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The Regional Water Quality Control Board and the Santa Clara Valley Water District have engaged in a major outreach effort that has received extensive press and community response. A well testing program is underway for approximately 1,200 residential, municipal, and agricultural wells in the area. Large ion exchange treatment units are operating in three public water supply systems that include seven municipal wells where perchlorate has been detected. The potentially responsible parties, Olin Corporation and Standard Fuse Incorporated, are supplying bottled water to nearly 800 households with private wells. The Regional Water Quality Control Board is overseeing potentially responsible party (PRP) cleanup efforts.[http://www.epa.gov/region09/toxic/perchlorate/per_ca.html#olin]
The Regional Water Quality Control Board and the Santa Clara Valley Water District have engaged in a major outreach effort that has received extensive press and community response. A well testing program is underway for approximately 1,200 residential, municipal, and agricultural wells in the area. Large ion exchange treatment units are operating in three public water supply systems that include seven municipal wells where perchlorate has been detected. The potentially responsible parties, Olin Corporation and Standard Fuse Incorporated, are supplying bottled water to nearly 800 households with private wells. The Regional Water Quality Control Board is overseeing potentially responsible party (PRP) cleanup efforts.[http://www.epa.gov/region09/toxic/perchlorate/per_ca.html#olin]

==Perchlorate Cleanup==


===Ex situ and in situ treatments===
There are numerous technologies being utilized in treating perchlorate, including ex situ and in situ treatments. Some of ex situ treatments include ion exchange using perchlorate-selective or nitrite-specific resins, bioremediation using packed-bed or fluidized-bed bioreactors, and membrane technologies via electrodialysis and reverse osmosis.<ref name="Technical Fact Sheet – Perchlorate.">{{cite web|title=Technical Fact Sheet – Perchlorate.|url=http://www.epa.gov/fedfac/pdf/technical_fact_sheet_perchlorate.pdf|work=US EPA|publisher=US EPA}}</ref> In addition, ex situ technology of liquid phase carbon adsorption is employed, where granular activated carbon (GAC) is used in eliminating low levels of perchlorate and pretreatment may be required in arranging GAC for perchlorate elimination.<ref name="Technical Fact Sheet – Perchlorate.">{{cite web|title=Technical Fact Sheet – Perchlorate.|url=http://www.epa.gov/fedfac/pdf/technical_fact_sheet_perchlorate.pdf|work=US EPA|publisher=US EPA}}</ref> Furthermore, in situ treatments, such as bioremediation via perchlorate-selective microbes and permeable reactive barrier, are also being used to treat perchlorate.<ref name="Technical Fact Sheet – Perchlorate.">{{cite web|title=Technical Fact Sheet – Perchlorate.|url=http://www.epa.gov/fedfac/pdf/technical_fact_sheet_perchlorate.pdf|work=US EPA|publisher=US EPA}}</ref> In situ technology of phytoremediation could also be utilized, even though perchlorate phytoremediation mechanism is not fully founded yet.<ref name="Technical Fact Sheet – Perchlorate.">{{cite web|title=Technical Fact Sheet – Perchlorate.|url=http://www.epa.gov/fedfac/pdf/technical_fact_sheet_perchlorate.pdf|work=US EPA|publisher=US EPA}}</ref>



