|Other names|| Zinc white|
|Molar mass||81.408 g/mol|
1975 °C (decomposes)
|Solubility in water||0.16 mg/100 mL (30 °C)|
|Band gap||3.3 eV (direct)|
|Refractive index (nD)||2.0041|
| Std enthalpy of|
| Standard molar|
|EU classification||Dangerous for the environment (N)|
|Flash point||1436 °C|
|Other anions|| Zinc sulfide|
|Other cations|| Cadmium oxide|
| Plantilla:Cross(what is this?) |
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Zinc oxide is an inorganic compound with the formula ZnO. It is a white powder that is 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 tires), lubricants, paints, ointments, adhesives, sealants, pigments, foods (source of Zn nutrient), batteries, ferrites, fire retardants, first aid tapes, etc. ZnO is present in the Earth's crust as the mineral zincite, however, most ZnO used commercially is synthetic.
In materials science, ZnO is a wide-bandgap semiconductor of the II-VI semiconductor group (since zinc and oxygen belong to the 2nd and 6th groups of the periodic table, respectively). The native doping of the semiconductor (due to oxygen vacancies) is n-type. 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 transistors and light-emitting diodes are forthcoming as of 2009.
Chemical propertiesEditar sección
ZnO occurs as white powder known as zinc white or as the mineral zincite. The mineral usually contains a certain amount of manganese and other elements that confer yellow to red color. Crystalline zinc oxide is thermochromic, changing from white to yellow when heated and in air reverting to white on cooling. This color change is caused by a very small loss of oxygen at high temperatures to form the non-stoichiometric Zn1+xO, where at 800 °C, x = 0.00007.
- ZnO + 2 HCl → ZnCl2 + H2O
Bases also degrade the solid to give soluble zincates:
- ZnO + 2 NaOH + 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 aqueous solution of zinc chloride and these are best described as zinc hydroxy chlorides. This cement was used in dentistry.
ZnO also forms cement-like products when treated with phosphoric acid; related materials are used in dentistry. A major component of zinc phosphate cement produced by this reaction is hopeite, Zn3(PO4)2·4H2O.
ZnO decomposes into zinc vapor and oxygen only at around 1975 °C, reflecting its considerable stability. Heating with carbon converts the oxide into the metal, which is more volatile than the oxide.
- ZnO + C → Zn + CO
- ZnO + H2S → ZnS + H2O
Physical propertiesEditar sección
Zinc oxide crystallizes in two main forms, hexagonal wurtzite and cubic zincblende. The wurtzite structure is most stable at ambient conditions and thus most common. The zincblende form can be stabilized by growing ZnO on substrates with cubic lattice structure. In both cases, the zinc and oxide centers are tetrahedral, the most characteristic geometry for Zn(II).
Hexagonal and zincblende polymorphs have no inversion symmetry (reflection of a crystal relative to any given point does not transform it into itself). This and other lattice symmetry properties result in piezoelectricity of the hexagonal and zincblende ZnO, and pyroelectricity of hexagonal ZnO.
The hexagonal structure has a point group 6 mm (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. As in most group II-VI materials, the bonding in ZnO is largely ionic (Zn2+–O2–) with the corresponding radii of 0.074 nm for Zn2+ and 0.140 nm for O2–. This property accounts for the preferential formation of wurtzite rather than zinc blende structure, as well as the strong piezoelectricity of ZnO. Because of the polar Zn-O bonds, zinc and oxygen planes are electrically charged. 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.
Mechanical propertiesEditar sección
ZnO is a relatively soft material with approximate hardness of 4.5 on the Mohs scale. Its elastic constants are smaller than those of relevant III-V semiconductors, such as GaN. The high heat capacity and heat conductivity, low thermal expansion and high melting temperature of ZnO are beneficial for ceramics. ZnO's most stable phase being wurtzite, ZnO exhibits a very long lived optical phonon E2(low) with a lifetime as high as 133 ps at 10 K 
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. This property makes it a technologically important material for many piezoelectrical applications, which require a large electromechanical coupling.
Electrical propertiesEditar sección
ZnO has a relatively large direct band gap of ~3.3 eV at room temperature. 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 to ~3–4 eV by its alloying with magnesium oxide or cadmium oxide.
Most ZnO has n-type character, even in the absence of intentional doping. Nonstoichiometry is typically the origin of n-type character, but the subject remains controversial. An alternative explanation has been proposed, based on theoretical calculations, that unintentional substitutional hydrogen impurities are responsible. Controllable n-type doping is easily achieved by substituting Zn with group-III elements such as Al, Ga, In or by substituting oxygen with group-VII elements chlorine or iodine.
