Chemistry:Zinc oxide

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Short description: White powder insoluble in water
Zinc oxide
Zinc oxide.jpg
Names
Other names
Zinc white, calamine, philosopher's wool, Chinese white, flowers of zinc
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
DrugBank
EC Number
  • 215-222-5
13738
KEGG
RTECS number
  • ZH4810000
UNII
UN number 3077
Properties
ZnO
Molar mass 81.406 g/mol[1]
Appearance White solid[1]
Odor Odorless
Density 5.6 g/cm3[1]
Melting point 1,974 °C (3,585 °F; 2,247 K) (decomposes)[1][7]
Boiling point 2,360 °C (4,280 °F; 2,630 K) (decomposes)
0.0004% (17.8°C)[2]
Band gap 3.2 eV (direct)[3]
Electron mobility 180 cm2/(V·s)[3]
−27.2·10−6 cm3/mol[4]
Thermal conductivity 0.6 W/(cm·K)[5]
n1=2.013, n2=2.029[6]
Structure[8]
Wurtzite
C6v4-P63mc
a = 3.2495 Å, c = 5.2069 Å
2
Tetrahedral
Thermochemistry[9]
40.3 J·K−1mol−1
43.65±0.40 J·K−1mol−1
-350.46±0.27 kJ mol−1
-320.5 kJ mol−1
Enthalpy of fusion (ΔfH⦵fus)
 70 kJ/mol
Pharmacology
1=ATCvet code} QA07XA91 (WHO)
Hazards
Safety data sheet ICSC 0208
GHS pictograms GHS09: Environmental hazard
GHS Signal word Warning
H400, H401
P273, P391, P501
NFPA 704 (fire diamond)
Flammability code 0: Will not burn. E.g. waterHealth code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no codeNFPA 704 four-colored diamond
0
2
0
Flash point 1,436 °C (2,617 °F; 1,709 K)
Lethal dose or concentration (LD, LC):
240 mg/kg (intraperitoneal, rat)[10]
7950 mg/kg (rat, oral)[11]
2500 mg/m3 (mouse)[11]
2500 mg/m3 (guinea pig, 3–4 h)[11]
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 5 mg/m3 (fume) TWA 15 mg/m3 (total dust) TWA 5 mg/m3 (resp dust)[2]
REL (Recommended)
 Dust: TWA 5 mg/m3 C 15 mg/m3

Fume: TWA 5 mg/m3 ST 10 mg/m3[2]

IDLH (Immediate danger)
 500 mg/m3[2]
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).
☒N verify (what is ☑Y☒N ?)
Infobox references

Zinc oxide is an inorganic compound with the formula ZnO. It is a white powder that is insoluble in water. ZnO is used as an additive in numerous materials and products including cosmetics, food supplements, rubbers, plastics, ceramics, glass, cement, lubricants,[12] paints, sunscreens, ointments, adhesives, sealants, pigments, foods, batteries, ferrites, fire retardants, semi conductors,[13] and first-aid tapes. Although it occurs naturally as the mineral zincite, most zinc oxide is produced synthetically.[14]

History

Zinc compounds were probably used by early humans, in processed[14] and unprocessed forms, as a paint or medicinal ointment, but their 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.[15] Zinc oxide ointment is also mentioned by the Greek physician Dioscorides (1st century AD).[16] Galen suggested treating ulcerating cancers with zinc oxide,[17] as did Avicenna in his The Canon of Medicine. It is used as an ingredient in products such as baby powder and creams against diaper rashes, calamine cream, anti-dandruff shampoos, and antiseptic ointments.[18]

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.[19] 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.[20] Zinc oxide has also been recovered from zinc mines at Zawar in India , dating from the second half of the first millennium BC.[16]

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.[21] Around 1782 Louis-Bernard Guyton de Morveau proposed replacing lead white pigment with zinc oxide.[22]

The main usage of zinc oxide (zinc white) was in paints and as an additive to ointments. Zinc white was accepted as a pigment in oil paintings by 1834 but it did not mix well with oil. This problem was solved by optimizing the synthesis of ZnO. In 1845, Edme-Jean 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 valuable for making tints with other colors, but 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.[23]

In recent times, most zinc oxide was used in the rubber industry to resist corrosion. In the 1970s, the second largest application of ZnO was photocopying. High-quality ZnO produced by the "French process" was added to photocopying paper as a filler. This application was soon displaced by titanium.[24]

Chemical properties

Pure ZnO is a white powder, but in nature it occurs as the rare mineral zincite, which usually contains manganese and other impurities that confer a yellow to red color.[25]

Crystalline zinc oxide is thermochromic, changing from white to yellow when heated in air and reverting to white on cooling.[26] This color change is caused by a small loss of oxygen to the environment at high temperatures to form the non-stoichiometric Zn1+xO, where at 800 °C, x = 0.00007.[26]

Zinc oxide is an amphoteric oxide. It is nearly insoluble in water, but it will dissolve in most acids, such as hydrochloric acid:[27]

ZnO + 2 HCl → ZnCl2 + H2O

Solid zinc oxide will also dissolve in alkalis 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. When mixed with a strong aqueous solution of zinc chloride, ZnO forms cement-like products best described as zinc hydroxy chlorides.[28] This cement was used in dentistry.[29]

Hopeite

ZnO also forms cement-like material when treated with phosphoric acid; related materials are used in dentistry.[29] A major component of zinc phosphate cement produced by this reaction is hopeite, Zn3(PO4)2·4H2O.[30]

ZnO decomposes into zinc vapor and oxygen at around 1975 °C with a standard oxygen pressure. In a carbothermic reaction, heating with carbon converts the oxide into zinc vapor at a much lower temperature (around 950 °C).[27]

ZnO + C → Zn(Vapor) + CO

Physical properties

Wurtzite structure
A zincblende unit cell

Structure

Zinc oxide crystallizes in two main forms, hexagonal wurtzite[31] 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). ZnO converts to the rocksalt motif at relatively high pressures about 10 GPa.[13]

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.[32] 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,[33] 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.[34] However, studies using wurtzoid structures explained the origin of surface flatness and the absence of reconstruction at ZnO wurtzite surfaces[35] in addition to the origin of charges on ZnO planes.

