Jump to content

Zinc oxide: Difference between revisions

From Wikipedia, the free encyclopedia
Browse history interactively
← Previous editNext edit →
Content deleted Content added
VisualWikitext
→Applications: clarify; otherwise it must be redundant
Line 157: Line 157:
available is the use of ZnO as the front contact for solar cells or of [[liquid crystal display]]s.<ref>B.-Y. Oh et al. "Transparent conductive Al-doped ZnO films for liquid crystal displays" [http://link.aip.org/link/?JAPIAU/99/124505/1 J. Appl. Phys. 99 (2006) 124505]</ref>
available is the use of ZnO as the front contact for solar cells or of [[liquid crystal display]]s.<ref>B.-Y. Oh et al. "Transparent conductive Al-doped ZnO films for liquid crystal displays" [http://link.aip.org/link/?JAPIAU/99/124505/1 J. Appl. Phys. 99 (2006) 124505]</ref>


Another application is ZnO:Al coating for energy-saving or heat-protecting windows. The coating lets the visible part of the spectrum in but either reflects the IR back into the room (energy saving) or does not let the IR radiation into the room (heat protection), depending on which side of the window has the coating.<ref name="k1"/>
Another application is ZnO:Al coating for energy-saving or heat-protecting windows. The coating lets the visible part of the spectrum in but either reflects the infrared (IR) radiation back into the room (energy saving) or does not let the IR radiation into the room (heat protection), depending on which side of the window has the coating.<ref name="k1"/>


==Potential applications==
==Potential applications==

Revision as of 22:23, 25 January 2009

Zinc oxide
Names
Other names
Zinc white
Calamine
Identifiers
ECHA InfoCard 100.013.839 Edit this at Wikidata
EC Number
  • 215-222-5
RTECS number
  • ZH4810000
Properties
ZnO
Molar mass 81.41 g/mol
Appearance White solid
Density 5.606 g/cm3
Melting point 1975 °C (decomposes)
1.6 g/L at 28°C
Thermochemistry
43.9 J K−1 mol−1
−348.0 kJ/mol
Related compounds
Other anions
 Zinc sulfide
Zinc selenide
Zinc telluride
Other cations
 Cadmium oxide
Mercury(II) oxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Zinc oxide is an inorganic compound with the formula ZnO. It usually appears as a white powder, nearly insoluble in water. The powder is widely used as an additive into numerous materials and products including plastics, ceramics, glass, cement, rubber (e.g. car tyres), lubricants,[1] paints, ointments, adhesives, sealants, pigments, foods (source of Zn nutrient), batteries, ferrites, fire retardants, etc. ZnO is present in the Earth crust as a mineral zincite; however, most ZnO used commercially is produced synthetically.

In materials science, ZnO is often called a II-VI semiconductor because zinc and oxygen belong to the 2nd and 6th groups of the periodic table, respectively. This semiconductor has several favorable properties: good transparency, high electron mobility, wide bandgap, strong room-temperature luminescence, etc. Those properties are already used in emerging applications for transparent electrodes in liquid crystal displays and in energy-saving or heat-protecting windows, and electronic applications of ZnO as thin-film transistor and light-emitting diode are forthcoming as of 2009.

Chemical properties

ZnO occurs as white powder commonly known as zinc white or as the mineral zincite. The mineral usually contains a certain amount of manganese and other elements and is of yellow to red color.[2] Crystalline zinc oxide is thermochromic, changing from white to yellow when heated.

Zinc oxide is an amphoteric oxide. It is nearly insoluble in water and alcohol, but it is soluble in (degraded by) most acids, such as hydrochloric acid:[3][4]

ZnO + 2 HCl → ZnCl2 + H2O

Bases also degrade the solid to give soluble zincates:

ZnO + 2NaOH + H2O → Na2(Zn(OH)4)

ZnO reacts slowly with fatty acids in oils to produce the corresponding carboxylates, such as oleate or stearate. ZnO forms cement-like products when mixed with a strong solution of zinc chloride or with phosphoric acid, owing to formation of oxysalts.