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. This problem is observed with GaN and ZnSe. Measurement of p-type in "intrinsically" n-type material is complicated by the inhomogeneity of samples.
Current limitations to p-doping does not limit electronic and optoelectronic applications of ZnO, 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.
Indirect (French) processEditar sección
Metallic zinc is melted in a graphite crucible and vaporized at temperatures above 907 °C (typically around 1000 °C). Zinc vapor 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 was popularized by LeClaire (France) in 1844 and therefore is commonly known as the French process. Its product normally consists of agglomerated zinc oxide particles with an average size of 0.1 to a few micrometers. By weight, most of the world's zinc oxide is manufactured via French process.
Direct (American) processEditar sección
The direct process starts with diverse contaminated zinc composites, such as zinc ores or smelter by-products. The zinc precursors are reduced (carbothermal reduction) by heating with a source of carbon such as anthracite to produce zinc vapor, which is then oxidized as in the indirect process. Because of the lower purity of the source material, the final product is also of lower quality in the direct process as compared to the indirect one.
Wet chemical processEditar sección
A small amount of industrial production involves wet chemical processes, which start with aqueous solutions of purified zinc salts, from which zinc carbonate or zinc hydroxide is precipitated. The precipitate is then filtered, washed, dried and calcined at temperatures around 800 °C.
Laboratory synthesisEditar sección
A large number of specialised methods exist for producing ZnO for scientific studies and niche applications. These methods can be classified by the resulting ZnO form (bulk, thin film, nanowire), temperature ("low", that is close to room temperature or "high", that is T ~ 1000 °C), 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, atomic layer deposition, spray pyrolysis, etc.
Ordinary white powdered zinc oxide can be produced in the laboratory by electrolyzing a solution of sodium bicarbonate with a zinc anode. Zinc hydroxide and hydrogen gas are produced. The zinc hydroxide upon heating decomposes to zinc oxide.
- Zn + 2 H2O → Zn(OH)2 + H2
- Zn(OH)2 → ZnO + H2O
Nanophase ZnOEditar sección
Nanophase ZnO can be synthesized into a variety of morphologies including nanowires, nanorods, tetrapods, nanobelts, nanoflowers, nanoparticles etc. Nanostructures can be obtained with most above-mentioned techniques, at certain conditions, and also with the vapor-liquid-solid method.
Rodlike nanostructures of ZnO can be produced via aqueous methods. They are attractive because of relatively low synthesis temperatures (<300 °C) and absence of complex vacuum setup. The synthesis is typically carried out at temperatures of about 90 °C, in an equimolar aqueous solution of zinc nitrate and hexamine, the latter providing the basic environment. Certain additives, such as polyethylene glycol or polyethylenimine, can improve the aspect ratio of the ZnO nanowires. Doping of the ZnO nanowires has been achieved by adding other metal nitrates to the growth solution. The morphology of the resulting nanostructures can be tuned by changing the parameters relating to the precursor composition (such as the zinc concentration and pH) or to the thermal treatment (such as the temperature and heating rate).
Aligned ZnO nanowires on pre-seeded silicon, glass and gallium nitride substrates have been grown in aqueous solutions using aqueous zinc salts such as Zinc nitrate and Zinc acetate in basic environments. Pre-seeding substrates with ZnO creates sites for homogeneous nucleation of ZnO crystal during the synthesis. Common pre-seeding methods include in-situ thermal decomposition of zinc acetate crystallites, spincoating of ZnO nanoparticles and the use of various physical vapor deposition methods to deposit ZnO thin films. Pre-seeding can be performed in conjunction with top down patterning methods such as electron beam lithography and nanosphere lithography to designate nucleation sites prior to growth. Aligned ZnO nanowires can be used in dye-sensitized solar cells and field emission devices.
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, high thermal conductivity, binding, antibacterial and UV-protection properties. Consequently, it is added into various materials and products, including plastics, ceramics, glass, cement, rubber, lubricants, paints, ointments, adhesive, sealants, pigments, foods, batteries, ferrites, fire retardants, etc.
Rubber manufactureEditar sección
About 50% of ZnO use is in the rubber industry. Zinc oxide along with stearic acid is used in the vulcanization of rubber ZnO additive also protect rubber from fungi (see medical applications) and UV light.
