This is a good article. Click here for more information.

Zirconium

From Wikipedia, the free encyclopedia
Jump to: navigation, search
Not to be confused with zircon, zirconia, or cubic zirconia.
"Zr" redirects here. For other uses, see ZR (disambiguation).
Zirconium,  40Zr
Zirconium crystal bar and 1cm3 cube.jpg
General properties
Name, symbol zirconium, Zr
Pronunciation /zərˈkniəm/
zər-KOH-ni-əm
Appearance silvery white
Zirconium in the periodic table
Hydrogen (diatomic nonmetal)
Helium (noble gas)
Lithium (alkali metal)
Beryllium (alkaline earth metal)
Boron (metalloid)
Carbon (polyatomic nonmetal)
Nitrogen (diatomic nonmetal)
Oxygen (diatomic nonmetal)
Fluorine (diatomic nonmetal)
Neon (noble gas)
Sodium (alkali metal)
Magnesium (alkaline earth metal)
Aluminium (post-transition metal)
Silicon (metalloid)
Phosphorus (polyatomic nonmetal)
Sulfur (polyatomic nonmetal)
Chlorine (diatomic nonmetal)
Argon (noble gas)
Potassium (alkali metal)
Calcium (alkaline earth metal)
Scandium (transition metal)
Titanium (transition metal)
Vanadium (transition metal)
Chromium (transition metal)
Manganese (transition metal)
Iron (transition metal)
Cobalt (transition metal)
Nickel (transition metal)
Copper (transition metal)
Zinc (transition metal)
Gallium (post-transition metal)
Germanium (metalloid)
Arsenic (metalloid)
Selenium (polyatomic nonmetal)
Bromine (diatomic nonmetal)
Krypton (noble gas)
Rubidium (alkali metal)
Strontium (alkaline earth metal)
Yttrium (transition metal)
Zirconium (transition metal)
Niobium (transition metal)
Molybdenum (transition metal)
Technetium (transition metal)
Ruthenium (transition metal)
Rhodium (transition metal)
Palladium (transition metal)
Silver (transition metal)
Cadmium (transition metal)
Indium (post-transition metal)
Tin (post-transition metal)
Antimony (metalloid)
Tellurium (metalloid)
Iodine (diatomic nonmetal)
Xenon (noble gas)
Caesium (alkali metal)
Barium (alkaline earth metal)
Lanthanum (lanthanide)
Cerium (lanthanide)
Praseodymium (lanthanide)
Neodymium (lanthanide)
Promethium (lanthanide)
Samarium (lanthanide)
Europium (lanthanide)
Gadolinium (lanthanide)
Terbium (lanthanide)
Dysprosium (lanthanide)
Holmium (lanthanide)
Erbium (lanthanide)
Thulium (lanthanide)
Ytterbium (lanthanide)
Lutetium (lanthanide)
Hafnium (transition metal)
Tantalum (transition metal)
Tungsten (transition metal)
Rhenium (transition metal)
Osmium (transition metal)
Iridium (transition metal)
Platinum (transition metal)
Gold (transition metal)
Mercury (transition metal)
Thallium (post-transition metal)
Lead (post-transition metal)
Bismuth (post-transition metal)
Polonium (post-transition metal)
Astatine (metalloid)
Radon (noble gas)
Francium (alkali metal)
Radium (alkaline earth metal)
Actinium (actinide)
Thorium (actinide)
Protactinium (actinide)
Uranium (actinide)
Neptunium (actinide)
Plutonium (actinide)
Americium (actinide)
Curium (actinide)
Berkelium (actinide)
Californium (actinide)
Einsteinium (actinide)
Fermium (actinide)
Mendelevium (actinide)
Nobelium (actinide)
Lawrencium (actinide)
Rutherfordium (transition metal)
Dubnium (transition metal)
Seaborgium (transition metal)
Bohrium (transition metal)
Hassium (transition metal)
Meitnerium (unknown chemical properties)
Darmstadtium (unknown chemical properties)
Roentgenium (unknown chemical properties)
Copernicium (transition metal)
Nihonium (unknown chemical properties)
Flerovium (post-transition metal)
Moscovium (unknown chemical properties)
Livermorium (unknown chemical properties)
Tennessine (unknown chemical properties)
Oganesson (unknown chemical properties)
Ti

