What exactly is a radical in inorganic chemistry? What is meant by a free radical?

Question

I am new to chemistry so please make your explanations easy to understand! Any help is appreciated.

Answer 1

Those are rebel elements in your physiology that roam your body, attack and destroy ordinary cells. They are destroyed by antioxidants.

Answer 2

Define Radical Chemistry

Answer 3

A radical (meaning = radix, root) was originally meant to be a hydrocarbon fragment that gave the identity to an organic compound. For example, CH3-OH is methyl alcohol, and methyl, CH3- is a radical. Ethyl chloride is CH3CH2-Cl, and ethyl, CH3CH2- is a radical. Chemists always wondered whether radicals had free existence apart from the compounds where they were.

About 1905, Moses Gomberg, organic chemistry professor at the University of Michigan, made hexaphenylethane. This is two carbon atoms surrounded by six benzene rings, (C6H5)3C-C(C6H5)3. He found that it was a white powder, but gave a yellow solution in benzene. Also, the benzene solution gave (C6H5)3C-OH. So he concluded that the yellow solution was triphenylmethyl radical, (C6H5)3C- (in 1905, every one knew that carbon atoms were connected by "-" bonds, but no one knew what "-" meant).

Nowadays, chemists know that "-" means an unpaired electron. So if "*" is an unpaired electron, then CH3* is a methyl free radical. As for your question about inorganic chemistry, there all sorts of other free radicals: *OH is hydroxyl, *Cl is chlorine, the atom. Oxygen gas, O2, is a diradical, because each atom of *O=O* has an unpaired electron on it. Because nitrogen has an odd number of valence electrons (5), oxides of nitrogen tend to be free radicals, which join together in bonds: 2*NO ===> O=N-N=O. An inorganic free radical has an unpaired electron on any atom other than carbon.

Answer 4

Free radicals only have 1 lone unpaired electron. This makes it very reactive. This means that when it reacts with another substance that doesn't have an unpaired electron, one of the products will have an unpaired electron. The only way to stop the chain reaction is to react 2 free radicals together, so the unpaired electrons pair with each other forming a stable product.

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Answer 5

Normally, atoms have pairs of electrons orbiting them. A pair may be used to form a bond with another atom, or it may be what's called a "lone pair" which is only attached to one atom, but it is a pair.

A radical is an atom which has an odd number of electrons around it, so that one electron is not part of a pair. Radicals tend to be very reactive, because unpaired electrons are less stable than paired ones. They're bad for you because they can react with DNA, causing mutations that lead to cancer.

A free radical is one that can move around and react with stuff. Most radicals are also free radicals.

Answer 6

The first part of yr Q I cannot answer but the second part I can
A free radical is a tree-hugger who has been released on bail after blocking a semi carrying trees for a the logging company.

Answer 7

If you zap Cl2 (chlorine molecule) with UV light, you get two chlorine radicals - they have no charge, they are neutral but desperate to combine with something, even if it's another chlorine radical.

Answer 8

hi

Answer 9

In chemistry, radicals (often referred to as free radicals) are atomic or molecular species with unpaired electrons on an otherwise open shell configuration. These unpaired electrons are usually highly reactive, so radicals are likely to take part in chemical reactions. Because they are uncharged, their reactivity is different from the reactivity of similar ions. Radicals play an important role in combustion, atmospheric chemistry, polymerization, plasma chemistry, biochemistry, and many other chemical processes, including human physiology. For example, superoxide and nitric oxide regulate many biological processes, such as controlling vascular tone. "Radical" and "Free Radical" are frequently used interchangeably, however a radical may be trapped within a solvent cage or be otherwise bound. The first organic free radical, the triphenylmethyl radical was identified by Moses Gomberg in 1900.

