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

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

A notable example of a 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.

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

Radicals are important in combustion, atmospheric chemistry, polymerization, plasma chemistry, biochemistry, and many other chemical processes. A majority of natural products are generated by radical-generating enzymes. In living organisms, the 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.

## Stability and formation

Although organic radicals are generally transient, some are quite long-lived. Generally organic radicals are stabilized by any or all of these factors: presence of electron-donating groups, delocalization, and steric protection.[3] The compound 2,2,6,6-tetramethylpiperidinyloxyl illustrates the combination of all three factors. It is a commercially available solid that, aside from being magnetic, behaves like a normal organic compound.

#### Facile H-atom donors

The stability of many (or most) organic radicals is not indicated by their isolability but is manifested in their ability to function as donors of H.. This property reflects a weakened bond to hydrogen, usually O-H but sometimes N-H or C-H. This behavior is important because these H. donors serve as antioxidants in biology and in commerce. Illustrative is α-tocopherol (vitamin E). The tocopherol radical itself is insufficiently stable for isolation, but the parent molecule is a highly effective H-atom donor. The C-H bond is weakened in triphenylmethyl (trityl) derivatives.

2,2,6,6-Tetramethylpiperidinyloxyl is an example of a robust organic radical.

The inorganic compound nitric oxide (NO) is a stable radical. Fremy's salt (Potassium nitrosodisulfonate, (KSO3)2NO) is a related example. There are also hundreds of examples of thiazyl radicals, despite limited extent of π resonance stabilization.[4][5]

Radicals form by breaking of covalent bonds by homolysis. The homolytic bond dissociation energies, usually abbreviated as "ΔH °" are a measure of bond strength. Splitting H2 into 2H•, for example, requires a ΔH ° of +435 kJ·mol-1, while splitting Cl2 into two Cl• requires a ΔH ° of +243 kJ·mol-1. For weak bonds, homolysis can be induced thermally. Strong bonds require high energy photons or even flames to induce homolysis.

Diradicals are molecules containing two radical centers. Dioxygen (O2) is the premier example of a stable diradical. Singlet oxygen, the lowest-energy non-radical state of dioxygen, is less stable than the diradical due to Hund's rule of maximum multiplicity. 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.[6] Diradicals can also occur in metal-oxo complexes, lending themselves for studies of spin forbidden reactions in transition metal chemistry.[7] Carbenes in their triplet state can be viewed as diradicals centred on the same atom, while these are usually highly reactive persistent carbenes are known, with N-heterocyclic carbenes being the most common example.

Triplet carbenes and nitrenes are diradicals. Their chemical properties are distinct from the properties of their singlet analogues.

### Combustion

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

A familiar 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 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 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·).

### Polymerization

Many polymerization reactions are initiated by radicals. Polymerization involves an initial radical adding to non-radical (usually an alkene) to give new radicals. This process is the basis of the radical chain reaction. The art of polymerization entails the method by which the initiating radical is introduced. For example, methyl methacrylate (MMA) can be polymerized to produce Poly(methyl methacrylate) (PMMA - Plexiglas or Perspex) via a repeating series of radical addition steps:

Radical intermediates in the formation of polymethacrylate (plexiglas or perspex).

Being a prevalent radical, O2 reacts with many organic compounds to generate radicals together with the hydroperoxide radical. Drying oils and alkyd paints harden due to radical crosslinking initiated by oxygen from the atmosphere.

The most common radical in the lower atmosphere is molecular dioxygen. Photodissociation of source molecules produces other radicals. In the lower atmosphere, important 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 of ozone to O2, thus facilitating 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 the depletion of the ozone layer, especially since the chlorine radical is free to engage in another reaction chain; consequently, the use of chlorofluorocarbons as refrigerants has been restricted.

### In biology

An approximate structure of lignin, which constitutes about 30% of plant matter. It is formed by radical reactions.

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. Radicals are involved in cell signalling processes,[9] known as redox signaling. For example, 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. Radical attacks on arachidonic acid and docosahexaenoic acid produce a similar but broader array of signaling products.[10]

Radicals may also be involved in Parkinson's disease, senile and drug-induced deafness, schizophrenia, and Alzheimer's.[11] 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 radicals underlie the aging process itself. Similarly, the process of mitohormesis suggests that repeated exposure to radicals may extend life span.

Because radicals are necessary for life, the body has a number of mechanisms to minimize 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 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.[12]

### Reactive oxygen species

Oxybenzone has been found to form 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.[16]

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.[17]

## History and nomenclature

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) radical identified was triphenylmethyl radical, (C6H5)3C•. This species was discovered by Moses Gomberg in 1900. In 1933 Morris S. Kharasch and Frank Mayo proposed that free radicals were responsible for anti-Markovnikov addition of hydrogen bromide to allyl bromide.[18][19]

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)".[20] 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.[21]

## Diagnostics

Radicals typically exhibit paramagnetism. Electron spin resonance is the definitive and widely used technique for characterizing radicals. The nature of the atom bearing the unpaired electron and its neighboring atoms can often be deduced by the EPR spectrum.[22]

The presence of 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.

