7440-47-3 Usage
Introduction
Chromium occurs in the minerals chromite, FeO?Cr2O3 and crocoite, PbCrO4. The element is never found free in nature. Its abundance in earth's crust is estimated in the range 0.01% and its concentration in sea water is 0.3 μg/L. The element was discovered by Vaquelin in 1797.
The most important application of chromium is in the production of steel. High-carbon and other grades of ferro-chomium alloys are added to steel to improve mechanical properties, increase hardening, and enhance corrosion resistance. Chromium also is added to cobalt and nickel-base alloys for the same purpose.
Refractory bricks composed of oxides of magnesium, chromium, aluminum and iron and trace amounts of silica and calcium oxide are used in roofs of open hearths, sidewalls of electric furnaces and vacuum apparatus and copper converters. Such refractories are made in an arc furnace by fusing mixtures of magnesite and chrome ore.
Chromium coatings are applied on the surface of other metals for decorative purposes, to enhance resistance, and to lower the coefficient of friction. Radioactive chromium–51 is used as a tracer in the diagnosis of blood volume.
Chemical Properties
Different sources of media describe the Chemical Properties of 7440-47-3 differently. You can refer to the following data:
1. Chromium occurs in oxidation states from Cr-2 through Cr+6 but exists mainly in the Cr(III) and Cr(VI) states; Cr(III) is the most stable. Hexavalent chromium compounds have varying physical and chemical properties. Most Cr(VI) compounds are solids; chromyl chloride is a liquid. Their properties include corrosion-resistance, durability, and hardness. Sodium dichromate is the most common chromium chemical from which other Cr(VI) compounds are produced. Examples of other Cr(VI) compounds include sodium chromate, potassium dichromate, potassium chromate, ammonium dichromate, and chromic oxide.
The reduction of Cr(VI) to Cr(III) and the oxidation of Cr(III) to Cr(VI) are important sampling considerations when determining Cr(VI) levels in workplace air (Ashley et al., 2003). Factors that affect the reduction of Cr(VI) or oxidation of Cr(III) include the presence of other compounds in the sample (e.g., iron), the ratio of Cr(VI) to Cr(III) concentrations in the sample, and solution pH. The reduction of Cr(VI) is favored in acidic conditions while Cr(VI) is stabilized in basic conditions.
2. Chromium may exist in one of three valence states in compounds, , , and . The most stable oxidation state is trivalent chromium; Hexavalent chromium is a less stable state. Chromium (element) blue-white to steel-gray, lustrous, brittle, hard, odorless solid. Elemental:
Physical Properties
Hard blue-white metal; body-centered cubic crystal; density 7.19 g/cm3; melts at 1,875°C; vaporizes at 2,199°C; electrical resistivity at 20°C, 12.9 microhm–cm; magnetic susceptibility at 20°C, 3.6x10–6 emu; standard electrode potential 0.71 V (oxidation state 0 to +3).
Reactions
Chromium is oxidized readily in air forming a thin, adherent, transparent coating of Cr2O3.
Chromium forms both the chromous (Cr2+) and chromic (Cr3+) compounds that are highly colored.
Chromium metal reacts readily with dilute acids forming a blue Cr2+ (aq) solution with the evolution of hydrogen:
Cr + 2HCl → CrCl2 + H2
Chromium in metallic form and as Cr2+ ion are reducing agents. The Cr2+ reduces oxygen within minutes, forming violet Cr3+ ion:
4Cr2+(aq) + O2(g) + 4H+ (aq) → 4Cr3+ + 2H2O (l)
The standard redox potential for the overall reaction is 1.64V.
Cr3+ ion forms many stable complex ions. In the aqueous medium, it forms the violet Cr(H2O)63+ ion which is slightly basic. Chromium(III) ion is amphoteric, exhibiting both base and acid behavior.
Chromium reaction in an aqueous solution with a base produces a pale blue-violet precipitate having composition: Cr(H2O)3(OH)3.
Cr(H2O)63+ (aq) + 3OH– (aq) → Cr(H2O)3(OH)3 (s) + H2O
The above precipitate redissolves in excess base:
Cr(H2O)3(OH)3 (s) + H+ (aq) → Cr(H2O)4(OH)2+ (aq) + H2O
Chromium forms chromium(VI) oxide in which the metal is in +6 oxidation state. In acid medium it yields yellow chromate ion, CrO42–, and the redorange dichromate ion, Cr2O72–.
Chromium is oxidized in nitric, phosphoric or perchloric acid forming a thin oxide layer on its surface, thus making the metal even more unreactive to dilute acids.
Elemental chromium reacts with anhydrous halogens, hydrogen fluoride, and hydrogen chloride forming the corresponding chromium halides. At elevated temperatures in the range 600 to 700°C, chromium reacts with hydrogen sulfide or sulfur vapor, forming chromium sulfides.
