12190-71-5 Usage
Chemical Description
Different sources of media describe the Chemical Description of 12190-71-5 differently. You can refer to the following data:
1. Iodine is a halogen element that is used in various chemical reactions as a catalyst or reagent.
2. Iodine is a halogen element that is a purple-black solid at room temperature and is commonly used as a disinfectant and in organic synthesis.
3. Iodine is a chemical element with the symbol I and atomic number 53.
4. Iodine and triethylsilane are also used in the reaction as reagents.
5. Iodine and triethylsilane are used as a promoter system for efficient glycosylation.
6. Iodine is a halogen element used as an oxidizing agent.
Description
Different sources of media describe the Description of 12190-71-5 differently. You can refer to the following data:
1. Iodine,I, is a nonmetallic element with an orthorhombic crystal structure, a violet to black color. This poisonous element sublimes readily and is easily purified in this manner. It is insoluble in water,but is soluble in common solvents such as alcohol, ether,and carbon tetrachloride. Iodine is used as a germicide, an antiseptic, in dyes,tinctures, and pharmaceuticals. It is also used in the production of vanadium metal in the McKechnie-Seybolt process, which is the reduction of vanadium pentoxide in the presence of iodine. Iodine is used in a similar manner in the production of high-purity zirconium.
For many years, iodine tincture(3% to 7% dissolved in ethyl alcohol) has been an important antiseptic. The commercial tinctures also usually contain 5% potassium iodide to provide stability. This form produces a mild burning of the skin and stains both skin and fabrics. A milder preparation is available in which about 2% iodine is contained in an oil-water emulsion which also contains lecithin.
2. Iodine, (I), is a nonmetallic element of family seven, the halogens. It is heavy, grayish-black in color, has a characteristic odor, and is readily sublimed to a violet vapor. It has a vapor density of 4.98, which is heavier than air. It melts at 236°F (113.5°C), has a boiling point of 363°F (184°C), and is insoluble in water. Iodine is toxic by ingestion and inhalation, and is a strong irritant to eyes and skin. The TLV ceiling is 0.1 ppm in air. Iodine is used for antiseptics, germicides, x-ray contrast material, food and feed additives, water treatment, and medicinal soaps. The four-digit UN identification number for iodine is only for the compounds iodine monochloride and iodine pentafluoride, and they are 1792 and 2495, respectively. The DOT lists iodine monochloride as a Class 8 corrosive, and iodine pentafluoride carries an oxidizer and poison label. Iodine does not have an NFPA 704 designation.
Chemical Properties
Heavy, grayish-black plates or granules having a metallic luster; characteristic odor.
Readily sublimed having a violet vapor.Soluble in alcohol, carbon
disulfide, chloroform, ether, carbon tetrachloride,
glycerol, and alkaline iodide solutions; insoluble
Physical properties
Iodine in its pure state is a black solid that sublimates (changes from a solid to a gas withoutgoing through a liquid state) at room temperature. It produces a deep purple vapor that is irritatingto the eyes, nose, and throat. Iodine tends to form nonmetallic diatomic molecules (I2).It is the heaviest of the naturally occurring halogens. (Although astatine, the fifth element ingroup 17, is heavier than iodine, it is a synthetic element and does not occur in nature exceptas a very small trace.) Iodine is the least reactive of the five halogens.Iodine’s melting point is 113.7°C, its boiling point is 184.4°C, and its density is 4.93g/cm3.
Isotopes
There are a total of 145 isotopes of iodine. Only one (I-127) is stable andaccounts for 100% of iodine’s natural abundance on Earth. All the other 146 isotopesare radioactive with half-lives ranging from a 150 nanoseconds to 1.57×10+7
Origin of Name
The name originates from the Greek word iodes, meaning “violet-colored,”
which is the color of iodine’s vapor.
