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The mineral pyrite, or iron pyrite, also known as fool's gold, is an iron sulfide with the chemical formula FeS2 (iron(II) disulfide). Pyrite
Pyrite
is considered the most common of the sulfide minerals. Pyrite's metallic luster and pale brass-yellow hue give it a superficial resemblance to gold, hence the well-known nickname of fool's gold. The color has also led to the nicknames brass, brazzle, and Brazil, primarily used to refer to pyrite found in coal.[5][6] The name pyrite is derived from the Greek πυρίτης (pyritēs), "of fire" or "in fire",[7] in turn from πύρ (pyr), "fire".[8] In ancient Roman times, this name was applied to several types of stone that would create sparks when struck against steel; Pliny the Elder described one of them as being brassy, almost certainly a reference to what we now call pyrite.[9] By Georgius Agricola's time, c. 1550, the term had become a generic term for all of the sulfide minerals.[10] Pyrite
Pyrite
is usually found associated with other sulfides or oxides in quartz veins, sedimentary rock, and metamorphic rock, as well as in coal beds and as a replacement mineral in fossils, but has also been identified in the sclerites of scaly-foot gastropods. [11] Despite being nicknamed fool's gold, pyrite is sometimes found in association with small quantities of gold. Gold
Gold
and arsenic occur as a coupled substitution in the pyrite structure. In the Carlin–type gold deposits, arsenian pyrite contains up to 0.37% gold by weight.[12]

Contents

1 Uses 2 Formal oxidation states for pyrite, marcasite, and arsenopyrite 3 Crystallography 4 Crystal habit 5 Varieties 6 Distinguishing similar minerals 7 Hazards

7.1 Acid drainage 7.2 Dust explosions 7.3 Weakened building materials

8 Pyritised fossils 9 Images 10 References 11 Further reading 12 External links

Uses[edit]

An abandoned pyrite mine near Pernek
Pernek
in Slovakia.

Pyrite
Pyrite
enjoyed brief popularity in the 16th and 17th centuries as a source of ignition in early firearms, most notably the wheellock, where the cock held a lump of pyrite against a circular file to strike the sparks needed to fire the gun. Pyrite
Pyrite
has been used since classical times to manufacture copperas, that is, iron(II) sulfate. Iron pyrite was heaped up and allowed to weather (an example of an early form of heap leaching). The acidic runoff from the heap was then boiled with iron to produce iron sulfate. In the 15th century, such leaching began to replace the burning of sulfur as a source of sulfuric acid. By the 19th century, it had become the dominant method.[13] Pyrite
Pyrite
remains in commercial use for the production of sulfur dioxide, for use in such applications as the paper industry, and in the manufacture of sulfuric acid. Thermal decomposition of pyrite into FeS (iron(II) sulfide) and elemental sulfur starts at 540 °C; at around 700 °C pS2 is about 1 atm.[14] A newer commercial use for pyrite is as the cathode material in Energizer
Energizer
brand non-rechargeable lithium batteries.[15] Pyrite
Pyrite
is a semiconductor material with a band gap of 0.95 eV.[16] During the early years of the 20th century, pyrite was used as a mineral detector in radio receivers, and is still used by 'crystal radio' hobbyists. Until the vacuum tube matured, the crystal detector was the most sensitive and dependable detector available – with considerable variation between mineral types and even individual samples within a particular type of mineral. Pyrite
Pyrite
detectors occupied a midway point between galena detectors and the more mechanically complicated perikon mineral pairs. Pyrite
Pyrite
detectors can be as sensitive as a modern 1N34A germanium diode detector.[17][18] Pyrite
Pyrite
has been proposed as an abundant, inexpensive material in low-cost photovoltaic solar panels.[19] Synthetic iron sulfide was used with copper sulfide to create the photovoltaic material.[20] Pyrite
Pyrite
is used to make marcasite jewelry. Marcasite
Marcasite
jewelry, made from small faceted pieces of pyrite, often set in silver, was known since ancient times and was popular in the Victorian era.[21] At the time when the term became common in jewelry making, "marcasite" referred to all iron sulfides including pyrite, and not to the orthorhombic FeS2 mineral marcasite which is lighter in color, brittle and chemically unstable, and thus not suitable for jewelry making. Marcasite
Marcasite
jewelry does not actually contain the mineral marcasite. Formal oxidation states for pyrite, marcasite, and arsenopyrite[edit] From the perspective of classical inorganic chemistry, which assigns formal oxidation states to each atom, pyrite is probably best described as Fe2+S22−. This formalism recognizes that the sulfur atoms in pyrite occur in pairs with clear S–S bonds. These persulfide units can be viewed as derived from hydrogen disulfide, H2S2. Thus pyrite would be more descriptively called iron persulfide, not iron disulfide. In contrast, molybdenite, MoS2, features isolated sulfide (S2−) centers and the oxidation state of molybdenum is Mo4+. The mineral arsenopyrite has the formula FeAsS. Whereas pyrite has S2 subunits, arsenopyrite has [AsS] units, formally derived from deprotonation of H2AsSH. Analysis of classical oxidation states would recommend the description of arsenopyrite as Fe3+[AsS]3−.[22] Crystallography[edit]