Chromium metal reacts at 600 to 700°C with sulfur dioxide and caustic alkalis. It combines with phosphorus at 800°C. Reaction with ammonia at 850°C produces chromium nitride, CrN. Reaction with nitric oxide forms chromium nitride and chromium oxide.
5Cr + 3NO → 3CrN + Cr2O3
Production
Chromium metal is produced by thermal reduction of chromium(III) oxide, Cr2O3 by aluminum, silicon or carbon. The starting material in all these thermal reduction processes are Cr2O3 which is obtained from the natural ore chromite after the removal of iron oxide and other impurities. In the aluminum reduction process, the oxide is mixed with Al powder and ignited in a refractory-lined vessel. The heat of reaction is sufficient to sustain the reaction at the required high temperature. Chromium obtained is about 98% pure, containing traces of carbon, sulfur and nitrogen.
Cr2O3 + 2Al→ 2Cr + Al2O3
The carbon reduction process is carried out at 1,300 to 1,400°C at low pressure in a refractory reactor:
Cr2O3 + 3C→ 2Cr + 3CO
The silicon reduction process is not thermally self-sustaining and, therefore, is done in an electric arc furnace:
2Cr2O3 + 3Si → 4Cr + 3 SiO2
Chromium may be produced from high-carbon ferrochrome by electrolytic process. Alternatively, the metal may be obtained by electrolysis of chromic acid, H2CrO4.
High-carbon ferrochromium alloys are made by the reduction of chromite ore with carbon in an arc furnace. On the other hand, low-carbon ferrochromium is obtained by silicon reduction of the ore. The carbon content of ferrochromium can be reduced further by heating high-carbon alloys with ground quartzite or by oxidation in vacuum and removal of carbon monoxide formed. Ferrochromium alloys are used in the manufacture of stainless steel.
Toxicity
While chromium metal or trivalent chromium is not very toxic, hexavalent chromium (Cr6+) is carcinogenic and moderately toxic. Cr6+ is corrosive to skin and causes denaturation and precipitation of tissue proteins. Inhalation of Cr6+ dust or mist can cause perforation of the nasal septum, lung irritation, and congestion of the respiratory passsages. Chronic exposure may produce cancer of the respiratory tract.
Description
Chromium as a metallic element was first discovered over 200
years ago, in 1797. But the history of chromium really began
several decades before this. In 1761, in the Beresof Mines of the
Ural Mountains, Johann Gottlob Lehmann obtained samples
of an orange-red mineral, which he called ‘Siberian red lead.’
He analyzed this mineral in 1766 and discovered that it contained
lead “mineralized with a selenitic spar and iron particles.”
The mineral he found was crocoite, a lead chromate
(PbCrO4).
Physical properties
Chromium is a silvery white/gray, hard, brittle noncorrosive metal that has chemical andphysical properties similar to the two preceding elements in period 4 (V and Ti). As one of thetransition elements, its uses its M shell rather than its outer N shell for valence electrons whencombining with other elements. Its melting point is 1,857°C, its boiling point is 2,672°C,and its density is 7.19 g/cm3.
Isotopes
There are 26 isotopes of the element chromium; four are stable and foundin nature, and the rest are artificially produced with half-lives from a few microsecondsto a few days. The four stable isotopes and their percentage of contribution to thetotal amount of chromium on Earth are as follows: 50Cr = 4.345%, 52Cr = 83.789%,53Cr = 9.501%, and 54Cr = 2.365%. Cr-50 is radioactive but has such a long halflife—1.8×10+17 years—that it is considered to contribute about 4% to the total amount ofchromium found on Earth.
Origin of Name
From the Greek word chroma or chromos, meaning “color,” because of
the many colors of its minerals and compounds.
Occurrence
Chromium is the 21st most common element found in the Earth’s crust, and chromiumoxide (Cr2O3) is the 10th most abundant of the oxide compounds found on Earth. It is notfound in a free metallic state.The first source of chromium was found in the mineral crocoite. Today it is obtained fromthe mineral chromite (FeCr2O4), which is found in Cuba, Zimbabwe, South Africa, Turkey,Russia, and the Philippines. Chromite is an ordinary blackish substance that was ignored formany years. There are different grades and forms of chromium ores and compounds, based onthe classification of use of the element. Most oxides of chromium are found mixed with othermetals, such as iron, magnesium, or aluminum.Astronauts found that the moon’s basalt rocks contain several times more chromium thanis found in basalt rocks of Earth.
