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GALLIUM

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Products Intro: Product Name:GALLIUM
CAS:7440-55-3
Purity:99% Package:100g,500g,1kg,5kg,10kg
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CAS:7440-55-3
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CAS:7440-55-3
Purity:99.9% Package:50g;1USD
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Products Intro: Product Name:Gallium, 99.99%, trace metal basis
CAS:7440-55-3
Purity:99.99% Package:10G;50G

Lastest Price from GALLIUM manufacturers

  • GALLIUM
  • US $1.00 / g
  • 2018-12-19
  • CAS:7440-55-3
  • Min. Order: 50 g
  • Purity: 99.9%
  • Supply Ability: 20kg
GALLIUM Basic information
History and occurrence Physical Properties Uses Production Chemical Reactions
Product Name:GALLIUM
Synonyms:GALLIUM, 99.99% METALS BASIS;Gallium,ElectronicGrade;Gallium, 99.99%;Gallium, 99.9999%;GALLIUM67;GALLIUM: 99.9999% MELT;GALLIUM METAL: 99.99%, 4N;GALLIUM METAL: 99.9999%, 6N
CAS:7440-55-3
MF:Ga
MW:69.72
EINECS:231-163-8
Product Categories:Inorganics;Gallium;Metal and Ceramic Science;Metals;AA Standard SolutionsAnalytical Standards;GSpectroscopy;AAS;Alphabetic;Matrix Selection;NitrateSpectroscopy;Reference/Calibration Standards;Single Solution;Standard Solutions;Analytical Standards;metal or element;GApplication CRMs;ICP CRMs;ICP-OES/-MS;ICPSpectroscopy;Spectroscopy
Mol File:7440-55-3.mol
GALLIUM Structure
GALLIUM Chemical Properties
Melting point 29.8 °C(lit.)
Boiling point 2403 °C(lit.)
density 5.904 g/mL at 25 °C(lit.)
storage temp. 0-6°C
form Solid and/or Liquid
color Silvery or grayish metallic
Specific Gravity5.904
resistivity25.795 μΩ-cm, 30°C
Water Solubility reacts with alkalies to evolve H2 [MER06]
Sensitive air sensitive, moisture sensitive
Merck 13,4367
Stability:Stable, but moisture sensitive. Incompatible with strong acids, strong bases, halogens, strong oxidizing agents.
CAS DataBase Reference7440-55-3(CAS DataBase Reference)
Safety Information
Hazard Codes C,Xi,T
Risk Statements 36/38-34-23/24/25
Safety Statements 26-45-36/37/39-36-28-27
RIDADR UN 3264 8/PG 3
WGK Germany 3
RTECS LW8600000
TSCA Yes
HazardClass 8
PackingGroup III
HS Code 81129290
MSDS Information
ProviderLanguage
SigmaAldrich English
ACROS English
ALFA English
GALLIUM Usage And Synthesis
History and occurrenceThe existence of this element was predicted by Mendeleev as a missing link between aluminum and indium during his periodic classification of elements. Mendeleev termed it ekaaluminum. The element was discovered in 1875 by French chemist Lecoq de Boisbaudran while he was carrying out spectroscopic examination of emission lines from Pyrenean zinc blende concentrates. Boisbaudran named this new element gallium, after Gallia, the Latin word for his native France. In the same year, Boisbaudran also separated gallium by electrolysis.
Gallium is widely distributed in nature, mostly found in trace amounts in many minerals including sphalerite, diaspore, bauxite, and germanite. It is found in all aluminum ores. Gallium sulfide occurs in several zinc and germanium ores in trace amounts. It also is often found in flue dusts from burning coal. Abundance of this element in the earth’s crust is about 19 mg/kg. Its average concentration in sea water is 30 ng/L.
Physical PropertiesGray orthogonal crystal or silvery liquid; the ultrapure material has silverlike appearance; density of solid 5.904 g/cm3 at 29.6°C; specific gravity of liquid 6.095 at 29.6°C; melts near room temperature at 29.6°C; supercools below its freezing point (seeding may be required for solidification); expands on solidification (3.1%); vaporizes at 2,204°C; exists in liquid state in the widest temperature range (i.e., among all elements gallium occurs as liquid in the widest range of temperature); vapor pressure 0.0001 torr at 900°C (lowest vapor pressure for any element in liquid state at this temperature), 0.0008 torr at 1,000°C, 1 torr at 1,350°C, and 5 torr at 1,478°C; surface tension 735 dynes/cm at 30°C; viscosity 1.60 and 0.81 centipoise at 100°C and 500°C, respectively.