Mechanical properties

ZnO is a wide-band gap semiconductor of the II-VI semiconductor group. The native doping of the semiconductor due to oxygen vacancies or zinc interstitials is n-type.[13]

ZnO is a relatively soft material with approximate hardness of 4.5 on the Mohs scale.[12] 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.[24] The E2 optical phonon in ZnO exhibits an unusually long lifetime of 133 ps at 10 K.[36]

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.[37] This property makes it a technologically important material for many piezoelectrical applications, which require a large electromechanical coupling. Therefore, ZnO in the form of thin film has been one of the most studied resonator materials for thin-film bulk acoustic resonators.

Electrical and optical properties

Favourable properties of zinc oxide include good transparency, high electron mobility, wide band gap, and strong room-temperature luminescence. Those properties make ZnO valuable for a variety of emerging applications: transparent electrodes in liquid crystal displays, energy-saving or heat-protecting windows, and electronics as thin-film transistors and light-emitting diodes.

ZnO has a relatively wide direct band gap of ~3.3 eV at room temperature. Advantages associated with a wide band gap include higher breakdown voltages, ability to sustain large electric fields, lower electronic noise, and high-temperature and high-power operation. The band gap of ZnO can further be tuned to ~3–4 eV by its alloying with magnesium oxide or cadmium oxide.[13] Due to this large band gap, there have been efforts to create visibly transparent solar cells utilising ZnO as a light absorbing layer. However, these solar cells have so far proven highly inefficient. [38]

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.[39] An alternative explanation has been proposed, based on theoretical calculations, that unintentional substitutional hydrogen impurities are responsible.[40] 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.[41]

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.[42]

Current limitations to p-doping 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.[13]

Electron mobility of ZnO strongly varies with temperature and has a maximum of ~2000 cm2/(V·s) at 80 K.[43] Data on hole mobility are scarce with values in the range 5–30 cm2/(V·s).[44]

ZnO discs, acting as a varistor, are the active material in most surge arresters.[45][46]

Zinc oxide is noted for its strongly nonlinear optical properties, especially in bulk. The nonlinearity of ZnO nanoparticles can be fine-tuned according to their size.[47]

Production

For industrial use, ZnO is produced at levels of 105 tons per year[25] by three main processes:[24]

Indirect process

In the indirect or French process, 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 Edme Jean LeClaire of Paris 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 process

The direct or American 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 process

A small amount of industrial production involves wet chemical processes, which start with aqueous solutions of zinc salts, from which zinc carbonate or zinc hydroxide is precipitated. The solid precipitate is then calcined at temperatures around 800 °C.

Laboratory synthesis

The red and green colors of these synthetic ZnO crystals result from different concentrations of oxygen vacancies.[48]

Numerous 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) can be grown by the gas transport (vapor-phase deposition), hydrothermal synthesis,[34][48][49] or melt growth.[7] However, because of the 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.[7] 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

ZnO nanostructures

Nanostructures of 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.[34][50][51] 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.[52] Doping of the ZnO nanowires has been achieved by adding other metal nitrates to the growth solution.[53] 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).[54]

Aligned ZnO nanowires on pre-seeded silicon, glass, and gallium nitride substrates have been grown using aqueous zinc salts such as zinc nitrate and zinc acetate in basic environments.[55] 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 physical vapor deposition methods to deposit ZnO thin films.[56][57] 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.[58][59]

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, high thermal conductivity, binding, antibacterial and UV-protection properties. Consequently, it is added into materials and products including plastics, ceramics, glass, cement,[60] rubber, lubricants,[12] paints, ointments, adhesive, sealants, concrete manufacturing, pigments, foods, batteries, ferrites, fire retardants, etc.[61]

Rubber industry

Between 50% and 60% of ZnO use is in the rubber industry.[62] Zinc oxide along with stearic acid is used in the sulfur vulcanization of rubber.[24][63] ZnO additives also protect rubber from fungi (see medical applications) and UV light.

Ceramic industry

Ceramic industry consumes a significant amount of zinc oxide, in particular in ceramic glaze and frit compositions. The relatively high heat capacity, thermal conductivity and high temperature stability of ZnO coupled with a comparatively low coefficient of expansion are desirable properties in the production of ceramics. ZnO affects the melting point and optical properties of the glazes, enamels, and ceramic formulations. Zinc oxide as a low expansion, secondary flux improves the elasticity of glazes by reducing the change in viscosity as a function of temperature and helps prevent crazing and shivering. By substituting ZnO for BaO and PbO, the heat capacity is decreased and the thermal conductivity is increased. Zinc in small amounts improves the development of glossy and brilliant surfaces. However, in moderate to high amounts, it produces matte and crystalline surfaces. With regard to color, zinc has a complicated influence.[62]

Medicine

Skin treatment

Zinc oxide as a mixture with about 0.5% iron(III) oxide (Fe2O3) is called calamine and is used in calamine lotion. Historically the mineral calamine is a mixture of the oxides zincite and hemimorphite.

Zinc oxide is widely used to treat a variety of skin conditions, including atopic dermatitis, contact dermatitis, itching due to eczema, diaper rash and acne.[64] It is used in products such as baby powder and barrier creams to treat diaper rashes, calamine cream, anti-dandruff shampoos, and antiseptic ointments.[18][65] It is often combined with castor oil to form an emollient and astringent, zinc and castor oil cream, commonly used to treat infants.[66][67]

It is also a component in tape (called "zinc oxide tape") used by athletes as a bandage to prevent soft tissue damage during workouts.[68]

Antibacterial

Zinc oxide is used in mouthwash products and toothpastes as an anti-bacterial agent proposed to prevent plaque and tartar formation,[69] and to control bad breath by reducing the volatile gases and volatile sulfur compounds (VSC) in the mouth.[70] Along with zinc oxide or zinc salts, these products also commonly contain other active ingredients, such as cetylpyridinium chloride,[71] xylitol,[72] hinokitiol,[73] essential oils and plant extracts.[74][75] Powdered zinc oxide has deodorizing and antibacterial properties.[76]

ZnO is added to cotton fabric, rubber, oral care products,[77][78] and food packaging.[79][80] Enhanced antibacterial action of fine particles compared to bulk material is not exclusive to ZnO and is observed for other materials, such as silver.[81] This property results from the increased surface area of the fine particles.

