7440-66-6

Zinc is one of the most common elements in the earth’s crust. Metal zinc was fi rst 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 sulfi de (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.

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.

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 DUST(7440-66-6), unpredictably ZINC DUST(7440-66-6) may either ignite and burn or explode [Mellor 8 1946-47].

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].

Inhalation or contact with vapors, substance or decomposition products may cause severe injury or death. May produce corrosive solutions on contact with water. Fire will produce irritating, corrosive and/or toxic gases. Runoff from fire control may cause pollution.

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.

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.

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.

If this chemical gets into the eyes, remove any contact lenses at once and irrigate immediately for at least 15 minutes, occasionally lifting upper and lower lids. Seek medical attention immediately. If this chemical contacts the skin, remove contaminated clothing and wash immediately with soap and water. Seek medical attention immediately. If this chemical has been inhaled, remove from exposure, begin rescue breathing (using universal precautions, including resuscitation mask) if breathing has stopped and CPR if heart action has stopped. Transfer promptly to a medical facility. When this chemical has been swallowed, get medical attention. Give large quantities of water and induce vomiting. Do not make an unconscious person vomit.

UN1436 Zinc powder or zinc dust, Hazard Class: 4.3; Labels: 4.3-Dangerous when wet material, 4.2-Spontaneously combustible material.

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.

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.

Zinc powder should be reclaimed. Unsalvageable waste may be buried in an approved landfill. Leachate should be monitored for zinc content.

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.

Although ancients used zinc compounds, the name “zinc” is assumed to be derived from the German word zinn, which was related to tin.

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.

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.

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.

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.

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.

Notclassified

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,

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.

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.

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.

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.

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.]

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.