Characteristics
Chromium is a hard, brittle metal that, with difficulty, can be forged, rolled, and drawn,unless it is in a very pure form, in which case the chromium is easier to work with. It is anexcellent alloying metal with iron. Its bright, silvery property makes it an appropriate metal toprovide a reflective, non-corrosive attractive finish for electroplating.Various compounds of chromium exhibit vivid colors, such as red, chrome green, andchromate yellow, all used as pigments.
History
Chromium was discovered in 1797 by Vauquelin, who prepared
the metal the next year, chromium is a steel-gray, lustrous,
hard metal that takes a high polish. The principal ore is chromite
(FeCr2O4), which is found in Zimbabwe, Russia, South
Africa, Turkey, Iran, Albania, Finland, Democratic Republic
of Madagascar, the Philippines, and elsewhere. The U.S. has
no appreciable chromite ore reserves. Chromium is usually
produced by reducing the oxide with aluminum. Chromium
is used to harden steel, to manufacture stainless steel, and to
form many useful alloys. Much is used in plating to produce
a hard, beautiful surface and to prevent corrosion. Chromium
is used to give glass an emerald green color. It finds wide
use as a catalyst. All compounds of chromium are colored;
the most important are the chromates of sodium and potassium
(K2CrO4) and the dichromates (K2Cr2O7) and the potassium
and ammonium chrome alums, as KCr(SO4)2·12H2O.
The dichromates are used as oxidizing agents in quantitative
analysis, also in tanning leather. Other compounds are of industrial
value; lead chromate is chrome yellow, a valued pigment.
Chromium compounds are used in the textile industry
as mordants, and by the aircraft and other industries for anodizing
aluminum. The refractory industry has found chromite
useful for forming bricks and shapes, as it has a high melting
point, moderate thermal expansion, and stability of crystalline
structure. Chromium is an essential trace element for human
health. Many chromium compounds, however, are acutely or
chronically toxic, and some are carcinogenic. They should be
handled with proper safeguards. Natural chromium contains
four isotopes. Twenty other isotopes are known. Chromium
metal (99.95%) costs about $1000/kg. Commercial grade
chromium (99%) costs about $75/kg.
Uses
Different sources of media describe the Uses of 7440-47-3 differently. You can refer to the following data:
1. In manufacture of chrome-steel or chrome-nickel-steel alloys (stainless steel), nonferrous alloys, heat resistant bricks for refractory furnaces. To greatly increase strength, hardness and resistance of metals to abrasion, corrosion and oxidation. For chrome plating of other metals; leather tanning; as pigment and mordant; wood preservative. Use of 51Cr as diagnostic aid see sodium chromate(VI).
2. Chromium is used in the manufacture ofits alloys, such as chrome-steel or chromenickel-steel. It is also used for chromeplatingof other metals, for tanning leather,and in catalysts. It occurs in chromite ores(FeO·Cr2O3).
3. The best-known use of chromium is for the plating of metal and plastic parts to producea shiny, reflective finish on automobile trim, household appliances, and other items where abright finish is considered attractive. It also protects iron and steel from corrosion.It is used to make alloys, especially stainless steel for cookware, and items for whichstrength and protection from rusting and high heat are important.Its compounds are used for high-temperature electrical equipment, for tanning leather, asa mordant (fixes the dyes in textiles so that they will not run), and as an antichalking agentfor paints.Some research has shown that, even though most chromium compounds are toxic, a smalltrace of chromium is important for a healthy diet for humans. A deficiency produces diabeteslike symptoms, which can be treated with a diet of whole-grain cereal, liver, and brewer’s yeast.Chromium’s most important radioisotope is chromium-51, which has a half-life of about27 days. It is used as a radioisotope tracer to check the rate of blood flowing in constrictedarteries.Some chromium compounds (e.g., chromium chloride, chromic hydroxide, chromic phosphate) are used as catalysts for organic chemical reactions.In 1960 the first ruby laser was made from a ruby crystal of aluminum oxide (Al2O3). Thesecrystals contain only a small amount of chromium, which stores the energy and is responsiblefor the laser action. A small amount of chromium found in the mineral corundum is responsible for the bright red color of the ruby gemstone.
Production Methods
Chromium metal is prepared by reducing the ore in a blast furnace with carbon (coke) or silicon to form an alloy of chromium and iron called ferrochrome, which is used as the starting material for the many iron-containing alloys that employ chromium. Chromium to be used in iron-free alloys is obtained by reduction or electrolysis of chromium compounds.Chromiumisdif?culttoworkinthepuremetalform; it is brittle at low temperatures, and its high melting point makes it dif?cult to cast.
