Iodine - wikipedia Iodine This is the latest accepted revision, reviewed on 8 January 2018. This article is about the chemical element. For other uses, see Iodine ( disambiguation ). Iodine, I General properties Pronunciation / ˈaɪ. ədaɪn / ​ ( EYE - ə - dyne ), or / ˈaɪ. ədɪn / ​ ( EYE - ə - din ), or / ˈaɪ. ədiːn / ​ ( EYE - ə - deen ) Appearance lustrous metallic gray, violet as a gas Standard atomic weight ( A ) 7002126904470000000 ♠ 126.904 47 ( 3 ) Iodine in the periodic table Hydrogen Helium Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury ( element ) Thallium Lead Bismuth Polonium Astatine Radon Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson Br ↑ ↓ At tellurium ← iodine → xenon Atomic number ( Z ) 53 Group, period group 17 ( halogens ), period 5 Block p - block Element category diatomic nonmetal Electron configuration ( Kr ) 4d 5s 5p Electrons per shell 2, 8, 18, 18, 7 Physical properties Phase ( at STP ) solid Melting point 386.85 K ​ ( 113.7 ° C, ​ 236.66 ° F ) Boiling point 457.4 K ​ ( 184.3 ° C, ​ 363.7 ° F ) Density ( near r.t. ) 4.933 g / cm Triple point 386.65 K, ​ 12.1 kPa Critical point 819 K, 11.7 MPa Heat of fusion ( I ) 15.52 kJ / mol Heat of vaporisation ( I ) 41.57 kJ / mol Molar heat capacity ( I ) 54.44 J / ( mol K ) Vapour pressure ( rhombic ) P ( Pa ) 10 100 1 k 10 k 100 k at T ( K ) 260 282 309 342 381 457 Atomic properties Oxidation states 7, 6, 5, 4, 3, 1, − 1 ​ ( a strongly acidic oxide ) Electronegativity Pauling scale : 2.66 Ionisation energies 1st : 1008.4 kJ / mol 2nd : 1845.9 kJ / mol 3rd : 3180 kJ / mol Atomic radius empirical : 140 pm Covalent radius 139 ± 3 pm Van der Waals radius 198 pm Spectral lines Miscellanea Crystal structure ​ orthorhombic Thermal conductivity 0.449 W / ( m K ) Electrical resistivity 1.3 × 10 Ω m ( at 0 ° C ) Magnetic ordering diamagnetic Magnetic susceptibility − 88.7 10 cm / mol ( 298 K ) Bulk modulus 7.7 GPa CAS Number 7553 - 56 - 2 History Discovery and first isolation Bernard Courtois ( 1811 ) Main isotopes of iodine Isotope Abundance Half - life ( t ) Decay mode Product syn 13 h ε, γ Te syn 4.176 d ε Te syn 59.40 d ε Te 100 % stable trace 1.57 × 10 y β Xe syn 8.02070 d β, γ Xe syn 6.57 h β Xe view talk references in Wikidata Iodine is a chemical element with symbol I and atomic number 53. The heaviest of the stable halogens, it exists as a lustrous, purple - black metallic solid at standard conditions that sublimes readily to form a violet gas. The elemental form was discovered by the French chemist Bernard Courtois in 1811. It was named two years later by Joseph - Louis Gay - Lussac from this property, after the Greek ἰωδης `` violet - coloured ''. Iodine occurs in many oxidation states, including iodide ( I ), iodate ( IO − 3 ), and the various periodate anions. It is the least abundant of the stable halogens, being the sixty - first most abundant element. It is even less abundant than the so - called rare earths. It is the heaviest essential mineral nutrient. Iodine is essential in the synthesis of thyroid hormones. Iodine deficiency affects about two billion people and is the leading preventable cause of intellectual disabilities. The dominant producers of iodine today are Chile and Japan. Iodine and its compounds are primarily used in nutrition. Due to its high atomic number and ease of attachment to organic compounds, it has also found favour as a non-toxic radiocontrast material. Because of the specificity of its uptake by the human body, radioactive isotopes of iodine can also be used to treat thyroid cancer. Iodine is also used as a catalyst in the industrial production of acetic acid and some polymers. Contents 1 History 2 Properties 2.1 Isotopes 3 Chemistry and compounds 3.1 Hydrogen iodide 3.2 Other binary iodides 3.3 Iodine halides 3.4 Iodine oxides and oxoacids 3.5 Polyiodine compounds 3.6 Organoiodine compounds 4 Occurrence and production 5 Applications 5.1 Analysis 5.2 Medicine 5.2. 1 Elemental iodine 5.2. 2 Other formulations 5.3 Others 6 Biological role 6.1 Dietary intake 6.2 Deficiency 7 Toxicity 7.1 Occupational exposure 7.2 Allergic reactions 8 References 9 Bibliography History In 1811, iodine was discovered by French chemist Bernard Courtois, who was born to a manufacturer of saltpeter ( an essential component of gunpowder ). At the time of the Napoleonic Wars, saltpeter was in great demand in France. Saltpeter produced from French nitre beds required sodium carbonate, which could be isolated from seaweed collected on the coasts of Normandy and Brittany. To isolate the sodium carbonate, seaweed was burned and the ash washed with water. The remaining waste was destroyed by adding sulfuric acid. Courtois once added excessive sulfuric acid and a cloud of purple vapour rose. He noted that the vapour crystallised on cold surfaces, making dark crystals. Courtois suspected that this material was a new element but lacked funding to pursue it further. Courtois gave samples to his friends, Charles Bernard Desormes ( 1777 -- 1838 ) and Nicolas Clément ( 1779 -- 1841 ), to continue research. He also gave some of the substance to chemist Joseph Louis Gay - Lussac ( 1778 -- 1850 ), and to physicist André - Marie Ampère ( 1775 -- 1836 ). On 29 November 1813, Desormes and Clément made Courtois ' discovery public. They described the substance to a meeting of the Imperial Institute of France. On 6 December, Gay - Lussac announced that the new substance was either an element or a compound of oxygen. It was Gay - Lussac who suggested the name `` iode '', from the Greek word ἰοειδής ( ioeidēs ) for violet ( because of the colour of iodine vapor ). Ampère had given some of his sample to English chemist Humphry Davy ( 1778 -- 1829 ), who experimented on the substance and noted its similarity to chlorine. Davy sent a letter dated 10 December to the Royal Society of London stating that he had identified a new element. Arguments erupted between Davy and Gay - Lussac over who identified iodine first, but both scientists acknowledged Courtois as the first to isolate the element. Properties Violet iodine vapour in a round - bottomed flask Iodine is the fourth halogen, being a member of group 17 in the periodic table, below fluorine, chlorine, and bromine ; it is the heaviest stable member of its group. ( The scarce and fugitive fifth halogen, the radioactive astatine, is not well - studied due to its expense and inaccessibility in large quantities, but appears to show various unusual properties due to relativistic effects. ) Iodine has an electron configuration of ( Kr ) 4d 5s 5p, with the seven electrons in the fifth and outermost shell being its valence electrons. Like the other halogens, it is one electron short of a full octet and is hence a strong oxidising agent, reacting with many elements in order to complete its outer shell, although in keeping with periodic trends, it is the weakest oxidising agent among the stable halogens : it has the lowest electronegativity among them, just 2.66 on the Pauling scale ( compare fluorine, chlorine, and bromine at 3.98, 3.16, and 2.96 respectively ; astatine continues the trend with an electronegativity of 2.2 ). Elemental iodine hence forms diatomic molecules with chemical formula I, where two iodine atoms share a pair of electrons in order to each achieve a stable octet for themselves ; at high temperatures, these diatomic molecules reversibly dissociate a pair of iodine atoms. Similarly, the iodide anion, I, is the strongest reducing agent among the stable halogens, being the most easily oxidised back to diatomic I. ( Astatine goes further, being indeed unstable as At and readily oxidised to At or At, although the existence of At is not settled. ) The halogens darken in colour as the group is descended : fluorine is a very pale yellow gas, chlorine is greenish - yellow, and bromine is a reddish - brown volatile liquid. Iodine conforms to the prevailing trend, being a shiny black crystalline solid that melts at 114 ° C and boils at 183 ° C to form a violet gas. 