Zr

Hf
yttriumzirconiumniobium
Atomic number (Z) 40
Group, block group 4, d-block
Period period 5
Element category   transition metal
Standard atomic weight (±) (Ar) 91.224(2)[1]
Electron configuration [Kr] 4d2 5s2
per shell
2, 8, 18, 10, 2
Physical properties
Phase solid
Melting point 2128 K ​(1855 °C, ​3371 °F)
Boiling point 4650 K ​(4377 °C, ​7911 °F)
Density near r.t. 6.52 g/cm3
when liquid, at m.p. 5.8 g/cm3
Heat of fusion 14 kJ/mol
Heat of vaporization 591 kJ/mol
Molar heat capacity 25.36 J/(mol·K)
vapor pressure
P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 2639 2891 3197 3575 4053 4678
Atomic properties
Oxidation states 4, 3, 2, 1, −2[2] ​(an amphoteric oxide)
Electronegativity Pauling scale: 1.33
Ionization energies 1st: 640.1 kJ/mol
2nd: 1270 kJ/mol
3rd: 2218 kJ/mol
Atomic radius empirical: 160 pm
Covalent radius 175±7 pm
Miscellanea
Crystal structure hexagonal close-packed (hcp)
Hexagonal close-packed crystal structure for zirconium
Speed of sound thin rod 3800 m/s (at 20 °C)
Thermal expansion 5.7 µm/(m·K) (at 25 °C)
Thermal conductivity 22.6 W/(m·K)
Electrical resistivity 421 nΩ·m (at 20 °C)
Magnetic ordering paramagnetic[3]
Young's modulus 88 GPa
Shear modulus 33 GPa
Bulk modulus 91.1 GPa
Poisson ratio 0.34
Mohs hardness 5.0
Vickers hardness 820–1800 MPa
Brinell hardness 638–1880 MPa
CAS Number 7440-67-7
History
Naming after zircon, zargun زرگون meaning "gold-colored".
Discovery Martin Heinrich Klaproth (1789)
First isolation Jöns Jakob Berzelius (1824)
Most stable isotopes of zirconium
iso NA half-life DM DE (MeV) DP
88Zr syn 83.4 d ε 88Y
γ 0.392D
89Zr syn 78.4 h ε 89Y
β+ 0.902 89Y
γ 0.909D
90Zr 51.45% is stable with 50 neutrons
91Zr 11.22% is stable with 51 neutrons
92Zr 17.15% is stable with 52 neutrons
93Zr trace 1.53×106 y β 0.060 93Nb
94Zr 17.38% is stable with 54 neutrons
96Zr 2.80% 2.0×1019 y[4] ββ 3.348 96Mo
| references | in Wikidata

Zirconium is a chemical element with symbol Zr and atomic number 40. The name of zirconium is taken from the name of the mineral zircon, the most important source of zirconium. The word zircon comes from the Persian word zargun زرگون, meaning "gold-colored".[5] It is a lustrous, grey-white, strong transition metal that resembles hafnium and, to a lesser extent, titanium. Zirconium is mainly used as a refractory and opacifier, although small amounts are used as an alloying agent for its strong resistance to corrosion. Zirconium forms a variety of inorganic and organometallic compounds such as zirconium dioxide and zirconocene dichloride, respectively. Five isotopes occur naturally, three of which are stable. Zirconium compounds have no known biological role.

Characteristics[edit]

Zirconium is a lustrous, greyish-white, soft, ductile and malleable metal that is solid at room temperature, though it is hard and brittle at lesser purities.[6][7] In powder form, zirconium is highly flammable, but the solid form is much less prone to ignition. Zirconium is highly resistant to corrosion by alkalis, acids, salt water and other agents.[8] However, it will dissolve in hydrochloric and sulfuric acid, especially when fluorine is present.[9] Alloys with zinc are magnetic at less than 35 K.[8]

The melting point of zirconium is 1855 °C (3371 °F), and the boiling point is 4371 °C (7900 °F).[8] Zirconium has an electronegativity of 1.33 on the Pauling scale. Of the elements within the d-block, zirconium has the fourth lowest electronegativity after yttrium, lanthanum (or lutetium), and hafnium.[10]

At room temperature zirconium exhibits a hexagonally close packed crystal structure, α-Zr, which changes to β-Zr a body-centered cubic crystal structure at 863 °C. Zirconium exists in the β-phase until the melting point.[11]

Isotopes[edit]

