Jump to content

Arsenic

Edit links
From Wikipedia, the free encyclopedia

This is an old revision of this page, as edited by 76.9.79.116 (talk) at 21:03, 28 September 2012 (→‎Physical characteristics). The present address (URL) is a permanent link to this revision, which may differ significantly from the current revision.

Arsenic, 33As
Arsenic
Pronunciation
Allotropesgrey (most common), yellow, black (see Allotropes of arsenic)
Appearancemetallic grey
Standard atomic weight Ar°(As)
Arsenic 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
P
↑
As
↓
Sb
germanium ← arsenic → selenium
Atomic number (Z)33
Groupgroup 15 (pnictogens)
Periodperiod 4
Block  p-block
Electron configuration[Ar] 3d10 4s2 4p3
Electrons per shell2, 8, 18, 5
Physical properties
Phase at STPsolid
Sublimation point887 K ​(615 °C, ​1137 °F)
Density (at 20° C)grey: 5.782 g/cm3[3]
when liquid (at m.p.)5.22 g/cm3
Triple point1090 K, ​3628 kPa[4]
Critical point1673 K, ? MPa
Heat of fusiongrey: 24.44 kJ/mol
Heat of vaporization34.76 kJ/mol (?)
Molar heat capacity24.64 J/(mol·K)
Vapor pressure
P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 553 596 646 706 781 874
Atomic properties
Oxidation states−3, −2, −1, 0,[5] +1,[6] +2, +3, +4, +5 (a mildly acidic oxide)
ElectronegativityPauling scale: 2.18
Ionization energies
  • 1st: 947.0 kJ/mol
  • 2nd: 1798 kJ/mol
  • 3rd: 2735 kJ/mol
  • (more)
Atomic radiusempirical: 119 pm
Covalent radius119±4 pm
Van der Waals radius185 pm
Color lines in a spectral range
Spectral lines of arsenic
Other properties
Natural occurrenceprimordial
Crystal structuregrey: ​rhombohedral (hR2)
Lattice constants
Rhombohedral crystal structure for grey: arsenic
ar = 413.15 pm
α = 54.133° pm ah = 375.99 pm
ch = 1054.58 pm (at 20 °C)[3]
Thermal expansion5.6 µm/(m⋅K)[7] (at r.t.)
Thermal conductivity50.2 W/(m⋅K)
Electrical resistivity333 nΩ⋅m (at 20 °C)
Magnetic orderingdiamagnetic[8]
Molar magnetic susceptibility−5.5×10−6 cm3/mol[9]
Young's modulus8 GPa
Bulk modulus22 GPa
Mohs hardness3.5
Brinell hardness1440 MPa
CAS Number7440-38-2
History
DiscoveryArabic alchemists (before AD 815)
Isotopes of arsenic
Main isotopes[10] Decay
abun­dance half-life (t1/2) mode pro­duct
73As synth 80.3 d ε 73Ge
γ –
74As synth 17.8 d ε 74Ge
β+ 74Ge
γ –
β− 74Se
75As 100% stable
 Category: Arsenic
| references

Arsenic (/[invalid input: 'icon']ˈɑːrs[invalid input: 'i-']nɪk/ AR-sə-nik) is a chemical element with symbol As and atomic number 33. Arsenic occurs in many minerals, usually in conjunction with sulfur and metals, and also as a pure elemental crystal. It was first documented by Albertus Magnus in 1250.[11] Arsenic is a metalloid. It can exist in various allotropes, although only the gray form has important use in industry.

The main use of metallic arsenic is for strengthening alloys of copper and especially lead (for example, in car batteries). Arsenic is a common n-type dopant in semiconductor electronic devices, and the optoelectronic compound gallium arsenide is the most common semiconductor in use after doped silicon. Arsenic and its compounds, especially the trioxide, are used in the production of pesticides (treated wood products), herbicides, and insecticides. These applications are declining, however.[12]

Arsenic is notoriously poisonous to multicellular life, although a few species of bacteria are able to use arsenic compounds as respiratory metabolites. Arsenic contamination of groundwater is a problem that affects millions of people across the world.

Characteristics

Physical characteristics

Crystal structure common to Sb, AsSb and gray As

The three most common arsenic allotropes are metallic gray, yellow and black arsenic, with gray being the most common.[13] Gray arsenic (α-As, space group R3m No. 166) adopts a double-layered structure consisting of many interlocked ruffled six-membered rings. Because of weak bonding between the layers, gray arsenic is brittle and has a relatively low Mohs hardness of 3.5. Nearest and next-nearest neighbors form a distorted octahedral complex, with the three atoms in the same double-layer being slightly closer than the three atoms in the next.[14] This relatively close packing leads to a high density of 5.73 g/cm3.[15] Gray arsenic is a semimetal, but becomes a semiconductor with a bandgap of 1.2–1.4 eV if amorphized.[16] Yellow arsenic is soft and waxy, and somewhat similar to tetraphosphorus (P
4). Both have four atoms arranged in a tetrahedral structure in which each atom is bound to each of the other three atoms by a single bond. This unstable allotrope, being molecular, is the most volatile, least dense and most toxic. Solid yellow arsenic is produced by rapid cooling of arsenic vapor, As
4. It is rapidly transformed into the gray arsenic by light. The yellow form has a density of 1.97 g/cm3.[15] Black arsenic is similar in structure to red phosphorus.[15]

Isotopes

Main article: Isotopes of arsenic

Naturally occurring arsenic is composed of one stable isotope, 75As.[17] As of 2003, at least 33 radioisotopes have also been synthesized, ranging in atomic mass from 60 to 92. The most stable of these is 73As with a half-life of 80.3 days. Isotopes that are lighter than the stable 75As tend to decay by β+ decay, and those that are heavier tend to decay by β- decay, with some exceptions.

At least 10 nuclear isomers have been described, ranging in atomic mass from 66 to 84. The most stable of arsenic's isomers is 68mAs with a half-life of 111 seconds.[17]

Chemistry

When heated in air, arsenic oxidizes to arsenic trioxide; the fumes from this reaction have an odor resembling garlic. This odor can be detected on striking arsenide minerals such as arsenopyrite with a hammer. Arsenic (and some arsenic compounds) sublimes upon heating at atmospheric pressure, converting directly to a gaseous form without an intervening liquid state at 887 K (614 °C).[4] The triple point is 3.63 MPa and 1,090 K (820 °C).[15][4] Arsenic makes arsenic acid with concentrated nitric acid, arsenious acid with dilute nitric acid, and arsenic trioxide with concentrated sulfuric acid.[18]

Arsenic burning in the air

Compounds

See also: Category:Arsenic compounds

Arsenic compounds resemble in some respects those of phosphorus, which occupies the same group (column) of the periodic table. Arsenic is less commonly observed in the pentavalent state, however. The most common oxidation states for arsenic are: −3 in the arsenides, such as alloy-like intermetallic compounds; and +3 in the arsenites, arsenates(III), and most organoarsenic compounds. Arsenic also bonds readily to itself as seen in the square As3−
4 ions in the mineral skutterudite. In the +3 oxidation state, arsenic is typically pyramidal, owing to the influence of the lone pair of electrons.