Sunscreen

Zinc oxide is used in sunscreen to absorb ultraviolet light.[64] It is the broadest spectrum UVA and UVB absorber[82][83] that is approved for use as a sunscreen by the U.S. Food and Drug Administration (FDA),[84] and is completely photostable.[85] When used as an ingredient in sunscreen, zinc oxide blocks both UVA (320–400 nm) and UVB (280–320 nm) rays of ultraviolet light. Zinc oxide and the other most common physical sunscreen, titanium dioxide, are considered to be nonirritating, nonallergenic, and non-comedogenic.[86] Zinc from zinc oxide is, however, slightly absorbed into the skin.[87]

Many sunscreens use nanoparticles of zinc oxide (along with nanoparticles of titanium dioxide) because such small particles do not scatter light and therefore do not appear white. The nanoparticles are not absorbed into the skin more than regular-sized zinc oxide particles are,[88] and are only absorbed into the outermost layer of the skin but not into the body.[88]

Dental restoration

When mixed with eugenol, zinc oxide eugenol is formed, which has applications as a restorative and prosthodontic in dentistry.[29][89]

Food additive

Zinc oxide is added to many food products, including breakfast cereals, as a source of zinc,[90] a necessary nutrient. Zinc sulfate is also used for the same purpose. Some prepackaged foods also include trace amounts of ZnO even if it is not intended as a nutrient.

Pigment

Main page: Zinc white

Zinc oxide (zinc white) is used as a pigment in paints and is more opaque than lithopone, but less opaque than titanium dioxide.[14] It is also used in coatings for paper. Chinese white is a special grade of zinc white used in artists' pigments.[91] The use of zinc white as a pigment in oil painting started in the middle of 18th century.[92] It has partly replaced the poisonous lead white and was used by painters such as Böcklin, Van Gogh,[93] Manet, Munch and others. It is also a main ingredient of mineral makeup (CI 77947).[94]

UV absorber

Micronized and nano-scale zinc oxide provides strong protection against UVA and UVB ultraviolet radiation, and are consequently used in sunscreens,[95] and also in UV-blocking sunglasses for use in space and for protection when welding, following research by scientists at Jet Propulsion Laboratory (JPL).[96]

Coatings

Paints containing zinc oxide powder have long been utilized as anticorrosive coatings for metals. They are especially effective for galvanized iron. Iron is difficult to protect because its reactivity with organic coatings leads to brittleness and lack of adhesion. Zinc oxide paints retain their flexibility and adherence on such surfaces for many years.[61]

ZnO highly n-type doped with aluminium, gallium, or indium is transparent and conductive (transparency ~90%, lowest resistivity ~10−4 Ω·cm[97]). ZnO:Al coatings are 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.[25]

Plastics, such as polyethylene naphthalate (PEN), can be protected by applying zinc oxide coating. The coating reduces the diffusion of oxygen through PEN.[98] Zinc oxide layers can also be used on polycarbonate in outdoor applications. The coating protects polycarbonate from solar radiation, and decreases its oxidation rate and photo-yellowing.[99]

Corrosion prevention in nuclear reactors

Main page: Physics:Depleted zinc oxide

Zinc oxide depleted in 64Zn (the zinc isotope with 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.[100]

Methane reforming

Zinc oxide (ZnO) is used as a pretreatment step to remove hydrogen sulfide (H2S) from natural gas following hydrogenation of any sulfur compounds prior to a methane reformer, which can poison the catalyst. At temperatures between about 230–430 °C (446–806 °F), H2S is converted to water by the following reaction:[101]

H2S + ZnO → H2O + ZnS

Electronics

Photograph of an operating ZnO UV laser diode and the corresponding device structure.[102]
Flexible gas sensor based on ZnO nanorods and its internal structure. ITO stands for indium tin oxide and PET for polyethylene terephthalate.[103]

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).[104] Moreover, ultrafast nonlinearities and photoconductive functions have been reported in ZnO.[105] Some optoelectronic applications of ZnO overlap with that of GaN, which has a similar band gap (~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, a transparent conducting oxide layer and ZnO nanostructures provide better light outcoupling.[106] Other properties of ZnO favorable for electronic applications include its stability to high-energy radiation and its ability to be patterned by wet chemical etching.[107] Radiation resistance[108] makes ZnO a suitable candidate for space applications. ZnO is the most promising candidate in the field of random lasers to produce an electronically pumped UV laser source.

The pointed tips of ZnO nanorods result in a strong enhancement of an electric field. Therefore, they can be used as field emitters.[109]

Aluminium-doped ZnO layers are used as transparent electrodes. The components Zn and Al are much cheaper and less toxic 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.[110]

Transparent thin-film transistors (TTFT) can be produced with ZnO. As field-effect transistors, they do not need a p–n junction,[111] thus avoiding the p-type doping problem of ZnO. Some of the field-effect transistors even use ZnO nanorods as conducting channels.[112]

Gas sensors

Zinc oxide is used in semiconductor gas sensors for detecting airborne compounds such as hydrogen sulfide, nitrogen dioxide, and volatile organic compounds. ZnO is a semiconductor that becomes n-doped by adsorption of reducing compounds, which reduces the detected electrical resistance through the device, in a manner similar to the widely used tin oxide semiconductor gas sensors. It is formed into nanostructures such as thin films, nanoparticles, nanopillars or nanowires in order to provide large surface area for interaction with gasses. The sensors are made selective for specific gasses by doping or surface-attaching materials such as catalytic noble metals.[113][114]

Piezoelectricity

The piezoelectricity in textile fibers coated in ZnO have been shown capable of fabricating "self-powered nanosystems" with everyday mechanical stress from wind or body movements.[115][116]

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.[117]

ZnO as anode of Li-ion battery

In form of a thin film ZnO has been demonstrated in miniaturised high frequency thin film resonators, sensors and filters.