Definition
chromium: Symbol Cr. A hard silverytransition element; a.n. 24;r.a.m. 52.00; r.d. 7.19; m.p. 1857°C;b.p. 2672°C. The main ore ischromite (FeCr2O4). The metal has abody-centred-cubic structure. It is extractedby heating chromite withsodium chromate, from whichchromium can be obtained by electrolysis.Alternatively, chromite can be heated with carbon in an electricfurnace to give ferrochrome, whichis used in making alloy steels. Themetal is also used as a shiny decorativeelectroplated coating and in themanufacture of certain chromiumcompounds.At normal temperatures the metalis corrosion-resistant. It reacts withdilute hydrochloric and sulphuricacids to give chromium(II) salts.These readily oxidize to the more stablechromium(III) salts. Chromiumalso forms compounds with the +6oxidation state, as in chromates,which contain the CrO42- ion. The elementwas discovered in 1797 byVauquelin.
General Description
Very hard gray solid with a metallic luster.
Air & Water Reactions
May be pyrophoric, as dust. Insoluble in water.
Reactivity Profile
Chromium reacts violently with NH4NO3, N2O2, Li, NO, KClO3, SO2 . Metal dusts when suspended in atmospheres of carbon dioxide may ignite and explode.
Hazard
Different sources of media describe the Hazard of 7440-47-3 differently. You can refer to the following data:
1. Hexavalent chromium compounds are
questionable carcinogens and corrosive on tissue,
resulting in ulcers and dermatitis on prolonged contact.
2. Even though chromium may be a necessary trace element in our diets, many of its compounds are very toxic when ingested. Some are very explosive when shocked or heated (e.g., chromium nitrate) or when in contact with organic chemicals. Dust from the mining of chromium ores, which is found in igneous rocks, is carcinogenic and can cause lung cancer, even when small amounts are inhaled. Workers in industries that produce and use chromium are subject to bronchogenic cancer if precautions are not taken.
Health Hazard
The toxicity of chromium alloys and compoundsvaries significantly. Chromium metaldoes not exhibit toxicity. Divalent and trivalentcompounds of chromium have a loworder of toxicity. Exposure to the dusts ofchromite or ferrochrome alloys may causelung diseases, including pneumoconiosis andpulmonary fibrosis.Among all chromium compounds onlythe hexavalent salts are a prime health hazard.Cr6+ is more readily taken up bycells, than any other valence state of themetal. Occupational exposure to these compoundscan produce skin ulceration, dermatitis,perforation of the nasal septa, and kidneydamage. It can induce hypersensitivityreactions of the skin and renal tubular necrosis.Examples of hexavalent salts are thechromates and dichromates of sodium, potassium,and other metals. The water-solublehexavalent chromium salts are absorbed intothe bloodstream through inhalation. Manychromium(VI) compounds are carcinogenic,causing lung cancers in animals and humans.The carcinogenicity may be attributed tointracellular conversion of Cr6+ to Cr3+,which is biologically more active. The trivalentCr3+ ion can bind with nucleic acid andthus initiate carcinogenesis.Paustenbach et al. (1996) reported a casestudy on the uptake and elimination ofCr(VI) in drinking water on a male volunteerwho ingested 2 L/day of water containing2 mg/L Cr(VI) for 17 consecutivedays. The total chromium was measured inurine, plasma and red blood cells. The eliminationhalf-life in plasma was 36 hoursand the bioavailability was estimated as 2%.The steady-state chromium concentrations inurine and blood were achieved after sevendays of Cr(VI) ingestion. This study furthermorerevealed that Cr(VI) in drinkingwater at concentrations below 10 mg/L couldbe completely reduced to Cr(III) prior tosystemic distribution. In a follow-up study,Kergen et al. (1997) examined the magnitudeof absorption, distribution and excretionof Cr(VI) in drinking water in human volunteersfollowing oral exposures to singleand repeated doses at 5 and 10 mg Cr(VI)/L.The data obtained from this study indicatedthat virtually all (> 99.7%) of the ingestedCr(VI) was reduced to Cr(III) before enteringthe blood stream. No toxicity was observed.The endogenous reducing agents within theupper GI tract and the blood were attributedto reduce hexavalent chromium into its trivalentstate and, thus, prevented any systemicuptake of Cr(VI). Such reduction appearedto be effective even under the fasting conditions.Wise et al. (2002) investigated the cytotoxicityand clastogenicity of both water-insolubleand water-soluble Cr(VI) compounds in primaryhuman bronchial fibroblasts and foundthat they were overall cytotoxic and genotoxicto human lung cells. Although the genotoxicmechanisms of both may be mediated bysoluble Cr(VI) ions the water-insoluble saltsapparently are the potent carcinogens comparedto the water-soluble salts (Wise et al.2004). Exposure to Cr(VI) enhanced the bindingof polycyclic aromatic hydrocarbons toDNA in human lung cells (Feng et al. 2003).Hexavalent chromium has been found to besynergistic to benzo a pyrene diol epoxide onmutagenesis and cell transformation.The catalytic effect of iron on enhancingthe rate of reduction of Cr(VI) byhuman microsomes has been reported earlier(Myers and Myers 1998). Various formsof exogenous iron markedly enhanced bothliver and lung microsomal rates of Cr(VI)reduction. Small increases in intracellulariron have shown to cause large increases inin the rate and extent of Cr(VI) reduction.Thus, individuals exposed simultaneously toCr(VI) and agents that may increase intracellulariron could, therefore, be at potentiallygreater risk for toxicity and carcinogenicityof Cr(VI).
