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{{Elementbox_isotopes_stable | mn=94 | sym=Zr | na=17.38% | n=54 }} |
{{Elementbox_isotopes_stable | mn=94 | sym=Zr | na=17.38% | n=54 }} |
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{{Elementbox_isotopes_decay | mn=96 | sym=Zr |
{{Elementbox_isotopes_decay | mn=96 | sym=Zr |
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| na=2.8% | hl=[[1 E19 s|2.0×10<sup>19</sup>y]] <ref> |
| na=2.8% | hl=[[1 E19 s|2.0×10<sup>19</sup>y]] <ref>{{cite web| last = Pritychenko| first = Boris| coauthors = V. Tretyak| title = Adopted Double Beta Decay Data| publisher = National Nuclear Data Center| url = http://www.nndc.bnl.gov/bbdecay/list.html| accessdate = 2008-02-11}}</ref> |
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| dm=[[double beta decay|β<sup>−</sup>β<sup>−</sup>]] | de=3.348 | pn=96 | ps=[[molybdenum|Mo]] }} |
| dm=[[double beta decay|β<sup>−</sup>β<sup>−</sup>]] | de=3.348 | pn=96 | ps=[[molybdenum|Mo]] }} |
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{{Elementbox_isotopes_end}} |
{{Elementbox_isotopes_end}} |
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== Characteristics == |
== Characteristics == |
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Zirconium is a lustrous, grayish-white metal which is solid at room temperature. In a powdered form, zirconium is highly flammable, but the solid form is far less prone to igniting.<ref>{{cite web| last = Winter| first = Mark| title = Key Information| work = Zirconium| publisher = University of Sheffield| date = 2007| url = http://www.webelements.com/webelements/elements/text/Zr/key.html| accessdate = 2008-02-12}}</ref> Zirconium is highly resistant to corrosion by alkalis, acids, salt water, and other agents.<ref name="Los Alamos">{{cite web | title = Zirconium| publisher = Los Alamos Chemistry Division| date = 2003-12-15| url = http://periodic.lanl.gov/elements/40.html| accessdate = 2008-02-12}}</ref> Alloys with zinc become magnetic below 35 K.<ref name="webuses">{{cite web| last = Winter| first = Mark| title = Uses| work = Zirconium| publisher = University of Sheffield| date = 2007| url = http://www.webelements.com/webelements/elements/text/Zr/uses.html| accessdate = 2008-02-12}}</ref> |
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Zirconium is a grayish-white [[metal]], lustrous, and quite corrosion-resistant. Zirconium is lighter than [[steel]] and its hardness is similar to [[copper]]. When it is finely divided into a powder, zirconium can spontaneously ignite in air, especially at high temperatures. (It is much more difficult to ignite the solid metal.) The Zirconium-zinc [[alloy]] becomes [[magnetism|magnetic]] at temperatures below 35 [[Kelvin|K]]. The [[oxidation state]] of zirconium is usually +4, although +3 and +2 can also be obtained inside of chemical compounds. |
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==Applications== |
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Because of Zirconium's excellent resistance to corrosion, it is often used as an alloying agent in materials that are exposed to corrosive agents, such as surgical appliances, explosive primers, vacuum tube [[getter]]s and filaments. Zirconium dioxide (ZrO<sub>2</sub>) is used in laboratory crucibles, metallurgical furnaces, and as a refractory material.<ref name="webuses"/> Zircon (ZrSiO<sub>4</sub>) is cut into gemstones for use in jewelry. Zirconium carbonate (3ZrO<sub>2</sub>·CO<sub>2</sub>·H<sub>2</sub>O) is used in lotions to treat poison ivy. Zirconium is also used in nuclear reactors because it does not easily absorb neutrons.<ref name="elemental">{{cite web| last = Gagnon| first = Steve| title = Zirconium| work = It's Elemental| publisher = Jefferson Lab| url = http://education.jlab.org/itselemental/ele040.html| accessdate = 2008-02-12}}</ref> |
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==History== |
==History== |
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Zirconium (from [[Syriac language|Syriac]] ''zargono'',<ref>http://www.tertullian.org/rpearse/oriental/syriac.htm</ref> [[Arabic language|Arabic]] ''zarkûn'' from [[Persian language|Persian]] ''zargûn'' ''زرگون'' meaning "gold like") was [[Discovery of the chemical elements|discovered]] in [[1789]] by [[Martin Heinrich Klaproth]], isolated in [[1824]] by [[Jöns Jakob Berzelius]], and finally put in a pure form in 1914. |