Li-ion battery and supercapacitors

ZnO is a promising anode material for lithium-ion battery because it is cheap, biocompatible, and environmentally friendly. ZnO has a higher theoretical capacity (978 mAh g−1) than many other transition metal oxides such as CoO (715 mAh g−1), NiO (718 mAh g−1) and CuO (674 mAh g−1).[118] ZnO is also used as an electrode in supercapacitors.[119]

Safety

As a food additive, zinc oxide is on the U.S. FDA's list of generally recognized as safe, or GRAS, substances.[120]

Zinc oxide itself is non-toxic; it is hazardous, however, to inhale high concentrations of zinc oxide fumes, such as generated when zinc or zinc alloys are melted and oxidized at high temperature. This problem occurs while melting alloys containing brass because the melting point of brass is close to the boiling point of zinc.[121] Inhalation of zinc oxide, which may occur when welding galvanized (zinc-plated) steel, can result in a malady called metal fume fever.[121]

In sunscreen formulations that combined zinc oxide with small-molecule UV absorbers, UV light caused photodegradation of the small-molecule asorbers and toxicity in embryonic zebrafish assays.[122]

See also


References

  1. ↑ 1.0 1.1 1.2 1.3 Haynes, pp. 4.95, 12.80
  2. ↑ 2.0 2.1 2.2 2.3 NIOSH Pocket Guide to Chemical Hazards. "#0675". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0675.html. 
  3. ↑ 3.0 3.1 Haynes, pp. 12.85, 12.89
  4. ↑ Haynes, p. 4.131
  5. ↑ Haynes, p. 12.80
  6. ↑ Haynes, pp. 4.138, 10.251
  7. ↑ 7.0 7.1 7.2 Takahashi, Kiyoshi; Yoshikawa, Akihiko; Sandhu, Adarsh (2007). Wide bandgap semiconductors: fundamental properties and modern photonic and electronic devices. Springer. p. 357. ISBN 978-3-540-47234-6. https://books.google.com/books?id=j_HEazhVxoMC&pg=PA357. 
  8. ↑ Haynes, p. 4.145
  9. ↑ Haynes, pp. 5.2, 5.42, 6.163
  10. ↑ Zinc oxide. Chem.sis.nlm.nih.gov. Retrieved on 2015-11-17.
  11. ↑ 11.0 11.1 11.2 "Zinc oxide". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/idlh/1314132.html. 
  12. ↑ 12.0 12.1 12.2 "CuO, ZrO2 and ZnO nanoparticles as antiwear additive in oil lubricants". Wear 265 (3–4): 422–428. 2008. doi:10.1016/j.wear.2007.11.013. 
  13. ↑ 13.0 13.1 13.2 13.3 13.4 "A comprehensive review of ZnO materials and devices". Journal of Applied Physics 98 (4): 041301–041301–103. 2005. doi:10.1063/1.1992666. Bibcode: 2005JAP....98d1301O. https://scholarscompass.vcu.edu/cgi/viewcontent.cgi?article=1158&context=egre_pubs. 
  14. ↑ 14.0 14.1 14.2 De Liedekerke, Marcel (2006). "2.3. Zinc Oxide (Zinc White): Pigments, Inorganic, 1". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a20_243.pub2. 
  15. ↑ "Zinc in India". 2000 years of zinc and brass. British Museum. 1998. p. 27. ISBN 978-0-86159-124-4. 
  16. ↑ 16.0 16.1 Oleson, John Peter, ed (2008). "Mining and Metallurgy, chapter 4". The Oxford Handbook of Engineering and Technology in the Classical World. Oxford University Press. pp. 111–112. ISBN 978-0-19-518731-1. https://books.google.com/books?id=OPOdZaIElRkC&pg=PA111. 
  17. ↑ Winchester, David J.; Winchester, David P.; Hudis, Clifford A.; Norton, Larry (2005). Breast Cancer (Atlas of Clinical Oncology). PMPH USA. p. 3. ISBN 978-1550092721. 
  18. ↑ 18.0 18.1 Harding, Fred John (2007). Breast Cancer: Cause – Prevention – Cure. Tekline Publishing. p. 83. ISBN 978-0-9554221-0-2. https://books.google.com/books?id=0h2gDLv3MOEC&pg=PT83. 
  19. ↑ "Zinc". Encyclopædia Britannica. 10 March 2009. http://www.britannica.com/EBchecked/topic/657264/zinc. 
  20. ↑ Craddock, Paul Terence (2009). "The origins and inspirations of zinc smelting". Journal of Materials Science 44 (9): 2181–2191. doi:10.1007/s10853-008-2942-1. Bibcode: 2009JMatS..44.2181C. 
  21. ↑ General Information of Zinc from the National Institute of Health, WHO, and International Zinc Association. Retrieved 10 March 2009
  22. ↑ "Zinc White". https://www.matisse.com.au/zinc-white. 
  23. ↑ "Zinc white: History of use". Pigments through the ages. webexhibits.org. http://www.webexhibits.org/pigments/indiv/history/zincwhite.html. 
  24. ↑ 24.0 24.1 24.2 24.3 Zinc Handbook: Properties, Processing, and Use in Design. CRC Press. 1991. ISBN 978-0-8247-8340-2. 
  25. ↑ 25.0 25.1 25.2 "ZnO: material, physics and applications". ChemPhysChem 8 (6): 782–803. April 2007. doi:10.1002/cphc.200700002. PMID 17429819. https://scholar.google.com/scholar?hl=en&as_sdt=0%2C5&q=ZnO%3A+Material%2C+Physics+and+Applications&btnG=. 
  26. ↑ 26.0 26.1 Inorganic Chemistry. Elsevier. 2001. ISBN 978-0-12-352651-9. 
  27. ↑ 27.0 27.1 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8. 
