# β

The hydroxyl radical, Lewis structure shown, contains one unpaired electron

In chemistry, a radical (more precisely, a free radical) is an atom, molecule, or ion that has an unpaired valence electron.[1][2] With some exceptions, these unpaired electrons make free radicals highly chemically reactive. Many free radicals spontaneously dimerize. Most organic radicals have short lifetimes.

A notable example of a free radical is the hydroxyl radical (HO•), a molecule that has one unpaired electron on the oxygen atom. Two other examples are triplet oxygen and triplet carbene (:CH
2
) which have two unpaired electrons.

Free radicals may be generated in a number of ways, but typical methods involve redox reactions. Ionizing radiation, heat, electrical discharges, electrolysis, are known to produce radicals. Radicals are intermediates in many chemical reactions, more so than is apparent from the balanced equations.

Free radicals are important in combustion, atmospheric chemistry, polymerization, plasma chemistry, biochemistry, and many other chemical processes. A large fraction of natural products are generated by radical-generating enzymes. In living organisms, the free radicals superoxide and nitric oxide and their reaction products regulate many processes, such as control of vascular tone and thus blood pressure. They also play a key role in the intermediary metabolism of various biological compounds. Such radicals can even be messengers in a process dubbed redox signaling. A radical may be trapped within a solvent cage or be otherwise bound.

## Depiction in chemical reactionsEdit

In chemical equations, free radicals are frequently denoted by a dot placed immediately to the right of the atomic symbol or molecular formula as follows:

${\displaystyle \mathrm {Cl} _{2}\;{\xrightarrow {UV}}\;{\mathrm {Cl} \cdot }+{\mathrm {Cl} \cdot }}$
Chlorine gas can be broken down by ultraviolet light to form atomic chlorine radicals.

Radical reaction mechanisms use single-headed arrows to depict the movement of single electrons:

The homolytic cleavage of the breaking bond is drawn with a 'fish-hook' arrow to distinguish from the usual movement of two electrons depicted by a standard curly arrow. The second electron of the breaking bond also moves to pair up with the attacking radical electron; this is not explicitly indicated in this case.

Free radicals also take part in radical addition and radical substitution as reactive intermediates. Chain reactions involving free radicals can usually be divided into three distinct processes. These are initiation, propagation, and termination.

• Initiation reactions are those that result in a net increase in the number of free radicals. They may involve the formation of free radicals from stable species as in Reaction 1 above or they may involve reactions of free radicals with stable species to form more free radicals.
• Propagation reactions are those reactions involving free radicals in which the total number of free radicals remains the same.
• Termination reactions are those reactions resulting in a net decrease in the number of free radicals. Typically two free radicals combine to form a more stable species, for example: 2Cl·→ Cl2

## FormationEdit

The formation of radicals may involve the breaking of covalent bonds by homolysis, a process that requires significant amounts of energy. Such energies are known as homolytic bond dissociation energies, usually abbreviated as "ΔH °". Splitting H2 into 2H•, for example, requires a ΔH ° of +435 kJ·mol-1, while splitting Cl2 into 2Cl• requires a ΔH ° of +243 kJ·mol-1.

The energy needed to break a specific bond (generally covalent) between two atoms known as bond energy is a result of all the relative attractions and repulsions between the atoms of the molecule, however the most relevant are the bond's atoms and the immediate neighbors. As an approximation the most important parameters that influence the bonding between two atoms in a molecule are the mutual energy match and overlap of covalent orbitals and the repulsion between nonbonding orbitals. Likewise, radicals requiring more energy to form are less stable than those requiring less energy. An additional barrier can be the selection rule. Propagation, however, is very exothermic.

Radical formation through homolytic bond cleavage most often happens between two atoms of similar electronegativity; in organic chemistry, this is often between the O–O bond in peroxide species or between O–N bonds. Radicals may also be formed by single-electron oxidation or reduction of an atom or molecule: an example is the production of superoxide by the electron transport chain. Early studies in organometallic chemistry – especially F. A. Paneth and K. Hahnfeld's studies of tetra-alkyl lead species during the 1930s – supported the heterolytic fission of bonds and a radical-based mechanism. Although radical ions do exist, most species are electrically neutral.