Occurrence
Iodine is the 64th most abundant element on Earth. It occurs widely over the Earth, butnever in the elemental form and never in high concentrations.It occurs in seawater where some species of seaweed and kelp accumulate the elementin their cells. It is also recovered from deep brine wells found in Chile, Indonesia, Japan,and Michigan, Arkansas, and Oklahoma in the United States. The iodine is recovered fromcremated ashes of seaweed. The ashes are leached with water to remove the unwanted salts.Finally, manganese dioxide (MnO2) is added to oxidize the iodine ions (I1-) to produceelemental diatomic iodine (I2). The following reaction takes place: 4I1- + MnO2 → MnI2 +I2 + 2O2-.Chilean saltpeter [potassium nitrate (KNO3)] has a number of impurities, includingsodium and calcium iodate. Iodine is separated from the impurities and, after being treatedchemically, finally produces diatomic iodine. Today, iodine is mostly recovered from sodiumiodate (NaIO3) and sodium periodate (NaIO4) obtained from Chile and Bolivia.
Characteristics
Iodine is the least reactive of the elements in the halogen group 17. Most people associateiodine with the dark-brown color of the tincture of iodine used as an antiseptic for minor skinabrasions and cuts. A tincture is a 50% solution of iodine in alcohol. Although it is still used,iodine is no longer the antibiotic of choice for small skin wounds. Since iodine is a poisonthat kills bacteria, iodine tablets are often used by campers and others to purify water that istaken from outdoor streams.
History
Discovered by Courtois in 1811. Iodine, a halogen, occurs sparingly in the form of iodides in sea water from which it is assimilated by seaweeds, in Chilean saltpeter and nitrate-bearing earth, known as caliche in brines from old sea deposits, and in brackish waters from oil and salt wells. Ultrapure iodine can be obtained from the reaction of potassium iodide with copper sulfate. Several other methods of isolating the element are known. Iodine is a bluish-black, lustrous solid, volatilizing at ordinary temperatures into a blue-violet gas with an irritating odor; it forms compounds with many elements, but is less active than the other halogens, which displace it from iodides. Iodine exhibits some metallic-like properties. It dissolves readily in chloroform, carbon tetrachloride, or carbon disulfide to form beautiful purple solutions. It is only slightly soluble in water. Iodine compounds are important in organic chemistry and very useful in medicine. Forty-two isotopes and isomers are recognized. Only one stable isotope, 127I, is found in nature. The artificial radioisotope 131I, with a half-life of 8 days, has been used in treating the thyroid gland. The most common compounds are the iodides of sodium and potassium (KI) and the iodates (KIO3). Lack of iodine is the cause of goiter. Iodides and thyroxin, which contains iodine, are used internally in medicine, and a solution of KI and iodine in alcohol is used for external wounds. Potassium iodide finds use in photography. The deep blue color with starch solution is characteristic of the free element. Care should be taken in handling and using iodine, as contact with the skin can cause lesions; iodine vapor is intensely irritating to the eyes and mucous membranes. Elemental iodine costs about 25 to 75￠/g depending on purity and quantity.
Uses
Different sources of media describe the Uses of 12190-71-5 differently. You can refer to the following data:
1. Dyes (aniline dyes, phthalein dyes), alkylation
and condensation catalyst, iodides, iodates, antiseptics and germicides, X-ray contrast media, food and
feed additive, stabilizers, photographic film, water
treatment, pharmaceuticals, medicinal soaps, unsat
2. Iodine is a halogen element extracted from chilean nitrate-bearing
earth or from seaweed. it functions by its presence in the thyroid
hormones. iodine deficiency is associated with goiter. sources are
potassium and cuprous iodide and potassium and calcium iodate, of
which the iodate form is preferred because of better stability. it is
used as a food supplement.
3. One of the most important uses of iodine is in the treatment of hypothyroidism, a conditionin which the thyroid gland is deficient in iodine. Iodine deficiency may lead to the formationof a goiter, wherein the gland that surrounds the windpipe in the neck becomes enlarged.There are other causes of goiter, including cancer of the thyroid gland. A deficiency of iodinecan also cause cretinism (infant hypothyroidism) in newborn babies, which can result inmental retardation unless the subject takes thyroid hormones for a lifetime. Green leafy foods,among other foods, contain iodine that when taken into the human body ends up in thethyroid gland. Some food grown in iodine-deficient soils do not contain adequate iodine forour diets. This is why iodine was added to table salt (about 0.01% potassium iodide) decadesago, specifically for people who live in regions with iodine-poor soils. The area around theGreat Lakes in the United States is one region with soil that is deficient in iodine. A healthydiet requires 90 to 150 micrograms of iodine each day that, in addition to being available iniodized salt, can be obtained from eating a balanced diet, including seafood.The isotope iodine-131 is an artificial radioisotope of iodine used as a tracer in biomedicalresearch and as a treatment for thyroid disease. I-131 has a half-life of about eight days, whichmeans it will be eliminated from the body in several weeks.In industry, iodine is used for dyes, antiseptics, germicides, X-ray contrast medium, foodand feed additives, pharmaceuticals, medical soaps, and photographic film emulsions and as alaboratory catalyst to either speed up or slow down chemical reactions.Iodine is also used as a test for starch. When placed on starch (a potato for example), iodineturns the starch a dark blue color. Silver iodide is used in the manufacture of photographicfilm and paper. It is also used to “seed” clouds because of its ability to form a large numberof crystals that act as nuclei upon which moisture in the clouds condenses, forming raindropsthat may result in rain.