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 ). Specifically, the violet colour of iodine gas results from the electron transition between the highest occupied antibonding π molecular orbital and the lowest vacant antibonding σ molecular orbital. Elemental iodine is slightly soluble in water, with one gram dissolving in 3450 ml at 20 ° C and 1280 ml at 50 ° C ; potassium iodide may be added to increase solubility via formation of triiodide ions, among other polyiodides. Nonpolar solvents such as hexane and carbon tetrachloride provide a higher solubility. Polar solutions, such as aqueous solutions, are brown, reflecting the role of these solvents as Lewis bases ; on the other hand, nonpolar solutions are violet, the color of iodine vapour. Charge - transfer complexes form when iodine is dissolved in polar solvents, hence changing the colour. Iodine is violet when dissolved in carbon tetrachloride and saturated hydrocarbons but deep brown in alcohols and amines, solvents that form charge - transfer adducts. I PPh charge - transfer complexes in CH Cl. From left to right : ( 1 ) I dissolved in dichloromethane - no CT complex. ( 2 ) A few seconds after excess PPh was added - CT complex is forming. ( 3 ) One minute later after excess PPh was added, the CT complex ( Ph PI ) I has been formed. ( 4 ) Immediately after excess I was added, which contains ( Ph PI ) ( I ). The melting and boiling points of iodine are the highest among the halogens, conforming to the increasing trend down the group, since iodine has the largest electron cloud among them that is the most easily polarised, resulting in its molecules having the strongest van der Waals interactions among the halogens. Similarly, iodine is the least volatile of the halogens. Because it has the largest atomic radius among the halogens, iodine has the lowest first ionisation energy, lowest electron affinity, lowest electronegativity and lowest reactivity of the halogens. Structure of solid iodine The interhalogen bond in diiodine is the weakest of all the halogens. As such, 1 % of a sample of gaseous iodine at atmospheric pressure is dissociated into iodine atoms at 575 ° C. Temperatures greater than 750 ° C are required for fluorine, chlorine, and bromine to dissociate to a similar extent. Most bonds to iodine are weaker than the analogous bonds to the lighter halogens. Gaseous iodine is composed of I molecules with an I -- I bond length of 266.6 pm. The I -- I bond is one of the longest single bonds known. It is even longer ( 271.5 pm ) in solid orthorhombic crystalline iodine, which has the same crystal structure as chlorine and bromine. ( The record is held by iodine 's neighbour xenon : the Xe -- Xe bond length is 308.71 pm. ) As such, within the iodine molecule, significant electronic interactions occur with the two next - nearest neighbours of each atom, and these interactions give rise, in bulk iodine, to a shiny appearance and semiconducting properties. Iodine is a two - dimensional semiconductor with a band gap of 1.3 eV ( 125 kJ / mol ) : it is a semiconductor in the plane of its crystalline layers and an insulator in the perpendicular direction. Isotopes Main article : Isotopes of iodine Of the thirty - seven known isotopes of iodine, only one occurs in nature, iodine - 127. The others are radioactive and have half - lives too short to be primordial. As such, iodine is monoisotopic and its atomic weight is known to great precision, as it is a constant of nature. The longest - lived of the radioactive isotopes of iodine is iodine - 129, which has a half - life of 15.7 million years, decaying via beta decay to stable xenon - 129. Some iodine - 129 was formed along with iodine - 127 before the formation of the Solar System, but it has by now completely decayed away, making it an extinct radionuclide that is nevertheless still useful in dating the history of the early Solar System or very old groundwaters, due to its mobility in the environment. Its former presence may be determined from an excess of its daughter xenon - 129. Traces of iodine - 129 still exist today, as it is also a cosmogenic nuclide, formed from cosmic ray spallation of atmospheric xenon : these traces make up 10 to 10 of all terrestrial iodine. It also occurs from open - air nuclear testing, and is not hazardous because of its incredibly long half - life, the longest of all fission products. At the peak of thermonuclear testing in the 1960s and 1970s, iodine - 129 still made up only about 10 of all terrestrial iodine. Excited states of iodine - 127 and iodine - 129 are often used in Mössbauer spectroscopy. The other iodine radioisotopes have much shorter half - lives, no longer than days. Some of them have medical applications involving the thyroid gland, where the iodine that enters the body is stored and concentrated. Iodine - 123 has a half - life of thirteen hours and decays by electron capture to tellurium - 123, emitting gamma radiation ; it is used in nuclear medicine imaging, including single photon emission computed tomography ( SPECT ) and X-ray computed tomography ( X-Ray CT ) scans. Iodine - 125 has a half - life of fifty - nine days, decaying by electron capture to tellurium - 125 and emitting low - energy gamma radiation ; the second - longest - lived iodine radioisotope, it has uses in biological assays, nuclear medicine imaging and in radiation therapy as brachytherapy to treat a number of conditions, including prostate cancer, uveal melanomas, and brain tumours. Finally, iodine - 131, 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 gamma radiation. It is a common fission product and thus is present in high levels in radioactive fallout. It may then be absorbed through contaminated food, and will also accumulate in the thyroid. As it decays, it may cause damage to the thyroid. The primary risk from exposure to high levels of iodine - 131 is the chance occurrence of radiogenic thyroid cancer in later life. Other risks include the possibility of non-cancerous growths and thyroiditis. The usual means of protection against the negative effects of iodine - 131 is by saturating the thyroid gland with stable iodine - 127 in the form of potassium iodide tablets, taken daily for optimal prophylaxis. However, iodine - 131 may also be used for medicinal purposes in radiation therapy for this very reason, when tissue destruction is desired after iodine uptake by the tissue. Iodine - 131 is also used as a radioactive tracer. Chemistry and compounds Halogen bond energies ( kJ / mol ) X XX HX BX AlX CX 159 574 645 582 456 Cl 243 428 444 427 327 Br 193 363 368 360 272 151 294 272 285 239 Though it is the least reactive of the halogens, iodine is still one of the more reactive elements. For example, while chlorine gas will halogenate carbon monoxide, nitrogen monoxide, and sulfur dioxide to phosgene, nitrosyl chloride, and sulfuryl chloride respectively, iodine will not do so. Furthermore, 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 only rhenium pentabromide and iodine can achieve only rhenium tetraiodide. By the same token, however, 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 rather more stable than those of bromine and chlorine, for example in iodine heptafluoride. Hydrogen iodide The simplest compound of iodine is hydrogen iodide, HI. It is a colourless gas that reacts with oxygen to give water and iodine. Although it is useful in iodination reactions in the laboratory, it does not have large - scale industrial uses, unlike the other hydrogen halides. Commercially, it is usually made by reacting iodine with hydrogen sulfide or hydrazine : 2 I + N H H O ⟶ 4 HI + N At room temperature, it is a colourless gas, like all of the hydrogen halides except hydrogen fluoride, since hydrogen can not form strong hydrogen bonds to the large and only mildly electronegative iodine atom. It melts at − 51.0 ° C and boils at − 35.1 ° C. It is an endothermic compound that can exothermically dissociate at room temperature, although the process is very slow unless a catalyst is present : the reaction between hydrogen and iodine at room temperature to give hydrogen iodide does not proceed to completion. The H -- I bond dissociation energy is likewise the smallest of the hydrogen halides, at 295 kJ / mol. Aqueous hydrogen iodide is known as hydroiodic acid, which is a strong acid. Hydrogen iodide is exceptionally soluble in water : one litre of water will dissolve 425 litres of hydrogen iodide, and the saturated solution has only four water molecules per molecule of hydrogen iodide. Commercial so - called `` concentrated '' hydroiodic acid usually contains 48 -- 57 % HI by mass ; the solution forms an azeotrope with boiling point 126.7 ° C at 56.7 g HI per 100 g solution. Hence hydroiodic acid can not be concentrated past this point by evaporation of water. Unlike hydrogen fluoride, anhydrous liquid hydrogen iodide is difficult to work with as a solvent, because its boiling point is low, it has a small liquid range, its dielectric constant is low and it does not dissociate appreciably into H I and HI − 2 ions -- the latter, in any case, are much less stable than the bifluoride ions ( HF − 2 ) due to the very weak hydrogen bonding between hydrogen and iodine, though its salts with very large and weakly polarising cations such as Cs and NR + 4 ( R = Me, Et, Bu ) may still be isolated. Anhydrous hydrogen iodide is a poor solvent, able to dissolve only small molecular compounds such as nitrosyl chloride and phenol, or salts with very low lattice energies such as tetraalkylammonium halides. Other binary iodides Nearly all elements in the periodic table form binary iodides. The exceptions are decidedly in the minority and stem in each case from one of three causes : extreme inertness and reluctance to participate in chemical reactions ( the noble gases ) ; extreme