Zirconium

Zirconium, 40Zr
Zirconium
Pronunciation/zɜːrˈkoʊniəm/ ⓘ ​(zur-KOH-nee-əm)
Appearancesilvery white
Standard atomic weight Ar°(Zr)
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 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
Ti
↑
Zr
↓
Hf
yttrium ← zirconium → niobium
Atomic number (Z)40
Groupgroup 4
Periodperiod 5
Block  d-block
Electron configuration[Kr] 4d2 5s2
Electrons per shell2, 8, 18, 10, 2
Physical properties
Phase at STPsolid
Melting point2125 K ​(1852 °C, ​3365 °F)
Boiling point4650 K ​(4377 °C, ​7911 °F)
Density (at 20° C)6.505 g/cm3[3]
when liquid (at m.p.)5.8 g/cm3
Heat of fusion14 kJ/mol
Heat of vaporization591 kJ/mol
Molar heat capacity25.36 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 statescommon: +4
−2,[4] 0,[5] +1,[6] +2,[7][8] +3[6]
ElectronegativityPauling scale: 1.33
Ionization energies
  • 1st: 640.1 kJ/mol
  • 2nd: 1270 kJ/mol
  • 3rd: 2218 kJ/mol
Atomic radiusempirical: 160 pm
Covalent radius175±7 pm
Spectral lines of zirconium
Other properties
Natural occurrenceprimordial
Crystal structure ​hexagonal close-packed (hcp) (hP2)
Lattice constants
a = 323.22 pm
c = 514.79 pm (at 20 °C)[3]
Thermal expansion5.69×10−6/K (at 20 °C)[3][a]
Thermal conductivity22.6 W/(m⋅K)
Electrical resistivity421 nΩ⋅m (at 20 °C)
Magnetic orderingparamagnetic[9]
Young's modulus88 GPa
Shear modulus33 GPa
Bulk modulus91.1 GPa
Speed of sound thin rod3800 m/s (at 20 °C)
Poisson ratio0.34
Mohs hardness5.0
Vickers hardness820–1800 MPa
Brinell hardness638–1880 MPa
CAS Number7440-67-7
History
Namingafter zircon, zargun زرگون meaning "gold-colored".
DiscoveryMartin Heinrich Klaproth (1789)
First isolationJöns Jakob Berzelius (1824)
Isotopes of zirconium
Main isotopes[10] Decay
abun­dance half-life (t1/2) mode pro­duct
88Zr synth 83.4 d ε 88Y
89Zr synth 78.4 h β+ 89Y
90Zr 51.5% stable
91Zr 11.2% stable
92Zr 17.1% stable
93Zr trace 1.61×106 y β− 93Nb
94Zr 17.4% stable
95Zr synth 64.032 d β− 95Nb
96Zr 2.80% 2.34×1019 y β−β− 96Mo

Zirconium is a chemical element; it has symbol Zr and atomic number 40. First identified in 1789, isolated in impure form in 1824, and manufactured at scale by 1925, pure zirconium is a lustrous transition metal with a greyish-white color that closely resembles hafnium and, to a lesser extent, titanium. It is solid at room temperature, ductile, malleable and corrosion-resistant. The name zirconium is derived 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").[11] Besides zircon, zirconium occurs in over 140 other minerals, including baddeleyite and eudialyte; most zirconium is produced as a byproduct of minerals mined for titanium and tin.

Zirconium forms a variety of inorganic compounds, such as zirconium dioxide, and organometallic compounds, such as zirconocene dichloride. Five isotopes occur naturally, four of which are stable. The metal and its alloys are mainly used as a refractory and opacifier; zirconium alloys are used to clad nuclear fuel rods due to their low neutron absorption and strong resistance to corrosion, and in space vehicles and turbine blades where high heat resistance is necessary. Zirconium also finds uses in flashbulbs, biomedical applications such as dental implants and prosthetics, deodorant, and water purification systems.

Zirconium compounds have no known biological role, though the element is widely distributed in nature and appears in small quantities in biological systems without adverse effects. There is no indication of zirconium as a carcinogen. The main hazards posed by zirconium are flammability in powder form and irritation of the eyes.

  1. ^ "Standard Atomic Weights: Zirconium". CIAAW. 2024.
  2. ^ Prohaska, Thomas; Irrgeher, Johanna; Benefield, Jacqueline; Böhlke, John K.; Chesson, Lesley A.; Coplen, Tyler B.; Ding, Tiping; Dunn, Philip J. H.; Gröning, Manfred; Holden, Norman E.; Meijer, Harro A. J. (2022-05-04). "Standard atomic weights of the elements 2021 (IUPAC Technical Report)". Pure and Applied Chemistry. doi:10.1515/pac-2019-0603. ISSN 1365-3075.
  3. ^ a b c d Arblaster, John W. (2018). Selected Values of the Crystallographic Properties of Elements. Materials Park, Ohio: ASM International. ISBN 978-1-62708-155-9.
  4. ^ Zr(–2) is known in Zr(CO)2−6; see John E. Ellis (2006). "Adventures with Substances Containing Metals in Negative Oxidation States". Inorganic Chemistry. 45 (8): 3167–3186. doi:10.1021/ic052110i.
  5. ^ Zr(0) occur in (η6-(1,3,5-tBu)3C6H3)2Zr and [(η5-C5R5Zr(CO)4]−, see Chirik, P. J.; Bradley, C. A. (2007). "4.06 - Complexes of Zirconium and Hafnium in Oxidation States 0 to ii". Comprehensive Organometallic Chemistry III. From Fundamentals to Applications. Vol. 4. Elsevier Ltd. pp. 697–739. doi:10.1016/B0-08-045047-4/00062-5. ISBN 9780080450476.
  6. ^ a b Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 28. doi:10.1016/C2009-0-30414-6. ISBN 978-0-08-037941-8.
  7. ^ Calderazzo, Fausto; Pampaloni, Guido (January 1992). "Organometallics of groups 4 and 5: Oxidation states II and lower". Journal of Organometallic Chemistry. 423 (3): 307–328. doi:10.1016/0022-328X(92)83126-3.
  8. ^ Ma, Wen; Herbert, F. William; Senanayake, Sanjaya D.; Yildiz, Bilge (2015-03-09). "Non-equilibrium oxidation states of zirconium during early stages of metal oxidation". Applied Physics Letters. 106 (10). Bibcode:2015ApPhL.106j1603M. doi:10.1063/1.4914180. hdl:1721.1/104888. ISSN 0003-6951.
  9. ^ 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.
  10. ^ Kondev, F. G.; Wang, M.; Huang, W. J.; Naimi, S.; Audi, G. (2021). "The NUBASE2020 evaluation of nuclear properties" (PDF). Chinese Physics C. 45 (3): 030001. doi:10.1088/1674-1137/abddae.
  11. ^ Harper, Douglas. "zircon". Online Etymology Dictionary.


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