Zinc#Alloys

File:Zinc-sheet.jpg

Zinc is a bluish-white, lustrous, diamagnetic metal, though most common commercial grades of the metal have a dull finish.{{harvnb|Heiserman|1992|p=123}} It is somewhat less dense than iron and has a hexagonal crystal structure, with a distorted form of hexagonal close packing, in which each atom has six nearest neighbors (at 265.9 pm) in its own plane and six others at a greater distance of 290.6 pm.Wells A.F. (1984) Structural Inorganic Chemistry 5th edition p 1277 Oxford Science Publications {{ISBN|0-19-855370-6}} The metal is hard and brittle at most temperatures but becomes malleable between 100 and 150 °C. Above 210 °C, the metal becomes brittle again and can be pulverized by beating.{{Cite book|url=https://books.google.com/books?id=SSkKAAAAIAAJ|title=The Useful Metals and Their Alloys|first=John|last=Scoffern|author-link=John Scoffern|publisher=Houlston and Wright|date=1861|pages=591–603|access-date=April 6, 2009}} Zinc is a fair conductor of electricity. For a metal, zinc has relatively low melting (419.5 °C) and boiling point (907 °C).{{cite web|url=http://www.galvanizeit.org/design-and-fabrication/design-considerations/zinc-metal-properties |title=Zinc Metal Properties |publisher=American Galvanizers Association |date=2008 |access-date=April 7, 2015 |archive-url=https://web.archive.org/web/20150328205508/http://www.galvanizeit.org/design-and-fabrication/design-considerations/zinc-metal-properties |archive-date=March 28, 2015 |url-status=live }} The melting point is the lowest of all the d-block metals aside from mercury and cadmium; for this reason among others, zinc, cadmium, and mercury are often not considered to be transition metals like the rest of the d-block metals.

Many alloys contain zinc, including brass. Other metals long known to form binary alloys with zinc are aluminium, antimony, bismuth, gold, iron, lead, mercury, silver, tin, magnesium, cobalt, nickel, tellurium, and sodium.{{Cite journal|title=Production and Properties of Zinc: A Treatise on the Occurrence and Distribution of Zinc Ore, the Commercial and Technical Conditions Affecting the Production of the Spelter, Its Chemical and Physical Properties and Uses in the Arts, Together with a Historical and Statistical Review of the Industry|last=Ingalls|first=Walter Renton|journal=The Engineering and Mining Journal|date=1902|pages=142–6|url=https://books.google.com/books?id=RhNDAAAAIAAJ&pg=PA133}} Although neither zinc nor zirconium is ferromagnetic, their alloy, {{chem|ZrZn|2}}, exhibits ferromagnetism below 35 K.

{{See also|:Category:Zinc minerals|l1=Zinc minerals}}

Zinc makes up about 75 ppm (0.0075%) of Earth's crust, making it the 22nd most abundant element.{{Cite book |last=Emsley |first=John |url=https://books.google.com/books?id=2EfYXzwPo3UC&q=24th+most+abundant+element&pg=PA626 |title=Nature's Building Blocks: An A-Z Guide to the Elements |date=2011-08-25 |publisher=OUP Oxford |isbn=978-0-19-960563-7 |language=en}} It also makes up 312 ppm of the Solar System, where it is the 22nd most abundant element.{{Citation |last=Brugger |first=Joël |title=Zinc |date=2018-07-18 |encyclopedia=Encyclopedia of Geochemistry: A Comprehensive Reference Source on the Chemistry of the Earth |series=Encyclopedia of Earth Sciences Series |pages=1521–1524 |url=https://research.monash.edu/en/publications/zinc |access-date=2024-06-21 |publisher=Springer |doi=10.1007/978-3-319-39312-4_212 |isbn=978-3-319-39311-7 |language=English}} Typical background concentrations of zinc do not exceed 1 μg/m³ in the atmosphere; 300 mg/kg in soil; 100 mg/kg in vegetation; 20 μg/L in freshwater and 5 μg/L in seawater.{{Cite book|last=Rieuwerts|first=John|url=https://www.worldcat.org/oclc/886492996|title=The Elements of Environmental Pollution|publisher=Earthscan Routledge|year=2015|isbn=978-0-415-85919-6|location=London and New York|pages=286|oclc=886492996}} The element is normally found in association with other base metals such as copper and lead in ores. Zinc is a chalcophile, meaning the element is more likely to be found in minerals together with sulfur and other heavy chalcogens, rather than with the light chalcogen oxygen or with non-chalcogen electronegative elements such as the halogens. Sulfides formed as the crust solidified under the reducing conditions of the early Earth's atmosphere.{{harvnb|Greenwood|Earnshaw|1997|p=1202}} Sphalerite, which is a form of zinc sulfide, is the most heavily mined zinc-containing ore because its concentrate contains 60–62% zinc.

Other source minerals for zinc include smithsonite (zinc carbonate), hemimorphite (zinc silicate), wurtzite (another zinc sulfide), and sometimes hydrozincite (basic zinc carbonate). With the exception of wurtzite, all these other minerals were formed by weathering of the primordial zinc sulfides.

Identified world zinc resources total about 1.9–2.8 billion tonnes.{{cite web|last=Sai Srujan|first=A.V|date=2021|title=Mineral Commodity Summaries 2021: Zinc|url=https://pubs.usgs.gov/periodicals/mcs2021/mcs2021-zinc.pdf|access-date=June 21, 2021|publisher=United States Geological Survey}}{{cite journal|last1=Erickson|first1=R. L.|title=Crustal Abundance of Elements, and Mineral Reserves and Resources|journal=U.S. Geological Survey Professional Paper |issue=820|date=1973|pages=21–25}} Large deposits are in Australia, Canada and the United States, with the largest reserves in Iran.{{cite web|url=http://www.etdb.org/StrategiesAndResearch/Countries/CSPReports/ReportsLibrary/CPS%20Report%20-%20Islamic%20Republic%20of%20Iran.doc |title=Country Partnership Strategy—Iran: 2011–12 |access-date=June 6, 2011 |publisher=ECO Trade and development bank |url-status=dead |archive-url=https://web.archive.org/web/20111026135641/http://www.etdb.org/StrategiesAndResearch/Countries/CSPReports/ReportsLibrary/CPS%20Report%20-%20Islamic%20Republic%20of%20Iran.doc |archive-date=October 26, 2011 }}{{cite web|url=http://www.iranconmin.de/en/leftnavigation/market|title=IRAN – a growing market with enormous potential|access-date=March 3, 2010|publisher=IMRG|date=July 5, 2010|url-status=live|archive-url=https://web.archive.org/web/20130217181730/http://www.iranconmin.de/en/leftnavigation/market|archive-date=February 17, 2013}} The most recent estimate of reserve base for zinc (meets specified minimum physical criteria related to current mining and production practices) was made in 2009 and calculated to be roughly 480 Mt.{{cite web|last=Tolcin|first=A. C.|date=2009|url=http://minerals.usgs.gov/minerals/pubs/commodity/zinc/mcs-2015-zinc.pdf|publisher=United States Geological Survey|access-date=August 4, 2016|title=Mineral Commodity Summaries 2009: Zinc|url-status=live|archive-url=https://web.archive.org/web/20160702053035/http://minerals.usgs.gov/minerals/pubs/commodity/zinc/mcs-2015-zinc.pdf|archive-date=July 2, 2016}} Zinc reserves, on the other hand, are geologically identified ore bodies whose suitability for recovery is economically based (location, grade, quality, and quantity) at the time of determination. Since exploration and mine development is an ongoing process, the amount of zinc reserves is not a fixed number and sustainability of zinc ore supplies cannot be judged by simply extrapolating the combined mine life of today's zinc mines. This concept is well supported by data from the United States Geological Survey (USGS), which illustrates that although refined zinc production increased 80% between 1990 and 2010, the reserve lifetime for zinc has remained unchanged. About 346 million tonnes have been extracted throughout history to 2002, and scholars have estimated that about 109–305 million tonnes are in use.{{Cite journal|last=Gordon|first=R. B.|author2=Bertram, M. |author3=Graedel, T. E. |title=Metal stocks and sustainability|journal=Proceedings of the National Academy of Sciences|volume=103|date=2006|pmid=16432205|pmc=1360560|doi=10.1073/pnas.0509498103|issue=5|bibcode = 2006PNAS..103.1209G|pages=1209–14 |doi-access=free}}{{cite journal|last1=Gerst|first1=Michael|title=In-Use Stocks of Metals: Status and Implications|journal=Environmental Science and Technology|date=2008|volume=42|issue=19|pages=7038–45|doi=10.1021/es800420p|pmid=18939524|bibcode=2008EnST...42.7038G}}{{cite journal|last1=Meylan|first1=Gregoire|title=The anthropogenic cycle of zinc: Status quo and perspectives|journal=Resources, Conservation and Recycling|volume=123|date=2016|pages=1–10|doi=10.1016/j.resconrec.2016.01.006}}

File:Sphalerite4.jpg (ZnS)|alt=A black shiny lump of solid with uneven surface]]

{{Main|Isotopes of zinc}}

Five stable isotopes of zinc occur in nature, with ⁶⁴Zn being the most abundant isotope (49.17% natural abundance).{{cite web|url=http://www.nndc.bnl.gov/chart/|editor=Alejandro A. Sonzogni (Database Manager)|title=Chart of Nuclides|publisher=National Nuclear Data Center, Brookhaven National Laboratory|access-date=September 13, 2008|date=2008|location=Upton (NY)|url-status=live|archive-url=https://web.archive.org/web/20080522125027/http://www.nndc.bnl.gov/chart|archive-date=May 22, 2008}}{{NUBASE2016|ref}} The other isotopes found in nature are {{chem|66|Zn}} (27.73%), {{chem|67|Zn}} (4.04%), {{chem|68|Zn}} (18.45%), and {{chem|70|Zn}} (0.61%).{{NUBASE2016|name}}

Several dozen radioisotopes have been characterized. {{chem|65|Zn}}, which has a half-life of 243.66 days, is the least active radioisotope, followed by {{chem|72|Zn}} with a half-life of 46.5 hours. Zinc has 10 nuclear isomers, of which ^69mZn has the longest half-life, 13.76 h. The superscript m indicates a metastable isotope. The nucleus of a metastable isotope is in an excited state and will return to the ground state by emitting a photon in the form of a gamma ray. {{chem|61|Zn}} has three excited metastable states and {{chem|73|Zn}} has two.{{NUBASE 2003}} The isotopes {{chem|65|Zn}}, {{chem|71|Zn}}, {{chem|77|Zn}} and {{chem|78|Zn}} each have only one excited metastable state.

The most common decay mode of a radioisotope of zinc with a mass number lower than 66 is electron capture. The decay product resulting from electron capture is an isotope of copper.

:{{nuclide|zinc|n}} + {{SubatomicParticle|link=yes|electron}} → {{nuclide|copper|n}} + {{SubatomicParticle|link=yes|Electron neutrino}}

The most common decay mode of a radioisotope of zinc with mass number higher than 66 is beta decay (β⁻), which produces an isotope of gallium.

:{{nuclide|zinc|n}} → {{nuclide|gallium|n}} + {{SubatomicParticle|electron}} + {{SubatomicParticle|link=yes|Electron antineutrino}}

{{Main|Zinc compounds}}

{{see also|Clemmensen reduction}}

Zinc has an electron configuration of [Ar]4s²3d¹⁰ and is a member of the group 12 of the periodic table. It is a moderately reactive metal and strong reducing agent;{{harvnb|CRC|2006|pp=8–29}} in the reactivity series it is comparable to manganese.{{cite video|first1=John W.|last1=Moore|first2=Lynn R.|last2=Hunsberger|first3=Steven D.|last3=Gammon|first4=Kelly|last4=Houston Jetzer|orig-date=6 Mar 2012|year=2022|title=Reaction of zinc with iodine|url=https://www.chemedx.org/video/reaction-zinc-iodine|type=web video|publisher=American Chemical Society, Division of Chemical Education|via=ChemEdX}} The surface of the pure metal tarnishes quickly, eventually forming a protective passivating layer of the basic zinc carbonate, {{chem|Zn|5|(OH)|6|(CO₃)|2}}, by reaction with atmospheric carbon dioxide.{{Cite book|publisher=CRC Press|date=1994|page=121|isbn=978-0-8247-9213-8|title=Corrosion Resistance of Zinc and Zinc Alloys| first=Frank C.|last=Porter}}

Zinc burns in air with a bright bluish-green flame, giving off fumes of zinc oxide. Zinc reacts readily with acids, alkalis and other non-metals.{{Cite book|last=Hinds|first=John Iredelle Dillard|title=Inorganic Chemistry: With the Elements of Physical and Theoretical Chemistry|publisher=John Wiley & Sons|location=New York|date=1908|edition=2nd|pages=506–508|url=https://books.google.com/books?id=xMUMAAAAYAAJ}} Extremely pure zinc reacts only slowly at room temperature with acids. Strong acids, such as hydrochloric or sulfuric acid, can remove the passivating layer and the subsequent reaction with the acid releases hydrogen gas.

Zinc chemistry resembles that of the late first-row transition metals, nickel and copper, as well as certain main group elements. Almost all zinc compounds have the element in the +2 oxidation state.{{Cite book|last=Brady|first=James E.|author2=Humiston, Gerard E.|author3=Heikkinen, Henry|title=General Chemistry: Principles and Structure|publisher=John Wiley & Sons|date=1983|edition=3rd|page=[https://archive.org/details/generalchemistry1982brad/page/671 671]|isbn=978-0-471-86739-5|url=https://archive.org/details/generalchemistry1982brad/page/671}} When Zn²⁺ compounds form, the outer shell s electrons are lost, yielding a bare zinc ion with the electronic configuration [Ar]3d¹⁰.{{Cite book|last=Ritchie|first=Rob|title=Chemistry|publisher=Letts and Lonsdale|date=2004|edition=2nd|page=71|isbn=978-1-84315-438-9|url=https://books.google.com/books?id=idT9j6406gsC}} The filled interior d shell generally does not participate in bonding, producing diamagnetic and mostly colorless compounds. In aqueous solution an octahedral complex, {{chem|[Zn(H|2|O)₆]|2+}} is the predominant species.{{Cite book|last=Burgess|first=John|title=Metal ions in solution|publisher=Ellis Horwood|location=New York|date=1978|page=147|isbn=978-0-470-26293-1}}

The ionic radii of zinc and magnesium happen to be nearly identical. Consequently some of the equivalent salts have the same crystal structure,{{harvnb|CRC|2006|pp=12–11–12}} and in other circumstances where ionic radius is a determining factor, the chemistry of zinc has much in common with that of magnesium.{{Cite book|publisher=Walter de Gruyter|date=1985|edition=91–100| pages=1034–1041|isbn=978-3-11-007511-3|title=Lehrbuch der Anorganischen Chemie|first1=Arnold F.|last1=Holleman|last2=Wiberg|first2=Egon|last3=Wiberg|first3=Nils|language=de|chapter=Zink}} Compared to the transition metals, zinc tends to form bonds with a greater degree of covalency. Complexes with N- and S- donors are much more stable.{{harvnb|Greenwood|Earnshaw|1997|p=1206}} Complexes of zinc are mostly 4- or 6- coordinate, although 5-coordinate complexes are known.

