What is the color of Iodine?
The symbol I is a chemical element.It is a lustrous, black non-metallic solid that can be melted to form a deep violet liquid at 114 degrees Celsius and then boiled to a violet gas at 184 degrees.Two years after Bernard Courtois discovered the element, Joseph Louis Gay-Lussac named it after the Greek "violet-coloured".
I, iodate, and the various periodate anions are oxidation states.The sixty-first most abundant element is the least abundant.It is the most essential mineral.Iodine is used in the synthesis of hormones.Iodine deficiency is the leading cause of intellectual disabilities and affects two billion people.
Japan and Chile are the main producers of iodine.Iodine is used in nutrition.It has been found to be a non-toxic radiocontrast material due to its high atomic number and ease of attachment to organic compounds.Because of the specificity of its absorption by the human body, radioactive iodine can be used to treat thyroid cancer.Iodine is used in the production of acetic acid.
Bernard Courtois was born to a manufacturer of saltpetre, an essential component of gunpowder.Saltpetre was in high demand during the time of the Napoleonic Wars.Saltpetre can be isolated from seaweed collected on the coast of Normandy and Brittany.The seaweed was burned and the ash washed.Adding sulfuric acid destroyed the remaining waste.A cloud of purple vapour rose when Courtois added excessive sulfuric acid.He noted that the liquid crystallised on cold surfaces.Courtois suspected that this was a new element but lacked funding to pursue it further.[8]
Courtois gave samples to his friends to continue their research.Some of the substance was given to chemist Joseph Louis Gay-Lussac and physicist André-Marie Ampre.Desormes and Clément made Courtois' discovery public.The substance was described to a meeting of the Imperial Institute of France.Gay-Lussac announced on 6 December that the new substance was either an element or a compound of oxygen.Gay-Lussac came up with the name "iode", from the Greek word for violet, ioeids.Ampre gave some of his sample to an English chemist who compared it to chlorine.The Royal Society of London received a letter from Davy stating that he had identified a new element.Both scientists acknowledged that Courtois was the first to identify the element.[8]
The antiseptic action of iodine was discovered by a French researcher in 1873.Antonio Grossich, an Istrian born surgeon, was one of the first to use sterilization.He came up with the idea of quickly sterilizing the human skin in the surgical field.[17]
Iodine is a member of group 17 in the periodic table and is the heaviest stable member.The fifth and sixth halogens, the radioactive astatine and tennessine, are not well-studied due to their expense and inaccessibility in large quantities.The seven electrons in the fifth and outermost shell are its valence electrons.Like the other halogens, it is one electron short of a full octet and is therefore a strong oxidising agent, reacting with many elements in order to complete its outer shell.The diatomic molecule formed with chemical formula I2 is where two iodine atoms share a pair of electrons in order to each achieve a stable octet for themselves.The strongest reducing agent among stable halogens is the iodide anion, which is easily oxidised back to diatomic I2.Astatine is unstable as At and readily oxidised to At0 or At+, although the existence of At2 is not settled.)[20]
fluorine is a pale yellow gas, chlorine is greenish-yellow, and bromine is reddish-brown volatile liquid.Iodine is a shiny black solid that forms a violet gas by boiling at 183 C.This trend occurs because the wavelengths of visible light absorbed by the halogens increase down the group, though astatine may not conform to it, depending on how metallic it turns out to be.The violet colour of iodine gas is a result of the electron transition between the highest occupied antibonding g and the lowest vacant one.[21]
One gram of irene can be dissolved in 3450 liters of water at 20 C and 1200 liters at 50.The higher the solubility, the more nonpolar the solvent is.The color of polar solutions is brown, reflecting their role as Lewis bases, while nonpolar solutions are violet.The charge-transfer complexes form when iodine is dissolved in polar solvents.Iodine is violet when dissolved in carbon tetrachloride and saturated hydrocarbons, but deep brown in alcohols and amines, which form charge-transfer adducts.[23]
The melting and boiling points of iodine are the highest among the halogens, due to the fact that it has the most easily polarised electron cloud among them.Iodide is the least volatile of the halogens.The lowest first ionisation energy, lowest electron affinity, and lowest reactivity of the halogens can be found in iodine.[19]