## Depiction in chemical reactions

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

${\displaystyle \mathrm {Cl} _{2}\;{\xrightarrow {UV}}\;2{\mathrm {Cl} \cdot }}$

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.

Radicals also take part in radical addition and radical substitution as reactive intermediates. Chain reactions involving 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 radicals. They may involve the formation of radicals from stable species as in Reaction 1 above or they may involve reactions of radicals with stable species to form more radicals.
• Propagation reactions are those reactions involving radicals in which the total number of radicals remains the same.
• Termination reactions are those reactions resulting in a net decrease in the number of radicals. Typically two radicals combine to form a more stable species, for example: 2Cl·→ Cl2

## References

2. ^ Hayyan, M.; Hashim, M.A.; AlNashef, I.M. (2016). "Superoxide Ion: Generation and Chemical Implications". Chem. Rev. 116 (5): 3029–85. doi:10.1021/acs.chemrev.5b00407. PMID 26875845.
3. ^ Griller, David; Ingold, Keith U. (1976). "Persistent carbon-centered radicals". Accounts of Chemical Research. 9: 13–19. doi:10.1021/ar50097a003.
4. ^ Oakley, Richard T. (1988). "Cyclic and Heterocyclic Thiazenes" (PDF). Progress in Inorganic Chemistry. Cyclic and Heterocyclic Thiazenes (section). Progress in Inorganic Chemistry. 36. pp. 299–391. doi:10.1002/9780470166376.ch4. ISBN 978-0-470-16637-6.
5. ^ Rawson, J; Banister, A; Lavender, I (1995). Advances in Heterocyclic Chemistry. The Chemistry of Dithiadiazolylium and Dithiadiazolyl Rings (section) =. Advances in Heterocyclic Chemistry. 62. pp. 137–247. doi:10.1016/S0065-2725(08)60422-5. ISBN 978-0-12-020762-6.
6. ^ However, paramagnetism does not necessarily imply radical character.
7. ^ Linde, C.; Åkermark, B.; Norrby, P.-O.; Svensson, M. (1999). "Timing is Critical: Effect of Spin Changes on the Diastereoselectivity in Mn(Salen)-Catalyzed Epoxidation". Journal of the American Chemical Society. 121 (21): 5083–84. doi:10.1021/ja9809915.
8. ^ Broderick, J.B.; Duffus, B.R.; Duschene, K.S.; Shepard, E.M. (2014). "Radical S-Adenosylmethionine Enzymes". Chemical Reviews. 114 (8): 4229–317. doi:10.1021/cr4004709. PMC 4002137. PMID 24476342.CS1 maint: uses authors parameter (link)
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 2248324. PMID 17237348.
10. ^ Njie-Mbye, Ya Fatou; Kulkarni-Chitnis, Madhura; Opere, Catherine A.; Barrett, Aaron; Ohia, Sunny E. (2013). "Lipid peroxidation: pathophysiological and pharmacological implications in the eye". Frontiers in Physiology. 4: 366. doi:10.3389/fphys.2013.00366. PMC 3863722. PMID 24379787.
11. ^ 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): 1346–55. doi:10.1016/s0891-5849(98)00293-7.
12. ^ An overview of the role of 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 978-0-7484-0916-7.
13. ^ 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 (2): 257–63. doi:10.1007/s10811-010-9564-0.
14. ^ 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): 8491–96. Bibcode:2004PNAS..101.8491M. doi:10.1073/pnas.0402531101. PMC 420421. PMID 15152078.
15. ^ Lyons, MA; Brown, AJ (1999). "7-Ketocholesterol". Int. J. Biochem. Cell Biol. 31 (3–4): 369–75. doi:10.1016/s1357-2725(98)00123-x. PMID 10224662.
16. ^ 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): 970–81. doi:10.1039/b206338g. PMID 12661594.
17. ^ Njie-Mbye, Ya Fatou; Kulkarni-Chitnis, Madhura; Opere, Catherine A.; Barrett, Aaron; Ohia, Sunny E. (2013). "Lipid peroxidation: pathophysiological and pharmacological implications in the eye". Frontiers in Physiology. 4. doi:10.3389/fphys.2013.00366. PMC 3863722. PMID 24379787.
18. ^ Kharasch, M. S. (1933). "The Peroxide Effect in the Addition of Reagents to Unsaturated Compounds. I. The Addition of Hydrogen Bromide to Allyl Bromide". Journal of the American Chemical Society. 55: 2468–2496. doi:10.1021/ja01333a041.
19. ^ Yan, M; Lo, JC; Edwards, JT; Baran, PS (2016). "Radicals: Reactive Intermediates with Translational Potential". J Am Chem Soc. 138: 12692–12714. doi:10.1021/jacs.6b08856. PMC 5054485. PMID 27631602.
20. ^ G. Herzberg (1971), "The spectra and structures of simple free radicals", ISBN 0-486-65821-X.
21. ^ 28th International Symposium on Free Radicals Archived 2007-07-16 at the Wayback Machine.
22. ^ Chechik, Victor; Carter, Emma; Murphy, Damien (2016). Electron Paramagnetic Resonance. Oxford University Press. ISBN 978-0-19-872760-6.