7440-66-6 Usage
Description
Zinc (Zn) is a metallic element discovered by a German
chemist, Andreas Marggraf, in 1746. It is environmentally
ubiquitous and essential for life. It exhibits a strong tendency to
react with both organic and inorganic compounds. Zinc is the
24th most abundant element, constitutes 0.027% bw of the
Earth’s crust, and has five stable isotopes. The largest mineable
amounts are found in Australia, Asia, and the United States. A
recent estimate suggests that approximately 20% of the world’s
population is at risk of Zn deficiency. However, free access to
uncontrolled amounts of Zn in nutritional supplements is the
most common cause of Zn excess. Both Zn deficiency and Zn
excess contribute to human Zn toxicity.
Chemical Properties
Zinc is a soft silvery colored metal; the dust is odorless and gray. It is one of the most common elements in the earth's crust. Metal zinc was first produced in India and China during the middle ages. Industrially important compounds of zinc are zinc chloride (ZnCl2), zinc oxide (ZnO), zinc stearate (Zn(C16H35O2)2), and zinc sulfide (Sphalerite, ZnS) found in hazardous waste sites. It is found in air, soil, and water, and is present in all foods.
Pure zinc is a bluish-white shiny metal. Zinc has many commercial uses as coatings to prevent rust, in dry-cell batteries, and mixed with other metals to make alloys like brass and bronze. Zinc combines with other elements to form zinc compounds. Zinc compounds are widely used in industry to make paint, rubber, dye, wood preservatives, and ointments.
Physical properties
Different sources of media describe the Physical properties of 7440-66-6 differently. You can refer to the following data:
1. Bluish-white lustrous metal; brittle at room temperature; malleable between 100 to 150°C; hexagonal close-packed structure; density 7.14 g/cm3; melts at 419.6°C; vaporizes at 907°C; vapor pressure 1 torr at 487°C, 5 torr at 558°C and 60 torr at 700°C; good conductor of electricity, electrical resistivity 5.46 microhm-cm at 0°C and 6.01 microhm-cm at 25°C; surface tension 768 dynes/cm at 600°C; viscosity 3.17 and 2.24 centipoise at 450 and 600°C, respectively; diamagnetic; magnetic susceptibility 0.139x10–6 cgs units in polycrystalline form; thermal neutron absorption cross-section 1.1 barns.
2. Zinc is a whitish metal with a bluish hue. As an electropositive metal, it readily gives up itstwo outer electrons located in the N shell as it combines with nonmetal elements. Zinc foilwill ignite in moist air, and zinc shavings and powder react violently with acids. Zinc’s meltingpoint is 419.58°C, its boiling point is 907°C, and its density is 7.14 g/cm3.Note: Zinc is not always included as one of the metals in the first series of the transitionelements, but it is the first element in group 12 (IIB).
Isotopes
There are 38 isotopes of zinc, ranging in atomic weights from Zn-54 to Zn-83.Just four of these are stable, and those four, plus one naturally radioactive isotope (Zn-70) that has a very long half-life (5×10+14 years), make up the element’s existence onEarth. Their proportional contributions to the natural existence of zinc on Earth are assuch: Zn-64 = 48.63%, Zn-66 = 27.90%, Zn-67 = 4.10%, Zn- 68 = 18.75%, and Zn-70 = 0.62%. All the other isotopes are radioactive and artificially produced.
Origin of Name
Although ancients used zinc compounds, the name “zinc” is assumed
to be derived from the German word zinn, which was related to tin.
Occurrence
Zinc is the 24th most abundant on Earth, which means it makes up only about 0.007%of the Earth’s crust. Even so, humans have found many uses for it over the past thousands ofyears.It is not found in its pure metallic form in nature but is refined from the mineral (compound) zinc sulfide (ZnSO4) known as the ores sphalerite and zincblende. It is also recoveredfrom minerals and ores known as willemite, hydrozincite, smithsonite, wurtzite, zincite, andFranklinite. Zinc ores are found in Canada, Mexico, Australia, and Belgium, as well as in theUnited States. Valuable grades of zinc ores are mined in Colorado and New Jersey.
Characteristics
Zinc is malleable and can be machined, rolled, die-cast, molded into various forms similarto plastic molding, and formed into rods, tubing, wires, and sheets. It is not magnetic, butit does resist corrosion by forming a hard oxide coating that prevents it from reacting anyfurther with air. When used to coat iron, it protects iron by a process called “galvanic protection,” also known as “sacrificial protection.” This protective characteristic occurs because theair will react with the zinc metal coating, which is a more electropositive (reactive) metal thanis the coated iron or steel, which is less electropositive than zinc. In other words, the zinc isoxidized instead of the underlying metal. (See the section under “Common Uses of Zinc” formore on galvanization.
History
Centuries before zinc was recognized as a distinct element,
zinc ores were used for making brass. Tubal-Cain, seven generations
from Adam, is mentioned as being an “instructor in
every artificer in brass and iron.” An alloy containing 87%
zinc has been found in prehistoric ruins in Transylvania.
Metallic zinc was produced in the 13th century A.D. in India
by reducing calamine with organic substances such as wool.
The metal was rediscovered in Europe by Marggraf in 1746,
who showed that it could be obtained by reducing calamine
with charcoal. The principal ores of zinc are sphalerite or
blende (sulfide), smithsonite (carbonate), calamine (silicate),
and franklinite (zinc, manganese, iron oxide). Canada, Japan,
Belgium, Germany, and the Netherlands are suppliers of zinc
ores. Zinc is also mined in Alaska, Tennessee, Missouri, and
elsewhere in the U.S. Zinc can be obtained by roasting its
ores to form the oxide and by reduction of the oxide with coal
or carbon, with subsequent distillation of the metal. Other
methods of extraction are possible. Naturally occurring zinc
contains five stable isotopes. Twenty-five other unstable
isotopes and isomers are recognized. Zinc is a bluish-white,
lustrous metal. It is brittle at ordinary temperatures but malleable
at 100 to 150°C. It is a fair conductor of electricity, and
burns in air at high red heat with evolution of white clouds
of the oxide. The metal is employed to form numerous alloys
with other metals. Brass, nickel silver, typewriter metal,
commercial bronze, spring brass, German silver, soft solder,
and aluminum solder are some of the more important alloys.