ZnO decomposes into zinc vapor and oxygen only at around 1975 °C, reflecting its considerable stability. Heating with carbon converts the oxide into zinc vapor:[5]

ZnO + C → Zn + CO

Zinc oxide reacts violently with aluminum and magnesium powders, with chlorinated rubber and linseed oil on heating causing fire and explosion hazard.[6][7]

It reacts with hydrogen sulfide to give the sulfide: this reaction is used commercially in removing H2S using ZnO powder (e.g., as deodorant).

ZnO + H2S → ZnS + H2O

When ointments containing ZnO and water are melted and exposed to ultraviolet light, hydrogen peroxide is produced.[4]

Physical properties

Unit cell of wurtzite zinc oxide.
Wurtzite structure
A zincblende unit cell

Crystal structure

Zinc oxide crystallizes in three forms: hexagonal wurtzite, cubic zincblende, and the rarely observed cubic rocksalt). The wurtzite structure is most stable and thus most common at ambient conditions. The zincblende form can be stabilized by growing ZnO on substrates with cubic lattice structure. In both cases, the zinc and oxide are tetrahedral. The rocksalt NaCl-type structure is only observed at relatively high pressures - ~10 GPa.[8]

None of these three ZnO structures possesses inversion symmetry (reflection of a crystal relatively any given point does not transform it into itself). This important property results in piezoelectricity, pyroelectricity and spontaneous polarization of ZnO.

The hexagonal structure has a point group 6mm (Hermann-Mauguin notation) or C6v (Schoenflies notation), and the space group is P63mc or C6v4. The lattice constants are a = 3.25 Å and c = 5.2 Å; their ratio c/a ~ 1.60 is close to the ideal value for hexagonal cell c/a = 1.633.[9] As in most II-VI materials, the bonding in ZnO is largely ionic, which explains its strong piezoelectricity. Due to this ionicity, zinc and oxygen planes bear electric charge (positive and negative, respectively). Therefore, to maintain electrical neutrality, those planes reconstruct at atomic level in most relative materials, but not in ZnO - its surfaces are atomically flat, stable and exhibit no reconstruction. This anomaly of ZnO is not fully explained yet.[10]

Mechanical properties

ZnO is a relatively soft material with approximate hardness of 4.5 on the Mohs scale.[1] Its elastic constants are smaller than those of relevant III-V semiconductors, such as GaN.

Among the tetrahedrally bonded semiconductors, it has been stated that ZnO has the highest piezoelectric tensor or at least one comparable to that of GaN and AlN.[11] This property makes it a technologically important material for many piezoelectrical applications, which require a large electromechanical coupling.

Electronic properties

ZnO has a relatively large direct band gap of ~3.3 eV at room temperature;[8] therefore, pure ZnO is colorless and transparent. Advantages associated with a large band gap include higher breakdown voltages, ability to sustain large electric fields, lower electronic noise, and high-temperature and high-power operation. The bandgap of ZnO can further be tuned from ~3–4 eV by its alloying with magnesium oxide or cadmium oxide.[8]

Most ZnO has n-type character, even in the absence of intentional doping. Native defects such as oxygen vacancies or zinc interstitials are often assumed to be the origin of this, but the subject remains controversial.[12] An alternative explanation has been proposed, based on theoretical calculations, that unintentional substitutional hydrogen impurities are responsible.[13] Controllable n-type doping is easily achieved by substituting Zn with group-III elements Al, Ga, In or by substituting oxygen with group-VII elements chlorine or iodine.[14]

Reliable p-type doping of ZnO remains difficult. This problem originates from low solubility of p-type dopants and their compensation by abundant n-type impurities, and it is pertinent not only to ZnO, but also to similar compounds GaN and ZnSe. Measurement of p-type in "intrinsically" n-type material is also not easy because inhomogeneity results in spurious signals.[15]

Current absence of p-type ZnO does limit its electronic and optoelectronic applications which usually require junctions of n-type and p-type material. Known p-type dopants include group-I elements Li, Na, K; group-V elements N, P and As; as well as copper and silver. However, many of these form deep acceptors and do not produce significant p-type conduction at room temperature.[8]

Electron mobility of ZnO strongly varies with temperature and has a maximum of ~2000 cm2/(V*s) at ~80 degrees Kelvin.[16]. Data on hole mobility are scarce with values in the range 5-30 cm2/(V*s).[17]

Production

See also: Zinc smelting

For industrial use, ZnO is produced at levels of 105 tons per year[2] by three main processes.