Fire Hazard
Non-combustible, substance itself does not burn but may decompose upon heating to produce corrosive and/or toxic fumes. Some are oxidizers and may ignite combustibles (wood, paper, oil, clothing, etc.). Contact with metals may evolve flammable hydrogen gas. Containers may explode when heated.
Industrial uses
An elementary metal, chromium (symbol Cr)is used in stainless steels, heat-resistant alloys,high-strength alloy steels, electrical-resistancealloys, wear-resistant and decorative electroplating,and, in its compounds, for pigments,chemicals, and refractories. The specific gravityis 6.92, melting point 1510°C, and boiling point2200°C. The color is silvery white with a bluishtinge. It is an extremely hard metal; the electrodepositedplates have a hardness of 9 Mohs.It is resistant to oxidation, is inert to HNO3, butdissolves in HCl and slowly in H2SO4. At temperaturesabove 816°C, it is subject to intergranularcorrosion.Chromium occurs in nature only in combination.Its chief ore is chromite, from which itis obtained by reduction and electrolysis. It ismarketed for use principally in the form of masteralloys with iron or copper.Most pure chromium is used for alloyingpurposes such as the production of Ni–Cr orother nonferrous alloys where the use of thecheaper ferrochrome grades of metal is not possible.In metallurgical operations such as theproduction of low-alloy and stainless steels, thechromium is added in the form of ferrochrome,an electric-arc furnace product that is the formin which most chromium is consumed.Its bright color and resistance to corrosion makechromium highly desirable for plating plumbingfixtures, automobile radiators and bumpers,and other decorative pieces. Unfortunately,chrome plating is difficult and expensive. Itmust be done by electrolytic reduction ofdichromate in H2SO4 solution. It is customary,therefore, to first plate the object with copper,then with nickel, and finally, with chromium.
Potential Exposure
Chromium metal is used in stainless and other alloy steels to impart resistance to corrosion, oxidation, and for greatly increasing the durability of metals; for chrome plating of other metals.
Veterinary Drugs and Treatments
Chromium supplementation may be useful in the adjunctive treatment
of diabetes mellitus or obesity, particularly in cats; there is
controversy whether this treatment is beneficial. It does not appear
to be useful in dogs with diabetes mellitus.
Carcinogenicity
Exposure to chromium compounds over a prolonged period has been observed in manyepidemiologicalstudiestoenhancetheriskofcancerof the respiratory organs among the exposed. The relationshipbetweenemploymentinindustriesproducingchromium compounds from chromite ore and enhanced risk of lungcancer iswell established.There isagreement inseveral studies that long-term exposure to some chromium-based pigments enhance the risk of lung cancer. An association has alsobeenobservedbetweenexposuretochromicacidinhard plating and lung cancer, but that association is not strong. Somestudieshaveweaklyindicatedexcessesofcancerofthe GItract,buttheresultsareinconsistentandarenotcon?rmed inwell-designedstudies.Thereisnoindicationthatchromite ore does have an associated enhanced risk of cancer. Although it has not yet been identi?ed which chromium compound (or compounds) is (are) responsible for enhanced risk of cancer in respiratory organs, there is general agreementthatitisthechromium(6+)speciesthatareresponsible for the elevated cancer risks and that the chromium species are not.
Environmental Fate
Chromium is distributed to the air, water, and soil from natural and anthropogenic sources. The environmental fate of chromium is dependent on the oxidation state and solubility of the compound and the environmental conditions affecting reduction or oxidation, such as pH. Oxidizing conditions favor the formation of Cr(VI) compounds, particularly at higher temperatures, while reducing conditions favor the formation of Cr(III) compounds. Chemical manufacturing and natural gas, oil, and gas combustion are the primary sources of chromium in the atmosphere.Most of the chromium in air eventually ends up in water or soil. Electroplating, textile manufacturing, cooling water, and leather tanning are major sources of chromium in wastewater discharges to surface waters. Chromium(III) is the predominant oxidation state of chromium in many soils. Cr(III) binds to soil and has low mobility. A lower soil pH favors the reduction of Cr(VI) to Cr(III). Runoff from soil and industrial processes may transport chromium to surface water.Cr(VI) compounds may leach into groundwater. The pH of the soil and aquatic environment is an important factor in chromium mobility, bioavailability, and toxicity. The chromate form predominates in most natural surface waters that are basic or neutral. The hydrochromate concentration increases in more acidic conditions.