Large quantities of zinc are used to produce die castings,
used extensively by the automotive, electrical, and hardware
industries. An alloy called Prestal?, consisting of 78% zinc
and 22% aluminum, is reported to be almost as strong as
steel but as easy to mold as plastic. It is said to be so plastic
that it can be molded into form by relatively inexpensive die
casts made of ceramics and cement. It exhibits superplasticity.
Zinc is also extensively used to galvanize other metals
such as iron to prevent corrosion. Neither zinc nor zirconium
is ferromagnetic; but ZrZn2 exhibits ferromagnetism
at temperatures below 35 K. Zinc oxide is a unique and very
useful material to modern civilization. It is widely used in the
manufacture of paints, rubber products, cosmetics, pharmaceuticals,
floor coverings, plastics, printing inks, soap,
storage batteries, textiles, electrical equipment, and other
products. It has unusual electrical, thermal, optical, and solid-
state properties that have not yet been fully investigated.
Lithopone, a mixture of zinc sulfide and barium sulfate, is
an important pigment. Zinc sulfide is used in making luminous
dials, X-ray and TV screens, and fluorescent lights. The
chloride and chromate are also important compounds. Zinc
is an essential element in the growth of human beings and
animals. Tests show that zinc-deficient animals require 50%
more food to gain the same weight as an animal supplied
with sufficient zinc. Zinc is not considered to be toxic, but
when freshly formed ZnO is inhaled a disorder known as the
oxide shakes or zinc chills sometimes occurs. It is recommended
that where zinc oxide is encountered good ventilation
be provided. The commercial price of zinc in January
2002 was roughly 40¢/lb ($90 kg). Zinc metal with a purity of
99.9999% is priced at about $5/g.
Uses
Different sources of media describe the Uses of 7440-66-6 differently. You can refer to the following data:
1. zinc is described as an oligo element, trace element, or micro nutrient. Zinc is believed to accelerate wound healing. It is also considered an anti-oxidant, offering protection against uV radiation. It appears to favor the sulfur uptake in sulfurated amino acids and facilitates the incorporation of cysteine, an amino acid, into the skin. It also has a synergistic effect with vitamins A and e. Zinc is a component of more than 70 metal enzymes. It promotes collagen synthesis in the dermis and keratinization of the corneum layer. Zinc is useful for acne treatments because it lowers sebaceous secretion, and is also used in the treatment of psoriasis.
2. (Zn) A metallic element that functions as a nutrient and dietary supplement. It is believed to be necessary for nucleic acid metabolism, protein synthesis, and cell growth. Sources of include zinc acetate, carbonate, chloride, citrate, gluconate, oxide, stearate, and sulfate. The gluconate form is used in lozenges. The sulfate form exists as prisms, needles, or powder. It has a solubility of 1 g in 0.6 ml of water and is found in frozen egg substitutes.
3. Zinc is another earliest known metal. Use of its alloy, brass, dates back to prehistoric times. The metal was produced in India in the 13th century by reducing calamine (a silicate mineral of zinc) with wool. Marggraf produced the metal in 1746 by reducing calamine with charcoal. The element took its name from the German word zink meaning “of obscure origin.” Lohneyes first used this name in 1697. Zinc occurs in nature, widely distributed. The principal ores are sphalerite (and wurtzite) known as zinc blende, ZnS; gahnite, ZnAl2O4; calamine; smithsonite, ZnCO3; franklinite, ZnFe2O4; and zincite, ZnO. Abundance in earth’s crust is about 70 mg/kg and average concentration in sea water is about 10 μg/L.
Some important applications of zinc include galvanizing steel; to produce die castings; as a chemical additive in rubber and paints; in dry cells; in making electrodes; and as a reducing agent. Steel is galvanized by a thin coating of zinc to protect it from corrosion. Such galvanized steel is used in buildings, cars, and appliances. High-purity zinc is alloyed with aluminum at varying compositions, along with small amounts of copper and magnesium, to produce die castings. Such die castings are used extensively in automotive, hardware, and electrical industries. Zinc forms numerous alloys including brass, nickel silver, German silver, commercial bronze, soft solder, aluminum solder, and spring brass. The laboratory use of zinc includes preparating hydrogen gas and as a reducing agent in a number of chemical reactions. Zinc salts have numerous uses (See under specific compounds). Zinc is an essential nutrient element required for growth of animals.
4. This bluish white metallic element is found in sphalerite ore
that is roasted to give an oxide that is reduced with carbon to
make zinc vapor, which is condensed. Elemental zinc foil was
occasionally used to decolorize old collodion rich in iodine.
The zinc halides were used primarily in collodion emulsions.
5. Zinc is a constituent of many common alloys,including brass, bronze, Babbit metal, andGerman Silver. It is used to make householdutensils, castings, printing plates, buildingmaterials, electrical apparatus, dry-cell batteriesand many zinc salts. It is also used to galvanize sheet iron, bleaching bone glue andas a reducing agent in many organic reactions.
Definition
zinc: Symbol Zn. A blue-white metallicelement; a.n. 30; r.a.m. 65.38; r.d.7.1; m.p. 419.88°C; b.p. 907°C. It occursin sphalerite (or zinc blende,ZnS), which is found associated withthe lead sulphide, and in smithsonite(ZnCO3). Ores are roasted to give theoxide and this is reduced with carbon(coke) at high temperature, the zincvapour being condensed. Alternatively,the oxide is dissolved in sulphuricacid and the zinc obtained byelectrolysis. There are five stable isotopes(mass numbers 64, 66, 67, 68,and 70) and six radioactive isotopesare known. The metal is used in galvanizingand in a number of alloys(brass, bronze, etc.). Chemically it is areactive metal, combining with oxygenand other nonmetals and reactingwith dilute acids to releasehydrogen. It also dissolves in alkalis to give zincates. Most of its compoundscontain the Zn2+ ion.
Production Methods
Zinc is widely distributed in nature, constituting 20–200 ppm
of the Earth’s crust.The principal zinc ore is in the form of sulfides, such as
sphalerite and wurtzite (cubic and hexagonal ZnS) and
willemite (Zn2SiO4). To obtain metallic zinc, the zinc ores
that are relatively low in zinc content are concentrated. Zinc
smelting is gradually being replaced by the electrolytic
processes. During smelting there are often large emissions
of zinc, and other heavy metals contained in the zinc ore such
as lead and cadmium, into the air.