French process

Metallic zinc is melted in a graphite crucible and vaporized above 907 °C. Zinc vapor instantaneously reacts with the oxygen in the air to give ZnO, accompanied by a drop in its temperature and bright luminescence. Zinc oxide particles are transported into a cooling duct and collected in a bag house. This indirect method is commonly known as the French process (FP) which was popularized by LeClaire (France) in 1844. In a typical FP, zinc oxide normally consists of agglomerated zinc oxide particles with an average size of 0.1 micrometres to a few micrometres. By weight, most of the world's zinc oxide is manufactured via French process. Major applications involve industries related to rubber, varistors, sunscreens, paints, healthcare, and poultry nutrients. Recent developments involve acicular nanostructures (rods, wires, tripods, tetrapods, plates) synthesized using a modified French process known as catalyst-free combust-oxidized mesh (CFCOM) process. Acicular nanostructures usually have micrometre-length nanorods with nanometric diameters (below 100 nm).[18]

Direct method

The so-called direct method is related to the French process. In this process, zinc ores or roasted sulfide concentrates are mixed with coal. In a reduction furnace, ore is reduced to metallic zinc and the vaporized zinc is allowed to react with oxygen to form zinc oxide.[citation needed]

American process

In this process ore of zinc (zinc ash) is dissolved (as ZnCl2) and precipitated with alkali. Zinc oxide made from this process is known as "Active Zinc Oxide".[citation needed]

Laboratory synthesis

A large number of ZnO production methods exist for producing ZnO for scientific studies and electronic applications. These methods can be classified by the resulting ZnO form (bulk, thin film, nanowire), temperature ("low", i.e. close to room temperature or "high", i.e. T ~ 1000 0C), process type (vapor deposition or growth from solution) and other parameters.

Large single crystals (many cubic centimeters) are usually grown by the gas transport (vapor-phase deposition), hydrothermal synthesis, or melt growth. However, because of high vapor pressure of ZnO, growth from the melt is problematic. Growth by gas transport is difficult to control, leaving the hydrothermal method as a preference. Thin films can be produced by chemical vapor deposition, metalorganic vapour phase epitaxy, electrodeposition, pulsed laser deposition, sputtering, sol-gel synthesis, spray pyrolysis, etc. Nanostructures can be obtained with most above-mentioned techniques, at certain conditions, and also with the vapor-liquid-solid method.[citation needed]

Applications

The applications of zinc oxide powder are numerous, and the principal ones are summarized below. Most applications exploit the reactivity of the oxide as a precursor to other zinc compounds. For material science applications, zinc oxide has high refractive index, good thermal, binding, antibacterial and UV-protection properties. Consequently, it is added into various materials and products, including plastics, ceramics, glass, cement, rubber, lubricants,[1] paints, ointments, adhesive, sealants, pigments, foods, batteries, ferrites, fire retardants, etc.[19]

Rubber manufacture

Zinc oxide and stearic acid are ingredients in the commercial manufacture of rubber goods. A mixture of these two compounds allows a quicker and more controllable rubber cure. ZnO is also an important additive to the rubber of car tyres. Vulcanization catalysts are derived from zinc oxide, and it considerably improves the thermal conductivity, which is crucial to dissipate the heat produced by the deformation when the tyre rolls.[20] ZnO additive also protect rubber from fungi (see medical applications) and UV light.

Concrete industry

Zinc oxide is widely used for concrete manufacturing. Addition of ZnO improves the processing time and the resistance of concrete against water.[20]

Medical

Zinc oxide as a mixture with about 0.5% iron(III) oxide (Fe2O3) is called calamine and is used in calamine lotion. There are also two minerals, zincite and hemimorphite, which have been called calamine historically (see: calamine (mineral)). When mixed with eugenol, the mixture is called zinc oxide eugenol and has restorative and prosthodontic applications in dentistry.

