlled.
iodination is endothermic and does not precede.
chlorination and bromination are useful reactions
236
118
The propagation step for free radical bromination is endergonic, as opposed to chlorination which is exergonic.
Cl: ΔH = – 21 KJ/mol Br: = + 42 KJ/mol
R
C
R
HR X+
R
C
R
R + H X• •
According to the Hammond postulate the transition state for bromination should resemble the product radical, and therefore be more selective for the product going through the more stable radical intermediate
237
11.5 Selectivity of Halogenation
Since the transition state for bromination resemble the product radical, the stability of the radical intermediate greatly influences the rate of the reaction. This results in higher selectivity for free radical bromination
CH3
C
CH3
HH3C
H
C
H
CH3H3CX2, hν
X
C
H
CH3H3C
H
C
H
CH2XH3C
X = Cl 60 : 40X = Br 97 : 3
+
X2, hν CH3
C
CH3
XH3C
CH3
C
CH2X
HH3C+
X = Cl 35 : 65X = Br 99 : 1
238
119
Halogenation reactions that create new chiral centers and involving existing chiral centers.
Selectivity (relative reactivity) for free radical . . . chlorination bromination
H
C
H
HR
H
C
R
HR
R
C
R
HR< <
primary (1°)hydrogens
secondary (2°)hydrogens
tertiary (3°)hydrogens
1.0 2.3 4.9
H
C
H
HR
H
C
R
HR
R
C
R
HR< <
primary (1°)hydrogens
secondary (2°)hydrogens
tertiary (3°)hydrogens
1.0 82 890
239
11.7 Allylic Bromination – allylic position is the next to a double bond
C CC H
allylic carbon
allylic hydrogen
NBS, hν
CCl4
Br
Allylic and benzylic bromination of an alkene takes place through a free radical mechanism.
240
120
C CR
H H
H
H–Br C CR
Br
H
HH
H+ C CR
H
H
HH
Br
C CR"
R H
H
H–Br C CR
Br
H
HR"
H+ C CR
H
H
HR"
Br
C CR"
R R'
H
H–Br C CR
Br
R'
HR"
H+ C CR
H
R'
HR"
Br
C CR
H R'
H
H–Br C CR
Br
R'
HH
H+ C CR
H
R'
HH
Br
Polar mechanism
11.10 Radical Addition to HBr: Anti-Markovnikov Addition
none of this
none of this
none of this
Both products observed
C CR
H H
H
H–Br
C CR"
R H
H
H–Br
C CR"
R R'
H
H–Br
C CR
H R'
H
H–Br
RO–OR(peroxides)
RO–OR(peroxides)
RO–OR(peroxides)
RO–OR(peroxides)
Radical mechanism
none of this
none of this
none of this
241
Polar mechanism (Markovnikov addition)
Radical mechanism (Anti-Markovnikov addition)
H3CH2C CC HH
H
H-BrC CBr
HH3CH2C
H
HH C C
H
HH3CH2C
Br
HH+
none of this
H3CH2C CC HH
H
H-BrC CBr
HH3CH2C
H
HH C C
H
HH3CH2C
Br
HH
+
peroxides(RO-OR)
none of this
The regiochemistry of HBr addition is reversed in the presence of peroxides. Peroxides are radical initiators - change in mechanism
242
121
243
11.13 Halogenation as a Synthetic Technique
244
Radical inhibitors (scavengers) – compounds that terminate radical chain reactions.
Phenols and hydroquinones OH OH
OH
phenol hydroquinone
O
O
- 2 H•
quinone
OH
BHT
11.8 Atmospheric Chemistry and the Ozone Layer (please read) 11.12 Radical Processes in the Petrochemical Industry
(please read) 11.11 Radical Polymerization (please read) 11.9 Autooxidation and Antioxidants (please read)
122
245
Oxidative Stress- a free radical chain process
Cellular respiration
O2•_ + Fe (III)
HO• + HO _ + Fe(III)
Fe (II) + O2
Fe (II) + H2O2
O2•_ + •NO ONO2
_
nitricoxide peroxynitrate
H+
ONO2H
peroxynitrousacid
NO2• + HO•
Reactive Oxygen Species (ROS)
O2
4 e ,4H+
2 H2O
•_
O2•_
Superoxide:one-electron reduction of O2
HO•
hydroxylradical
H2O2
hydrogen peroxide
The Oxygen Paradox: oxygen is necessary for cellular metabolism; however, oxygen is transformed into highly reactive species that can damage biomolecules.
246
OH
O
Linoleic Acid (unsaturated fatty acid)H-atom abstractionala the free radicalchlorination of methane
HO•
OH
O
•
OH
OO O • linoleic acid
Propagation OH
OO OH
+ linoleate radical
anti-oxidants(vitamin e)
Termination
Degrada)on (lipid peroxida)on)
Linked to DNA damage, protein damage, diabetes, neurodegenerative disease, cardiovascular disease
O
HO
Vitamin Eα-tocopherol
OO
OHHO
OH
OH
H
Vitamin C
123
247
Chapter 12: Synthesis
12.1 One-Step Syntheses
12.1 Identify the reagents necessary to accomplish each pf the transformations shown below. (Chapter 9)
248
12.2 Identify the reagents necessary to accomplish each pf the transformations shown below. (Chapter 10)
124