Iodine



53 xenon
At
General
Number iodine, I, 53
halogens
Block p
Appearance violet-dark gray, lustrous
(3)  g·mol−1
Kr] 4d10 5s2 5p5
shell 2, 8, 18, 18, 7
Physical properties
Phase solid
r.t.) 4.933  g·cm−3
F)
F)
K, 11.7 MPa
kJ·mol−1
kJ·mol−1
Heat capacity (25 °C) (I2) 54.44  J·mol−1·K−1
Vapor pressure (rhombic)
P(Pa) 1 10 100 1 k 10 k 100 k
at T(K) 260 282 309 342 381 457
Atomic properties
Crystal structure orthorhombic
acidic oxide)
Electronegativity 2.66 (Pauling scale)
Ionization energies 1st: 1008.4 kJ/mol
2nd: 1845.9 kJ/mol
3rd: 3180 kJ/mol
Atomic radius 140  pm
Atomic radius (calc.) 115  pm
Covalent radius 133  pm
Van der Waals radius 198 pm
Miscellaneous
Magnetic ordering nonmagnetic
Electrical resistivity (0 °C) 1.3×107 Ω·m
Thermal conductivity (300 K) 0.449  W·m−1·K−1
Bulk modulus 7.7  GPa
CAS registry number 7553-56-2
Selected isotopes
Main article: Isotopes of iodine
iso NA half-life DM DE (MeV) DP
127I 100% I is neutrons
129I syn 15.7×106y β- 0.194 129Xe
131I syn 8.02070 d β- 0.971 131Xe
References

Iodine (dyes. It is required in trace amounts by most living organisms.

As with all other molecules, and hence has the molecular formula of I2.

Characteristics

Iodine is a dark-gray/purple-brown solid that starch-iodine complexes is produced only by the free element.

Many students who have seen the classroom demonstration where iodine crystals are gently heated in a test tube come away with the impression that liquid iodine cannot exist at atmospheric pressure. This misconception arises because sublimation occurs without the intermediacy of liquid. The truth is that if iodine crystals are heated carefully to their melting point of 113.7 °C, the crystals will fuse into a liquid, which will be present under a dense blanket of the vapour.

History

Iodine was discovered by Bernard Courtois in 1811. He was born to a manufacturer of sulfuric acid. One day Courtois added too much sulfuric acid and a cloud of purple vapor rose. Courtois noted that the vapor crystallized on cold surfaces making dark crystals. Courtois suspected that this was a new element but lacked the money to pursue his observations.

However he gave samples to his friends, Charles Bernard Desormes (1777 - 1862) and Nicolas Clément (1779 - 1841), to continue research. He also gave some of the substance to chlorine. Davy sent a letter dated December 10 to the Royal Society of London stating that he had identified a new element. A large argument erupted between Davy and Gay-Lussac over who identified iodine first but both scientists acknowledged Courtois as the first to isolate the chemical element.

Applications

Iodine is used in pharmaceuticals, antiseptics, medicine, food supplements, dyes, catalysts, halogen lights, photography, water purifying, and starch detection.

  • iodophor type antiseptics, are also available as effective elemental iodine sources for this purpose.
  • Iodine compounds are important in the field of organic chemistry
  • Iodine, as a heavy element, is quite CT scanning
  • Silver iodide is used in photography.
  • Tungsten iodide is used to stabilize the filaments in light bulbs.

Occurrence on earth

Iodine naturally occurs in the environment chiefly as dissolved copper(II) sulfate. There are also a few other methods of isolating this element. Although the element is actually quite rare, kelp and certain other plants have some ability to concentrate iodine, which helps introduce the element into the food chain as well as keeping its cost down.

Sources

  Iodine is found in the mineral caliche, found in Chile, between the Andes and the sea. It can also be found in some seaweeds as well as extracted from seawater, however extracting iodine from the mineral is the only economical way to extract the substance.[citation needed]

Extraction from seawater involves electrolysis. The brine is first purified and acidified using sulphuric acid and is then reacted with chlorine. An iodine solution is produced but it is yet too dilute and has to be concentrated. To do this air is blown into the solution which causes the iodine to evaporate, then it is passed into an absorbing tower containing acid where sulfur dioxide is added to reduce the iodine. The solution is then added to chlorine again to concentrate the solution more, and the final solution is at a level of about 99%.[citation needed]

Another source is from kelp. This source was used in the 18th and 19th centuries but is no longer economically viable.

In 2005, Chile was the top producer of iodine with almost two-thirds world share followed by Japan and the USA, reports the British Geological Survey.