A zirconium rod
Main article: Isotopes of zirconium

Naturally occurring zirconium is composed of five isotopes. 90Zr, 91Zr, 92Zr and 94Zr are stable, although 94Zr is predicted to undergo double beta decay (not observed experimentally) with a half-life of more than 1.10×1017 years. 96Zr has a half-life of 2.4×1019 years, and is the longest-lived radioisotope of zirconium. Of these natural isotopes, 90Zr is the most common, making up 51.45% of all zirconium. 96Zr is the least common, comprising only 2.80% of zirconium.[12]

Twenty-eight artificial isotopes of zirconium have been synthesized, ranging in atomic mass from 78 to 110. 93Zr is the longest-lived artificial isotope, with a half-life of 1.53×106 years. 110Zr, the heaviest isotope of zirconium, is the most radioactive, with an estimated half-life of 30 milliseconds. Radioactive isotopes at or above mass number 93 decay by electron emission, whereas those at or below 89 decay by positron emission. The only exception is 88Zr, which decays by electron capture.[12]

Five isotopes of zirconium also exist as metastable isomers: 83mZr, 85mZr, 89mZr, 90m1Zr, 90m2Zr and 91mZr. Of these, 90m2Zr has the shortest half-life at 131 nanoseconds. 89mZr is the longest lived with a half-life of 4.161 minutes.[12]

Occurrence[edit]

World production trend of zirconium mineral concentrates

Zirconium has a concentration of about 130 mg/kg within the Earth's crust and about 0.026 μg/L in sea water.[13] It is not found in nature as a native metal, reflecting its intrinsic instability with respect to water. The principal commercial source of zirconium is zircon (ZrSiO4), a silicate mineral,[6] which is found primarily in Australia, Brazil, India, Russia, South Africa and the United States, as well as in smaller deposits around the world.[7] As of 2013, two-thirds of zircon mining occurs in Australia and South Africa.[14] Zircon resources exceed 60 million tonnes worldwide[15] and annual worldwide zirconium production is approximately 900,000 tonnes.[13] Zirconium also occurs in more than 140 other minerals, including the commercially useful ores baddeleyite and kosnarite.[16]

Zirconium 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 missions to the moon have a high zirconium oxide content relative to terrestrial rocks.[8]

Production[edit]

Zirconium output in 2005

Zirconium is a by-product of the mining and processing of the titanium minerals ilmenite and rutile, as well as tin mining.[17] From 2003 to 2007, while prices for the mineral zircon steadily increased from $360 to $840 per tonne, the price for unwrought zirconium metal decreased from $39,900 to $22,700 per ton. Zirconium metal is much higher priced than zircon because the reduction processes are expensive.[15]

Collected from coastal waters, zircon-bearing sand is purified by spiral concentrators to remove lighter materials, which are then returned to the water because they are natural components of beach sand. Using magnetic separation, the titanium ores ilmenite and rutile are removed.

Most zircon is used directly in commercial applications, but a small percentage is converted to the metal. Most Zr metal is produced by the reduction of the zirconium(IV) chloride with magnesium metal in the Kroll process.[8] Commercial-quality zirconium for most uses still has a content of 1% to 3% hafnium.[18] This contaminant is important only in nuclear applications. The resulting metal is sintered until sufficiently ductile for metalworking.[7]

Separation of zirconium and hafnium[edit]

Commercial zirconium metal typically contains 1–2.5% of hafnium, which is not problematic because the chemical properties of hafnium and zirconium are very similar. Their neutron-absorbing properties differ strongly, however, necessitating the separation of hafnium from zirconium for nuclear reactors.[19] Several separation schemes are in use.[18] The liquid-liquid extraction of the thiocyanate-oxide derivatives exploits the fact that the hafnium derivative is slightly more soluble in methyl isobutyl ketone than in water. This method is used mainly in United States.

Zr and Hf can also be separated by fractional crystallization of potassium hexafluorozirconate (K2ZrF6), which is less soluble in water than the analogous hafnium derivative.

Fractional distillation of the tetrachlorides, also called extractive distillation, is used primarily in Europe.

The product of a quadruple VAM (vacuum arc melting) process, combined with hot extruding and different rolling applications is cured using high-pressure, high-temperature gas autoclaving. This produces reactor-grade zirconium that is about 10 times more expensive than the hafnium-contaminated commercial grade.

