Zirconium

Chemical element with atomic number 40

Not to be confused with zircon, zirconia, or cubic zirconia.

Chemical element, symbol Zr and atomic number 40

Zirconium, 40ZrFile:Zirconium crystal bar and 1cm3 cube.jpg

Zirconium
Pronunciation| /zɜːrˈkoʊniəm/ ​(zur-KOH-nee-əm)
Appearance| silvery white
Standard atomic weight Ar°(Zr)|

* 91.224±0.002
* 91.224±0.002 (abridged)[1]

Zirconium 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

yttrium ← zirconium → niobium
Atomic number (Z)| 40
Group| group 4
Period| period 5
Block|  d-block
Electron configuration| [Kr] 4d2 5s2
Electrons per shell| 2, 8, 18, 10, 2
Physical properties
Phase at STP| solid
Melting point| 2125 K ​(1852 °C, ​3365 °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| −2, 0, +1,[2] +2, +3, +4 (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

File:Zirconium spectrum visible.png

Spectral lines of zirconium
Other properties
Natural occurrence| primordial
Crystal structure|  ​hexagonal close-packed (hcp)

File:Hexagonal close packed.svg

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)
Main isotopes of zirconium
| Iso­tope | Abun­dance | Half-life (t1/2) | Decay mode | Pro­duct

|
|
|
|

88Zr  | syn | 83.4 d  | ε | 88Y
γ | –
89Zr  | syn  | 78.4 h  | ε  | 89Y
β+ | 89Y
γ  | –
90Zr  | 51.45%  | stable
91Zr  | 11.22%  | stable
92Zr  | 17.15%  | stable
93Zr  | trace | 1.53×106 y  | β− | 93Nb
94Zr  | 17.38%  | stable
96Zr  | 2.80%  | 2.0×1019 y[4] | β−β− | 96Mo
Category: Zirconium

* view
* talk
* edit

| references

Zirconium is a chemical element with the symbol Zr and atomic number 40\. The name zirconium is taken from the name of the mineral zircon, the most important source of zirconium. The word is related to Persian zargun (zircon; zar-gun, "gold-like" or "as gold").[5] It is a lustrous, grey-white, strong transition metal that closely 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, four of which are stable. Zirconium compounds have no known biological role.

## Contents

* 1 Characteristics
* 1.1 Isotopes
* 1.2 Occurrence
* 2 Production
* 2.1 Occurrence
* 2.2 Separation of zirconium and hafnium
* 3 Compounds
* 3.1 Oxides, nitrides, and carbides
* 3.2 Halides and pseudohalides
* 3.3 Organic derivatives
* 4 History
* 5 Applications
* 5.1 Compounds
* 5.2 Metal
* 5.2.1 Nuclear applications
* 5.2.2 Space and aeronautic industries
* 5.3 Medical uses
* 5.4 Defunct applications
* 6 Safety
* 7 See also
* 8 References
* 9 External links

## Characteristics[edit | edit source]

File:Zirconium rod.jpg

Zirconium rod

Zirconium is a lustrous, greyish-white, soft, ductile, malleable metal that is solid at room temperature, though it is hard and brittle at lesser purities.[6] 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.[7] However, it will dissolve in hydrochloric and sulfuric acid, especially when fluorine is present.[8] Alloys with zinc are magnetic at less than 35 K.[7]

The melting point of zirconium is 1855 °C (3371 °F), and the boiling point is 4409 °C (7968 °F).[7] Zirconium has an electronegativity of 1.33 on the Pauling scale. Of the elements within the d-block with known electronegativities, zirconium has the fifth lowest electronegativity after hafnium, yttrium, lanthanum, and actinium.[9]

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.[10]

### Isotopes[edit | edit source]

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.[11]

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.[11]

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.[11]

### Occurrence[edit | edit source]

See also: Category:Zirconium minerals

File:Zirconium mineral concentrates - world production trend.svg

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.[12] 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.[13] 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.[12] Zirconium also occurs in more than 140 other minerals, including the commercially useful ores baddeleyite and eudialyte.[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.[7]

