Wikipedia

Zinc

chemical element with symbol Zn and atomic number 30
(Redirected from Zinc compounds)

Zinc, sometimes called spelter,[4] is a chemical element. It is in the group of metals called the transition metals. It is sometimes considered a post-transition metal. Its symbol on the periodic table is "Zn". Zinc is the 30th element on the periodic table, and has an atomic number of 30. Zinc has a mass number of 65.38. It contains 30 protons and 30 electrons. In total, 29 isotopes of zinc are known, and five of these occur in nature. Some isotopes are radioactive. Their half-lives are between 40 milliseconds for 57Zn and 5x1018 years for 70Zn.

Zinc, 00Zn
Zinc
Appearancesilver-gray
Standard atomic weight Ar°(Zn)
65.38(2)[1]
Zinc in the periodic table
Hydrogen Helium
Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon
Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon
Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton
Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon
Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon
Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson
–
↑
Zn
↓
Cd
copper ← zinc → gallium
Groupgroup 12
Periodperiod 4
Block  d-block
Electron configuration[Ar] 3d10 4s2
Electrons per shell2, 8, 18, 2
Physical properties
Phase at STPsolid
Melting point692.68 K ​(419.53 °C, ​787.15 °F)
Boiling point1180 K ​(907 °C, ​1665 °F)
Density (near r.t.)7.14 g/cm3
when liquid (at m.p.)6.57 g/cm3
Heat of fusion7.32 kJ/mol
Heat of vaporization115 kJ/mol
Molar heat capacity25.470 J/(mol·K)
Vapor pressure
P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 610 670 750 852 990 1179
Atomic properties
Oxidation states−2, 0, +1, +2 (an amphoteric oxide)
ElectronegativityPauling scale: 1.65
Ionization energies
  • 1st: 906.4 kJ/mol
  • 2nd: 1733.3 kJ/mol
  • 3rd: 3833 kJ/mol
  • (more)
Atomic radiusempirical: 134 pm
Covalent radius122±4 pm
Van der Waals radius139 pm
Color lines in a spectral range
Spectral lines of zinc
Other properties
Natural occurrenceprimordial
Crystal structure ​hexagonal close-packed (hcp)
Hexagonal close packed crystal structure for zinc
Speed of sound thin rod3850 m/s (at r.t.) (rolled)
Thermal expansion30.2 µm/(m⋅K) (at 25 °C)
Thermal conductivity116 W/(m⋅K)
Electrical resistivity59.0 nΩ⋅m (at 20 °C)
Magnetic orderingdiamagnetic
Molar magnetic susceptibility−11.4·10−6 cm3/mol (298 K)[2]
Young's modulus108 GPa
Shear modulus43 GPa
Bulk modulus70 GPa
Poisson ratio0.25
Mohs hardness2.5
Brinell hardness327–412 MPa
CAS Number7440-66-6
History
DiscoveryIndian metallurgists (before 1000 BCE)
First isolationAndreas Sigismund Marggraf (1746)
Recognized as a unique metal byRasaratna Samuccaya (800)
Isotopes of zinc
Main isotopes[3] Decay
abun­dance half-life (t1/2) mode pro­duct
64Zn 49.2% stable
65Zn synth 244 d β+ 65Cu
66Zn 27.7% stable
67Zn 4% stable
68Zn 18.5% stable
69Zn synth 56 min β− 69Ga
69mZn synth 13.8 h β− 69Ga
70Zn 0.6% stable
71Zn synth 2.4 min β− 71Ga
71mZn synth 4 h β− 71Ga
72Zn synth 46.5 h β− 72Ga
 Category: Zinc
| references

Zinc is a metal that is mostly used for galvanizing and batteries. It is the fourth most common metal used by people.

Properties

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Physical properties

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Zinc is a shiny bluish grey metal. When it has just been cut, zinc has a whitish-grey color. If it is exposed to air, it will not stay shiny for long. Its melting point is (419.58 °C (787.24 °F)), and its boiling point is (907.0 °C (1,664.6 °F)). This temperature is lower than most transition metals but higher than tin or lead. It can be melted on a cooking stove. It boils at a low temperature for a metal.[5] It is not magnetic. When heated a little, it becomes very flexible. If it is heated more, it becomes very brittle.[6] It forms alloys easily with other metals.

Chemical properties

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Zinc is a reactive metal. It is about as reactive as aluminium and more reactive than most of the more common metals, such as iron, copper, nickel, and chromium. It is less reactive than magnesium. Zinc can react with acids, bases, and nonmetals.[7] It does not rust in air, though. A coating of zinc oxide and zinc carbonate forms on the surface of the zinc when it is in air.[8] This coating stops corrosion. Acids can dissolve this coating and react with the zinc metal.[9] This reaction of zinc with an acid makes a zinc(II) salt such as zinc chloride and hydrogen gas. This is a very common chemical reaction. The reaction below is the reaction with hydrochloric acid.