Other oxidation states require unusual physical conditions, and the only positive oxidation states demonstrated are +1 or +2. The volatilization of zinc in combination with zinc chloride at temperatures above 285 °C indicates the formation of {{chem|Zn|2|Cl|2}}, a zinc compound with a +1 oxidation state. Calculations indicate that a zinc compound with the oxidation state of +4 is unlikely to exist.{{Cite journal|journal=Inorganic Chemistry|date=1994|volume=33|issue=10|pages=2122–2131|title=Oxidation state +IV in group 12 chemistry. Ab initio study of zinc(IV), cadmium(IV), and mercury(IV) fluorides|author=Kaupp M.|author2=Dolg M.|author3=Stoll H.|author4=Von Schnering H. G.|doi=10.1021/ic00088a012|url=https://nbn-resolving.org/urn:nbn:de:bvb:20-opus-60018}} Zn(III) is predicted to exist in the presence of strongly electronegative trianions;{{cite journal |last1=Samanta |first1=Devleena |last2=Jena |first2=Puru |title=Zn in the +III Oxidation State |url=https://pubs.acs.org/doi/abs/10.1021/ja3029119# |journal=Journal of the American Chemical Society |date=2012|volume=134 |issue=20 |pages=8400–8403 |doi=10.1021/ja3029119 |pmid=22559713 |arxiv=1201.1014 |bibcode=2012JAChS.134.8400S }}{{cite journal |last1=Fang |first1=Hong |last2=Banjade |first2=Huta |last3=Deepika |last4=Jena |first4=Puru |title=Realization of the Zn3+ oxidation state |journal=Nanoscale |date=2021|volume=13 |issue=33 |pages=14041–14048 |doi=10.1039/D1NR02816B |pmid=34477685 |s2cid=237400349 |doi-access=free }} however, there exists some doubt around this possibility.{{cite journal |last1=Schlöder |first1=Tobias |display-authors=etal |title=Can Zinc Really Exist in Its Oxidation State +III? |url=https://pubs.acs.org/doi/10.1021/ja3052409# |journal=Journal of the American Chemical Society |date=2012|volume=134 |issue=29 |pages=11977–11979 |doi=10.1021/ja3052409 |pmid=22775535 |bibcode=2012JAChS.13411977S }}

Zinc(I) compounds are very rare. The [Zn₂]²⁺ ion is implicated by the formation of a yellow diamagnetic glass by dissolving metallic zinc in molten ZnCl₂.{{Housecroft3rd|page=739–741, 843}} The [Zn₂]²⁺ core would be analogous to the [Hg₂]²⁺ cation present in mercury(I) compounds. The diamagnetic nature of the ion confirms its dimeric structure. The first zinc(I) compound containing the Zn–Zn bond, (η⁵-C₅Me₅)₂Zn₂ has been reported in 2004.{{cite journal |author1=Resa, I. |author2=Carmona, E. |author3=Gutierrez-Puebla, E. |author4=Monge, A. | title = Decamethyldizincocene, a Stable Compound of Zn(I) with a Zn-Zn Bond | journal = Science | doi = 10.1126/science.1101356 | pmid = 15326350 | year = 2004 | volume = 305 | issue = 5687 | pages = 1136–8|bibcode=2004Sci...305.1136R |s2cid=38990338 }}

File:Zinc acetate.JPG, {{chem|Zn|(|C|H|3|C|O|2|)|2}}|alt=Sheets of zinc acetate formed by slow evaporation]]

File:Zinc chloride.jpg

Binary compounds of zinc are known for most of the metalloids and all the nonmetals except the noble gases. The oxide ZnO is a white powder that is nearly insoluble in neutral aqueous solutions, but is amphoteric, dissolving in both strong basic and acidic solutions. The other chalcogenides (ZnS, ZnSe, and ZnTe) have varied applications in electronics and optics.{{cite web|url=http://www.americanelements.com/znsu.html|title=Zinc Sulfide|publisher=American Elements|access-date=February 3, 2009|url-status=live|archive-url=https://archive.today/20120717190353/http://www.americanelements.com/znsu.html|archive-date=July 17, 2012}} Pnictogenides (Zinc nitride, zinc phosphide, zinc arsenide and zinc antimonide),{{cite book|title=Academic American Encyclopedia|url=https://books.google.com/books?id=YgI4E7w5JI8C|date=1994|publisher=Grolier Inc.| location=Danbury, Connecticut |isbn=978-0-7172-2053-3|page=202}}{{cite web|url=http://www.americanelements.com/znp.html|title=Zinc Phosphide|publisher=American Elements|access-date=February 3, 2009|url-status=live|archive-url=https://archive.today/20120717120313/http://www.americanelements.com/znp.html|archive-date=July 17, 2012}} the peroxide (zinc peroxide), the hydride (zinc hydride), and the carbide ({{chem|ZnC|2}}) are also known.{{Cite journal|journal=Diamond and Related Materials|volume=9|date=2000|title=Peculiarities of interaction in the Zn–C system under high pressures and temperatures |issue=2|vauthors=Shulzhenko AA, Ignatyeva IY, Osipov AS, Smirnova TI |doi=10.1016/S0925-9635(99)00231-9|pages=129–133|bibcode = 2000DRM.....9..129S }} Of the four halides, zinc fluoride has the most ionic character, while the others (zinc chloride, zinc bromide, and zinc iodide) have relatively low melting points and are considered to have more covalent character.{{harvnb|Greenwood|Earnshaw|1997|p=1211}}

In weak basic solutions containing {{chem|Zn|2+}} ions, the hydroxide Zinc hydroxide forms as a white precipitate. In stronger alkaline solutions, this hydroxide is dissolved to form zincates (zincate). The nitrate Zinc nitrate, chlorate Zinc chlorate, sulfate Zinc sulfate, phosphate Zinc phosphate, molybdate Zinc molybdate, cyanide Zinc cyanide, arsenite {{chem|Zn(AsO₂)|2}}, arsenate {{chem|Zn(AsO₄)|2|·8H|2|O}} and the chromate Zinc chromate (one of the few colored zinc compounds) are a few examples of other common inorganic compounds of zinc.{{Cite journal| last=Rasmussen| first=J. K.| author2=Heilmann, S. M.| title=In situ Cyanosilylation of Carbonyl Compounds: O-Trimethylsilyl-4-Methoxymandelonitrile| journal=Organic Syntheses, Collected Volume| volume=7| page=521| date=1990| url=http://www.orgsyn.org/orgsyn/prep.asp?prep=cv7p0521| url-status=live| archive-url=https://web.archive.org/web/20070930230236/http://www.orgsyn.org/orgsyn/prep.asp?prep=cv7p0521| archive-date=September 30, 2007| df=mdy-all}}{{Cite book|title=Handbook of Inorganic Compounds|last=Perry|first=D. L.|pages=448–458|date=1995|isbn=978-0-8493-8671-8|publisher=CRC Press}}

Organozinc compounds are those that contain zinc–carbon covalent bonds. Diethylzinc (Diethylzinc) is a reagent in synthetic chemistry. It was first reported in 1848 from the reaction of zinc and ethyl iodide, and was the first compound known to contain a metal–carbon sigma bond.{{Cite journal|title=On the isolation of the organic radicals|author=Frankland, E.|journal=Quarterly Journal of the Chemical Society|date=1850|volume=2|issue=3|page=263|doi=10.1039/QJ8500200263|url=https://zenodo.org/record/1861200|author-link=Edward Frankland}}

Cobalticyanide paper (Rinnmann's test for Zn) can be used as a chemical indicator for zinc. 4 g of K₃Co(CN)₆ and 1 g of KClO₃ is dissolved on 100 ml of water. Paper is dipped in the solution and dried at 100 °C. One drop of the sample is dropped onto the dry paper and heated. A green disc indicates the presence of zinc.{{Cite book|title=CRC- Handbook of Chemistry and Physics|last=Lide|first=David|publisher=CRC press|year=1998|isbn=978-0-8493-0479-8|pages=Section 8 Page 1}}

{{clear}}

Various isolated examples of the use of impure zinc in ancient times have been discovered. Zinc ores were used to make the zinc–copper alloy brass thousands of years prior to the discovery of zinc as a separate element. Judean brass from the 14th to 10th centuries BC contains 23% zinc.{{harvnb|Greenwood|Earnshaw|1997|p=1201}}

Knowledge of how to produce brass spread to Ancient Greece by the 7th century BC, but few varieties were made.{{cite journal|last=Craddock|first=Paul T.|date=1978|title=The composition of copper alloys used by the Greek, Etruscan and Roman civilizations. The origins and early use of brass|journal=Journal of Archaeological Science|volume=5|issue=1|pages=1–16|doi=10.1016/0305-4403(78)90015-8}} Ornaments made of alloys containing 80–90% zinc, with lead, iron, antimony, and other metals making up the remainder, have been found that are 2,500 years old.{{harvnb|Lehto|1968|p=822}} A possibly prehistoric statuette containing 87.5% zinc was found in a Dacian archaeological site.{{harvnb|Weeks|1933|p=20}}

Strabo writing in the 1st century BC (but quoting a now lost work of the 4th century BC historian Theopompus) mentions "drops of false silver" which when mixed with copper make brass. This may refer to small quantities of zinc that is a by-product of smelting sulfide ores.{{Cite book |author=Craddock, P. T. |chapter=Zinc in classical antiquity |editor=Craddock, P.T. |title=2000 years of zinc and brass |publisher=British Museum |location=London |date=1998 |isbn=978-0-86159-124-4 |pages=3–5 |edition=rev.}} Zinc in such remnants in smelting ovens was usually discarded as it was thought to be worthless.{{harvnb|Weeks|1933|p=21}}

The manufacture of brass was known to the Romans by about 30 BC. They made brass by heating powdered calamine (zinc silicate or carbonate), charcoal and copper together in a crucible.{{harvnb|Emsley|2001|p=501}} The resulting calamine brass was then either cast or hammered into shape for use in weaponry.{{cite web|title=How is zinc made? |work=How Products are Made |date=2002 |publisher=The Gale Group |url=http://www.answers.com/zinc |access-date=February 21, 2009 |url-status=dead |archive-url=https://web.archive.org/web/20060411200556/http://www.answers.com/zinc |archive-date=April 11, 2006 }} Some coins struck by Romans in the Christian era are made of what is probably calamine brass.{{harvnb|Chambers|1901|p=799}}

File:Hemmoorer Eimer.jpger Eimer from Warstade, Germany, second to third century AD|alt=Large black bowl-shaped bucket on a stand. The bucket has incrustation around its top.]]

The oldest known pills were made of the zinc carbonates hydrozincite and smithsonite. The pills were used for sore eyes and were found aboard the Roman ship Relitto del Pozzino, wrecked in 140 BC.{{cite web |url=https://www.newscientist.com/article/dn23049-worlds-oldest-pills-treated-sore-eyes.html |title=World's oldest pills treated sore eyes |work=New Scientist |date=January 7, 2013 |access-date=February 5, 2013 |url-status=live |archive-url=https://web.archive.org/web/20130122102750/http://www.newscientist.com/article/dn23049-worlds-oldest-pills-treated-sore-eyes.html |archive-date=January 22, 2013 }}{{cite journal|doi= 10.1073/pnas.1216776110|pmid=23297212|pmc=3557061|title=Ingredients of a 2,000-y-old medicine revealed by chemical, mineralogical, and botanical investigations|journal=Proceedings of the National Academy of Sciences|volume=110|issue=4|pages=1193–1196|bibcode=2013PNAS..110.1193G|year=2013|last1=Giachi|first1=Gianna|last2=Pallecchi|first2=Pasquino|last3=Romualdi|first3=Antonella|last4=Ribechini|first4=Erika|last5=Lucejko|first5=Jeannette Jacqueline|last6=Colombini|first6=Maria Perla|last7=Mariotti Lippi|first7=Marta|doi-access=free}}

The Berne zinc tablet is a votive plaque dating to Roman Gaul made of an alloy that is mostly zinc.{{Cite book|last=Rehren|first=Th.|date=1996|title=A Roman zinc tablet from Bern, Switzerland: Reconstruction of the Manufacture|publisher=Archaeometry 94. The Proceedings of the 29th International Symposium on Archaeometry|editor=S. Demirci|display-editors=etal|pages=35–45}}

The Charaka Samhita, thought to have been written between 300 and 500 AD,{{cite book|author=Meulenbeld, G. J.|title=A History of Indian Medical Literature|publisher=Forsten|location=Groningen|date=1999|oclc=165833440|volume=IA|pages=130–141}} mentions a metal which, when oxidized, produces pushpanjan, thought to be zinc oxide.{{Cite book |author=Craddock, P. T. |display-authors=etal|chapter=Zinc in India |title=2000 years of zinc and brass |publisher=British Museum |location=London |date=1998 |isbn=978-0-86159-124-4 |page=27 |edition=rev.}} Zinc mines at Zawar, near Udaipur in India, have been active since the Mauryan period ({{circa| 322}} and 187 BCE). The smelting of metallic zinc here, however, appears to have begun around the 12th century AD.p. 46, Ancient mining and metallurgy in Rajasthan, S. M. Gandhi, chapter 2 in Crustal Evolution and Metallogeny in the Northwestern Indian Shield: A Festschrift for Asoke Mookherjee, M. Deb, ed., Alpha Science Int'l Ltd., 2000, {{ISBN|1-84265-001-7}}.{{Cite journal|last=Craddock|first=P. T.|author2=Gurjar L. K. |author3=Hegde K. T. M. |title=Zinc production in medieval India|journal=World Archaeology|volume=15|issue=2|date=1983|jstor=124653

|pages=211–217|doi=10.1080/00438243.1983.9979899}} One estimate is that this location produced an estimated million tonnes of metallic zinc and zinc oxide from the 12th to 16th centuries.{{harvnb|Emsley|2001|p=502}} Another estimate gives a total production of 60,000 tonnes of metallic zinc over this period. The Rasaratna Samuccaya, written in approximately the 13th century AD, mentions two types of zinc-containing ores: one used for metal extraction and another used for medicinal purposes.

Zinc was distinctly recognized as a metal under the designation of Yasada or Jasada in the medical Lexicon ascribed to the Hindu king Madanapala (of Taka dynasty) and written about the year 1374.{{cite book|last=Ray|first=Prafulla Chandra|title=A History of Hindu Chemistry from the Earliest Times to the Middle of the Sixteenth Century, A.D.: With Sanskrit Texts, Variants, Translation and Illustrations|publisher=The Bengal Chemical & Pharmaceutical Works, Ltd|date=1903|edition=2nd|volume=1|pages=157–158|url=https://books.google.com/books?id=DL1HAAAAIAAJ}} (public domain text) Smelting and extraction of impure zinc by reducing calamine with wool and other organic substances was accomplished in the 13th century in India.{{harvnb|CRC|2006|p=4–41}}{{cite web|last=Habashi|first=Fathi|title=Discovering the 8th Metal|publisher=International Zinc Association (IZA)|url=http://www.iza.com/Documents/Communications/Publications/History.pdf|archive-url=https://web.archive.org/web/20090304154217/http://www.iza.com/Documents/Communications/Publications/History.pdf|archive-date=March 4, 2009|access-date=December 13, 2008}} The Chinese did not learn of the technique until the 17th century.

File:Zinc symbol (fixed width).svg for the element zinc]]

Alchemists burned zinc metal in air and collected the resulting zinc oxide on a condenser. Some alchemists called this zinc oxide lana philosophica, Latin for "philosopher's wool", because it collected in wooly tufts, whereas others thought it looked like white snow and named it nix album.{{Cite book|last=Arny|first=Henry Vinecome|url=https://books.google.com/books?id=gRNKAAAAMAAJ|title=Principles of Pharmacy|publisher=W. B. Saunders company|date=1917|edition=2nd|page=483}}

The name of the metal was probably first documented by Paracelsus, a Swiss-born German alchemist, who referred to the metal as "zincum" or "zinken" in his book Liber Mineralium II, in the 16th century.{{Cite book|title=Georgius Agricola de Re Metallica|first=Herbert Clark|last=Hoover|publisher=Kessinger Publishing|date=2003|page=409|isbn=978-0-7661-3197-2}} The word is probably derived from the German {{lang|de|zinke}}, and supposedly meant "tooth-like, pointed or jagged" (metallic zinc crystals have a needle-like appearance).{{Cite book|title=Ullmann's Encyclopedia of Industrial Chemistry|last=Gerhartz|display-authors=etal |edition=5th|date=1996|isbn=978-3-527-20100-6|publisher=VHC|page=509|first=Wolfgang}} Zink could also imply "tin-like" because of its relation to German zinn meaning tin.{{Cite book|author=Skeat, W. W|title=Concise Etymological Dictionary of the English Language|url=https://books.google.com/books?id=ls_XijT33IUC&pg=PA622|page=622|publisher=Cosimo, Inc.|date=2005|isbn=978-1-59605-092-1}} Yet another possibility is that the word is derived from the Persian word {{lang|fa|سنگ}} seng meaning stone.{{Cite book|title=Handbook of Extractive Metallurgy|author=Fathi Habashi|date=1997|isbn=978-3-527-28792-5|publisher=Wiley-VHC|page=642}} The metal was also called Indian tin, tutanego, calamine, and spinter.