EPR spectroscopy has been used in investigations of the unusual 3+ valence state of zirconium. The EPR spectrum of Zr3+, which has been initially observed as a parasitic signal in Fe‐doped single crystals of ScPO4, was definitively identified by preparing single crystals of ScPO4 doped with isotopically enriched (94.6%)91Zr. Single crystals of LuPO4 and YPO4 doped with both naturally abundant and isotopically enriched Zr have also been grown and investigated.[17]

## Production[edit | edit source]

### Occurrence[edit | edit source]

File:2005zirconium.PNG

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.[18] 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 more expensive than zircon because the reduction processes are costly.[15]

Collected from coastal waters, zircon-bearing sand is purified by spiral concentrators to separate 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.[7] The resulting metal is sintered until sufficiently ductile for metalworking.[13]

### Separation of zirconium and hafnium[edit | edit source]

Commercial zirconium metal typically contains 1–3% of hafnium,[19] which is usually 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.[20] Several separation schemes are in use.[19] 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. In India, TBP-Nitrate solvent extraction process is used for the separation

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.[21] The separated hafnium can be used for reactor control rods.[22]

## Compounds[edit | edit source]

See also the categories Zirconium compounds and Zirconium minerals

Like other transition metals, zirconium forms a wide range of inorganic compounds and coordination complexes.[23] 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 | edit source]

The most common oxide is zirconium dioxide, ZrO2, also known as zirconia. This clear to white-coloured solid has exceptional fracture toughness (for a ceramic) and chemical resistance, especially in its cubic form.[24] These properties make zirconia useful as a thermal barrier coating,[25] although it is also a common diamond substitute.[24] Zirconium monoxide, ZrO, is also known and S-type stars are recognised by detection of its emission lines.[26]

Zirconium tungstate has the unusual property of shrinking in all dimensions when heated, whereas most other substances expand when heated.[7] 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.

Lead zirconate titanate (PZT) is the most commonly used piezoelectric material, with applications such as ultrasonic transducers, hydrophones, common rail injectors, piezoelectric transformers and micro-actuators.

### Halides and pseudohalides[edit | edit source]

All four common halides are known, ZrF4, ZrCl4, ZrBr4, and 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.[27]

### Organic derivatives[edit | edit source]

File:Zirconocene-dichloride-from-xtal-3D-balls.png

Zirconocene dichloride, a representative organozirconium compound.

Organozirconium chemistry is key to Ziegler–Natta catalysts, used to produce polypropylene. This application exploits the ability of zirconium to reversibly form bonds to carbon. Zirconocene dibromide ((C5H5)2ZrBr2), reported in 1952 by Birmingham and Wilkinson, was the first organozirconium compound.[28] Schwartz's reagent, prepared in 1970 by P. C. Wailes and H. Weigold,[29] is a metallocene used in organic synthesis for transformations of alkenes and alkynes.[30]

Most complexes of Zr(II) are derivatives of zirconocene, one example being (C5Me5)2Zr(CO)2.

## History[edit | edit source]

The zirconium-containing mineral zircon and related minerals (jargoon, hyacinth, jacinth, ligure) were mentioned in biblical writings.[7][20] The mineral was not known to contain a new element until 1789,[31] when Klaproth analyzed a jargoon from the island of Ceylon (now Sri Lanka). He named the new element Zirkonerde (zirconia).[7] 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.[7]

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:[13][32]

ZrCl 4 + 2 Mg ⟶ Zr + 2 MgCl 2 {\displaystyle {\ce {ZrCl4 + 2Mg -> Zr + 2MgCl2}}}

## Applications[edit | edit source]

Approximately 900,000 tonnes of zirconium ores were mined in 1995, mostly as zircon.[19]

### Compounds[edit | edit source]

Most zircon is used directly in high-temperature applications. Because it is refractory, hard, and resistant to chemical attack, zircon finds many applications. 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.[7] Because it is mechanically strong and flexible, it can be sintered into ceramic knives and other blades.[33] Zircon (ZrSiO4) and cubic zirconia (ZrO2) are cut into gemstones for use in jewelry.