The interhalogen bond in diiodine is weak.A small amount of a sample of iodine at atmospheric pressure is converted to iodine atoms at 575 C.The required temperatures for fluorine, chlorine, and bromine are greater than 750 C.The bonds to the lighter halogens are stronger.Gaseous iodine has an I–I bond length of 266.6 pm.One of the longest bonds is the I–I bond.It is even longer in the same crystal structure as chlorine and bromine.The Xe–Xe bond length is more than three hours.Significant electronic interactions occur with the two next-nearest neighbours of each atom, and these interactions give rise to a shiny appearance and semiconducting properties.Iodine is a two-dimensional Semiconductor with a band gap of 1.3 eV.[19]
Only one of the thirty-seven known isotopes of iodine is found in nature.The others have half-lives that are too short to be primordial.iodine is both monoisotopic and mononuclidic and its atomic weight is known to great precision as it is a constant of nature.[19]
Isidore-129 has a half-life of 15.7 million years and is stable.It is still possible to date the history of the early Solar System using an extinct radionuclide that was formed along with iodine-129.Its former presence may be determined by the amount of its daughter.The traces of iodine-129 still exist today, as it is a nuclide formed from atmospheric xenon.It occurs from open-air nuclear testing and is not hazardous because of its long half-life.At the peak of thermonuclear testing in the 1960s and 1970s, iodine-129 made up only 10% of the total.Mssbauer spectroscopy uses excited states of iodine-129 and 127.[19]
The other radioisotopes have half-lives that are shorter than days.Some of them have medical applications that involve storing and concentrating the iodine that enters the body.Nuclear medicine uses tellurium-123, which has a half-life of thirteen hours and decays by electron capture.Iodine-125 has a half-life of fifty-nine days and is the second-longest-lived radioisotope.With a half-life of eight days,beta decays to an excited state of stable xenon-131 that then converts to the ground state by emitting radiation.It is a common product and is present in high levels.It can be absorbed through food and accumulate in the body.It may cause damage to the thyroid as it decays.Radiogenic thyroid cancer is a risk from exposure to high levels of iodine-131.There is a possibility of non-cancerous growths.[35]
The best way to protect against the negative effects of iodine-131 is to take a daily dose of potassium iodide tablets.In radiation therapy, iodine-131 may be used for therapeutic purposes when tissue destruction is desired.Iodine-131 is used as a radioactive tracer.38,39,40,41
Iodine is not as reactive as the other halogens.Carbon monoxide, nitric oxide, and sulfur dioxide will not be halogenated by chlorine gas.iodination of metals tends to result in lower oxidation states than chlorination or bromination; for example, rhenium metal reacts with chlorine to form Rhenium hexachloride, but with bromine it forms onlyRhenium trichloride.Since iodine has the lowest ionisation energy among the halogens and is the most easily oxidised of them, it has a more significant cationic chemistry and its higher oxidation states are more stable than those of bromine and chlorine.[21]
I2 is dissolved in CCl4 and aliphatic hydrocarbons to give bright violet solutions.The absorption band maximum is assigned to a transition in the 520 - 540 nm region.When I2 reacts with Lewis bases, there is a blue shift in the peak and the new peak is due to the formation of adducts, which are referred to as charge-transfer complexes.[42]
H2O is the simplest compound of iodine.Oxygen reacts with colourless gas to give water and iodine.Unlike the other hydrogen halides, it does not have large-scale industrial uses.It is usually made with hydrogen sulfide or hydrazine.
It is a colourless gas, like all of the hydrogen halides except hydrogen fluoride, since hydrogen can't form strong hydrogen bonds to the large and only mildly negative iodine atom.It is able to melt at 51.0 and boil at 35.1C.It is an endothermic compound that can be dissociation at room temperature, although the process is very slow unless a catalyst is present.The smallest of hydrogen halides, the H–I bond dissociation energy, is 295 kJ/mol.[42]
A strong acid is known as hydroiodic acid.The saturated solution has only four water molecule per molecule of hydrogen iodide, which is why it is so soluble in water.The solution forms an azeotrope with a boiling point of 56.7 g HI per 100 g solution.It is not possible to concentrate hydroiodic acid past this point.[42]
Anhydrous liquid hydrogen iodide is difficult to work with as a solvent because its boiling point is low, it has a small liquid range, and it does not dissociate into H2I+ and HI2 ion.Anhydrous hydrogen iodide is not a good solvent for dissolving small molecule compounds, such as nitrosyl chloride and phenol, or salts with very low lattice energies.[42]
The periodic table has nearly all elements in it.Extreme nuclear instability, extreme inertness and reluctance to participate in chemical reactions are some of the reasons why the exceptions are in the minority.Nitrogen triiodide is similar to the other nitrogen trihalides.)