Zirconium (from [[Syriac language|Syriac]] ''zargono'',<ref>{{cite web| last = Pearse| first = Roger| title = Syriac Literature| date = 2002-09-16| url = http://www.tertullian.org/rpearse/oriental/syriac.htm| accessdate = 2008-02-11}}</ref> [[Arabic language|Arabic]] ''zarkûn'' from [[Persian language|Persian]] ''zargûn'' ''زرگون'' meaning "gold like") was [[Discovery of the chemical elements|discovered]] in [[1789]] by [[Martin Heinrich Klaproth]], isolated in [[1824]] by [[Jöns Jakob Berzelius]], and finally put in a pure form in 1914.<ref name="elemental"/> |
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The zirconium-containing [[mineral]] zircon, or its variations (jargoon, hyacinth, jacinth, or ligure), were mentioned in biblical writings. The mineral was not known to contain a new element until Klaproth analyzed a [[jargoon]] from the island of Ceylon in the Indian Ocean. He named the new element |
The zirconium-containing [[mineral]] zircon, or its variations (jargoon, hyacinth, jacinth, or ligure), were mentioned in biblical writings. The mineral was not known to contain a new element until Klaproth analyzed a [[jargoon]] from the island of Ceylon in the Indian Ocean. He named the new element Zirkonertz (zirconia). The impure metal was isolated first by Berzelius by heating a mixture of potassium and potassium-zirconium fluoride in a small decomposition process conducted in an iron tube. |
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The ''[[crystal bar process]]'' (or ''Iodide process''), discovered by [[Anton Eduard van Arkel]] and Jan Hendrik de Boer in 1925, was the first industrial process for the commercial production of pure metallic zirconium. It was later superseded by the [[Kroll process]]. |
The ''[[crystal bar process]]'' (or ''Iodide process''), discovered by [[Anton Eduard van Arkel]] and Jan Hendrik de Boer in 1925, was the first industrial process for the commercial production of pure metallic zirconium. It was later superseded by the [[Kroll process]]. |
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[[Image:2005zirconium.PNG|thumb|left|Zirconium output in 2005]] |
[[Image:2005zirconium.PNG|thumb|left|Zirconium output in 2005]] |
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[[Image:Zirconium mineral concentrates - world production trend.svg|thumb|left|World production trend of zirconium mineral concentrates]] |
[[Image:Zirconium mineral concentrates - world production trend.svg|thumb|left|World production trend of zirconium mineral concentrates]] |
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Zirconium is never found in nature as a native metal. The principal economic source of zirconium is the zirconium [[silicate mineral]], [[zircon]] (ZrSiO<sub>4</sub>), which is found in deposits located in |
Zirconium is never found in nature as a native metal. The principal economic source of zirconium is the zirconium [[silicate mineral]], [[zircon]] (ZrSiO<sub>4</sub>), which is found in deposits located in Australia, Brazil, India, Malysis, Russia, and the United States. Zirconium and [[hafnium]] are both contained in zircon and they are quite difficult to separate chemically.<ref name="webgeo"/> [[Zircon]] resources exceed 60 million metric tons worldwide.<ref name="usgs2008">{{cite journal| title = Zirconium and Hafnium| journal = Mineral Commodity Summaries| pages = 192-193| publisher = US Geological Survey| date = January 2008| url = http://minerals.usgs.gov/minerals/pubs/commodity/zirconium/mcs-2008-zirco.pdf| format = PDF| accessdate = 2008-02-24}}</ref> |
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Zircon, the principle economic source of zirconium, is a by-product of the mining and processing of the [[titanium]] minerals [[ilmenite]] and [[rutile]], as well as from [[tin]] mining.<ref>{{cite web| last = Callaghan| first = R.| title = Zirconium and Hafnium Statistics and Information| publisher = US Geological Survey| date = 2008-02-21| url = http://minerals.usgs.gov/minerals/pubs/commodity/zirconium/| accessdate = 2008-02-24}}</ref> From 2003 to 2007, zircon prices have steadily increased from $360 to $840 per metric ton.<ref name="usgs2008"/> Zirconium also occurs in more than 140 other recognized mineral species including [[baddeleyite]] and [[kosnarite]].