Zirconium dioxide is a component in some abrasives, such as grinding wheels and sandpaper.[31]

### Metal[edit | edit source]

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 nanoparticles as pyrophoric material in explosive weapons such as the BLU-97/B Combined Effects Bomb. Burning zirconium was used as a light source in some photographic flashbulbs. Zirconium powder with a mesh size from 10 to 80 is occasionally used in pyrotechnic compositions to generate sparks. The high reactivity of zirconium leads to bright white sparks.[34]

#### Nuclear applications[edit | edit source]

Cladding for nuclear reactor fuels consumes about 1% of the zirconium supply,[19] 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.[13][7] Efficient methods for removing the hafnium impurities were developed to serve this purpose.

One disadvantage of zirconium alloys is the reactivity with water, producing hydrogen, leading to degradation of the fuel rod cladding:

Zr + 2 H 2 O ⟶ ZrO 2 + 2 H 2 {\displaystyle {\ce {Zr + 2H2O -> ZrO2 + 2H2}}}

Hydrolysis is very slow below 100 °C, but rapid at temperature above 900 °C. Most metals undergo similar reactions. The redox reaction is relevant to the instability of fuel assemblies at high temperatures.[35] This 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.

Zirconium is a constituent of the uranium zirconium hydride (UZrH) nuclear fuel used in TRIGA reactors.

#### Space and aeronautic industries[edit | edit source]

Materials fabricated from zirconium metal and ZrO2 are used in space vehicles where resistance to heat is needed.[20]

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.[36]

### Medical uses[edit | edit source]

Zirconium-bearing compounds are used in many biomedical applications, including dental implants and crowns, knee and hip replacements, middle-ear ossicular chain reconstruction, and other restorative and prosthetic devices.[37]

Zirconium binds urea, a property that has been utilized extensively to the benefit of patients with chronic kidney disease.[37] 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.[38] 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]

Sodium zirconium cyclosilicate is used by mouth in the treatment of hyperkalemia. It is a selective sorbent designed to trap potassium ions in preference to other ions throughout the gastrointestinal tract.[39]

A mixture of monomeric and polymeric Zr4+ and Al3+ complexes with hydroxide, chloride and glycine, called Aluminium zirconium tetrachlorohydrex gly or AZG, is used in a preparation as an antiperspirant in many deodorant products. It is selected for its ability to obstruct pores in the skin and prevent sweat from leaving the body.

### Defunct applications[edit | edit source]

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 | edit source]

Zirconium  Hazards

NFPA 704 (fire diamond)  |

Error: Image is invalid or non-existent.

Chemical compound

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.[40] 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.[40] 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).[37]

Short-term exposure to zirconium powder can cause irritation, but only contact with the eyes requires medical attention.[41] 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.[42] 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.[43] However, zirconium is not considered an industrial health hazard.[37] Furthermore, reports of zirconium-related adverse reactions are rare and, in general, rigorous cause-and-effect relationships have not been established.[37] No evidence has been validated that zirconium is carcinogenic or genotoxic.[44]

Among the numerous radioactive isotopes of zirconium, 93Zr is among the most common. It is released as a product of nuclear fission of 235U and 239Pu, mainly in nuclear power 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.[45]