nuclear instability hampering chemical investigation before decay and transmutation ( many of the heaviest elements beyond bismuth ) ; and having an electronegativity higher than iodine 's ( oxygen and the first three halogens ), so that the resultant binary compounds are formally not iodides but rather oxides or halides of iodine. Given the large size of the iodide anion and iodine 's weak oxidising power, high oxidation states are difficult to achieve in binary iodides, the maximum known being in the pentaiodides of niobium, tantalum, and protactinium. Iodides can be made by reaction of an element or its oxide, hydroxide, or carbonate with hydroiodic acid, and then dehydrated by mildly high temperatures combined with either low pressure or anhydrous hydrogen iodide gas. These methods work best when the iodide product is stable to hydrolysis ; otherwise, the possibilities include high - temperature oxidative iodination of the element with iodine or hydrogen iodide, high - temperature iodination of a metal oxide or other halide by iodine, a volatile metal halide, carbon tetraiodide, or an organic iodide. For example, molybdenum ( IV ) oxide reacts with aluminium ( III ) iodide at 230 ° C to give molybdenum ( II ) iodide. An example involving halogen exchange is given below, involving the reaction of tantalum ( V ) chloride with excess aluminium ( III ) iodide at 400 ° C to give tantalum ( V ) iodide : 3 TaCl 5 + 5 AlI 3 ( excess ) ⟶ 3 TaI 5 + 5 AlCl 3 ( displaystyle ( ce ( ( 3TaCl5 ) + ( \underset ( ( excess ) ) ( 5AlI3 ) ) - > ( 3TaI5 ) + 5AlCl3 ) ) ) Lower iodides may be produced either through thermal decomposition or disproportionation, or by reducing the higher iodide with hydrogen or a metal, for example : TaI 5 + Ta → 630 ∘ C ⟶ 575 ∘ C thermal gradient Ta 6 I 14 ( displaystyle ( ce ( ( TaI5 ) + Ta - > ( ( \text ( thermal gradient ) ) ) ( ( ce ( 630 ^ ( circ ) C - > 575 ^ ( circ ) C ) ) ) Ta6I14 ) ) ) Most of the iodides of the pre-transition metals ( groups 1, 2, and 3, along with the lanthanides and actinides in the + 2 and + 3 oxidation states ) are mostly ionic, while nonmetals tend to form covalent molecular iodides, as do metals in high oxidation states from + 3 and above. Ionic iodides MI tend to have the lowest melting and boiling points among the halides MX of the same element, because the electrostatic forces of attraction between the cations and anions are weakest for the large iodide anion. In contrast, covalent iodides tend to instead have the highest melting and boiling points among the halides of the same element, since iodine is the most polarisable of the halogens and, having the most electrons among them, can contribute the most to van der Waals forces. Naturally, exceptions abound in intermediate iodides where one trend gives way to the other. Similarly, solubilities in water of predominantly ionic iodides ( e.g. potassium and calcium ) are the greatest among ionic halides of that element, while those of covalent iodides ( e.g. silver ) are the lowest of that element. In particular, silver iodide is very insoluble in water and its formation is often used as a qualitative test for iodine. Iodine halides The halogens form many binary, diamagnetic interhalogen compounds with stoichiometries XY, XY, XY, and XY ( where X is heavier than Y ), and iodine is no exception. Iodine forms all three possible diatomic interhalogens, a trifluoride and trichloride, as well as a pentafluoride and, exceptionally among the halogens, a heptafluoride. Numerous cationic and anionic derivatives are also characterised, such as the wine - red or bright orange compounds of ICl + 2 and the dark brown or purplish black compounds of I Cl. Apart from these, some pseudohalides are also known, such as cyanogen iodide ( ICN ), iodine thiocyanate ( ISCN ), and iodine azide ( IN ). Iodine monochloride Iodine monofluoride ( IF ) is unstable at room temperature and disproportionates very readily and irreversibly to iodine and iodine pentafluoride, and thus can not be obtained pure. It can be synthesised from the reaction of iodine with fluorine gas in trichlorofluoromethane at − 45 ° C, with iodine trifluoride in trichlorofluoromethane at − 78 ° C, or with silver ( I ) fluoride at 0 ° C. Iodine monochloride ( ICl ) and iodine monobromide ( IBr ), on the other hand, are moderately stable. The former, a volatile red - brown compound, was discovered independently by Joseph Louis Gay - Lussac and Humphry Davy in 1813 -- 4 not long after the discoveries of chlorine and iodine, and it mimics the intermediate halogen bromine so well that Justus von Liebig was misled into mistaking bromine ( which he had found ) for iodine monochloride. Iodine monochloride and iodine monobromide may be prepared simply by reacting iodine with chlorine or bromine at room temperature and purified by fractional crystallisation. Both are quite reactive and attack even platinum and gold, though not boron, carbon, cadmium, lead, zirconium, niobium, molybdenum, and tungsten. Their reaction with organic compounds depends on conditions. Iodine chloride vapour tends to chlorinate phenol and salicyclic acid, since when iodine chloride undergoes homolytic dissociation, chlorine and iodine are produced and the former is more reactive. However, iodine chloride in tetrachloromethane solution results in iodination being the main reaction, since now heterolytic fission of the I -- Cl bond occurs and I attacks phenol as an electrophile. However, iodine monobromide tends to brominate phenol even in tetrachloromethane solution because it tends to dissociate into its elements in solution, and bromine is more reactive than iodine. When liquid, iodine monochloride and iodine monobromide dissociate into I 2X + and IX − 2 anions ( X = Cl, Br ) ; thus they are significant conductors of electricity and can be used as ionising solvents. Iodine trifluoride ( IF ) is an unstable yellow solid that decomposes above − 28 ° C. It is thus little - known. It is difficult to produce because fluorine gas would tend to oxidise iodine all the way to the pentafluoride ; reaction at low temperature with xenon difluoride is necessary. Iodine trichloride, which exists in the solid state as the planar dimer I Cl, is a bright yellow solid, synthesised by reacting iodine with liquid chlorine at − 80 ° C ; caution is necessary during purification because it easily dissociates to iodine monochloride and chlorine and hence can act as a strong chlorinating agent. Liquid iodine trichloride conducts electricity, possibly indicating dissociation to ICl + 2 and ICl − 4 ions. Iodine pentafluoride ( IF ), a colourless, volatile liquid, is the most thermodynamically stable iodine fluoride, and can be made by reacting iodine with fluorine gas at room temperature. It is a fluorinating agent, but is mild enough to store in glass apparatus. Again, slight electrical conductivity is present in the liquid state because of dissociation to IF + 4 and IF − 6. The pentagonal bipyramidal iodine heptafluoride ( IF ) is an extremely powerful fluorinating agent, behind only chlorine trifluoride, chlorine pentafluoride, and bromine pentafluoride among the interhalogens : it reacts with almost all the elements even at low temperatures, fluorinates Pyrex glass to form iodine ( VII ) oxyfluoride ( IOF ), and sets carbon monoxide on fire. Iodine oxides and oxoacids Structure of iodine pentoxide Iodine oxides are the most stable of all the halogen oxides, because of the strong I -- O bonds resulting from the large electronegativity difference between iodine and oxygen, and they have been known for the longest time. The stable, white, hygroscopic iodine pentoxide ( I O ) has been known since its formation in 1813 by Gay - Lussac and Davy. It is most easily made by the dehydration of iodic acid ( HIO ), which it is the anhydride of. It will quickly oxidise carbon monoxide completely to carbon dioxide at room temperature, and is thus a useful reagent in determining carbon monoxide concentration. It also oxidises nitrogen oxide, ethylene, and hydrogen sulfide. It reacts with sulfur trioxide and peroxydisulfuryl difluoride ( S O F ) to form salts of the iodyl cation, ( IO ), and is reduced by concentrated sulfuric acids to iodosyl salts involving ( IO ). It may be fluorinated by fluorine, bromine trifluoride, sulfur tetrafluoride, or chloryl fluoride, resulting iodine pentafluoride, which also reacts with iodine pentoxide, giving iodine ( V ) oxyfluoride, IOF. A few other less stable oxides are known, notably I O and I O ; their structures have not been determined, but reasonable guesses are I ( I O ) and ( IO ) ( IO ) respectively. Standard reduction potentials for aqueous I species E ° ( couple ) a ( H ) = 1 ( acid ) E ° ( couple ) a ( OH ) = 1 ( base ) I / I + 0.535 I / I + 0.535 HOI / I + 0.987 IO / I + 0.48 IO − 3 / I + 0.26 HOI / I + 1.439 IO / I + 0.42 IO − 3 / I + 1.195 IO − 3 / HOI + 1.134 IO − 3 / IO + 