Reflecting the basic properties of ZnO, fine particles of the oxide have deodorizing and antibacterial[21] action and for that reason are added into various materials including cotton fabric, rubber, food packaging, etc.[22][23] Enhanced antibacterial action of fine particles compared to bulk material is not intrinsic to ZnO and is observed for other materials, such as silver.[24]

Cigarette filters

Zinc oxide is a constituent of cigarette filters for removal of selected components from tobacco smoke. A filter consisting of charcoal impregnated with zinc oxide and iron oxide removes significant amounts of HCN and H2S from tobacco smoke without affecting its flavour.[19]

Food additive

Zinc oxide is added to many food products, e.g., breakfast cereals, as a source of zinc,[25] a necessary nutrient. (Other cereals may contain zinc sulfate for the same purpose.) Some prepackaged foods also include trace amounts of ZnO even if it is not intended as a nutrient.

Pigment

Zinc white is used as a pigment[26] in paints and is more opaque than lithopone, but less opaque than titanium dioxide. It is also used in coatings for paper. Chinese white is a special grade of zinc white used in artists' pigments. Because it absorbs both UVA and UVB rays of ultraviolet light, zinc oxide can be used in ointments, creams, and lotions to protect against sunburn and other damage to the skin caused by ultraviolet light (see sunscreen). It is the broadest spectrum UVA and UVB absorber that is approved for use as a sunscreen by the FDA, and is completely photostable. It is also a main ingredient of mineral makeup.

Coatings

Paints containing zinc oxide powder have long been utilized as anticorrosive coatings for various metals. They are especially effective for galvanised Iron. The latter is difficult to protect because its reactivity with organic coatings leads to brittleness and lack of adhesion. Zinc oxide paints however, retain their flexibility and adherence on such surfaces for many years.[19]

ZnO highly n-type doped with Al, Ga or nitrogen is transparent and conductive (transparency ~90%, lowest resistivity ~10-4 Ωcm[27]), and is used as a transparent electrode. The constituents Zn and Al are much cheaper and less poisonous compared to the generally used indium tin oxide (ITO). One application which has begun to be commercially available is the use of ZnO as the front contact for solar cells or of liquid crystal displays.[28]

Another application is ZnO:Al coating for energy-saving or heat-protecting windows. The coating lets the visible part of the spectrum in but either reflects the infrared (IR) radiation back into the room (energy saving) or does not let the IR radiation into the room (heat protection), depending on which side of the window has the coating.[2]

Potential applications

Electronics

ZnO has wide direct band gap (3.37 eV or 375 nm at room temperature). Therefore, its most common potential applications are in laser diodes and light emitting diodes (LEDs). Some optoelectronic applications of ZnO overlap with that of GaN, which has a similar bandgap (~3.4 eV at room temperature). Compared to GaN, ZnO has a larger exciton binding energy (~60 meV, 2.4 times of the room-temperature thermal energy), which results in bright roo-temperature emission from ZnO. Other favorable for electronic applications properties of ZnO include its stability to high-energy radiation and to wet chemical etching.[29] Radiation resistance[30] makes ZnO a suitable candidate for space applications.

The pointed tips of ZnO nanorods result in a strong enhancement of an electric field. Therefore, they can be used as field emitters.[31]

Transparent thin-film transistors (TTFT) can be produced with ZnO. As field-effect transistors, they even may not need a p–n junction [32], thus avoiding the p-type doping problem of ZnO. Some of the field-effect transistors even use ZnO nanorods as conducting channels.[33]

Zinc oxide nanorod sensor

Zinc oxide nanorod sensors or ZnO nanorod sensors are devices detecting changes in electrical current passing through zinc oxide nanowires due to adsorption of gas (e.g., hydrogen) molecules. Selectivity to hydrogen gas was achieved by sputtering Pd clusters on the nanorod surface. The addition of Pd appears to be effective in the catalytic dissociation of hydrogen molecules into atomic hydrogen, increasing the sensitivity of the sensor device. The sensor detects hydrogen concentrations down to 10 parts per million at room temperature, whereas there is no response to oxygen.[34][35].

Spintronics

ZnO has also been considered for spintronics applications: if doped with 1-10% of magnetic ions (Mn, Fe, Co, V, etc.), ZnO could become ferromagnetic, even at room temperature. Such room temperature ferromagnetism in ZnO:Mn has been observed[36], but it is not clear yet whether it originates from the matrix itself or from Mn-containing precipitates.