Shipping
UN3089 Metal powders, flammable, n.o.s., Hazard Class: 4.1; Labels: 4.1-Flammable solid. UN1759 Corrosive solids, n.o.s., Hazard class: 8; Labels: 8-Corrosive material, Technical Name required
Toxicity evaluation
Chromium enters the air, water, and soil mostly in the chromium(
III) and chromium(VI) forms. In air, chromium
compounds are present mostly as fine dust particles, which
eventually settle over land and water. Chromium can strongly
attach to sediment and soil, and only a small amount is
expected to dissolve in water and leach though the soil to
groundwater. Fish do not accumulate much chromium in their
bodies.Most chromium exposure in the general population is
through ingestion of the chemical in food containing chromium(
II), although exposure is also possible as a result of
drinking contaminated well water, or living near uncontrolled
hazardous waste sites containing chromium or industries that
use chromium. Inhalation of chromium dust and skin contact
during use in the workplace are the main routes of occupational
exposure.
Incompatibilities
Dust may be pyrophoric in air. Chromium metal (especially in finely divided or powder form) and insoluble salts reacts violently with strong oxidants, such as hydrogen peroxide, causing fire and explosion hazard. Reacts with diluted hydrochloric and sulfuric acids. Incompatible with alkalis and alkali carbonates
Waste Disposal
Recovery and recycling is a viable alternative to disposal for chromium in plating wastes; tannery wastes; cooling tower blowdown water and chemical plant wastes.
Check Digit Verification of cas no
The CAS Registry Mumber 7440-47-3 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, 4 and 7 respectively.
Calculate Digit Verification of CAS Registry Number 7440-47:
(6*7)+(5*4)+(4*4)+(3*0)+(2*4)+(1*7)=93
93 % 10 = 3
So 7440-47-3 is a valid CAS Registry Number.
InChI:InChI=1/Cr
7440-47-3Relevant articles and documents
Tyndall, George W.,Jackson, Robert L.
, p. 582 - 583 (1987)
Electrolytic preparation and characterization of VCr alloys in molten salt from vanadium slag
Liu, Shiyuan,Wang, Lijun,Chou, Kuo-chih,Kumar, Ramachandran Vasant
, p. 875 - 881 (2019)
Vanadium slag contains several critical elements like V, Ti, Cr, Fe and Mn. In our previous work, V and Cr have been enriched by selective chlorination, increasing from 10.05% to 14.95% and 5.84%–8.69% separately. V and Cr still maintain the trivalence state in molten salt. In the current work, the electrodeposition behaviors of V3+ and Cr3+ in NaCl–KCl molten salt at 800 °C were investigated using cyclic voltammetry (CV) and square wave voltammetry (SWV) with a tungsten electrode. It was found that the reduction processes of V3+ and Cr3+ consist of two steps, M3+/M2+, M2+/M. The diffusion coefficients of V3+ and Cr3+ in NaCl–KCl molten salt were measured by CV. The effect of VCl3/CrCl3 mass ratio on VCr alloy was investigated by a two-electrode under constant voltage. Pure Cr can be obtained at 2.8 V in the NaCl–KCl molten salt, while VCr alloy (3.71 mass % V-94.28 mass% Cr-2.01 mass % O) was obtained when electrolysis voltage was controlled to 2.8 V at 800 °C. The composition of VCr alloy can be designed by changing the molten salt composition. This method can be applied for direct preparation of VCr alloy from vanadium slag, thus offering the use of low cost raw materials with direct environmental benefits.
Reactions of Cr atoms with NO, N2O, CO2, NO 2, and SO2 molecules
Smirnov,Akhmadov
, p. 617 - 623 (2010)
Experimental results on the interaction of Cr atoms with various oxygen-containing molecules (NO, N2O, CO2, NO2, and SO2) at high temperatures (>1000 K) are presented. It is demonstrated that activation barrier
Fabrication and characterization of electrodeposited Co1-xCrx nanowires
Chaure,Coey
, p. 232 - 236 (2006)
Co1-xCrx alloy nanowires with 0.0 1 a porous alumina membrane from an electrolyte containing Co and Cr ions. The composition, structure and magnetic properties of the nanowires have been characterized. Cobalt-rich nanowires were electrodeposited at a potential of -1.0 V relative to Ag/AgCl and chromium-rich nanowires were deposited beyond -3.5 V. The optimized processing conditions include hydrogen annealing to give hysteresis loops for the Co80Cr20 nanowires with coercivity of up to 200 mT and squareness of up to 0.95. Magnetization of the Co80Cr20 nanowire is 77 A m2 kg-1 and the energy product of the arrays is 35 kJ m-3.