Hafnium must be removed from zirconium for nuclear applications because hafnium has a neutron absorption cross-section 600 times greater than zirconium.[20] The separated hafnium can be used for reactor control rods.[21]

Compounds[edit]

See also: the categories Zirconium compounds, and Zirconium minerals.

Like other transition metals, zirconium forms a wide range of inorganic compounds and coordination complexes.[22] In general, these compounds are colourless diamagnetic solids wherein zirconium has the oxidation state +4. Far fewer Zr(III) compounds are known, and Zr(II) is very rare.

Oxides, nitrides and carbides[edit]

The most common oxide is zirconium dioxide, ZrO2, also known as zirconia. This colourless solid has exceptional fracture toughness and chemical resistance, especially in its cubic form.[23] These properties make zirconia useful as a thermal barrier coating,[24] although it is also a common diamond substitute.[23] Zirconium monoxide, ZrO, is also known and S-type stars are recognised by detection of its emission lines in the visual spectrum.[25]

Zirconium tungstate has the unusual property of shrinking in all dimensions when heated, whereas most other substances expand when heated.[8] Zirconyl chloride is a rare water-soluble zirconium complex with the relatively complicated formula [Zr4(OH)12(H2O)16]Cl8.

Zirconium carbide and zirconium nitride are refractory solids. The carbide is used for drilling tools and cutting edges. Zirconium hydride phases are also known.

Halides and pseudohalides[edit]

All four common halides are known, ZrF4, ZrCl4, ZrBr4, ZrI4. All have polymeric structures and are far less volatile than the corresponding monomeric titanium tetrahalides. All tend to hydrolyse to give the so-called oxyhalides and dioxides.

The corresponding tetraalkoxides are also known. Unlike the halides, the alkoxides dissolve in nonpolar solvents. Dihydrogen hexafluorozirconate is used in the metal finishing industry as an etching agent to promote paint adhesion.[26]

Organic derivatives[edit]

Zirconocene dichloride, a representative organozirconium compound.

Organozirconium chemistry is the study of compounds containing a carbon-zirconium bond. The first such compound was zirconocene dibromide ((C5H5)2ZrBr2), reported in 1952 by Birmingham and Wilkinson.[27] Schwartz's reagent, prepared in 1970 by P. C. Wailes and H. Weigold,[28] is a metallocene used in organic synthesis for transformations of alkenes and alkynes.[29]

Zirconium is also a component of some Ziegler-Natta catalysts, used to produce polypropylene. This application exploits the ability of zirconium to reversibly form bonds to carbon. Most complexes of Zr(II) are derivatives of zirconocene, one example being (C5Me5)2Zr(CO)2.

History[edit]

The zirconium-containing mineral zircon and related minerals (jargoon, hyacinth, jacinth, ligure) were mentioned in biblical writings.[8][19] The mineral was not known to contain a new element until 1789,[30] when Klaproth analyzed a jargoon from the island of Ceylon (now Sri Lanka). He named the new element Zirkonerde (zirconia).[8] Humphry Davy attempted to isolate this new element in 1808 through electrolysis, but failed.[6] Zirconium metal was first obtained in an impure form in 1824 by Berzelius by heating a mixture of potassium and potassium zirconium fluoride in an iron tube.[8]

The crystal bar process (also known as the 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 metallic zirconium. It involves the formation and subsequent thermal decomposition of zirconium tetraiodide, and was superseded in 1945 by the much cheaper Kroll process developed by William Justin Kroll, in which zirconium tetrachloride is reduced by magnesium:[7][31]

ZrCl4 + 2 Mg → Zr + 2 MgCl2

Applications[edit]

Approximately 900,000 tonnes of Zr ores were mined in 1995, mostly as zircon.[18]

Compounds[edit]

Most zircon is used directly in high temperature applications. This material is refractory, hard, and resistant to chemical attack. Because of these properties, zircon finds many applications, few of which are highly publicized. Its main use is as an opacifier, conferring a white, opaque appearance to ceramic materials. Because of its chemical resistance, zircon is also used in aggressive environments, such as moulds for molten metals.

Zirconium dioxide (ZrO2) is used in laboratory crucibles, in metallurgical furnaces, and as a refractory material.[8] Because it is mechanically strong and flexible, it can be sintered into ceramic knives and other blades.[32] Zircon (ZrSiO4) and the cubic zirconia (ZrO2) are cut into gemstones for use in jewelry.