German metallurgist Andreas Libavius received a quantity of what he called "calay" (from the Malay or Hindi word for tin) originating from Malabar off a cargo ship captured from the Portuguese in the year 1596.{{Cite book|last=Lach|first=Donald F.|title=Asia in the Making of Europe|chapter=Technology and the Natural Sciences|page=426|chapter-url=https://books.google.com/books?id=N0xD7BYXv_YC&pg=PA426|date=1994|isbn=978-0-226-46734-4|publisher=University of Chicago Press}} Libavius described the properties of the sample, which may have been zinc. Zinc was regularly imported to Europe from the Orient in the 17th and early 18th centuries, but was at times very expensive.{{efn|An East India Company ship carrying a cargo of nearly pure zinc metal from the Orient sank off the coast Sweden in 1745.{{harv|Emsley|2001|p=502}}}}

File:Andreas Sigismund Marggraf-flip.jpg is given credit for first isolating pure zinc|alt=Picture of an old man head (profile). The man has a long face, short hair and tall forehead.]]

Metallic zinc was isolated in India by 1300 AD.{{cite book|last=Vaughan|first=L Brent |date=1897 |title=The Junior Encyclopedia Britannica A Reference Library of General Knowledge Volume III P-Z|location=Chicago |publisher=E. G. Melven & Company|article=Zincography}}{{cite web|url=http://science.marshall.edu/castella/chm448/elements3.pdf|title=Transition Metal Elements|author=Castellani, Michael|access-date=October 14, 2014|url-status=live|archive-url=https://web.archive.org/web/20141010201408/http://science.marshall.edu/castella/chm448/elements3.pdf|archive-date=October 10, 2014}}{{cite book |last1=Habib |first1=Irfan |editor-last=Chatopadhyaya |editor-first=D. P. |date=2011 |title=Economic History of Medieval India, 1200–1500 |url=https://books.google.com/books?id=K8kO4J3mXUAC&pg=PA86 |location=New Delhi |publisher=Pearson Longman |page=86 |isbn=978-81-317-2791-1 |url-status=live |archive-url=https://web.archive.org/web/20160414222551/https://books.google.com/books?id=K8kO4J3mXUAC&pg=PA86 |archive-date=April 14, 2016 }} Before it was isolated in Europe, it was imported from India in about 1600 CE. Postlewayt's Universal Dictionary, a contemporary source giving technological information in Europe, did not mention zinc before 1751 but the element was studied before then.{{Cite journal|title=Ancient Lead and Zinc Mining in Rajasthan, India|author1=Willies, Lynn|author2=Craddock, P. T.|author3=Gurjar, L. J.|author4=Hegde, K. T. M. |volume=16|issue=2, Mines and Quarries|date=1984|journal=World Archaeology|jstor=124574|pages=222–233|doi=10.1080/00438243.1984.9979929}}

Flemish metallurgist and alchemist P. M. de Respour reported that he had extracted metallic zinc from zinc oxide in 1668. By the start of the 18th century, Étienne François Geoffroy described how zinc oxide condenses as yellow crystals on bars of iron placed above zinc ore that is being smelted. In Britain, John Lane is said to have carried out experiments to smelt zinc, probably at Landore, prior to his bankruptcy in 1726.{{Cite journal|last=Roberts|first=R. O.|date=1951|title=Dr John Lane and the foundation of the non-ferrous metal industry in the Swansea valley|journal=Gower|publisher=Gower Society|issue=4|page=19}}

In 1738 in Great Britain, William Champion patented a process to extract zinc from calamine in a vertical retort-style smelter.{{Cite book|last=Comyns|first=Alan E.|title=Encyclopedic Dictionary of Named Processes in Chemical Technology|edition=3rd|publisher=CRC Press|isbn=978-0-8493-9163-7|date=2007|page=71|url=https://books.google.com/books?id=Jlq-ckWvQSQC}} His technique resembled that used at Zawar zinc mines in Rajasthan, but no evidence suggests he visited the Orient.{{Cite journal|first=Rhys|last=Jenkins|title=The Zinc Industry in England: the early years up to 1850|journal=Transactions of the Newcomen Society|volume=25|date=1945|pages=41–52|doi=10.1179/tns.1945.006}} Champion's process was used through 1851.

German chemist Andreas Marggraf normally gets credit for isolating pure metallic zinc in the West, even though Swedish chemist Anton von Swab had distilled zinc from calamine four years previously. In his 1746 experiment, Marggraf heated a mixture of calamine and charcoal in a closed vessel without copper to obtain a metal.{{cite journal |last1=Marggraf |title=Experiences sur la maniere de tirer le Zinc de sa veritable miniere, c'est à dire, de la pierre calaminaire |journal=Histoire de l'Académie Royale des Sciences et Belles-Lettres de Berlin |date=1746 |volume=2 |pages=49–57 |url=https://babel.hathitrust.org/cgi/pt?id=mdp.39015026296437&view=1up&seq=93 |trans-title=Experiments on a way of extracting zinc from its true mineral; i.e., the stone calamine |language=fr}} This procedure became commercially practical by 1752.{{harvnb|Heiserman|1992|p=122}}

File:Luigi Galvani, oil-painting.jpg was named after Luigi Galvani.|alt=Painting of a middle-aged man sitting by the table, wearing a wig, black jacket, white shirt and white scarf.]]

William Champion's brother, John, patented a process in 1758 for calcining zinc sulfide into an oxide usable in the retort process. Prior to this, only calamine could be used to produce zinc. In 1798, Johann Christian Ruberg improved on the smelting process by building the first horizontal retort smelter.{{Cite book|last=Gray|title=Zinc|date=2005|isbn=978-0-7614-1922-8|publisher=Marshall Cavendish|page=[https://archive.org/details/zinc0000gray/page/8 8]|first=Leon|url=https://archive.org/details/zinc0000gray/page/8}} Jean-Jacques Daniel Dony built a different kind of horizontal zinc smelter in Belgium that processed even more zinc.

Italian doctor Luigi Galvani discovered in 1780 that connecting the spinal cord of a freshly dissected frog to an iron rail attached by a brass hook caused the frog's leg to twitch.{{Cite book|title=Excel Preliminary Physics|last=Warren|first=Neville G.|publisher=Pascal Press|date=2000|page=47|isbn=978-1-74020-085-1|url=https://books.google.com/books?id=eL9Xn6nQ6XQC}} He incorrectly thought he had discovered an ability of nerves and muscles to create electricity and called the effect "animal electricity".{{Cite book|title=The New International Encyclopaedia|chapter=Galvanic Cell|page=80|date=1903|publisher=Dodd, Mead and Company|chapter-url=https://books.google.com/books?id=gV1MAAAAMAAJ&pg=PA80}} The galvanic cell and the process of galvanization were both named for Luigi Galvani, and his discoveries paved the way for electrical batteries, galvanization, and cathodic protection.

Galvani's friend, Alessandro Volta, continued researching the effect and invented the Voltaic pile in 1800. Volta's pile consisted of a stack of simplified galvanic cells, each being one plate of copper and one of zinc connected by an electrolyte. By stacking these units in series, the Voltaic pile (or "battery") as a whole had a higher voltage, which could be used more easily than single cells. Electricity is produced because the Volta potential between the two metal plates makes electrons flow from the zinc to the copper and corrode the zinc.

The non-magnetic character of zinc and its lack of color in solution delayed discovery of its importance to biochemistry and nutrition. This changed in 1940 when carbonic anhydrase, an enzyme that scrubs carbon dioxide from blood, was shown to have zinc in its active site. The digestive enzyme carboxypeptidase became the second known zinc-containing enzyme in 1955.{{harvnb|Cotton et al.|1999|p=626}}

{{clear}}

{{Main|Zinc mining|Zinc smelting}}

{{See also|List of countries by zinc production}}

File:Price of Zinc.webp

File:World Zinc Production 2006.svg

File:Zinc world production.svg

File:Zink Mine Rosh Pinah.jpg
{{coord|27|57|17|S|016|46|00|E|region:NA_type:landmark|name=Rosh Pinah}}]]

File:Skorpion Zink Mine.jpg
{{coord|27|49|09|S|016|36|28|E|region:NA_type:landmark|name=Skorpion}}]]

Zinc is the fourth most common metal in use, trailing only iron, aluminium, and copper with an annual production of about 13 million tonnes. The world's largest zinc producer is Nyrstar, a merger of the Australian OZ Minerals and the Belgian Umicore.{{cite web|url=https://www.wsj.com/articles/SB116590371844647445|title=Zinifex, Umicore Combine to Form Top Zinc Maker|last=Attwood|first=James|work=The Wall Street Journal|date=February 13, 2006|url-status=live|archive-url=https://web.archive.org/web/20170126122526/http://www.wsj.com/articles/SB116590371844647445|archive-date=January 26, 2017}} About 70% of the world's zinc originates from mining, while the remaining 30% comes from recycling secondary zinc.{{cite web|url=http://www.zincworld.org/recycling.html |title=Zinc Recycling |publisher=International Zinc Association |access-date=November 28, 2008 |url-status=dead |archive-url=https://web.archive.org/web/20111021135539/http://www.zincworld.org/recycling.html |archive-date=October 21, 2011 }}

{{anchor|Commercially pure zinc}}

Commercially pure zinc is known as Special High Grade, often abbreviated SHG, and is 99.995% pure.{{cite web|title=Special High Grade Zinc (SHG) 99.995%|url=http://nyrstar.com/nyrstar/en/products/zinccongalvanising/techdownloads/shg_budel.pdf|archive-url=https://web.archive.org/web/20090304154218/http://nyrstar.com/nyrstar/en/products/zinccongalvanising/techdownloads/shg_budel.pdf|archive-date=March 4, 2009| access-date=December 1, 2008|date=2008|publisher=Nyrstar}}

Worldwide, 95% of new zinc is mined from sulfidic ore deposits, in which sphalerite (ZnS) is nearly always mixed with the sulfides of copper, lead and iron.{{Rp|page=6}} Zinc mines are scattered throughout the world, with the main areas being China, Australia, and Peru. China produced 38% of the global zinc output in 2014.

Zinc metal is produced using extractive metallurgy.{{Cite book|title=Principles of Extractive Metallurgy|last=Rosenqvist|first=Terkel|pages=7, 16, 186|edition=2nd|date=1922|isbn=978-82-519-1922-7|publisher=Tapir Academic Press}}{{Rp|page=7}} The ore is finely ground, then put through froth flotation to separate minerals from gangue (on the property of hydrophobicity), to get a zinc sulfide ore concentrate{{Rp|page=16}} consisting of about 50% zinc, 32% sulfur, 13% iron, and 5% {{chem|SiO|2}}.{{Rp|page=16}}

Roasting converts the zinc sulfide concentrate to zinc oxide:{{Cite book|url=https://books.google.com/books?id=laACw9i0D_wC|title=Zinc Handbook|first=Frank C.|last=Porter|publisher=CRC Press|date=1991|isbn=978-0-8247-8340-2}}

:2ZnS + 3O2 ->[t^o] 2ZnO + 2SO2

The sulfur dioxide is used for the production of sulfuric acid, which is necessary for the leaching process. If deposits of zinc carbonate, zinc silicate, or zinc-spinel (like the Skorpion Deposit in Namibia) are used for zinc production, the roasting can be omitted.{{Cite journal|journal=Economic Geology|date=2003|volume=98|issue=4|pages=749–771|doi=10.2113/98.4.749|title=Geology of the Skorpion Supergene Zinc Deposit, Southern Namibia|first=Gregor|last=Borg|author2=Kärner, Katrin |author3=Buxton, Mike |author4=Armstrong, Richard |author5= van der Merwe, Schalk W. }}

For further processing two basic methods are used: pyrometallurgy or electrowinning. Pyrometallurgy reduces zinc oxide with carbon or carbon monoxide at {{convert|950|C|F|abbr=on}} into the metal, which is distilled as zinc vapor to separate it from other metals, which are not volatile at those temperatures.{{Cite book|last=Bodsworth|first=Colin|title=The Extraction and Refining of Metals|page=148|date=1994|isbn=978-0-8493-4433-6|publisher=CRC Press}} The zinc vapor is collected in a condenser. The equations below describe this process:

: ZnO + C ->[950^oC] Zn + CO

: ZnO + CO ->[950^oC] Zn + CO2

In electrowinning, zinc is leached from the ore concentrate by sulfuric acid and impurities are precipitated:{{Cite book|title=Hydrometallurgy in Extraction Processes|last=Gupta|first=C. K.|author2=Mukherjee, T. K. |page=62|publisher=CRC Press|isbn=978-0-8493-6804-2|date=1990}}

:ZnO + H2SO4 -> ZnSO4 + H2O

Finally, the zinc is reduced by electrolysis.

:2ZnSO4 + 2H2O -> 2Zn + O2 + 2H2SO4

The sulfuric acid is regenerated and recycled to the leaching step.

When galvanised feedstock is fed to an electric arc furnace, the zinc is recovered from the dust by a number of processes, predominantly the Waelz process (90% as of 2014).{{citation| title = Handbook of Recycling: State-of-the-art for Practitioners, Analysts, and Scientists| editor-first = Ernst| editor-last = Worrell| editor-first2= Markus|editor-last2= Reuter| date = 2014| chapter =9. Zinc and Residue Recycling| first1 = Jürgen| last1 = Antrekowitsch| first2= Stefan| last2= Steinlechner| first3 = Alois| last3= Unger| first4 = Gernot| last4 = Rösler| first5 = Christoph| last5 = Pichler| first6 = Rene| last6 = Rumpold}}

Refinement of sulfidic zinc ores produces large volumes of sulfur dioxide and cadmium vapor. Smelter slag and other residues contain significant quantities of metals. About 1.1 million tonnes of metallic zinc and 130 thousand tonnes of lead were mined and smelted in the Belgian towns of La Calamine and Plombières between 1806 and 1882.{{Cite journal|journal=Environmental Geology|date=1996|volume=27|first=H.|last=Kucha|issue=1|author2=Martens, A.|author3=Ottenburgs, R.|author4=De Vos, W.|author5=Viaene, W.|title=Primary minerals of Zn-Pb mining and metallurgical dumps and their environmental behavior at Plombières, Belgium|doi=10.1007/BF00770598|pages=1–15|bibcode=1996EnGeo..27....1K|s2cid=129717791}} The dumps of the past mining operations leach zinc and cadmium, and the sediments of the Geul River contain non-trivial amounts of metals. About two thousand years ago, emissions of zinc from mining and smelting totaled 10 thousand tonnes a year. After increasing 10-fold from 1850, zinc emissions peaked at 3.4 million tonnes per year in the 1980s and declined to 2.7 million tonnes in the 1990s, although a 2005 study of the Arctic troposphere found that the concentrations there did not reflect the decline. Man-made and natural emissions occur at a ratio of 20 to 1.