==Biological functions==
==Biological functions==

Revision as of 00:30, 15 March 2014

Perchlorate
Skeletal model of perchlorate showing various dimensions
Ball-and-stick model of the perchlorate ion
Ball-and-stick model of the perchlorate ion
Spacefill model of perchlorate
Spacefill model of perchlorate
Names
Systematic IUPAC name
Perchlorate[1]
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
DrugBank
ECHA InfoCard 100.152.366 Edit this at Wikidata
2136
MeSH 180053
  • InChI=1S/ClHO4/c2-1(3,4)5/h(H,2,3,4,5)/p-1 checkY
    Key: VLTRZXGMWDSKGL-UHFFFAOYSA-M checkY
  • [O-][Cl](=O)(=O)=O
Properties
ClO4−
Molar mass 99.451 g mol−1
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Perchlorates are the salts derived from perchloric acid—in particular when referencing the polyatomic anions found in solution, perchlorate is often written with the formula ClO4−. Perchlorates are often produced by natural processes but can also be produced artificially. They have been used for more than fifty years to treat thyroid disorders. They are used extensively within the pyrotechnics industry, and ammonium perchlorate is also a component of solid rocket fuel. Lithium perchlorate, which decomposes exothermically to produce oxygen, is used in oxygen "candles" on spacecraft, submarines, and in other situations where a reliable backup oxygen supply is needed. Most perchlorates are soluble in water,[2] except for potassium perchlorate which has the lowest solubility of any alkali metal perchlorate (1.5 g in 100 mL of water at 25 °C).

Production and use

Perchlorate salts are produced industrially by the oxidation of solutions of sodium chlorate by electrolysis. This method is used to prepare sodium perchlorate. Four perchlorates are of primary commercial interest: ammonium perchlorate (NH4ClO4), perchloric acid (HClO4), potassium perchlorate (KClO4), and sodium perchlorate (NaClO4). The main application is for rocket fuel.[3]

Reactivity as an oxidant

The perchlorate ion is the least reactive oxidizer of the generalized chlorates. This appears to be a paradox, since higher oxidation numbers are expected to be progressively stronger oxidizers, and less stable. A table of reduction potentials of the four chlorates shows that, contrary to expectation, perchlorate is the weakest oxidant among the four in water.[4]

Ion Acidic reaction E° (V) Neutral/basic reaction E° (V)
Hypochlorite H+ + HOCl + e− → ½Cl2(g) + H2O 1.63 ClO− + H2O + 2e− → Cl− + 2OH− 0.89
Chlorite 3H+ + HOClO + 3e− → ½Cl2(g) + 2H2O 1.64 ClO2− + 2H2O + 4e− → Cl− + 4OH− 0.78
Chlorate 6H+ + ClO3− + 5e− → ½Cl2(g) + 3H2O 1.47 ClO3− + 3H2O + 6e− → Cl− + 6OH− 0.63
Perchlorate 8H+ + ClO4− + 7e− → ½Cl2(g) + 4H2O 1.42 ClO4− + 4H2O + 8e− → Cl− + 8OH− 0.56

These data show that the perchlorate and chlorate are stronger oxidizers in acidic conditions than in basic conditions.

Gas phase measurements of heats of reaction (which allow computation of ΔHf°) of various chlorine oxides do follow the expected trend wherein Cl2O7 exhibits the largest endothermic value of ΔHf° (238.1 kJ/mol) while Cl2O exhibits the lowest endothermic value of ΔHf° (80.3 kJ/mol).[5]

The central chlorine in the perchlorate anion is a closed shell atom and is well protected by the four oxygens. Hence, perchlorate reacts sluggishly. Most perchlorate compounds, especially salts of electropositive metals such as sodium perchlorate or potassium perchlorate, are slow to react unless heated. This property is useful in many applications, such as flares, where the device should not explode, or even catch fire spontaneously.

Mixtures of perchlorates with organic compounds are more reactive. Although they do not usually catch fire or explode unless heated, there are a number of exceptions. Large amounts of improperly stored ammonium perchlorate led to the PEPCON disaster, in which an explosion destroyed one of the two large-scale production plants for ammonium perchlorate in the US.