Reactions
Zinc exhibits a valence of +2 in all its compounds. It also is a highly electropositive metal. It replaces less electropositive metals from their aqueous salt solutions or melts. For example, a zinc metal bar put into Cu2+ solution acquires a brown-black crust of copper metal deposited on it. At the same time the blue color of the solution fades. Zinc reduces Cu2+ ions to copper metal. The overall reaction is:
Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)
This spontaneous reaction was used first in 1830 to make a voltaic cell. The metal is attacked by mineral acids. Reactions with sulfuric and hydrochloric acids produce hydrogen. With nitric acid, no hydrogen is evolved but the pentavalent nitrogen is reduced to nitrogen at lower valence states. Zinc is attacked by moist air at room temperature. Dry air has no action at ambient temperatures but the metal combines with dry oxygen rapidly above 225°C. Zinc reacts with carbon dioxide in the presence of moisture at ordinary temperatures forming a hydrated basic carbonate. The metal, on heating with dry halogen gases, yields zinc halides. However, in the presence of moisture the reaction occurs rapidly at ambient temperatures. The metal dissolves in hot solutions of caustic alkalis to form zincates and evolves hydrogen:
Zn + 2NaOH → Na2ZnO2 + H2
General Description
A grayish powder. Insoluble in water. May produce toxic zinc oxide fumes when heated to very high temperatures or when burned. Used in paints, bleaches and to make other chemicals.
Air & Water Reactions
Can evolve gaseous hydrogen in contact with water or damp air. The heat of the reaction may be sufficient to ignite the hydrogen produced [Haz. Chem. Data 1966. p. 171]. Flammable. May form an explosive mixture with air [Hawley].
Reactivity Profile
ZINC METAL is a reducing agent. Reacts violently with oxidants causing fire and explosion hazards [Handling Chemicals Safely 1980. p. 966]. In the presence of carbon, the combination of chlorine trifluoride with zinc results in a violent reaction [Mellor 2, Supp. 1: 1956]. Sodium peroxide oxidizes zinc with incandescence [Mellor 2:490-93 1946-47]. Zinc powder or dust in contact with acids forms hydrogen. The heat generated by the reaction is sufficient to ignite the hydrogen evolved [Lab. Govt. Chemist 1965]. A mixture of powdered zinc and an oxidizing agent such as potassium chlorate or powdered sulfur can be exploded by percussion. Zinc burns in moist chlorine. A mixture of zinc and carbon disulfide reacts with incandescence. Zinc powder reacts explosively when heated with manganese chloride. The reaction between zinc and selenium or tellurium is accompanied by incandescence [Mellor 4:476-480 1946-47]. When zinc and ammonium nitrate are mixed and wetted with a minimum of water, a violent reaction occurs with evolution of steam and zinc oxide. When hydrazine mononitrate is heated in contact with zinc a flaming decomposition occurs at temperatures a little above its melting point. Hydroxylamine is reduced when heated with ZINC, unpredictably ZINC may either ignite and burn or explode [Mellor 8 1946-47].
Hazard
As mentioned, zinc dust and powder are very explosive. When zinc shavings are placedin acid or strong alkaline solutions, hydrogen gas is produced, which may explode. Many ofzinc’s compounds are toxic if inhaled or ingested. A deficiency of zinc in humans will retard growth, both physically and mentally, andcontribute to anemia. It is present in many foods, particularly proteins (meat). A balanceddiet provides an adequate amount of zinc. Not more than 50 milligrams per day of dietaryzinc supplement should be taken, given that high levels of zinc in the body are toxic. Humanbodies contain about two grams of zinc. A deficiency of zinc can cause a lack of taste and candelay growth as well as cause retardation in children.Zinc intoxication can occur both from inhaling zinc fumes and particles, mainly in industrialprocesses, and from orally ingesting an excess of zinc in dietary supplements. Zinc intoxicationcan cause stomach pains, vomiting, and bleeding. Excess zinc also can cause prematurebirth in pregnant women.
Health Hazard
Zinc and its compounds are relatively non-toxic, but very large doses can produce an acute gastroenteritis characterized by nausea, vomiting, and diarrhea. The recommended dietary allowance (RDA) for zinc is 15 mg/day for men, 12 mg/day for women, 10 mg/day for children, and 5 mg/day for infants. Insuffi cient zinc in the diet can result in a loss of appetite, a decreased sense of taste and smell, slow wound healing and skin sores, or a damaged immune system. Pregnant women with low zinc intake have babies with growth retardation. Exposure to zinc in excess, however, can also be damaging to health. Harmful health effects generally begin at levels from 10–15 times the RDA (in the 100–250 mg/day range). Eating large amounts of zinc, even for a short time, can cause stomach cramps, nausea, and vomiting. Chronic exposures to zinc chloride fumes cause irritation, pulmonary edema, bronchopneumonia, pulmonary fi brosis, and cyanosis. It also causes anemia, pancreas damage, and lower levels of high-density lipoprotein cholesterol. Breathing large amounts of zinc (as dust or fumes) can cause a specifi c short-term disease, called metal fume fever, including disturbances in the adrenal secretion. Information on the possible toxicological effects following prolonged period of exposures to high concentrations of zinc is not known.
Fire Hazard
Produce flammable gases on contact with water. May ignite on contact with water or moist air. Some react vigorously or explosively on contact with water. May be ignited by heat, sparks or flames. May re-ignite after fire is extinguished. Some are transported in highly flammable liquids. Runoff may create fire or explosion hazard.
Flammability and Explosibility
Notclassified
Agricultural Uses
Zinc (Zn) is a bluish-white metal belonging to the 12th Group of the Periodic Table. It occurs naturally as sphalerite, smithsonite, hemimorphite and wurzite, and is extracted by roasting the oxide and reducing with carbon. It is used for galvanizing,
Pharmaceutical Applications
The average human body contains around 2 g of Zn2+. Therefore, zinc (after iron) is the second most abundant
d-block metal in the human body. Zinc occurs in the human body as Zn2+ (closed d10 shell configuration),
which forms diamagnetic and mainly colourless complexes. In biological systems, zinc ions are often
found as the active centre of enzymes, which can catalyse metabolism or degradation processes, and are
known to be essential for stabilising certain protein structures that are important for a variety of biological
processes.