Historically, the term radical has also been used for bound parts of the molecule, especially when they remain unchanged in reactions. For example, methyl alcohol was described as consisting of a methyl 'radical' and a hydroxyl 'radical'. Neither were radicals in the usual chemical sense, as they were permanently bound to each other, and had no unpaired, reactive electrons. In mass spectrometry, such radicals are observed after breaking down the substance with a hail of energetic electrons.
[edit] Depicting radicals in chemical reactions
In written chemical equations, free radicals are frequently denoted by a dot placed immediately to the right of the atomic symbol or molecular formula as follows:

Cl2 + hν → 2 Cl·
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. It should be noted that 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.

In chemistry, free radicals take part in radical addition and radical substitution as reactive intermediates. Reactions involving free radicals can usually be divided into three distinct processes: initiation, propagation, and termination.

Initiation reactions are those which 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

[edit] Formation
The formation of radicals requires covalent bonds to be broken homolytically, a process that requires significant amounts of energy. For example, splitting H2 into 2H· has a ΔH° of +435 kJ/mol, and Cl2 into 2Cl· has a ΔH° of +243 kJ/mol. This is known as the homolytic bond dissociation energy, and is usually abbreviated as the symbol DH°. The bond energy between two covalently bonded atoms is affected by the structure of the molecule as a whole, not just the identity of the two atoms, and radicals requiring more energy to form are less stable than those requiring less energy. Homolytic bond cleavage most often happens between two atoms of similar electronegativity. In organic chemistry this is often the O-O bond in peroxide species or O-N bonds.

However, propagation is a very exothermic reaction. Note that all species are electrically neutral although radical ions do exist.


[edit] Persistence and stability

The radical derived from α-tocopherolLong lived radicals can be placed into two categories

Stable Radicals
Purely organic radicals can be long lived if they occur in a conjugated π system, such as the radical derived from α-tocopherol (vitamin E). Albeit there exist hundreds of known examples of heterocyclic thiazyl radicals which show remarkable kinetic and thermodynamic stability, with only a very limited extent of π resonance stabilization [Oakley, R.T. Prog. Inorg. Chem. 1998, 36, 299; Banister, A.J., et al. Adv. Hetero. Chem. 1995, 62, 137].
Persistent Radicals
Persistent radical compounds are those whose longevity is due to steric crowding around the radical center and makes it physically difficult for the radical to react with another molecule. Examples of these include Gomberg's radical (triphenylmethyl), Fremy's salt (Potassium nitrosodisulfonate, (KSO3)2NO·), nitroxides, (general formula R2NO·) such as TEMPO, verdazyls, nitronyl nitroxides, and azephenylenyls. The longest-lived free radical is melanin, which may persist for millions of years.
biradicals are molecules containing two radical centers. Multiple radical centers can exist in a molecule.

[edit] Reactivity
Radical alkyl intermediates are stabilized by similar criteria as carbocations: the more substituted the radical center is, the more stable it is. This will direct their reactions: formation of a tertiary radical (R3C·) is favored over secondary (R2HC·) or primary (RH2C·). However, radicals next to functional groups, such as carbonyl, nitrile, and ether are even more stable than tertiary alkyl radicals.

Radicals attack double bonds, but unlike similar ions, they are slightly less 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. Nonetheless, the electrophilic/neutrophilic character of radicals has been shown in a variety of instances (e.g., in the alternating tendency of the copolymerization of malieic anhydride (electrophilic) and styrene (slightly nuecleophilic).

In intramolecular reactions, precise control can be achieved despite the extreme reactivity of radicals. Radicals will 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 five or more atoms away in the chain are infrequent.


[edit] Combustion

Spectrum of the blue flame from a butane torch showing excited molecular radical band emission and Swan bands.Probably the most familiar free-radical reaction for most people is combustion. The oxygen molecule is a stable diradical, best represented by ·O-O·, which is stable because the spins of the electrons are parallel. The ground state of oxygen is an unreactive spin-paired (triplet) radical, but an extremely reactive spin-unpaired (singlet) radical is available. In order for combustion to occur, the energy barrier between these must be overcome. This barrier can be overcome by heat, requiring high temperatures, or can be lowered by enzymes to initiate reactions at the temperatures inside living things.