Crystal structure of pyrite. In the center of the cell a S22− pair is seen in yellow.

Iron-pyrite FeS2 represents the prototype compound of the crystallographic pyrite structure. The structure is simple cubic and was among the first crystal structures solved by X-ray diffraction.[23] It belongs to the crystallographic space group Pa3 and is denoted by the Strukturbericht notation C2. Under thermodynamic standard conditions the lattice constant

a

displaystyle a

of stoichiometric iron pyrite FeS2 amounts to 541.87 pm.[24] The unit cell is composed of a Fe face-centered cubic sublattice into which the S ions are embedded. The pyrite structure is also used by other compounds MX2 of transition metals M and chalcogens X = O, S, Se and Te. Also certain dipnictides with X standing for P, As and Sb etc. are known to adopt the pyrite structure.[25] In the first bonding sphere, the Fe atoms are surrounded by six S nearest neighbours, in a distorted octahedral arrangement. The material is a diamagnetic semiconductor and the Fe ions should be considered to be in a low spin divalent state (as shown by Mössbauer spectroscopy as well as XPS), rather than a tetravalent state as the stoichiometry would suggest. The positions of X ions in the pyrite structure may be derived from the fluorite structure, starting from a hypothetical Fe2+(S−)2 structure. Whereas F− ions in CaF2 occupy the centre positions of the eight subcubes of the cubic unit cell (​1⁄4 ​1⁄4 ​1⁄4) etc., the S− ions in FeS2 are shifted from these high symmetry positions along <111> axes to reside on (uuu) and symmetry-equivalent positions. Here, the parameter u should be regarded as a free atomic parameter that takes different values in different pyrite-structure compounds (iron pyrite FeS2: u(S) = 0.385 [26]). The shift from fluorite u = 0.25 to pyrite u = 0.385 is rather large and creates a S-S distance that is clearly a binding one. This is not surprising as in contrast to F− an ion S− is not a closed shell species. It is isoelectronic with a chlorine atom, also undergoing pairing to form Cl2 molecules. Both low spin Fe2+ and the disulfide S22− moeties are closed shell entities, explaining the diamagnetic and semiconducting properties. The S atoms have bonds with three Fe and one other S atom. The site symmetry at Fe and S positions is accounted for by point symmetry groups C3i and C3, respectively. The missing center of inversion at S lattice sites has important consequences for the crystallographic and physical properties of iron pyrite. These consequences derive from the crystal electric field active at the sulfur lattice site, which causes a polarisation of S ions in the pyrite lattice.[27] The polarisation can be calculated on the basis of higher-order Madelung constants and has to be included in the calculation of the lattice energy by using a generalised Born–Haber cycle. This reflects the fact that the covalent bond in the sulfur pair is inadequately accounted for by a strictly ionic treatment. Arsenopyrite
Arsenopyrite
has a related structure with heteroatomic As-S pairs rather than homoatomic ones. Marcasite
Marcasite
also possesses homoatomic anion pairs, but the arrangement of the metal and diatomic anions is different from that of pyrite. Despite its name a chalcopyrite does not contain dianion pairs, but single S2− sulfide anions. Crystal habit[edit]

Dodecahedron- shaped crystals from Italy.

Pyrite
Pyrite
usually forms cuboid crystals, sometimes forming in close association to form raspberry-shaped masses called framboids. However, under certain circumstances, it can form anastamozing filaments or T-shaped crystals.[28] Pyrite
Pyrite
can also form almost perfect dodecahedral shapes known as pyritohedra and this suggests an explanation for the artificial geometrical models found in Europe as early as the 5th century BC.[29] Varieties[edit] Cattierite (Co S2) and vaesite (Ni S2) are similar in their structure and belong also to the pyrite group. Bravoite is a nickel-cobalt bearing variety of pyrite, with > 50% substitution of Ni2+ for Fe2+ within pyrite. Bravoite is not a formally recognised mineral, and is named after Peruvian scientist Jose J. Bravo (1874–1928).[30] Distinguishing similar minerals[edit] It is distinguishable from native gold by its hardness, brittleness and crystal form. Natural gold tends to be anhedral (irregularly shaped), whereas pyrite comes as either cubes or multifaceted crystals. Pyrite
Pyrite
can often be distinguished by the striations which, in many cases, can be seen on its surface. Chalcopyrite
Chalcopyrite
is brighter yellow with a greenish hue when wet and is softer (3.5–4 on Mohs' scale).[31] Arsenopyrite
Arsenopyrite
is silver white and does not become more yellow when wet. Hazards[edit]

A pyrite cube (center) has dissolved away from a host rock, leaving behind trace gold.