Zn + 2HCl → ZnCl2 + H2
 
Zinc burning

Zinc can burn when powdered or in small pieces to make zinc oxide, a white powder. The flame is bright blue-green.[10]

2 Zn + O2 → 2 ZnO

Zinc oxide can dissolve in strong bases. This reaction happens in some batteries that have zinc in them.

ZnO + H2O + 2 OH- → Zn(OH)42-.

Zinc is a chalcophile. This means that it would rather react with sulfur and elements below it on the periodic table than oxygen. That is why zinc sulfide is the most common zinc ore, not zinc oxide.

Chemical compounds

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See also: Category:Zinc compounds

Zinc can make chemical compounds with other elements. These chemical compounds are only in one oxidation state: +2. A +1 compound has been found but it is hard to make. There are no other oxidation states other than +1 or +2.[11] Most of these compounds have no color. If they have a color, it is not the zinc that is making the color.

Zinc chloride is one of the most common zinc compounds. They are quite unreactive. They are a little acidic when dissolved in water. They make a green flame when heated in a fire.[source?]

Other zinc compounds are:

  •  
    Zinc chloride
  •  
    Zinc oxide
  •  
    Zinc sulfate

Occurence

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Five isotopes of zinc are found in nature. 64Zn is the most common isotope, with 48.63% of naturally occurring Zinc.[12] This isotope has a half-life of 4.3x1018 years.[13] This is so long, that its radioactivity can be ignored.[14] Similarly, 70
Zn (0.6%), with a half life of 1.3x1016 years is usually considered to not be radioactive. The other isotopes found in nature are 66
Zn (28%), 67
Zn (4%) and 68
Zn (19%).

 
Sphalerite, a common zinc ore

Zinc is not found as a metal in the earth's crust. Zinc is only found as zinc compounds. Sphalerite, a mineral that is made of zinc sulfide, is a main ore of zinc. Very little zinc is in the ocean. Zinc ore is normally found with copper and lead ores.

There are some other zinc ores, such as smithsonite (zinc carbonate) and a zinc silicate mineral. They are less common.

Preparation

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The zinc sulfide is concentrated by flotation. There is a detergent that collects the zinc sulfide. The impurities sink to the bottom and are removed. Then the zinc sulfide is heated in air to make zinc oxide and sulfur dioxide.[15]

2 ZnS + 3 O2 → 2 ZnO + 2 SO2

The sulfur dioxide is oxidized to sulfur trioxide.

2 SO2 + O2 → 2 SO3

The sulfur trioxide reacts with the zinc oxide to make zinc sulfate.[16] This makes a soluble form of zinc which can be processed more.

SO3 + ZnO → ZnSO4

The zinc sulfate is purified and electrolyzed.[15] This electrolysis makes oxygen, zinc, and sulfuric acid. This makes a pure zinc that is known as "SHG" or special high grade.[17]

2 ZnSO4 + 2 H2O → 2 Zn + 2 H2SO4 + O2

The sulfuric acid is reused in place of the sulfur trioxide to leach more zinc oxide.

Zinc oxide can also be reduced by carbon to zinc metal and carbon dioxide at high temperatures.[18] This is a blast furnace process similar to how iron is made.

2 ZnO + C → 2 Zn + CO2

This form of zinc is cheaper but is not pure.

Zinc is the fourth most commonly used metal in the world.[19] About 10 million tons are made every year.[19]

Uses

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As a metal

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A hot-dipped galvanized item
 
Common alkaline batteries. These batteries have a bluish-gray zinc powder in the middle of the battery.

Zinc is used in electrical batteries.[20][21] The alkaline cell and the Leclanche cell are the ones that use zinc the most. It becomes oxidized and provides electrons for the battery to run.

About 59% of zinc is used for corrosion prevention, which includes galvanizing. 47% of the world's zinc is used for galvanizing.[22] This is used to protect another metal, usually iron, from rusting. The zinc coating corrodes instead of the iron. The zinc coating can be placed on the metal in two ways. The metal can be dipped into a pot of melted zinc. The zinc can also be electroplated on to the metal. Dipping lasts longer but has a patchy surface that some do not think looks nice. It is also used in motorboats and pipelines to slow rusting.[23] The motor of a motorboat often has a "bullet" of zinc, that will corrode easily, but will help other metal parts of the motor to stay rust free.

Zinc is used in alloys. Brass is an alloy of copper and zinc. Brass is the most common zinc alloy. Zinc can form alloys with many other metals. Zinc aluminium is an alloy of zinc and aluminium, which makes good bearings. Commercial bronze has zinc in it. Sometimes cadmium telluride is reacted with zinc to make cadmium zinc telluride, a semiconductor. Nickel silver is another zinc alloy.