Zirconia is a component in some abrasives, such as grinding wheels and sandpaper.[30]

Metal[edit]

A small fraction of the zircon is converted to the metal, which finds various niche applications. Because of zirconium's excellent resistance to corrosion, it is often used as an alloying agent in materials that are exposed to aggressive environments, such as surgical appliances, light filaments, and watch cases. The high reactivity of zirconium with oxygen at high temperatures is exploited in some specialised applications such as explosive primers and as getters in vacuum tubes. The same property is (probably) the purpose of including Zr nano-particles as pyrophoric material in explosive weapons such as the BLU-97/B Combined Effects Bomb.

Nuclear applications[edit]

Cladding for nuclear reactor fuels consumes about 1% of the zirconium supply,[18] mainly in the form of zircaloys. The desired properties of these alloys are a low neutron-capture cross-section and resistance to corrosion under normal service conditions.[7][8] Efficient methods for removing the hafnium impurities were developed to serve this purpose.

One disadvantage of zirconium alloys is that zirconium reacts with water at high temperatures, producing hydrogen gas and accelerated degradation of the fuel rod cladding:

Zr + 2 H2O → ZrO2 + 2 H2

This exothermic reaction is very slow below 100 °C, but at temperature above 900 °C the reaction is rapid. Most metals undergo similar reactions. The redox reaction is relevant to the instability of fuel assemblies at high temperatures.[33] This reaction was responsible for a small hydrogen explosion first observed inside the reactor building of Three Mile Island nuclear power plant in 1979, but at that time, the containment building was not damaged. The same reaction occurred in the reactors 1, 2 and 3 of the Fukushima I Nuclear Power Plant (Japan) after the reactor cooling was interrupted by the earthquake and tsunami disaster of March 11, 2011 leading to the Fukushima I nuclear accidents. After venting the hydrogen in the maintenance hall of those three reactors, the mixture of hydrogen with atmospheric oxygen exploded, severely damaging the installations and at least one of the containment buildings. To avoid explosion, the direct venting of hydrogen to the open atmosphere would have been a preferred design option. Now, to prevent the risk of explosion in many pressurized water reactor (PWR) containment buildings, a catalyst-based recombinator is installed that converts hydrogen and oxygen into water at room temperature before the hazard arises.

Space and aeronautic industries[edit]

Materials fabricated from zirconium metal and ZrO2 are used in space vehicles where resistance to heat is needed.[19]

High temperature parts such as combustors, blades, and vanes in jet engines and stationary gas turbines are increasingly being protected by thin ceramic layers, usually composed of a mixture of zirconia and yttria.[34]

Positron emission tomography cameras[edit]

The isotope 89Zr has been applied to the tracking and quantification of molecular antibodies with positron emission tomography (PET) cameras (a method called "immuno-PET"). Immuno-PET has reached a maturity of technical development and is now entering the phase of wide-scale clinical applications.[35][36][37] Until recently, radiolabeling with 89Zr was a complicated procedure requiring multiple steps. In 2001–2003 an improved multistep procedure was developed using a succinylated derivative of desferrioxamine B (N-sucDf) as a bifunctional chelate,[38] and a better way of binding 89Zr to mAbs was reported in 2009. The new method is fast, consists of only two steps, and uses two widely available ingredients: 89Zr and the appropriate chelate.[39]

Biomedical applications[edit]

Zirconium-bearing compounds are used in many biomedical applications, including dental implants, knee and hip replacements, middle-ear ossicular chain reconstruction, and other restorative and prosthetic devices.[40]

Zirconium binds urea, a property that has been utilized extensively to the benefit of patients with chronic kidney disease.[40] For example, zirconium is a primary component of the sorbent column dependent dialysate regeneration and recirculation system known as the REDY system, which was first introduced in 1973. More than 2,000,000 dialysis treatments have been performed using the sorbent column in the REDY system.[41] Although the REDY system was superseded in the 1990s by less expensive alternatives, new sorbent-based dialysis systems are being evaluated and approved by the U.S. Food and Drug Administration (FDA). Renal Solutions developed the DIALISORB technology, a portable, low water dialysis system. Also, developmental versions of a Wearable Artificial Kidney have incorporated sorbent-based technologies.[citation needed]

Zirconium cyclosilicate is under investigation for oral therapy in the treatment of hyperkalemia. It is a highly selective oral sorbent designed specifically to trap potassium ions in preference to other ions throughout the gastrointestinal tract.[42]