Already from ancient times, Zn2+ was known to have important biological properties. Zinc-based
ointments were traditionally used for wound healing. Low Zn2+ concentrations can lead to a variety of
health-related problems especially in connection with biological systems of high Zn2+ demand such as the
reproductive system. The daily requirement for Zn2+ is between 3 and 25 mg, depending on the age and
circumstances.
The enzymatic function of Zn2+ is based on its Lewis acid activity, which are electron-deficient species. In the following chapters, examples will be shown to further explain this. Carboanhydrase (CA),carboxypeptidase and superoxide dismutase are some examples for well-studied zinc-containing enzymes.
The so-called zinc fingers have been discovered because of the crucial role of Zn2+ in the growth of organisms.
Within the zinc finger, Zn2+ stabilises the protein structure and therefore enables its biological function.
Industrial uses
Hot-dipped or galvanized zinc coatings havebeen popular for many years for protecting ferrousproducts because of their ideal combinationof high corrosion protection and low cost.Their corrosion protection stems from threeimportant factors:zinc has a slower rate ofcorrosion than iron,zinc corrosion productsare white and nonstaining, and zinc affordselectrolytic protection to iron. The amount of protection against corrosiondepends largely upon coating weight — theheavier the coating, the longer the life of the base metal. For example, a coating 0.04 mmthick is expected to have a life of 25 years inrural atmospheres, whereas a 0.88-mm coatingwill last 50 years. The life of zinc coatings maybe five to ten times greater in rural atmospheresthan in industrial atmospheres containing sulfurand acid gases. Nevertheless, the coatings arestill popular for industrial use because of theirlow cost.Hot dipping is particularly valuable for zinccoating parts that cannot conveniently be madeof galvanized sheet. Thus, it is quite popular forstructural parts, castings, bolts, nuts, nails, polelinehardware, heater and condenser coils,windlasses, and many other products.
Safety Profile
Human systemic effects
by ingestion: cough, dyspnea, and sweating.
A human skin irritant. Pure zinc powder,
dust, and fume are relatively nontoxic to
humans by inhalation. The dfficulty arises
from oxidation of zinc fumes immedately
prior to inhalation or presence of impurities
such as Cd, Sb, As, Pb. Inhalation may cause
sweet taste, throat dryness, cough, weakness,
generalized aches, chills, fever, nausea,
vomiting.
Flammable in the form of dust when
exposed to heat or flame. May i p t e
spontaneously in air when dry. Explosive in
the form of dust when reacted with acids.
Incompatible with NH4NO3, BaO2,
Ba(NO3)2, Cd, CS2, chlorates, Cl2, ClF3,
CrO3, (ethyl acetoacetate + tribromoneo-
pentyl alcohol), F2, hydrazine mononitrate,
hydroxylamine, Pb(N3)2, (Mg + Ba(NO3)2 +
BaO2), MnCl2, HNO3, performic acid,
KCLO3, KNO3, K2O2, Se, NaClO3, Na2O2,
S, Te, H2O2 (NH4)2S, As2O3, CS2, CaCl2,
NaOH, chlorinated rubber, catalytic metals,
halocarbons, o-nitroanisole, nitrobenzene,
nonmetals, oxidants, paint primer base,
pentacarbonyliron, transition metal halides,
seleninyl bromide. To fight fire, use special
mixtures of dry chemical. When heated to
decomposition it emits toxic fumes of ZnO.
See also ZINC COMPOUNDS.
Potential Exposure
Zinc is used most commonly as a
protective coating of other metals. In addition, it is
used in alloys, such as bronze and brass, for electrical
apparatus in many common goods; and in organic
chemical extractions and reductions. Zinc chloride is a
primary ingredient in smoke bombs used by military
for screening purposes, crowd dispersal and occasionally
in firefighting exercises by both military and civilian
communities. In pharmaceuticals, salts of zinc are
used as solubilizing agents in many drugs, including
insulin.
Carcinogenicity
Repeated intratesticular injections
of zinc chloride to chickens and rats have been reported
to produce testicular sarcomas. There is no evidence that zinc
compounds are carcinogenic after administration by any
other route. Zinc oxide, zinc chloride, and zinc stearate
have been classified by the U.S. EPAas belonging to group D.
Environmental Fate
Zinc enters the air, water, and soil as a result of both natural
processes and human activities. Most zinc enters the environment
as the result of human activities, such as mining, purifying
of zinc, lead, and cadmium ores, steel production, coal
burning, and burning of wastes. These releases can increase zinc
levels in the atmosphere. Waste streams from zinc and other
metal manufacturing and zinc chemical industries, domestic
wastewater, and runoff from soil containing zinc can discharge
zinc into waterways. The level of zinc in soil increases mainly
from disposal of zinc wastes from metal manufacturing
industries and coal ash from electric utilities. In air, zinc is
present mostly as fine dust particles. This dust eventually settles
over land and water. Rain and snow aid in removing zinc from
air. Most of the zinc in bodies of water, such as lakes or rivers,
settles on the bottom. However, a small amount may remain
either dissolved in water or as fine suspended particles. The
level of dissolved zinc in water may increase as the acidity of
water increases. Some fish can collect zinc in their bodies if they
live in water containing zinc. Most of the zinc in soil is bound
to the soil and does not dissolve in water. However, depending
on the characteristics of the soil, some zinc may reach
groundwater. Contamination of groundwater from hazardous
waste sites has been noticed. Zinc may be taken up by animals
eating soil or drinking water containing zinc. If other animals
eat these animals, they will also have increased amounts of zinc
in their bodies.
Shipping
UN1436 Zinc powder or zinc dust, Hazard
Class: 4.3; Labels: 4.3-Dangerous when wet material,
4.2-Spontaneously combustible material.
Purification Methods
Commercial zinc dust (1.2kg) is stirred with 2% HCl (3L) for 1minute, then the acid is removed by filtration, and washed in a 4L beaker with a 3L portion of 2% HCl, three 1L portions of distilled water, two 2L portions of 95% EtOH, and finally with 2L of absolute Et2O. (The wash solutions were removed each time by filtration.) The material is then dried thoroughly, and if necessary, any lumps are broken up in a mortar. [Wagenknecht & Juza Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol II p 1067 1965.]
