- Product Name:Oxygen
- Synonyms: Dioxygen hyperoxia liquidoxygen Liquid-oxygen- AUTOMOTIVE STANDARD R99-5 AUTOMOTIVE STANDARD R99-6 HYDROGEN AND OXYGEN OXYGEN, PRESSURE TIN WITH 1 L
- Product Categories: refrigerants Inorganics Analytical Reagents Replacement Kit Items Water Test OGas Standards Alphabetic Analytical Standards Pure Gases SCOTTY Gases Chemical Synthesis Compressed and Liquefied Gases Synthetic Reagents Compressed and Liquefied GasesMicro/Nanoelectronics Electronic Chemicals Gases
- Mol File:7782-44-7.mol
Oxygen Chemical Properties
- Melting point:−218 °C(lit.)
- Boiling point:−183 °C(lit.)
- Density 1.429（0℃）
- vapor density 1.11 (vs air)
- vapor pressure >760 mmHg at 20 °C
- storage temp. -20°C
- solubility At 20 °C and at a pressure of 101 kPa, 1 volume dissolves in about 32 volumes of water.
- form colorless gas
- OdorOdorless gas
- Water Solubility one vol gas dissolves in 32 volumes H2O (20°C), in 7 volumes alcohol (20°C); soluble other organic liq, usually higher solubility than in H2O [MER06]
- Merck 13,7033
- Stability:Stable. Vigorously supports combustion. Incompatible with phosphorus, organic materials, many powdered metals.
- CAS DataBase Reference7782-44-7(CAS DataBase Reference)
- NIST Chemistry ReferenceOxygen(7782-44-7)
- EPA Substance Registry SystemOxygen(7782-44-7)
- Hazard Codes O,C
- Risk Statements 8-52/53-34-48/20/22-37
- Safety Statements 17-45-36/37/39-26-61
- RIDADR UN 1072 2.2
- WGK Germany -
- RTECS RS2060000
- F 4.5-31
- HazardClass 2.2
- Hazardous Substances Data7782-44-7(Hazardous Substances Data)
- ToxicityOSHA recommends a minimum oxygen concentration of 19.5% for human occupancy.
Oxygen Usage And Synthesis
- Chemical PropertiesOxygen, O2, is a colorless, tasteless, gaseous element essential to almost all forms of life. It promotes respiration and combustion. Oxygen comprises 20% of the earth's atmosphere and is the most abundant element in seawater and in the earth's crust. It is slightly soluble in water and alcohol, but combines readily with most other elements to form oxides. The electrolysis of water produces both oxygen and hydrogen.
- Chemical PropertiesOxygen is a colorless odorless gas or a bluish cryogenic liquid.
- Physical propertiesThere are three allotropes (different forms) of oxygen: (1) atomic oxygen (O), sometimesreferred to as nascent or “newborn” oxygen; (2) diatomic oxygen (O2), or molecular oxygen(gas); and (3) ozone (O3), also a gas.
The atmospheric oxygen that we breathe is a very reactive nonmetal and is colorless, odorless,and tasteless, but it is essential to all living organisms. It readily forms compounds withmost other elements. With six electrons in its outer valence shell, it easily gains two moreelectrons to form a negative (–2) ion; or as covalent, it can share electrons with other elementsto complete its outer shell.
Almost all the oxygen in the atmosphere (?21%) is the allotropic form of molecular oxygen(O2). This essential gas we breathe is the result of photosynthesis, which is how green plants(with chlorophyll) use the energy of the sun to convert carbon dioxide (CO2) and water tostarches and sugars with molecular oxygen as the by-product.
Liquid oxygen has a slightly bluish cast to it. As it boils, pure oxygen gas is released. Themelting point for oxygen is –218.79°C, its boiling point is –182.95°C, and its density is0.001429 g/cm3.