## Persistence and stabilityEdit

Although radicals are generally short-lived due to their reactivity, there are long-lived radicals. These are categorized as follows:

The prime example of a stable radical is molecular dioxygen (O2). Another common example is nitric oxide (NO). Organic radicals can be long lived if they occur in a conjugated π system, such as the radical derived from α-tocopherol (vitamin E). There are also hundreds of examples of thiazyl radicals, which show low reactivity and remarkable thermodynamic stability with only a very limited extent of π resonance stabilization.[3][4]

Persistent radical compounds are those whose longevity is due to steric crowding around the radical center, which makes it physically difficult for the radical to react with another molecule.[5] Examples of these include Gomberg's triphenylmethyl radical, Fremy's salt (Potassium nitrosodisulfonate, (KSO3)2NO·), aminoxyls, (general formula R2NO·) such as TEMPO, TEMPOL, nitronyl nitroxides, and azephenylenyls and radicals derived from PTM (perchlorophenylmethyl radical) and TTM (tris(2,4,6-trichlorophenyl)methyl radical). Persistent radicals are generated in great quantity during combustion, and "may be responsible for the oxidative stress resulting in cardiopulmonary disease and probably cancer that has been attributed to exposure to airborne fine particles."[6]

Diradicals are molecules containing two radical centers. Multiple radical centers can exist in a molecule. Atmospheric oxygen naturally exists as a diradical in its ground state as triplet oxygen. The low reactivity of atmospheric oxygen is due to its diradical state. Non-radical states of dioxygen are actually less stable than the diradical. The relative stability of the oxygen diradical is primarily due to the spin-forbidden nature of the triplet-singlet transition required for it to grab electrons, i.e., "oxidize". The diradical state of oxygen also results in its paramagnetic character, which is demonstrated by its attraction to an external magnet.[7] Diradicals can also occur in metal-oxo complexes, lending themselves for studies of spin forbidden reactions in transition metal chemistry.[8]

## ReactivityEdit

Radical alkyl intermediates are stabilized by similar physical processes to carbocations: as a general rule, the more substituted the radical center is, the more stable it is. This directs their reactions. Thus, formation of a tertiary radical (R3C·) is favored over secondary (R2HC·), which is favored over primary (RH2C·). Likewise, radicals next to functional groups such as carbonyl, nitrile, and ether are more stable than tertiary alkyl radicals.

Radicals attack double bonds. However, unlike similar ions, such radical reactions are not as much directed by electrostatic interactions. For example, the reactivity of nucleophilic ions with α,β-unsaturated compounds (C=C–C=O) is directed by the electron-withdrawing effect of the oxygen, resulting in a partial positive charge on the carbonyl carbon. There are two reactions that are observed in the ionic case: the carbonyl is attacked in a direct addition to carbonyl, or the vinyl is attacked in conjugate addition, and in either case, the charge on the nucleophile is taken by the oxygen. Radicals add rapidly to the double bond, and the resulting α-radical carbonyl is relatively stable; it can couple with another molecule or be oxidized. Nonetheless, the electrophilic/neutrophilic character of radicals has been shown in a variety of instances. One example is the alternating tendency of the copolymerization of maleic anhydride (electrophilic) and styrene (slightly nucleophilic).

In intramolecular reactions, precise control can be achieved despite the extreme reactivity of radicals. In general, radicals attack the closest reactive site the most readily. Therefore, when there is a choice, a preference for five-membered rings is observed: four-membered rings are too strained, and collisions with carbons six or more atoms away in the chain are infrequent.

Triplet carbenes and nitrenes, which are diradicals, have distinctive chemistry.

## CombustionEdit

Spectrum of the blue flame from a butane torch showing excited molecular radical band emission and Swan bands

A familiar free-radical reaction is combustion. The oxygen molecule is a stable diradical, best represented by ·O-O·. Because spins of the electrons are parallel, this molecule is stable. While the ground state of oxygen is this unreactive spin-unpaired (triplet) diradical, an extremely reactive spin-paired (singlet) state is available. For combustion to occur, the energy barrier between these must be overcome. This barrier can be overcome by heat, requiring high temperatures. The triplet-singlet transition is also "forbidden". This presents an additional barrier to the reaction. It also means molecular oxygen is relatively unreactive at room temperature except in the presence of a catalytic heavy atom such as iron or copper.

Combustion consists of various radical chain reactions that the singlet radical can initiate. The flammability of a given material strongly depends on the concentration of free radicals that must be obtained before initiation and propagation reactions dominate leading to combustion of the material. Once the combustible material has been consumed, termination reactions again dominate and the flame dies out. As indicated, promotion of propagation or termination reactions alters flammability. For example, because lead itself deactivates free radicals in the gasoline-air mixture, tetraethyl lead was once commonly added to gasoline. This prevents the combustion from initiating in an uncontrolled manner or in unburnt residues (engine knocking) or premature ignition (preignition).