0.15 IO − 4 / IO − + 1.653 H IO / IO − + 1.601 3IO2 − 6 / IO − + 0.65 More important are the four oxoacids : hypoiodous acid ( HIO ), iodous acid ( HIO ), iodic acid ( HIO ), and periodic acid ( HIO or H IO ). When iodine dissolves in aqueous solution, the following reactions occur : I + H O ⇌ HIO + H + I K = 2.0 × 10 mol l I + 2 OH ⇌ IO + H O + I K = 30 mol l Hypoiodous acid is unstable to disproportionation. The hypoiodite ions thus formed disproportionate immediately to give iodide and iodate : 3 IO ⇌ 2 I + IO − K = 10 Iodous acid and iodite are even less stable and exist only as a fleeting intermediate in the oxidation of iodide to iodate, if at all. Iodates are by far the most important of these compounds, which can be made by oxidising alkali metal iodides with oxygen at 600 ° C and high pressure, or by oxidising iodine with chlorates. Unlike chlorates, which disproportionate very slowly to form chloride and perchlorate, iodates are stable to disproportionation in both acidic and alkaline solutions. From these, salts of most metals can be obtained. Iodic acid is most easily made by oxidation of an aqueous iodine suspension by electrolysis or fuming nitric acid. Iodate has the weakest oxidising power of the halates, but reacts the quickest. Many periodates are known, including not only the expected tetrahedral IO − 4, but also square - pyramidal IO 3 − 5, octahedral orthoperiodate IO 5 − 6, ( IO ( OH ) ), ( I O ( OH ) ), and I 2O4 − 9. They are usually made by oxidising alkaline sodium iodate electrochemically ( with lead ( IV ) oxide as the anode ) or by chlorine gas : IO − 3 + 6 OH → IO 5 − 6 + 3 H O + 2 e IO − 3 + 6 OH + Cl → IO 5 − 6 + 2 Cl + 3 H O They are thermodymically and kinetically powerful oxidising agents, quickly oxidising Mn to MnO − 4, and cleaving glycols, α - diketones, α - ketols, α - aminoalcohols, and α - diamines. Orthoperiodate especially stabilises high oxidation states among metals because of its very high negative charge of − 5. Orthoperiodic acid, H IO, is stable, and dehydrates at 100 ° C in a vacuum to metaperiodic acid, HIO. Attempting to go further does not result in the nonexistent iodine heptoxide ( I O ), but rather iodine pentoxide and oxygen. Periodic acid may be protonated by sulfuric acid to give the I ( OH ) + 6 cation, isoelectronic to Te ( OH ) and Sb ( OH ) − 6, and giving salts with bisulfate and sulfate. Polyiodine compounds When iodine dissolves in strong acids, such as fuming sulfuric acid, a bright blue paramagnetic solution including I + 2 cations is formed. A solid salt of the diiodine cation may be obtained by oxidising iodine with antimony pentafluoride : 2 I + 5 SbF SO ⟶ 20 ° C 2 I Sb F + SbF The salt I Sb F is dark blue, and the blue tantalum analogue I Ta F is also known. Whereas the I -- I bond length in I is 267 pm, that in I + 2 is only 256 pm as the missing electron in the latter has been removed from an antibonding orbital, making the bond stronger and hence shorter. In fluorosulfuric acid solution, deep - blue I + 2 reversibly dimerises below − 60 ° C, forming red rectangular diamagnetic I2 + 4. Other polyiodine cations are not as well - characterised, including bent dark - brown or black I + 3 and centrosymmetric C green or black I + 5, known in the AsF − 6 and AlCl − 4 salts among others. The only important polyiodide anion in aqueous solution is linear triiodide, I − 3. Its formation explains why the solubility of iodine in water may be increased by the addition of potassium iodide solution : I + I ⇌ I − 3 ( K = ~ 700 at 20 ° C ) Many other polyiodides may be found when solutions containing iodine and iodide crystallise, such as I − 5, I − 9, I2 − 4, and I2 − 8, whose salts with large, weakly polarising cations such as Cs may be isolated. Organoiodine compounds Main article : Organoiodine compound Structure of the oxidising agent 2 - iodoxybenzoic acid Organoiodine compounds have been fundamental in the development of organic synthesis, such as in the Hofmann elimination of amines, the Williamson ether synthesis, the Wurtz coupling reaction, and in Grignard reagents. The carbon -- iodine bond is a common functional group that forms part of core organic chemistry ; formally, these compounds 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 ; these may then be used in nucleophilic substitution reactions, or for preparing Grignard reagents. The C -- I bond is the weakest of all the carbon -- halogen bonds due to the minuscule difference in electronegativity between carbon ( 2.55 ) and iodine ( 2.66 ). 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 decomposition into elemental iodine ; as such, they are commonly used in organic synthesis, because of the easy formation and cleavage of the C -- I bond. They are also significantly denser than the other organohalogen compounds thanks to the high atomic weight of iodine. A few organic oxidising agents like the iodanes contain iodine in a higher oxidation state than − 1, such as 2 - iodoxybenzoic acid, a common reagent for the oxidation of alcohols to aldehydes, and iodobenzene dichloride ( PhICl ), used for the selective chlorination of alkenes and alkynes. One of the more well - known uses of organoiodine compounds is the so - called iodoform test, where iodoform ( CHI ) is produced by the exhaustive iodination of a methyl ketone ( or another compound capable of being oxidised to a methyl ketone ), as follows : Some drawbacks of using organoiodine compounds as compared to organochlorine or organobromine compounds is the greater expense and toxicity of the iodine derivatives, since iodine is expensive and organoiodine compounds are stronger alkylating agents. For example, iodoacetamide and iodoacetic acid denature proteins by irreversibly alkylating cysteine residues and preventing the reformation of disulfide linkages. Halogen exchange to produce iodoalkanes by the Finkelstein reaction is slightly complicated by the fact that iodide is a better leaving group than chloride or bromide. The difference is nevertheless 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 chloride or an alkyl bromide is converted to an alkyl iodide by treatment with a solution of sodium iodide in acetone. Sodium iodide is soluble in acetone and sodium chloride and sodium bromide are not. The reaction is driven toward products by mass action due to the precipitation of the insoluble salt. Occurrence and production Iodine is the least abundant of the stable halogens, comprising only 0.46 parts per million of Earth 's crustal rocks ( compare : fluorine 544 ppm, chlorine 126 ppm, bromine 2.5 ppm ). Among the eighty - four elements which occur in significant quantities ( elements 1 -- 42, 44 -- 60, 62 -- 83, and 90 -- 92 ), it ranks sixty - first in abundance. Iodide minerals are rare, and most deposits that are concentrated enough for economical extraction are iodate minerals instead. Examples include lautarite, Ca ( IO ), and dietzeite, 7Ca ( IO ) 8CaCrO. These are the minerals that occur as trace impurities in the caliche, found in Chile, whose main product is sodium nitrate. In total, they can contain at least 0.02 % and at most 1 % iodine by weight. Sodium iodate is extracted from the caliche and reduced to iodide by sodium bisulfite. This solution is then reacted with freshly extracted iodate, resulting in comproportionation to iodine, which may be filtered off. The caliche was the main source of iodine in the 19th century and continues to be important today, replacing kelp ( which is no longer an economically viable source ), but in the late 20th century brines emerged as a comparable source. The Japanese Minami Kanto gas field east of Tokyo and the American Anadarko Basin gas field in northwest Oklahoma are the two largest such sources. The brine is hotter than 60 ° C from the depth of the source. The brine is first purified and acidified using sulfuric acid, then the iodide present is oxidised to iodine with chlorine. An iodine solution is produced, but is dilute and must be concentrated. Air is blown into the solution to evaporate the iodine, which is passed into an absorbing tower where sulfur dioxide reduces the iodine. The hydrogen iodide ( HI ) is reacted with chlorine to precipitate the iodine. After filtering and purification the iodine is packed. 