Prices

The average price for iodine in 2005 was $7.03 US dollars per kilogram. In 2006 this suddenly changed to $17.03 US dollars per kilogram. In Chile, the world’s largest producer of iodine, prices dramatically changed too (2005 $16.97 US dollars 2006 $20.00 US dollars for one kilogram). Japan’s prices of iodine also changed. The DNSC (Defence National Stockpile Center) claims they sold one kilogram of iodine in 2005 for $18.36 US dollars. Then in 2006 they claimed they sold each kilogram for $21.29 US dollars. [1]

Descriptive chemistry

Elemental iodine is poorly soluble in water, with one gram dissolving in 3450 ml at 20 °C and 1280 ml at 50 °C. By contrast with chlorine, the formation of the hypohalite ion (IO–) in neutral aqueous solutions of iodine is negligible.

I2+ H2O ↔ H+ + I– + HIO   (K = 2.0×10-13) [2]

Solubility in water is greatly improved if the solution contains dissolved carbon disulfide (16.47 g/100 ml at 25 °C)[3]. Aqueous and ethanol solutions are brown. Solutions in chloroform, carbon tetrachloride, and carbon disulfide are violet.

Elemental iodine can be prepared by oxidizing iodides with chlorine:

2I– + Cl2 → I2 + 2Cl–

or with manganese dioxide in acid solution:[2]

2I– + 4H+ + MnO2 → I2 + 2H2O + Mn2+

Iodine is reduced to hydroiodic acid by hydrogen sulfide:[4]

I2 + H2S → 2HI + S↓

or by hydrazine:

2I2 + N2H4 → 4HI + N2

Iodine is oxidized to nitric acid:[5]

I2 + 10HNO3 → 2HIO3 + 10NO2 + 4H2O

or by chlorates:[5]

I2 + 2ClO3– → 2IO3– + Cl2

Iodine is converted in a two stage reaction to sodium hydroxide):[2]

I2 + 2OH– → I– + IO– + H2O (K = 30)
3IO– → 2I– + IO3– (K = 1020)

Notable inorganic iodine compounds

HI He
LiI BeI2 BI3 CI4 NI3 I4O9 IF IF3 IF5 IF7 Ne
NaI MgI2 AlI3 SiI4 PI3 S ICl ICl3 Ar
KI CaI2 Sc TiI4 V Cr MnI2 Fe Co Ni CuI ZnI2 Ga2I6 GeI4 As Se Br Kr
Rb SrI2 Y ZrI4 Nb Mo Tc Ru Rh Pd AgI CdI2 InI3 SnI4 SnI2 SbI3 TeI4 CI Xe
CsI BaI Hf Ta W Re Os Ir Pt AuI HgI2 TlI PbI2 Bi Po At Rn
Fr Ra Rf Db Sg Bh Hs Mt Ds Rg Uub Uut Uuq Uup Uuh Uus Uuo
↓
La Ce Pr Nd Pm SmI2 Eu Gd TbI3 Dy Ho Er Tm Yb Lu
Ac ThI4 Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr


See also iodine compounds

Stable iodine in biology

Iodine is an essential trace element; its only known roles in biology are as constituents of the thyroid tyrosine, and are stored prior to release in a protein-like molecule called thryroglobulin. T4 and T3 contain four and three atoms of iodine per molecule, respectively. The thyroid gland actively absorbs iodide from the blood to make and release these hormones into the blood, actions which are regulated by a second hormone TSH from the pituitary. Thyroid hormones are phylogenetically very old molecules which are synthesized by most multicellular organisms, and which even have some effect on unicellular organisms.

Thyroid hormones play a very basic role in biology, acting on gene transcription to regulate the basal metabolic rate. The total deficiency of thyroid hormones can reduce basal metabolic rate up to 50%, while in excessive production of thyroid hormones the basal metabolic rate can be increased by 100%. T4 acts largely as a precursor to T3, which is (with some minor exceptions) the biologically active hormone.

Human dietary intake

The United States iodized salt.

Iodine 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—goitre, mental slowing, depression, weight gain, and low basal body temperatures.[citation needed]

Iodine deficiency is also the leading cause of preventable mental retardation, an effect which happens primarily when babies and small children are made hypothyroid by 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 in the developing world.[citation needed]

Radioiodine and biology

Radioiodine and the thyroid

The artificial KI) and the iodates (KIO3).

129I (plutonium fission, both in subsurface rocks and nuclear reactors. Nuclear processes, in particular nuclear fuel reprocessing and atmospheric nuclear weapons tests have now swamped the natural signal for this isotope. 129I was used in rainwater studies following the Chernobyl accident. It also has been used as a ground-water tracer and as an indicator of nuclear waste dispersion into the natural environment.