Concrete industryEditar sección
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 historically called calamine. When mixed with eugenol, a ligand, zinc oxide eugenol is formed, which has applications as restorative and prosthodontic in dentistry.
Reflecting the basic properties of ZnO, fine particles of the oxide have deodorizing and antibacterial action and for that reason are added into various materials including cotton fabric, rubber, food packaging, etc. Enhanced antibacterial action of fine particles compared to bulk material is not intrinsic to ZnO and is observed for other materials, such as silver.
Zinc oxide is widely used to treat a variety of other skin conditions, in products such as baby powder and barrier creams to treat diaper rashes, calamine cream, anti-dandruff shampoos, and antiseptic ointments. It is also a component in tape (called "zinc oxide tape") used by athletes as a bandage to prevent soft tissue damage during workouts.
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 reflector that is approved for use as a sunscreen by the FDA, and is completely photostable. When used as an ingredient in sunscreen, zinc oxide sits on the skin’s surface i.e. is not absorbed into the skin, and blocks both UVA (320–400 nm) and UVB (280–320 nm) rays of ultraviolet light. Because zinc oxide (and the other most common physical sunscreen, titanium dioxide) are not absorbed into the skin, they are nonirritating and nonallergenic.
Many sunscreens use nano-sized zinc oxide (along with nano titanium dioxide) because such small particles do not scatter light and therefore do not appear white. Although there has been concern that they might be absorbed into the skin, comprehensive reviews of the medical literature have not uncovered any risk.
Cigarette filtersEditar sección
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 flavor.
Food additiveEditar sección
Zinc oxide is added to many food products, e.g., breakfast cereals, as a source of zinc, 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.
Zinc white is used as a pigment 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. It is also a main ingredient of mineral makeup.
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.
ZnO highly n-type doped with Al, Ga or In is transparent and conductive (transparency ~90%, lowest resistivity ~10−4 Ω·cm). ZnO:Al coatings are being used 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.
Various plastics, such as polyethylene naphthalate (PEN), can be protected by applying zinc oxide coating. The coating reduces the diffusion of oxygen with PEN. Zinc oxide layers can also be used on polycarbonate (PC) in outdoor applications. The coating protects PC form solar radiation and decreases the oxidation rate and photo-yellowing of PC.
Corrosion prevention in nuclear reactorsEditar sección
- Main gallery: Depleted zinc oxide.
Zinc oxide depleted in the zinc isotope with the atomic mass 64 is used in corrosion prevention in nuclear pressurized water reactors. The depletion is necessary, because 64Zn is transformed into radioactive 65Zn under irradiation by the reactor neutrons.
Potential applicationsEditar sección
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 room-temperature emission from ZnO. ZnO can be combined with GaN for LED-applications. For instance as TCO layer and ZnO nanostructures provide better light outcoupling. Other properties of ZnO favorable for electronic applications include its stability to high-energy radiation and to wet chemical etching. Radiation resistance makes ZnO a suitable candidate for space applications. ZnO is currently the most promising candidate in the field of random lasers to produce an electronically pumped UV laser source.
Aluminium-doped ZnO layers are used as a transparent electrodes. 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.
Transparent thin-film transistors (TTFT) can be produced with ZnO. As field-effect transistors, they even may not need a p–n junction, thus avoiding the p-type doping problem of ZnO. Some of the field-effect transistors even use ZnO nanorods as conducting channels.
Zinc oxide nanorod sensorEditar sección
Zinc oxide nanorod sensors are devices detecting changes in electrical current passing through zinc oxide nanowires due to adsorption of gas 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.
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, but it is not clear yet whether it originates from the matrix itself or from secondary oxide phases.
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 nanowires. 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 0.2–0.3 mm and diameters of three to five micrometers, but the device could be scaled down to smaller size.
It is hardly possible to trace the first usage of zinc oxide – various zinc compounds were widely used by early humans, in various processed and unprocessed forms, as a paint or medicinal ointment, but their exact composition is uncertain.
The use of pushpanjan, probably zinc oxide, as a salve for eyes and open wounds, is mentioned in the Indian medical text the Charaka Samhita, thought to date from 500 BC or before. Zinc oxide ointment is also mentioned by the Greek physician Dioscorides (1st century AD.) Avicenna mentions zinc oxide in The Canon of Medicine (1025 AD), which mentioned it as a preferred treatment for a variety of skin conditions, including skin cancer. Though it is no longer used for treating skin cancer, it is still widely used to treat a variety of other skin conditions, in products such as baby powder and creams against diaper rashes, calamine cream, anti-dandruff shampoos, and antiseptic ointments.