It is difficult to achieve high oxidation states in binary iodides due to the large size of the anion and weak oxidising power.Iodides can be made by reaction of an element or its oxide, hydroxide, or carbonate with hydroiodic acid, and then dehydrated by either low pressure or anhydrous hydrogen iodide gas.The best way to use these methods is if the iodide product is stable to hydrolysis.Molybdenum(IV) oxide reacts with a metal at a temperature of 230 C.An example of a halogen exchange is given below, with the reaction of tantalum(V) chloride with excess aluminium(III) iodide at 400 C.
Lower iodides can be produced either through thermal decomposition or disproportionation, or by reducing the higher iodide with hydrogen or a metal.
Most of the pre-transition metals, along with the lanthanides and actinides in the +2 and +3 oxidation states, are mostly ionic.The strongest attraction between the cations and anions is found in the large iodide anion, which is why it has the lowest melting and boiling points among the halides.When it comes to van der Waals forces, the highest melting and boiling points among the halides of the same element are found in covalent iodides.One trend gives way to the other in intermediate iodides.There are solubilities in the water of predominantly ionic iodides.The greatest ionic halides of that element are calcium and potassium.The lowest element is silver.The formation of silver iodide in water is used as a qualitative test for iodine.[46]
The interhalogen compounds formed by the halogens are diamagnetic and include XY3 and X7, where X is heavier than Y.Iodine forms all three possible diatomic interhalogens, a trifluoride and trichloride, as well as a pentaFluoride.There are many cationic and anionic derivatives, such as wine-red or bright orange compounds, and dark brown or black compounds.Some pseudohalides, such as ICN, ISCN and IN3 are also known.[47]
Iodine monofluoride is unstable at room temperature and can't be obtained pure.It can be synthesised from the reaction of iodine with fluorine gas in trichlorofluoromethane.Iodine monochloride and IBr are stable.The former, a volatile red-brown compound, was discovered independently by Joseph Louis Gay-Lussac and Humphry Davy, and it mimics the intermediate halogen bromine so well that Justus von Liebig was misled into believing it.Iodine monochloride can be prepared by reacting it with chlorine or bromine at room temperature.Platinum and gold are not the only things that are attacked by both of them.Conditions affect their reaction with organic compounds.The chlorination of phenol and salicyclic acid is caused by the production of chlorine and iodine, which are more reactive.Heterolytic fission of the I–Cl bond occurs and I+ attacks phenol, which results in iodination being the main reaction.The bromine is more reactive than the iodine, so it tends to brominate phenol even in the solution.I2X+ and IX2 anions are significant conductors of electricity and can be used as ionising solvents.[47]
Iodine trifluoride is an unstable yellow solid.It is not well-known.It is difficult to produce because fluorine gas oxidizes all the way to the pentafluoride and reaction at low temperature is necessary.Iodine trichloride is a bright yellow solid, synthesised by reacting with liquid chlorine at 80C, but caution is needed during purification because it easily dissociates to iodine monochloride and chlorine.Liquid iodine trichloride conducts electricity.48
The most stable of all the iodines is Iodine, which can be made by reacting it with fluorine gas at room temperature.It's mild enough to be stored in glass apparatus.The liquid state has a slight electrical conductivity.It reacts with almost all the elements even at low temperatures, and is an extremely powerful fluorinating agent.[49]
The I–O bonds resulting from the large electronegativity difference between iodine and oxygen have been known for the longest time.The stable, white, hygroscopic I2O5 has been known since 1813.It can be made by dehydration of iodic acid and anhydride.It can be used as a reagent in determining the concentration of carbon monoxide.It oxidizes nitrogen oxide, ethylene, and hydrogen sulfide.It reacts with sulfur trioxide and peroxydisulfuryl difluoride to form salts of the iodyl cation.It may be fluorinated by chloryl fluoride, bromine trifluoride, or sulfur dioxide.The structures of I4O9 and I2O4 have not been determined, but reasonable guesses are IIII(IVO3)3 and [IO]+[IO3].50
The four oxoacids are hypoiodous acid (HIO), iodous acid, iodic acid and periodic acid.The following reactions occur when iodine is dissolved in water.