Occurrence

Low levels of perchlorate have been detected in both drinking water and groundwater in 26 states in the U.S., according to the Environmental Protection Agency. In 2004, the chemical was also found in cow's milk in California with an average level of 1.3 parts per billion ("ppb" or µg/L), which may have entered the cows through feeding on crops that had exposure to water containing perchlorates.[6] According to the Impact Area Groundwater Study Program, the chemical has been detected as high as 5 µg/L in Massachusetts, well over the state regulation of 2 µg/L.[7] Fireworks are also a source of perchlorate in lakes.[8]

Natural perchlorate on Earth

In some places, perchlorate is detected because of contamination from industrial sites that use or manufacture it. In other places, there is no clear source of perchlorate. In those areas it may be naturally occurring. Natural perchlorate on Earth was first identified in terrestrial nitrate deposits of the Atacama Desert in Chile as early as in the 1880s[9] and for a long time considered a unique perchlorate source. Interestingly, the perchlorate released from the historic use of Chilean nitrate based fertilizer which were imported to the U.S. by the hundreds of tons in the early 19th century can still be found in some groundwater sources of the United States.[10] Recent improvements in analytical sensitivity using ion chromatography based techniques have revealed a more widespread presence of natural perchlorate, particularly in subsoils of Southwest USA,[11] salt evaporites in California and Nevada,[12] Pleistocene groundwater in New Mexico,[13] and even present in extremely remote places such as Antarctica.[14] The data from these studies and others indicate that natural perchlorate is globally deposited on Earth with the subsequent accumulation and transport governed by the local hydrologic conditions.

Despite its importance to environmental contamination, the specific source and processes involved in natural perchlorate production still remain poorly understood. Recent laboratory experiments in conjunction with isotopic studies[15] have implied that perchlorate may be produced on Earth by the oxidation of chlorine species through pathways involving ozone or its photochemical products.[16] Other studies have suggested that perchlorate can also be created by lightnining activated oxidation of chloride aerosols (e.g., chloride in sea salt sprays),[17] and ultraviolet or thermal oxidation of chlorine (e.g., bleach solutions used in swimming pools) in water.[18][19][20]

Perchlorate on surface of Mars

In May 2008, the Wet Chemistry Laboratory (WCL) on board the 2007 Phoenix Mars Lander performed the first wet chemical analysis of martian soil. The analyses on three samples, two from the surface and one from 5 cm depth, revealed a slightly alkaline soil and low levels of salts typically found on Earth. Unexpected though was the presence of ~ 0.6 wt % perchlorate (ClO4−), most likely as a Mg(ClO4)2 phase.[21] The salts formed from perchlorates discovered at the Phoenix landing site act as "anti-freeze" and will substantially lower the freezing point of water. Based on the temperature and pressure conditions on present-day Mars at the Phoenix lander site, conditions would allow a perchlorate salt solution to be present in liquid form for a few hours each day during the summer.[22]

The possibility that the perchlorate was a contaminant brought from Earth has been eliminated by several lines of evidence. The Phoenix retro-rockets used ultra pure hydrazine and launch propellants consisted of ammonium perchlorate. Sensors on board Phoenix found no traces of ammonium, and thus the perchlorate in the quantities present in all three soil samples is indigenous to the martian soil.

In 2006, a mechanism was proposed for the formation of perchlorates that is particularly relevant to the discovery of perchlorate at the Mars Phoenix lander site. It was shown that soils with high concentrations of chloride converted to perchlorate in the presence of sunlight and/or ultraviolet light. The conversion was reproduced in the lab using chloride-rich soils from Death Valley.[23] Other experiments have demonstrated the formation of perchlorate is associated with wide band gap semiconducting oxides.[24]

Further findings by the Mars Curiosity rover in 2012-2013 support perchlorates as being widespread,[25][26] and even inspired a Science article titled "Pesky Perchlorates All Over Mars".[27]

Regulatory issues in the U.S.

On February 11, 2011, the U.S. Environmental Protection Agency (EPA) issued a "regulatory determination" that perchlorate meets the Safe Drinking Water Act criteria for regulation as a contaminant. The agency found that perchlorate may have an adverse effect on the health of persons and is known to occur in public water systems with a frequency and at levels that it presents a public health concern. As a result of EPA's regulatory determination, it begins a process to determine what level of contamination is the appropriate level for regulation. The EPA prepared, as part of its regulatory determination, extensive responses to submitted public comments. The "docket ID" for EPA's regulatory action is EPA-HQ-OW-2009-0297 and can be found on regulations.gov.