Zinc in rivers flowing through industrial and mining areas can be as high as 20 ppm.{{harvnb|Emsley|2001|p=504}} Effective sewage treatment greatly reduces this; treatment along the Rhine, for example, has decreased zinc levels to 50 ppb. Concentrations of zinc as low as 2 ppm adversely affects the amount of oxygen that fish can carry in their blood.{{Cite book|last=Heath|first=Alan G.|title=Water pollution and fish physiology|publisher=CRC Press|location=Boca Raton, Florida|date=1995|page=57|isbn=978-0-87371-632-1|url=https://books.google.com/books?id=5NPVTuBtGF4C}}

{{wide image|The Zinc Works and Incat.jpg|1150px|Historically responsible for high metal levels in the Derwent River,{{cite web|url=http://www.derwentestuary.org.au/file.php?id=193 |title=Derwent Estuary – Water Quality Improvement Plan for Heavy Metals |date=June 2007 |publisher=Derwent Estuary Program |access-date=July 11, 2009 |url-status=dead |archive-url=https://web.archive.org/web/20120321090648/http://www.derwentestuary.org.au/file.php?id=193 |archive-date=March 21, 2012 }} the zinc works at Lutana is the largest exporter in Tasmania, generating 2.5% of the state's GDP, and producing more than 250,000 tonnes of zinc per year.{{cite web|title=The Zinc Works|url=http://www.tchange.com.au/resources/zinifex_smelter.html|publisher=TChange|access-date=July 11, 2009|url-status=live|archive-url=https://web.archive.org/web/20090427031313/http://www.tchange.com.au/resources/zinifex_smelter.html|archive-date=April 27, 2009}}|alt=A panorama featuring a large industrial plant on a sea side, in front of mountains.}}

Soils contaminated with zinc from mining, refining, or fertilizing with zinc-bearing sludge can contain several grams of zinc per kilogram of dry soil. Levels of zinc in excess of 500 ppm in soil interfere with the ability of plants to absorb other essential metals, such as iron and manganese. Zinc levels of 2000 ppm to 180,000 ppm (18%) have been recorded in some soil samples.

Major applications of zinc include, with percentages given for the US

1. Galvanizing (55%)
2. Brass and bronze (16%)
3. Other alloys (21%)
4. Miscellaneous (8%)

File:Feuerverzinkte Oberfläche.jpg crystalline surface|alt=Merged elongated crystals of various shades of gray.]]

File:Zinkanode neu.jpg]]

Zinc is most commonly used as an anti-corrosion agent,{{harvnb|Greenwood|Earnshaw|1997|p=1203}} and galvanization (coating of iron or steel) is the most familiar form. In 2009 in the United States, 55% or 893,000 tons of the zinc metal was used for galvanization.{{cite web |date=February 2010 |url=http://minerals.usgs.gov/minerals/pubs/commodity/zinc/myb1-2009-zinc.pdf|access-date=June 6, 2001 |title=Zinc: World Mine Production (zinc content of concentrate) by Country |work=2009 Minerals Yearbook: Zinc |publisher=United States Geological Survey |location=Washington, D.C. |url-status=live|archive-url=https://web.archive.org/web/20110608154555/http://minerals.usgs.gov/minerals/pubs/commodity/zinc/myb1-2009-zinc.pdf|archive-date=June 8, 2011}}

Zinc is more reactive than iron or steel and thus will attract almost all local oxidation until it completely corrodes away.{{harvnb|Stwertka|1998|p=99}} A protective surface layer of oxide and carbonate ({{chem|Zn|5|(OH)|6|(CO|3|)|2|)}} forms as the zinc corrodes.{{harvnb|Lehto|1968|p=829}} This protection lasts even after the zinc layer is scratched but degrades through time as the zinc corrodes away. The zinc is applied electrochemically or as molten zinc by hot-dip galvanizing or spraying. Galvanization is used on chain-link fencing, guard rails, suspension bridges, lightposts, metal roofs, heat exchangers, and car bodies.{{harvnb|Emsley|2001|p=503}}

The relative reactivity of zinc and its ability to attract oxidation to itself makes it an efficient sacrificial anode in cathodic protection (CP). For example, cathodic protection of a buried pipeline can be achieved by connecting anodes made from zinc to the pipe. Zinc acts as the anode (negative terminus) by slowly corroding away as it passes electric current to the steel pipeline.{{efn|Electric current will naturally flow between zinc and steel but in some circumstances inert anodes are used with an external DC source.}} Zinc is also used to cathodically protect metals that are exposed to sea water.{{Cite journal|title=A comparative study of the electrochemical behaviour of Algerian zinc and a zinc from a commercial sacrificial anode|last=Bounoughaz|first=M.|author2=Salhi, E.|author3=Benzine, K.|author4=Ghali E.|author5=Dalard F.|journal=Journal of Materials Science|volume =38|issue=6|pages=1139–1145|doi=10.1023/A:1022824813564|date=2003|bibcode = 2003JMatS..38.1139B |s2cid=135744939}} A zinc disc attached to a ship's iron rudder will slowly corrode while the rudder stays intact. Similarly, a zinc plug attached to a propeller or the metal protective guard for the keel of the ship provides temporary protection.

With a standard electrode potential (SEP) of −0.76 volts, zinc is used as an anode material for batteries. (More reactive lithium (SEP −3.04 V) is used for anodes in lithium batteries ). Powdered zinc is used in this way in alkaline batteries and the case (which also serves as the anode) of zinc–carbon batteries is formed from sheet zinc.{{Cite book|first=Jürgen O.|last=Besenhard|title=Handbook of Battery Materials|publisher=Wiley-VCH|isbn=978-3-527-29469-5|date=1999|bibcode=1999hbm..book.....B}}{{Cite journal|doi=10.1016/0378-7753(95)02242-2|date=1995|title=Recycling zinc batteries: an economical challenge in consumer waste management|first=J.-P.|last=Wiaux|author2=Waefler, J. -P. |journal=Journal of Power Sources|volume=57|issue=1–2|pages=61–65|bibcode = 1995JPS....57...61W }} Zinc is used as the anode or fuel of the zinc–air battery/fuel cell.{{Cite book|chapter=A design guide for rechargeable zinc–air battery technology|last=Culter|first=T.|doi=10.1109/SOUTHC.1996.535134|title=Southcon/96. Conference Record|isbn=978-0-7803-3268-3|date=1996|page=616|s2cid=106826667}}{{cite web|url=http://www.electric-fuel.com/evtech/papers/paper11-1-98.pdf |title=Zinc Air Battery-Battery Hybrid for Powering Electric Scooters and Electric Buses |first=Jonathan |last=Whartman |author2=Brown, Ian |publisher=The 15th International Electric Vehicle Symposium |access-date=October 8, 2008 |url-status=dead |archive-url=https://web.archive.org/web/20060312003601/http://www.electric-fuel.com/evtech/papers/paper11-1-98.pdf |archive-date=March 12, 2006 }}{{cite journal|title=A refuelable zinc/air battery for fleet electric vehicle propulsion|journal=NASA Sti/Recon Technical Report N|volume=96|pages=11394|last=Cooper|first=J. F.|author2=Fleming, D.|author3=Hargrove, D.|author4=Koopman, R.|author5=Peterman, K|publisher=Society of Automotive Engineers future transportation technology conference and exposition|osti = 82465|bibcode=1995STIN...9611394C|year=1995}} The zinc-cerium redox flow battery also relies on a zinc-based negative half-cell.{{cite journal|last1=Xie|first1=Z.|last2=Liu|first2=Q.|last3=Chang|first3=Z.|last4=Zhang|first4=X.|title=The developments and challenges of cerium half-cell in zinc–cerium redox flow battery for energy storage|journal=Electrochimica Acta|date=2013|volume=90|pages=695–704|doi=10.1016/j.electacta.2012.12.066}}

A widely used zinc alloy is brass, in which copper is alloyed with anywhere from 3% to 45% zinc, depending upon the type of brass. Brass is generally more ductile and stronger than copper, and has superior corrosion resistance. These properties make it useful in communication equipment, hardware, musical instruments, and water valves.

File:Microstructure of rolled and annealed brass; magnification 400X.jpg

Other widely used zinc alloys include nickel silver, typewriter metal, soft and aluminium solder, and commercial bronze. Zinc is also used in contemporary pipe organs as a substitute for the traditional lead/tin alloy in pipes.{{Cite book|first=Douglas Earl|last=Bush|author2=Kassel, Richard |title=The Organ: An Encyclopedia|isbn=978-0-415-94174-7|url=https://books.google.com/books?id=cgDJaeFFUPoC|publisher=Routledge|date=2006|page=679}} Alloys of 85–88% zinc, 4–10% copper, and 2–8% aluminium find limited use in certain types of machine bearings. Zinc has been the primary metal in American one cent coins (pennies) since 1982.{{cite web|url=http://www.usmint.gov/about_the_mint/?action=coin_specifications|publisher=United States Mint|access-date=October 8, 2008|title=Coin Specifications|url-status=live|archive-url=https://web.archive.org/web/20150218061037/http://www.usmint.gov/about_the_mint/?action=coin_specifications|archive-date=February 18, 2015}} The zinc core is coated with a thin layer of copper to give the appearance of a copper coin. In 1994, {{convert|33200|t|ST}} of zinc were used to produce 13.6 billion pennies in the United States.{{cite web|url=http://minerals.usgs.gov/minerals/pubs/commodity/zinc/720494.pdf|publisher=United States Geological Survey|title=Mineral Yearbook 1994: Zinc|first=Stephen M.|last=Jasinski|access-date=November 13, 2008|url-status=live|archive-url=https://web.archive.org/web/20081029065604/http://minerals.usgs.gov/minerals/pubs/commodity/zinc/720494.pdf|archive-date=October 29, 2008}}

Alloys of zinc with small amounts of copper, aluminium, and magnesium are useful in die casting as well as spin casting, especially in the automotive, electrical, and hardware industries. These alloys are marketed under the name Zamak.{{cite web|url=http://www.eazall.com/diecastalloys.aspx|title=Diecasting Alloys|publisher=Eastern Alloys|access-date=January 19, 2009|location=Maybrook, NY|url-status=live|archive-url=https://web.archive.org/web/20081225003739/http://www.eazall.com/diecastalloys.aspx|archive-date=December 25, 2008}} An example of this is zinc aluminium. The low melting point together with the low viscosity of the alloy makes possible the production of small and intricate shapes. The low working temperature leads to rapid cooling of the cast products and fast production for assembly.{{Cite journal|first=D.|last=Apelian|author2=Paliwal, M. |author3=Herrschaft, D. C. |title=Casting with Zinc Alloys|journal=Journal of Metals|volume=33|issue=11|date=1981|pages =12–19|doi=10.1007/bf03339527|bibcode = 1981JOM....33k..12A }} Another alloy, marketed under the brand name Prestal, contains 78% zinc and 22% aluminium, and is reported to be nearly as strong as steel but as malleable as plastic.{{Cite book|url=https://books.google.com/books?id=s0i32LSfrJ4C&pg=PA157|page=157|title=Materials for automobile bodies|author=Davies, Geoff|publisher=Butterworth-Heinemann|date=2003|isbn=978-0-7506-5692-4}} This superplasticity of the alloy allows it to be molded using die casts made of ceramics and cement.

Similar alloys with the addition of a small amount of lead can be cold-rolled into sheets. An alloy of 96% zinc and 4% aluminium is used to make stamping dies for low production run applications for which ferrous metal dies would be too expensive.{{Cite book|last=Samans|first=Carl Hubert|title=Engineering Metals and Their Alloys|publisher=Macmillan Co.|date=1949}} For building facades, roofing, and other applications for sheet metal formed by deep drawing, roll forming, or bending, zinc alloys with titanium and copper are used.{{Cite book|chapter-url=https://books.google.com/books?id=C-pAiedmqp8C|title=Corrosion Resistance of Zinc and Zinc Alloys|first=Frank|last=Porter|publisher =CRC Press|date=1994|isbn=978-0-8247-9213-8|chapter=Wrought Zinc|pages=6–7}} Unalloyed zinc is too brittle for these manufacturing processes.

As a dense, inexpensive, easily worked material, zinc is used as a lead replacement. In the wake of lead concerns, zinc appears in weights for various applications ranging from fishing{{cite book|author=McClane, Albert Jules|author2=Gardner, Keith|name-list-style=amp|title=The Complete book of fishing: a guide to freshwater, saltwater & big-game fishing|url=https://books.google.com/books?id=b3nWAAAAMAAJ|access-date=June 26, 2012|date=1987|publisher=Gallery Books|isbn=978-0-8317-1565-6|url-status=live|archive-url=https://web.archive.org/web/20121115010409/http://books.google.com/books?id=b3nWAAAAMAAJ|archive-date=November 15, 2012}} to tire balances and flywheels.{{cite web

|url=http://www.minourausa.com/english/support-e/recall-e.html

|title=Cast flywheel on old Magturbo trainer has been recalled since July 2000

|work=Minoura

|url-status=dead

|archive-url=https://web.archive.org/web/20130323175731/http://www.minourausa.com/english/support-e/recall-e.html

|archive-date=March 23, 2013

}}

Cadmium zinc telluride (CZT) is a semiconductive alloy that can be divided into an array of small sensing devices. These devices are similar to an integrated circuit and can detect the energy of incoming gamma ray photons. When behind an absorbing mask, the CZT sensor array can determine the direction of the rays.{{Cite book|title=The Biggest Bangs|last=Katz|first=Johnathan I.|page=[https://archive.org/details/biggestbangsmyst00katz_0/page/18 18]|publisher=Oxford University Press|date=2002|isbn=978-0-19-514570-0|url=https://archive.org/details/biggestbangsmyst00katz_0/page/18}}

File:Zinc oxide.jpg in paints.|alt=White powder on a glass plate]]

Roughly one quarter of all zinc output in the United States in 2009 was consumed in zinc compounds; a variety of which are used industrially. Zinc oxide is widely used as a white pigment in paints and as a catalyst in the manufacture of rubber to disperse heat. Zinc oxide is used to protect rubber polymers and plastics from ultraviolet radiation (UV). The semiconductor properties of zinc oxide make it useful in varistors and photocopying products.{{Cite book|last=Zhang|first=Xiaoge Gregory|title=Corrosion and Electrochemistry of Zinc|publisher=Springer|date=1996|page=93|isbn=978-0-306-45334-2|url=https://books.google.com/books?id=Qmf4VsriAtMC}} The zinc zinc-oxide cycle is a two step thermochemical process based on zinc and zinc oxide for hydrogen production.{{cite web|url=http://www.hydrogen.energy.gov/pdfs/review06/pd_10_weimer.pdf|title=Development of Solar-powered Thermochemical Production of Hydrogen from Water|last=Weimer|first=Al|date=May 17, 2006|access-date=January 10, 2009|publisher=U.S. Department of Energy|url-status=live|archive-url=https://web.archive.org/web/20090205122514/http://www.hydrogen.energy.gov/pdfs/review06/pd_10_weimer.pdf|archive-date=February 5, 2009}}

Zinc chloride is often added to lumber as a fire retardant{{harvnb|Heiserman|1992|p=124}} and sometimes as a wood preservative.{{cite web|title=Wood preservatives |last=Blew|first=Joseph Oscar|date=1953|publisher=Department of Agriculture, Forest Service, Forest Products Laboratory|url=http://ir.library.oregonstate.edu/xmlui/bitstream/handle/1957/816/FPL_D149ocr.pdf |hdl=1957/816|url-status=live|archive-url=https://web.archive.org/web/20120114143025/http://ir.library.oregonstate.edu/xmlui/bitstream/handle/1957/816/FPL_D149ocr.pdf|archive-date=January 14, 2012}} It is used in the manufacture of other chemicals. Zinc methyl ({{chem|Zn(CH₃)|2}}) is used in a number of organic syntheses.{{Cite journal|first=Edward|last=Frankland|author-link=Edward Frankland|journal=Liebig's Annalen der Chemie und Pharmacie|title=Notiz über eine neue Reihe organischer Körper, welche Metalle, Phosphor u. s. w. enthalten|date=1849|volume=71|issue=2|pages=213–216|doi=10.1002/jlac.18490710206|language=de|url=https://zenodo.org/record/1427026}} Zinc sulfide (ZnS) is used in luminescent pigments such as on the hands of clocks, X-ray and television screens, and luminous paints.{{harvnb|CRC|2006|p=4{{hyphen}}42}} Crystals of ZnS are used in lasers that operate in the mid-infrared part of the spectrum.{{Cite book|last=Paschotta|first=Rüdiger|title=Encyclopedia of Laser Physics and Technology|publisher=Wiley-VCH|date=2008|page=798|isbn=978-3-527-40828-3|url=https://books.google.com/books?id=2p9WvgAACAAJ}} Zinc sulfate is a chemical in dyes and pigments. Zinc pyrithione is used in antifouling paints.{{Cite journal|journal=Environment International|volume=30|date=2004|issue=2|pages=235–248|doi=10.1016/S0160-4120(03)00176-4 |pmid=14749112|title=Worldwide occurrence and effects of antifouling paint booster biocides in the aquatic environment: a review|first=I. K.|last=Konstantinou|author2=Albanis, T. A. |bibcode=2004EnInt..30..235K }}