Hypoiodous acid is not stable to disproportionation.The hypoiodite ion formed quickly to give iodide and iodate.
Iodous acid and iodite are only fleeting intermediates in the oxidation of iodide to iodate.Iodates are the most important of these compounds because they can be oxidised with oxygen at 600 C or with chlorates.iodates are stable to disproportionation in both acidic and alkaline solutions.Salts of most metals can be obtained from these.Iodic acid can be made by oxidation of a suspension.Iodate has the weakest oxidising power.[52]
There are many periodates, including the expected IO4 and square-pyramidal IO35.They are usually made by oxidising alkaline sodium iodate with lead and chlorine gas.
They are powerful oxidising agents that can be used quickly and easily.The orthoperiodate has a very high negative charge of 5.H5IO6 is stable and can be dried in a vacuum at 100 C.Attempting to go further does not result in the existence of I2O7.It is possible to give the I(OH)+6 cation, isoelectronic to Te, and Sb, with the help of Periodic acid.[23]
A bright blue paramagnetic solution is formed when iodine is dissolved in strong acids.A solid salt of the diiodine cation can be obtained by oxidising iodine.
The dark blue salt I2Sb2F11 is also known as the blue tantalum analogue.As the missing electron in the latter has been removed from an antibonding orbital, the bond is stronger and therefore shorter.Red rectangular diamagnetic I2+4 can be formed in fluorosulfuric acid solution.The bent dark-brown or black I+3 and centrosymmetric C2h green I+5 are not as well-characterised as other polyiodine cations.There are 23 and 54 words.
Linear triiodide, I3 is the most important polyion in the solution.The formation of this explains why the amount of iodine in the water may be increased.
Many other polyiodides can be found when solutions with large, weakly polarising cations such as Cs+ are isolated.There are 23 and 55 words.
The development of organic synthesis can be traced back to the use of Organoiodine compounds.[59]
The carbon–iodine bond is a functional group that forms part of core organic chemistry and may be thought of as organic derivatives of the iodide anion.The simplest organoiodine compounds, alkyl iodides, may be synthesised by the reaction of alcohols with phosphorus triiodide.The weakest of the carbon–halogen bonds is the C–I bond due to the minuscule difference in electronegativity between carbon and iodine.As such, iodide is the best leaving group among the halogens, to such an extent that many organoiodine compounds turn yellow when stored over time, due to the easy formation and cleavage of the C–.They are denser than the other organohalogen compounds due to the high atomic weight of iodine.2-iodoxybenzoic acid, a common reagent for the oxidation of alcohols to aldehydes, and iodobenzene dichloride are some organic oxidising agents that contain iodine in a higher oxidation state than 1.One of the more well-known uses of organoiodine compounds is the iodoform test, in which a compound capable of being oxidised to a methyl ketone is produced.