Prior to issuance of its regulatory determination, the U.S. EPA issued a recommended Drinking Water Equivalent Level (DWEL) for perchlorate of 24.5 µg/L. In early 2006, EPA issued a "Cleanup Guidance" for this same amount. Both the DWEL and the Cleanup Guidance were based on a thorough review of the existing research by the National Academy of Science (NAS).[28] This followed numerous other studies, including one that suggested human breast milk had an average of 10.5 µg/L of perchlorate.[29] Both the Pentagon and some environmental groups have voiced questions about the NAS report, but no credible science has emerged to challenge the NAS findings. In February 2008, U.S. Food and Drug Administration said that U.S. toddlers on average are being exposed to more than half of the U.S. EPA's safe dose from food alone.[30] In March 2009, a Centers for Disease Control study found 15 brands of infant formula contaminated with perchlorate. Combined with existing perchlorate drinking water contamination, infants could be at risk for exposure to perchlorate above the levels considered safe by E.P.A.[31]

The US Environmental Protection Agency has issued substantial guidance and analysis concerning the impacts of perchlorate on the environment as well as drinking water.[1] California has also issued guidance regarding perchlorate use.[2]

Several states in the U.S. have enacted drinking water standard for perchlorate including Massachusetts in 2006. California's legislature enacted AB 826, the Perchlorate Contamination Prevention Act of 2003, requiring California's Department of Toxic Substance Control (DTSC) to adopt regulations specifying best management practices for perchlorate and perchlorate-containing substances. The Perchlorate Best Management Practices were adopted on December 31, 2005, and became operative on July 1, 2006. [3] California issued drinking water standards in 2007. Several other states, including Arizona, Maryland, Nevada, New Mexico, New York, and Texas have established non-enforceable, advisory levels for perchlorate.

In 2003, a federal district court in California found that the Comprehensive Environmental Response, Compensation and Liability Act (CERCLA) applied because perchlorate is ignitable and therefore a "characteristic" hazardous waste. (see Castaic Lake Water Agency v. Whittaker, 272 F. Supp. 2d 1053, 1059–61 (C.D. Cal. 2003)).

One example of perchlorate related problems was found at the Olin Flare Facility, Morgan Hill, California—Perchlorate contamination beneath a former flare manufacturing plant in California was first discovered in 2000, several years after the plant had closed. The plant had used potassium perchlorate as one of the ingredients during its 40 years of operation. By late 2003, the state of California and the Santa Clara Valley Water District had confirmed a groundwater plume currently extending over nine miles through residential and agricultural communities.

The Regional Water Quality Control Board and the Santa Clara Valley Water District have engaged in a major outreach effort that has received extensive press and community response. A well testing program is underway for approximately 1,200 residential, municipal, and agricultural wells in the area. Large ion exchange treatment units are operating in three public water supply systems that include seven municipal wells where perchlorate has been detected. The potentially responsible parties, Olin Corporation and Standard Fuse Incorporated, are supplying bottled water to nearly 800 households with private wells. The Regional Water Quality Control Board is overseeing potentially responsible party (PRP) cleanup efforts.[4]

Perchlorate Cleanup

Ex situ and in situ treatments

There are numerous technologies being utilized in treating perchlorate, including ex situ and in situ treatments. Some of ex situ treatments include ion exchange using perchlorate-selective or nitrite-specific resins, bioremediation using packed-bed or fluidized-bed bioreactors, and membrane technologies via electrodialysis and reverse osmosis.[32] In addition, ex situ technology of liquid phase carbon adsorption is employed, where granular activated carbon (GAC) is used in eliminating low levels of perchlorate and pretreatment may be required in arranging GAC for perchlorate elimination.[32] Furthermore, in situ treatments, such as bioremediation via perchlorate-selective microbes and permeable reactive barrier, are also being used to treat perchlorate.[32] In situ technology of phytoremediation could also be utilized, even though perchlorate phytoremediation mechanism is not fully founded yet.[32]