Definition
Different sources of media describe the Definition of 12190-71-5 differently. You can refer to the following data:
1. A dark-violet volatile solid element belonging to the halogens (group 17 of the periodic table). It occurs in seawater and is concentrated by various marine organisms in the form of iodides. Significant deposits also occur in the form of iodates. The element is conveniently prepared by the oxidation of iodides in acid solution (using MnO2). Industrial methods similarly use oxidation of iodides or reduction of iodates to iodides by sulfur(IV) oxide (sulfur dioxide) followed by oxidation, depending on the source of the raw materials. Iodine and its compounds are used in chemical synthesis, photography, pharmaceuticals, and dyestuffs manufacture.
Iodine has the lowest electronegativity of the stable halogens and consequently is the least reactive. It combines only slowly with hydrogen to form hydroiodic acid, HI. Iodine also combines directly with many electropositive elements, but does so much more slowly than does bromine or chlorine. Because of the larger size of the iodine ion and the consequent low lattice energies, the iodides are generally more soluble than related bromides or chlorides. As with the other halides, iodides of Ag(I), Cu(I), Hg(I), and Pb(II) are insoluble unless complexing ions are present.
Iodine also forms a range of covalent iodides with the metalloids and non-metallic elements (this includes a vast range of organic iodides) but these are generally less thermodynamically stable and are more readily hydrolyzed than chlorine or bromine analogs.
2. Symbol I. A dark violet nonmetallic element belonging to group 17 of the periodic table; a.n. 53; r.a.m. 126.9045;r.d. 4.94; m.p. 113.5°C; b.p. 184.35°C.The element is insoluble in water but soluble in ethanol and other organic solvents. When heated it gives a violet vapour that sublimes. Iodine is required as a trace element by living organisms;in animals it is concentrated in the thyroid gland as a constituent of thyroid hormones. The element is present in sea water and was formerly extracted from seaweed. It is now obtained from oil-well brines (displacement by chlorine). There is one stable isotope, iodine-127, and fourteen radioactive isotopes. It is used in medicine as a mild antiseptic(dissolved in ethanol as tincture of iodine),and in the manufacture of iodine compounds. Chemically, it is less reactive than the other halogens and the most electropositive (metallic)halogen. In solution it can bedetermined by titration using thiosulphate solution: I2 + 252O32-→ 2I- + SuO62-. The molecule forms an intense bluecomplex with starch, which is consequentlyused as an indicator. It was discovered in 1812 by Courtois.
3. Nonmetallic halogen element of atomic number 53;
group VIIA of the periodic table; the least reactive
of the halogens, aw 126.9045; valences = 1,3,5,7;
no stable isotopes but many artificial radioactive
isotopes.
Hazard
Different sources of media describe the Hazard of 12190-71-5 differently. You can refer to the following data:
1. Toxic by ingestion and inhalation, strong
irritant to eyes and skin. Questionable carcinogen.
2. less than pure form, it can damage the skin, eyes, and mucous membranes. Both the elementalform and its compounds (gases, liquids, or solids) are toxic if inhaled or ingested. Even indiluted form (e.g., a tincture of iodine to treat minor skin wounds), it should be used withcare.Although a poison in high concentrations, iodine is required as a trace element in our dietsto prevent thyroid problems and mental retardation in the very young.