Inorganic

Arsenic forms colorless, odorless, crystalline oxides As2O3 ("white arsenic") and As2O5, which are hygroscopic and readily soluble in water to form acidic solutions. Arsenic(V) acid is a weak acid. Its salts are called arsenates, which is the basis of arsenic contamination of groundwater, a problem that affects many people. Synthetic arsenates include Paris Green (copper(II) acetoarsenite), calcium arsenate, and lead hydrogen arsenate. The latter three have been used as agricultural insecticides and poisons.

The protonation steps between the arsenate and arsenic acid are similar to those between phosphate and phosphoric acid. Unlike phosphorus acid, arsenous acid is genuinely tribasic, with the formula As(OH)3.

A broad variety of sulfur compounds of arsenic are known. Orpiment (As2S3) and realgar (As4S4) are somewhat abundant and were formerly used as painting pigments. In As4S10, arsenic has a formal oxidation state of +2 in As4S4, which features As-As bonds so that the total covalency of As is still three.[19]

The trifluoride, trichloride, tribromide, and triiodide of arsenic(III) are well known, whereas only Arsenic pentafluoride (AsF5) is the only important pentahalide. Again reflecting the lower stability of the 5+ oxidation state, the pentachloride is stable only below −50 °C.[15]

Organoarsenic compounds

Main article: organoarsenic chemistry
Trimethylarsine

A large variety of organoarsenic compounds are known. Several were developed as chemical warfare agents during World War I, including vesicants such as lewisite and vomiting agents such as adamsite.[20][21][22] Cacodylic acid, which is of historic and practical interest, arises from the methylation of arsenic trioxide, a reaction that has no analogy in phosphorus chemistry.

Alloys

Arsenic is used as the group 5 element in the III-V semiconductors gallium arsenide, indium arsenide, and aluminium arsenide. The valence electron count of GaAs is the same as a pair of Si atoms, but the band structure is completely different, which results distinct bulk properties. Other arsenic alloys include the II-IV semiconductor cadmium arsenide.

Occurrence and production

See also: Arsenide minerals and Arsenate minerals
A large sample of native arsenic

Minerals with the formula MAsS and MAs2 (M = Fe, Ni, Co) are the dominant commercial sources of arsenic, together with realgar (an arsenic sulfide mineral) and native arsenic. An illustrative mineral is arsenopyrite (FeAsS), which is structurally related to iron pyrite. Many minor As-containing minerals are known. Arsenic also occurs in various organic forms in the environment.[23] Inorganic arsenic and its compounds, upon entering the food chain, are progressively metabolized to a less toxic form of arsenic through a process of methylation.[24]

Other naturally occurring pathways of exposure include volcanic ash, weathering of arsenic-containing minerals and ores, and dissolved in groundwater. It is also found in food, water, soil, and air.[25] Arsenic is absorbed by all plants, but is more concentrated in leafy vegetables, rice, apple and grape juice, and seafood.[26] An additional route of exposure is through inhalation.[27]

Arsenic output in 2006[28]

In 2005, China was the top producer of white arsenic with almost 50% world share, followed by Chile, Peru, and Morocco, according to the British Geological Survey and the United States Geological Survey.[28] Most operations in the US and Europe have closed for environmental reasons. The arsenic is recovered mainly as a side product from the purification of copper. Arsenic is part of the smelter dust from copper, gold, and lead smelters.[29]

On roasting in air of arsenopyrite, arsenic sublimes as arsenic(III) oxide leaving iron oxides,[23] while roasting without air results in the production of metallic arsenic. Further purification from sulfur and other chalcogens is achieved by sublimation in vacuum or in a hydrogen atmosphere or by distillation from molten lead-arsenic mixture.[30]

History

Realgar
Alchemical symbol for arsenic

The word arsenic was borrowed from the Syriac word ܠܐ ܙܐܦܢܝܐ (al) zarniqa[31] and the Persian word زرنيخ Zarnikh, meaning "yellow orpiment", into Greek as arsenikon (Αρσενικόν). It is also related to the similar Greek word arsenikos (Αρσενικός), meaning "masculine" or "potent". The word was adopted in Latin arsenicum and Old French arsenic, from which the English word arsenic is derived.[31] Arsenic sulfides (orpiment, realgar) and oxides have been known and used since ancient times.[32] Zosimos (circa 300 AD) describes roasting sandarach (realgar) to obtain cloud of arsenic (arsenious oxide), which he then reduces to metallic arsenic.[33] As the symptoms of arsenic poisoning were somewhat ill-defined, it was frequently used for murder until the advent of the Marsh test, a sensitive chemical test for its presence. (Another less sensitive but more general test is the Reinsch test.) Owing to its use by the ruling class to murder one another and its potency and discreetness, arsenic has been called the Poison of Kings and the King of Poisons.[34]

During the Bronze Age, arsenic was often included in bronze, which made the alloy harder (so-called "arsenical bronze").[35][36] Albertus Magnus (Albert the Great, 1193–1280) is believed to have been the first to isolate the element from a compound in 1250, by heating soap together with arsenic trisulfide.[11] In 1649, Johann Schröder published two ways of preparing arsenic.[37] Crystals of elemental (native) arsenic are found in nature, although rare.

Cadet's fuming liquid (impure cacodyl), often claimed as the first synthetic organometallic compound, was synthesized in 1760 by Louis Claude Cadet de Gassicourt by the reaction of potassium acetate with arsenic trioxide.[38]

In the Victorian era, "arsenic" ("white arsenic" or arsenic trioxide) was mixed with vinegar and chalk and eaten by women to improve the complexion of their faces, making their skin paler to show they did not work in the fields. Arsenic was also rubbed into the faces and arms of women to "improve their complexion". The accidental use of arsenic in the adulteration of foodstuffs led to the Bradford sweet poisoning in 1858, which resulted in approximately 20 deaths.[39]

Applications

Agricultural

Roxarsone is a controversial arsenic compound used as a nutritional supplement for chickens

The toxicity of arsenic to insects, bacteria and fungi led to its use as a wood preservative.[40] In the 1950s a process of treating wood with chromated copper arsenate (also known as CCA or Tanalith) was invented, and for decades this treatment was the most extensive industrial use of arsenic. An increased appreciation of the toxicity of arsenic resulted in a ban for the use of CCA in consumer products; the European Union and United States initiated this process in 2004.[41][42] CCA remains in heavy use in other countries however, e.g. Malaysian rubber plantations.[12]

Arsenic was also used in various agricultural insecticides, termination and poisons. For example, lead hydrogen arsenate was a common insecticide on fruit trees,[43] but contact with the compound sometimes resulted in brain damage among those working the sprayers. In the second half of the 20th century, monosodium methyl arsenate (MSMA) and disodium methyl arsenate (DSMA) – less toxic organic forms of arsenic – have replaced lead arsenate in agriculture.