The Romans produced considerable quantities of brass (an alloy of zinc and copper) as early as 200 BC by a cementation process where copper was reacted with zinc oxide. The zinc oxide is thought to have been produced by heating zinc ore in a shaft furnace. This liberated metallic zinc as a vapor, which then ascended the flue and condensed as the oxide. This process was described by Dioscorides in the 1st century AD. Zinc oxide has also been recovered from zinc mines at Zawar in India, dating from the second half of the first millennium BC. This was presumably also made in the same way and used to produce brass.
From the 12th to the 16th century zinc and zinc oxide were recognized and produced in India using a primitive form of the direct synthesis process. From India, zinc manufacture moved to China in the 17th century. In 1743, the first European zinc smelter was established in Bristol, United Kingdom.
The main usage of zinc oxide (zinc white) was again paints and additive to ointments. Zinc white was accepted as a watercolor by 1834 but it did not mix well with oil. This problem was quickly solved by optimizing the synthesis of ZnO. In 1845, LeClaire in Paris was producing the oil paint on a large scale, and by 1850, zinc white was being manufactured throughout Europe. The success of zinc white paint was due to its advantages over the traditional white lead: zinc white is essentially permanent in sunlight, it is not blackened by sulfur-bearing air, it is non-toxic and more economical. Because zinc white is so "clean" it is very valuable for making tints with other colors; however, it makes a rather brittle dry film when unmixed with other colors. For example, during the late 1890s and early 1900s, some artists used zinc white as a ground for their oil paintings. All those paintings developed cracks over the years.
In the recent times, most zinc oxide was used in the rubber industry (see applications above). In the 1970s, the second largest application of ZnO was photocopying. High-quality ZnO produced by the "French process" was added into the photocopying paper as a filler. This application was however soon displaced.
Zinc oxide itself is non-toxic; however it is hazardous to inhale zinc oxide fumes, as generated when zinc or zinc alloys are melted and oxidized at high temperature. This problem occurs while melting brass because the melting point of brass is close to the boiling point of zinc. 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. For this reason, typically galvanized steel is not welded, or the zinc is removed first.
In popular cultureEditar sección
Reflecting its many varied but relatively unobtrusive and unglamorous uses, zinc oxide was the theme of a spoof in The Kentucky Fried Movie as a short educational film Zinc Oxide and You.
See alsoEditar sección
- ↑ 1,0 1,1 1,2 Takahashi, Kiyoshi; Yoshikawa, Akihiko; Sandhu, Adarsh (2007). Wide bandgap semiconductors: fundamental properties and modern photonic and electronic devices. Springer. p. 357. ISBN 3540472347. http://books.google.com/?id=j_HEazhVxoMC&pg=PA357.
- ↑ 2,0 2,1 2,2 Hernandezbattez, A; Gonzalez, R; Viesca, J; Fernandez, J; Diazfernandez, J; MacHado, A; Chou, R; Riba, J (2008). "CuO, ZrO2 and ZnO nanoparticles as antiwear additive in oil lubricants". Wear 265 (3–4): 422. doi:10.1016/j.wear.2007.11.013.
- ↑ 3,0 3,1 3,2 Klingshirn, C (2007). "ZnO: Material, Physics and Applications". ChemPhysChem 8 (6): 782–803. doi:10.1002/cphc.200700002. PMID 17429819.
- ↑ 4,0 4,1 Wiberg, E. and Holleman, A. F. (2001). Inorganic Chemistry. Elsevier. ISBN 0123526515.
- ↑ Plantilla:Greenwood&Earnshaw2nd
- ↑ 6,0 6,1 Spero, J. M.; Devito, B.; Theodore, L. (2000). Regulatory chemical handbook. CRC Press. ISBN 0824703901.
- ↑ Nicholson, J. W; Nicholson, J. W (1998). "The chemistry of cements formed between zinc oxide and aqueous zinc chloride". Journal of Materials Science 33 (9): 2251. doi:10.1023/A:1004327018497.
- ↑ 8,0 8,1 8,2 Ferracane, Jack L. (2001). Materials in Dentistry: Principles and Applications. Lippincott Williams & Wilkins. pp. 70,143. ISBN 0781727332. http://books.google.com/?id=5uvuvNKpIkQC&pg=PA143.