Combustion is comprised of various radical chain reactions that the singlet radical can initiate. The flammability of a given material is strongly dependent 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. Propagation or termination reactions can be promoted to alter flammability. Tetraethyl lead was once commonly added to gasoline, because it very easily breaks up into radicals, which consume other free radicals in the gasoline-air mixture. This prevents the combustion from initiating prematurely (see engine knock).


[edit] Polymerization
In addition to combustion, many polymerization reactions involve free radicals. As a result many plastics, enamels, and other polymers are formed through radical polymerization.

Recent advances in radical polymerization methods, known as Living Radical Polymerization, include:

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.


[edit] Atmospheric radicals
In the upper atmosphere free radicals are produced through dissociation of the source molecules, particularly the normally unreactive chlorofluorocarbons by solar ultraviolet radiation or by reactions with other stratospheric constituents. These free radicals then react with ozone in a catalytic chain reaction which destroys the ozone, but regenerates the free radical, allowing it to participate in additional reactions. Such reactions are believed to be the primary cause of depletion of the ozone layer and this is why the use of chlorofluorocarbons as refrigerants has been restricted.


[edit] Free radicals in biology
Free radicals play an important role in a number of biological processes, some of which are necessary for life, such as the intracellular killing of bacteria by neutrophil granulocytes. Free radicals have also been implicated in certain cell signalling processes. The two most important oxygen-centered free radicals are superoxide and hydroxyl radical. They are derived from molecular oxygen under reducing conditions. However, because of their reactivity, these same free radicals can participate in unwanted side reactions resulting in cell damage. Many forms of cancer are thought to be the result of reactions between free radicals and DNA, resulting in mutations that can adversely affect the cell cycle and potentially lead to malignancy. Some of the symptoms of aging such as atherosclerosis are also attributed to free-radical induced oxidation of many of the chemicals making up the body. In addition free radicals contribute to alcohol-induced liver damage, perhaps more than alcohol itself. Radicals in cigarette smoke have been implicated in inactivation of alpha 1-antitrypsin in the lung. This process promotes the development of emphysema.

Free radicals may also be involved in Parkinson's disease, senile and drug-induced deafness, schizophrenia, and Alzheimer's. 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. The free radical theory of aging proposes that free radicals underlie the aging process itself.

Because free radicals are necessary for life, the body has a number of mechanisms to minimize free radical induced damage and to repair damage which does occur, 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. Further, there is good evidence 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 [1].


[edit] Reactive oxygen species
Main article: Reactive oxygen species
Reactive oxygen species or ROS are species such as superoxide, hydrogen peroxide, and hydroxyl radical and are associated with cell damage.

Free radicals are also produced inside (and also released towards the cytosol) organelles, such as the mitochondrion. Mitochondria convert energy for the cell into a usable form, adenosine triphosphate (ATP). The process in which ATP is produced, called oxidative phosphorylation, inovolves the transport of protons (Hydrogen ions) across the inner mitochondrial membrane by means of the electron transport chain. In the electron transport chain, electrons are passed through a series of proteins via oxidation-reduction reactions, with each acceptor protein along the chain having a greater reduction potential than the last. The last destination for an electron along this chain is an oxygen molecule. Normally the oxygen is reduced to produce water; however, in about 1-2% of all cases, the oxygen is instead reduced to give the superoxide radical,·O2-. Superoxide needs an additional electron to make it more stable, so it steals an electron from the nearest source, such as: mitochondrial DNA, the mitochondrial membrane (called lipid peroxidation), or from protein, or from reductants such as Vitamins C or E, or, from non enzymatic antioxidants such as glutathione or thioredoxin. If too much damage is caused to the mitochondrion, it experiences apoptosis, or programmed cell death.