2 HI + Cl → I ↑ + 2 HCl I + 2 H O + SO → 2 HI + H SO 2 HI + Cl → I ↓ + 2 HCl These sources ensure that Chile and Japan are the largest producers of iodine today. Alternatively, the brine may be treated with silver nitrate to precipitate out iodine as silver iodide, which is then decomposed by reaction with iron to form metallic silver and a solution of iron ( II ) iodide. The iodine may then be liberated by displacement with chlorine. Applications Unlike chlorine and bromine which have one significant main use dwarfing all others, iodine is used in many applications of varying importance. About half of all produced iodine goes into various organoiodine compounds ; another 15 % remains as the pure element, another 15 % is used to form potassium iodide, and another 15 % for other inorganic iodine compounds. The remaining 5 % is for minor uses. Among the major uses of iodine compounds are catalysts, animal feed supplements, stabilisers, dyes, colourants and pigments, pharmaceutical, sanitation ( from tincture of iodine ), and photography ; minor uses include smog inhibition, cloud seeding, and various uses in analytical chemistry. Analysis Testing a seed for starch with a solution of iodine Potassium tetraiodomercurate ( II ), K HgI, is also known as Nessler 's reagent. It is often used as a sensitive spot test for ammonia. Similarly, Cu HgI is used as a precipitating reagent to test for alkaloids. The iodide and iodate anions are often used for quantitative volumetric analysis, for example in iodometry and the iodine clock reaction ( in which iodine also serves as a test for starch, forming a dark blue complex ), and aqueous alkaline iodine solution is used in the iodoform test for methyl ketones. The iodine test for starch is still used to detect counterfeit banknotes printed on starch - containing paper. Medicine Elemental iodine Main article : Iodine ( medical use ) Elemental iodine is used as a disinfectant either as the element, or as the water - soluble triiodide anion I generated in situ by adding iodide to poorly water - soluble elemental iodine ( the reverse chemical reaction makes some free elemental iodine available for antisepsis ). Elemental iodine may also be used to treat iodine deficiency. In the alternative, iodine may be produced from iodophors, which contain iodine complexed with a solubilizing agent ( iodide ion may be thought of loosely as the iodophor in triiodide water solutions ). Examples of such preparations include : Tincture of iodine : iodine in ethanol, or iodine and sodium iodide in a mixture of ethanol and water. Lugol 's iodine : iodine and iodide in water alone, forming mostly triiodide. Unlike tincture of iodine, Lugol 's iodine has a minimised amount of the free iodine ( I ) component. Povidone iodine ( an iodophor ). The antimicrobial action of iodine is quick and works at low concentrations, and thus it is used in operating theatres. Its specific mode of action is unknown. It penetrates into microorganisms and attacks particular amino acids ( such as cysteine and methionine ), nucleotides, and fatty acids, ultimately resulting in cell death. It also has an antiviral action, but nonlipid viruses and parvoviruses are less sensitive than lipid enveloped viruses. Iodine probably attacks surface proteins of enveloped viruses, and it may also destabilise membrane fatty acids by reacting with unsaturated carbon bonds. Other formulations In medicine, a saturated solution of potassium iodide is used to treat acute thyrotoxicosis. It is also used to block uptake of iodine - 131 in the thyroid gland ( see isotopes section above ), when this isotope is used as part of radiopharmaceuticals ( such as iobenguane ) that are not targeted to the thyroid or thyroid - type tissues. Iodine - 131 ( usually as iodide ) is a component of nuclear fallout, and is particularly dangerous owing to the thyroid gland 's propensity to concentrate ingested iodine and retain it for periods longer than this isotope 's radiological half - life of eight days. For this reason, people at risk of exposure to environmental radioactive iodine ( iodine - 131 ) in fallout may be instructed to take non-radioactive potassium iodide tablets. The typical adult dose is one 130 mg tablet per 24 hours, supplying 100 mg ( 100,000 micrograms ) of ionic iodine. ( The typical daily dose of iodine for normal health is of order 100 micrograms ; see `` Dietary Intake '' below. ) Ingestion of this large dose of non-radioactive iodine minimises the uptake of radioactive iodine by the thyroid gland. Diatrizoic acid, an iodine - containing radiocontrast agent As an element with high electron density and atomic number, iodine absorbs X-rays weaker than 33.3 keV due to the photoelectric effect of the innermost electrons. Organoiodine compounds are used with intravenous injection as X-ray radiocontrast agents. This application is often in conjunction with advanced X-ray techniques such as angiography and CT scanning. At present, all water - soluble radiocontrast agents rely on iodine. Others The production of ethylenediamine dihydroiodide, provided as a nutritional supplement for livestock, consumes a large portion of available iodine. Another significant use is a catalyst for the production of acetic acid by the Monsanto and Cativa processes. In these technologies, which support the world 's demand for acetic acid, hydroiodic acid converts the methanol feedstock into methyl iodide, which undergoes carbonylation. Hydrolysis of the resulting acetyl iodide regenerates hydroiodic acid and gives acetic acid. Inorganic iodides find specialised uses. Titanium, zirconium, hafnium, and thorium are purified by the van Arkel process, which involves the reversible formation of the tetraiodides of these elements. Silver iodide is a major ingredient to traditional photographic film. Thousands of kilograms of silver iodide are used annually for cloud seeding to induce rain. The organoiodine compound erythrosine is an important food coloring agent. Perfluoroalkyl iodides are precursors to important surfactants, such as perfluorooctanesulfonic acid. Biological role Main article : Iodine in biology The thyroid system of the thyroid hormones T and T Iodine is an essential element for life and is the heaviest element commonly needed by living organisms. ( Lanthanum and the other lanthanides, as well as tungsten, are used by a few microorganisms. ) It is required for the synthesis of the growth - regulating thyroid hormones thyroxine and triiodothyronine ( T and T respectively, named after their number of iodine atoms ). A deficiency of iodine leads to decreased production of T and T and a concomitant enlargement of the thyroid tissue in an attempt to obtain more iodine, causing the disease known as simple goitre. The major form of thyroid hormone in the blood is thyroxine ( T ), which has a longer half - life than T. In humans, the ratio of T to T released into the blood is between 14 : 1 and 20 : 1. T is converted to the active T ( three to four times more potent than T ) within cells by deiodinases ( 5 ' - iodinase ). These are further processed by decarboxylation and deiodination to produce iodothyronamine ( T a ) and thyronamine ( T a ' ). All three isoforms of the deiodinases are selenium - containing enzymes ; thus dietary selenium is essential for T production. Iodine accounts for 65 % of the molecular weight of T and 59 % of T. Fifteen to 20 mg of iodine is concentrated in thyroid tissue and hormones, but 70 % of all iodine in the body is found in other tissues, including mammary glands, eyes, gastric mucosa, fetal thymus, cerebro - spinal fluid and choroid plexus, arterial walls, the cervix, and salivary glands. In the cells of those tissues, iodide enters directly by sodium - iodide symporter ( NIS ). The action of iodine in mammary tissue is related to fetal and neonatal development, but in the other tissues, it is ( at least ) partially unknown. Dietary intake Recommendations by the United States Institute of Medicine are between 110 and 130 μg for infants up to 12 months, 90 μg for children up to eight years, 130 μg for children up to 13 years, 150 μg for adults, 220 μg for pregnant women and 290 μg for lactation. The Tolerable Upper Intake Level ( UL ) for adults is 1,100 μg / day. This upper limit was assessed by analyzing the effect of supplementation on thyroid - stimulating hormone. The thyroid gland needs no more than 70 μg / day to synthesise the requisite daily amounts of T4 and T3. The higher recommended daily allowance levels of iodine seem necessary for optimal function of a number of body systems, including lactating breast, gastric mucosa, salivary glands, brain cells, choroid plexus, thymus, and arterial walls. Natural sources of dietary iodine include seafood, such as fish, seaweeds ( such as kelp ) and shellfish, dairy products and eggs so long as the animals received enough iodine, and plants grown on iodine - rich soil. Iodised salt is fortified with iodine in the form of sodium iodide. As of 2000, the median intake of iodine from food in the United States was 240 to 300 μg / day for men and 190 to 210 μg / day for women. The general US population has adequate iodine nutrition, with women of childbearing age and pregnant women having a possible mild risk of deficiency. In Japan, consumption was considered much higher, ranging between 5,280 μg / day to 13,800 μg / day from dietary seaweed or kombu kelp, often in the form of Kombu Umami extracts for soup stock and potato chips. However, new studies suggest that Japan 's consumption is closer