<ref>{{cite web| last = Ralph| first = Jolyon| coauthors = Ida Ralph| title = Minerals that include Zr| publisher = Mindat.org| date = 2008| url = http://www.mindat.org/chemsearch.php?inc=Zr%2C&exc=&sub=Search+for+Minerals| accessdate = 2008-02-23}}</ref> This metal is commercially produced mostly by the reduction of the zirconium(IV) [[chloride]] with [[magnesium]] metal in the [[Kroll process]]. Commercial-quality zirconium for most uses still has a content of 1% to 3% hafnium.<ref>{{cite encyclopedia| encyclopedia = Infoplease| title = Zirconium| url = http://www.infoplease.com/encyclopedia/zirconium| accessdate = 2008-02-24| date = 2007| publisher = Pearson Education}}</ref> |
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⚫ | This element is relatively-abundant in [[Stellar classification#Class S|S-type stars]], and it has been detected in the sun and in meteorites. Lunar rock samples brought back from several [[Apollo program]] missions to the moon have a quite high zirconium oxide content relative to terrestrial rocks. |
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⚫ | This element is relatively-abundant in [[Stellar classification#Class S|S-type stars]], and it has been detected in the sun and in meteorites. Lunar rock samples brought back from several [[Apollo program]] missions to the moon have a quite high zirconium oxide content relative to terrestrial rocks.<ref name="Los Alamos"/><ref name="webgeo">{{cite web| last = Winter| first = Mark| title = Geological Information| work = Zirconium| publisher = University of Sheffield| date = 2007| url = http://www.webelements.com/webelements/elements/text/Zr/geol.html| accessdate = 2008-02-19}}</ref> |
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''See also [[:category:Zirconium minerals|zirconium minerals]].'' |
''See also [[:category:Zirconium minerals|zirconium minerals]].'' |
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== Precautions == |
== Precautions == |
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[[Image:Zirconium rod.jpg|thumb|right|Zirconium rod]] |
[[Image:Zirconium rod.jpg|thumb|right|Zirconium rod]] |
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Inhalation of zirconium compounds can cause skin and lung [[granuloma]]s. Zirconium aerosols can cause [[pulmonary]] granulomas. Persistent exposure to zirconium tetrachloride resulted in increased mortality in rats and guinea pigs and a decrease of blood hemoglobin and red blood cells in dogs. OSHA recommends a 5 mg/m<sup>3</sup> [[permissible exposure limit|time weighted average]] limit and a 10 mg/m<sup>3</sup> short-term exposure limit.<ref>{{cite web| title = Zirconium Compounds| publisher = National Institute for Occupational Health and Safety| date = 2007-12-17| url = http://www.cdc.gov/niosh/pel88/7440-67.html| accessdate = 2008-02-17}}</ref> |
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Compounds containing zirconium are not noted for toxicity. The metal dust can ignite in air and should be regarded as a fire and explosion hazard. Zirconium has no known [[biology|biological]] role. |
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==References== |
==References== |
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{{reflist}} |
{{reflist}} |
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{{Commons|Zirconium}} |
{{Commons|Zirconium}} |
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{{wiktionary|zirconium}} |
{{wiktionary|zirconium}} |
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⚫ | |||
*[http://www.webelements.com/webelements/elements/text/Zr/index.html WebElements.com – Zirconium] |
*[http://www.webelements.com/webelements/elements/text/Zr/index.html WebElements.com – Zirconium] |
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Revision as of 17:09, 24 February 2008