Biological functions

Over 40 phylogenetically and metabolically diverse microorganisms capable of perchlorate reduction have been isolated since 1996, including members of the Proteobacteria as well as two recently identified Firmicutes, Moorella perchloratireducens and Sporomusa sp.[33]

Health effects

Thyroidal problems

Perchlorate is a potent competitive inhibitor of the thyroid sodium-iodide symporter.[34] Thus, it has been used to treat hyperthyroidism since the 1950s.[35] At very high doses (70,000–300,000 ppb) the administration of potassium perchlorate was considered the standard of care in the United States, and remains the approved pharmacologic intervention for many countries.

Perchlorate, in large amounts, interferes with iodine uptake into the thyroid gland. In adults, the thyroid gland helps regulate the metabolism by releasing hormones, while in children, the thyroid helps in proper development. The NAS, in its 2005 report, Health Implications of Perchlorate Ingestion, emphasized that this effect, also known as IUI is not an adverse health effect. In January 2008, California's Department of Toxic Substances Control stated that perchlorate is becoming a serious threat to human health and water resources.[36] However, in 2010, the Environmental Protectional Agency's (EPA) Office of the Inspector General determined that the EPA's own perchlorate reference dose of 24.5 parts per billion protects against all human biological effects from exposure. This finding was due to a significant shift in policy at the EPA in basing its risk assessment on non-adverse effects such as IUI instead of adverse effects. The Office of the Inspector General also found that because the EPA's perchlorate reference dose is conservative and protective of human health further reducing perchlorate exposure below the reference dose does not effectively lower risk.[37]

The NAS found that perchlorate affects only the thyroid gland. It is not stored in the body, it is not metabolized, and any effects of perchlorate on the thyroid gland are fully reversible once exposure stops.[38] There has been some concern on perchlorate's effects on fetuses, newborns and children, but several peer-reviewed studies on children and newborns also provide reason to believe that low levels of perchlorate do not pose a threat to these populations. On October 1, 2004, the American Thyroid Association (ATA) reported that perchlorate may not be as harmful to newborns, pregnant women and other adults as previously thought. This finding was later supported in 2010 and 2011 by research on thousands of pregnant women in Italy, Wales, Argentina, and the United States.[39][40]

A study involving healthy adult volunteers determined that at levels above 0.007 milligrams per kilogram per day (mg/(kg·d)), perchlorate can temporarily inhibit the thyroid gland's ability to absorb iodine from the bloodstream ("iodide uptake inhibition", thus perchlorate is a known goitrogen).[41] The EPA converted this dose into a reference dose of 0.0007 mg/(kg·d) by dividing this level by the standard intraspecies uncertainty factor of 10. The agency then calculated a "drinking water equivalent level" of 24.5 ppb by assuming a person weighs 70 kilograms (154 pounds) and consumes 2 liters (68 ounces) of drinking water per day over a lifetime.[42]

In 2006, a study by Blount, et al. reported a statistical association between environmental levels of perchlorate and changes in thyroid hormones of women with low iodine. The study authors were careful to point out that hormone levels in all the study subjects remained within normal ranges. Importantly, the authors also indicated that they did not normalize their findings for creatinine, which essentially accounts for fluctuations in the concentrations of one-time urine samples like those used in this study.[43] When the Blount research was re-analyzed with the creatinine adjustment made, the study population limited to women of reproductive age, and results not shown in the original analysis, the association with perchlorate disappeared.[44] Soon after the Blount Study was released, NAS panelist Dr. Robert Utiger, a physician with the Harvard Institutes of Medicine, testified before Congress and stated: "I continue to believe that that reference dose, 0.007 milligrams per kilo (24.5 ppb,) which includes a factor of 10 to protect those who might be more vulnerable, is quite adequate."[45]