UsesThe most important use of gallium is as a doping agent for semiconductors, transistors, and other solid state devices. It is used to produce semiconducting compounds. Miscellaneous important semiconductor applications include magnetic field sensing, temperature sensing, and voltage amplification. Some gallium compounds, such as gallium arsenide, gallium phosphide, and magnesium gallate have major applications in electroluminescent light emission, microwave generation, and UV activated powder phosphors. Another important use of gallium in oxide form involves spectroscopic analysis of uranium oxide. Gallium also is used to make many low melting alloys. Some other uses for gallium are in high-temperature thermometers as a thermometric fluid; in high vacuum systems as a liquid sealant; as a heat-transfer medium; and to produce mirrors on glass surfaces.
ProductionAll gallium minerals contain the element only in very small amounts. It is, therefore, obtained as a by-product during production of aluminum or zinc.
Gallium occurs as a hydrated oxide (hydroxide) in all aluminum minerals including bauxite, clay, and laterite. The ore is digested with a hot solution of caustic soda (Bayer process). This converts aluminum to sodium aluminate and the small quantities of gallium that are present in the ore into sodium gallate. On cooling and seeding the liquor most aluminum salt precipitates along with small quantities of gallum as coprecipitate. After aluminum separates, the supernatant solution becomes richer in gallium. Its concentration even at this stage is not adequate for electrolytic recovery from the solution.
Also, supernatant solution in the Bayer liquor still contains an appreciable amount of soluble aluminum salt that needs to be removed by electrolysis prior to gallium recovery. This may be done either by treating the solution with lime to precipitate out calcium aluminate or by neutralizing the solution with carbon dioxide to precipitate alumina hydrate (Hudson, L.K. 1965. J. Metals, 17, pp. 948-51). Removal of most aluminum by these processes enhances the concentration of gallium in the solution to a level of approximately 0.1% whereupon the solution may be electrolyzed using an anode, cathode, and cell made of stainless steel.
Chemical ReactionsChemical properties of gallium fall between those of aluminum and indium. It forms mostly the binary and oxo compounds in +3 oxidation state. It forms a stable oxide, Ga2O3 and a relatively volatile suboxide, Ga2O.
Gallium combines with halogens forming the halides, GaX3. Similarly, it combines with phosphorus, arsenic and antimony forming the corresponding binary compounds, which exhibit interesting semiconductor properties. With sulfur it forms sulfide. No reaction occurs with bismuth, although Ga dissolves in it. Reaction with nitrogen occurs at high temperatures forming gallium nitride, GaN, which is relatively unstable (decomposes above 600°C). Unlike aluminum, gallium does not form any carbide. Reactions with mineral acids are slow on high purity gallium.
Chemical Propertieslight grey solid
Chemical PropertiesGallium is a lustrous, silvery liquid, metal, or gray solid.
HistoryGallium was predicted and described by Mendeleev as ekaaluminum, and discovered spectroscopically by Lecoq de Boisbaudran in 1875, who in the same year obtained the free metal by electrolysis of a solution of the hydroxide in KOH, it is often found as a trace element in diaspore, sphalerite, germanite, bauxite, and coal. Some flue dusts from burning coal have been shown to contain as much as 1.5% gallium. Gallium is the only metal, except for mercury, cesium, and rubidium, which can be liquid near room temperatures; this makes possible its use in high-temperature thermometers. It has one of the longest liquid ranges of any metal and has a low vapor pressure even at high temperatures. There is a strong tendency for gallium to supercool below its freezing point. Therefore, seeding may be necessary to initiate solidification. Ultra-pure gallium has a beautiful, silvery appearance, and the solid metal exhibits a conchoidal fracture similar to glass. The metal expands 3.1% on solidifying; therefore, Gallium should not be stored in glass or metal containers, as they may break as the metal solidifies. Gallium wets glass or porcelain, and forms a brilliant mirror when it is painted on glass. It is widely used in doping semiconductors and producing solid-state devices such as transistors. High-purity gallium is attacked slowly only bymineral acids. Magnesium gallate containing divalent impurities such as Mn+2 is finding use in commercial ultraviolet activated powder phosphors. Gallium nitride has been used to produce blue light-emitting diodes such as those used in CD and DVD readers. Gallium has found application in the Gallex Detector Experiment located in the Gran Sasso Underground Laboratory in Italy. This underground facility has been built by the Italian Istituto Nazionale di Fisica Nucleare in the middle of a highway tunnel through the Abruzzese mountains, about 150 km east of Rome. In this experiment, 30.3 tons of gallium in the form of 110 tons of GaCl3-HCl solution are being used to detect solar neutrinos. The production of 71Ge from gallium is being measured. Gallium arsenide is capable of converting electricity directly into coherent light. Gallium readily alloys with most metals, and has been used as a component in low melting alloys. Its toxicity appears to be of a low order, but it should be handled with care until more data are forthcoming. Natural gallium contains two stable isotopes. Twenty-six other isotopes, one of which is an isomer, are known. The metal can be supplied in ultrapure form (99.99999+%). The cost is about $5/g (99.999%).