Valence-to-core X-ray emission spectroscopy identification of carbide compounds in nanocrystalline Cr coatings deposited from Cr(III) electrolytes containing organic substances
Safonov, Viktor A.,Vykhodtseva, Ludmila N.,Polukarov, Yurii M.,Safonova, Olga V.,Smolentsev, Grigory,Sikora, Marcin,Eeckhout, Sigrid G.,Glatzel, Pieter
, p. 23192 - 23196 (2006)
Valence-to-core X-ray emission spectroscopy was applied to study a composition of chromium coatings electrodeposited from Cr(III) sulfate electrolytes with the addition of formic or oxalic acid. It was shown that the obtained crystallographically amorphous deposits contain chromium carbide compounds. These results indicate that nanodimensional Cr crystallites formed during the electrodeposition process are characterized by very high electrocatalytic activity.
Thermal studies of chromium, molybdenum and ruthenium complexes of chloranilic acid
Soliman,Ali,Khalil,Ramadan
, p. 37 - 42 (2000)
Chromium, molybdenum and ruthenium complexes of chloranilic acid (H2CA) were investigated by the thermogravimetric (TG) technique. The TG plot of Cr(H2CA)3 showed three decompositions in the temperature range 336-802°K. On
Chirnside, R. C.,Dauncey, L. A.,Proffitt, P. M. C.
, p. 175 - 180 (1943)
Cheung, Nai-Ho,Yeung, Edward S.
, p. 164 - 170 (1992)
Physicochemical model for choosing complexes for chromium-plating solutions based on Cr(III) compounds
Vinokurov,Demidov,Bondar'
, p. 14 - 18 (2005)
A prognostic physicochemical model for choosing complexes for chromium-plating solutions is constructed on the basis of a combination of the thermodynamic principles and data on the kinetics of some electrochemical reactions. It is shown that high-quality chromium coating can be produced from solutions of Cr(III) complexes, whose logarithm of stability constants ranges from 10 to 20, and the logarithm of stability constants of Cr(II) complexes formed in electrolysis ranges from 7 to 10. The influence of the nature of ligands on chromium electrodeposition is studied. Using the model proposed, a chromium-plating solution based on a chromium(III) malonate complex is developed. This solution makes it possible to produce high-quality coatings in a wide interval of current densities.
Bevan, D. J. M.,Kordis, J.
, p. 1509 - 1523 (1964)
Barker, Marten G.,Hooper, Alan J.
, (1976)
Nano-synthesis, characterization, modeling and molecular docking analysis of Mn (II), Co (II), Cr (III) and Cu (II) complexes with azo pyrazolone ligand as new favorable antimicrobial and antitumor agents
Gaber, Mohamed,Khedr, Abdalla M.,Mansour, Mohammed A.,Elsharkawy, Mohsen
, (2018)
Novel nanosized Mn (II), Co (II), Cr (III) and Cu (II) complexes were synthesized with 2-((5-oxo-1,3-diphenyl-4,5-dihydro-1H-pyrazol-4-yl)diazenyl) benzoic acid, HL applying precipitation method. Their structures were characterized based on the elemental and thermal analyses, spectra (FT-IR, UV–Vis, MS, ESR and XRD), conductivity and magnetic moment measurements. IR spectra offered that HL behaves as monobasic tri-dentate ligand towards Mn (II), Cr (III) and Cu (II) and monobasic bi-dentate towards Co (II). The XRD results unambiguously confirmed the crystalline nature and nano-sized particles of Cu (II) complex while HL and other complexes exhibited amorphous phases. The magnetic moment data, UV–Vis and ESR spectra supported the formation of octahedral geometries for Mn (II), and Cr (III) complexes, whereas Co (II), and Cu (II) complexes showed tetrahedral arrangement. The activation parameters for the thermal degradation stages were theoretically calculated using TGA curves. The obtained data showed the inspected complexes as favorable antimicrobial drug candidates. The studied compounds were screened out for their antitumor and antimicrobial activities. The inspected compounds exhibited a reasonable antibacterial activity and weak antitumor efficacy. The in vitro results were confirmed using the in silico molecular docking analysis (docking server) applying x-ray crystallographic structures of the proteins (4?m01, 3?t88, 1zap & 4ynt) from PDB (Protein Data Bank). HL and probably its complexes displayed adequate binding with the receptors of 4?m01, 3?t88, 1zap, and 4ynt microorganisms. The obtained data show the inspected complexes as favorable antimicrobial drug candidates.