- ↑ Park C.-K., Silsbee M. R., Roy D. M. (1998). "Setting reaction and resultant structure of zinc phosphate cement in various orthophosphoric acid cement-forming liquids". Cement and concrete research 28 (1): 141–150. doi:10.1016/S0008-8846(97)00223-8.
- ↑ Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements. Oxford:Butterworth-Heinemann. ISBN 0-7506-3365-4.
- ↑ International Occupational Safety and Health Information Centre (CIS) Access date January 25, 2009.
- ↑ Zinc oxide MSDS. Access date January 25, 2009.
- ↑ 13,0 13,1 13,2 Özgür, Ü.; Alivov, Ya. I.; Liu, C.; Teke, A.; Reshchikov, M. A.; Doğan, S.; Avrutin, V.; Cho, S.-J. et al. (2005). "A comprehensive review of ZnO materials and devices". Journal of Applied Physics 98 (4): 041301. doi:10.1063/1.1992666.
- ↑ Rossler, U., ed (1999). Landolt-Bornstein, New Series, Group III. Vol. 17B, 22, 41B. Springer, Heidelberg.
- ↑ Claus Franz Klingshirn; Bruno K. Meyer; Andreas Waag; Axel Hoffmann, Johannes M. M. Geurts (1 August 2010). Zinc Oxide: From Fundamental Properties Towards Novel Applications. Springer. pp. 9–10. ISBN 978-3-642-10576-0. http://books.google.com/books?id=TYXinw6pKk4C&pg=PA9. Retrieved 9 December 2011.
- ↑ 16,0 16,1 16,2 Baruah, S. and Dutta, J. (2009). "Hydrothermal growth of ZnO nanostructures" (free download pdf). Sci. Technol. Adv. Mater. 10: 013001. doi:10.1088/1468-6996/10/1/013001.
- ↑ 17,0 17,1 17,2 17,3 Porter, F. (1991). Zinc Handbook: Properties, Processing, and Use in Design. CRC Press. ISBN 0824783409.
- ↑ Millot, Marius; et al.,, Ramon; Munoz-Sanjose, Vicente; Broto, Jean-Marc; Gonzalez, Jesus (2010). "Anharmonic effects in ZnO optical phonons probed by Raman spectroscopy". Applied Physics letters 96 (15): 152103. doi:10.1063/1.3387843.
- ↑ Dal Corso, Andrea; Posternak, Michel; Resta, Raffaele; Baldereschi, Alfonso (1994). "Ab initio study of piezoelectricity and spontaneous polarization in ZnO". Physical Review B 50 (15): 10715. doi:10.1103/PhysRevB.50.10715.
- ↑ Look, D.C.; Hemsky, J.W.; Sizelove, J.R. (1999). "Residual Native Shallow Donor in ZnO". Physical Review Letters 82 (12): 2552. doi:10.1103/PhysRevLett.82.2552.
- ↑ Janotti, A; Van De Walle, CG (2007). "Hydrogen multicentre bonds". Nature Materials 6 (1): 44–7. doi:10.1038/nmat1795. PMID 17143265.
- ↑ Kato, H (2002). "Growth and characterization of Ga-doped ZnO layers on a-plane sapphire substrates grown by molecular beam epitaxy". Journal of Crystal Growth 237–239: 538. doi:10.1016/S0022-0248(01)01972-8.
- ↑ Ohgaki, Takeshi; Ohashi, Naoki; Sugimura, Shigeaki; Ryoken, Haruki; Sakaguchi, Isao; Adachi, Yutaka; Haneda, Hajime (2008). "Positive Hall coefficients obtained from contact misplacement on evident n-type ZnO films and crystals". Journal of Materials Research 23 (9): 2293. doi:10.1557/JMR.2008.0300.
- ↑ Wagner, P; Helbig, R (1974). "Halleffekt und anisotropie der beweglichkeit der elektronen in ZnO". Journal of Physics and Chemistry of Solids 35 (3): 327. doi:10.1016/S0022-3697(74)80026-0.
- ↑ Ryu, Y. R.; Lee, T. S.; White, H. W. (2003). "Properties of arsenic-doped p-type ZnO grown by hybrid beam deposition". Applied Physics Letters 83: 87. doi:10.1063/1.1590423.
- ↑ 26,0 26,1 Schulz, D. et al. (2008). "Inductively heated Bridgman method for the growth of zinc oxide single crystals". Journal of Crystal Growth 310 (7–9): 1832. doi:10.1016/j.jcrysgro.2007.11.050.