Template:Elementbox header Template:Elementbox series Template:Elementbox groupperiodblock Template:Elementbox appearance img Template:Elementbox atomicmass gpm Template:Elementbox econfig Template:Elementbox epershell Template:Elementbox section physicalprop Template:Elementbox phase Template:Elementbox density gpcm3nrt Template:Elementbox densityliq gpcm3mp Template:Elementbox meltingpoint Template:Elementbox boilingpoint Template:Elementbox heatfusion kjpmol Template:Elementbox heatvaporiz kjpmol Template:Elementbox heatcapacity jpmolkat25 Template:Elementbox vaporpressure katpa Template:Elementbox section atomicprop Template:Elementbox crystalstruct Template:Elementbox oxistates Template:Elementbox electroneg pauling Template:Elementbox ionizationenergies4 Template:Elementbox atomicradius pm Template:Elementbox atomicradiuscalc pm Template:Elementbox covalentradius pm Template:Elementbox section miscellaneous Template:Elementbox magnetic Template:Elementbox eresist ohmmat20 Template:Elementbox thermalcond wpmkat300k Template:Elementbox thermalexpansion umpmkat25 Template:Elementbox speedofsound rodmpsat20 Template:Elementbox youngsmodulus gpa Template:Elementbox shearmodulus gpa Template:Elementbox poissonratio Template:Elementbox mohshardness Template:Elementbox vickershardness mpa Template:Elementbox brinellhardness mpa Template:Elementbox cas number Template:Elementbox isotopes begin |- ! rowspan="2" style="text-align:right; vertical-align:middle;" | 88Zr | rowspan="2" style="text-align:center; vertical-align:middle;" | syn | rowspan="2" style="text-align:right; vertical-align:middle;" | 83.4 d | ε | style="text-align:right;" | 88Y |- | γ | style="text-align:right;" | - |- ! rowspan="3" style="text-align:right; vertical-align:middle;" | 89Zr | rowspan="3" style="vertical-align:middle; text-align:center" | syn | rowspan="3" style="vertical-align:middle; text-align:right;" | 78.4 h | ε | style="text-align:right;" | 89Y |- | β+ | style="text-align:right;" | 89Y |- | γ | style="text-align:right;" | - Template:Elementbox isotopes stable Template:Elementbox isotopes stable Template:Elementbox isotopes stable |- ! style="text-align:right;" | 93Zr | style="text-align:center;" | syn | style="text-align:right;" | 1.53×106y | β− | style="text-align:right;" | 93Nb Template:Elementbox isotopes stable |- ! style="text-align:right;" | 96Zr | style="text-align:right;" | 2.8% | style="text-align:right;" | 2.0×1019y [1] | β−β− | style="text-align:right;" | 96Mo Template:Elementbox isotopes end Template:Elementbox footer
Zirconium (Template:PronEng, /ˌzɝˈkoʊniəm/) is a chemical element that has the symbol Zr and has the atomic number 40. A lustrous, very corrosion resistant, gray-white, strong transition metal that resembles titanium, zirconium is obtained mainly from the mineral zircon. Zirconium is primarily used in nuclear reactors, especially in the cladding of the fuel rods, due to its low neutron-capture cross-section and its resistance to corrosion.
Characteristics
Zirconium is a lustrous, grayish-white metal which is solid at room temperature. In a powdered form, zirconium is highly flammable, but the solid form is far less prone to igniting.[2] Zirconium is highly resistant to corrosion by alkalis, acids, salt water, and other agents.[3] Alloys with zinc become magnetic below 35 K.[4]
Applications
Because of Zirconium's excellent resistance to corrosion, it is often used as an alloying agent in materials that are exposed to corrosive agents, such as surgical appliances, explosive primers, vacuum tube getters and filaments. Zirconium dioxide (ZrO2) is used in laboratory crucibles, metallurgical furnaces, and as a refractory material.[4] Zircon (ZrSiO4) is cut into gemstones for use in jewelry. Zirconium carbonate (3ZrO2·CO2·H2O) is used in lotions to treat poison ivy. Zirconium is also used in nuclear reactors because it does not easily absorb neutrons.[5]
History
Zirconium (from Syriac zargono,[6] Arabic zarkûn from Persian zargûn زرگون meaning "gold like") was discovered in 1789 by Martin Heinrich Klaproth, isolated in 1824 by Jöns Jakob Berzelius, and finally put in a pure form in 1914.[5]
The zirconium-containing mineral zircon, or its variations (jargoon, hyacinth, jacinth, or ligure), were mentioned in biblical writings. The mineral was not known to contain a new element until Klaproth analyzed a jargoon from the island of Ceylon in the Indian Ocean. He named the new element Zirkonertz (zirconia). The impure metal was isolated first by Berzelius by heating a mixture of potassium and potassium-zirconium fluoride in a small decomposition process conducted in an iron tube.
The crystal bar process (or Iodide process), discovered by Anton Eduard van Arkel and Jan Hendrik de Boer in 1925, was the first industrial process for the commercial production of pure metallic zirconium. It was later superseded by the Kroll process.