INTERACTION OF TRIETHYLALUMINIUM WITH ACETYLACETONATES OF TRANSITION METALS
Schmidt, F. K.,Ratovskii, G. V.,Dmitrieva, T. V.,Ivleva, I. N.,Borodko, Yu. G.
, p. 309 - 330 (1983)
The reaction of AlEt3 with acetylacetonates of CrIII, FeIII, CoIII, NiII and PdII in benzene and cyclohexane has been studied in a wide range of initial ratios of AlEt3/M(acac)n.Quantitative analysis of the reaction mixture, performed with the help of UV spectra, showed that acetylacetonate ligands were transferred from the transition metals to aluminium.A scheme involving stepwise substitution of ethyl radicals by acetylacetonate ligands on AlEt3 with further formation of an Al(acac)3Et2Al(acac) mixture is proposed for Al/M III, CoIII, NiII were reduced to the zerovalent state in their reaction with AlEt3 (Al/Mn n).The content of the finely dispersed metal component is negligible small and the greater part of transition metal is present as M0 complexes, where Et2Al(acac) formed in the reaction is the main stabilizing ligand.
Electrochemical corrosion behavior of carbon nanotube-doped hard chromium coatings electrodeposited from Cr(III) baths
Zeng, Zhixiang,Yu, Yuanlie,Zhang, Junyan
, p. C123-C126 (2009)
Homogeneous chromium-multiwalled carbon nanotube (Cr-MWNT) composite coatings were electrodeposited from trivalent chromium [Cr(III)] electrolyte containing MWNTs under ultrasonic agitation. The microstructure, mechanical properties, and electrochemical c
Coordination modes of multidentate azodye ligand derived from 4,4′-methylenedianiline towards some transition metal ions: Synthesis, spectral characterization, thermal investigation and biological activity
Abouel-Enein, Saeyda A.,Emam, Sanaa M.,Monir, Eman
, (2018/01/27)
Nine new azodye metal complexes of Mn(II), Co(II), Ni(II), Cu(II), Cr(III), Fe(III), Ru(III), Hf(IV) and Zr(IV) ions have been prepared via the reaction of 5,5′-((1E,1′E)-(methylenebis(1,4-phenylene))bis(diazene-2,1-diyl))bis(6-hydroxy-2-thioxo-2,3-dihydropyrimidin-4(5H)-one) (H4L) with the corresponding metal salts affording sandwich (1?L:1?M), mononuclear (2?L:1?M), binuclear (1?L,2?M) and tetranuclear (1?L,4?M) complexes. Elemental analyses, spectral methods, magnetic moment measurements and thermal studies were utilized to confirm the mode of bonding and geometrical structure for the ligand and its metal complexes. Infrared spectral data show that the H4L ligand chelates with some metal ions in keto–enol–thione or keto–thione manner. It behaves in a neutral/dibasic tetradentate fashion in sandwich and binuclear complexes. Also, it acts as a neutral bidentate moiety in the Cr(III) complex. The spectra reveal that azo group participates in chelation in all complexes. Octahedral geometry was suggested for all chelates but the Cu(II) complex with square planar geometry. The thermal stability and decomposition of the compounds were studied, the data showing that the thermal decomposition ended with metal or metal oxide mixed with carbon as final product. The electron spin resonance spectrum of the Cu(II) complex demonstrates that the free electron is located in the (d x2-y2) orbital. Measurements of biological activity against human cell lines Hep-G2 and MCF-7 reveal that the Cu(II) complex has a higher cytotoxicity in comparison to the free ligand and other metal complexes, with IC50 values of 6.10 and 5.2 μg ml?1, respectively, while the ligand has anti-tumour activity relative to some of the investigated metal complexes.
Fabrication and characterization of thermoelectric CrSi2 compound by mechanical alloying and spark plasma sintering
Lee, Chung-Hyo
, p. 5070 - 5073 (2015/03/03)
A mixture of elemental Cr-Si powders has been subjected to mechanical alloying (MA) at room temperature to prepare CrSi2 thermoelectric compound.The MA powders were sintered at 800-1000?°C Cunder 60 MPa using spark plasma sintering (SPS) technique. Due to the observed larger loss of Si relative Cr during ball milling, the starting composition was modified to Cr30Si70, Cr31.5Si68.5 and Cr33Si67 to get a single phase of CrSi2 compound. The single phase CrSi2 has been obtained by MA of Cr31.5Si68.5 mixture powders for 70 h and subsequently sintered at 1000?°C. X-ray diffraction data shows that the SPS compact sintered at 1000?°C consists of only nanocrystalline CrSi2 compound with a grain size of 250 nm. The value of Seebeck coefficient of CrSi2 compound increases with temperature and reaches maximum value of 245 ??V/K at 300?°C.