Zinc can be used in the pipes of a pipe organ. An alloy of tin and lead was used in the past.[24] Zinc is used in the US penny, which only has a thin layer of copper. The core is zinc.[25] Older pennies were made completely out of bronze.

A mixture of powdered zinc and sulfur can be used to propel a model rocket. This reaction makes zinc sulfide, heat, light, and gases.[26] Zinc sheet metal is used to make zinc bars.[27]

As zinc compounds

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About 1/4 of zinc is used to make zinc compounds. Zinc oxide can be used for sunscreen or paint pigment. Zinc oxide also is a semiconductor.[28] Zinc chloride is used to preserve wood so it does not rot.[29] Some fungicides have zinc in them. Zinc sulfate is used in dyes and pigments. Zinc sulfide is used in fluorescent bulbs to convert the ultraviolet light to visible light.

In biology

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Humans need a little bit of zinc to help their body run well.[30] If they do not get enough zinc in their food, they can get a mineral deficiency. Almost two billion people have a zinc deficiency.[31] Zinc deficiency makes one more easily get infections. Some people say that when we get colds, we should take more zinc. Others say that zinc does not make a difference.[32] There are medicines that one can use when they have a cold.[33] People add tiny amounts of zinc compounds to vitamin pills and cereals to make sure that they get enough zinc. Most single-tablet vitamins have zinc in them.[34] Zinc is found in at least 100 enzymes.[35] It is the second most common transition metal other than iron. Zinc also is used by the brain. The human body contains 2 to 4 grams of zinc. A zinc enzyme helps remove carbon dioxide from blood. Whole wheat has much zinc in it.

Safety

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Large amounts of zinc metal are toxic. It can dissolve in stomach acid. When too much zinc is eaten, copper and iron levels go down in the body. Zinc compounds can be corrosive in the stomach.[36] Zinc compounds put in the nose can ruin the sense of smell.[37]

Zinc ions are very toxic to fish and many things that live in water.[38]