Piezoelectricity

The piezoelectricity in textile fibers coated in ZnO have been shown capable of "self-powering nanosystems" with everyday mechanical stress generated by wind or body movements.[37][38]

In 2008 the Center for Nanostructure Characterization at the Georgia Institute of Technology reported producing an electricity generating device (called flexible charge pump generator) delivering alternating current by stretching and releasing zinc oxide wires. This mini-generator creates an oscillating voltage up to 45 millivolts, converting close to seven percent of the applied mechanical energy into electricity. Researchers used wires with lengths of 200-300 microns and diameters of three to five microns, but the device could be scaled down to nanometer size.[39]

Biosensor

ZnO has high biocompatibility and fast electron transfer kinetics. Such features advocate the use of this material as a biomimic membrane to immobilize and modify biomolecules.[40]

Safety

As a food additive, Zinc oxide is on FDA's generally recognized as safe, or GRAS, substances.[41]

Zinc oxide itself is non-toxic; however it is hazardous to breathe zinc oxide fumes. Fumes of zinc oxide are generated when zinc or zinc alloys are melted and oxidized at high temperature. This occurs while melting brass because the melting point of brass is close to the boiling point of zinc.[42] Exposure to zinc oxide in the air, which also occurs while welding galvanized (zinc plated) steel, can result in a nervous malady called metal fume fever.[43] For this reason, typically galvanized steel is not welded, or the zinc is removed first.