Zinc powder is sometimes used as a propellant in model rockets. When a compressed mixture of 70% zinc and 30% sulfur powder is ignited there is a violent chemical reaction. This produces zinc sulfide, together with large amounts of hot gas, heat, and light.{{cite web|url=http://www.angelo.edu/faculty/kboudrea/demos/zinc_sulfur/zinc_sulfur.htm|title=Zinc + Sulfur|last=Boudreaux|first=Kevin A.|publisher=Angelo State University|access-date=October 8, 2008|url-status=live|archive-url=https://web.archive.org/web/20081202034703/http://www.angelo.edu/faculty/kboudrea/demos/zinc_sulfur/zinc_sulfur.htm|archive-date=December 2, 2008}}

Zinc sheet metal is used as a durable covering for roofs, walls, and countertops, the last often seen in bistros and oyster bars, and is known for the rustic look imparted by its surface oxidation in use to a blue-gray patina and susceptibility to scratching.{{cite web |url=https://rolled.zinc.org/ |title=Rolled and Titanium Zinc Sheet |access-date=October 21, 2022}}{{cite web |url=https://www.hunker.com/13466339/things-you-should-know-about-zinc-countertops |title=Things You Should Know About Zinc Countertops |date=August 4, 2017 |access-date=October 21, 2022}}{{cite web | url=https://www.masterclass.com/articles/guide-to-zinc-countertops |title=Guide to Zinc Countertops: Benefits of Zinc Kitchen Counters |access-date=October 21, 2022}}{{cite web|title=Technical Information|date=2008|publisher=Zinc Counters|url=http://www.zinccounters.co.uk/html/tech/tech.htm|access-date=November 29, 2008|url-status=dead|archive-url=https://web.archive.org/web/20081121002508/http://www.zinccounters.co.uk/html/tech/tech.htm|archive-date=November 21, 2008}}

{{chem|64|Zn}}, the most abundant isotope of zinc, is very susceptible to neutron activation, being transmuted into the highly radioactive {{chem|65|Zn}}, which has a half-life of 244 days and produces intense gamma radiation. Because of this, zinc oxide used in nuclear reactors as an anti-corrosion agent is depleted of {{chem|64|Zn}} before use, this is called depleted zinc oxide. For the same reason, zinc has been proposed as a salting material for nuclear weapons (cobalt is another, better-known salting material). A jacket of isotopically enriched {{chem|64|Zn}} would be irradiated by the intense high-energy neutron flux from an exploding thermonuclear weapon, forming a large amount of {{chem|65|Zn}} significantly increasing the radioactivity of the weapon's fallout. Such a weapon is not known to have ever been built, tested, or used.{{Cite journal|title=Weapons of Mass Destruction|first=David Tin|last=Win|author2=Masum, Al|url=http://www.journal.au.edu/au_techno/2003/apr2003/aujt6-4_article07.pdf|date=2003|journal=Assumption University Journal of Technology|volume=6|issue=4|page=199|publisher=Assumption University|access-date=April 6, 2009|url-status=live|archive-url=https://web.archive.org/web/20090326001457/http://www.journal.au.edu/au_techno/2003/apr2003/aujt6-4_article07.pdf|archive-date=March 26, 2009}}

{{chem|65|Zn}} is used as a tracer to study how alloys that contain zinc wear out, or the path and the role of zinc in organisms.{{cite book|url=http://www.encyclopedia.com/doc/1G2-3427000114.html|isbn=978-0-7876-2846-8|publisher=U. X. L. /Gale|date=1999|title=Chemical Elements: From Carbon to Krypton|author=David E. Newton|access-date=April 6, 2009|url-status=live|archive-url=https://web.archive.org/web/20080710132328/http://www.encyclopedia.com/doc/1G2-3427000114.html|archive-date=July 10, 2008}}

Zinc dithiocarbamate complexes are used as agricultural fungicides; these include Zineb, Metiram, Propineb and Ziram.{{Cite book|url=https://books.google.com/books?id=cItuoO9zSjkC&pg=PA591|title=Ullmann's Agrochemicals|date=2007|publisher=Wiley-Vch (COR)|isbn=978-3-527-31604-5|pages=591–592}}{{Dead link|date=June 2024 |bot=InternetArchiveBot |fix-attempted=yes }} Zinc naphthenate is used as wood preservative.{{Cite book|title=Primary Wood Processing: Principles and Practice| last=Walker|first =J. C. F.|date=2006|publisher=Springer|isbn=978-1-4020-4392-5|page=317}} Zinc in the form of ZDDP, is used as an anti-wear additive for metal parts in engine oil.{{cite news|title=ZDDP Engine Oil – The Zinc Factor|url=http://www.mustangmonthly.com/techarticles/mump_0907_zddp_zinc_additive_engine_oil/index.html|newspaper=Mustang Monthly|access-date=September 19, 2009|url-status=live|archive-url=https://web.archive.org/web/20090912041431/http://www.mustangmonthly.com/techarticles/mump_0907_zddp_zinc_additive_engine_oil/index.html|archive-date=September 12, 2009}}

File:DiphenylzincCarbonylAddition.png

Organozinc chemistry is the science of compounds that contain carbon-zinc bonds, describing the physical properties, synthesis, and chemical reactions. Many organozinc compounds are commercially important.{{cite book | doi = 10.1002/0471264180.or066.01 | title = The Allylic Trihaloacetimidate Rearrangement | series = Organic Reactions | date = 2005 | last1 = Overman | first1 = Larry E. | last2 = Carpenter | first2 = Nancy E. | isbn = 978-0-471-26418-7 | volume = 66 | pages =1–107}}{{cite book | isbn = 978-0-470-09337-5 | url = https://books.google.com/books?id=Y3wYEmIHlqUC | title = The Chemistry of Organozinc Compounds: R-Zn | last1 = Rappoport | first1 = Zvi | last2 = Marek | first2 = Ilan | date = December 17, 2007 | publisher=John Wiley & Sons | url-status=live | archive-url = https://web.archive.org/web/20160414165728/https://books.google.com/books?id=Y3wYEmIHlqUC | archive-date = April 14, 2016 | df = mdy-all }}{{cite book | isbn = 978-0-19-850121-3 | url = https://books.google.com/books?id=UH5tQgAACAAJ | title = Organozinc reagents: A practical approach | last1 = Knochel | first1 = Paul | last2 = Jones | first2 = Philip | date = 1999 | publisher=Oxford University Press | url-status=live | archive-url = https://web.archive.org/web/20160414152600/https://books.google.com/books?id=UH5tQgAACAAJ | archive-date = April 14, 2016 | df = mdy-all }}{{cite book | url = https://books.google.com/books?id=hgUqZkG23PAC | isbn = 978-3-13-103061-0 | title = Synthetic Methods of Organometallic and Inorganic Chemistry: Catalysis | last1 = Herrmann | first1 = Wolfgang A. | date = January 2002 | publisher = Georg Thieme Verlag | url-status=live | archive-url = https://web.archive.org/web/20160414190931/https://books.google.com/books?id=hgUqZkG23PAC | archive-date = April 14, 2016 | df = mdy-all }} Among important applications are:

• The Frankland-Duppa Reaction in which an oxalate ester (ROCOCOOR) reacts with an alkyl halide R'X, zinc and hydrochloric acid to form α-hydroxycarboxylic esters RR'COHCOORE. Frankland, Ann. 126, 109 (1863)E. Frankland, B. F. Duppa, Ann. 135, 25 (1865)
• Organozincs have similar reactivity to Grignard reagents but are much less nucleophilic, and they are expensive and difficult to handle. Organozincs typically perform nucleophilic addition on electrophiles such as aldehydes, which are then reduced to alcohols. Commercially available diorganozinc compounds include dimethylzinc, diethylzinc and diphenylzinc. Like Grignard reagents, organozincs are commonly produced from organobromine precursors.

Zinc has found many uses in catalysis in organic synthesis including enantioselective synthesis, being a cheap and readily available alternative to precious metal complexes. Quantitative results (yield and enantiomeric excess) obtained with chiral zinc catalysts can be comparable to those achieved with palladium, ruthenium, iridium and others.{{cite journal|last1=Łowicki|first1=Daniel|author2=Baś, Sebastian|author3=Mlynarski, Jacek|title=Chiral zinc catalysts for asymmetric synthesis|journal=Tetrahedron|date=2015|volume=71|issue=9|pages=1339–1394|doi=10.1016/j.tet.2014.12.022}}

File:Zinc pills.jpg supplement pills]]

File:Zinc gluconate structure.svg is one compound used for the delivery of zinc as a dietary supplement.|alt=Skeletal chemical formula of a planar compound featuring a Zn atom in the center, symmetrically bonded to four oxygens. Those oxygens are further connected to linear COH chains.]]

{{see also|Zinc sulfate (medical use)|Zinc gluconate}}

In most single-tablet, over-the-counter, daily vitamin and mineral supplements, zinc is included in such forms as zinc oxide, zinc acetate, zinc gluconate, or zinc amino acid chelate.{{Cite book|title=Handbook of Minerals as Nutritional Supplements|last=DiSilvestro|first=Robert A.|date=2004|publisher=CRC Press|isbn=978-0-8493-1652-4|pages=135, 155}}{{cite report

|url=https://clinicaltrials.gov/ct2/show/NCT01791608

|title=Zinc Sulphate vs. Zinc Amino Acid Chelate (ZAZO)

|via=U.S. National Library of Medecine

|date=February 13, 2013

|publisher=USA Government

|access-date=April 6, 2022|last1=Sanchez

|first1=Juliana

|id=NCT01791608

}}

Generally, zinc supplement is recommended where there is high risk of zinc deficiency (such as low and middle income countries) as a preventive measure.{{cite journal |last1=Mayo-Wilson |first1=E |last2=Junior |first2=JA |last3=Imdad |first3=A |last4=Dean |first4=S |last5=Chan |first5=XH |last6=Chan |first6=ES |last7=Jaswal |first7=A |last8=Bhutta |first8=ZA |title=Zinc supplementation for preventing mortality, morbidity, and growth failure in children aged 6 months to 12 years of age. |journal=The Cochrane Database of Systematic Reviews |date=May 15, 2014 |issue=5 |pages=CD009384 |doi=10.1002/14651858.CD009384.pub2 |pmid=24826920}} Although zinc sulfate is a commonly used zinc form, zinc citrate, gluconate and picolinate may be valid options as well. These forms are better absorbed than zinc oxide.{{cite journal|title=Dietary vs. pharmacological doses of zinc: A clinical review. |journal=Clin Nutr. |volume=130 |issue=5 |doi=10.1016/j.clnu.2019.06.024|pmid=31303527|year=2019 |vauthors=Santos HO, Teixeira FJ, Schoenfeld BJ |pages=1345–1353|s2cid=196616666 }}

Zinc is an inexpensive and effective part of treatment of diarrhea among children in the developing world. Zinc becomes depleted in the body during diarrhea and replenishing zinc with a 10- to 14-day course of treatment can reduce the duration and severity of diarrheal episodes and may also prevent future episodes for as long as three months.{{cite journal|title=Therapeutic effects of oral zinc in acute and persistent diarrhea in children in developing countries: pooled analysis of randomized controlled trials|pmid=11101480|date=2000|vauthors=Bhutta ZA, Bird SM, Black RE, Brown KH, Gardner JM, Hidayat A, Khatun F, Martorell R, Ninh NX, Penny ME, Rosado JL, Roy SK, Ruel M, Sazawal S, Shankar A|display-authors=8|volume=72|issue=6 |pages=1516–1522|journal=The American Journal of Clinical Nutrition |doi=10.1093/ajcn/72.6.1516|doi-access=free}} Gastroenteritis is strongly attenuated by ingestion of zinc, possibly by direct antimicrobial action of the ions in the gastrointestinal tract, or by the absorption of the zinc and re-release from immune cells (all granulocytes secrete zinc), or both.{{cite journal|last=Aydemir |first=T. B.|author2=Blanchard, R. K. |author3=Cousins, R. J. |date=2006|title=Zinc supplementation of young men alters metallothionein, zinc transporter, and cytokine gene expression in leukocyte populations |journal=PNAS|pmid=16434472|volume=103|issue=6|pmc=1413653|doi=10.1073/pnas.0510407103|bibcode = 2006PNAS..103.1699A |pages=1699–704|doi-access=free}}{{cite journal |last=Valko|first=M. |author2=Morris, H. |author3=Cronin, M. T. D. |date=2005|title=Metals, Toxicity and Oxidative stress|journal=Current Medicinal Chemistry |issue=10 |volume=12 |doi=10.2174/0929867053764635 |pmid=15892631 |pages=1161–208 |url=http://webmail.stuba.sk/~marian.valko/PDF/CMC_2005.pdf|url-status=dead|archive-url=https://web.archive.org/web/20170808080110/http://webmail.stuba.sk/~marian.valko/PDF/CMC_2005.pdf |archive-date=August 8, 2017}}

{{Excerpt|Zinc and the common cold}}

{{See also|Zinc deficiency#Appetite}}

Zinc deficiency may lead to loss of appetite.{{cite journal | vauthors = Suzuki H, Asakawa A, Li JB, Tsai M, Amitani H, Ohinata K, Komai M, Inui A | title = Zinc as an appetite stimulator – the possible role of zinc in the progression of diseases such as cachexia and sarcopenia | journal = Recent Patents on Food, Nutrition & Agriculture | volume = 3 | issue = 3 | pages = 226–231 | date =2011 | pmid = 21846317 | doi = 10.2174/2212798411103030226 }} The use of zinc in the treatment of anorexia has been advocated since 1979. At least 15 clinical trials have shown that zinc improved weight gain in anorexia. A 1994 trial showed that zinc doubled the rate of body mass increase in the treatment of anorexia nervosa. Deficiency of other nutrients such as tyrosine, tryptophan and thiamine could contribute to this phenomenon of "malnutrition-induced malnutrition".{{cite journal|title=Neurobiology of Zinc-Influenced Eating Behavior |journal=The Journal of Nutrition|volume=130|issue=5|pages=1493S–1499S|doi=10.1093/jn/130.5.1493S|pmid=10801965|year=2000|last1=Shay|first1=Neil F.|last2=Mangian|first2=Heather F.|doi-access=free}}

A meta-analysis of 33 prospective intervention trials regarding zinc supplementation and its effects on the growth of children in many countries showed that zinc supplementation alone had a statistically significant effect on linear growth and body weight gain, indicating that other deficiencies that may have been present were not responsible for growth retardation.{{cite journal|title=Zinc|journal=StatPearls [Internet]|pmid=31613478|year=2019|vauthors=Rabinovich D, Smadi Y}}

People taking zinc supplements may slow down the progress to age-related macular degeneration.{{cite journal |vauthors=Evans JR, Lawrenson JG |date=13 Sep 2023 |title=Antioxidant vitamin and mineral supplements for slowing the progression of age-related macular degeneration |journal=Cochrane Database Syst Rev |volume=2023 |issue=9 |pages=CD000254 |doi=10.1002/14651858.CD000254.pub5 |pmid=37702300|pmc=10498493 }} Zinc supplement is an effective treatment for acrodermatitis enteropathica, a genetic disorder affecting zinc absorption that was previously fatal to affected infants. Zinc deficiency has been associated with major depressive disorder (MDD), and zinc supplements may be an effective treatment.{{cite journal | vauthors = Swardfager W, Herrmann N, McIntyre RS, Mazereeuw G, Goldberger K, Cha DS, Schwartz Y, Lanctôt KL | title = Potential roles of zinc in the pathophysiology and treatment of major depressive disorder | journal = Neurosci. Biobehav. Rev. | volume = 37 | issue = 5 | pages = 911–929 | date = June 2013 | pmid = 23567517 | doi = 10.1016/j.neubiorev.2013.03.018 | s2cid = 1725139 }} Zinc may help individuals sleep more.