Arsenic is still added to animal food, in particular in the US as a method of disease prevention[44][45] and growth stimulation. One example is roxarsone, which is used as a broiler starter by about 70% of the broiler growers since 1995.[46] The Poison-Free Poultry Act of 2009 proposes to ban the use of roxarsone in industrial swine and poultry production.[47] Alpharma, a subsidiary of Pfizer Inc., which produces Roxarsone, has voluntarily suspended sales of the drug in response to studies showing elevated levels of arsenic in treated chickens.[48]

Medical use

During the 18th, 19th, and 20th centuries, a number of arsenic compounds have been used as medicines, including arsphenamine (by Paul Ehrlich) and arsenic trioxide (by Thomas Fowler). Arsphenamine as well as neosalvarsan was indicated for syphilis and trypanosomiasis, but has been superseded by modern antibiotics. Arsenic trioxide has been used in a variety of ways over the past 500 years, but most commonly in the treatment of cancer. The US Food and Drug Administration in 2000 approved this compound for the treatment of patients with acute promyelocytic leukemia that is resistant to ATRA.[49] It was also used as Fowler's solution in psoriasis.[50] Recently new research has been done in locating tumors using arsenic-74 (a positron emitter). The advantages of using this isotope instead of the previously used iodine-124 is that the signal in the PET scan is clearer as the body tends to transport iodine to the thyroid gland producing a lot of noise.[51]

In subtoxic doses, soluble arsenic compounds act as stimulants, and were once popular in small doses as medicine by people in the mid-18th century.[15]

Alloys

The main use of metallic arsenic is for alloying with lead. Lead components in car batteries are strengthened by the presence of a few percent of arsenic.[12][52] Dezincification can be strongly reduced by adding arsenic to brass a copper zinc alloy.[53] Gallium arsenide is an important semiconductor material, used in integrated circuits. Circuits made from GaAs are much faster (but also much more expensive) than those made in silicon. Unlike silicon it has a direct bandgap, and so can be used in laser diodes and LEDs to directly convert electricity into light.[12]

Military

After World War I, the United States built up a stockpile of 20,000 tonnes of lewisite (ClCH=CHAsCl2), a chemical weapon that is a vesicant (blister agent) and lung irritant. The stockpile was neutralized with bleach and dumped into the Gulf of Mexico after the 1950s.[54] During the Vietnam War the United States used Agent Blue, a mixture of sodium cacodylate and its acid form, as one of the rainbow herbicides to deprive invading North Vietnamese soldiers of foliage cover and rice.[55][56]

Other uses

  • Copper acetoarsenite was used as a green pigment known under many names, including 'Paris Green' and 'Emerald Green'. It caused numerous arsenic poisonings. Scheele's Green, a copper arsenate, was used in the 19th century as a coloring agent in sweets.[57]
  • Also used in bronzing[58] and pyrotechnics.
  • Up to 2% of arsenic is used in lead alloys for lead shots and bullets.[59]
  • Arsenic is added in small quantities to alpha-brass to make it dezincification resistant. This grade of brass is used to make plumbing fittings or other items that are in constant contact with water.[60]
  • Arsenic is also used for taxonomic sample preservation.
  • Until recently arsenic was used in optical glass. Modern glass manufacturers, under pressure from environmentalists, have removed it, along with lead.[61]

Biological role

Main article: Arsenic biochemistry

Bacteria

Arsenobetaine

Some species of bacteria obtain their energy by oxidizing various fuels while reducing arsenate to arsenite. Under oxidative environmental conditions some bacteria use arsenite, which is oxidized to arsenate as fuel for their metabolism.[62] The enzymes involved are known as arsenate reductases (Arr).

In 2008, bacteria were discovered that employ a version of photosynthesis in the absence of oxygen with arsenites as electron donors, producing arsenates (just as ordinary photosynthesis uses water as electron donor, producing molecular oxygen). Researchers conjecture that, over the course of history, these photosynthesizing organisms produced the arsenates that allowed the arsenate-reducing bacteria to thrive. One strain PHS-1 has been isolated and is related to the Gammaproteobacterium Ectothiorhodospira shaposhnikovii. The mechanism is unknown, but an encoded Arr enzyme may function in reverse to its known homologues.[63]

Although the arsenate and phosphate anions are similar structurally, no evidence exists for the replacement of phosphate in ATP or nucleic acids by arsenic.[64]

Heredity

Arsenic has been linked to epigenetic changes, heritable changes in gene expression that occur without changes in DNA sequence. These include DNA methylation, histone modification, and RNA interference. Toxic levels of arsenic cause significant DNA hypermethylation of tumor suppressor genes p16 and p53, thus increasing risk of carcinogenesis. These epigenetic events have been studied in vitro using human kidney cells and in vivo using rat liver cells and peripheral blood leukocytes in humans.[65] Inductive coupled plasma mass spectrometry (ICP-MS) is used to detect precise levels of intracellular arsenic and its other bases involved in epigenetic modification of DNA.[66] Studies investigating arsenic as an epigenetic factor will help in developing precise biomarkers of exposure and susceptibility.

The Chinese brake fern (Pteris vittata) hyperaccumulates arsenic present in the soil into its leaves and has a proposed use in phytoremediation.[67]

Biomethylation

Inorganic arsenic and its compounds, upon entering the food chain, are progressively metabolized through a process of methylation.[68] For example, the mold Scopulariopsis brevicaulis produce significant amounts of trimethylarsine if inorganic arsenic is present.[69] The organic compound arsenobetaine is found in some marine foods such as fish and algae, and also in mushrooms in larger concentrations. The average person's intake is about 10–50 µg/day. Values about 1000 µg are not unusual following consumption of fish or mushrooms, but there is little danger in eating fish because this arsenic compound is nearly non-toxic.[70]

Environmental issues

Occurrence in drinking water

Main article: Arsenic contamination of groundwater

Widespread arsenic contamination of groundwater has led to a massive epidemic of arsenic poisoning in Bangladesh[71] and neighboring countries. It is estimated that approximately 57 million people in the Bengal basin are drinking groundwater with arsenic concentrations elevated above the World Health Organization's standard of 10 parts per billion (ppb).[72] However, a study of cancer rates in Taiwan[73] suggested that significant increases in cancer mortality appear only at levels above 150 ppb. The arsenic in the groundwater is of natural origin, and is released from the sediment into the groundwater, owing to the anoxic conditions of the subsurface. This groundwater began to be used after local and western NGOs and the Bangladeshi government undertook a massive shallow tube well drinking-water program in the late twentieth century. This program was designed to prevent drinking of bacteria-contaminated surface waters, but failed to test for arsenic in the groundwater. Many other countries and districts in Southeast Asia, such as Vietnam and Cambodia have geological environments conducive to generation of high-arsenic groundwaters. Arsenicosis was reported in Nakhon Si Thammarat, Thailand in 1987, and the dissolved arsenic in the Chao Phraya River is suspected of containing high levels of naturally occurring arsenic, but has not been a public health problem owing to the use of bottled water.[74]