Defunct applications[edit]

Zirconium carbonate (3ZrO2·CO2·H2O) was used in lotions to treat poison ivy but was discontinued because it occasionally caused skin reactions.[6]

Safety[edit]

Although zirconium has no known biological role, the human body contains, on average, 250 milligrams of zirconium, and daily intake is approximately 4.15 milligrams (3.5 milligrams from food and 0.65 milligrams from water), depending on dietary habits.[43] Zirconium is widely distributed in nature and is found in all biological systems, for example: 2.86 μg/g in whole wheat, 3.09 μg/g in brown rice, 0.55 μg/g in spinach, 1.23 μg/g in eggs, and 0.86 μg/g in ground beef.[44] Further, zirconium is commonly used in commercial products (e.g. deodorant sticks, aerosol antiperspirants) and also in water purification (e.g. control of phosphorus pollution, bacteria- and pyrogen-contaminated water).[40]

Short-term exposure to zirconium powder can cause irritation, but only contact with the eyes requires medical attention.[45] Persistent exposure to zirconium tetrachloride results in increased mortality in rats and guinea pigs and a decrease of blood hemoglobin and red blood cells in dogs. However, in a study of 20 rats given a standard diet containing ~4% zirconium oxide, there were no adverse effects on growth rate, blood and urine parameters, or mortality.[46] The U.S. Occupational Safety and Health Administration (OSHA) legal limit (permissible exposure limit) for zirconium exposure is 5 mg/m3 over an 8-hour workday. The National Institute for Occupational Safety and Health (NIOSH) recommended exposure limit (REL) is 5 mg/m3 over an 8-hour workday and a short term limit of 10 mg/m3. At levels of 25 mg/m3, zirconium is immediately dangerous to life and health.[47] However, zirconium is not considered an industrial health hazard.[40] Furthermore, reports of zirconium-related adverse reactions are rare and, in general, rigorous cause-and-effect relationships have not been established.[40] No evidence has been validated that zirconium is carcinogenic or genotoxic.[48]

Among the numerous radioactive isotopes of zirconium, 93Zr is among the most common. It is released as a product of 235U, mainly in nuclear plants and during nuclear weapons tests in the 1950s and 1960s. It has a very long half-life (1.53 million years), its decay emits only low energy radiations, and it is not considered as highly hazardous.[citation needed]

See also[edit]

References[edit]