{{further|Zinc oxide#Medicine}}

Topical preparations of zinc include those used on the skin, often in the form of zinc oxide. Zinc oxide is generally recognized by the FDA as safe and effective{{Cite journal |last=Research |first=Center for Drug Evaluation and |date=November 16, 2021 |title=Questions and Answers: FDA posts deemed final order and proposed order for over-the-counter sunscreen |url=https://www.fda.gov/drugs/understanding-over-counter-medicines/questions-and-answers-fda-posts-deemed-final-order-and-proposed-order-over-counter-sunscreen |journal=FDA |language=en}} and is considered a very photo-stable.{{Citation |last1=Chauhan |first1=Ravi |title=Advancing of Zinc Oxide Nanoparticles for Cosmetic Applications |date=2021 |work=Handbook of Consumer Nanoproducts |pages=1–16 |editor-last=Mallakpour |editor-first=Shadpour |place=Singapore |publisher=Springer |language=en |doi=10.1007/978-981-15-6453-6_100-1 |isbn=978-981-15-6453-6 |last2=Kumar |first2=Amit |last3=Tripathi |first3=Ramna |last4=Kumar |first4=Akhilesh |s2cid=245778598 |editor2-last=Hussain |editor2-first=Chaudhery Mustansar}} Zinc oxide is one of the most common active ingredients formulated into a sunscreen to mitigate sunburn. Applied thinly to a baby's diaper area (perineum) with each diaper change, it can protect against diaper rash.

Chelated zinc is used in toothpastes and mouthwashes to prevent bad breath; zinc citrate helps reduce the build-up of calculus (tartar).{{Cite journal|volume =30|issue =5|pages=427–434|date=2003|title=The effects of a new mouthrinse containing chlorhexidine, cetylpyridinium chloride and zinc lactate on the microflora of oral halitosis patients: a dual-centre, double-blind placebo-controlled study|author=Roldán, S.|author2=Winkel, E. G.|author3=Herrera, D.|author4=Sanz, M.|author5=Van Winkelhoff, A. J.|doi=10.1034/j.1600-051X.2003.20004.x|pmid =12716335|journal =Journal of Clinical Periodontology}}{{Cite web|title=Toothpastes|url=https://www.ada.org/en/member-center/oral-health-topics/toothpastes|access-date=September 27, 2020|website=www.ada.org|archive-date=March 5, 2016|archive-url=https://web.archive.org/web/20160305154431/http://ada.org/1322.aspx|url-status=dead}}

Zinc pyrithione is widely included in shampoos to prevent dandruff.{{cite journal|journal=British Journal of Dermatology|volume=112|issue=4|pages=415–422|title=The effects of a shampoo containing zinc pyrithione on the control of dandruff|first=R.|last=Marks|author2=Pearse, A. D. |author3=Walker, A. P. |doi=10.1111/j.1365-2133.1985.tb02314.x|pmid=3158327|date=1985|s2cid=23368244}}

Topical zinc has also been shown to effectively treat, as well as prolong remission in genital herpes.{{cite journal |last1=Mahajan |first1=BB |last2=Dhawan |first2=M |last3=Singh |first3=R |title=Herpes genitalis – Topical zinc sulfate: An alternative therapeutic and modality. |journal=Indian Journal of Sexually Transmitted Diseases and AIDS |date=January 2013 |volume=34 |issue=1 |pages=32–4 |doi=10.4103/0253-7184.112867 |pmid=23919052 |pmc=3730471 |doi-access=free }}

{{Main|Zinc in biology}}

Zinc is an essential trace element for humans.{{cite book|first1= Wolfgang |last1= Maret|chapter= Zinc and Human Disease|editor=Astrid Sigel|editor2=Helmut Sigel|editor3=Roland K. O. Sigel|title=Interrelations between Essential Metal Ions and Human Diseases|series=Metal Ions in Life Sciences|volume=13|date=2013|publisher=Springer|pages=389–414|doi=10.1007/978-94-007-7500-8_12|pmid= 24470098|isbn= 978-94-007-7499-5}} and other animals,{{cite journal|author=Prasad A. S.|title=Zinc in Human Health: Effect of Zinc on Immune Cells|journal=Mol. Med.|volume=14|date=2008|pmid=18385818|pmc=2277319|doi=10.2119/2008-00033.Prasad|issue=5–6|pages=353–7}} for plants{{cite journal|last=Broadley|first=M. R.|author2=White, P. J. |author3=Hammond, J. P. |author4=Zelko I. |author5= Lux A. |title=Zinc in plants|journal=New Phytologist|volume=173|date=2007|pmid=17286818|doi=10.1111/j.1469-8137.2007.01996.x|issue=4|pages=677–702|doi-access=free|bibcode=2007NewPh.173..677B }} and for microorganisms.Zinc's role in microorganisms is particularly reviewed in: {{cite journal|author=Sugarman B|title=Zinc and infection|journal=Reviews of Infectious Diseases|volume=5|date=1983|pmid=6338570|issue=1|pages=137–47 |doi=10.1093/clinids/5.1.137}} Zinc is required for the function of over 300 enzymes and 1000 transcription factors,{{cite journal | vauthors = Cherasse Y, Urade Y | title = Dietary Zinc Acts as a Sleep Modulator | journal = International Journal of Molecular Sciences | volume = 18 | issue = 11 | pages = 2334 | date = November 2017 | pmid = 29113075 | pmc = 5713303 | doi = 10.3390/ijms18112334 | quote = Zinc is the second most abundant trace metal in the human body, and is essential for many biological processes.  ... The trace metal zinc is an essential cofactor for more than 300 enzymes and 1000 transcription factors [16]. ... In the central nervous system, zinc is the second most abundant trace metal and is involved in many processes. In addition to its role in enzymatic activity, it also plays a major role in cell signaling and modulation of neuronal activity.| doi-access = free }} and is stored and transferred in metallothioneins.{{harvnb|Cotton et al.|1999|pp=625–629}}{{Cite journal |last1=Plum|first1=Laura|last2=Rink |first2=Lothar|last3=Haase|first3=Hajo|title=The Essential Toxin: Impact of Zinc on Human Health|journal=Int J Environ Res Public Health|volume=7|issue=4|pages=1342–1365 |doi=10.3390/ijerph7041342|date=2010 |pmc=2872358 |pmid=20617034|doi-access=free}} It is the second most abundant trace metal in humans after iron and it is the only metal which appears in all enzyme classes.

In proteins, zinc ions are often coordinated to the amino acid side chains of aspartic acid, glutamic acid, cysteine and histidine. The theoretical and computational description of this zinc binding in proteins (as well as that of other transition metals) is difficult.{{cite journal|title = Molecular dynamics study of zinc binding to cysteines in a peptide mimic of the alcohol dehydrogenase structural zinc site|journal = Phys. Chem. Chem. Phys. |volume = 11|issue = 6|pages = 975–83|date = 2009|pmid = 19177216|doi = 10.1039/b815482a|bibcode = 2009PCCP...11..975B|last1 = Brandt|first1 = Erik G.|last2 = Hellgren|first2 = Mikko|last3 = Brinck|first3 = Tore|last4 = Bergman|first4 = Tomas|last5 = Edholm|first5 = Olle|url = https://zenodo.org/record/996012}}

Roughly {{nowrap|2–4}} grams of zinc{{cite journal|last=Rink|first =L.|author2=Gabriel P. |title=Zinc and the immune system|journal=Proc Nutr Soc|volume=59|date=2000|pmid=11115789|doi=10.1017/S0029665100000781|issue=4|pages=541–52|doi-access=free}} are distributed throughout the human body. Most zinc is in the brain, muscle, bones, kidney, and liver, with the highest concentrations in the prostate and parts of the eye.{{cite book|last=Wapnir|first=Raul A.|title=Protein Nutrition and Mineral Absorption|publisher=CRC Press|location=Boca Raton, Florida|date=1990|isbn=978-0-8493-5227-0|url=https://books.google.com/books?id=qfKdaCoZS18C}} Semen is particularly rich in zinc, a key factor in prostate gland function and reproductive organ growth.{{cite book|last=Berdanier|first=Carolyn D.|author2=Dwyer, Johanna T. |author3=Feldman, Elaine B. |title=Handbook of Nutrition and Food|publisher=CRC Press|location=Boca Raton, Florida|date=2007|isbn=978-0-8493-9218-4|url=https://books.google.com/books?id=PJpieIePsmUC}}

Zinc homeostasis of the body is mainly controlled by the intestine. Here, ZIP4 and especially TRPM7 were linked to intestinal zinc uptake essential for postnatal survival.{{Cite journal|last1=Mittermeier|first1=Lorenz|last2=Gudermann|first2=Thomas|last3=Zakharian|first3=Eleonora|last4=Simmons|first4=David G.|last5=Braun|first5=Vladimir|last6=Chubanov|first6=Masayuki|last7=Hilgendorff|first7=Anne|last8=Recordati|first8=Camilla|last9=Breit|first9=Andreas|date=February 15, 2019|title=TRPM7 is the central gatekeeper of intestinal mineral absorption essential for postnatal survival|journal=Proceedings of the National Academy of Sciences|volume=116|issue=10|pages=4706–4715|doi=10.1073/pnas.1810633116|issn=0027-8424|pmid=30770447|pmc=6410795|bibcode=2019PNAS..116.4706M |doi-access=free}}{{Cite journal|last1=Kasana|first1=Shakhenabat|last2=Din|first2=Jamila|last3=Maret|first3=Wolfgang|date=January 2015|title=Genetic causes and gene–nutrient interactions in mammalian zinc deficiencies: acrodermatitis enteropathica and transient neonatal zinc deficiency as examples|journal=Journal of Trace Elements in Medicine and Biology|volume=29|pages=47–62|doi=10.1016/j.jtemb.2014.10.003|issn=1878-3252|pmid=25468189|bibcode=2015JTEMB..29...47K }}

In humans, the biological roles of zinc are ubiquitous. It interacts with "a wide range of organic ligands", and has roles in the metabolism of RNA and DNA, signal transduction, and gene expression. It also regulates apoptosis. A review from 2015 indicated that about 10% of human proteins (~3000) bind zinc,{{cite journal | vauthors = Djoko KY, Ong CL, Walker MJ, McEwan AG | title = The Role of Copper and Zinc Toxicity in Innate Immune Defense against Bacterial Pathogens | journal = The Journal of Biological Chemistry | volume = 290 | issue = 31 | pages = 18954–61 | date = July 2015 | pmid = 26055706 | pmc = 4521016 | doi = 10.1074/jbc.R115.647099 | quote = Zn is present in up to 10% of proteins in the human proteome and computational analysis predicted that ~30% of these ~3000 Zn-containing proteins are crucial cellular enzymes, such as hydrolases, ligases, transferases, oxidoreductases, and isomerases (42,43).| doi-access = free }} in addition to hundreds more that transport and traffic zinc; a similar in silico study in the plant Arabidopsis thaliana found 2367 zinc-related proteins.

In the brain, zinc is stored in specific synaptic vesicles by glutamatergic neurons and can modulate neuronal excitability.{{cite journal | vauthors = Bitanihirwe BK, Cunningham MG | title = Zinc: the brain's dark horse | journal = Synapse | volume = 63 | issue = 11 | pages = 1029–1049 | date = November 2009 | pmid = 19623531 | doi = 10.1002/syn.20683 | s2cid = 206520330 }} It plays a key role in synaptic plasticity and so in learning.{{cite journal|author=Nakashima AS|author2=Dyck RH|date=2009|title=Zinc and cortical plasticity|journal=Brain Res Rev|volume=59|doi=10.1016/j.brainresrev.2008.10.003|pmid=19026685|issue=2|pages=347–73|s2cid=22507338}} Zinc homeostasis also plays a critical role in the functional regulation of the central nervous system. Dysregulation of zinc homeostasis in the central nervous system that results in excessive synaptic zinc concentrations is believed to induce neurotoxicity through mitochondrial oxidative stress (e.g., by disrupting certain enzymes involved in the electron transport chain, including complex I, complex III, and α-ketoglutarate dehydrogenase), the dysregulation of calcium homeostasis, glutamatergic neuronal excitotoxicity, and interference with intraneuronal signal transduction.{{cite journal | vauthors = Tyszka-Czochara M, Grzywacz A, Gdula-Argasińska J, Librowski T, Wiliński B, Opoka W | title = The role of zinc in the pathogenesis and treatment of central nervous system (CNS) diseases. Implications of zinc homeostasis for proper CNS function | journal = Acta Pol. Pharm. | volume = 71 | issue = 3 | pages = 369–377 | date = May 2014 | pmid = 25265815 | url = http://www.ptfarm.pl/pub/File/Acta_Poloniae/2014/3/369.pdf | url-status=live | archive-url = https://web.archive.org/web/20170829234531/http://www.ptfarm.pl/pub/File/Acta_Poloniae/2014/3/369.pdf | archive-date = August 29, 2017 | df = mdy-all }} L- and D-histidine facilitate brain zinc uptake.{{Cite journal |pmid=17119290|year=2006|last1=Yokel|first1=R. A.|title=Blood-brain barrier flux of aluminum, manganese, iron and other metals suspected to contribute to metal-induced neurodegeneration|journal=Journal of Alzheimer's Disease |volume=10|issue=2–3|pages=223–53|doi=10.3233/JAD-2006-102-309}} SLC30A3 is the primary zinc transporter involved in cerebral zinc homeostasis.{{cite journal | vauthors = Prakash A, Bharti K, Majeed AB | title = Zinc: indications in brain disorders | journal = Fundam Clin Pharmacol | volume = 29 | issue = 2 | pages = 131–149 | date = April 2015 | pmid = 25659970 | doi = 10.1111/fcp.12110| s2cid = 21141511 }}

File:Carbonic anhydrase.png of human carbonic anhydrase II, with zinc atom visible in the center|alt=Interconnected stripes, mostly of yellow and blue color with a few red segments.]]

File:Zinc finger rendered.png help read DNA sequences.|alt=A twisted band, with one side painted blue and another gray. Its two ends are connected through some chemical species to a green atom (zinc).]]