Environmental exposure in pregnancy to perchlorate in women with hypothyroidism causes a significant risk of low IQ in the child.[46]

Treatment of aplastic anemia

In the early 1960s, potassium perchlorate was implicated in the development of aplastic anemia—a condition where the bone marrow fails to produce new blood cells in sufficient quantity—in thirteen patients, seven of whom died.[47] Subsequent investigations have indicated the connection between administration of potassium perchlorate and development of aplastic anemia to be "equivocable at best", which means that the benefit of treatment, if it is the only known treatment, outweighs the risk, and it appeared a contaminant poisoned the 13.[48]

Appendix: oxyanions of chlorine

Chlorine can assume oxidation states of −1, +1, +3, +5, or +7, an additional oxidation state of +4 is seen in the neutral compound chlorine dioxide ClO2, which has a similar structure. Several other chlorine oxides are also known.

Chlorine oxidation state −1 +1 +3 +5 +7
Name chloride hypochlorite chlorite chlorate perchlorate
Formula Cl- ClO− ClO2− ClO3− ClO4−
Structure The chloride ion The hypochlorite ion The chlorite ion The chlorate ion The perchlorate ion

References

  1. ^ "Perchlorate - PubChem Public Chemical Database". The PubChem Project. USA: National Center for Biotechnology Information.
  2. ^ Draft Toxicological Profile for Perchlorates, Agency for Toxic Substances and Disease Registry, U.S. Department of Health and Human Services, September, 2005.
  3. ^ Helmut Vogt, Jan Balej, John E. Bennett, Peter Wintzer, Saeed Akbar Sheikh, Patrizio Gallone "Chlorine Oxides and Chlorine Oxygen Acids" in Ullmann's Encyclopedia of Industrial Chemistry 2002, Wiley-VCH. doi:10.1002/14356007.a06_483
  4. ^ Cotton, F. Albert; Wilkinson, Geoffrey (1988), Advanced Inorganic Chemistry (5th ed.), New York: Wiley-Interscience, p. 564, ISBN 0-471-84997-9
  5. ^ Wagman, D. D.; Evans, W. H.; Parker, V. P.; Schumm, R. H.; Halow, I.; Bailey, S. M.; Churney, K. L.; Nuttall, R. L. J. Phys. Chem. Ref. Data Vol. 11(2); &169;1982 by the American Chemical Society and the American Institute of Physics.
  6. ^ Associated Press. "Toxic chemical found in California milk". MSNBC. June 22, 2004.
  7. ^ http://www.mass.gov/dep/water/dwstand.pdf
  8. ^ Fireworks Displays Linked To Perchlorate Contamination In Lakes
  9. ^ Ericksen, G. E. Geology and origin of the Chilean nitrate deposits;U.S. Geological Survey Prof. Paper 1188; USGS: Reston, VA,1981, 37 pp.
  10. ^ Böhlke, J. K.;Hatzinger, P. B.; Sturchio, N. C.; Gu, B.; Abbene, I.; Mroczkowski, S. J.,Atacama perchlorate as an agricultural contaminant in groundwater: Isotopic andchronologic evidence from Long Island, New York. Environmental science & technology 2009, 43 (15), 5619-5625.
  11. ^ Rao, B.; Anderson, T. A.;Orris, G. J.; Rainwater, K. A.; Rajagopalan, S.; Sandvig, R. M.; Scanlon, B.R.; Stonestrom, S. A.; Walvoord, M. A.; Jackson, W. A. Widespread NaturalPerchlorate in Unsaturated zones of the Southwest United States" Environ. Sci. Technol 2007, 41, 4522-4528
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  14. ^ S. P. Kounaves; et al. (2010). "Natural Perchlorate in the Antarctic Dry Valleys and Implications for its Global Distribution and History". Environmental Science & Technology. 44 (7): 2360–2364. Bibcode:2010EnST...44.2360K. doi:10.1021/es9033606. PMID 20155929. {{cite journal}}: Explicit use of et al. in: |author= (help)