## See also[edit | edit source]

* Zirconium alloys
* Zirconia light

## References[edit | edit source]

1. ^ "Standard Atomic Weights: Zirconium". CIAAW. 1983.
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 978-0-19-850341-5.
7. ^ a b c d e f g h i j k Lide, David R., ed. (2007–2008). "Zirconium". CRC Handbook of Chemistry and Physics. Vol. 4\. New York: CRC Press. p. 42\. ISBN 978-0-8493-0488-0.
8. ^ Considine, Glenn D., ed. (2005). "Zirconium". Van Nostrand's Encyclopedia of Chemistry. New York: Wylie-Interscience. pp. 1778–1779. ISBN 978-0-471-61525-5.
9. ^ Winter, Mark (2007). "Electronegativity (Pauling)". University of Sheffield. Retrieved 2008-03-05.
10. ^ Schnell I & Albers RC (January 2006). "Zirconium under pressure: phase transitions and thermodynamics". Journal of Physics: Condensed Matter. 18 (5): 16. Bibcode:2006JPCM...18.1483S. doi:10.1088/0953-8984/18/5/001. S2CID 56557217.
11. ^ a b c Audi, Georges; Bersillon, Olivier; Blachot, Jean; Wapstra, Aaldert Hendrik (2003), "The NUBASE evaluation of nuclear and decay properties", Nuclear Physics A, 729: 3–128, Bibcode:2003NuPhA.729....3A, doi:10.1016/j.nuclphysa.2003.11.001
12. ^ 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. Archived from the original (PDF) on 2008-05-28. Retrieved 2008-02-26.
13. ^ a b c d "Zirconium". How Products Are Made. Advameg Inc. 2007. Retrieved 2008-03-26.
14. ^ "Zirconium and Hafnium - Mineral resources" (PDF). 2014.
15. ^ a b "Zirconium and Hafnium" (PDF). Mineral Commodity Summaries: 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. ^ Abraham, M. M.; Boatner, L. A.; Ramey, J. O.; Rappaz, M. (1984-12-20). "The occurrence and stability of trivalent zirconium in orthophosphate single crystals". The Journal of Chemical Physics. 81 (12): 5362–5366. Bibcode:1984JChPh..81.5362A. doi:10.1063/1.447678. ISSN 0021-9606.
18. ^ Callaghan, R. (2008-02-21). "Zirconium and Hafnium Statistics and Information". US Geological Survey. Retrieved 2008-02-24.
19. ^ 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
20. ^ a b c Stwertka, Albert (1996). A Guide to the Elements. Oxford University Press. pp. 117–119. ISBN 978-0-19-508083-4.
21. ^ 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.
22. ^ 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.
23. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
24. ^ a b "Zirconia". AZoM.com. 2008. Retrieved 2008-03-17.
25. ^ Gauthier, V.; Dettenwanger, F.; Schütze, M. (2002-04-10). "Oxidation behavior of γ-TiAl coated with zirconia thermal barriers". Intermetallics. 10 (7): 667–674. doi:10.1016/S0966-9795(02)00036-5.
26. ^ Keenan, P. C. (1954). "Classification of the S-Type Stars". Astrophysical Journal. 120: 484–505. Bibcode:1954ApJ...120..484K. doi:10.1086/145937.
27. ^ MSDS sheet for Duratec 400, DuBois Chemicals, Inc.
28. ^ Wilkinson, G.; Birmingham, J. M. (1954). "Bis-cyclopentadienyl Compounds of Ti, Zr, V, Nb and Ta". Journal of the American Chemical Society. 76 (17): 4281–4284. doi:10.1021/ja01646a008.; Rouhi, A. Maureen (2004-04-19). "Organozirconium Chemistry Arrives". Chemical & Engineering News. 82 (16): 36–39. doi:10.1021/cen-v082n016.p036. ISSN 0009-2347. Retrieved 2008-03-17.
29. ^ 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.
30. ^ Hart, D. W. & Schwartz, J. (1974). "Hydrozirconation. Organic Synthesis via Organozirconium Intermediates. Synthesis and Rearrangement of Alkylzirconium(IV) Complexes and Their Reaction with Electrophiles". Journal of the American Chemical Society. 96 (26): 8115–8116. doi:10.1021/ja00833a048.
31. ^ a b Krebs, Robert E. (1998). The History and Use of our Earth's Chemical Elements. Westport, Connecticut: Greenwood Press. pp. 98–100. ISBN 978-0-313-30123-0.
32. ^ Hedrick, James B. (1998). "Zirconium". Metal Prices in the United States through 1998 (PDF). US Geological Survey. pp. 175–178. Retrieved 2008-02-26.
33. ^ "Fine ceramics - zirconia". Kyocera Inc.
34. ^ Kosanke, Kenneth L.; Kosanke, Bonnie J. (1999), "Pyrotechnic Spark Generation", Journal of Pyrotechnics: 49–62, ISBN 978-1-889526-12-6
35. ^ Gillon, Luc (1979). Le nucléaire en question, Gembloux Duculot, French edition.
36. ^ 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: 250–257. doi:10.1115/1.2906801. S2CID 53414132.
37. ^ 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.
38. ^ Ash SR. Sorbents in treatment of uremia: A short history and a great future. 2009 Semin Dial 22: 615-622
39. ^ 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.
40. ^ a b Schroeder, Henry A.; Balassa, Joseph J. (May 1966). "Abnormal trace metals in man: zirconium". Journal of Chronic Diseases. 19 (5): 573–586. doi:10.1016/0021-9681(66)90095-6. PMID 5338082.
41. ^ "Zirconium". International Chemical Safety Cards. International Labour Organization. October 2004. Retrieved 2008-03-30.
42. ^ Zirconium and its compounds 1999. The MAK Collection for Occupational Health and Safety. 224–236
43. ^ "CDC - NIOSH Pocket Guide to Chemical Hazards - Zirconium compounds (as Zr)". www.cdc.gov. Retrieved 2015-11-27.
44. ^ toxnet.nlm.nih.gov/cgi-bin/sis/search/f?./temp/~EHRbeW:2
45. ^ "ANL Human Health Fact Sheet: Zirconium (October 2001)" (PDF). Argonne National Laboratory. Retrieved 15 July 2020.