If humans are exposed to radioactive iodine, the thyroid gland will absorb it as if it were non-radioactive iodine, leading to elevated chances of thyroid cancer. Isotopes with shorter half-lives such as 131I present a greater risk than those with longer half-lives since they generate more radiation per unit of time. Taking large amounts of regular iodine will saturate the thyroid and prevent uptake. Iodine pills are sometimes distributed to persons living close to nuclear establishments, for use in case of accidents that could lead to releases of radioactive iodine.

  • Iodine-123 and iodine-125 are used in medicine as tracers for imaging and evaluating the function of the thyroid.
  • Iodine-131 is used in medicine for treatment of thyroid cancer and Graves' Disease.
  • Uncombined (elemental) iodine is mildly toxic to all living things.
  • fission has taken place, to flush out the radioactive iodine-131 fission product. The half-life of iodine-131 is only eight days, so the treatment would need to continue only a couple of weeks. In cases of leakage of certain nuclear materials without fission, or certain types of dirty bomb made with other than radioiodine, this precaution would be of no avail.

Radioiodine and the kidney

In the 1970s imaging techniques were developed in California to utilize radioiodine in diagnostics for renal hypertension.

Isotopes

Main article: isotopes of iodine

There are 37 isotopes of iodine and only one, 127I, is stable.

In many ways, 129I is similar to 36Cl. It is a soluble halogen, fairly non-reactive, exists mainly as a non-sorbing anion, and is produced by cosmogenic, thermonuclear, and in-situ reactions. In hydrologic studies, 129I concentrations are usually reported as the ratio of 129I to total I (which is virtually all 127I). As is the case with 36Cl/Cl, 129I/I ratios in nature are quite small, 10−14 to 10−10 (peak thermonuclear 129I/I during the 1960s and 1970s reached about 10−7). 129I differs from 36Cl in that its half-life is longer (15.7 vs. 0.301 million years), it is highly biophilic, and occurs in multiple IO3−) which have different chemical behaviors. This makes it fairly easy for 129I to enter the biosphere as it becomes incorporated into vegetation, soil, milk, animal tissue, etc.

Excesses of stable 129Xe in meteorites have been shown to result from decay of "primordial" 129I produced newly by the supernovas which created the dust and gas from which the solar system formed. 129I was the first extinct radionuclide to be identified as present in the early solar system. Its decay is the basis of the I-Xe radiometric dating scheme, which covers the first 83 million years of solar system evolution.

Effects of various radioiodine isotopes in biology are discussed below.

Toxicity of iodine

Excess iodine has symptoms similar to those of iodine deficiency. Commonly encountered symptoms are abnormal growth of the thyroid gland and disorders in functioning and growth of the organism as a whole. Elemental iodine, I2, is a deadly poison if taken in larger amounts; if 2-3 grams of it is consumed, it is fatal to humans. Iodides are similar in toxicity to bromides.

Precautions for stable iodine

Direct contact with skin can cause lesions, so it should be handled with care. Iodine vapor is very irritating to the eye and to mucous membranes. Concentration of iodine in the air should not exceed 1 mg/nitrogen triiodide which is extremely sensitive and can explode unexpectedly.

Clandestine use

In the United States, the Drug Enforcement Agency (DEA) regards iodine and compounds containing iodine (ionic iodides, iodoform, ethyl iodide, and so on) as reagents useful for the clandestine manufacture of methamphetamine. Persons who attempt to purchase significant quantities of such chemicals without establishing a legitimate use are likely to find themselves the target of a DEA investigation. Persons selling such compounds without doing due diligence to establish that the materials are not being diverted to clandestine use may be subject to stiff penalties, such as expensive fines or even imprisonment.[7][8]

See also

 v • d • e chemical elements

Hydrogen H2 | Nitrogen N2 | Oxygen O2 | Fluorine F2 | Chlorine Cl2 | Bromine Br2 | Iodine I2 | Astatine At2

References

  1. ^ DNSC, 2006
  2. ^ a b c Advanced Inorganic Chemistry by Cotton and Wilkinson, 2nd ed.
  3. ^ Merck Index of Chemicals and Drugs, 9th ed.
  4. ^ General Chemistry (volume 2) by N.L. Glinka, Mir Publishing 1981
  5. ^ a b General Chemistry by Linus Pauling, 1947 ed.
  6. ^ 21 CFR 101.9 (c)(8)(iv)
  7. ^ 21 USC Sec. 872 01/22/02
  8. ^ Chemical Supplier Convicted of Diversion of Iodine
 
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