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  16. ^ Rao, B.; Anderson, T. A.;Redder, A.; Jackson, W. A. Perchlorate Formation by Ozone Oxidation of AqueousChlorine/Oxy-Chlorine Species: Role of ClxOy Radicals" Environ. Sci. Technol 2010, 44, 2961-2967 
  17. ^ Dasgupta,P. K.; Martinelango, P. K.; Jackson, W. A.; Anderson, T. A.; Tian, K.; Tock, R.W.; Rajagopalan, S., The origin of naturally occurring perchlorate: the role ofatmospheric processes. Environmental science& technology 2005, 39 (6), 1569-1575.
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  21. ^ Hecht, M. H., S. P. Kounaves, R. Quinn; et al. (2009). "Detection of Perchlorate & the Soluble Chemistry of Martian Soil at the Phoenix Mars Lander Site". Science. 325 (5936): 64–67. Bibcode:2009Sci...325...64H. doi:10.1126/science.1172466. PMID 19574385. {{cite journal}}: Explicit use of et al. in: |author= (help)CS1 maint: multiple names: authors list (link)
  22. ^ Chevrier, V. C., Hanley, J., and Altheide, T.S. (2009). "Stability of perchlorate hydrates and their liquid solutions at the Phoenix landing site, Mars". Geophysical Research Letters. 36 (10): L10202. Bibcode:2009GeoRL..3610202C. doi:10.1029/2009GL037497.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  23. ^ Miller, Glen. "Photooxidation of chloride to perchlorate in the presence of desert soils and titanium dioxide". American Chemical Society. March 29, 2006
  24. ^ Jennifer D. Schuttlefield, Justin B. Sambur, Melissa Gelwicks, Carrick M. Eggleston, and B. A. Parkinson "Photooxidation of Chloride by Oxide Minerals: Implications for Perchlorate on Mars" J. Am. Chem. Soc. 2011, vol. 133, pp. 17521–17523. doi:10.1021/ja2064878
  25. ^ Adam Mann. "Look What We Found on Mars - Curiosity Rover Serves Up Awesome Science". Slate (magazine). 26 September 2013.
  26. ^ Chang, Kenneth (1 October 2013). "Hitting Pay Dirt on Mars". New York Times. Retrieved 2 October 2013.
  27. ^ Richard A. Kerr. "Pesky Perchlorates All Over Mars". Science (journal). 12 April 2013. Vo. 340 No. 6129 P. 138. doi:10.1126/science.340.6129.138-b
  28. ^ Committee to Assess the Health Implications of Perchlorate Ingestion, National Research Council (2005). Health Implications of Perchlorate Ingestion. Washington, DC: The National Academies Press. ISBN 10: 0-309-09568-9. {{cite book}}: Check |isbn= value: invalid character (help)
  29. ^ McKee, Maggie. "Perchlorate found in breast milk across US". New Scientist. February 23, 2005
  30. ^ Perchlorate In Food
  31. ^ "CDC Scientists Find Rocket Fuel Chemical In Infant Formula". Anila Jacob, M.D., M.P.H.. Environmental Working Group. 2 April 2009.
  32. ^ a b c d "Technical Fact Sheet – Perchlorate" (PDF). US EPA. US EPA.
  33. ^ John D. Coates, Laurie A. Achenbach (2004). "Microbial perchlorate reduction: rocket-fuelled metabolism". Nature Reviews Microbiology. 2 (7): 569–580. doi:10.1038/nrmicro926. PMID 15197392.
  34. ^ Braverman, L. E.; He X.; Pino S.; et al. (2005). "The effect of perchlorate, thiocyanate, and nitrate on thyroid function in workers exposed to perchlorate long-term". J Clin Endocrinol Metab. 90 (2): 700–706. doi:10.1210/jc.2004-1821. PMID 15572417. {{cite journal}}: Explicit use of et al. in: |author= (help)CS1 maint: multiple names: authors list (link)