to 1,000 -- 3,000 μg / day. The adult UL in Japan was last revised to 3,000 μg / day in 2015. After iodine fortification programs such as iodisation of salt have been implemented, some cases of iodine - induced hyperthyroidism have been observed ( so - called Jod - Basedow phenomenon ). The condition seems to occur mainly in people over forty, and the risk appears higher when iodine deficiency is severe and the initial rise in iodine intake is high. Deficiency Main article : Iodine deficiency In areas where there is little iodine in the diet, typically remote inland areas and semi-arid equatorial climates where no marine foods are eaten, iodine deficiency gives rise to hypothyroidism, symptoms of which are extreme fatigue, goitre, mental slowing, depression, weight gain, and low basal body temperatures. Iodine deficiency is the leading cause of preventable intellectual disability, a result that occurs primarily when babies or small children are rendered hypothyroidic by a lack of the element. The addition of iodine to table salt has largely eliminated this problem in the wealthier nations, but iodine deficiency remains a serious public health problem today in the developing world. Iodine deficiency is also a problem in certain areas of Europe. Information processing, fine motor skills, and visual problem solving are improved by iodine repletion in moderately iodine - deficient children. Toxicity NFPA 704 fire diamond Fire diamond hazard sign for elemental iodine Elemental iodine ( I ) is toxic if taken orally undiluted. The lethal dose for an adult human is 30 mg / kg, which is about 2.1 -- 2.4 grams for a human weighing 70 to 80 kg ( even if experiments on rats demonstrated that these animals could survive after eating a 14000 mg / kg dose ). Excess iodine can be more cytotoxic in the presence of selenium deficiency. Iodine supplementation in selenium - deficient populations is, in theory, problematic, partly for this reason. The toxicity derives from its oxidizing properties, through which it denaturates proteins ( including enzymes ). Elemental iodine is also a skin irritant, and direct contact with skin can cause damage and solid iodine crystals should be handled with care. Solutions with high elemental iodine concentration, such as tincture of iodine and Lugol 's solution, are capable of causing tissue damage if used in prolonged cleaning or antisepsis ; similarly, liquid Povidone - iodine ( Betadine ) trapped against the skin resulted in chemical burns in some reported cases. Occupational exposure People can be exposed to iodine in the workplace by inhalation, ingestion, skin contact, and eye contact. The Occupational Safety and Health Administration ( OSHA ) has set the legal limit ( Permissible exposure limit ) for iodine exposure in the workplace at 0.1 ppm ( 1 mg / m ) during an 8 - hour workday. The National Institute for Occupational Safety and Health ( NIOSH ) has set a Recommended exposure limit ( REL ) of 0.1 ppm ( 1 mg / m ) during an 8 - hour workday. At levels of 2 ppm, iodine is immediately dangerous to life and health. Allergic reactions Some people develop a hypersensitivity to products and foods containing iodine. Applications of tincture of iodine or Betadine can cause rashes, sometimes severe. Parenteral use of iodine - based contrast agents ( see above ) can cause reactions ranging from a mild rash to fatal anaphylaxis. Such reactions have led to the misconception ( widely held, even among physicians ) that some people are allergic to iodine itself ; even allergies to iodine - rich seafood have been so construed. In fact, there has never been a confirmed report of a true iodine allergy, and an allergy to elemental iodine or simple iodide salts is theoretically impossible. Hypersensitivity reactions to products and foods containing iodine are apparently related to their other molecular components ; thus, a person who has demonstrated an allergy to one food or product containing iodine may not be have an allergic reaction to another. Patients with various food allergies ( shellfish, egg, milk, etc. ) or asthma are more likely to suffer reactions to contrast media containing iodine. As with all medications, the patient 's allergy history should be questioned and consulted before any containing iodine are administered. References Jump up ^ Meija, J. ; et al. ( 2016 ). `` Atomic weights of the elements 2013 ( IUPAC Technical Report ) ''. Pure and Applied Chemistry. 88 ( 3 ) : 265 -- 91. doi : 10.1515 / pac - 2015 - 0305. Jump up ^ Magnetic susceptibility of the elements and inorganic compounds, in Handbook of Chemistry and Physics 81st edition, CRC press. Jump up ^ Weast, Robert ( 1984 ). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida : Chemical Rubber Company Publishing. pp. E110. ISBN 0 - 8493 - 0464 - 4. ^ Jump up to : `` Iodine ''. Micronutrient Information Center, Linus Pauling Institute, Oregon State University, Corvallis, OR. 2015. Retrieved 20 November 2017. ^ Jump up to : Courtois, Bernard ( 1813 ). `` Découverte d'une substance nouvelle dans le Vareck ''. Annales de chimie. 88 : 304. In French, seaweed that had been washed onto the shore was called `` varec '', `` varech '', or `` vareck '', whence the English word `` wrack ''. Later, `` varec '' also referred to the ashes of such seaweed : The ashes were used as a source of iodine and salts of sodium and potassium. Jump up ^ Swain, Patricia A. ( 2005 ). `` Bernard Courtois ( 1777 -- 1838 ) famed for discovering iodine ( 1811 ), and his life in Paris from 1798 '' ( PDF ). Bulletin for the History of Chemistry. 30 ( 2 ) : 103. Jump up ^ Greenwood and Earnshaw, p. 794 ^ Jump up to : `` 53 Iodine ''. Elements.vanderkrogt.net. Retrieved 23 October 2016. Jump up ^ Desormes and Clément made their announcement at the Institut impérial de France on 29 November 1813 ; a summary of their announcement appeared in the Gazette nationale ou Le Moniteur Universel of 2 December 1813. See : F.D. Chattaway ( 23 April 1909 ) `` The discovery of iodine, '' The Chemical News..., 99 ( 2578 ) : 193 -- 195. ^ Jump up to : Gay - Lussac, J. ( 1813 ). `` Sur un nouvel acide formé avec la substance décourverte par M. Courtois ''. Annales de chimie. 88 : 311. Jump up ^ Gay - Lussac, J. ( 1813 ). `` Sur la combination de l'iode avec d'oxigène ''. Annales de chimie. 88 : 319. Jump up ^ Gay - Lussac, J. ( 1814 ). `` Mémoire sur l'iode ''. Annales de chimie. 91 : 5. Jump up ^ Liddell -- Scott -- Jones Greek -- English Lexicon at the Perseus Digital Library Jump up ^ Davy, H. ( 1813 ). `` Sur la nouvelle substance découverte par M. Courtois, dans le sel de Vareck ''. Annales de chimie. 88 : 322. Jump up ^ Davy, Humphry ( 1 January 1814 ). `` Some Experiments and Observations on a New Substance Which Becomes a Violet Coloured Gas by Heat ''. Phil. Trans. R. Soc. Lond. 104 : 74. doi : 10.1098 / rstl. 1814.0007. ^ Jump up to : Greenwood and Earnshaw, pp. 800 -- 4 Jump up ^ Kugler, H.K. ; Keller, C. ( 1985 ). ' At, Astatine ', System No. 8a. Gmelin Handbook of Inorganic and Organometallic Chemistry. 8 ( 8th ed. ). Springer - Verlag. ISBN 3 - 540 - 93516 - 9. ^ Jump up to : Greenwood and Earnshaw, pp. 804 -- 9 Jump up ^ Windholz, Martha ; Budavari, Susan ; Stroumtsos, Lorraine Y. ; Fertig, Margaret Noether, eds. ( 1976 ). Merck Index of Chemicals and Drugs ( 9th ed. ). JA Majors Company. ISBN 0 - 911910 - 26 - 3. ^ Jump up to : King, R. Bruce ( 1995 ). Inorganic Chemistry of Main Group Elements. Wiley - VCH. pp. 173 -- 98. ISBN 0 - 471 - 18602 - 3. Jump up ^ Housecroft, C.E. ; Sharpe, A.G. ( 2008 ). Inorganic Chemistry ( 3rd ed. ). Prentice Hall. p. 541. ISBN 978 - 0131755536. Jump up ^ Li, Wai - Kee ; Zhou, Gong - Du ; Mak, Thomas C.W. ( 2008 ). Advanced Structural Inorganic Chemistry. Oxford University Press. p. 674. ISBN 0 - 19 - 921694 - 0. ^ Jump up to : Audi, G. ; Bersillon, O. ; Blachot, J. ; Wapstra, A.H. ( 2003 ). `` The NUBASE evaluation of nuclear and decay properties '' ( PDF ). Nuclear Physics A. 729 : 3 -- 128. Bibcode : 2003NuPhA. 729... 3A. doi : 10.1016 / j. nuclphysa. 2003.11. 001. Archived from the original ( PDF ) on 2008 - 09 - 23. Jump up ^ J. Watson et al. ( 1965 ) `` Iodine - 129 as a Nonradioactive Tracer '', Radiation Research, 26, 159 -- 163. Jump up ^ https://e-reports-ext.llnl.gov/pdf/234761.pdf P. Santschi et al. ( 1998 ) `` 129Iodine : A new tracer for surface water / groundwater interaction. '' Lawrence Livermore National Laboratory preprint UCRL - JC - 132516. Livermore, USA. Jump up ^ * G. Snyder and J. Fabryka - Martin. ( 2007 ). I - 129 and Cl - 36 in dilute hydrocarbon waters : Marine - cosmogenic, in situ, and anthropogenic sources. '' Applied Geochemistry, 22 ( 3 ) 692 -- 714. Jump up ^ Clayton, Donald D. ( 1983 ). Principles of Stellar Evolution and Nucleosynthesis ( 2nd ed. ). University of Chicago Press. p. 75. ISBN 0 - 226 - 10953 - 4. Jump up ^ Bolt, B.A. ; Packard, R.E. ; Price, P.B. ( 2007 ). `` John H. Reynolds, Physics : Berkeley ''. The University of California, Berkeley. Retrieved 2007 - 10 - 01. Jump up ^ SCOPE 50 - Radioecology after Chernobyl Archived 13 May 2014 at the Wayback Machine., the Scientific Committee on Problems of the Environment ( SCOPE ), 1993. See table 1.9 in Section 1.4. 