  1. ^ Standard Atomic Weights 2013. Commission on Isotopic Abundances and Atomic Weights
  2. ^ "Zirconium: zirconium(I) fluoride compound data". OpenMOPAC.net. Retrieved 2007-12-10. 
  3. ^ Lide, D. R., ed. (2005). "Magnetic susceptibility of the elements and inorganic compounds". CRC Handbook of Chemistry and Physics (PDF) (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5. 
  4. ^ Pritychenko, Boris; Tretyak, V. "Adopted Double Beta Decay Data". National Nuclear Data Center. Retrieved 2008-02-11. 
  5. ^ Harper, Douglas. "zircon". Online Etymology Dictionary. 
  6. ^ a b c d Emsley, John (2001). Nature's Building Blocks. Oxford: Oxford University Press. pp. 506–510. ISBN 0-19-850341-5. 
  7. ^ a b c d e "Zirconium". How Products Are Made. Advameg Inc. 2007. Retrieved 2008-03-26. 
  8. ^ a b c d e f g h i j k Lide, David R., ed. (2007–2008). "Zirconium". CRC Handbook of Chemistry and Physics. 4. New York: CRC Press. p. 42. ISBN 978-0-8493-0488-0. 
  9. ^ Considine, Glenn D., ed. (2005). "Zirconium". Van Nostrand's Encyclopedia of Chemistry. New York: Wylie-Interscience. pp. 1778–1779. ISBN 0-471-61525-0. 
  10. ^ Winter, Mark (2007). "Electronegativity (Pauling)". University of Sheffield. Retrieved 2008-03-05. 
  11. ^ Schnell I & Albers RC (January 2006). "Zirconium under pressure: phase transitions and thermodynamics". Journal of Physics: Condensed Matter. Institute of Physics. 18 (5): 16. Bibcode:2006JPCM...18.1483S. doi:10.1088/0953-8984/18/5/001. 
  12. ^ a b c Audi, G; Bersillon, O.; Blachot, J.; Wapstra, A.H. (2003). "Nubase2003 Evaluation of Nuclear and Decay Properties". Nuclear Physics A. Atomic Mass Data Center. 729: 3–128. Bibcode:2003NuPhA.729....3A. doi:10.1016/j.nuclphysa.2003.11.001. 
  13. ^ a b Peterson, John; MacDonell, Margaret (2007). "Zirconium". Radiological and Chemical Fact Sheets to Support Health Risk Analyses for Contaminated Areas (PDF). Argonne National Laboratory. pp. 64–65. Retrieved 2008-02-26. 
  14. ^ "Zirconium and Hafnium - Mineral resources" (PDF). 2014. 
  15. ^ a b "Zirconium and Hafnium" (PDF). Mineral Commodity Summaries. US Geological Survey: 192–193. January 2008. Retrieved 2008-02-24. 
  16. ^ Ralph, Jolyon & Ralph, Ida (2008). "Minerals that include Zr". Mindat.org. Retrieved 2008-02-23. 
  17. ^ Callaghan, R. (2008-02-21). "Zirconium and Hafnium Statistics and Information". US Geological Survey. Retrieved 2008-02-24. 
  18. ^ a b c d Nielsen, Ralph (2005) "Zirconium and Zirconium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim. doi:10.1002/14356007.a28_543
  19. ^ a b c Stwertka, Albert (1996). A Guide to the Elements. Oxford University Press. pp. 117–119. ISBN 0-19-508083-1. 
  20. ^ Brady, George Stuart; Clauser, Henry R. & Vaccari, John A. (24 July 2002). Materials handbook: an encyclopedia for managers, technical professionals, purchasing and production managers, technicians, and supervisors. McGraw-Hill Professional. pp. 1063–. ISBN 978-0-07-136076-0. Retrieved 2011-03-18. 
  21. ^ Zardiackas, Lyle D.; Kraay, Matthew J. & Freese, Howard L. (1 January 2006). Titanium, niobium, zirconium and tantalum for medical and surgical applications. ASTM International. pp. 21–. ISBN 978-0-8031-3497-3. Retrieved 2011-03-18. 
  22. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9. 
  23. ^ a b "Zirconia". AZoM.com. 2008. Retrieved 2008-03-17. 
  24. ^ Gauthier, V.; Dettenwanger, F.; Schütze, M. (2002-04-10). "Oxidation behavior of γ-TiAl coated with zirconia thermal barriers". Intermetallics. Frankfurt, Germany: Karl Winnacker Institut der Dechema. 10 (7): 667–674. doi:10.1016/S0966-9795(02)00036-5. 
  25. ^ Keenan, P. C. (1954). "Classification of the S-Type Stars". Astrophysical Journal. 120: 484–505. doi:10.1086/145937. 
  26. ^ MSDS sheet for Duratec 400,DuBois Chemicals, Inc.
  27. ^ Wilkinson, G.; Birmingham, J. M. (1954). "Bis-cyclopentadienyl Compounds of Ti, Zr, V, Nb and Ta". J. Am. Chem. Soc. 76 (17): 4281–4284. doi:10.1021/ja01646a008. Rouhi, A. Maureen (2004-04-19). "Organozirconium Chemistry Arrives". Science & Technology. Chemical & Engineering News. 82 (16): 36–39. doi:10.1021/cen-v082n015.p035. ISSN 0009-2347. Retrieved 2008-03-17. 