  28. ↑ "The chemistry of cements formed between zinc oxide and aqueous zinc chloride". Journal of Materials Science 33 (9): 2251–2254. 1998. doi:10.1023/A:1004327018497. Bibcode: 1998JMatS..33.2251N. 
  29. ↑ 29.0 29.1 29.2 Materials in Dentistry: Principles and Applications. Lippincott Williams & Wilkins. 2001. pp. 70, 143. ISBN 978-0-7817-2733-4. https://books.google.com/books?id=5uvuvNKpIkQC&pg=PA143. 
  30. ↑ "Setting reaction and resultant structure of zinc phosphate cement in various orthophosphoric acid cement-forming liquids". Cement and Concrete Research 28 (1): 141–150. 1998. doi:10.1016/S0008-8846(97)00223-8. 
  31. ↑ Metal Oxides: Chemistry & Applications. CRC Press. 2006. p. 182. ISBN 978-0824723712. 
  32. ↑ Landolt-Bornstein, New Series, Group III. 17B, 22, 41B. Springer, Heidelberg. 1999. 
  33. ↑ Zinc Oxide: From Fundamental Properties Towards Novel Applications. Springer. 2010. pp. 9–10. ISBN 978-3-642-10576-0. https://books.google.com/books?id=TYXinw6pKk4C&pg=PA9. 
  34. ↑ 34.0 34.1 34.2 "Hydrothermal growth of ZnO nanostructures". Science and Technology of Advanced Materials 10 (1): 013001. February 2009. doi:10.1088/1468-6996/10/1/013001. PMID 27877250. Bibcode: 2009STAdM..10a3001B. 
  35. ↑ Abdulsattar, Mudar Ahmed (2015). "Capped ZnO (3, 0) nanotubes as building blocks of bare and H passivated wurtzite ZnO nanocrystals". Superlattices and Microstructures 85: 813–819. doi:10.1016/j.spmi.2015.07.015. Bibcode: 2015SuMi...85..813A. 
  36. ↑ "Anharmonic effects in ZnO optical phonons probed by Raman spectroscopy". Applied Physics Letters 96 (15): 152103. 2010. doi:10.1063/1.3387843. Bibcode: 2010ApPhL..96o2103M. 
  37. ↑ "Ab initio study of piezoelectricity and spontaneous polarization in ZnO". Physical Review B 50 (15): 10715–10721. October 1994. doi:10.1103/PhysRevB.50.10715. PMID 9975171. Bibcode: 1994PhRvB..5010715D. 
  38. ↑ Koyama, Miki; Ichimura, Masaya (2019). "Fabrication of ZnO/NiO transparent solar cells by electrochemical deposition". Japanese Journal of Applied Physics 58 (12). doi:10.7567/1347-4065/ab532a. Bibcode: 2019JaJAP..58l8003K. 
  39. ↑ "Residual Native Shallow Donor in ZnO". Physical Review Letters 82 (12): 2552–2555. 1999. doi:10.1103/PhysRevLett.82.2552. Bibcode: 1999PhRvL..82.2552L. https://corescholar.libraries.wright.edu/physics/216. 
  40. ↑ "Hydrogen multicentre bonds". Nature Materials 6 (1): 44–7. January 2007. doi:10.1038/nmat1795. PMID 17143265. Bibcode: 2007NatMa...6...44J. 
  41. ↑ "Growth and characterization of Ga-doped ZnO layers on a-plane sapphire substrates grown by molecular beam epitaxy". Journal of Crystal Growth 237–239: 538–543. 2002. doi:10.1016/S0022-0248(01)01972-8. Bibcode: 2002JCrGr.237..538K. 
  42. ↑ "Positive Hall coefficients obtained from contact misplacement on evident n-type ZnO films and crystals". Journal of Materials Research 23 (9): 2293–2295. 2008. doi:10.1557/JMR.2008.0300. Bibcode: 2008JMatR..23.2293O. 
  43. ↑ "Halleffekt und anisotropie der beweglichkeit der elektronen in ZnO". Journal of Physics and Chemistry of Solids 35 (3): 327–335. 1974. doi:10.1016/S0022-3697(74)80026-0. Bibcode: 1974JPCS...35..327W. 
  44. ↑ "Properties of arsenic-doped p-type ZnO grown by hybrid beam deposition". Applied Physics Letters 83 (1): 87. 2003. doi:10.1063/1.1590423. Bibcode: 2003ApPhL..83...87R. 
  45. ↑ René Smeets, Lou van der Sluis, Mirsad Kapetanovic, David F. Peelo, Anton Janssen. "Switching in Electrical Transmission and Distribution Systems". 2014. p. 316.
  46. ↑ Mukund R. Patel. "Introduction to Electrical Power and Power Electronics". 2012. p. 247.
  47. ↑ "Size-dependent enhancement of nonlinear optical properties in nanocolloids of ZnO". Journal of Applied Physics 103 (3): 033105–033105–7. 2008. doi:10.1063/1.2838178. Bibcode: 2008JAP...103c3105I. http://dyuthi.cusat.ac.in/xmlui/bitstream/purl/2586/1/Dyuthi-P0146.pdf. 
  48. ↑ 48.0 48.1 "Inductively heated Bridgman method for the growth of zinc oxide single crystals". Journal of Crystal Growth 310 (7–9): 1832–1835. 2008. doi:10.1016/j.jcrysgro.2007.11.050. Bibcode: 2008JCrGr.310.1832S. 
  49. ↑ "Growth of ZnO nanowires on nonwoven polyethylene fibers". Science and Technology of Advanced Materials 9 (2): 025009. April 2008. doi:10.1088/1468-6996/9/2/025009. PMID 27877984. Bibcode: 2008STAdM...9b5009B. 
  50. ↑ "Synthesis, microstructure and photoluminescence of well-aligned ZnO nanorods on Si substrate". Science and Technology of Advanced Materials 8 (6): 443–447. 2007. doi:10.1016/j.stam.2007.02.012. Bibcode: 2007STAdM...8..443M. 