Iron pyrite is unstable in the natural environment: in nature it is always being created or being destroyed. Iron pyrite exposed to air and water decomposes into iron oxides and sulfate. This process is hastened by the action of Acidithiobacillus bacteria which oxidize the pyrite to produce ferrous iron and sulfate. These reactions occur more rapidly when the pyrite is in fine crystals and dust, which is the form it takes in most mining operations. Acid drainage[edit] Sulfate
Sulfate
released from decomposing pyrite combines with water, producing sulfuric acid, leading to acid rock drainage. An example of acid rock drainage caused by pyrite is the 2015 Gold
Gold
King Mine waste water spill. Dust explosions[edit] Pyrite
Pyrite
oxidation is sufficiently exothermic that underground coal mines in high-sulfur coal seams have occasionally had serious problems with spontaneous combustion in the mined-out areas of the mine. The solution is to hermetically seal the mined-out areas to exclude oxygen.[citation needed] In modern coal mines, limestone dust is sprayed onto the exposed coal surfaces to reduce the hazard of dust explosions. This has the secondary benefit of neutralizing the acid released by pyrite oxidation and therefore slowing the oxidation cycle described above, thus reducing the likelihood of spontaneous combustion. In the long term, however, oxidation continues, and the hydrated sulfates formed may exert crystallization pressure that can expand cracks in the rock and lead eventually to roof fall.[33] Weakened building materials[edit] Building stone containing pyrite tends to stain brown as the pyrite oxidizes. This problem appears to be significantly worse if any marcasite is present.[34] The presence of pyrite in the aggregate used to make concrete can lead to severe deterioration as the pyrite oxidizes.[35] In early 2009, problems [clarification needed] with Chinese drywall
Chinese drywall
imported into the United States
United States
after Hurricane Katrina were attributed to oxidation of pyrite.[36] In the United States, in Canada,[37] and more recently in Ireland,[38][39][40] where it was used as underfloor infill, pyrite contamination has caused major structural damage. Modern tests for aggregate materials[41] certify such materials as free of pyrite. Pyritised fossils[edit]

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Pyrite
Pyrite
and marcasite commonly occur as replacement pseudomorphs after fossils in black shale and other sedimentary rocks formed under reducing environmental conditions.[42] However, pyrite dollars or pyrite suns which have an appearance similar to sand dollars are pseudofossils and lack the pentagonal symmetry of the animal. Images[edit]

As a replacement mineral in an ammonite from France

Pyrite
Pyrite
from Ampliación a Victoria Mine, Navajún, La Rioja, Spain

Pyrite
Pyrite
from the Sweet Home Mine, with golden striated cubes intergrown with minor tetrahedrite, on a bed of transparent quartz needles

Radiating form of pyrite

Paraspirifer
Paraspirifer
bownockeri in pyrite

Pink fluorite perched between pyrite on one side and metallic galena on the other side

References[edit]