  35. ^ Godley, A. F.; Stanbury, J. B. (1954). "Preliminary experience in the treatment of hyperthyroidism with potassium perchlorate". J Clin Endocrinol Metab. 14 (1): 70–78. doi:10.1210/jcem-14-1-70. PMID 13130654. {{cite journal}}: Cite has empty unknown parameter: |month= (help)
  36. ^ California Department of Toxic Substances Control Jan 26, 2008
  37. ^ Scientific Analysis of Perchlorate (Report). United States Environmental Protection Agency, Office of the Inspector General. 19 April 2010. What We Found
  38. ^ J. Wolff (1998). "Perchlorate and the Thyroid Gland". Pharmacological Reviews. 50 (1): 89–105. PMID 9549759.
  39. ^ "Various Levels of Perchlorate Exposure Found Not to Be Harmful to Newborns, Pregnant Women, and Other Adults" (Press release). American Thyroid Association. 1 October 2004.
  40. ^ Pearce; et al. (2010). "Perchlorate and Thiocyanate Exposure and Thyroid Function in First Trimester Pregnant Women". The Journal of Clinical Endocrinology and Metabolism. {{cite journal}}: Explicit use of et al. in: |author= (help)
  41. ^ Greer, M. A., Goodman, G., Pleuss, R. C., Greer, S. E. (2002). "Health effect assessment for environmental perchlorate contamination: The dose response for inhibition of thyroidal radioiodide uptake in humans" (free online). Environmental Health Perspectives. 110 (9): 927–937. doi:10.1289/ehp.02110927. PMC 1240994. PMID 12204829.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  42. ^ US EPA Memorandum Jan 26, 2006
  43. ^ Benjamin C. Blount, James L. Pirkle, John D. Osterloh, Liza Valentin-Blasini, and Kathleen L. Caldwell (2006). "Urinary Perchlorate and Thyroid Hormone Levels in Adolescent and Adult Men and Women Living in the United States". Environmental Health Perspectives. 114 (12): 1865–71. doi:10.1289/ehp.9466. PMC 1764147. PMID 17185277.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  44. ^ Tarone; et al. (2010). "The Epidemiology of Environmental Perchlorate Exposure and Thyroid Function: A Cmprehensive Review". Journal of Occupational and Environmental Medicine. 52 (June): 653–60. doi:10.1097/JOM.0b013e3181e31955. PMID 20523234. {{cite journal}}: Explicit use of et al. in: |author= (help)
  45. ^ "Perchlorate: Health and Environmental Impacts of Unregulated Exposure". United States Congress. Retrieved 15 April 2012.
  46. ^ Attention: This template ({{cite doi}}) is deprecated. To cite the publication identified by doi:10.1186/ISRCTN46178175, please use {{cite journal}} (if it was published in a bona fide academic journal, otherwise {{cite report}} with |doi=10.1186/ISRCTN46178175 instead.. Also described in Medscapearticle: Perchlorate Levels in Pregnancy Linked to Low Childhood IQ, by Nancy A. Melville, October 22, 2013
  47. ^ National Research Council (2005). "Perchlorate and the thyroid". Health implications of perchlorate ingestion. Washington, D.C: National Academies Press. p. 7. ISBN 0-309-09568-9. Retrieved on April 3, 2009 through Google Book Search.
  48. ^ Clark, J. J. J. (2000). "Toxicology of perchlorate". In Urbansky ET (ed.) (ed.). Perchlorate in the environment. New York: Kluwer Academic/Plenum Publishers. pp. 19–20. ISBN 978-0-306-46389-1. {{cite book}}: |editor= has generic name (help) Retrieved on April 3, 2009 through Google Book Search.
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