Bcl-2 proteins are layered on the surface of the mitochondria, detect damage, and activate a class of proteins called Bax, which punch holes in the mitochondrial membrane, causing cytochrome C to leak out. This cytochrome C binds to Apaf-1, or apoptotic protease activating factor-1, which is free-floating in the cell’s cytoplasm. Using energy from the ATPs in the mitochondrion, the Apaf-1 and cytochrome C bind together to form apoptosomes. The apoptosomes binds to and activates caspase-9, another free-floating protein. The caspase-9 then cleaves the proteins of the mitochondrial membrane, causing it to break down and start a chain reaction of protein denaturation and eventually phagocytosis of the cell.

According to the Free Radical Theory of Aging, aging occurs (via a loss of energy producing cells) either when mitochondria begin to die out because of free radical damage or, when less functional mitochondria remain within these cells. The focus of the project is to neutralize the effect of these free radicals with antioxidants. Antioxidants neutralize free radicals by donating one of their own electrons. The antioxidant nutrients themselves don’t become free radicals by donating an electron because they are stable in either form.

Superoxide dismutase (SOD) is present in two places naturally in the cell. SOD that is present in the mitochondria contains manganese (MnSod). This SOD is transcribed in the nucleus and has a mitochondrial targeting sequence, thereby localizing it to the miotchondrial matrix. SOD that is present in the cytoplasm of the cell contains copper and zinc (CuZnSod). The genes that control the formation of SOD are located on chromosomes 21, 6, and 4. When superoxide dismutase comes in contact with superoxide, it reacts with it and forms hydrogen peroxide. The stoichiometry of this reaction is that for each 2 superoxide radicals encountered by SOD, 1 H2O2 is formed. This hydrogen peroxide is dangerous in the cell because it can easily transform into a hydroxyl radical (via reaction with Fe2+:Fenton chemistry), one of the most destructive free radicals. Catalase, which is concentrated in peroxisomes located next to mitochondria but formed in the rough endoplasmic reticulum and located everywhere in the cell, reacts with the hydrogen peroxide and forms water and oxygen. Glutathione peroxidase reduces hydrogen peroxide by transferring the energy of the reactive peroxides to a very small sulfur containing protein called glutathione. The selenium contained in these enzymes acts as the reactive center, carrying reactive electrons from the peroxide to the glutathione. Peroxiredoxins also degrade H2O2, both within the mitochondria, cytosol and nucleus.


[edit] Diagnostics
Free Radical diagnostic techniques include:

Electron Spin Resonance
A widely-used technique for studying free radicals, and other paramagnetic species, is electron spin resonance spectroscopy (ESR). This is alternately referred to as "electron paramagnetic resonance" (EPR) spectroscopy. It is conceptually related to nuclear magnetic resonance, though electrons resonate with higher-frequency fields at a given fixed magnetic field than do most nuclei.
Nuclear magnetic resonance using a phenomenon called CIDNP
Chemical Labelling
Chemical labelling by quenching with free radicals, e.g. with NO or DPPH, followed by spectroscopic methods like X-ray photoelectron spectroscopy (XPS) or absorption spectroscopy, respectively.
Use of free radical markers
Stable, specific or non-specific derivates of physiological substances can be measured e.g. lipid peroxidation products (isoprostanes, TBARS), amino acid oxidation products (meta-tyrosine, ortho-tyrosine, hydroxy-Leu, dityrosine etc.), peptide oxidation products (oxidized glutathione - GSSG)
Indirect method
Measurement of the decrease in the amount of antioxidants (e.g. TAS, reduced glutathione - GSH)

[edit] Elimination of systemic free radicals
Through the uptake of essential vitamins and coenzymes, such as retinoic acid, vitamin E, co-enzyme Q-10 and green teas/dark chocolates, the prevention of free radical formation may occur through the induced mediation of the MnSOD oxidative-stress response gene. Since reactive oxidative species (ROS) like sunlight and carcinogens lead to the formation of free radicals, inhibition of free radicals therefore decreases the risk of tumoric growth. In addition, since free radical regulators such as catalase and glutathione exist in equilibrium with ROS, any disruption in this balance will lead to oxidative stress which can be detrimental to the health of cells.[citation needed]