  51. ↑ "One-dimensional ZnO nanostructures: Solution growth and functional properties". Nano Res. 4 (11): 1013–1098. 2011. doi:10.1007/s12274-011-0160-7. 
  52. ↑ "Hydrothermal synthesis of ZnO nanorod arrays with the addition of polyethyleneimine". Materials Research Bulletin 43 (8–9): 2113–2118. 2008. doi:10.1016/j.materresbull.2007.09.024. 
  53. ↑ "Synthesis and magnetic properties of Co-doped ZnO nanowires". Journal of Applied Physics 99 (8): 08M113. 2006-04-15. doi:10.1063/1.2169411. Bibcode: 2006JAP....99hM113C. 
  54. ↑ "Hydrothermal synthesis of ZnO nanorods: a statistical determination of the significant parameters in view of reducing the diameter". Nanotechnology 20 (5): 055608. February 2009. doi:10.1088/0957-4484/20/5/055608. PMID 19417355. Bibcode: 2009Nanot..20e5608E. 
  55. ↑ "Low-temperature wafer-scale production of ZnO nanowire arrays". Angewandte Chemie 42 (26): 3031–4. July 2003. doi:10.1002/anie.200351461. PMID 12851963. 
  56. ↑ Wu, Wan-Yu (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. 
  57. ↑ "General route to vertical ZnO nanowire arrays using textured ZnO seeds". Nano Letters 5 (7): 1231–6. July 2005. doi:10.1021/nl050788p. PMID 16178216. Bibcode: 2005NanoL...5.1231G. 
  58. ↑ Hua, Guomin (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. 
  59. ↑ "Density-controlled growth and field emission property of aligned ZnO nanorod arrays". Applied Physics A 97 (2): 403–408. 2009-05-07. doi:10.1007/s00339-009-5226-y. Bibcode: 2009ApPhA..97..403L. 
  60. ↑ "The nucleotide sequence of the tetracycline resistance determinant tetM from Ureaplasma urealyticum". Nucleic Acids Research 16 (3): 1216–7. February 1988. doi:10.1093/nar/16.3.1216. PMID 3344217. 
  61. ↑ 61.0 61.1 Ambica Dhatu Private Limited. Applications of ZnO. Access date January 25, 2009.
  62. ↑ 62.0 62.1 "Review: Zinc oxide particles: Synthesis, properties and applications". Chemical Engineering Journal 185–186: 1–22. 2012. doi:10.1016/j.cej.2012.01.076. 
  63. ↑ Zinc Oxide Rediscovered. New York: The New Jersey Zinc Company. 1957. 
  64. ↑ 64.0 64.1 Gupta, Mrinal; Mahajan, Vikram K.; Mehta, Karaninder S.; Chauhan, Pushpinder S. (2014). "Zinc Therapy in Dermatology: A Review". Dermatology Research and Practice 2014: 709152. doi:10.1155/2014/709152. PMID 25120566. 
  65. ↑ British National Formulary (2008). "Section 13.2.2 Barrier Preparations".
  66. ↑ Williams, Cheryll (1 July 2012) (in en). Medicinal Plants in Australia Volume 3: Plants, Potions and Poisons. Rosenberg Publishing. p. 309. ISBN 978-1-925078-07-7. https://books.google.com/books?id=ieVUAQAAQBAJ&dq=zinc+and+castor+oil+cream&pg=PA309. Retrieved 8 March 2023. 
  67. ↑ Nathan, Alan (2010) (in en). Non-prescription Medicines. Pharmaceutical Press. p. 206. ISBN 978-0-85369-886-9. https://books.google.com/books?id=lW-0IoSYMBYC&dq=zinc+and+castor+oil+cream&pg=PA206. Retrieved 8 March 2023. 
  68. ↑ "Zinc oxide tape: a useful dressing for the recalcitrant finger-tip and soft-tissue injury". Archives of Emergency Medicine 5 (4): 223–7. December 1988. doi:10.1136/emj.5.4.223. PMID 3233136. 
  69. ↑ Lynch, Richard J.M. (August 2011). "Zinc in the mouth, its interactions with dental enamel and possible effects on caries; a review of the literature". International Dental Journal 61 (Suppl 3): 46–54. doi:10.1111/j.1875-595X.2011.00049.x. PMID 21762155. 
  70. ↑ Cortelli, José Roberto; Barbosa, Mônica Dourado Silva; Westphal, Miriam Ardigó (August 2008). "Halitosis: a review of associated factors and therapeutic approach". Brazilian Oral Research 22 (suppl 1): 44–54. doi:10.1590/S1806-83242008000500007. PMID 19838550. 
  71. ↑ "SmartMouth Clinical DDS Activated Mouthwash". https://smartmouth.com/products/clinical-mouthwash/#toggle-id-1. 
  72. ↑ "Oxyfresh" (in en). https://oxyfresh.com/products/patented-zinc-mouthwash-with-fresh-mint. 
  73. ↑ "Dr ZinX" (in en). https://www.drzinx.com/ingredients. 
  74. ↑ Steenberghe, Daniel Van; Avontroodt, Pieter; Peeters, Wouter; Pauwels, Martine; Coucke, Wim; Lijnen, An; Quirynen, Marc (September 2001). "Effect of Different Mouthrinses on Morning Breath". Journal of Periodontology 72 (9): 1183–1191. doi:10.1902/jop.2000.72.9.1183. PMID 11577950. 
  75. ↑ Harper, D. Scott; Mueller, Laura J.; Fine, James B.; Gordon, Jeffrey; Laster, Larry L. (June 1990). "Clinical Efficacy of a Dentifrice and Oral Rinse Containing Sanguinaria Extract and Zinc Chloride During 6 Months of Use". Journal of Periodontology 61 (6): 352–358. doi:10.1902/jop.1990.61.6.352. PMID 2195152. 