Industrial uses
Iodine is a purplish-black, crystalline, poisonouselementary solid, chemical symbol I, bestknown for its use as a strong antiseptic in medicine,but also used in many chemical compoundsand war gases. In tablet form it is usedfor sterilizing drinking water, and has less odorand taste than chlorine for this purpose. It isalso used in cattle feeds. Although poisonousin quantity, iodine is essential to proper cellgrowth in the human body, and is found in everycell in a normal body, with larger concentrationin the thyroid gland.A wide range of compounds are made forelectronic and chemical uses. Iodine is also achemical reagent, used for reducing vanadiumpentoxide and zirconium oxide into highpuritymetals.
Check Digit Verification of cas no
The CAS Registry Mumber 12190-71-5 includes 8 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 5 digits, 1,2,1,9 and 0 respectively; the second part has 2 digits, 7 and 1 respectively.
Calculate Digit Verification of CAS Registry Number 12190-71:
(7*1)+(6*2)+(5*1)+(4*9)+(3*0)+(2*7)+(1*1)=75
75 % 10 = 5
So 12190-71-5 is a valid CAS Registry Number.
InChI:InChI=1/I2/c1-2
12190-71-5Relevant articles and documents
Mesoporous carbon supported platinum nanocatalyst: Application for hydrogen production by HI decomposition reaction in S-I cycle
Tyagi, Deepak,Varma, Salil,Bharadwaj, Shyamala R.
, p. 2177 - 2184 (2017)
Platinum supported on carbon as a catalyst is widely reported and have a wide range of applications ranging from fuel cell application to hydrogenation reactions, where structure and properties of carbon support play an important role in the functioning of the catalyst. Mesoporous carbon supported platinum nanocatalyst was synthesized by hard templating route using mesoporous silica as template. The catalyst prepared has been characterized by X-ray diffraction, Raman, SEM, TEM, XPS and BET surface area. This catalyst has been employed for liquid phase HI decomposition reaction of sulfur iodine thermochemical cycle for production of hydrogen. The catalyst was evaluated for its activity for HI decomposition reaction and stability in the reaction environment. From present study we conclude that Pt supported on mesoporous carbon is a suitable and stable catalyst for liquid phase HI decomposition reaction.
Ashley, S. E.,West, W.
, p. 308 - 308 (1931)
Lamb,Bray,Geldard
, p. 1636 - 1636 (1920)
Liebhafsky, H. A.
, p. 3499 - 3499 (1932)
Chlorite-Iodide Reaction: A Versatile System for the Study of Nonlinear Dynamical Behavior
Kepper, Patrick De,Boissonade, Jacques,Epstein, Irving R.
, p. 6525 - 6536 (1990)
The autocatalytic reaction between chlorite and iodide ions exhibits a remarkable range of dynamical behavior.In a stirred tank reactor it shows bistability between steady states and between a steady and an oscillatory state.It forms the core of a large f
Francis, A. W.
, p. 655 - 655 (1926)
Rosenthaler
, p. 219 - 222 (1922)
The Oscillatory Briggs-Rauscher Reaction. 1. Examination of Subsystems
Furrow, Stanley D.,Noyes, Richard M.
, p. 38 - 42 (1982)
In acidic aqueous solution at 25 deg C, only slow or nonexistent reaction is observed for any two of three species iodate ion, hydrogen peroxide, and manganous ion.However, if all three species are present, 0.002 M Mn2+ catalyzes the iodate oxidation of peroxide at a rate almost 1000 times that in the absence of a catalyst! This remarkable observation, which has already been reported by Cooke, can be explained by postulating that the radical oxidant *IO2 is very sluggish at abstracting hydrogen atoms from the species like H2O2 but can oxidize Mn2+ by electron transfer.A detailed mechanism has been proposed that models semiquantitatively not only the manganous catalyzed iodate oxidation of peroxide but also the simultaneous induced disproportionation of the peroxide and the fact that the concentration of elementary iodine does not increase to a limiting value but rises to a maximum and then decreases toward a small value.Despite this single extremum, the subsystem does not exhibit oscillatory behavior.
Synthesis and Characterization of 2-Pyridinylmethylene-2-quinolyl Hydrazone Cobalt(III) Complexes. Reactivity Trends and Solvent Effect on the Initial and Transition States of Base Catalyzed Hydrolysis
Mohamad, Ahmad Desoky M.