5.2. Jump up ^ Hupf HB, Eldridge JS, Beaver JE ( April 1968 ). `` Production of iodine - 123 for medical applications ''. Int J Appl Radiat Isot. 19 ( 4 ) : 345 -- 51. doi : 10.1016 / 0020 - 708X ( 68 ) 90178 - 6. PMID 5650883. Jump up ^ Harper, P.V. ; Siemens, W.D. ; Lathrop, K.A. ; Brizel, H.E. ; Harrison, R.W. Iodine - 125. Proc. Japan Conf. Radioisotopes ; Vol : 4th Jan 01, 1961 Jump up ^ Rivkees, Scott A. ; Sklar, Charles ; Freemark, Michael ( 1998 ). `` The Management of Graves ' Disease in Children, with Special Emphasis on Radioiodine Treatment ''. Journal of Clinical Endocrinology & Metabolism. 83 ( 11 ) : 3767 -- 76. doi : 10.1210 / jc. 83.11. 3767. PMID 9814445. Jump up ^ Zanzonico PB, Becker DV ( 2000 ). `` Effects of time of administration and dietary iodine levels on potassium iodide ( KI ) blockade of thyroid irradiation by 131I from radioactive fallout ''. Health Phys. 78 ( 6 ) : 660 -- 7. doi : 10.1097 / 00004032 - 200006000 - 00008. PMID 10832925. Jump up ^ `` Medical isotopes the likely cause of radiation in Ottawa waste ''. CBC News. 4 February 2009. Retrieved 30 September 2015. Jump up ^ Moser, H. ; Rauert, W. ( 2007 ). `` Isotopic Tracers for Obtaining Hydrologic Parameters ''. In Aggarwal, Pradeep K. ; Gat, Joel R. ; Froehlich, Klaus F. Isotopes in the water cycle : past, present and future of a developing science. Dordrecht : Springer. p. 11. ISBN 978 - 1 - 4020 - 6671 - 9. Retrieved 6 May 2012. Jump up ^ Rao, S.M. ( 2006 ). `` Radioisotopes of hydrological interest ''. Practical isotope hydrology. New Delhi : New India Publishing Agency. pp. 12 -- 13. ISBN 978 - 81 - 89422 - 33 - 2. Retrieved 6 May 2012. Jump up ^ `` Investigating leaks in Dams & Reservoirs '' ( PDF ). IAEA.org. Retrieved 6 May 2012. Jump up ^ Araguás, Luis Araguás ; Plata Bedmar, Antonio ( 2002 ). `` Artificial radioactive tracers ''. Detection and prevention of leaks from dams. Taylor & Francis. pp. 179 -- 181. ISBN 978 - 90 - 5809 - 355 - 4. Retrieved 6 May 2012. Jump up ^ Greenwood and Earnshaw, pp. 809 -- 12 ^ Jump up to : Greenwood and Earnshaw, pp. 812 -- 9 Jump up ^ Holleman, A.F. ; Wiberg, E. `` Inorganic Chemistry '' Academic Press : San Diego, 2001. ISBN 0 - 12 - 352651 - 5. ^ Jump up to : Greenwood and Earnshaw, pp. 821 -- 4 ^ Jump up to : Greenwood and Earnshaw, pp. 824 -- 8 Jump up ^ Greenwood and Earnshaw, pp. 828 -- 31 Jump up ^ Greenwood and Earnshaw, pp. 832 -- 5 Jump up ^ Greenwood and Earnshaw, pp. 851 -- 3 ^ Jump up to : Greenwood and Earnshaw, pp. 853 -- 9 Jump up ^ Greenwood and Earnshaw, pp. 863 -- 4 ^ Jump up to : Greenwood and Earnshaw, pp. 872 -- 5 Jump up ^ Greenwood and Earnshaw, pp. 842 -- 4 Jump up ^ Greenwood and Earnshaw, pp. 835 -- 9 Jump up ^ Aug. Wilh. von Hofmann ( 1851 ). `` Beiträge zur Kenntniss der flüchtigen organischen Basen ''. Annalen der Chemie und Pharmacie. 78 ( 3 ) : 253 -- 286. doi : 10.1002 / jlac. 18510780302. Jump up ^ `` Theory of Aetherification ''. Philosophical Magazine. 37 : 350 -- 356. 1850. doi : 10.1080 / 14786445008646627. ( Link to excerpt. ) Jump up ^ Adolphe Wurtz ( 1855 ). `` Ueber eine neue Klasse organischer Radicale ''. Annalen der Chemie und Pharmacie. 96 ( 3 ) : 364 -- 375. doi : 10.1002 / jlac. 18550960310. Jump up ^ Grignard, V. ( 1900 ). `` Sur quelques nouvelles combinaisons organométaliques du magnésium et leur application à des synthèses d'alcools et d'hydrocabures ''. Compt. Rend. 130 : 1322 -- 25. Jump up ^ Phyllis A. Lyday ( 2005 ), `` Iodine and Iodine Compounds '', Ullmann 's Encyclopedia of Industrial Chemistry, Weinheim : Wiley - VCH, doi : 10.1002 / 14356007. a14_381 Jump up ^ Blanksby SJ, Ellison GB ( April 2003 ). `` Bond dissociation energies of organic molecules '' ( PDF ). Acc. Chem. Res. 36 ( 4 ) : 255 -- 63. doi : 10.1021 / ar020230d. PMID 12693923. Jump up ^ Boeckman, R.K. Jr. ; Shao, P. ; Mullins, J.J. ( 2000 ). `` Dess -- Martin periodinane : 1, 1, 1 - Triacetoxy - 1, 1 - dihydro - 1, 2 - benziodoxol - 3 ( 1H ) - one '' ( PDF ). Organic Syntheses. 77 : 141. ; Collective Volume, 10, p. 696 Jump up ^ Michael E. Jung and Michael H. Parker ( 1997 ). `` Synthesis of Several Naturally Occurring Polyhalogenated Monoterpenes of the Halomon Class ''. Journal of Organic Chemistry. 62 ( 21 ) : 7094 -- 7095. doi : 10.1021 / jo971371. PMID 11671809. ^ Jump up to : Smith, Michael B. ; March, Jerry ( 2007 ), Advanced Organic Chemistry : Reactions, Mechanisms, and Structure ( 6th ed. ), New York : Wiley - Interscience, ISBN 0 - 471 - 72091 - 7 Jump up ^ `` Safety data for iodomethane ''. Oxford University. Jump up ^ Polgar, L ( 1979 ). `` Deuterium isotope effects on papain acylation. Evidence for lack of general base catalysis and for enzyme - leaving group. interaction ''. Eur. J. Biochem. 98 ( 2 ) : 369 -- 374. doi : 10.1111 / j. 1432 - 1033.1979. tb13196. x. PMID 488108. Jump up ^ Ervithayasuporn, V. ( 2013 ). `` One - pot synthesis of halogen exchanged silsesquioxanes : octakis ( 3 - bromopropyl ) octasilsesquioxane and octakis ( 3 - iodopropyl ) octasilsesquioxane ''. Dalton Trans. 42 : 13747 -- 13753. doi : 10.1039 / C3DT51373D. Jump up ^ Streitwieser, A. ( 1956 ). `` Solvolytic Displacement Reactions at Saturated Carbon Atoms ''. Chem. Rev. 56 ( 4 ) : 571 -- 752. doi : 10.1021 / cr50010a001. Jump up ^ Bordwell, F.G. ; Brannen, W.T. ( 1964 ). `` The Effect of the Carbonyl and Related Groups on the Reactivity of Halides in S 2 Reactions ''. J. Am. Chem. Soc. 86 ( 21 ) : 4645 -- 4650. doi : 10.1021 / ja01075a025. ^ Jump up to : Greenwood and Earnshaw, pp. 795 -- 6 ^ Jump up to : Kogel, Jessica Elzea ; et al. ( 2006 ). Industrial Minerals & Rocks : Commodities, Markets, and Uses. SME. pp. 541 -- 552. ISBN 978 - 0 - 87335 - 233 - 8. Jump up ^ Stanford, Edward C.C. ( 1862 ). `` On the Economic Applications of Seaweed ''. Journal of the Society of Arts : 185 -- 189. Jump up ^ Maekawa, Tatsuo ; Igari, Shun - Ichiro ; Kaneko, Nobuyuki ( 2006 ). `` Chemical and isotopic compositions of brines from dissolved - in - water type natural gas fields in Chiba, Japan ''. Geochemical Journal. 40 ( 5 ) : 475. doi : 10.2343 / geochemj. 40.475. Jump up ^ Greenwood and Earnshaw, p. 799 Jump up ^ Emsley, John ( 2001 ). Nature 's Building Blocks ( Hardcover, First ed. ). Oxford University Press. pp. 244 -- 250. ISBN 0 - 19 - 850340 - 7. Jump up ^ WHO Model Formulary 2008 ( PDF ). World Health Organization. 2009. p. 499. ISBN 9789241547659. Retrieved 8 January 2017. Jump up ^ Block, Seymour Stanton ( 2001 ). Disinfection, sterilization, and preservation. Hagerstwon, MD : Lippincott Williams & Wilkins. p. 159. ISBN 0 - 683 - 30740 - 1. Jump up ^ Patwardhan, Narendra ; Kelkar, Uday ( 2011 ). `` Disinfection, sterilization and operation theater guidelines for dermatosurgical practitioners in India ''. Dermatosurgery Specials. 77 ( 1 ) : 83 -- 93. doi : 10.4103 / 0378 - 6323.74965. Retrieved 23 October 2016. Jump up ^ McDonnell G, Russell AD ( 1999 ). `` Antiseptics and disinfectants : activity, action, and resistance ''. Clin Microbiol Rev. 12 ( 1 ) : 147 -- 79. PMC 88911. PMID 9880479. Jump up ^ `` Solubility of KI in water ''. Hazard.com. 1998 - 04 - 21. Retrieved 2013 - 01 - 21. Jump up ^ https://web.archive.org/web/20111007202042/https://www.eanm.org/scientific_info/guidelines/gl_radio_ther_benzyl.pdf?PHPSESSID=46d05b62d235c36a12166bf939b656c7 Jump up ^ U.S. Centers for Disease Control `` CDC Radiation Emergencies '', U.S. Centers for Disease Control, 11 October 2006, accessed 14 November 2010. Jump up ^ Lancaster, Jack L. Chapter 4 : Physical Determinants of Contrast Archived 10 October 2015 at the Wayback Machine., in Physics of Medical X-Ray Imaging. The University of Texas Health Science Center. ^ Jump up to : Lyday, Phyllis A. ; Tatsuo Kaiho `` Iodine and Iodine Compounds '' in Ullmann 's Encyclopedia of Industrial Chemistry, 2015, Wiley - VCH, Weinheim, doi : 10.1002 / 14356007. a14_381. pub2 Vol. A14 pp. 382 -- 390. Jump up ^ Pol, Arjan ; Barends, Thomas R.M. ; Dietl, Andreas ; Khadem, Ahmad F. ; Eygensteyn, Jelle ; Jetten, Mike S.M. ; Op Den Camp, Huub J.M. ( 2013 ). `` Rare earth metals are essential for methanotrophic life in volcanic mudpots ''. Environmental Microbiology. 16 ( 1 ) : 255 -- 64. doi : 10.1111 / 1462 - 2920.12249. PMID 24034209. Jump up ^ Koribanics, N.M. ; Tuorto, S.J. ; Lopez - Chiaffarelli, N. ; McGuinness, L.R. ; Häggblom, M.M. ; Williams, K.H. ; Long, P.E. ; Kerkhof, L.J. ( 2015 ). `` Spatial Distribution of an Uranium - Respiring Betaproteobacterium at the Rifle, CO Field Research Site ''. PLoS ONE. 10 ( 4 ) : e0123378. doi : 10.1371 / journal. pone. 0123378. PMC 4395306. PMID 25874721. Jump up ^ Irizarry, Lisandro ( 23 April 2014 ). `` Thyroid Hormone Toxicity ''. Medscape. WedMD LLC. Retrieved 2 May 2014. ^ Jump up to : Patrick, L. ( 2008 ). `` Iodine : deficiency and therapeutic considerations '' ( PDF ). Altern Med Rev. 13 ( 2 ) : 116 -- 27. PMID 18590348. Archived from the original ( PDF ) on 31 May 2013. Jump up ^ `` Dietary Reference Intakes ( DRIs ) : Recommended Intakes for Individuals, Vitamins ''. Institute of Medicine. 