In the United States, arsenic is most commonly found in the ground waters of the southwest.[75] Parts of New England, Michigan, Wisconsin, Minnesota and the Dakotas are also known to have significant concentrations of arsenic in ground water.[76] Increased levels of skin cancer have been associated with arsenic exposure in Wisconsin, even at levels below the 10 part per billion drinking water standard, although this link has not been proven.[77] According to a recent film funded by the US Superfund, millions of private wells have unknown arsenic levels, and in some areas of the US, over 20% of wells may contain levels that exceed established limits.[78]

Low-level exposure to arsenic at concentrations found commonly in US drinking water compromises the initial immune response to H1N1 or swine flu infection according to NIEHS-supported scientists. The study, conducted in laboratory mice, suggests that people exposed to arsenic in their drinking water may be at increased risk for more serious illness or death in response to infection from the virus.[79]

Epidemiological evidence from Chile shows a dose-dependent connection between chronic arsenic exposure and various forms of cancer, in particular when other risk factors, such as cigarette smoking, are present. These effects have been demonstrated to persist below 50 ppb.[80]

Analyzing multiple epidemiological studies on inorganic arsenic exposure suggests a small but measurable risk increase for bladder cancer at 10 ppb.[81] According to Peter Ravenscroft of the Department of Geography at the University of Cambridge,[82] roughly 80 million people worldwide consume between 10 and 50 ppb arsenic in their drinking water. If they all consumed exactly 10 ppb arsenic in their drinking water, the previously cited multiple epidemiological study analysis would predict an additional 2,000 cases of bladder cancer alone. This represents a clear underestimate of the overall impact, since it does not include lung or skin cancer, and explicitly underestimates the exposure. Those exposed to levels of arsenic above the current WHO standard should weigh the costs and benefits of arsenic remediation.

Early (1973) evaluations of the removal of dissolved arsenic by drinking water treatment processes demonstrated that arsenic is very effectively removed by co-precipitation with either iron or aluminum oxides. The use of iron as a coagulant, in particular, was found to remove arsenic with efficiencies exceeding 90%.[83][84] Several adsorptive media systems have been approved for point-of-service use in a study funded by the United States Environmental Protection Agency (US EPA) and the National Science Foundation (NSF). A team of European and Indian scientists and engineers have set up six arsenic treatment plants in West Bengal based on in-situ remediation method (SAR Technology). This technology does not use any chemicals and arsenic is left as an insoluble form (+5 state) in the subterranean zone by recharging aerated water into the aquifer and thus developing an oxidation zone to support arsenic oxidizing micro-organisms. This process does not produce any waste stream or sludge and is relatively cheap.[85]

Another effective and inexpensive method to remove arsenic from contaminated well water is to sink wells 500 feet or deeper to reach purer waters. A recent 2011 study funded by the US National Institute of Environmental Health Sciences' Superfund Research Program shows that deep sediments can remove arsenic and take it out of circulation. Through this process called adsorption in which arsenic sticks to the surfaces of deep sediment articles, arsenic can be naturally removed from well water.[86]

Magnetic separations of arsenic at very low magnetic field gradients have been demonstrated in point-of-use water purification with high-surface-area and monodisperse magnetite (Fe3O4) nanocrystals. Using the high specific surface area of Fe3O4 nanocrystals the mass of waste associated with arsenic removal from water has been dramatically reduced.[87]

Epidemiological studies have suggested a correlation between chronic consumption of drinking water contaminated with arsenic and the incidence of all leading causes of mortality.[88] The literature provides reason to believe arsenic exposure is causative in the pathogenesis of diabetes.[89]

Hungarian engineer László Schremmer has recently discovered that by the use of chaff-based filters it is possible to reduce the arsenic content of water to 3 µg/L. This is especially important in areas where the potable water is provided by filtering the water extracted from the underground aquifer.[90]

Wood preservation in the US

As of 2002, US-based industries consumed 19,600 metric tons of arsenic. Ninety percent of this was used for treatment of wood with chromated copper arsenate (CCA). In 2007, 50% of the 5,280 metric tons of consumption was still used for this purpose.[29][91] In the United States, the use of arsenic in consumer products was discontinued for residential, and general consumer construction on December 31, 2003 and alternative chemicals are now used, such as Alkaline Copper Quaternary, borates, copper azole, cyproconazole, and propiconazole.[92]

Although discontinued, this application is also one of the most concern to the general public. The vast majority of older pressure-treated wood was treated with CCA. CCA lumber is still in widespread use in many countries, and was heavily used during the latter half of the 20th century as a structural and outdoor building material. Although the use of CCA lumber was banned in many areas after studies showed that arsenic could leach out of the wood into the surrounding soil (from playground equipment, for instance), a risk is also presented by the burning of older CCA timber. The direct or indirect ingestion of wood ash from burnt CCA lumber has caused fatalities in animals and serious poisonings in humans; the lethal human dose is approximately 20 grams of ash. Scrap CCA lumber from construction and demolition sites may be inadvertently used in commercial and domestic fires. Protocols for safe disposal of CCA lumber do not exist evenly throughout the world; there is also concern in some quarters about the widespread landfill disposal of such timber.

Mapping of industrial releases in the US

One tool that maps releases of arsenic to particular locations in the United States[93] and also provides additional information about such releases is TOXMAP. TOXMAP is a Geographic Information System (GIS) from the Division of Specialized Information Services of the United States National Library of Medicine (NLM) that uses maps of the United States to help users visually explore data from the United States Environmental Protection Agency's (EPA) Toxics Release Inventory and Superfund Basic Research Programs. TOXMAP is a resource funded by the US Federal Government. TOXMAP's chemical and environmental health information is taken from NLM's Toxicology Data Network (TOXNET)[94] and PubMed, and from other authoritative sources.

Toxicity and precautions

Main articles: Arsenic poisoning and Arsenic toxicity

Arsenic and many of its compounds are especially potent poisons. Many water supplies close to mines are contaminated by these poisons. In the United States, the maximum allowed concentration in drinking water is 10 ppb and 5 ppb for bottled water.[95] There is no standard for food, though in 2012 press coverage prompted calls for developing such.[95] The People's Republic of China does have a food standard.[95]

Elemental arsenic and arsenic compounds are classified as "toxic" and "dangerous for the environment" in the European Union under directive 67/548/EEC. The International Agency for Research on Cancer (IARC) recognizes arsenic and arsenic compounds as group 1 carcinogens, and the EU lists arsenic trioxide, arsenic pentoxide and arsenate salts as category 1 carcinogens.