- ↑ Baruah, Sunandan; Thanachayanont, Chanchana; Dutta, Joydeep (2008). "Growth of ZnO nanowires on nonwoven polyethylene fibers" (free download pdf). Science and Technology of Advanced Materials 9 (2): 025009. doi:10.1088/1468-6996/9/2/025009.
- ↑ Miao, L.; Ieda, Y.; Tanemura, S.; Cao, Y.G.; Tanemura, M.; Hayashi, Y.; Toh, S.; Kaneko, K. (2007). "Synthesis, microstructure and photoluminescence of well-aligned ZnO nanorods on Si substrate" (free download pdf). Science and Technology of Advanced Materials 8 (6): 443. doi:10.1016/j.stam.2007.02.012.
- ↑ Ying Zhou et al. (2008). "Hydrothermal synthesis of ZnO nanorod arrays with the addition of polyethyleneimine". Materials Research Bulletin 43 (8–9): 2113–2118. doi:10.1016/j.materresbull.2007.09.024.
- ↑ Cui, Jingbiao et al. (2006). "Synthesis and magnetic properties of Co-doped ZnO nanowires". Journal of Applied Physics 99 (8): 08M113. doi:10.1063/1.2169411.
- ↑ Elen, K. et al. (2009). "Hydrothermal synthesis of ZnO nanorods: a statistical determination of the significant parameters in view of reducing the diameter". Nanotechnology 20 (5): 055608. doi:10.1088/0957-4484/20/5/055608. PMID 19417355.
- ↑ Greene, L. E. et al. (2003). "Low-Temperature Wafer-Scale Production of ZnO Nanowire Arrays". Angew. Chem. Int. Ed 42 (26): 3031–3032. doi:10.1002/anie.200351461. PMID 12851963.
- ↑ Wu, Wan-Yu et al. (2009). "Effects of Seed Layer Characteristics on the Synthesis of ZnO Nanowires". Journal of the American Ceramic Society 92 (11): 2718–2723. doi:10.1111/j.1551-2916.2009.03022.x.
- ↑ Greene, L. E.; Law, M; Tan, DH; Montano, M; Goldberger, J; Somorjai, G; Yang, P (2005). "General Route to Vertical ZnO Nanowire Arrays Using Textured ZnO Seeds". Nano Letters 5 (7): 1231–1236. doi:10.1021/nl050788p. PMID 16178216.
- ↑ Hua, Guomin et al. (2008). "Fabrication of ZnO nanowire arrays by cycle growth in surfactantless aqueous solution and their applications on dye-sensitized solar cells". Materials Letters 62 (25): 4109–4111. doi:10.1016/j.matlet.2008.06.018.
- ↑ Lee, J.-H. et al. (2009). "Density-controlled growth and field emission property of aligned ZnO nanorod arrays". Appl Phys A 97 (2): 403–408. doi:10.1007/s00339-009-5226-y.
- ↑ 37,0 37,1 37,2 Nav Bharat Metallic Oxide Industries Pvt. Limited. Applications of ZnO. Access date January 25, 2009.
- ↑ 38,0 38,1 Brown, H. E. (1957). Zinc Oxide Rediscovered. New York: The New Jersey Zinc Company.
- ↑ Brown, H. E. (1976). Zinc Oxide Properties and Applications. New York: International Lead Zinc Research Organization.
- ↑ van Noort, Richard (2002). Introduction to Dental Materials, 2d Edition. Elsevier Health Sciences. ISBN 0723432155.
- ↑ Padmavathy, Nagarajan; Vijayaraghavan, Rajagopalan (2008). "Enhanced bioactivity of ZnO nanoparticles—an antimicrobial study" (free download pdf). Science and Technology of Advanced Materials 9 (3): 035004. doi:10.1088/1468-6996/9/3/035004.
- ↑ Li, Qun; Chen, Shui-Lin; Jiang, Wan-Chao (2007). "Durability of nano ZnO antibacterial cotton fabric to sweat". Journal of Applied Polymer Science 103: 412. doi:10.1002/app.24866.
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- Zincite properties
- International Chemical Safety Card 0208.
- NIOSH Pocket Guide to Chemical Hazards.
- Nav Bharat Metallic Oxide Industries. (describes industrial uses of zinc oxide)
- External MSDS (Material Safety Data Sheet) on zinc oxide
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