Toxicity evaluation
Zinc is essential for humans and animals. It is necessary for
the function of numerous enzymes include alcohol dehydrogenase,
alkaline phosphatase, carbonic anhydrase, and
superoxide dismutase. However, excessive zinc interferes with
iron and copper metabolism; the latter leads to copper-deficiency
anemia. Salts of strong mineral acids are corrosive to
skin and intestine. Zinc also plays an essential role in the
maintenance of the nucleic acid structure of genes and an
integral component of DNA polymerase and RNA polymerase.
Yet, a limited amount of zinc consumed leads to zinc
deficiency. Zinc deficiency decreases the production of DNA
and RNA, which results in the reduction of protein synthesis.
Incompatibilities
Dust is pyrophoric and may self-ignite in
air. A strong reducing agent. Violent reaction with oxidizers,
chromic anhydride; manganese chloride; chlorates,
chlorine and magnesium. Reacts with water and reacts violently
with acids, alkali hydroxides; and bases forming
highly flammable hydrogen gas. Reacts violently with sulfur,
halogenated hydrocarbons and many other substances,
causing fire and explosion hazard.
Waste Disposal
Zinc powder should be
reclaimed. Unsalvageable waste may be buried in an
approved landfill. Leachate should be monitored for zinc
content.
Check Digit Verification of cas no
The CAS Registry Mumber 7440-66-6 includes 7 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 4 digits, 7,4,4 and 0 respectively; the second part has 2 digits, 6 and 6 respectively.
Calculate Digit Verification of CAS Registry Number 7440-66:
(6*7)+(5*4)+(4*4)+(3*0)+(2*6)+(1*6)=96
96 % 10 = 6
So 7440-66-6 is a valid CAS Registry Number.
InChI:InChI=1/Zn
7440-66-6Relevant articles and documents
Excitons and excitonic molecules in mixed Zn(P1-xAsx)2 crystals
Yeshchenko,Biliy,Yanchuk
, p. 231 - 238 (2001)
Low-temperature (1.8 K) excitonic absorption, reflection and photoluminescence spectra of mixed Zn(P1-xAsx)2 crystals have been studied at x = 0.01, 0.02, 0.03 and 0.05. Energy gap and rydbergs of excitonic B-, C- and A-series decrease monotonically with increasing of x. The spectral half-widths of the absorption n = 1 lines of the B- and A-series increase monotonically with increase in x due to fluctuations of crystal potential. Emission lines of excitonic molecules have been observed in photoluminescence spectra of Zn(P1-xAsx)2 crystals. The binding energy of the molecule increases with increase in x due to the decrease of the electron-hole mass ratio.
Investigation of Sn-Zn electrodeposition from acidic bath on EQCM
Arici, Mürsel,Nazir, Hasan,Aksu, M. Levent
, p. 1534 - 1537 (2011)
Tin-zinc (Sn-Zn) alloy with low tin content was deposited on gold electrode and steel substrate with use of chronoamperometric technique from an acidic bath. In order to evaluate coating efficiency of Sn-Zn alloy in 0.5 M NaCl solution, open circuit potential-time curve (EOCP-t), polarization curves, mass change of the electrode (Δm-t) using quartz crystal microbalance (QCM) were compared to those of pure Sn and Zn coatings. Anodic stripping measurements were carried out simultaneously with the mass loss of the deposit. Scanning electron microscopy (SEM) and energy dispersive X-ray spectra (EDS) analysis were performed to characterize the surface morphology. Anodic stripping experiment and EDS analysis indicated that Sn, Zn, and SnO2 formed on the electrode surface when Sn-Zn was coated from acidic bath. Furthermore, local mapping demonstrated homogeneous distribution of Sn and Zn atoms throughout the surface.
Electron-poor antimonides: Complex framework structures with narrow band gaps and low thermal conductivity
Haeussermann, Ulrich,Mikhaylushkin, Arkady S.
, p. 1036 - 1045 (2010)
Binary zinc and cadmium antimonides and their ternary relatives with indium display complex crystal structures, but reveal at the same time narrow band gaps in their electronic structure at or close to the Fermi level. It is argued that these systems represent electron-poor framework semiconductors (EPFS) with average valence electron concentrations between three and four. EPFS materials constituted of metal and semimetal atoms form a common, weakly polar framework containing multi-center bonded structural entities. The localized multi-center bonding feature is thought to be the key to structurally complex semiconductors. In this respect electron-poor antimonides become related to modifications of elemental boron. Electron-poor antimonides show promising thermoelectric properties, especially through a remarkably low thermal conductivity. At the same time the thermal stability of these compounds is rather limited because of temperature polymorphism and/or comparatively low melting or decomposition temperatures (usually below 600 K).
Activation of Reduction Agents. Sodium Hydride Containing Complex Reducing Agents. 18. Study of the Nature of Complex Reducing Agents Prepared from Nickel and Zinc Salts
Brunet, Jean-Jacques,Besozzi, Denis,Courtois, Alain,Caubere, Paul
, p. 7130 - 7135 (1982)
Complex reducing agents NaH-RONa-MXn (referred to as MCRA) are new versatile reagents that have already found many applications in organic synthesis.In the present study, the composition and structure of NiCRA and ZnCRA (CRA prepared from a nickel salt and a zinc salt, respectively) have been investigated.It has been found that, in both reagents, the metal (Ni or Zn) is formallly in a zero-valent oxidation state.The active part of NiCRA is constituted of new species (formed from Ni0 (1 equiv), RONa (R = t-Bu) (2 equiv), NaH (2 equiv), and maybe some AcONa) in which each constituent has lost its own characteristics.A picture of the structure of these new species is proposed.The composition of the active part of ZnCRA is less clear.Indeed, associations between RONa (R = t-Am) and Zn0 have been evidenced, but these species do not exhibit the reducing properties of ZnCRA, e.g., toward carbonyl compounds.In fact, control experiments have shown that no ketone reduction occured in the absence of NaH.These observations led us to propose that the active part of ZnCRA should be constituted of associations of the type n, which may be formed, in low concentration, from NaH and the inactive species n.