## External links[edit | edit source]

Justapedia supports:

* File:Wiktionary-logo-v2.svgDefinitions from Wiktionary
* File:Commons-logo.svgMedia from Commons

* Chemistry in its element podcast (MP3) from the Royal Society of Chemistry's Chemistry World: Zirconium
* Zirconium at The Periodic Table of Videos (University of Nottingham)

* v
* t
* e

Periodic table

|  | 1 | 2 |  | 3 | 4 | 5 | 6 | 7 | 8 | 9 | 10 | 11 | 12 | 13 | 14 | 15 | 16 | 17 | 18

|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|

1 | H |  | He
2 | Li | Be |  | B | C | N | O | F | Ne
3 | Na | Mg |  | Al | Si | P | S | Cl | Ar
4 | K | Ca |  | Sc | Ti | V | Cr | Mn | Fe | Co | Ni | Cu | Zn | Ga | Ge | As | Se | Br | Kr
5 | Rb | Sr |  | Y | Zr | Nb | Mo | Tc | Ru | Rh | Pd | Ag | Cd | In | Sn | Sb | Te | I | Xe
6 | Cs | Ba | La | Ce | Pr | Nd | Pm | Sm | Eu | Gd | Tb | Dy | Ho | Er | Tm | Yb | Lu | Hf | Ta | W | Re | Os | Ir | Pt | Au | Hg | Tl | Pb | Bi | Po | At | Rn
7 | Fr | Ra | Ac | Th | Pa | U | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og

| s-block | f-block | d-block | p-block

|
|
|

* v
* t
* e

Zirconium compounds

Zr(II)|

* ZrB2
* ZrH2
* ZrSi2

Zr(III)|

* ZrN
* ZrCl3
* ZrBr3
* ZrI3

Zr(IV)|

* ZrBr4
* ZrC
* ZrCl4
* ZrF4
* ZrI4
* Zr(NO3)4
* ZrOCl2
* Zr(OH)4
* ZrO2
* Zr(HPO4)2
* ZrS2
* Zr(SO4)2
* ZrSiO4
* Zr(WO4)2

| Organozirconium(IV)|

* Zr(acac)4
* Cp2ZrCl2

|

*[r.t.]: room temperature
*[m.p.]: melting point
*[P]: Pressure (in Pascal)
*[T]: Temperature (in kelvins)
*[v]: View this template
*[t]: Discuss this template
*[e]: Edit this template