Occurrence
![](https://upload.wikimedia.org/wikipedia/commons/thumb/7/75/Zirconium_mineral_concentrates_-_world_production_trend.svg/220px-Zirconium_mineral_concentrates_-_world_production_trend.svg.png)
Zirconium is never found in nature as a native metal. The principal economic source of zirconium is the zirconium silicate mineral, zircon (ZrSiO4), which is found in deposits located in Australia, Brazil, India, Malysis, Russia, and the United States. Zirconium and hafnium are both contained in zircon and they are quite difficult to separate chemically.[7] Zircon resources exceed 60 million metric tons worldwide.[8]
Zircon, the principle economic source of zirconium, is a by-product of the mining and processing of the titanium minerals ilmenite and rutile, as well as from tin mining.[9] From 2003 to 2007, zircon prices have steadily increased from $360 to $840 per metric ton.[8] Zirconium also occurs in more than 140 other recognized mineral species including baddeleyite and kosnarite.[10] This metal is commercially produced mostly by the reduction of the zirconium(IV) chloride with magnesium metal in the Kroll process. Commercial-quality zirconium for most uses still has a content of 1% to 3% hafnium.[11]
This element is relatively-abundant in S-type stars, and it has been detected in the sun and in meteorites. Lunar rock samples brought back from several Apollo program missions to the moon have a quite high zirconium oxide content relative to terrestrial rocks.[3][7]
See also zirconium minerals.
Isotopes
Naturally-occurring zirconium is composed of four stable isotopes, and one extremely long-lived radioisotope (96Zr). The second most stable radioisotope is 93Zr which has a half-life of 1.53 million years. Eighteen other radioisotopes have been observed. Most of these have half-lives that are less than a day except for 95Zr (64.02 days), 88Zr (63.4 days), and 89Zr (78.41 hours). The primary decay mode is electron capture for isotopes lighter than 92Zr, and the primary mode for heavier isotopes is beta decay. Other isotopes of zirconium include 90Zr, 91Zr, and 94Zr
Compounds
Some common zirconium compounds are: ZrC, ZrO2, ZrN, ZrCl4, ZrS2, ZrSi2, ZrSiO4, ZrF4, ZrBr4, ZrI4, Zr(OH)4, C10H11ClZr, Zr(CH3CH2COO)4, Zr(WO4)2, ZrH2, Pb(ZrxTi1-x)O3
Precautions
![](https://upload.wikimedia.org/wikipedia/commons/thumb/d/d3/Zirconium_rod.jpg/220px-Zirconium_rod.jpg)
Inhalation of zirconium compounds can cause skin and lung granulomas. Zirconium aerosols can cause pulmonary granulomas. Persistent exposure to zirconium tetrachloride resulted in increased mortality in rats and guinea pigs and a decrease of blood hemoglobin and red blood cells in dogs. OSHA recommends a 5 mg/m3 time weighted average limit and a 10 mg/m3 short-term exposure limit.[12]
References
- ^ Pritychenko, Boris. "Adopted Double Beta Decay Data". National Nuclear Data Center. Retrieved 2008-02-11.
{{cite web}}
: Unknown parameter|coauthors=
ignored (|author=
suggested) (help) - ^ Winter, Mark (2007). "Key Information". Zirconium. University of Sheffield. Retrieved 2008-02-12.
- ^ a b "Zirconium". Los Alamos Chemistry Division. 2003-12-15. Retrieved 2008-02-12.
- ^ a b Winter, Mark (2007). "Uses". Zirconium. University of Sheffield. Retrieved 2008-02-12.
- ^ a b Gagnon, Steve. "Zirconium". It's Elemental. Jefferson Lab. Retrieved 2008-02-12.
- ^ Pearse, Roger (2002-09-16). "Syriac Literature". Retrieved 2008-02-11.
- ^ a b Winter, Mark (2007). "Geological Information". Zirconium. University of Sheffield. Retrieved 2008-02-19.
- ^ a b "Zirconium and Hafnium" (PDF). Mineral Commodity Summaries. US Geological Survey: 192–193. January 2008. Retrieved 2008-02-24.
- ^ Callaghan, R. (2008-02-21). "Zirconium and Hafnium Statistics and Information". US Geological Survey. Retrieved 2008-02-24.
- ^ Ralph, Jolyon (2008). "Minerals that include Zr". Mindat.org. Retrieved 2008-02-23.
{{cite web}}
: Unknown parameter|coauthors=
ignored (|author=
suggested) (help) - ^ "Zirconium". Infoplease. Pearson Education. 2007. Retrieved 2008-02-24.
- ^ "Zirconium Compounds". National Institute for Occupational Health and Safety. 2007-12-17. Retrieved 2008-02-17.