Unexpected visible light driven photocatalytic activity without cocatalysts and sacrificial reagents from a (GaN)1-: X(ZnO)x solid solution synthesized at high pressure over the entire composition range
Dharmagunawardhane, H. A. Naveen,James, Alwin,Wu, Qiyuan,Woerner, William R.,Palomino, Robert M.,Sinclair, Alexandra,Orlov, Alexander,Parise, John B.
, p. 8976 - 8982 (2018)
Optical and photocatalytic properties were determined for the solid solution series (GaN)1-x(ZnO)x synthesized at high pressure over the entire compositional range (x = 0.07 to 0.9). We report for the first time photocatalytic H2 evolution activity from water for (GaN)1-x(ZnO)x without cocatalysts, pH modifiers and sacrificial reagents. Syntheses were carried out by reacting GaN and ZnO in appropriate amounts at temperatures ranging from 1150 to 1200 °C, and at a pressure of 1 GPa. ZnGa2O4 was observed as a second phase, with the amount decreasing from 12.8 wt% at x = 0.07 to ~0.5 wt% at x = 0.9. The smallest band gap of 2.65 eV and the largest average photocatalytic H2 evolution rate of 2.31 μmol h-1 were observed at x = 0.51. Samples with x = 0.07, 0.24 and 0.76 have band gaps of 2.89 eV, 2.78 eV and 2.83 eV, and average hydrogen evolution rates of 1.8 μmol h-1, 0.55 μmol h-1 and 0.48 μmol h-1, respectively. The sample with x = 0.9 has a band gap of 2.82 eV, but did not evolve hydrogen. An extended photocatalytic test showed considerable reduction of activity over 20 hours.
PHOTOCATALYSIS OF ZINC SULFIDE MICROCRYSTALS IN REDUCTIVE HYDROGEN EVOLUTION IN WATER/METHANOL SYSTEMS
Yanagida, Shozo,Kawakami, Hiroshi,Hashimoto, Kazuhito,Sakata, Tadayoshi,Pac, Chyongjin,Sakurai, Hiroshi
, p. 1449 - 1452 (1984)
In photocatalytic H2 evolution using an aq. methanol system, high quality microcrystalline (cubic) ZnS powders have been found to be active under an appropriate light intensity, which is comparable in activity with freshly prepared ZnS suspensions.Compari
A method for covering a substrate with highly-oriented single crystalline hexagonal zinc structures under ambient pressure and room temperature
Cho, Seungho,Kim, Hye-Jin,Lee, Kun-Hong
, p. 6053 - 6055 (2009)
We report a novel method for covering a substrate with highly-oriented single crystalline hexagonal zinc structures under atmospheric pressure and room temperature without an external source of electric current, any templates or the use of epitaxial growt
Morphological evolution in zinc electrodeposition
Kahanda,Tomkiewicz
, p. 1497 - 1502 (1989)
We present an experimental study of the electrodeposition of zinc in a thin layer, three-electrode electrochemical cell. We show that as the steady-state current-potential behavior approaches mass transfer limited kinetics, the fractal dimension of the morphology of the deposit converges to the DLA value of 5/3. We also compare the evolution of the growth patterns with and without supporting electrolyte.
Breisch, K.
, p. 13 - 23 (1924)
Tunable Light Emission through the Range 1.8-3.2 eV and p-Type Conductivity at Room Temperature for Nitride Semiconductors, Ca(Mg1- xZn x)2N2 (x = 0-1)
Tsuji, Masatake,Hiramatsu, Hidenori,Hosono, Hideo
, p. 12311 - 12316 (2019)
The ternary nitride CaZn2N2, composed only of earth-abundant elements, is a novel semiconductor with a band gap of ~1.8 eV. First-principles calculations predict that continuous Mg substitution at the Zn site will change the optical band gap in a wide range from ~3.3-1.9 eV for Ca(Mg1-xZnx)2N2 (x = 0-1). In this study, we demonstrate that a solid-state reaction at ambient pressure and a high-pressure synthesis at 5 GPa produce x = 0 and 0.12 and 0.12 1-xZnx)2N2 converts its highly resistive state to a p-type conducting state. Particularly, the x = 0.50 sample exhibits intense green emission with a peak at 2.45 eV (506 nm) without any other emission from deep-level defects. These features meet the demands of III-V group nitride and arsenide/phosphide light-emitting semiconductors.
Electrochemical synthesis of zinc nanoparticles via a metal-ligand- coordinated vesicle phase
Gao, Yue,Hao, Jingcheng
, p. 9461 - 9471 (2009)
Two salt-free Zn2+-ligand-coordinated vesicle phases were prepared from the mixtures of alkyldimethylamine oxide (CnDMAO, n) 14 and 16, i.e., C14DMAO and C16DMAO) and zinc laurate [(CH3(CH2)10/s
New route for the synthesis of boron suboxide B7O
Liu,Zhao,Hou,Su
, p. L7-L9 (1995)
Boron suboxide B7O is synthesized with the aid of the oxidation of boron with zinc oxide ZnO under extreme conditions of high pressure, 3.50 GPa and high temperature, 1200 °C, and characterized by means of X-ray powder diffraction. This new rou
Synthesis and thermal characterization of zinc(II) di(o-aminobenzoate) complexes of imidazole and its methyl derivatives
Olczak-Kobza
, p. 67 - 71 (2004)
Mixed complexes of the type: Zn(Han)2(Him)3, Zn(Han)2(Him)5, Zn(Han)2(4-MeHim)2 and Zn(Han)2(1,2-diMeim)2 (where Han: NH2C 6H4COO
Electrocrystallisation of zinc from acidic sulphate baths; A nucleation and crystal growth process
Vasilakopoulos,Bouroushian,Spyrellis
, p. 2509 - 2514 (2009)
The electrochemical nucleation and growth of zinc on low-carbon steel from acidic (pH 2.0-4.5) baths containing ZnSO4, NaCl, and H3BO3, was studied by means of chronoamperometry at various cathodic potentials under a charg
Chromate conversion coatings formation on zinc studied by electrochemical and electrohydrodynamical impedances
Magalhaes,Tribollet,Mattos,Margarit,Barcia
, p. B16-B25 (2003)
The formation of chromate conversion coatings on zinc was studied by chronopotentiometric, electrochemical, and electrohydrodynamic impedances, and interfacial pH measurements. The electrochemical experiments were performed with a rotating disk electrode of pure zinc, and the pH measurements were obtained with a zinc deposit on a gold grid electrode in a submerged impinging jet cell. The electrolyte was an industrial chromate bath. The experimental results were achieved for different immersion times, temperatures, and rotation speeds. Kinetic reactions and physical model for the chromate layer formation on zinc were proposed, and the electrochemical and electrodynamic impedances were well simulated.