One of the drawbacks of using organoiodine compounds is that they are more expensive and have more toxicity than the other compounds.It is possible to prevent the reformation of disulfide linkages with the help of iodoacetic acid.66
It is slightly complicated by the fact that iodide is a better leaving group than bromide or chloride.The difference is small enough that the reaction can be driven to completion by exploiting the differential solubility of halide salts, or by using a large excess of the halide salt.In the classic Finkelstein reaction, an alkyl bromide is converted to a benzyl bromide by treatment with a solution of sodium iodide in acetone.There are some things that are notsoluble in acetone and sodium bromide.Mass action is driven by the precipitation of the insoluble salt.[68]
Iodine is the least abundant of the stable halogens, with only 0.46 parts per million of Earth's crustal rocks.It is 61st in abundance among the 84 elements that occur in significant quantities.Iodide minerals are rare and most deposits are iodate minerals.Lautarite, Ca(IO3)2, and dietzeite are examples.These are the minerals that occur as trace impurities in the caliche, which has the main product being sodium nitrate.They can contain at least 0.05% and at most 1% of the radioactive substance.The iodate is taken from the caliche and reduced to iodide.The solution is reacted with freshly extract iodate, which resulted in comproportionation to iodine.[19]
In the 19th century the caliche was the main source of iodine, but in the 20th it was replaced by brines.The Minami Kanto gas field east of Tokyo is one of the largest sources.From the depth of the source, the brine is hotter than 60 C.The brine is first acidified with sulfuric acid, then it is oxidised with chlorine.The solution must be concentrated.Air is blown into the solution to evaporate the iodine, which is passed into an absorbing tower.The chlorine is used to make the hydrogen iodide.The iodine is packed after purification.71 and 73.
Chile and Japan are the largest producers of the radioactive substance.Alternatively, the brine can be treated with silver nitrate to make a solution of iron and silver.The chlorine may be used to liberate the iodine.[74]
About half of the produced iodine goes into various organoiodine compounds, another 15% remains as the pure element, and the last 15% is used to form potassium iodide.Major uses of iodine compounds include catalysts, animal feed supplements, stabilisers, dyes, colourants and pigments, pharmaceutical, Sanitation, and photography.[19]
Quantitative volumetric analysis is often done using the iodate anions.The blue complex formed by Iodine and starch is often used as an indicator in iodometry.The test is still used to detect counterfeit money.75
The mass of iodine in grams that is consumed by 100 grams of a chemical substance is known as the irium value.Iodine numbers can be used to determine the amount of unsaturation.The double bonds react with the iodine compounds.In biology, linoleic acid, alpha-linolenic, and arachidonic acid are found.There are 76 and 77 words.
K2HgI4 is also known as Nessler's reagent.It is a sensitive spot test for ammonia.Cu2HgI4 is used to test for alkaloids.The iodoform test uses aqueous alkaline iodine solution.[64]
The spectrum of the I2 molecule consists of tens of thousands of lines.It's a commonly used wavelength reference.The hyperfine structure of the iodine molecule is revealed by measuring with a spectroscopic Doppler-free technique while focusing on one of these lines.A line is now resolved so that either 15 or 21 components are measurable.[78]
Cesium and thallium are used in crystal scintillators.The efficiency is high, but the resolution is poor.
There are two ways in which water-soluble triiodide anion I3 can be generated in situ, either as a disinfectant or antisepsis.It is possible to treat iodine deficiency with erbium.[80]
The iodide ion is thought to be the iodophor in triiodide water solutions.There are examples of such preparations.
It works at low concentrations and is used in operating theatres.Its specific mode of action is not known.It causes cell death by attacking specific amino acids, such as cysteine and methionine.It has an anti-viral action, but parvoviruses and nonlipid viruses are less sensitive.Iodine attacks the surface of the viruses and may also destabilise them by reacting with carbon bonds.[83]
Acute thyrotoxicosis can be treated with a saturated solution of potassium iodide.When iobenguane is used as part of radiopharmaceuticals that are not targeted to the thyroid or thyroid-type tissues, it is also used to block the absorption of iodine-131.It was 83 and 84.
Iodine-131 is a component of nuclear fallout and is particularly dangerous due to the tendency of the thyroid to retain it for periods longer than the radioactive half-life of eight days.There is a chance that people at risk of exposure to environmental radioactive iodine may be told to take non-radioactive tablets.The typical adult dose is 130 tablets per 24 hours.The typical daily dose of iodine for normal health is 100 micrograms.The large dose of non-radioactive iodine reduces the amount of radioactive iodine in the body.[85]
As an element with high electron density and atomic number, it absorbs X-rays that are weaker than 33.3 keV due to the photoelectric effect of the innermost electrons.X-ray radiocontrast agents are injected with Organoiodine compounds.This application is often used with advanced X-ray techniques.All water-soluble radiocontrast agents rely on iodine.