, p. 1575 - 1595 (2017)
The complexes of pyridine-2-aldehyde-2-quinolylhydrazone Co(III) nitrate [Co(paqh)2](NO3)2, methyl-2-pyridylketone-2-quinolinhyrazone Co(III) nitrate [Co(mpkqh)2](NO3)2, and phenyl-2-pyridylketon-2-quinolinhyrazone Co(III) nitrate [Co(ppkqh)2](NO3)2 were prepared and characterized. Solubilities of Co(III)–hydrazone complexes were measured. Transfer chemical potentials were calculated from the measured solubilities of the Co(III) complexes in aqueous methanol mixtures at 25?°C. The reactivity trends in the transfer chemical potentials are discussed in terms of the nature of the bonded ligands. Kinetics of the base hydrolysis of Co(III)–hydrazone complexes in the aqueous methanol mixtures have been studied at 25?°C, and follow the rate law kobs?=?k2[OH?]. The solvent effects on the reactivity trends of Co(III) complexes are analyzed into initial state (is) and transition states (ts) components. The reaction rates are reduced by the increase of methanol content. The destabilization of the transition state is remarkable compared to the initial state in the aqueous methanol mixtures. The initial state is more hydrophobic in nature than the transition state for Co(III) complex reactions.
Kinetics of the Oxidation of Substrate Ligands by Transition-metal Cations
Nazar, Abdul Fattah M.,Wells, Cecil F.
, p. 801 - 812 (1985)
The kinetics of the oxidation of iodide ions by CeaqIV have been investigated.The reaction is found to be first order in each of IV>, and , in contrast to the oxidation of Br(1-) by CeaqIV, which is second order in both and .Nevertheless, the direct order of one in found for the CeIV + I(1-) reaction can only be interpreted by assuming the involvement of intermediate Ce(4+) - I(1-) complexes.The second-order rate constant for the oxidation of I(1-) by CoaqIII is shown to vary with ionic strength, so the entalphy ΔH* and entropy ΔS* of activation have been determined in conditions where the rate is invariant with ionic strength.These values for ΔH* and ΔS* are compared with the values for other substrates.The oxidation of iodide ions is discussed in relation to a general mechanism for the oxidation of substrate ligands by aquatransition-metal cations.
Luther, R.,Rutter, T. F.
, p. 521 - 522 (1907)
Kruisheer, C. I.
, p. 196 - 197 (1932)
Smith, D. F.,Mayer, J. E.
, p. 75 - 83 (1924)
On-site detection of phosgene agents by surface-enhanced Raman spectroscopy coupled with a chemical transformation approach
Gao, Haiyue,Wu, Jianfeng,Zhu, Yingjie,Guo, Lei,Xie, Jianwei
, p. 233 - 239 (2016)
Phosgene and its analogs are greatly harmful to the public health, environmental safety and homeland security as widely used industrial substances with extremely high toxicity. In order to rapidly evaluate the emergency risk caused by these chemicals, a new highly sensitive method based on surface-enhanced Raman spectroscopy (SERS) technique for measurement of phosgene agents was developed for the first time. Coupled with a chemical transformation approach, the highly toxic phosgene was conveniently converted to a SERS-sensitive probe, i.e. iodine (I2), with low toxicity or non-toxicity. The characteristic SERS peak in 459 cm-1 was used for quantitation and was presumed as a formation of triiodide anion (I3-), which was induced in an iodide (I-)-aggregation Au NPs system. The total measurement can be completed in ~20 min with the limits of detection of ~60 μg/l (phosgene) and ~30 μg/l (diphosgene), respectively, on a portable Raman spectrometer. This work is the first report of SERS measurement on phosgene and diphosgene in a quantitative level. This method is expected to meet the requirements of on-site detection of phosgene agents, promote emergency responses and raise more opportunities for the portable SERS applications. A sensitive surface-enhanced Raman spectroscopy method for measurement of phosgene agents with a chemical transformation approach was reported for the first time. With the transformed product iodine, a more stable triiodide anion was formed in an iodide-aggregated Au nanoparticles system appeared as a characteristic ultraviolet-visible absorption peak at 352 nm and a surface-enhanced Raman spectroscopy peak of 459 cm-1. Three phosgene agents exhibit different reaction rates.
Juan, Julian de,Smith, Ian W. M.
, (1985)
Edgar, G.