Clark, G. L.,Pish, G.,Weeg, L. E.
, p. 193 - 200 (1944)
Electrochemical preparation of porous copper surfaces in zinc chloride-1-ethyl-3-methyl imidazolium chloride ionic liquid
Lin, Yi-Wen,Tai, Chia-Cheng,Sun, I-Wen
, p. D316-D321 (2007)
The preparation of porous copper or copper-zinc surfaces by electrochemical formation of binary Cu-Zn alloys on Cu substrate and subsequent electrochemical etching of the zinc was investigated in a zinc chloride-1-ethyl-3- methylimidazolium chloride ionic liquid at 120°C. Cyclic voltammetry and X-ray diffraction measurements suggested that phase transformation from γ - to Β′ - Cu-Zn alloy occurred during constant potential dealloying. Essentially all the Zn content in the Cu-Zn could be removed from the alloy with dealloying at a sufficiently positive potential. Dealloyed materials exhibited well-developed bicontinuous porous structure. The dependence of the surface morphology of the porous Cu film on several experimental parameters, including deposition current and charge, and anodizing potential and temperature, were examined.
High-temperature decomposition of B-site-ordered perovskite Ba(Zn 1/2W1/2)O3
Jancar, Bostjan,Bezjak, Jana,Davies, Peter K.
, p. 758 - 764 (2010)
The reactions during high-temperature decomposition of Ba(Zn 1/2W1/2)O3 double perovskite, a potential microwave dielectric material, were studied by using X-ray diffraction, electron microscopy, and Knudsen effusion combined with mass spectrometry. The results show that above 1200°C, the perovskite decomposes due to the sublimation of ZnO, which results in the formation of BaWO4, Ba2WO 5, and amorphous BaO-rich phases. The simultaneous presence of BaWO4 and Ba2WO5 causes the formation of a liquid phase above 1320°C, which in the case of ceramics results in a progressive deterioration of the microstructure. As a consequence, the dielectric losses of Ba(Zn1/2W1/2)O3-based ceramics strongly depend on the processing parameters.
Zn electrodeposition in the presence of surfactants. Part I. Voltammetric and structural studies
Gomes,da Silva Pereira
, p. 863 - 871 (2006)
The zinc electrodeposition onto steel substrates in the presence of surfactants with different charged head groups, namely anionic sodium dodecylsulphate (SDS), cationic dodecyltrimethylammonium bromide (CTAB), and non-ionic octylphenolpoly(ethyleneglycolether)n, n = 10 (Triton X-100) was studied by cyclic voltammetry. The effect of the switching potential and scanning rate on the deposition process was investigated. The structural characterisation and the chemical composition of the samples prepared potentiostaticaly, in the potential range where the voltammetric cathodic peaks appear, was performed by X-ray powder diffraction (XRD) and by energy-dispersive X-ray analysis (EDS), respectively. The experimental results show that the voltammetric behaviour, namely the deposition potential depends on the presence, nature and concentration of the tested surfactants. Zn deposition occurs at potential values more positive than the estimated equilibrium potential, peak C1, simultaneously with hydrogen formation. This fact is confirmed by XRD measurements. Zn bulk deposits prepared in the absence of surfactants and in the presence of SDS are more crystalline and with a higher grain size than the ones obtained in the presence of CTAB and Triton X-100. These facts may be justified by an increase on the overpotential deposition as the electrochemical study confirms.
Schaffer, G. B.,McCormick, P. G.
, p. 45 - 46 (1989)
Trimetallic borohydride Li3MZn5(BH4) 15 (M = Mg, Mn) containing two weakly interconnected frameworks
Cerny, Radovan,Schouwink, Pascal,Sadikin, Yolanda,Stare, Katarina,Smrcok, L'Ubomir,Richter, Bo,Jensen, Torben R.
, p. 9941 - 9947 (2013)
The compounds, Li3MZn5(BH4)15, M = Mg and Mn, represent the first trimetallic borohydrides and are also new cationic solid solutions. These materials were prepared by mechanochemical synthesis from LiBH4, MCl2 or M(BH4) 2, and ZnCl2. The compounds are isostructural, and their crystal structure was characterized by in situ synchrotron radiation powder X-ray and neutron diffraction and DFT calculations. While diffraction provides an average view of the structure as hexagonal (a = 15.371(3), c = 8.586(2) A, space group P63/mcm for Mg-compound at room temperature), the DFT optimization of locally ordered models suggests a related ortho-hexagonal cell. Ordered models that maximize Mg-Mg separation have the lowest DFT energy, suggesting that the hexagonal structure seen by diffraction is a superposition of three such orthorhombic structures in three orientations along the hexagonal c-axis. No conclusion about the coherent length of the orthorhombic structure can be however done. The framework in Li 3MZn5(BH4)15 is of a new type. It contains channels built from face-sharing (BH4)6 octahedra. While X-ray and neutron powder diffraction preferentially localize lithium in the center of the octahedra, thus resulting in two weakly interconnected frameworks of a new type, the DFT calculations clearly favor lithium inside the shared triangular faces, leading to two interpenetrated mco-nets (mco-c type) with the basic tile being built from three tfa tiles, which is the framework type of the related bimetallic LiZn2(BH 4)5. The new borohydrides Li3MZn 5(BH4)15 are potentially interesting as solid-state electrolytes, if the lithium mobility within the octahedral channels is improved by disordering the site via heterovalent substitution. From a hydrogen storage point of view, their application seems to be limited as the compounds decompose to three known metal borohydrides.
Karschulin, M.,Ban, S.