Arsenic is known to cause arsenicosis owing to its manifestation in drinking water, "the most common species being arsenate [HAsO2−
4; As(V)] and arsenite [H3AsO3; As(III)]".

Treatment

Treatment of chronic arsenic poisoning is easily accomplished. British anti-lewisite (dimercaprol) is prescribed in dosages of 5 mg/kg up to 300 mg each 4 hours for the first day. Then administer the same dosage each 6 hours for the second day. Then prescribe this dosage each 8 hours for eight additional days.[96] However the USA's Agency for Toxic Substances and Disease Registry (ATSDR) states that the long-term effects of arsenic exposure cannot be predicted.[27] Blood, urine, hair, and nails may be tested for arsenic; however, these tests cannot foresee possible health outcomes from the exposure.[27] Excretion occurs in the urine and long-term exposure to arsenic has been linked to bladder and kidney cancer in addition to cancer of the liver, prostate, skin, lungs and nasal cavity.[97]

Exposure risks and remediation

Occupational exposure and arsenic poisoning may occur in persons working in industries involving the use of inorganic arsenic and its compounds, such as wood preservation, glass production, nonferrous metal alloys, and electronic semiconductor manufacturing. Inorganic arsenic is also found in coke oven emissions associated with the smelter industry.[98]

The ability of arsenic to undergo redox conversion between As(III) and As(V) makes its availability in the environment more abundant. According to Croal, Gralnick, Malasarn and Newman, "[the] understanding [of] what stimulates As(III) oxidation and/or limits As(V) reduction is relevant for bioremediation of contaminated sites (Croal). The study of chemolithoautotrophic As(III) oxidizers and the heterotrophic As(V) reducers can help the understanding of the oxidation and/or reduction of arsenic.[99]

Biological mechanism

The high affinity of arsenic(III) oxides for thiols is usually assigned as the cause of the high toxicity. Thiols, usually in the form of cysteine residues, but also in cofactors such as lipoic acid and coenzyme A, are situated at the active sites of many important enzymes.[12]

Arsenic disrupts ATP production through several mechanisms. At the level of the citric acid cycle, arsenic inhibits lipoic acid, which is a cofactor for pyruvate dehydrogenase. In addition, by competing with phosphate, arsenate uncouples oxidative phosphorylation, thus inhibiting energy-linked reduction of NAD+, mitochondrial respiration and ATP synthesis. Hydrogen peroxide production is also increased, which, it is speculated, has potential to form reactive oxygen species and oxidative stress. These metabolic interferences lead to death from multi-system organ failure. The organ failure is presumed to be from necrotic cell death, not apoptosis, since energy reserves have been too depleted for apoptosis to occur.

A post mortem in an arsenic poisoning death reveals brick-red-colored mucosa, owing to severe hemorrhage.

Although arsenic causes toxicity, it can also play a protective role.[100]