^ Hurlbut, Cornelius S.; Klein, Cornelis, 1985, Manual of Mineralogy, 20th ed., John Wiley and Sons, New York, pp 285–286, ISBN 0-471-80580-7 ^ Pyrite
Pyrite
on webmineral. Webmineral.com. Retrieved on 2011-05-25. ^ Pyrite
Pyrite
on. Mindat.org. Retrieved on 2011-05-25. ^ Handbook of Mineralogy. (PDF) . Retrieved on 2011-05-25. ^ Julia A. Jackson, James Mehl and Klaus Neuendorf, Glossary of Geology, American Geological Institute (2005) p. 82. ^ Albert H. Fay, A Glossary of the Mining and Mineral
Mineral
Industry, United States Bureau of Mines (1920) pp. 103–104. ^ πυρίτης, Henry George Liddell, Robert Scott, A Greek-English Lexicon, on Perseus ^ πύρ, Henry George Liddell, Robert Scott, A Greek-English Lexicon, on Perseus ^ James Dwight Dana, Edward Salisbury Dana, Descriptive Mineralogy, 6th Ed., Wiley, New York (1911) p. 86. ^ Herbert Clark Hoover
Herbert Clark Hoover
and Lou Henry Hoover, translators of Georgius Agricola, [De Re Metallica], The Mining Magazine, London (1912; Dover reprint, 1950); see footnote, p. 112. ^ "Armor-Plated Snail Discovered in Deep Sea". news.nationalgeographic.com. Retrieved 2016-08-29.  ^ M. E. Fleet and A. Hamid Mumin, Gold-bearing arsenian pyrite and marcasite and arsenopyrite from Carlin Trend gold deposits and laboratory synthesis, American Mineralogist 82 (1997) pp. 182–193 ^ "Industrial England in the Middle of the Eighteenth Century". Nature. 83 (2113): 264–268. 1910-04-28. Bibcode:1910Natur..83..264.. doi:10.1038/083264a0.  ^ Terkel Rosenqvist (2004). Principles of extractive metallurgy (2nd ed.). Tapir Academic Press. p. 52. ISBN 82-519-1922-3.  ^ Energizer
Energizer
Corporation, Lithium Iron Disulfide ^ K. Ellmer & H. Tributsch (2000-03-11). "Iron Disulfide (Pyrite) as Photovoltaic
Photovoltaic
Material: Problems and Opportunities". Proceedings of the 12th Workshop on Quantum Solar Energy Conversion – (QUANTSOL 2000). Archived from the original on 2010-01-15.  ^ The Principles Underlying Radio
Radio
Communication, Radio
Radio
Pamphlet No. 40, U.S. Army Signal Corps, Dec. 10 (1918) section 179, pp. 302–305. ^ Thomas H. Lee, The Design of Radio
Radio
Frequency Integrated Circuits, 2nd Ed., Cambridge University Press (2004) pp. 4–6. ^ Wadia, Cyrus; Alivisatos, A. Paul; Kammen, Daniel M. (2009). "Materials Availability Expands the Opportunity for Large-Scale Photovoltaics Deployment". Environmental Science & Technology. 43 (6): 2072–7. Bibcode:2009EnST...43.2072W. doi:10.1021/es8019534. PMID 19368216.  ^ Cheaper materials could be key to low-cost solar cells by Robert Sanders, 17 February 2009 ^ Hesse, Rayner W. (2007). Jewelrymaking Through History: An Encyclopedia. Greenwood Publishing Group. p. 15. ISBN 0-313-33507-9.  ^ Vaughan, D. J.; Craig, J. R. " Mineral
Mineral
Chemistry of Metal Sulfides" Cambridge University Press, Cambridge (1978) ISBN 0-521-21489-0 ^ W. L. Bragg (1913). "The structure of some crystals as indicated by their diffraction of X-rays". Proceedings of the Royal Society A. 89 (610): 248–277. Bibcode:1913RSPSA..89..248B. doi:10.1098/rspa.1913.0083. JSTOR 93488.  ^ M. Birkholz; S. Fiechter; A. Hartmann & H. Tributsch (1991). " Sulfur
Sulfur
deficiency in iron pyrite (FeS2−x) and its consequences for band structure models". Phys. Rev. B. 43 (14): 11926–11936. Bibcode:1991PhRvB..4311926B. doi:10.1103/PhysRevB.43.11926.  ^ N. E. Brese & H. G. von Schnering (1994). "Bonding Trends in Pyrites and a Reinvestigation of the Structure of PdAs2, PdSb2, PtSb2 and PtBi2". Z. Anorg. Allg. Chem. 620 (3): 393–404. doi:10.1002/zaac.19946200302.  ^ E. D. Stevens; M. L. de Lucia & P. Coppens (1980). "Experimental observation of the Effect of Crystal Field Splitting on the Electron Density
Density
Distribution of Iron Pyrite". Inorg. Chem. 19 (4): 813–820. doi:10.1021/ic50206a006.  ^ M. Birkholz (1992). "The crystal energy of pyrite". J. Phys.: Condens. Matt. 4 (29): 6227–6240. Bibcode:1992JPCM....4.6227B. doi:10.1088/0953-8984/4/29/007.  ^ Bonev, I. K.; Garcia-Ruiz, J. M.; Atanassova, R.; Otalora, F.; Petrussenko, S. (2005). "Genesis of filamentary pyrite associated with calcite crystals". European Journal of Mineralogy. 17 (6): 905–913. doi:10.1127/0935-1221/2005/0017-0905.  ^ The pyritohedral form is described as a dodecahedron with pyritohedral symmetry; Dana J. et al., (1944), System of mineralogy, New York, p 282 ^ Mindat – bravoite. Mindat.org (2011-05-18). Retrieved on 2011-05-25. ^ Pyrite
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on. Minerals.net (2011-02-23). Retrieved on 2011-05-25. ^ Andrew Roy, Coal
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Mining in Iowa, Coal
Coal
Trade Journal, quoted in History of Lucas County Iowa, State Historical Company, Des Moines (1881) pp. 613–615. ^ Zodrow, E (2005). "Colliery and surface hazards through coal-pyrite oxidation (Pennsylvanian Sydney Coalfield, Nova Scotia, Canada)". International Journal of Coal
Coal
Geology. 64: 145–155. doi:10.1016/j.coal.2005.03.013.  ^ Oliver Bowles, The Structural and Ornamental Stones of Minnesota, Bulletin 663, United States
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Geological Survey, Washington (1918) p. 25. ^ Tagnithamou, A; Sariccoric, M; Rivard, P (2005). "Internal deterioration of concrete by the oxidation of pyrrhotitic aggregates". Cement and Concrete
Concrete
Research. 35: 99–107. doi:10.1016/j.cemconres.2004.06.030.  ^ William Angelo, A Material Odor Mystery Over Foul-Smelling Drywall, from the web site of Engineering News-Record, dated 1/28/2009. ^ "PYRITE and Your House, What Home-Owners Should Know Archived 2012-01-06 at the Wayback Machine." – ISBN 2-922677-01-X - Legal deposit – National Library of Canada, May 2000 ^ Shrimer, F. and Bromley, AV: Pyritic Heave in Ireland; published in Proceedings of the Euroseminar on Building Materials/International Cement Microscopy Association, 2012 (Halle Germany) ^ The Irish Times – Saturday, June 11, 2011 – Homeowners in protest over pyrite damage to houses (Subscription required) ^ Irish Independent — 22 February 2010 (Michael Brennan) Devastating 'pyrite epidemic' hits 20,000 newly built houses ^ I.S. EN 13242:2002 Aggregates for unbound and hydraulically bound materials for use in civil engineering work and road construction ^ Briggs, D. E. G.; Raiswell, R.; Bottrell, S. H.; Hatfield, D.; Bartels, C. (1996-06-01). "Controls on the pyritization of exceptionally preserved fossils; an analysis of the Lower Devonian Hunsrueck Slate of Germany". American Journal of Science. 296 (6): 633–663. doi:10.2475/ajs.296.6.633. ISSN 0002-9599. 