See also

References

  1. ^ a b c A. Hernández Battez et al. "CuO, ZrO2 and ZnO nanoparticles as antiwear additive in oil lubricants" Wear 265 (2008) 422
  2. ^ a b c C. Klingshirn "ZnO: Material, Physics and Applications" ChemPhysChem 8 (2007) 782
  3. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  4. ^ a b J. M. Spero, B. Devito, L. Theodore "Regulatory chemical handbook" CRC Press, 2000, ISBN 0824703901, 9780824703905
  5. ^ IPCS Intox databank entry for "Zinc oxide." Access date January 25, 2009.
  6. ^ International Occupational Safety and Health Information Centre (CIS)
  7. ^ Zinc oxide MSDS. Access date January 25, 2009.
  8. ^ a b c d U. Ozgur et al. "A comprehensive review of ZnO materials and devices" J. Appl. Phys. 98 (2005) 041301
  9. ^ Landolt-Bornstein, New Series, Group III, Vol. 17 B, 22, 41B (Ed.: U. Rossler), Springer, Heidelberg, 1999.
  10. ^ S. Baruah and J. Dutta "Hydrothermal growth of ZnO nanostructures" (18 pages) Sci. Technol. Adv. Mater. 10 (2009) 013001 free download
  11. ^ A. Dal Corso et al. "Ab initio study of piezoelectricity and spontaneous polarization in ZnO" Phys. Rev. B 50 (1994) 10715
  12. ^ Look, D.C. (1999). "Residual Native Shallow Donor in ZnO". Physical Review Letters. 82 (12): 2552. doi:10.1103/PhysRevLett.82.2552. {{cite journal}}: Unknown parameter |coauthors= ignored (|author= suggested) (help)
  13. ^ Janotti, A. (2007). "Hydrogen multicentre bonds". Nat Mater. 6 (1): 44. doi:10.1038/nmat1795. {{cite journal}}: Unknown parameter |coauthors= ignored (|author= suggested) (help)
  14. ^ H. Kato et al. "Growth and characterization of Ga-doped ZnO layers on a-plane sapphire substrates grown by molecular beam epitaxy" J. Cryst. Growth 237–239 (2002) 538
  15. ^ T. Ohgaki et al. "Positive Hall coefficients obtained from contact misplacement on evident n-type ZnO films and crystals" J. Mat. Res. 23(9) (2008) 2293
  16. ^ P. Wagner, R. Helbig "Halleffekt und anisotropie der beweglichkeit der elektronen in ZnO" J. Phys. Chem. Solid 35 (1974) 327
  17. ^ Y. R. Ryu et al. "Properties of arsenic-doped p-type ZnO grown by hybrid beam deposition" Appl. Phys. Lett. 83 (2003) 87
  18. ^ S. Mahmud et al. "Nanostructure of ZnO fabricated via French Process and its correlation to electrical properties of semiconducting varistors" J. Syn. React. Inorg. Met-org. and Nano-metal Chem. 36 (2006) 155
  19. ^ a b c Nav Bharat Metallic Oxide Industries Pvt. Limited. Applications of ZnO. Access date January 25, 2009.>
  20. ^ a b H. E. Brown, Zinc Oxide Rediscovered, The New Jersey Zinc Company, New York, 1957; and Zinc Oxide Properties and Applications, Pergamon, New York, 1976.
  21. ^ N. Padmavathy et al. "Enhanced bioactivity of ZnO nanoparticles—an antimicrobial study" Sci. Technol. Adv. Mater. 9 (2007) 035004 free download
  22. ^ Q. Li "Durability of nano ZnO antibacterial cotton fabric to sweat" J. Appl. Polymer Sci. 103 (2006) 41
  23. ^ M. Saito "Antibacterial, Deodorizing, and UV Absorbing Materials Obtained with Zinc Oxide (ZnO) Coated Fabrics" J. Industrial Textiles 23 (1993) 150
  24. ^ O. Akhavan and E. Ghaderi "Enhancement of antibacterial properties of Ag nanorods by electric field" Sci. Technol. Adv. Mater. 10 (2009) 015003 free download
  25. ^ Quaker cereals content
  26. ^ Zinc Oxide as a pigment
  27. ^ L. Schmidt-Mende and J. L. MacManus-Driscoll "ZnO – nanostructures, defects, and devices" Materials Today 10 (2007) 40
  28. ^ B.-Y. Oh et al. "Transparent conductive Al-doped ZnO films for liquid crystal displays" J. Appl. Phys. 99 (2006) 124505
  29. ^ D. C. Look "Recent advances in ZnO materials and devices" Mater. Sci. Eng., B 80 (2001) 383
  30. ^ S. O. Kucheyev et al. "Ion-beam-produced structural defects in ZnO" Phys. Rev. B 67 (2003) 094115
  31. ^ Y. B. Li et al. "ZnO nanoneedles with tip surface perturbations: Excellent field emitters" Appl. Phys. Lett. 84 (2004) 3603
  32. ^ K. Nomura et al. "Thin-Film Transistor Fabricated in Single-Crystalline Transparent Oxide Semiconductor" Science 300 (2003) 1269
  33. ^ Y. W. Heo et al. "Depletion-mode ZnO nanowire field-effect transistor" Appl. Phys. Lett. 85 (2004) 2274
  34. ^ H. T. Wang et al. "Hydrogen-selective sensing at room temperature with ZnO nanorods" Appl. Phys. Lett. 86 (2005) 243503
  35. ^ L. C. Tien et al. "Hydrogen sensing at room temperature with Pt-coated ZnO thin films and nanorods" Appl. Phys. Lett. 87 (2005) 222106
  36. ^ A. C. Mofor et al. "Magnetic property investigations on Mn-doped ZnO Layers on sapphire" Appl. Phys. Lett. 87 (2005) 62501
  37. ^ Keim, Brandon (February 13, 2008). "Piezoelectric Nanowires Turn Fabric Into Power Source". Wired News. CondéNet. {{cite news}}: Check date values in: |date= (help)
  38. ^ Yong Qin, Xudong Wang & Zhong Lin Wang (February 14, 2008). "Editor's summary: Nanomaterial: power dresser". Nature. 451. Nature Publishing Group: 809–813. doi:10.1038/nature06601. {{cite journal}}: Check date values in: |date= (help); More than one of |work= and |journal= specified (help)
  39. ^ Science Daily "New Small-scale Generator Produces Alternating Current By Stretching Zinc Oxide Wires". November 10, 2008. {{cite web}}: Check |url= value (help)
  40. ^ Kumar, S. Ashok (2008-01). "Nanostructured Zinc Oxide Particles in Chemically Modified Electrodes for Biosensor Applications". Analytical Letters. 41 (2): 141–58. doi:10.1080/00032710701792612. {{cite journal}}: Check date values in: |date= (help); Unknown parameter |coauthors= ignored (|author= suggested) (help)
  41. ^ "Database of Select Committee on GRAS Substances (SCOGS) Reviews".
  42. ^ The Safety of Zinc Casting
  43. ^ Zinc and Cadmium

Reviews

Retrieved from "https://en.wikipedia.org/w/index.php?title=Zinc_oxide&oldid=266400121"