  76. ↑ "Enhanced bioactivity of ZnO nanoparticles-an antimicrobial study". Science and Technology of Advanced Materials 9 (3): 035004. July 2008. doi:10.1088/1468-6996/9/3/035004. PMID 27878001. Bibcode: 2008STAdM...9c5004P. 
  77. ↑ "Contemporary perspective on the use of fluoride products in caries prevention". British Dental Journal 214 (4): 161–7. February 2013. doi:10.1038/sj.bdj.2013.162. PMID 23429124. 
  78. ↑ "The cariostatic mechanisms of fluoride". Acta Medica Academica 42 (2): 179–88. November 2013. doi:10.5644/ama2006-124.85. PMID 24308397. 
  79. ↑ Li, Qun; Chen, Shui-Lin; Jiang, Wan-Chao (2007). "Durability of nano ZnO antibacterial cotton fabric to sweat". Journal of Applied Polymer Science 103: 412–416. doi:10.1002/app.24866. 
  80. ↑ "Antibacterial, Deodorizing, and UV Absorbing Materials Obtained with Zinc Oxide (ZnO) Coated Fabrics". Journal of Industrial Textiles 23 (2): 150–164. 1993. doi:10.1177/152808379302300205. 
  81. ↑ "Enhancement of antibacterial properties of Ag nanorods by electric field". Science and Technology of Advanced Materials 10 (1): 015003. February 2009. doi:10.1088/1468-6996/10/1/015003. PMID 27877266. Bibcode: 2009STAdM..10a5003A. 
  82. ↑ "Critical Wavelength & Broad Spectrum UV Protection". https://mycpss.com/skin/sunscreens/critical-wavelength-broad-spectrum-uv-protection/. 
  83. ↑ "Physical sunscreens: on the comeback trail". Indian Journal of Dermatology, Venereology and Leprology 73 (2): 80–5. 2007. doi:10.4103/0378-6323.31890. PMID 17456911. http://www.bioline.org.br/pdf?dv07029. 
  84. ↑ "Sunscreen". U.S. Food and Drug Administration. https://www.fda.gov/Radiation-EmittingProducts/RadiationEmittingProductsandProcedures/Tanning/ucm116445.htm. 
  85. ↑ "Microfine zinc oxide (Z-cote) as a photostable UVA/UVB sunblock agent". Journal of the American Academy of Dermatology 40 (1): 85–90. January 1999. doi:10.1016/S0190-9622(99)70532-3. PMID 9922017. 
  86. ↑ "What to Look for in a Sunscreen". The New York Times. June 10, 2009. http://consults.blogs.nytimes.com/2009/06/10/what-to-look-for-in-a-sunscreen/. 
  87. ↑ "Percutaneous absorption of zinc from zinc oxide applied topically to intact skin in man". Dermatologica 180 (1): 36–9. 2009. doi:10.1159/000247982. PMID 2307275. 
  88. ↑ 88.0 88.1 "Current sunscreen controversies: a critical review". Photodermatology, Photoimmunology & Photomedicine 27 (2): 58–67. April 2011. doi:10.1111/j.1600-0781.2011.00557.x. PMID 21392107. 
  89. ↑ van Noort, Richard (2002). Introduction to Dental Materials (2d ed.). Elsevier Health Sciences. ISBN 978-0-7234-3215-9. 
  90. ↑ Quaker cereals content. quakeroats.com
  91. ↑ St. Clair, Kassia (2016). The Secret Lives of Colour. London: John Murray. p. 40. ISBN 9781473630819. OCLC 936144129. 
  92. ↑ Kuhn, H. (1986) "Zinc White", pp. 169–186 in Artists’ Pigments. A Handbook of Their History and Characteristics, Vol. 1. L. Feller (ed.). Cambridge University Press, London. ISBN:978-0521303743
  93. ↑ Vincent van Gogh, 'Wheatfield with Cypresses, 1889, pigment analysis at ColourLex
  94. ↑ Bouchez, Colette. "The Lowdown on Mineral Makeup". WebMD. http://www.webmd.com/skin-beauty/features/the-lowdown-on-mineral-makeup. Retrieved January 25, 2009. 
  95. ↑ US Environment Protection Agency: Sunscreen What are the active Ingredients in Sunscreen – Physical Ingredients:"The physical compounds titanium dioxide and zinc oxide reflect, scatter, and absorb both UVA and UVB rays." A table lists them as providing extensive physical protection against UVA and UVB
  96. ↑ Look Sharp While Seeing Sharp. NASA Scientific and Technical Information (2006). Retrieved 17 October 2009. JPL scientists developed UV-protective sunglasses using dyes and "zinc oxide, which absorbs ultraviolet light"
  97. ↑ "ZnO – nanostructures, defects, and devices". Materials Today 10 (5): 40–48. 2007. doi:10.1016/S1369-7021(07)70078-0. 
  98. ↑ "Photoprotection of poly(ethylene-naphthalate) by zinc oxide coating". Surface and Coatings Technology 180–181: 71–75. 2004. doi:10.1016/j.surfcoat.2003.10.039. 
  99. ↑ "Sputtered zinc oxide coatings: structural study and application to the photoprotection of the polycarbonate". Surface and Coatings Technology 180–181: 642–645. 2004. doi:10.1016/j.surfcoat.2003.10.109. 
  100. ↑ "BWR water chemistry?a delicate balance". Nuclear Energy 40 (4): 245–252. 2001. doi:10.1680/nuen.40.4.245.39338. 
  101. ↑ Robinson, Victor S. (1978) "Process for desulfurization using particulate zinc oxide shapes of high surface area and improved strength" U.S. Patent 4,128,619