, p. 244 - 247 (1940)
Ductility and crystallographic structure of zinc foils electrodeposited from acid zinc sulfate solutions
Ye,Celis,De Bonte,Roos
, p. 2698 - 2708 (1994)
A study of the relation between electrodeposition process parameters, structure and ductility of electrodeposited zinc foils was carried out. A stretching test was used to determine the ductility of zinc coatings after stripping them from the substrate. Depending on the relative texture coefficient coatings appeared to be more or less ductile. A loss of ductility when the pH of the electrolyte exceeds 4, was identified as due to zinc hydroxide precipitates. These particulates precipitate at the cathode and/or at the anode, then are transferred to the vicinity of the cathode where they can be codeposited with zinc.
Fabrication of a nanometric Zn dot by nonresonant near-field optical chemical-vapor deposition
Kawazoe, Tadashi,Yamamoto, Yoh,Ohtsu, Motoichi
, p. 1184 - 1186 (2001)
We demonstrate a technique for the deposition of nanometric Zn dots by photodissociation of gas-phase diethylzinc using an optical near field under nonresonant conditions. The observed deposited Zn dot was less than 50 nm in size. The photodissociation mechanisms are based on the unique properties of optical near fields, i.e., enhanced two-photon absorption, induced near-field transition, and a direct excitation of the vibration-dissociation mode of diethylzinc.
Density functional theory/B3LYP study of nanometric 4-(2,4-dihydroxy-5-formylphen-1-ylazo)-N-(4-methylpyrimidin-2-yl)benzenesulfonamide complexes: Quantitative structure–activity relationship, docking, spectral and biological investigations
Saad, Fawaz A.,Elghalban, Marwa G.,El-Metwaly, Nashwa M.,El-Ghamry, Hoda,Khedr, Abdalla M.
, (2017)
New metal ion complexes were isolated after coupling with 4-(2,4-dihydroxy-5-formylphen-1-ylazo)-N-(4-methylpyrimidin-2-yl)benzenesulfonamide (H2L) drug ligand. The structural and molecular formulae of drug derivative and its complexes were elucidated using spectral, analytical and theoretical tools. Vibrational spectral data proved that H2L behaves as a monobasic bidentate ligand through one nitrogen from azo group and ionized hydroxyl oxygen towards all metal ions. UV–visible and magnetic moment measurements indicated that Fe(III), Cr(III), Mn(II) and Ni(II) complexes have octahedral configuration whereas Cd(II), Zn(II) and Co(II) complexes are in tetrahedral form. The Cu(II)complex has square planar geometry as verified through electron spin resonance essential parameters. X-ray diffraction data indicated the amorphous nature of all compounds with no regular arrangement for the solid constituents during the precipitation process. Transmission electron microscopy images showed homogeneous metal ion distribution on the surface of the complexes with nanometric particles. Coats–Redfern equations were applied for calculating thermo-kinetic parameters for suitable thermal decomposition stages. Gaussian09 and quantitative structure–activity relationship modelling studies were used to verify the structural and biological features. Docking study using microorganism protein receptors was implemented to throw light on the biological behaviour of the proposed drug. The investigated ligand and metal complexes were screened for their in vitro antimicrobial activities against fungal and bacterial strains. The resulting data indicated that the investigated compounds are highly promising bactericides and fungicides. The antitumour activities of all compounds were evaluated towards human liver carcinoma (HEPG2) cell line.
Ultrasonic assisted preparation of some new zinc complexes of a new tetradentate Schiff base ligand: thermal analyses data, antimicrobial and DNA cleavage potential
Akbari, Zahra,Montazerozohori, Morteza,Hoseini, Seyed Jafar,Naghiha, Reza
, (2021/02/03)
A new tetradentate Schiff base ligand (L) (L = obtained by condensation reaction between triethylenetetraamine and (E)-3-(2-nitrophenyl)acrylaldehyde) and some of its zinc (II) complexes formulated as ZnLX2 in which X = halide/pseudohalide were synthesized and characterized by some physical and spectral techniques such as infra-red (IR), nuclear magnetic resonance (NMR), UV–Visible, microanalyses, and conductivity measurements. Among the complexes, zinc chloride, iodide, and nitrate complexes were also prepared as nanostructure powder under sonication conditions confirmed by x-ray diffraction (XRD), scanning electron microscopy (SEM), and energy dispersive x-ray analysis (EDAX). Moreover, zinc oxide nanoparticles were prepared by direct thermolysis of nanopowder of ZnLI2 complex under air atmosphere. Moreover, the thermal behaviors of the compounds were studied based on thermo-gravimetric (TG)/differential thermal gravimetric (DTG)/differential thermal analyses (DTA) analyses data under nitrogen atmosphere. Furthermore, antibacterial/antifungal activities of the ligand and its zinc complexes were screened by the well diffusion method against some bacteria and funguses. Ultimately, the DNA cleavage potential of the compounds was evaluated by gel electrophoresis technique.
Synthesis, Structural characterization, thermal, molecular modeling and biological studies of chalcone and Cr(III), Mn(II), Cu(II) Zn(II) and Cd(II) chelates
Diab, H. A.,El-Gamil, Mohammed M.,El-Nahass, Marwa N.,Fayed, Tarek A.,Gaber, M.
, (2020/07/13)
A number of new Cr(III), Mn(II), Cu(II) Zn(II) and Cd(II) chelates of (E)-3-(4-(dimethyl-amino)phenyl)-1-(pyridin-2-yl)prop-2-en-1-one were synthesized. The structures were elucidated by elemental and thermal analysis as well as spectral techniques (mass, IR, and electronic spectra) and magnetic measurements. The IR data suggested that the investigated chalcone acted as a bidentate ligand via the O and N atoms of the C[dbnd]O and C[dbnd]N groups, respectively. The spectral plus magnetic data revealed the formation of octahedral structures for all chelates while Cu(II) chelate has the square planar geometry. The kinetic and thermodynamic parameters of the thermal decomposition stages have been evaluated. Molecular orbital calculations have been performed to confirm the geometry of the isolated compounds. The in vitro antimicrobial activities of the chalcone and its metal chelates have been performed against some bacterial strains. The data indicated that all the metal chelates demonstrated a higher activity than the free chalcone. The anticancer activity of the mentioned metal chelates is evaluated against MCF7 cell. These compounds exhibited a moderate and weak activity against the tested cell line. The results were correlated with the experimental data.