See also

Template:Wikipedia books

References

  1. ^ "Standard Atomic Weights: Arsenic". CIAAW. 2013.
  2. ^ Prohaska, Thomas; Irrgeher, Johanna; Benefield, Jacqueline; Böhlke, John K.; Chesson, Lesley A.; Coplen, Tyler B.; Ding, Tiping; Dunn, Philip J. H.; Gröning, Manfred; Holden, Norman E.; Meijer, Harro A. J. (2022-05-04). "Standard atomic weights of the elements 2021 (IUPAC Technical Report)". Pure and Applied Chemistry. doi:10.1515/pac-2019-0603. ISSN 1365-3075.
  3. ^ a b Arblaster, John W. (2018). Selected Values of the Crystallographic Properties of Elements. Materials Park, Ohio: ASM International. ISBN 978-1-62708-155-9.
  4. ^ a b c Gokcen, N. A (1989). "The As (arsenic) system". Bull. Alloy Phase Diagrams. 10: 11–22. doi:10.1007/BF02882166.
  5. ^ Abraham, Mariham Y.; Wang, Yuzhong; Xie, Yaoming; Wei, Pingrong; Shaefer III, Henry F.; Schleyer, P. von R.; Robinson, Gregory H. (2010). "Carbene Stabilization of Diarsenic: From Hypervalency to Allotropy". Chemistry: A European Journal. 16 (2): 432–5. doi:10.1002/chem.200902840. PMID 19937872.
  6. ^ Ellis, Bobby D.; MacDonald, Charles L. B. (2004). "Stabilized Arsenic(I) Iodide: A Ready Source of Arsenic Iodide Fragments and a Useful Reagent for the Generation of Clusters". Inorganic Chemistry. 43 (19): 5981–6. doi:10.1021/ic049281s. PMID 15360247.
  7. ^ Cverna, Fran (2002). ASM Ready Reference: Thermal properties of metals. ASM International. pp. 8–. ISBN 978-0-87170-768-0. pdf.
  8. ^ Lide, David R., ed. (2000). "Magnetic susceptibility of the elements and inorganic compounds". Handbook of Chemistry and Physics (PDF) (81 ed.). CRC press. ISBN 0849304814.
  9. ^ Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN 0-8493-0464-4.
  10. ^ Kondev, F. G.; Wang, M.; Huang, W. J.; Naimi, S.; Audi, G. (2021). "The NUBASE2020 evaluation of nuclear properties" (PDF). Chinese Physics C. 45 (3): 030001. doi:10.1088/1674-1137/abddae.
  11. ^ a b Emsley, John (2001). Nature's Building Blocks: An A-Z Guide to the Elements. Oxford: Oxford University Press. pp. 43, 513, 529. ISBN 0-19-850341-5.
  12. ^ a b c d e Sabina C. Grund, Kunibert Hanusch, Hans Uwe Wolf. "Arsenic and Arsenic Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a03_113.pub2. ISBN 978-3527306732.{{cite encyclopedia}}: CS1 maint: multiple names: authors list (link)
  13. ^ Norman, Nicholas C (1998). Chemistry of Arsenic, Antimony and Bismuth. Springer. p. 50. ISBN 978-0-7514-0389-3.
  14. ^ Biberg, Egon; Wiberg, Nils; Holleman, Arnold Frederick (2001). Inorganic Chemistry. Academic Press. ISBN 978-0-12-352651-9.
  15. ^ a b c d e f Holleman, Arnold F. (1985). "Arsen". Lehrbuch der Anorganischen Chemie (in German) (91–100 ed.). Walter de Gruyter. pp. 675–681. ISBN 3-11-007511-3. {{cite book}}: Unknown parameter |coauthors= ignored (|author= suggested) (help)
  16. ^ Madelung, Otfried (2004). Semiconductors: data handbook. Birkhäuser. pp. 410–. ISBN 978-3-540-40488-0. Retrieved 24 October 2011.
  17. ^ a b Georges, Audi; Bersillon, O.; Blachot, J.; Wapstra, A.H. (2003). "The NUBASE Evaluation of Nuclear and Decay Properties". Nuclear Physics A. 729. Atomic Mass Data Center: 3–128. Bibcode:2003NuPhA.729....3A. doi:10.1016/j.nuclphysa.2003.11.001.
  18. ^  Chisholm, Hugh, ed. (1911). "Arsenic". Encyclopædia Britannica (11th ed.). Cambridge University Press.
  19. ^ "Arsenic: arsenic(II) sulfide compound data". WebElements.com. Archived from the original on 11 December 2007. Retrieved 2007-12-10. {{cite web}}: Unknown parameter |deadurl= ignored (|url-status= suggested) (help)
  20. ^ Ellison, Hank D. (2007). Handbook of chemical and biological warfare agents. CRC Press. ISBN 978-0-8493-1434-6.
  21. ^ Girard, James (2010). Principles of Environmental Chemistry. Jones & Bartlett Learning. ISBN 978-0-7637-5939-1.
  22. ^ Somani, Satu M (2001). Chemical warfare agents: toxicity at low levels. CRC Press. ISBN 978-0-8493-0872-7.
  23. ^ a b Matschullat, Jörg (2000). "Arsenic in the geosphere — a review". The Science of the Total Environment. 249 (1–3): 297–312. doi:10.1016/S0048-9697(99)00524-0. PMID 10813460.
  24. ^ Reimer, K.J. (2010). "Organoarsenicals. Distribution and transformation in the environment". Metal ions in life sciences. 7: 165–229. doi:10.1039/BK9781847551771-00165. ISBN 978-1-84755-177-1. PMID 20877808. {{cite journal}}: Unknown parameter |coauthors= ignored (|author= suggested) (help)
  25. ^ "Case Studies in Environmental Medicine (CSEM) Arsenic Toxicity Exposure Pathways" (PDF). Agency for Toxic Substances & Disease Registry. Retrieved 2010-05-15.
  26. ^ "Arsenic in Food: FAQ". 2011-12-05. Retrieved 2012-04-11.
  27. ^ a b c Arsenic. The Agency for Toxic Substances and Disease Registry (2009).
  28. ^ a b Brooks, William E. "Mineral Commodity Summaries 2007: Arsenic" (PDF). United States Geological Survey. Archived from the original (PDF) on 17 December 2008. Retrieved 2008-11-25. {{cite web}}: Unknown parameter |deadurl= ignored (|url-status= suggested) (help)
  29. ^ a b Brooks, William E. "Minerals Yearbook 2007: Arsenic" (PDF). United States Geological Survey. Archived from the original (PDF) on 17 December 2008. Retrieved 2008-11-08. {{cite web}}: Unknown parameter |deadurl= ignored (|url-status= suggested) (help)
  30. ^ Whelan, J. M.; Struthers, J. D.; Ditzenberger, J. A. (1960). "Separation of Sulfur, Selenium, and Tellurium from Arsenic". Journal of the Electrochemical Society. 107 (12): 982–985. doi:10.1149/1.2427585.
  31. ^ a b "arsenic". Online Etymology Dictionary. Retrieved 2010-05-15.
  32. ^ Bentley, Ronald; Chasteen, Thomas G. (2002). "Arsenic Curiosa and Humanity" (PDF). The Chemical Educator. 7 (2): 51. doi:10.1007/s00897020539a.
  33. ^ Holmyard John Eric (2007). Makers of Chemistry. Read Books. ISBN 1-4067-3275-3.
  34. ^ Vahidnia, A.; Van Der Voet, G. B.; De Wolff, F. A. (2007). "Arsenic neurotoxicity – a review". Human & Experimental Toxicology. 26 (10): 823–32. doi:10.1177/0960327107084539. PMID 18025055.
  35. ^ Lechtman, H. (1996). "Arsenic Bronze: Dirty Copper or Chosen Alloy? A View from the Americas". Journal of Field Archaeology. 23 (4): 477–514. doi:10.2307/530550. JSTOR 530550.
  36. ^ Charles, J. A. (1967). "Early Arsenical Bronzes-A Metallurgical View". American Journal of Archaeology. 71 (1): 21–26. doi:10.2307/501586. JSTOR 501586.
  37. ^ (Comte), Antoine-François de Fourcroy (1804). A general system of chemical knowledge, and its application to the phenomena of nature and art. pp. 84–.