2004. Archived from the original on 30 October 2009. Retrieved 9 June 2010. ^ Jump up to : United States National Research Council ( 2000 ). Dietary Reference Intakes for Vitamin A, Vitamin K, Arsenic, Boron, Chromium, Copper, Iodine, Iron, Manganese, Molybdenum, Nickel, Silicon, Vanadium, and Zinc. National Academies Press. pp. 258 -- 259. Jump up ^ Venturi, S, Venturi. M ( 2009 ). `` Iodine, thymus, and immunity ''. Nutrition. 25 ( 9 ) : 977 -- 979. doi : 10.1016 / j. nut. 2009.06. 002 /. CS1 maint : Multiple names : authors list ( link ) Jump up ^ Ullberg, S. ; Ewaldsson, B. ( 1964 ). `` Distribution of radio - iodine studied by whole - body autoradiography ''. Acta Radiologica Therapy Physics Biology. 41 : 24 -- 32. doi : 10.3109 / 02841866409134127. Jump up ^ Venturi, Sebastiano ( 2014 ). `` Iodine, PUFAs and Iodolipids in Health and Disease : An Evolutionary Perspective ''. Human Evolution -. 29 ( 1 -- 3 ) : 185 -- 205. ISSN 0393 - 9375. Jump up ^ `` Where do we get iodine from ? ''. Iodine Global Network. Archived from the original on 13 August 2015. ^ Jump up to : `` Iodine in diet ''. MedlinePlus Medical Encyclopedia. Jump up ^ `` American Thyroid Association ''. thyroid.org. American Thyroid Association. Retrieved 4 April 2014. Jump up ^ Caldwell KL, Makhmudov A, Ely E, Jones RL, Wang RY ( 2011 ). `` Iodine status of the U.S. population, National Health and Nutrition Examination Survey, 2005 -- 2006 and 2007 -- 2008 ''. Thyroid. 21 ( 4 ) : 419 -- 27. doi : 10.1089 / thy. 2010.0077. PMID 21323596. ^ Jump up to : Leung AM, Braverman LE, Pearce EN ( 2012 ). `` History of U.S. iodine fortification and supplementation ''. Nutrients. 4 ( 11 ) : 1740 -- 6. doi : 10.3390 / nu4111740. PMC 3509517. PMID 23201844. Jump up ^ Zava, T.T. ; Zava, D.T. ( 2011 ). `` Assessment of Japanese iodine intake based on seaweed consumption in Japan : A literature - based analysis ''. Thyroid Research. 4 : 14. doi : 10.1186 / 1756 - 6614 - 4 - 14. PMC 3204293. PMID 21975053. Jump up ^ Overview of Dietary Reference Intakes for Japanese ( 2015 ) Minister of Health, Labour and Welfare, Japan url = http://www.mhlw.go.jp/file/06-Seisakujouhou-10900000-Kenkoukyoku/Overview.pdf Jump up ^ Wu, T. ; Liu, G.J. ; Li, P. ; Clar, C. ( 2002 ). Wu, Taixiang, ed. `` Iodised salt for preventing iodine deficiency disorders ''. Cochrane Database Syst Rev ( 3 ) : CD003204. doi : 10.1002 / 14651858. CD003204. PMID 12137681. Jump up ^ Dissanayake, C.B. ; Chandrajith, Rohana ; Tobschall, H.J. ( 1999 ). `` The iodine cycle in the tropical environment -- implications on iodine deficiency disorders ''. International Journal of Environmental Studies. 56 ( 3 ) : 357. doi : 10.1080 / 00207239908711210. Jump up ^ Felig, Philip ; Frohman, Lawrence A. ( 2001 ). `` Endemic Goiter ''. Endocrinology & metabolism. McGraw - Hill Professional. ISBN 978 - 0 - 07 - 022001 - 0. Jump up ^ `` Micronutrient deficiency : iodine deficiency disorders ''. WHO. Jump up ^ Zimmermann, Michael B. ; Connolly, K. ; et al. ( 2006 ). `` Iodine supplementation improves cognition in iodine - deficient schoolchildren in Albania : a randomized, controlled, double - blind study ''. American Journal of Clinical Nutrition. 83 ( 1 ) : 108 -- 114. PMID 16400058. Jump up ^ Technical data for Iodine. periodictable.com Jump up ^ Smyth, P.P. ( 2003 ). `` Role of iodine in antioxidant defence in thyroid and breast disease ''. BioFactors ( Oxford, England ). 19 ( 3 -- 4 ) : 121 -- 30. doi : 10.1002 / biof. 5520190304. PMID 14757962. Jump up ^ Yerkes, Christine ( 2007 ). `` Lecture 29 : Protein Structure and Denaturation ''. chem.uiuc.edu. University of Illinois. Retrieved 23 October 2016. Jump up ^ Lowe, D.O. ; Knowles, S.R. ; et al. ( 2006 ). `` Povidone - iodine - induced burn : case report and review of the literature ''. Pharmacotherapy. 26 ( 11 ) : 1641 -- 5. doi : 10.1592 / phco. 26.11. 1641. PMID 17064209. Jump up ^ `` CDC - NIOSH Pocket Guide to Chemical Hazards - Iodine ''. www.cdc.gov. Retrieved 2015 - 11 - 06. Jump up ^ DermNet New Zealand Trust, Iodine Jump up ^ Boehm, I ( 2008 ). `` Seafood allergy and radiocontrast media : Are physicians propagating a myth ? ''. Am J Med. 121 ( 8 ) : E19 -- E19. doi : 10.1016 / j. amjmed. 2008.03. 035. ^ Jump up to : UCSF Department of Radiology & Biomedical Imaging, Iodine Allergy and Contrast Administration Jump up ^ Katelaris, Constance ( 2009 ). `` ' Iodine Allergy ' label is misleading ''. Australian Prescriber. 32 ( 5 ) : 125 -- 128. Archived from the original on 3 March 2016. Bibliography Greenwood, Norman N. ; Earnshaw, Alan ( 1997 ). Chemistry of the Elements ( 2nd ed. ). Butterworth - Heinemann. ISBN 0 - 08 - 037941 - 9. Books View or order collections of articles Iodine Period 5 elements Halogens Chemical elements ( sorted alphabetically ) Chemical elements ( sorted by number ) Portals Access related topics Chemistry portal Find out more on Wikipedia 's Sister projects Media from Commons Definitions from Wiktionary Textbooks from Wikibooks Quotations from Wikiquote Source texts from Wikisource Learning resources from Wikiversity Periodic table ( Large cells ) 5 6 7 8 9 10 11 12 13 14 15 16 17 18 He Li Be O Ne Na Mg Al Si Cl Ar Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 5 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te Xe 6 Cs Ba La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Hf Ta Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn 7 Fr Ra Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og Alkali metal Alkaline earth metal Lanthanide Actinide Transition metal Post - ​ transition metal Metalloid Polyatomic nonmetal Diatomic nonmetal Noble gas Unknown chemical properties Iodine compounds Iodine ( - I ) HI AtI ICN Iodine ( I ) HIO ICl IF IBr Iodine ( III ) HIO ICl IF Iodine ( V ) HIO IF I O Iodine ( VII ) HIO H IO IF Diatomic chemical elements Normal O Cl Br Others Li Thyroid hormone receptor modulators Receptor ( ligands ) THR Agonists : Dextrothyroxine DIMIT DITPA Eprotirome ( KB - 2115 ) KB - 141 KB - 2611 KB - 130015 Levothyroxine Liothyronine Liotrix MB - 07344 MB - 07811 MGL - 3196 ( VIA - 3196 ) Sobetirome ( GC - 1, GRX - 431 ) Thyroxine Tiratricol ( TRIAC ) Triiodothyronine Thyroid extract VK - 0214 VK - 2809 ZYT1 Antagonists : 1 - 850 NH3 Tetraiodothyroacetic acid ( Tetrac ) Transporter ( blockers ) NIS Inhibitors : Cyanogenic glycosides Perchlorates ( e.g., potassium perchlorate ) Pertechnetates ( e.g., sodium pertechnetate ) Thiocyanates Enzyme ( inhibitors ) TPO Inhibitors : Benzylthiouracil Carbimazole Genistein Methimazole Methylthiouracil Propylthiouracil Thiouracil Thiourea DIO Inhibitors : Dexpropranolol Iopanoic acid Ipodate sodium ( sodium iopodate ) Propranolol Propylthiouracil Others Iodine Iodine - 131 Selenium Thyroglobulin Tyrosine See also : Receptor / signaling modulators Nuclear receptor modulators LCCN : sh85067769 GND : 4162271 - 6 BNF : cb11966629x ( data ) NDL : 00574371 BNE : XX529206 Retrieved from `` https://en.wikipedia.org/w/index.php?title=Iodine&oldid=819268867 '' Categories : Iodine Chemical elements Diatomic nonmetals Halogens Biology and pharmacology of chemical elements Dietary minerals Oxidizing agents Hidden categories : Webarchive template wayback links CS1 maint : Multiple names : authors list Wikipedia pending changes protected pages Use dmy dates from July 2014 WikiProject Elements pages using ENGVAR Articles containing Ancient Greek - language text Good articles Wikipedia articles with LCCN identifiers Wikipedia articles with GND identifiers Wikipedia articles with BNF identifiers Talk Contents About Wikipedia Wikiquote Afrikaans አማርኛ Aragonés Armãneashti Asturianu Azərbaycanca تۆرکجه বাংলা Bân - lâm - gú Башҡортса Беларуская Беларуская ( тарашкевіца ) ‎ भोजपुरी Bislama Български བོད ་ ཡིག Bosanski Brezhoneg Català Чӑвашла Cebuano Čeština Corsu Cymraeg Dansk Deutsch ދިވެހިބަސް Eesti Ελληνικά Эрзянь Español Esperanto Euskara فارسی Fiji Hindi Føroyskt Français Furlan Gaeilge Gaelg Gàidhlig Galego 贛 語 ગુજરાતી 客家 語 / Hak - kâ - ngî Хальмг 한국어 Հայերեն हिन्दी Hrvatski Ido Bahasa Indonesia Interlingua Ирон Íslenska Italiano עברית Basa Jawa ಕನ್ನಡ ქართული Қазақша Kiswahili Коми Kreyòl ayisyen Кыргызча Кырык мары Latina Latviešu Lëtzebuergesch Lietuvių Ligure Limburgs La. lojban. 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Question: where is iodine found in the periodic table
Answer: heaviest of the stable halogens; the fourth halogen, being a member of group 17 in the periodic table, below fluorine, chlorine, and bromine