Zinc is an efficient Lewis acid, making it a useful catalytic agent in hydroxylation and other enzymatic reactions. The metal also has a flexible coordination geometry, which allows proteins using it to rapidly shift conformations to perform biological reactions.{{cite book|last=Stipanuk|first=Martha H.|title=Biochemical, Physiological & Molecular Aspects of Human Nutrition|date=2006|pages=1043–1067|publisher=W. B. Saunders Company|isbn=978-0-7216-4452-3}} Two examples of zinc-containing enzymes are carbonic anhydrase and carboxypeptidase, which are vital to the processes of carbon dioxide ({{chem|CO|2}}) regulation and digestion of proteins, respectively.{{harvnb|Greenwood|Earnshaw|1997|pp=1224–1225}}

In vertebrate blood, carbonic anhydrase converts {{chem|CO|2}} into bicarbonate and the same enzyme transforms the bicarbonate back into {{chem|CO|2}} for exhalation through the lungs.{{cite book|last=Kohen|first=Amnon |author2=Limbach, Hans-Heinrich |title=Isotope Effects in Chemistry and Biology|publisher=CRC Press|location=Boca Raton, Florida|date=2006|page=850|isbn=978-0-8247-2449-8|url=https://books.google.com/books?id=7EiIqrRBBQgC}} Without this enzyme, this conversion would occur about one million times slower{{harvnb|Greenwood|Earnshaw|1997|p=1225}} at the normal blood pH of 7 or would require a pH of 10 or more.{{harvnb|Cotton et al.|1999|p=627}} The non-related β-carbonic anhydrase is required in plants for leaf formation, the synthesis of indole acetic acid (auxin) and alcoholic fermentation.{{cite journal|title=Effects of indole-3-acetic acid and zinc on the growth, osmotic potential and soluble carbon and nitrogen components of soybean plants growing under water deficit|last=Gadallah|first=MA |journal=Journal of Arid Environments|volume=44|date=2000|issue=4|pages=451–467|doi=10.1006/jare.1999.0610|bibcode=2000JArEn..44..451G}}

Carboxypeptidase cleaves peptide linkages during digestion of proteins. A coordinate covalent bond is formed between the terminal peptide and a C=O group attached to zinc, which gives the carbon a positive charge. This helps to create a hydrophobic pocket on the enzyme near the zinc, which attracts the non-polar part of the protein being digested.

Zinc has been recognized as a messenger, able to activate signalling pathways. Many of these pathways provide the driving force in aberrant cancer growth. They can be targeted through ZIP transporters.{{cite book|last1=Ziliotto|first1=Silvia| last2=Ogle |first2=Olivia| last3=Yaylor |first3=Kathryn M.|editor1-last=Sigel|editor1-first=Astrid|editor2-last=Sigel|editor2-first=Helmut|editor3-last=Freisinger|editor3-first=Eva|editor4-last=Sigel|editor4-first=Roland K. O.|title=Metallo-Drugs: Development and Action of Anticancer Agents|series=Metal Ions in Life Sciences|date=2018|volume= 18|doi= 10.1515/9783110470734-023 |pmid=29394036|publisher=de Gruyter GmbH|location=Berlin|chapter= Chapter 17. Targeting Zinc(II) Signalling to Prevent Cancer|pages= 507–529|isbn=9783110470734}}

Zinc serves a purely structural role in zinc fingers, twists and clusters.{{harvnb|Cotton et al.|1999|p=628}} Zinc fingers form parts of some transcription factors, which are proteins that recognize DNA base sequences during the replication and transcription of DNA. Each of the nine or ten {{chem|Zn|2+}} ions in a zinc finger helps maintain the finger's structure by coordinately binding to four amino acids in the transcription factor.

In blood plasma, zinc is bound to and transported by albumin (60%, low-affinity) and transferrin (10%). Because transferrin also transports iron, excessive iron reduces zinc absorption, and vice versa. A similar antagonism exists with copper.{{Cite book|first=Eleanor Noss|last=Whitney|author2=Rolfes, Sharon Rady |date=2005|title=Understanding Nutrition|pages=447–450|edition=10th|publisher=Thomson Learning|isbn=978-1-4288-1893-4}} The concentration of zinc in blood plasma stays relatively constant regardless of zinc intake. Cells in the salivary gland, prostate, immune system, and intestine use zinc signaling to communicate with other cells.{{Cite journal|last=Hershfinkel|first=M|author2=Silverman WF |author3=Sekler I |title=The Zinc Sensing Receptor, a Link Between Zinc and Cell Signaling |journal=Molecular Medicine|volume=13|date=2007|doi= 10.2119/2006-00038.Hershfinkel |pmid=17728842|issue=7–8|pmc=1952663|pages=331–336}}

Zinc may be held in metallothionein reserves within microorganisms or in the intestines or liver of animals.{{harvnb|Cotton et al.|1999|p=629}} Metallothionein in intestinal cells is capable of adjusting absorption of zinc by 15–40%.{{Cite book|title=Vitamins and Minerals Demystified|last=Blake|first=Steve|publisher=McGraw-Hill Professional|date=2007|isbn=978-0-07-148901-0|page=242}} However, inadequate or excessive zinc intake can be harmful; excess zinc particularly impairs copper absorption because metallothionein absorbs both metals.

The human dopamine transporter contains a high affinity extracellular zinc binding site which, upon zinc binding, inhibits dopamine reuptake and amplifies amphetamine-induced dopamine efflux in vitro.{{cite journal | vauthors = Krause J | title = SPECT and PET of the dopamine transporter in attention-deficit/hyperactivity disorder | journal = Expert Rev. Neurother. |volume = 8 |issue = 4 |pages = 611–625 |date = 2008 | pmid = 18416663 | doi = 10.1586/14737175.8.4.611| s2cid = 24589993 }}{{cite journal | vauthors = Sulzer D | title = How addictive drugs disrupt presynaptic dopamine neurotransmission |journal = Neuron |volume = 69 |issue = 4 |pages = 628–649 | date =2011 |pmid = 21338876 |pmc = 3065181 |doi = 10.1016/j.neuron.2011.02.010}}{{cite journal | vauthors = Scholze P, Nørregaard L, Singer EA, Freissmuth M, Gether U, Sitte HH | title = The role of zinc ions in reverse transport mediated by monoamine transporters | journal = J. Biol. Chem. | volume = 277 | issue = 24 | pages = 21505–21513 | date = 2002 | pmid = 11940571 | doi = 10.1074/jbc.M112265200 | quote = The human dopamine transporter (hDAT) contains an endogenous high affinity Zn²⁺ binding site with three coordinating residues on its extracellular face (His193, His375, and Glu396). ... Thus, when Zn²⁺ is co-released with glutamate, it may greatly augment the efflux of dopamine.| doi-access = free }} The human serotonin transporter and norepinephrine transporter do not contain zinc binding sites. Some EF-hand calcium binding proteins such as S100 or NCS-1 are also able to bind zinc ions.{{cite journal |last1=Tsvetkov |first1=PO |last2=Roman |first2=AY |last3=Baksheeva |first3=VE |last4=Nazipova |first4=AA |last5=Shevelyova |first5=MP |last6=Vladimirov |first6=VI |last7=Buyanova |first7=MF |last8=Zinchenko |first8=DV |last9=Zamyatnin AA |first9=Jr |last10=Devred |first10=F |last11=Golovin |first11=AV |last12=Permyakov |first12=SE |last13=Zernii |first13=EY |title=Functional Status of Neuronal Calcium Sensor-1 Is Modulated by Zinc Binding. |journal=Frontiers in Molecular Neuroscience |date=2018 |volume=11 |pages=459 |doi=10.3389/fnmol.2018.00459 |pmid=30618610|pmc=6302015 |doi-access=free }}

The U.S. Institute of Medicine (IOM) updated Estimated Average Requirements (EARs) and Recommended Dietary Allowances (RDAs) for zinc in 2001. The current EARs for zinc for women and men ages 14 and up is 6.8 and 9.4 mg/day, respectively. The RDAs are 8 and 11 mg/day. RDAs are higher than EARs so as to identify amounts that will cover people with higher than average requirements. RDA for pregnancy is 11 mg/day. RDA for lactation is 12 mg/day. For infants up to 12 months the RDA is 3 mg/day. For children ages 1–13 years the RDA increases with age from 3 to 8 mg/day. As for safety, the IOM sets Tolerable upper intake levels (ULs) for vitamins and minerals when evidence is sufficient. In the case of zinc the adult UL is 40 mg/day including both food and supplements combined (lower for children). Collectively the EARs, RDAs, AIs and ULs are referred to as Dietary Reference Intakes (DRIs).{{cite book |author=Institute of Medicine |year=2001 |chapter=Zinc |chapter-url=https://www.nap.edu/read/10026/chapter/14/ |doi=10.17226/10026 |pmid=25057538 |isbn=978-0-309-07279-3 |url-status=live |archive-url=https://web.archive.org/web/20170919234044/https://www.nap.edu/read/10026/chapter/14/ |archive-date=September 19, 2017 |pages=442–501 |title=Dietary Reference Intakes for Vitamin A, Vitamin K, Arsenic, Boron, Chromium, Copper, Iodine, Iron, Manganese, Molybdenum, Nickel, Silicon, Vanadium, and Zinc |location=Washington, DC |publisher=National Academy Press}}

The European Food Safety Authority (EFSA) refers to the collective set of information as Dietary Reference Values, with Population Reference Intake (PRI) instead of RDA, and Average Requirement instead of EAR. AI and UL are defined the same as in the United States. For people ages 18 and older the PRI calculations are complex, as the EFSA has set higher and higher values as the phytate content of the diet increases. For women, PRIs increase from 7.5 to 12.7 mg/day as phytate intake increases from 300 to 1200 mg/day; for men the range is 9.4 to 16.3 mg/day. These PRIs are higher than the U.S. RDAs.{{cite web| title = Overview on Dietary Reference Values for the EU population as derived by the EFSA Panel on Dietetic Products, Nutrition and Allergies| year = 2017| url = https://www.efsa.europa.eu/sites/default/files/assets/DRV_Summary_tables_jan_17.pdf| url-status=live| archive-url = https://web.archive.org/web/20170828082247/https://www.efsa.europa.eu/sites/default/files/assets/DRV_Summary_tables_jan_17.pdf| archive-date = August 28, 2017| df = mdy-all}} The EFSA reviewed the same safety question and set its UL at 25 mg/day, which is much lower than the U.S. value.{{citation| title = Tolerable Upper Intake Levels For Vitamins And Minerals| publisher = European Food Safety Authority| year = 2006| url = http://www.efsa.europa.eu/sites/default/files/efsa_rep/blobserver_assets/ndatolerableuil.pdf| url-status=live| archive-url = https://web.archive.org/web/20160316225123/http://www.efsa.europa.eu/sites/default/files/efsa_rep/blobserver_assets/ndatolerableuil.pdf| archive-date = March 16, 2016| df = mdy-all}}

For U.S. food and dietary supplement labeling purposes the amount in a serving is expressed as a percent of Daily Value (%DV). For zinc labeling purposes 100% of the Daily Value was 15 mg, but on May 27, 2016, it was revised to 11 mg.{{cite web |url=https://www.gpo.gov/fdsys/pkg/FR-2016-05-27/pdf/2016-11867.pdf |title=Federal Register May 27, 2016 Food Labeling: Revision of the Nutrition and Supplement Facts Labels. FR page 33982. |url-status=live |archive-url=https://web.archive.org/web/20160808164651/https://www.gpo.gov/fdsys/pkg/FR-2016-05-27/pdf/2016-11867.pdf |archive-date=August 8, 2016 }}{{cite web | title=Daily Value Reference of the Dietary Supplement Label Database (DSLD) | website=Dietary Supplement Label Database (DSLD) | url=https://www.dsld.nlm.nih.gov/dsld/dailyvalue.jsp | access-date=May 16, 2020 | archive-date=April 7, 2020 | archive-url=https://web.archive.org/web/20200407073956/https://dsld.nlm.nih.gov/dsld/dailyvalue.jsp | url-status=dead }} A table of the old and new adult daily values is provided at Reference Daily Intake.

File:Foodstuff-containing-Zinc.jpg containing zinc|alt=Several plates full of various cereals, fruits and vegetables on a table.]]

Animal products such as meat, fish, shellfish, fowl, eggs, and dairy contain zinc. The concentration of zinc in plants varies with the level in the soil. With adequate zinc in the soil, the food plants that contain the most zinc are wheat (germ and bran) and various seeds, including sesame, poppy, alfalfa, celery, and mustard.{{Cite book|last=Ensminger|first=Audrey H.|author2=Konlande, James E. |title=Foods & Nutrition Encyclopedia|publisher=CRC Press|location=Boca Raton, Florida|date=1993|edition=2nd|pages=2368–2369|isbn=978-0-8493-8980-1|url=https://books.google.com/books?id=XMA9gYIj-C4C}} Zinc is also found in beans, nuts, almonds, whole grains, pumpkin seeds, sunflower seeds, and blackcurrant.{{cite web|url=http://www.nal.usda.gov/fnic/foodcomp/Data/SR20/nutrlist/sr20w309.pdf |title=Zinc content of selected foods per common measure |access-date=December 6, 2007 |publisher=United States Department of Agriculture |work=USDA National Nutrient Database for Standard Reference, Release 20 |url-status=dead |archive-url=https://web.archive.org/web/20090305081926/http://www.nal.usda.gov/fnic/foodcomp/Data/SR20/nutrlist/sr20w309.pdf |archive-date=March 5, 2009 }}

Other sources include fortified food and dietary supplements in various forms. A 1998 review concluded that zinc oxide, one of the most common supplements in the United States, and zinc carbonate are nearly insoluble and poorly absorbed in the body. This review cited studies that found lower plasma zinc concentrations in the subjects who consumed zinc oxide and zinc carbonate than in those who took zinc acetate and sulfate salts.{{Cite journal|first=Lindsay H.|last=Allen|title=Zinc and micronutrient supplements for children|journal=American Journal of Clinical Nutrition|volume=68|issue=2 Suppl|date=1998|pmid=9701167|pages=495S–498S|doi=10.1093/ajcn/68.2.495S|doi-access=free}} For fortification, however, a 2003 review recommended cereals (containing zinc oxide) as a cheap, stable source that is as easily absorbed as the more expensive forms.{{Cite journal|last=Rosado|first=J. L.|title=Zinc and copper: proposed fortification levels and recommended zinc compounds|journal=Journal of Nutrition|volume=133|date=2003|pmid=12949397|issue=9|pages=2985S–9S|doi=10.1093/jn/133.9.2985S|doi-access=free}} A 2005 study found that various compounds of zinc, including oxide and sulfate, did not show statistically significant differences in absorption when added as fortificants to maize tortillas.{{cite journal|last=Hotz|first=C.|author2=DeHaene, J. |author3=Woodhouse, L. R. |author4=Villalpando, S. |author5=Rivera, J. A. |author6= King, J. C. |title=Zinc absorption from zinc oxide, zinc sulfate, zinc oxide + EDTA, or sodium-zinc EDTA does not differ when added as fortificants to maize tortillas|journal=Journal of Nutrition|volume=135|date=2005|pmid=15867288|issue=5|pages=1102–5|doi=10.1093/jn/135.5.1102|doi-access=free}}

{{Main|Zinc deficiency}}

Nearly two billion people in the developing world are deficient in zinc. Groups at risk include children in developing countries and elderly with chronic illnesses.{{cite journal|last=Prasad|first =AS|title=Zinc deficiency : Has been known of for 40 years but ignored by global health organisations|journal=British Medical Journal |volume=326 |date=2003|pmid=12595353|pmc=1125304|doi=10.1136/bmj.326.7386.409|issue=7386|pages=409–410}} In children, it causes an increase in infection and diarrhea and contributes to the death of about 800,000 children worldwide per year. The World Health Organization advocates zinc supplementation for severe malnutrition and diarrhea.{{cite web|title=The impact of zinc supplementation on childhood mortality and severe morbidity|publisher=World Health Organization |url=https://www.who.int/child_adolescent_health/documents/zinc_mortality/en/index.html|date=2007| archive-url=https://web.archive.org/web/20090302033104/http://www.who.int/child_adolescent_health/documents/zinc_mortality/en/index.html |archive-date=March 2, 2009}} Zinc supplements help prevent disease and reduce mortality, especially among children with low birth weight or stunted growth. However, zinc supplements should not be administered alone, because many in the developing world have several deficiencies, and zinc interacts with other micronutrients.{{cite journal |last=Shrimpton |first=R|author2=Gross R |author3=Darnton-Hill I |author4= Young M |title=Zinc deficiency: what are the most appropriate interventions?|journal=British Medical Journal|volume=330|date=2005|pmid=15705693|pmc =548733|doi=10.1136/bmj.330.7487.347|issue=7487|pages=347–349}} While zinc deficiency is usually due to insufficient dietary intake, it can be associated with malabsorption, acrodermatitis enteropathica, chronic liver disease, chronic renal disease, sickle cell disease, diabetes, malignancy, and other chronic illnesses.