  38. ^ Seyferth, Dietmar (2001). "Cadet's Fuming Arsenical Liquid and the Cacodyl Compounds of Bunsen". Organometallics. 20 (8): 1488–1498. doi:10.1021/om0101947.
  39. ^ Turner, Alan (1999). "Viewpoint: the story so far: An overview of developments in UK food regulation and associated advisory committees". British Food Journal. 101 (4): 274–283. doi:10.1108/00070709910272141.
  40. ^ Rahman, FA; Allan, DL; Rosen, CJ; Sadowsky, MJ (2004). "Arsenic availability from chromated copper arsenate (CCA)-treated wood". Journal of environmental quality. 33 (1): 173–80. doi:10.2134/jeq2004.0173. PMID 14964372.
  41. ^ Lichtfouse, Eric (2004). "Electrodialytical Removal of Cu, Cr and As from Threaded Wood". Environmental Chemistry: Green Chemistry and Pollutants in Ecosystems. Berlin: Springer. ISBN 978-3-540-22860-8. {{cite book}}: Unknown parameter |editors= ignored (|editor= suggested) (help)
  42. ^ Mandal, Badal Kumar; Suzuki, K. T. (2002). "Arsenic round the world: a review". Talanta. 58 (1): 201–235. doi:10.1016/S0039-9140(02)00268-0. PMID 18968746.
  43. ^ Peryea, F. J. (20–26 August). Historical use of lead arsenate insecticides, resulting in soil contamination and implications for soil remediation. 16th World Congress of Soil Science. Montpellier, France. {{cite conference}}: Check date values in: |date= and |year= / |date= mismatch (help)
  44. ^ Nachman, Keeve E; Graham, Jay P.; Price, Lance B.; Silbergeld, Ellen K. (2005). "Arsenic: A Roadblock to Potential Animal Waste Management Solutions". Environmental Health Perspective. 113 (9): 1123–1124. doi:10.1289/ehp.7834.
  45. ^ "Arsenic. Section 5.3, p. 310" (PDF). Agency for Toxic Substances and Disease Registry.
  46. ^ Jones, F. T. (2007). "A Broad View of Arsenic". Poultry Science. 86 (1): 2–14. PMID 17179408.
  47. ^ Bottemiller, Helena (September 26, 2009). "Bill Introduced to Ban Arsenic Antibiotics in Feed". Food Safety News. Retrieved 2011-01-10.
  48. ^ "Questions and Answers Regarding 3-Nitro (Roxarsone)". U.S. Food and Drug Administration. June 8, 2011. Retrieved September 21, 2012. {{cite web}}: Cite has empty unknown parameter: |1= (help); Cite uses deprecated parameter |authors= (help)
  49. ^ Antman, Karen H. (2001). "The History of Arsenic Trioxide in Cancer Therapy". The oncologist. 6 (Suppl 2): 1–2. doi:10.1634/theoncologist.6-suppl_2-1. PMID 11331433.
  50. ^ Huet, P. M.; Guillaume, E.; Cote, J.; Légaré, A.; Lavoie, P.; Viallet, A. (1975). "Noncirrhotic presinusoidal portal hypertension associated with chronic arsenical intoxication". Gastroenterology. 68 (5 Pt 1): 1270–1277. PMID 1126603.
  51. ^ Jennewein, Marc; Lewis, M. A.; Zhao, D.; Tsyganov, E.; Slavine, N.; He, J.; Watkins, L.; Kodibagkar, V. D.; O'Kelly, S. (2008). "Vascular Imaging of Solid Tumors in Rats with a Radioactive Arsenic-Labeled Antibody that Binds Exposed Phosphatidylserine". Journal of Clinical Cancer. 14 (5): 1377–1385. doi:10.1158/1078-0432.CCR-07-1516. PMID 18316558.
  52. ^ Bagshaw, N.E. (1995). "Lead alloys: Past, present and future". Journal of Power Sources. 53: 25. doi:10.1016/0378-7753(94)01973-Y.
  53. ^ Joseph, Günter; Kundig, Konrad J. A; Association, International Copper (1999). "Dealloying". Copper: Its Trade, Manufacture, Use, and Environmental Status. pp. 123–124. ISBN 978-0-87170-656-0.
  54. ^ "Blister Agents". Code Red – Weapons of Mass Destruction. Retrieved 2010-05-15.
  55. ^ Westing, Arthur H. (1972). "Herbicides in war: Current status and future doubt". Biological Conservation. 4 (5): 322. doi:10.1016/0006-3207(72)90043-2.
  56. ^ Westing, Arthur H. (1971). "Forestry and the War in South Vietnam". Journal of Forestry. 69: 777–783.
  57. ^ Timbrell, John (2005). "Butter Yellow and Scheele's Green". The Poison Paradox: Chemicals as Friends and Foes. Oxford University Press. ISBN 978-0-19-280495-2.
  58. ^ Cross, J. D.; Dale, I. M.; Leslie, A. C. D.; Smith, H. (1979). "Industrial exposure to arsenic". Journal of Radioanalytical Chemistry. 48: 197. doi:10.1007/BF02519786.
  59. ^ Guruswamy, Sivaraman (1999). "XIV. Ammunition". Engineering Properties and Applications of Lead Alloys. CRC Press. pp. 569–570. ISBN 978-0-8247-8247-4.
  60. ^ Davis, Joseph R; Handbook Committee, ASM International (2001-08-01). "Dealloying". Copper and copper alloys. p. 390. ISBN 978-0-87170-726-0.
  61. ^ "Arsenic Supply Demand and the Environment". Pollution technology review 214: Mercury and arsenic wastes: removal, recovery, treatment, and disposal. William Andrew. 1993. p. 68. ISBN 978-0-8155-1326-1.
  62. ^ Stolz, John F.; Basu, Partha; Santini, Joanne M.; Oremland, Ronald S. (2006). "Arsenic and Selenium in Microbial Metabolism*". Annual Review of Microbiology. 60: 107–30. doi:10.1146/annurev.micro.60.080805.142053. PMID 16704340.
  63. ^ Kulp, T. R; Hoeft, S. E.; Asao, M.; Madigan, M. T.; Hollibaugh, J. T.; Fisher, J. C.; Stolz, J. F.; Culbertson, C. W.; Miller, L. G. (2008). "Arsenic(III) fuels anoxygenic photosynthesis in hot spring biofilms from Mono Lake, California". Science. 321 (5891): 967–970. Bibcode:2008Sci...321..967K. doi:10.1126/science.1160799. PMID 18703741. {{cite journal}}: Unknown parameter |laysource= ignored (help); Unknown parameter |laysummary= ignored (help)
  64. ^ T. J. Erb, P. Kiefer, B. Hattendorf, D. Günther and J. A. Vorholt, "GFAJ-1 Is an Arsenate-Resistant, Phosphate-Dependent Organism", Science 2012 doi:10.1126/science.1218455; M. L. Reaves, S. Sinha, J. D. Rabinowitz, L. Kruglyak and R. J. Redfield, "Absence of Detectable Arsenate in DNA from Arsenate-Grown GFAJ-1 Cells", Science 2012 doi:10.1126/science.1219861
  65. ^ Baccarelli, A.; Bollati, V. (2009). "Epigenetics and environmental chemicals". Current opinion in Pediatrics. 21 (2): 243–251. doi:10.1097/MOP.0b013e32832925cc. PMC 3035853. PMID 19663042.
  66. ^ Nicholis, I.; Curis, E.; Deschamps, P.; Bénazeth, S. (2009). "Arsenite medicinal use, metabolism, pharmacokinetics and monitoring in human hair". Biochimie. 91 (10): 12601267. doi:10.1016/j.biochi.2009.06.003. PMID 19527769. {{cite journal}}: More than one of |pages= and |page= specified (help)
  67. ^ Attention: This template ({{cite jstor}}) is deprecated. To cite the publication identified by jstor:1514012, please use {{cite journal}} with |jstor=1514012 instead.