Further reading[edit]

American Geological Institute, 2003, Dictionary of Mining, Mineral, and Related Terms, 2nd ed., Springer, New York, ISBN 978-3-540-01271-9. David Rickard, Pyrite: A Natural History of Fool's Gold, Oxford, New York, 2015, ISBN 978-0-19-020367-2.

External links[edit]

Wikimedia Commons has media related to Pyrite.

Educational article about the famous pyrite crystals from the Navajun Mine How Minerals Form and Change " Pyrite
Pyrite
oxidation under room conditions". Poliakoff, Martyn (2009). "Fool's Gold". The Periodic Table of Videos. University of Nottingham. 

v t e

Sulfur
Sulfur
compounds

Al2S3 As2S2 As2S3 As5S2 As4S4 Au2S3 B2S3 BaS BeS Bi2S3 Br2S Br2S2 CS2 C3S2 CaS CdS CeS SCl2 S2Cl2 CoS Cr2S3 CuS D2S Dy2S3 Er2S3 EuS SF4 SF6 FeS2 GaS H2S HfS2 HgS InS I2S LaS LiS MgS MoS3 NiS SO2 SO3 P4S7 PbS PbS2 PtS ReS2 SrS TlS SV SeS2 S2U WS2 Sb2S3 Sb2S5 Sm2S3 Y2S3 Ag2SO4 SOBr2 CSTe C2H4S C2H6S3 C4H4S CaSO4 C32H66S2 CuFeS2 H2SO4 H2SO3 F2OS NaHS K2SO3 O3S3Sb4 Yb2(SO4)3 AlKO8S2 CHCl3S KSCN CdSO3 PSCl3 SOCl2 Cs2O4S Re2S7 Na2S K2S H2S2O7 H2SO5 NH5S HgSO4 K2SO4 RaSO4 SnSO4 SrSO4 Zr(SO4)2 Ti(SO4)2 Tm2(SO4)3 AlNa(SO4)2 Er2(SO4)3 Eu2(SO4)3 CHNS Co(SCN)2 C2H3SN PSI3 ZrS2 SiS CSSe

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