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In organic chemistry, free-radical addition is an addition reaction which involves free radicals. These reactions can happen due to the free radicals having an unpaired electron in their valence shell, making them highly reactive. <ref>{{#invoke:citation/CS1|citation |CitationClass=web }}</ref> Radical additions are known for a variety of unsaturated substrates, both olefinic or aromatic and with or without heteroatoms.
Free-radical reactions depend on one or more relatively weak bonds in a reagent. Under reaction conditions (typically heat or light), some weak bonds homolyse into radicals, which then induce further decomposition in their compatriots before recombination. Different mechanisms typically apply to reagents without such a weak bond.
Mechanism and regiochemistryEdit
The basic steps in any free-radical process (the radical chain mechanism) divide into:<ref name=Wade />
- Radical initiation: A radical is created from a non-radical precursor.
- Chain propagation: A radical reacts with a non-radical to produce a new radical species
- Chain termination: Two radicals react with each other to create a non-radical species
In a free-radical addition, there are two chain propagation steps. In one, the adding radical attaches to a multiply-bonded precursor to give a radical with lesser bond order. In the other, the newly-formed radical product abstracts another substituent from the adding reagent to regenerate the adding radical.<ref name="March" />Template:Rp
In general, the adding radical attacks the alkene at the most sterically accessible (typically, least substituted) carbon; the radical then stabilizes on the more substituted carbon.<ref name="March" />Template:Rp The result is typically anti-Markovnikov addition, a phenomenon Morris Kharasch called the "peroxide effect".<ref name="Kharasch" /> Reaction is slower with alkynes than alkenes.<ref name="March" />Template:Rp
In the paradigmatic example, hydrogen bromide radicalyzes to monatomic bromine. These bromine atoms add to an alkene at the most accessible site, to give a bromoalkyl radical, with the radical on the more substituted carbon. That radical then abstracts a hydrogen atom from another HBr molecule to regenerate the monatomic bromine and continue the reaction.<ref name="March" />Template:Rp
Compounds that add radicallyEdit
Template:See also Radical addition of hydrogen bromide is a valuable synthetic technique for anti-Markovnikov carbon substitution,Template:Citation needed but free-radical addition does not occur with the other hydrohalic acids. Radical formation from HF, HCl, or HI is extremely endothermic and chemically disfavored.<ref name="March" />Template:Rp Hydrogen bromide is incredibly selective as a reagent,<ref name="March" />Template:Rp and does not produce detectable quantities of polymeric byproducts.<ref name="OrgRxn" />Template:Rp
The behavior of hydrogen bromide generalizes in two separate directions. Halogenated compounds with a relatively stable radical can dissociate from the halogen. Thus, for example, sulfonyl, sulfenyl, and other sulfur halides can add radically to give respectively βTemplate:Nbhhalo sulfones, sulfoxides, or sulfides.<ref name="OrgRxn" />Template:Rp
Separately, unsubsituted compounds with a relative stable radical can dissociate from hydrogen. In general, these reactions risk polymerized byproducts (see Template:Slink). For example, in the thiol-ene reaction, thiols,<ref name="OrgRxn" />Template:Rp disulfides,<ref name="OrgRxn" />Template:Rp and hydrogen sulfide<ref name="OrgRxn" />Template:Rp add across a double bond. But if the unsaturated substrate polymerizes easily, they catalyze polymerization instead.<ref name="OrgRxn" />Template:Rp In thermal silane additions, telomerization usually proceeds to about 6 units.<ref name="OrgRxn" />Template:Rp
In the case of silicon, germanium, or phosphorus, the energetics are unfavorable unless the heavy atom bears a pendant hydrogen.<ref name="OrgRxn" />Template:Rp Other electronegative substituents on silicon appear to reduce the barrier.<ref name="OrgRxn" />Template:Rp
Although nitrogen oxides naturally radicalize, careful control of the radical species is difficult. Dinitrogen tetroxide adds to give a mixture: a vicinal dinitro compound, but also a nitro substituent adjacent to a nitrite ester.<ref name="OrgRxn" />Template:Rp
To aryl radicalsEdit
Template:See also Although aromatic resonance stabilizes aryl radicals, bonds between arenes and their substituents are (in)famously strong. Radical reactions with arenes typically present retrosynthetically as instances of nucleophilic aromatic substitution,Template:Citation needed because generating the aryl radical requires a strong (radical) leaving group.<ref name="March" />Template:Rp One example is the Meerwein arylation.
Side reactionsEdit
A radical addition which leaves an unsaturated product can undergo radical cyclization between the two propagation steps.<ref name="March" />Template:Rp In general, radical additions can also start radical polymerization processes.<ref name="OrgRxn" />Template:Rp
With stable inorganic radicalsEdit
In self-terminating oxidative radical cyclization, inorganic radicals oxidize alkynes to ketones through an intramolecular radical cyclization. This reaction is not catalytic, and requires the oxidized radical source in stoichiometric amounts. In effect, the radical species is synthetically equivalent to monatomic oxygen.<ref name="SelfTerm" />
In the paradigmatic example, a nitrate radical (from photolysis of ceric ammonium nitrate) adds to an alkyne to generate a very reactive vinyl nitrate ester radical. The vinyl radical abstracts an intramolecular hydrogen atom 5 atoms away before 5-exo-trig ring-closure. The resulting alkyl nitrate radical can then fragment to a ketone and the stable radical nitrogen dioxide.<ref name="SelfTerm" />
Sulfate (from ammonium persulfate) and hydroxyl radicals show similar reactivity.<ref name="SelfTerm" />
See alsoEdit
The other radical reactions:
ReferencesEdit
<references> <ref name=SelfTerm>Dreessen, Tim; Jargstorff, Christian; Lietzau, Lars; Plath, Christian; Stademann, Arne; and Wille, Uta (2004). "Self-Terminating, Oxidative Radical Cyclizations". Molecules, issue 9, pp. 480–497.</ref> <ref name=Kharasch>Template:Cite journal</ref> <ref name=March>Template:March4th</ref> <ref name=OrgRxn>Template:Cite book</ref> <ref name=Wade>L.G. Wade's Organic Chemistry 5th Ed. (p 319) – Mechanism supplements original.</ref> </references>