When a hydrocarbon is burned, a large number of different oxygen radicals are involved. Initially, hydroperoxyl radical (HOO·) are formed. These then react further to give organic hydroperoxides that break up into hydroxyl radicals (HO·).

## PolymerizationEdit

In addition to combustion, many polymerization reactions involve free radicals. As a result, many plastics, enamels, and other polymers are formed through radical polymerization. For instance, drying oils and alkyd paints harden due to radical crosslinking by oxygen from the atmosphere.

• Reversible addition-fragmentation chain transfer (RAFT)
• Atom transfer radical polymerization (ATRP)
• Nitroxide mediated polymerization (NMP)

These methods produce polymers with a much narrower distribution of molecular weights.

The most common radical in the lower atmosphere is molecular dioxygen. Photodissociation of source molecules produces other free radicals. In the lower atmosphere, important free radical are produced by the photodissociation of nitrogen dioxide to an oxygen atom and nitric oxide (see eq. 1. 1 below), which plays a key role in smog formation—and the photodissociation of ozone to give the excited oxygen atom O(1D) (see eq. 1. 2 below). The net and return reactions are also shown (eq. 1. 3 and eq. 1. 4, respectively).

${\displaystyle {\ce {{NO2}->[h \nu] {NO}+ {O}}}}$

(eq. 1. 1)

${\displaystyle {\ce {{O}+ {O2}-> {O3}}}}$

(eq. 1. 2)

${\displaystyle {\ce {{NO2}+ {O2}->[h \nu] {NO}+ {O3}}}}$

(eq. 1. 3)

${\displaystyle {\ce {{NO}+ {O3}-> {NO2}+ {O2}}}}$

(eq. 1. 4)

In the upper atmosphere, the photodissociation of normally unreactive chlorofluorocarbons (CFCs) by solar ultraviolet radiation is an important source of radicals (see eq. 1 below). These reactions give the chlorine radical, Cl•, which catalyzes the conversion ofozone to O2, i.e., Ozone depletion (eq. 2. 2eq. 2. 4 below).

${\displaystyle {\ce {{CFCS}->[h \nu] {Cl.}}}}$

(eq. 2. 1)

${\displaystyle {\ce {{Cl.}+ {O3}-> {ClO.}+ {O2}}}}$

(eq. 2. 2)

${\displaystyle {\ce {{O3}->[h \nu] {O}+ {O2}}}}$

(eq. 2. 3)

${\displaystyle {\ce {{O}+ {ClO.}-> {Cl.}+ {O2}}}}$

(eq. 2. 4)

${\displaystyle {\ce {{2O3}->[h \nu] 3O2}}}$

(eq. 2. 5)

Such reactions cause of depletion of the ozone layer. Consequently, the use of chlorofluorocarbons as refrigerants has been restricted.

## In biologyEdit

Free radicals play important roles in biology. Many of these are necessary for life, such as the intracellular killing of bacteria by phagocytic cells such as granulocytes and macrophages. Free radicals are involved in cell signalling processes,[9] known as redox signaling. For example, free radical attack of linoleic acid produces a series of 13-Hydroxyoctadecadienoic acids and 9-Hydroxyoctadecadienoic acids, which may act to regulate localized tissue inflammatory and/or healing responses, pain perception, and the proliferation of malignant cells. Free radical attacks on arachidonic acid and docosahexaenoic acid produce a similar but broader array of signaling products.[10]

Free radicals may also be involved in Parkinson's disease, senile and drug-induced deafness, schizophrenia, and Alzheimer's.[12] The classic free-radical syndrome, the iron-storage disease hemochromatosis, is typically associated with a constellation of free-radical-related symptoms including movement disorder, psychosis, skin pigmentary melanin abnormalities, deafness, arthritis, and diabetes mellitus. The free-radical theory of aging proposes that free radicals underlie the aging process itself. Similarly, the process of mitohormesis suggests that repeated exposure to free radicals may extend life span.