UsesThe metal has no significant commercial uses. Its compounds are used as semiconductors.
DefinitionMetallic element of atomic number 31, group IIIA of the periodic table, aw 69.72, valences of 2, 3; two stable isotopes.
General DescriptionGALLIUM is a silvery-white liquid at room temperature. Ingestion of GALLIUM may be toxic. GALLIUM is corrosive to aluminum. If exposed to high temperatures, GALLIUM may emit toxic fumes which may form a corrosive alkaline solution with water. GALLIUM is soluble in most acids and alkalis. GALLIUM is used as a semiconductor material.
Air & Water ReactionsStable in dry air, in moist air GALLIUM tarnishes
Reactivity ProfileMetals, such as GALLIUM METAL, are reducing agents and tend to react with oxidizing agents (i.e. hydrogen peroxide). Their reactivity is strongly influenced by their state of subdivision: in bulk they often resist chemical combination; in powdered form they may react more rapidly. Reacts violently with chlorine and other halogens at ambient temperatures [Bretherick, 5th Ed., 1995].
Health HazardInhalation of vapors or contact with substance will result in contamination and potential harmful effects. Fire will produce irritating, corrosive and/or toxic gases.
Fire HazardNon-combustible, substance itself does not burn but may react upon heating to produce corrosive and/or toxic fumes. Runoff may pollute waterways.
Potential ExposureA potential danger to those involved in preparing such semiconductor compounds as gallium arsenide. Used in light-emitting diodes, batteries, and microwave equipment.
First aidEye Contact: Immediately remove any contact lenses and flush with large amounts of water for at least 15 minutes, occasionally lifting upper and lower lids. Skin Contact: Remove contaminated clothing. Wash contami nated skin with water. Breathing: Remove the person from exposure. Begin (using universal precautions, including resuscitation mask) if breathing has stopped and CPR if heart action has stopped. Transfer promptly to a medical facility. If swallowed, do not induce vomiting. Medical observation is recommended for 24 to 48 hours after breathing overexposure, as pulmonary edema may be delayed. As first aid for pulmonary edema, a qualified med ical professional might consider administering a corticoste roid spray. Cigarette smoking may exacerbate pulmonary injury and should be discouraged for at least 72 hours following exposure. If symptoms develop or overexposure is suspected, chest X-ray should be considered.
ShippingUN2803 Gallium, Hazard class: 8; Labels: 8-Corrosive material.
Purification MethodsDissolve the metal in dilute HCl and extract it with Et2O. Bubbling H2S through the solution removes many metals, and a second extraction with Et2O frees Ga further from metal impurities, except for Mo, Th(III) and Fe which are largely removed by precipitation with NaOH. The solution is then electrolysed in 10% NaOH with a Pt anode and cathode (2-5A at 4-5V) to deposit Ga, In, Zn and Pb, from which Ga was obtained by fractional crystallisation of the melt [Hoffman J Res Nat Bur Stand 13 665 1934]. Ga is also purified by heating to boiling in 0.5-1M HCl, then heating to 40o in water and pouring the molten Ga with water under vacuum through a glass filter (30-50 Y pore size), to remove any unmelted metals or oxide film. The Ga is then fractionally crystallised from the melt under water. [D.nges in Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol I p 837 1963.]
IncompatibilitiesIncompatible with oxidizers (chlorates, nitrates, peroxides, permanganates, perchlorates, chlorine, bromine, fluorine, etc.); contact may cause fires or explo sions. Keep away from alkaline materials, strong bases, strong acids, oxoacids, and epoxides such as lyes, halogens, and alloys of aluminum. Contact with hydrogen chloride/ hydrochloric acid or hydrogen peroxide may result in explosion. Corrosive on contact with metals. Moisture, oxygen, and air sensitive.
Waste DisposalUse a licensed professional waste disposal service to dispose of this material. Dissolve or mix the material with a combustible solvent and burn in a chemical incinerator equipped with an afterburner and scrubber. All federal, state, and local environmental regula tions must be observed.
GALLIUM Preparation Products And Raw materials
Raw materialsGold trichloride
Tag:GALLIUM(7440-55-3) Related Product Information
Gallium iodide (GaI3) GALLIUM ARSENIDE Gallium oxide (Ga2O3),Gallium trioxide GALLIUM SELENIDE TRIETHYLGALLIUM GALLIUM(III) SULFIDE GALLIUM NITRIDE GALLIUM PERCHLORATE, HYDRATED GADOLINIUM GALLIUM GARNET GALLIUM (III) TELLURIDE gallium(3+)sulfat gallium(iii)nitrate(1:3 GALLIUM ANTIMONIDE gallium(iii DIETHYLGALLIUM CHLORIDE Gallium fluoride (GaF3) Gallium,tris[2,4-pentanedionato-O,O’]-(OC-6-11) Gallium bromide (GaBr3)