In the United States, a federal survey of food consumption determined that for women and men over the age of 19, average consumption was 9.7 and 14.2 mg/day, respectively. For women, 17% consumed less than the EAR, for men 11%. The percentages below EAR increased with age.{{cite web|author1=Moshfegh, Alanna |author2=Goldman, Joseph |author3=Cleveland, Linda|date=2005|url=https://www.ars.usda.gov/SP2UserFiles/Place/80400530/pdf/0102/usualintaketables2001-02.pdf|access-date=January 6, 2015|title=NHANES 2001–2002: Usual Nutrient Intakes from Food Compared to Dietary Reference Intakes|publisher=U.S. Department of Agriculture, Agricultural Research Service|at=Table A13: Zinc}} The most recent published update of the survey (NHANES 2013–2014) reported lower averages – 9.3 and 13.2 mg/day – again with intake decreasing with age.[https://www.ars.usda.gov/ARSUserFiles/80400530/pdf/1314/Table_1_NIN_GEN_13.pdf What We Eat In America, NHANES 2013–2014] {{webarchive|url=https://web.archive.org/web/20170224042515/https://www.ars.usda.gov/ARSUserFiles/80400530/pdf/1314/Table_1_NIN_GEN_13.pdf |date=February 24, 2017 }}.

Symptoms of mild zinc deficiency are diverse. Clinical outcomes include depressed growth, diarrhea, impotence and delayed sexual maturation, alopecia, eye and skin lesions, impaired appetite, altered cognition, impaired immune functions, defects in carbohydrate use, and reproductive teratogenesis. Zinc deficiency depresses immunity,{{cite journal|last=Ibs|first=KH|author2=Rink L|title=Zinc-altered immune function|journal=Journal of Nutrition |volume=133|issue=5 Suppl 1|date=2003|pmid=12730441|pages=1452S–1456S|doi=10.1093/jn/133.5.1452S|doi-access=free}} but excessive zinc does also.

Despite some concerns,{{cite journal|url=https://www.vrg.org/nutrition/2003_ADA_position_paper.pdf|pmid=12778049|year=2003|title=Position of the American Dietetic Association and Dietitians of Canada: Vegetarian diets|journal=Journal of the American Dietetic Association|volume=103|issue=6|pages=748–765 |doi=10.1053/jada.2003.50142|url-status=live|archive-url=https://web.archive.org/web/20170114103128/http://www.vrg.org/nutrition/2003_ADA_position_paper.pdf|archive-date=January 14, 2017|author1=American Dietetic Association}} western vegetarians and vegans do not suffer any more from overt zinc deficiency than meat-eaters.{{cite journal|author=Freeland-Graves JH|author2=Bodzy PW|author3=Epright MA|title=Zinc status of vegetarians|pmid=7440860|journal=Journal of the American Dietetic Association |date=1980 |volume=77|pages=655–661|issue=6|doi=10.1016/S1094-7159(21)03587-X|s2cid=8424197}} Major plant sources of zinc include cooked dried beans, sea vegetables, fortified cereals, soy foods, nuts, peas, and seeds. However, phytates in many whole-grains and fibers may interfere with zinc absorption and marginal zinc intake has poorly understood effects. The zinc chelator phytate, found in seeds and cereal bran, can contribute to zinc malabsorption. Some evidence suggests that more than the US RDA (8 mg/day for adult women; 11 mg/day for adult men) may be needed in those whose diet is high in phytates, such as some vegetarians. The European Food Safety Authority (EFSA) guidelines attempt to compensate for this by recommending higher zinc intake when dietary phytate intake is greater. These considerations must be balanced against the paucity of adequate zinc biomarkers, and the most widely used indicator, plasma zinc, has poor sensitivity and specificity.{{cite journal|last=Hambidge|first=M|title=Biomarkers of trace mineral intake and status|journal=Journal of Nutrition|volume=133|series=133|date=2003|pmid=12612181|issue=3|pages=948S–955S|doi=10.1093/jn/133.3.948S|doi-access=free}}

Species of Calluna, Erica and Vaccinium can grow in zinc-metalliferous soils, because translocation of toxic ions is prevented by the action of ericoid mycorrhizal fungi.{{cite journal|url=http://mic.sgmjournals.org/content/156/3/609.full|title=Metals, minerals and microbes: geomicrobiology and bioremediation|journal=Microbiology|author1-link=Geoffrey Michael Gadd|author=Geoffrey Michael Gadd|volume=156|date=March 2010|pages=609–643|doi=10.1099/mic.0.037143-0|pmid=20019082|issue=3|url-status=live|archive-url=https://web.archive.org/web/20141025153753/http://mic.sgmjournals.org/content/156/3/609.full|archive-date=October 25, 2014|doi-access=free}}

Zinc deficiency appears to be the most common micronutrient deficiency in crop plants; it is particularly common in high-pH soils.{{cite web

|last1=Alloway

|first1=Brian J.

|title=Zinc in Soils and Crop Nutrition, International Fertilizer Industry Association, and International Zinc Association

|date=2008

|url=http://www.fertilizer.org/HomePage/LIBRARY/Our-selection2/Fertilizer-use.html/Zinc-in-Soils-and-Crop-Nutrition.html

|url-status=dead

|archive-url=https://web.archive.org/web/20130219203257/http://www.fertilizer.org/HomePage/LIBRARY/Our-selection2/Fertilizer-use.html/Zinc-in-Soils-and-Crop-Nutrition.html

|archive-date=February 19, 2013

}} Zinc-deficient soil is cultivated in the cropland of about half of Turkey and India, a third of China, and most of Western Australia. Substantial responses to zinc fertilization have been reported in these areas. Plants that grow in soils that are zinc-deficient are more susceptible to disease. Zinc is added to the soil primarily through the weathering of rocks, but humans have added zinc through fossil fuel combustion, mine waste, phosphate fertilizers, pesticide (zinc phosphide), limestone, manure, sewage sludge, and particles from galvanized surfaces. Excess zinc is toxic to plants, although zinc toxicity is far less widespread.

{{main|Zinc toxicity}}

Although zinc is an essential requirement for good health, excess zinc can be harmful. Excessive absorption of zinc suppresses copper and iron absorption. The free zinc ion in solution is highly toxic to plants, invertebrates, and even vertebrate fish.{{cite journal|journal=Contaminant Hazard Reviews |date=1993 |issue=10 |title=Zinc Hazard to Fish, Wildlife, and Invertebrates: A Synoptic Review |last=Eisler |first=Ronald |page=5 |publisher=U.S. Department of the Interior, Fish and Wildlife Service |location=Laurel, Maryland |bibcode=1993usgs.rept....5E |url=https://pubs.er.usgs.gov/publication/5200116 |url-status=live |archive-url=https://web.archive.org/web/20120306032807/http://www.pwrc.usgs.gov/infobase/eisler/chr_26_zinc.pdf |archive-date=March 6, 2012 }} The Free Ion Activity Model is well-established in the literature, and shows that just micromolar amounts of the free ion kills some organisms. A recent example showed 6 micromolar killing 93% of all Daphnia in water.{{cite journal|title=Mechanisms of chronic waterborne Zn toxicity in Daphnia magna|first1=Brita T. A.|last1=Muyssen|last2=De Schamphelaere|first2=Karel A. C.|last3=Janssen|first3=Colin R.|journal=Aquatic Toxicology|volume=77|issue=4|date=2006|pmid=16472524|doi=10.1016/j.aquatox.2006.01.006|pages=393–401|bibcode=2006AqTox..77..393M }}

The free zinc ion is a powerful Lewis acid up to the point of being corrosive. Stomach acid contains hydrochloric acid, in which metallic zinc dissolves readily to give corrosive zinc chloride. Swallowing a post-1982 American one cent piece (97.5% zinc) can cause damage to the stomach lining through the high solubility of the zinc ion in the acidic stomach.{{cite journal|title=Chronic Ingestion of a Zinc-Based Penny|first=Dawn N.|last=Bothwell|author2=Mair, Eric A. |author3=Cable, Benjamin B. |journal=Pediatrics|volume=111|date=2003|doi=10.1542/peds.111.3.689|pmid=12612262|issue=3|pages=689–91}}

Evidence shows that people taking 100–300 mg of zinc daily may suffer induced copper deficiency. A 2007 trial observed that elderly men taking 80 mg daily were hospitalized for urinary complications more often than those taking a placebo.{{cite journal|author=Johnson AR|author2=Munoz A|author3=Gottlieb JL|author4=Jarrard DF|title=High dose zinc increases hospital admissions due to genitourinary complications|journal=J. Urol.|volume=177|date=2007|pmid=17222649|doi=10.1016/j.juro.2006.09.047|issue=2|pages=639–43}} Levels of 100–300 mg may interfere with the use of copper and iron or adversely affect cholesterol.{{cite journal|journal=American Journal of Clinical Nutrition|volume=51|date=1990|title=Zinc toxicity|first=G. J.|last=Fosmire|pmid=2407097|issue=2|pages=225–7|doi=10.1093/ajcn/51.2.225}} Zinc in excess of 500 ppm in soil interferes with the plant absorption of other essential metals, such as iron and manganese. A condition called the zinc shakes or "zinc chills" can be induced by inhalation of zinc fumes while brazing or welding galvanized materials. Zinc is a common ingredient of denture cream which may contain between 17 and 38 mg of zinc per gram. Disability and even deaths from excessive use of these products have been claimed.{{Cite news |url=http://www.tampabay.com/news/health/lawsuits-blame-denture-adhesives-for-neurological-damage/1073320 |title=Lawsuits blame denture adhesives for neurological damage (Denture adhesives cited in lawsuits) |newspaper=St. Petersburg Times |author=Richard Martin |date=February 15, 2010 |access-date=December 31, 2022 |archive-url=https://web.archive.org/web/20121011122902/https://www.tampabay.com/news/health/lawsuits-blame-denture-adhesives-for-neurological-damage/1073320/ |archive-date=October 11, 2012 |url-status=dead}}

The U.S. Food and Drug Administration (FDA) states that zinc damages nerve receptors in the nose, causing anosmia. Reports of anosmia were also observed in the 1930s when zinc preparations were used in a failed attempt to prevent polio infections.{{Cite book|url=https://books.google.com/books?id=n24Pju7kHIYC&pg=PA142|page=142|title=Conquest of viral diseases: a topical review of drugs and vaccines|author=Oxford, J. S.|author2=Öberg, Bo|publisher=Elsevier|date=1985|isbn=978-0-444-80566-9}} On June 16, 2009, the FDA ordered removal of zinc-based intranasal cold products from store shelves. The FDA said the loss of smell can be life-threatening because people with impaired smell cannot detect leaking gas or smoke, and cannot tell if food has spoiled before they eat it.{{cite news|url=https://www.latimes.com/archives/la-xpm-2009-jun-17-sci-zicam17-story.html|title=FDA says Zicam nasal products harm sense of smell|newspaper=Los Angeles Times|date=June 17, 2009|url-status=live|archive-url=https://web.archive.org/web/20120621011505/http://articles.latimes.com/2009/jun/17/science/sci-zicam17|archive-date=June 21, 2012}}

Recent research suggests that the topical antimicrobial zinc pyrithione is a potent heat shock response inducer that may impair genomic integrity with induction of PARP-dependent energy crisis in cultured human keratinocytes and melanocytes.{{cite journal |author=Lamore SD |author2=Cabello CM |author3=Wondrak GT |title=The topical antimicrobial zinc pyrithione is a heat shock response inducer that causes DNA damage and PARP-dependent energy crisis in human skin cells |journal=Cell Stress & Chaperones |volume=15 |issue=3 |pages=309–22 |date=2010 |pmid=19809895 |doi=10.1007/s12192-009-0145-6 |pmc=2866994 }}

In 1982, the US Mint began minting pennies coated in copper but containing primarily zinc. Zinc pennies pose a risk of zinc toxicosis, which can be fatal. One reported case of chronic ingestion of 425 pennies (over 1 kg of zinc) resulted in death due to gastrointestinal bacterial and fungal sepsis. Another patient who ingested 12 grams of zinc showed only lethargy and ataxia (gross lack of coordination of muscle movements).{{cite journal

|title=Zinc|first=Donald G.|last=Barceloux|journal=Clinical Toxicology|author2=Barceloux, Donald |volume=37

|issue=2|pages=279–292|date=1999|doi =10.1081/CLT-100102426|pmid=10382562}} Several other cases have been reported of humans suffering zinc intoxication by the ingestion of zinc coins.{{cite journal|title=Zinc Toxicity Following Massive Coin Ingestion|journal=American Journal of Forensic Medicine and Pathology|volume=18|issue=2|pages=148–153|date=1997|last=Bennett|first=Daniel R. M. D.|author2=Baird, Curtis J. M.D. |author3=Chan, Kwok-Ming |author4=Crookes, Peter F. |author5=Bremner, Cedric G. |author6=Gottlieb, Michael M. |author7= Naritoku, Wesley Y. M.D. |doi=10.1097/00000433-199706000-00008|pmid=9185931}}{{cite journal|journal=Radiology|volume=158|page=512|date=1986|title=Coin ingestion: unusual appearance of the penny in a child|first=S. K.|last=Fernbach|author2=Tucker G. F. |pmid=3941880|issue=2|doi=10.1148/radiology.158.2.3941880}}

Pennies and other small coins are sometimes ingested by dogs, requiring veterinary removal of the foreign objects. The zinc content of some coins can cause zinc toxicity, commonly fatal in dogs through severe hemolytic anemia and liver or kidney damage; vomiting and diarrhea are possible symptoms.{{cite journal|title=Zinc phosphide poisoning in dogs|journal=Journal of the American Veterinary Medical Association|volume=173|page=270|date=1978|pmid=689968|issue=3|last1=Stowe|first1=C. M.|last2=Nelson|first2=R.|last3=Werdin|first3=R.|last4=Fangmann|first4=G.|last5=Fredrick|first5=P.|last6=Weaver|first6=G.|last7=Arendt|first7=T. D.}} Zinc is highly toxic in parrots and poisoning can often be fatal.{{cite journal|journal =Australian Veterinary Journal|volume=63|issue =6|page=199|title=Zinc toxicity (new wire disease) in aviary birds|first=R. L.|last=Reece|author2=Dickson, D. B. |author3=Burrowes, P. J. |doi=10.1111/j.1751-0813.1986.tb02979.x|pmid=3767804|date =1986}} The consumption of fruit juices stored in galvanized cans has resulted in mass parrot poisonings with zinc.

• List of countries by zinc production
• Spelter
• Wet storage stain
• Zinc alloy electroplating
• Metal fume fever
• Piotr Steinkeller

{{notelist}}

{{reflist}}

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{{refend}}

{{Spoken Wikipedia|Zinc spoken.ogg|date=January 25, 2012}}

{{Commons}}

{{Wiktionary|zinc}}

• [http://ods.od.nih.gov/factsheets/zinc/ Zinc Fact Sheet] from the U.S. National Institutes of Health
• [http://elements.vanderkrogt.net/element.php?sym=Zn History & Etymology of Zinc]
• [http://minerals.usgs.gov/minerals/pubs/commodity/zinc/index.html Statistics and Information from the U.S. Geological Survey]{{Dead link|date=March 2025 |bot=InternetArchiveBot |fix-attempted=yes }}
• [https://www.organic-chemistry.org/chemicals/reductions/zinc-zn.shtm Reducing Agents > Zinc]
• [http://www.zinc.org American Zinc Association] Information about the uses and properties of zinc.
• [http://www.iszb.org ISZB] International Society for Zinc Biology, founded in 2008. An international, nonprofit organization bringing together scientists working on the biological actions of zinc.
• [http://zinc-uk.org Zinc-UK] Founded in 2010 to bring together scientists in the United Kingdom working on zinc.
• [http://www.periodicvideos.com/videos/030.htm Zinc] at The Periodic Table of Videos (University of Nottingham)
• [https://zincbind.net ZincBind] – a database of biological zinc binding sites.

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