Because free radicals are necessary for life, the body has a number of mechanisms to minimize free-radical-induced damage and to repair damage that occurs, such as the enzymes superoxide dismutase, catalase, glutathione peroxidase and glutathione reductase. In addition, antioxidants play a key role in these defense mechanisms. These are often the three vitamins, vitamin A, vitamin C and vitamin E and polyphenol antioxidants. Furthermore, there is good evidence indicating that bilirubin and uric acid can act as antioxidants to help neutralize certain free radicals. Bilirubin comes from the breakdown of red blood cells' contents, while uric acid is a breakdown product of purines. Too much bilirubin, though, can lead to jaundice, which could eventually damage the central nervous system, while too much uric acid causes gout.[13]

### Reactive oxygen speciesEdit

An explanation of cellular injury caused by reactive oxygen species.

Oxybenzone has been found to form free radicals in sunlight, and therefore may be associated with cell damage as well. This only occurred when it was combined with other ingredients commonly found in sunscreens, like titanium oxide and octyl methoxycinnamate.[17]

ROS attack the polyunsaturated fatty acid, linoleic acid, to form a series of 13-Hydroxyoctadecadienoic acid and 9-Hydroxyoctadecadienoic acid products that serve as signaling molecules that may trigger responses that counter the tissue injury which caused their formation. ROS attacks other polyunsaturated fatty acids, e.g. arachidonic acid and docosahexaenoic acid, to produce a similar series of signaling products.[18]

## History and nomenclatureEdit

Moses Gomberg (1866–1947), the founder of radical chemistry

Until late in the 20th century the word "radical" was used in chemistry to indicate any connected group of atoms, such as a methyl group or a carboxyl, whether it was part of a larger molecule or a molecule on its own. The qualifier "free" was then needed to specify the unbound case. Following recent nomenclature revisions, a part of a larger molecule is now called a functional group or substituent, and "radical" now implies "free". However, the old nomenclature may still appear in some books.

In a modern context the first organic (carbon–containing) free radical identified was triphenylmethyl radical, (C6H5)3C•. This species was discovered by Moses Gomberg in 1900. In 1933 Morris Kharash and Frank Mayo proposed that free radicals were responsible for anti-Markovnikov addition of hydrogen bromide to allyl bromide.[19][20]

In most fields of chemistry, the historical definition of radicals contends that the molecules have nonzero electron spin. However, in fields including spectroscopy, chemical reaction, and astrochemistry, the definition is slightly different. Gerhard Herzberg, who won the Nobel prize for his research into the electron structure and geometry of radicals, suggested a looser definition of free radicals: "any transient (chemically unstable) species (atom, molecule, or ion)".[21] The main point of his suggestion is that there are many chemically unstable molecules that have zero spin, such as C2, C3, CH2 and so on. This definition is more convenient for discussions of transient chemical processes and astrochemistry; therefore researchers in these fields prefer to use this loose definition.[22]

## DiagnosticsEdit

Radicals typically exhibit paramagnetism, but the bulk magnetic properties of a ion or molecule are often not conveniently measured. Electron spin resonance is instead the definitive and most widely used technique for characterizing free radicals. The nature of the atom bearing the unpaired electron and its neighboring atoms can often be deduced by the EPR spectrum.[23]

The presence of free radicals can also be detected or inferred by chemical reagents that trap (i.e. combine with) radicals. Often these traps are themselves radicals, such as TEMPO.