The production of ethylenediamine dihydroiodide is used as a supplement for livestock.acetic acid can be produced by the Monsanto and Cativa processes.The world's demand for acetic acid is supported by the use of hydroiodic acid in these technologies.hydroiodic acid and acetic acid can be regenerated by hydrolysis.[87]
Inorganic iodides are used in different ways.The van Arkel process is used to purify titanium, zirconium, hafnium, and thorium.A lot of traditional photographic film is made with silver iodide.Cloud seeding uses thousands of kilograms of silver iodide each year.[87]
erythrosine is an important food coloring agent.Perfluoroalkyl iodides are used to make perfluorooctanesulfonic acid.[87]
A popular educational demonstration experiment and example of a seemingly oscillating reaction is the iodine clock reaction, in which iodine also serves as a test for starch, forming a dark blue complex.
In an agricultural system, agents containing it can exert a differential effect on different species.At concentrations that do not harm the crop, the growth of all strains of Fusarium verticillioides is greatly reduced.The natural chemistry of this treatment might make it less toxic.[88]
Iodine is an essential element for life and, at atomic number Z, is the heaviest element commonly needed by living organisms.Lanthanum and the other lanthanides are used by some organisms.T4 and T3 are growth-regulating hormones named after their number of iodine atoms.Simple goitre is caused by a deficiency of iodine that leads to decreased production of T3 and T4 and an attempt to get more of the radioactive substance.T4 has a longer half-life than T3 and is the major form of thyroid hormone in the blood.Humans have a ratio of T4 to T3 in their blood.The active T3 is three to four times more potent than the inactive T4 within cells.Decarboxylation and deiodination are used to produce iodothyronamine and T0a'.T3 production is dependent on the selenium content of the deiodinases.92
Sixty-five percent of the weight of T4 and T3 is Iodine.70% of the total amount of iodine in the body is found in other tissues, including mammary glands, eyes, gastric mucosa, fetal thymus, cerebro-spinal fluid and choroid plexus.The cells of those tissues contain iodide.Fetal and neonatal development are related to the action of iodine in mammary tissue.93
The United States Institute of Medicine recommends between 120 and 130 g for infants up to 12 months, 90 to 120 for children between eight and eight years, 130 to 150 for adults, and 220 for pregnant women.The Tolerable Upper Intake Level for adults is 1,100 g/day.The upper limit was assessed by analyzing the effect of supplementation.93
The required daily amounts of T4 and T3 are 70 g/day.The higher recommended daily allowance levels of iodine seem necessary for optimal function of a number of body systems.96 and 77 were the days.
seafood, seaweeds, dairy products, eggs, and plants grown on soil with high levels of iodine are all natural sources of dietary iodine.Iodised salt is fortified with a radioactive substance.99 to 100
In 2000, the median intake of Iodide from food in the United States was between 200 and 300 g/day for men and between 190 and 200 for women.The general US population has adequate iodine nutrition, with women of childbearing age and pregnant women having a slight risk of deficiency.Kombu Umami extracts were often used for soup stock and potato chips in Japan.Japan's consumption is closer to 1,000–3,000 g/day, according to new studies.The adultUL in Japan was last revised to 3000 g/day in 2015.104
Some cases of hyperthyroidism have been observed after the implementation of iodisation of salt.The risk of the condition appears to be higher in people over forty when the initial rise in iodine intake is high.105
Extreme fatigue, mental slowing, depression, weight gain, and low moods are some of the symptoms of hypothyroidism in areas where there is little iodine in the diet.When babies or small children are rendered hypothyroidic by a lack of the element, it is the leading cause of preventable intellectual disability.In wealthier nations, the problem of iodine deficiency has been eliminated thanks to the addition of table salt, but it is still a serious problem in the developing world.Iodine deficiency is a problem in Europe.Information processing, fine motor skills, and visual problem solving can be improved by iodine repletion.[109]
If you take I2 orally, it is toxic.The lethal dose for an adult human is 30 percent of their body weight, which is about 2.3 grams for a human weighing 70 to 80 kilograms.In the presence of selenium deficiency, excess iodine can be more harmful.In theory, it's problematic to give iodine to people who don't have enough of it.The toxicity derives from its oxidizing properties.[113]