References

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  1. ↑ "Standard Atomic Weights: Zinc". CIAAW. 2007.
  2. ↑ Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN 0-8493-0464-4.
  3. ↑ Kondev, F. G.; Wang, M.; Huang, W. J.; Naimi, S.; Audi, G. (2021). "The NUBASE2020 evaluation of nuclear properties" (PDF). Chinese Physics C. 45 (3): 030001. doi:10.1088/1674-1137/abddae.
  4. ↑ Spelter, Encyclo, 1916, ISBN 0665822448, retrieved 2009-08-01
  5. ↑ Zinc Metal Properties, American Galvanizers Association, 2008, archived from the original on 2009-02-21, retrieved 2009-02-15
  6. ↑ Scoffern, John (1861), The Useful Metals and Their Alloys, Houlston and Wright, pp. 591–603, retrieved 2009-04-06
  7. ↑ Hinds, John Iredelle Dillard (1908), Inorganic Chemistry: With the Elements of Physical and Theoretical Chemistry (2nd ed.), New York: John Wiley & Sons, pp. 506–508
  8. ↑ Porter, Frank C. (1994), Corrosion Resistance of Zinc and Zinc Alloys, CRC Press, p. 121, ISBN 0824792130
  9. ↑ Holleman, Arnold F.; Wiberg, Egon; Wiberg, Nils (1985), "Zink", Lehrbuch der Anorganischen Chemie (in German) (91–100 ed.), Walter de Gruyter, pp. 1034–1041, ISBN 3110075113
  10. ↑ "Zinc--overview". chemistryexplained.com. Archived from the original on 2010-01-12. Retrieved 2010-11-07.
  11. ↑ Brady, James E.; Humiston, Gerard E.; Heikkinen, Henry (1983), General Chemistry: Principles and Structure (3rd ed.), John Wiley & Sons, p. 671, ISBN 047186739X
  12. ↑ Alejandro A. Sonzogni (Database Manager), ed. (2008), Chart of Nuclides, Upton (NY): National Nuclear Data Center, Brookhaven National Laboratory, archived from the original on 2018-10-10, retrieved 2008-09-13
  13. ↑ CRC 2006, p. 11-70
  14. ↑ Five-Year Wilkinson Microwave Anisotropy Probe (WMAP) Observations: Data Processing, Sky Maps, and Basic Results (PDF), NASA, archived from the original (PDF) on 2015-04-10, retrieved 2008-03-06
  15. ↑ 15.0 15.1 Porter, Frank C. (1991), Zinc Handbook, CRC Press, ISBN 9780824783402
  16. ↑ Gupta, C. K.; Mukherjee, T. K. (1990), Hydrometallurgy in Extraction Processes, CRC Press, p. 62, ISBN 0849368049
  17. ↑ Special High Grade Zinc (SHG) 99.995% (PDF), Nyrstar, 2008, retrieved 2008-12-01
  18. ↑ Bodsworth, Colin (1994), The Extraction and Refining of Metals, CRC Press, p. 148, ISBN 0849344336
  19. ↑ 19.0 19.1 "Zinc: World Mine Production (zinc content of concentrate) by Country" (PDF), 2006 Minerals Yearbook: Zinc, Washington, D.C.: United States Geological Survey, p. Table 15, February 2008, retrieved 2009-01-19
  20. ↑ Besenhard, Jürgen O. (1999), Handbook of Battery Materials (PDF), Wiley-VCH, Bibcode:1999hbm..book.....B, ISBN 3527294694, retrieved 2008-10-08
  21. ↑ Wiaux, J. -P.; Waefler, J. -P. (1995), "Recycling zinc batteries: an economical challenge in consumer waste management", Journal of Power Sources, 57 (1–2): 61, Bibcode:1995JPS....57...61W, doi:10.1016/0378-7753(95)02242-2
  22. ↑ Panagapko, Doug (2006), Zinc, Natural Resources Canada, archived from the original on 2009-02-06, retrieved 2008-12-12
  23. ↑ Bounoughaz, M. (2003), "A comparative study of the electrochemical behaviour of Algerian zinc and a zinc from a commercial sacrificial anode", Journal of Materials Science, 38 (6), Salhi, E.; Benzine, K.; Ghali E.; Dalard F.: 1139, doi:10.1023/A:1022824813564, S2CID 135744939
  24. ↑ Bush, Douglas Earl; Kassel, Richard (2006), The Organ: An Encyclopedia, Routledge, p. 679, ISBN 9780415941747
  25. ↑ Coin Specifications, United States Mint, archived from the original on 2015-02-18, retrieved 2008-10-08
  26. ↑ Boudreaux, Kevin A, Zinc + Sulfur, Angelo State University, archived from the original on 2008-12-02, retrieved 2008-10-08
  27. ↑ Technical Information, Zinc Counters, 2008, archived from the original on 2008-11-21, retrieved 2008-11-29
  28. ↑ Zhang, Xiaoge Gregory (1996), Corrosion and Electrochemistry of Zinc, Springer, p. 93, ISBN 0306453347
  29. ↑ Blew, Joseph Oscar (1953), Wood preservatives, Department of Agriculture, Forest Service, Forest Products Laboratory, hdl:1957/816
  30. ↑ Prasad A. S. (2008), "Zinc in human health: effect of zinc on immune cells", Mol. Med., 14 (5–6): 353–357, doi:10.2119/2008-00033.Prasad, PMC 2277319, PMID 18385818
  31. ↑ Prasad, A. S. (2003), "Zinc deficiency", British Medical Journal, 326 (7386): 409–410, doi:10.1136/bmj.326.7386.409, PMC 1125304, PMID 12595353
  32. ↑ "Zinc and Health : The Common Cold". Office of Dietary Supplements, National Institutes of Health. Retrieved 2010-05-01.
  33. ↑ Ananda S., Prasad (2000), "Duration of Symptoms and Plasma Cytokine Levels in Patients with the Common Cold Treated with Zinc Acetate: A Randomized, Double-Blind, Placebo-Controlled Trial" (PDF), Annals of Internal Medicine, 133 (4), Fitzgerald, James T.; Bao, Bin; Beck, Frances W.J.; Chandrasekar, Pranatharthi H.: 245–252, doi:10.7326/0003-4819-133-4-200008150-00006, PMID 10929163, S2CID 2532146
  34. ↑ DiSilvestro, Robert A. (2004), Handbook of Minerals as Nutritional Supplements, CRC Press, pp. 135, 155, ISBN 0849316529
  35. ↑ Cotton 1999, pp. 625–629
  36. ↑ Bothwell, Dawn N. (2003), "Chronic Ingestion of a Zinc-Based Penny", Pediatrics, 111 (3), Mair, Eric A.; Cable, Benjamin B.: 689–691, doi:10.1542/peds.111.3.689, PMID 12612262
  37. ↑ "FDA says Zicam nasal products harm sense of smell". Los Angeles Times. 17 June 2009. Retrieved 17 June 2009.
  38. ↑ Eisler, Ronald (1993), "Zinc Hazard to Fish, Wildlife, and Invertebrates: A Synoptic Review" (PDF), Contaminant Hazard Reviews (10), Laurel, Maryland: U.S. Department of the Interior, Fish and Wildlife Service
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