## ReferencesEdit

2. ^ Hayyan, M.; Hashim, M.A.; AlNashef, I.M. (2016). "Superoxide Ion: Generation and Chemical Implications". Chem. Rev. 116 (5): 3029–3085. doi:10.1021/acs.chemrev.5b00407.
3. ^ Oakley, Richard T. (1988). "Progress in Inorganic Chemistry" (PDF). Cyclic and Heterocyclic Thiazenes (section). Progress in Inorganic Chemistry. 36: 299–391. doi:10.1002/9780470166376.ch4. ISBN 978-0-470-16637-6.
4. ^ Rawson, J; Banister, A; Lavender, I (1995). "Advances in Heterocyclic Chemistry". The Chemistry of Dithiadiazolylium and Dithiadiazolyl Rings (section) =. Advances in Heterocyclic Chemistry. 62: 137–247. doi:10.1016/S0065-2725(08)60422-5. ISBN 978-0-12-020762-6.
5. ^ Griller, David; Ingold, Keith U. (1976). "Persistent carbon-centered radicals". Accounts of Chemical Research. 9: 13–19. doi:10.1021/ar50097a003.
6. ^ Lomnicki S.; Truong H.; Vejerano E.; Dellinger B. (2008). "Copper oxide-based model of persistent free radical formation on combustion-derived particulate matter". Environ. Sci. Technol. 42 (13): 4982–4988. Bibcode:2008EnST...42.4982L. doi:10.1021/es071708h. PMID 18678037.
7. ^ However, paramagnetism does not necessarily imply radical character.
8. ^ Svensson, Mats (1999). "Timing is Critical: Effect of Spin Changes on the Diastereoselectivity in Mn(Salen)-Catalyzed Epoxidation". Journal of the American Chemical Society. 121: 5083–4. doi:10.1021/ja9809915.
9. ^ Pacher P, Beckman JS, Liaudet L (2007). "Nitric oxide and peroxynitrite in health and disease". Physiol. Rev. 87 (1): 315–424. doi:10.1152/physrev.00029.2006. PMC . PMID 17237348.
10. ^ "Lipid peroxidation: pathophysiological and pharmacological implications in the eye". Frontiers in Physiology. 4. doi:10.3389/fphys.2013.00366.
11. ^ Broderick, J. B.; Duffus, B. R.; Duschene, K. S.; Shepard, E. M., (2014). "Radical S-Adenosylmethionine Enzymes". Chemical Reviews. 114: 4229–4317. doi:10.1021/cr4004709.
12. ^ Floyd, R. A. (1999). "Neuroinflammatory processes are important in neurodegenerative diseases: An hypothesis to explain the increased formation of reactive oxygen and nitrogen species as major factors involved in neurodegenerative disease development". Free Radical Biology and Medicine. 26 (9–10): 1346–1355. doi:10.1016/s0891-5849(98)00293-7.
13. ^ An overview of the role of free radicals in biology and of the use of electron spin resonance in their detection may be found in Rhodes C.J. (2000). Toxicology of the Human Environment – the critical role of free radicals. London: Taylor and Francis. ISBN 0-7484-0916-5.
14. ^ Rajamani Karthikeyan; Manivasagam T; Anantharaman P; Balasubramanian T; Somasundaram ST (2011). "Chemopreventive effect of Padina boergesenii extracts on ferric nitrilotriacetate (Fe-NTA)-induced oxidative damage in Wistar rats". J. Appl. Phycol. 23, Issue 2, Page 257 (2): 257–263. doi:10.1007/s10811-010-9564-0.
15. ^ Mukherjee, P. K.; Marcheselli, V. L.; Serhan, C. N.; Bazan, N. G. (2004). "Neuroprotecin D1: A docosahexanoic acid-derived docosatriene protects human retinal pigment epithelial cells from oxidative stress". Proceedings of the National Academy of Sciences of the USA. 101 (22): 8491–8496. Bibcode:2004PNAS..101.8491M. doi:10.1073/pnas.0402531101. PMC . PMID 15152078.
16. ^ Lyons, MA; Brown, AJ (1999). "7-Ketocholesterol". Int. J. Biochem. Cell Biol. 31: 369–75. doi:10.1016/s1357-2725(98)00123-x. PMID 10224662.
17. ^ Serpone, N; Salinaro, A; Emeline, AV; Horikoshi, S; Hidaka, H; Zhao, JC (2002). "An in vitro systematic spectroscopic examination of the photostabilities of a random set of commercial sunscreen lotions and their chemical UVB/UVA active agents". Photochemical & Photobiological Sciences. 1 (12): 970–981. doi:10.1039/b206338g.
18. ^ "Lipid peroxidation: pathophysiological and pharmacological implications in the eye". Frontiers in Physiology. 4. doi:10.3389/fphys.2013.00366.
19. ^ The Peroxide Effect in the Addition of Reagents to Unsaturated Compounds. I. The Addition of Hydrogen Bromide to Allyl Bromide M. S. Kharasch, Frank R. Mayo J. Am. Chem. Soc., 1933, 55, pp 2468–2496 doi:10.1021/ja01333a041
20. ^ Radicals: Reactive Intermediates with Translational Potential Ming Yan, Julian C. Lo, Jacob T. Edwards, and Phil S. Baran J. Am. Chem. Soc., 2016, 138 (39), pp 12692–12714 doi:10.1021/jacs.6b08856
21. ^ G. Herzberg (1971), "The spectra and structures of simple free radicals", ISBN 0-486-65821-X.
22. ^ 28th International Symposium on Free Radicals Archived 2007-07-16 at the Wayback Machine..
23. ^ Chechik, Victor; Carter, Emma; Murphy, Damien (2016). Electron Paramagnetic Resonance. Oxford University Press. ISBN 978-0-19-872760-6.