  68. ^ Sakurai, Teruaki Sakurai (2003). "Biomethylation of Arsenic is Essentially Detoxicating Event". Journal of Health Science. 49 (3): 171–178. doi:10.1248/jhs.49.171.
  69. ^ Bentley, Ronald; Chasteen, TG (2002). "Microbial Methylation of Metalloids: Arsenic, Antimony, and Bismuth". Microbiology and Molecular Biology Reviews. 66 (2): 250–271. doi:10.1128/MMBR.66.2.250-271.2002. PMC 120786. PMID 12040126.
  70. ^ Cullen, William R; Reimer, Kenneth J. (1989). "Arsenic speciation in the environment". Chemical Reviews. 89 (4): 713–764. doi:10.1021/cr00094a002.
  71. ^ Meharg, Andrew (2005). Venomous Earth – How Arsenic Caused The World's Worst Mass Poisoning. Macmillan Science. ISBN 978-1-4039-4499-3.
  72. ^ Henke, Kevin R (2009-04-28). Arsenic: Environmental Chemistry, Health Threats and Waste Treatment. p. 317. ISBN 978-0-470-02758-5.
  73. ^ Lamm, S. H.; Engel, A.; Penn, C. A.; Chen, R.; Feinleib, M. (2006). "Arsenic cancer risk confounder in southwest Taiwan data set". Environ. Health Perspect. 114 (7): 1077–82. doi:10.1289/ehp.8704. PMC 1513326. PMID 16835062.
  74. ^ Kohnhorst, Andrew (2005). "Arsenic in Groundwater in Selected Countries in South and Southeast Asia: A Review" (PDF). J Trop Med Parasitol. 28: 73.
  75. ^ "Arsenic in Drinking Water: 3. Occurrence in U.S. Waters" (PDF). Retrieved 2010-05-15.
  76. ^ . doi:10.1111/j.1745-6584.2000.tb00251.x. {{cite journal}}: Cite journal requires |journal= (help); Missing or empty |title= (help)
  77. ^ Knobeloch, L. M.; Zierold, K. M.; Anderson, H. A. (2006). "Association of arsenic-contaminated drinking-water with prevalence of skin cancer in Wisconsin's Fox River Valley". J. Health Popul Nutr. 24 (2): 206–13. PMID 17195561.
  78. ^ "In Small Doses:Arsenic". The Dartmouth Toxic Metals Superfund Research Program. Dartmouth College.
  79. ^ Courtney, D; Ely, Kenneth H.; Enelow, Richard I.; Hamilton, Joshua W. (2009). "Low Dose Arsenic Compromises the Immune Response to Influenza A Infection in vivo". Environmental Health Perspectives. 117 (9): 1441–7. doi:10.1289/ehp.0900911. PMC 2737023. PMID 19750111. {{cite journal}}: More than one of |magazine= and |journal= specified (help)
  80. ^ Ferreccio, C.; Sancha, A. M. (2006). "Arsenic exposure and its impact on health in Chile". J Health Popul Nutr. 24 (2): 164–75. PMID 17195557.
  81. ^ Chu, H. A.; Crawford-Brown, D. J. (2006). "Inorganic arsenic in drinking water and bladder cancer: a meta-analysis for dose-response assessment". Int. J. Environ. Res. Public Health. 3 (4): 316–22. doi:10.3390/ijerph2006030039. PMID 17159272.{{cite journal}}: CS1 maint: unflagged free DOI (link)
  82. ^ "Arsenic in drinking water seen as threat - USATODAY.com". USA Today. 2007-08-30. Retrieved 2008-01-01.
  83. ^ Gulledge, John H.; O'Connor, John T. (1973). "Removal of Arsenic (V) from Water by Adsorption on Aluminum and Ferric Hydroxides". J. American Water Works Assn. 65 (8): 548–552.
  84. ^ O'Connor, J. T.; O'Connor, T. L. "Arsenic in Drinking Water: 4. Removal Methods" (PDF).
  85. ^ "In situ arsenic treatment". insituarsenic.org. Retrieved 2010-05-13.
  86. ^ Radloff, K. A.; Zheng, Y.; Michael, H. A.; Stute, M.; Bostick, B. C.; Mihajlov, I.; Bounds, M.; Huq, M. R.; Choudhury, I. (2011). "Arsenic migration to deep groundwater in Bangladesh influenced by adsorption and water demand". Nature Geoscience. 4 (11): 793–798. Bibcode:2011NatGe...4..793R. doi:10.1038/ngeo1283. PMC 3269239. PMID 22308168.
  87. ^ Yavuz, Cafer T; Mayo, J. T.; Yu, W. W.; Prakash, A.; Falkner, J. C.; Yean, S.; Cong, L.; Shipley, H. J.; Kan, A. (2005). "Low-Field Magnetic Separation of Monodisperse Fe3O4 Nanocrystals". Science. 314 (5801): 964–967. doi:10.1126/science.1131475. PMID 17095696.
  88. ^ Meliker, JR; Wahl, RL; Cameron, LL; Nriagu, JO (2007). "Arsenic in drinking water and cerebrovascular disease, diabetes mellitus, and kidney disease in Michigan: A standardized mortality ratio analysis". Environmental Health. 6: 4. doi:10.1186/1476-069X-6-4. PMC 1797014. PMID 17274811.{{cite journal}}: CS1 maint: unflagged free DOI (link)
  89. ^ Tseng, Chin-Hsiao; Tai, Tong-Yuan; Chong, Choon-Khim; Tseng, Ching-Ping; Lai, Mei-Shu; Lin, Boniface J.; Chiou, Hung-Yi; Hsueh, Yu-Mei; Hsu, Kuang-Hung (2000). "Long-Term Arsenic Exposure and Incidence of Non-Insulin-Dependent Diabetes Mellitus: A Cohort Study in Arseniasis-Hyperendemic Villages in Taiwan". Environmental Health Perspectives. 108 (9): 847–51. doi:10.1289/ehp.00108847. PMC 2556925. PMID 11017889.
  90. ^ Newspaper article (in Hungarian) published by Magyar Nemzet on April 15, 2012.
  91. ^ Reese, Jr, Robert G. "Commodity Summaries 2002: Arsenic" (PDF). United States Geological Survey. Archived from the original (PDF) on 17 December 2008. Retrieved 2008-11-08. {{cite web}}: Unknown parameter |deadurl= ignored (|url-status= suggested) (help)
  92. ^ "Chromated Copper Arsenate (CCA)". US Environmental Protection Agency.
  93. ^ "TRI Releases Map". Toxmap.nlm.nih.gov. Archived from the original on 20 March 2010. Retrieved 2010-03-23. {{cite web}}: Unknown parameter |deadurl= ignored (|url-status= suggested) (help)
  94. ^ TOXNET – Databases on toxicology, hazardous chemicals, environmental health, and toxic releases. Toxnet.nlm.nih.gov. Retrieved on 2011-10-24.
  95. ^ a b c Lawmakers Urge FDA to Act on Arsenic Standards. Foodsafetynews.com (2012-02-24). Retrieved on 2012-05-23.
  96. ^ The Psychiatric, Psychogenic ans Somatopsychic Disorders Handbook. New Hyde Park, NY: Medical Examination Publishing Co. 1978. pp. 81–82. ISBN 0-87488-596-5.
  97. ^ The Tox Guide for Arsenic (2007). The US Agency for Toxic Substances and Disease Registry.
  98. ^ "OSHA Arsenic". United States Occupational Safety and Health Administration. Archived from the original on 12 October 2007. Retrieved 2007-10-08. {{cite web}}: Unknown parameter |deadurl= ignored (|url-status= suggested) (help)
  99. ^ Croal, Laura R.; Gralnick, Jeffrey A.; Malasarn, Davin; Newman, Dianne K. (2004). "The Genetics of Geochemisty". Annual Review of Genetics. 38: 175–206. doi:10.1146/annurev.genet.38.072902.091138. PMID 15568975.
  100. ^ Klaassen, Curtis; Watkins, John (2003). Casarett and Doull's Essentials of Toxicology. McGraw-Hill. p. 512. ISBN 978-0-07-138914-3.

Further reading

Wikimedia Commons has media related to Arsenic.
Look up arsenic in Wiktionary, the free dictionary.

Template:Link FA Template:Link GA

Retrieved from "https://en.wikipedia.org/w/index.php?title=Arsenic&oldid=515061418"