  28. ^ Wailes, P. C. & Weigold, H. (1970). "Hydrido complexes of zirconium I. Preparation". Journal of Organometallic Chemistry. 24 (2): 405–411. doi:10.1016/S0022-328X(00)80281-8. 
  29. ^ Hart, D. W. & Schwartz, J. (1974). "Hydrozirconation. Organic Synthesis via Organozirconium Intermediates. Synthesis and Rearrangement of Alkylzirconium(IV) Complexes and Their Reaction with Electrophiles". J. Am. Chem. Soc. 96 (26): 8115–8116. doi:10.1021/ja00833a048. 
  30. ^ a b Krebs, Robert E. (1998). The History and Use of our Earth's Chemical Elements. Westport, Connecticut: Greenwood Press. pp. 98–100. ISBN 0-313-30123-9. 
  31. ^ Hedrick, James B. (1998). "Zirconium". Metal Prices in the United States through 1998 (PDF). US Geological Survey. pp. 175–178. Retrieved 2008-02-26. 
  32. ^ "Fine ceramics - zirconia". Kyocera Inc. 
  33. ^ Luc Gillon (1979). Le nucléaire en question, Gembloux Duculot, French edition, 240 pp.
  34. ^ Meier, S. M.; Gupta, D. K. (1994). "The Evolution of Thermal Barrier Coatings in Gas Turbine Engine Applications". Journal of Engineering for Gas Turbines and Power. 116: 250. doi:10.1115/1.2906801. 
  35. ^ Heuveling, Derek A.; Visser, Gerard W. M.; Baclayon, Marian; Roos, Wouter H.; Wuite, Gijs J. L.; Hoekstra, Otto S.; Leemans, C. René; de Bree, Remco; van Dongen, Guus A. M. S. (2011). "89Zr-Nanocolloidal Albumin–Based PET/CT Lymphoscintigraphy for Sentinel Node Detection in Head and Neck Cancer: Preclinical Results". The Journal of Nuclear Medicine. 52 (10): 1580–1584. doi:10.2967/jnumed.111.089557. PMID 21890880. 
  36. ^ van Rij, Catharina M.; Sharkey, Robert M.; Goldenberg, David M.; Frielink, Cathelijne; Molkenboer, Janneke D. M.; Franssen, Gerben M.; van Weerden, Wietske M.; Oyen, Wim J. G.; Boerman, Otto C. (2011). "Imaging of Prostate Cancer with Immuno-PET and Immuno-SPECT Using a Radiolabeled Anti-EGP-1 Monoclonal Antibody". The Journal of Nuclear Medicine. 52 (10): 1601–1607. doi:10.2967/jnumed.110.086520. PMID 21865288. 
  37. ^ Ruggiero, A; Holland, JP; Hudolin, T; Shenker, L; Koulova, A; Bander, NH; Lewis, JS; Grimm, J (2011). "Targeting the internal epitope of prostate-specific membrane antigen with 89Zr-7E11 immuno-PET". The Journal of Nuclear Medicine. 52 (10): 1608–15. doi:10.2967/jnumed.111.092098. PMC 3537833Freely accessible. PMID 21908391. 
  38. ^ Verel, I; Visser, GW; Boellaard, R; Stigter-Van Walsum, M; Snow, GB; Van Dongen, GA (2003). "89Zr immuno-PET: Comprehensive procedures for the production of 89Zr-labeled monoclonal antibodies" (PDF). J Nucl Med. 44 (8): 1271–81. PMID 12902418. 
  39. ^ Perk, L, "The Future of Immuno-PET in Drug Development Zirconium-89 and Iodine-124 as Key Factors in Molecular Imaging" Archived April 25, 2012, at the Wayback Machine., Amsterdam, Cyclotron, 2009.
  40. ^ a b c d e Lee DBN, Roberts M, Bluchel CG, Odell RA. (2010) Zirconium: Biomedical and nephrological applications. ASAIO J 56(6):550-556.
  41. ^ Ash SR. Sorbents in treatment of uremia: A short history and a great future. 2009 Semin Dial 22: 615-622
  42. ^ Ingelfinger, Julie R. (2015). "A New Era for the Treatment of Hyperkalemia?". New England Journal of Medicine. 372 (3): 275–7. doi:10.1056/NEJMe1414112. PMID 25415806. 
  43. ^ Schroeder, HA; Balassa JJ (1966). "Abnormal trace materials in man: Zirconium". J Chron Dis. 19 (5): 573–586. doi:10.1016/0021-9681(66)90095-6. PMID 5338082. 
  44. ^ Schroeder HA and Balassa JJ. (1966) Abnormal trace materials in man: Zirconium. J Chron Dis 19: 573-586.
  45. ^ "Zirconium". International Chemical Safety Cards. International Labour Organization. October 2004. Retrieved 2008-03-30. 
  46. ^ Zirconium and its compounds 1999. The MAK Collection for Occupational Health and Safety. 224–236
  47. ^ "CDC - NIOSH Pocket Guide to Chemical Hazards - Zirconium compounds (as Zr)". www.cdc.gov. Retrieved 2015-11-27. 
  48. ^ toxnet.nlm.nih.gov/cgi-bin/sis/search/f?./temp/~EHRbeW:2

External links[edit]