  102. ↑ "Ultraviolet Lasers Realized via Electrostatic Doping Method". Scientific Reports 5: 13641. September 2015. doi:10.1038/srep13641. PMID 26324054. Bibcode: 2015NatSR...513641L. 
  103. ↑ "Light-controlling, flexible and transparent ethanol gas sensor based on ZnO nanoparticles for wearable devices". Scientific Reports 5: 11070. June 2015. doi:10.1038/srep11070. PMID 26076705. Bibcode: 2015NatSR...511070Z. 
  104. ↑ "ZnMgO-ZnO quantum wells embedded in ZnO nanopillars: Towards realisation of nano-LEDs". Physica Status Solidi C 4 (1): 158–161. 2007. doi:10.1002/pssc.200673557. Bibcode: 2007PSSCR...4..158B. 
  105. ↑ Torres-Torres, C.; Castro-Chacón, J. H.; Castañeda, L.; Rojo, R. Rangel; Torres-Martínez, R.; Tamayo-Rivera, L.; Khomenko, A. V. (2011-08-15). "Ultrafast nonlinear optical response of photoconductive ZnO films with fluorine nanoparticles" (in EN). Optics Express 19 (17): 16346–16355. doi:10.1364/OE.19.016346. ISSN 1094-4087. PMID 21934998. Bibcode: 2011OExpr..1916346T. https://www.osapublishing.org/oe/abstract.cfm?uri=oe-19-17-16346. 
  106. ↑ "ZnO – GaN Hybrid Heterostructures as Potential Cost Efficient LED Technology". Proceedings of the IEEE 98 (7): 1281–1287. 2010. doi:10.1109/JPROC.2009.2037444. 
  107. ↑ "Recent advances in ZnO materials and devices". Materials Science and Engineering B 80 (1–3): 383–387. 2001. doi:10.1016/S0921-5107(00)00604-8. 
  108. ↑ "Ion-beam-produced structural defects in ZnO". Physical Review B 67 (9): 094115. 2003-03-31. doi:10.1103/physrevb.67.094115. Bibcode: 2003PhRvB..67i4115K. http://espace.library.uq.edu.au/view/UQ:115991/UQ115991.pdf. 
  109. ↑ "ZnO nanoneedles with tip surface perturbations: Excellent field emitters". Applied Physics Letters 84 (18): 3603. 2004. doi:10.1063/1.1738174. Bibcode: 2004ApPhL..84.3603L. 
  110. ↑ "Transparent conductive Al-doped ZnO films for liquid crystal displays". Journal of Applied Physics 99 (12): 124505–124505–4. 2006. doi:10.1063/1.2206417. Bibcode: 2006JAP....99l4505O. 
  111. ↑ "Thin-film transistor fabricated in single-crystalline transparent oxide semiconductor". Science 300 (5623): 1269–72. May 2003. doi:10.1126/science.1083212. PMID 12764192. Bibcode: 2003Sci...300.1269N. 
  112. ↑ "Depletion-mode ZnO nanowire field-effect transistor". Applied Physics Letters 85 (12): 2274. 2004. doi:10.1063/1.1794351. Bibcode: 2004ApPhL..85.2274H. 
  113. ↑ Zhou, Xin; Lee, Songyi; Xu, Zhaochao; Yoon, Juyoung (2015). "Recent Progress on the Development of Chemosensors for Gases". Chemical Reviews 115 (15): 7944–8000. doi:10.1021/cr500567r. ISSN 0009-2665. PMID 25651137. 
  114. ↑ Sun, Yu-Feng; Liu, Shao-Bo; Meng, Fan-Li; Liu, Jin-Yun; Jin, Zhen; Kong, Ling-Tao; Liu, Jin-Huai (2012). "Metal Oxide Nanostructures and Their Gas Sensing Properties: A Review". Sensors 12 (3): 2610–2631. doi:10.3390/s120302610. ISSN 1424-8220. PMID 22736968. Bibcode: 2012Senso..12.2610S. 
  115. ↑ Keim, Brandon (February 13, 2008). "Piezoelectric Nanowires Turn Fabric Into Power Source". Wired News (CondéNet). http://blog.wired.com/wiredscience/2008/02/piezoelectric-n.html. 
  116. ↑ "Microfibre-nanowire hybrid structure for energy scavenging". Nature 451 (7180): 809–13. February 2008. doi:10.1038/nature06601. PMID 18273015. Bibcode: 2008Natur.451..809Q. 
  117. ↑ "New Small-scale Generator Produces Alternating Current By Stretching Zinc Oxide Wires". November 10, 2008. https://www.sciencedaily.com/releases/2008/11/081109193342.htm. 
  118. ↑ "Bio-inspired Murray materials for mass transfer and activity". Nature Communications 8: 14921. April 2017. doi:10.1038/ncomms14921. PMID 28382972. Bibcode: 2017NatCo...814921Z. 
  119. ↑ Sreejesh, M.; Dhanush, S.; Rossignol, F.; Nagaraja, H. S. (2017-04-15). "Microwave assisted synthesis of rGO/ZnO composites for non-enzymatic glucose sensing and supercapacitor applications" (in en). Ceramics International 43 (6): 4895–4903. doi:10.1016/j.ceramint.2016.12.140. ISSN 0272-8842. https://www.sciencedirect.com/science/article/pii/S0272884216324105. 
  120. ↑ "Zinc oxide". Database of Select Committee on GRAS Substances (SCOGS) Reviews. U.S. Food and Drug Administration. http://www.accessdata.fda.gov/scripts/fcn/fcnDetailNavigation.cfm?rpt=scogsListing&id=372. 
  121. ↑ 121.0 121.1 Gray, Theodore. "The Safety of Zinc Casting". The Wooden Periodic Table Table. http://www.theodoregray.com/PeriodicTable/ZincSafety.html. 
  122. ↑ "Zinc oxide-induced changes to sunscreen ingredient efficacy and toxicity under UV irradiation.". Photochem Photobiol Sci 20 (10): 1273–1285. 2021. doi:10.1007/s43630-021-00101-2. PMID 34647278. 

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