, p. 2369 - 2377 (1916)
Experimental and modeling study of oscillations in the chlorine dioxide-iodine-malonic acid reaction
Lengyel, István,Rábai, Gyula,Epstein, Irving R.
, p. 9104 - 9110 (1990)
At pH 0.5-5.0, a closed system containing an aqueous mixture of chlorine dioxide, iodine, and a species such as malonic acid (MA) or ethyl acetoacetate, which reacts with iodine to produce iodide, shows periodic changes in the light absorbance of I3-. This behavior can be modeled by a simple scheme consisting of three component reactions: (1) the reaction between MA and iodine, which serves as a continuous source of I-; (2) the reaction between ClO2? and I-, which acts as a source of ClO2-; and (3) the self-inhibited reaction of chlorite and iodide that kinetically regulates the system. The fast component reaction between chlorine dioxide and iodide ion was studied by stopped-flow spectrophotometry. The rate law is -[ClO2?]/df = 6 × 103 (M-2 s-1)[ClO2?][I-]. A two-variable model obtained from the empirical rate laws of the three component reactions gives a good description of the dynamics of the system. The oscillatory behavior results not from autocatalysis but from the self-inhibitory character of the chlorite-iodide reaction.
Amis, E. S.,Potts, J. E.
, p. 2883 - 2888 (1941)
Weak acids enhance halogen activation on atmospheric waters surfaces
Hayase, Sayaka,Yabushita, Akihiro,Kawasaki, Masahiro,Enami, Shinichi,Hoffmann, Michael R.,Colussi, Agustin J.
, p. 4935 - 4940 (2011)
We report that rates of I2(g) emissions, measured via cavity ring-down spectroscopy, during the heterogeneous ozonation of interfacial iodide: I-(surface, s) + O3(g) + H+(s) →→ I2(g), are enhanced several-fold, whereas those of IO · (g) are unaffected, by the presence of undissociated alkanoic acids on water. The amphiphilic weak carboxylic acids appear to promote I2(g) emissions by supplying the requisite interfacial protons H+(s) more efficiently than water itself, at pH values representative of submicrometer marine aerosol particles. We infer that the organic acids coating aerosol particles ejected from oceans topmost films should enhance I2(g) production in marine boundary layers.
Bates, J. R.,Lavin, G. I.
, p. 81 - 81 (1933)
Spontaneous Formation of Cellular Chemical System that Sustains Itself far from Thermodynamic Equilibrium
Maselko, Jerzy,Strizhak, Peter
, p. 4937 - 4939 (2004)
We report the observation of the spontaneous formation of a cellular structure in a simple inorganic system. The system is obtained by immersing a pellet of calcium and copper chlorides in an alkali solution containing sodium carbonate, sodium iodide, and hydrogen peroxide. The system produces a cell surrounded by a semipermeable membrane. Reactants diffuse and react inside the cell with copper ions serving as catalyst. The products diffuse out of the cell. The system sustains itself far from thermodynamic equilibrium.
Liebhafsky, H. A.
, p. 1792 - 1792 (1932)
Chaumeil, A.
, p. 194 - 194 (1903)
Lewis, B.
, p. 493 - 493 (1927)
Masson, I.,Argument, C.
, (1938)
Synthesis, structural and magnetic characterizations of a dinuclear copper(II) complex with an (N,S,O) donor ligand: Catecholase and phenoxazinone synthase activities
Ghosh, Ayon Kanti,Ali, Anzar,Singh, Yogesh,Purohit, Chandra Shekhar,Ghosh, Rajarshi
, p. 156 - 163 (2018/02/20)
A new dinuclear Cu(II) complex (1) was synthesized and crystallographically characterized. Each of the Cu(II) centres has penta coordination and been found to adopt square pyramidal geometry. Variable temperature magnetic measurements showed that there is weak ferromagnetic interaction between the Cu(II) centres in 1. 1 shows catecholase as well as phenoxazinone synthase activities in different solvents. The turn over numbers for the catecholase activity were 4.02 × 103 h?1 (MeOH) and 9.57 × 103 h?1 (MeCN), and that of phenoxazinone synthase activity were 1.065 × 103 h?1 (MeOH), 2.13 × 102 h?1 (MeCN) and 2.844 × 103 h?1 (DCM).
Xn:Harmful;