- IsotopesThere are a total of 15 isotopes of oxygen, three of which are stable. The stableones are O-16, which accounts for 99.762% of all the oxygen on Earth; O-17, whichcontributes only 0.038% of the Earth’s oxygen; and O-18, which makes up just 0.200%of Earth’s oxygen.
- OccurrenceOxygen is the third most abundant element in the universe, making up nearly half themass of the Earth’s crust and nine-tenths of the total mass of water. Even the mass of ourbodies consists of two-thirds oxygen. Oxygen is also the most abundant element in the Earth’satmosphere at 20.947% by volume.
Oxygen is produced commercially by liquefying air under reduced temperatures andincreased pressure. Then oxygen (and other gases) can be collected as the temperature rises inthe liquid air, allowing the various gases to boil off at their specific boiling points. This processis known as fractional distillation. Liquid air can be transported in vacuum vessels in theliquid form as long as there is a small vent to allow the escape of some of the gas that boilsaway as temperatures rise above the boiling point.
Fractional distillation is based on the principle that each element has its own temperatureat which it changes from a liquid to a gas. Thus, any gas can be separated from other liquefiedcomponents of air and then collected. The same process is used in the petroleum industry toseparate various fractions from the crude oil.
There are several methods of producing oxygen gas in the laboratory.
Oxygen can be produced by electrolysis of water using a salt as an electrolyte that produceshydrogen at the opposite electrode. When potassium chlorate (KClO3) is heated in a testtube with a small amount of manganese dioxide (MnO2) as a catalyst, the chemical reactionthat releases the oxygen from potassium chlorate will be accelerated. Use of potassium nitrate(KNO3) will also produce small amounts of oxygen.
A recent, and more productive, method is to pass air through fine molecular-size sievesof material that will absorb the nitrogen gas of air, which then allows the oxygen gas to passthrough the sieve to be collected.
- CharacteristicsOxygen is, without a doubt, the most essential element on Earth. It is required to supportall plant and animal life, and it forms more compounds with other elements than any otherelement.
Oxygen is soluble in both water and alcohol. Contrary to what many people believe, oxygenis NOT combustible (it will not burn), but rather it actively supports the combustion ofmany other substances. After all, if oxygen burned, every time a fire was lit, all the O2 in theatmosphere would be consumed!
Burning is a form of oxidation wherein oxygen chemically combines with a substance rapidlyenough to produce adequate heat to cause fire and light, or to maintain a fire once started.The oxidation of iron is called rusting. Rusting in an example of “slow oxidation,” which isthe reaction of O2 with Fe to form Fe2O3 or Fe3O4. This chemical reaction is so slow that theheat it produces is dissipated; thus, there is no fire.
Recently a new allotrope of oxygen was discovered. When O2 is subjected to great pressure,it is converted intoO4, which is a deep red solid that is a much more powerful oxidizer thanthe other forms of oxygen.
- HistoryOxygen, as a gaseous element, forms 21% of the atmosphere by volume from which it can be obtained by liquefaction and fractional distillation. The atmosphere of Mars contains about 0.15% oxygen. The element and its compounds make up 49.2%, by weight, of the Earth’s crust. About two thirds of the human body and nine tenths of water is oxygen. In the laboratory it can be prepared by the electrolysis of water or by heating potassium chlorate with manganese dioxide as a catalyst. The gas is colorless, odorless, and tasteless. The liquid and solid forms are a pale blue color and are strongly paramagnetic. Ozone (O3), a highly active compound, is formed by the action of an electrical discharge or ultraviolet light on oxygen. Ozone’s presence in the atmosphere (amounting to the equivalent of a layer 3 mm thick at ordinary pressures and temperatures) is of vital importance in preventing harmful ultraviolet rays of the sun from reaching the Earth’s surface. There has been recent concern that pollutants in the atmosphere may have a detrimental effect on this ozone layer. Ozone is toxic and exposure should not exceed 0.2 mg/m3 (8-hour time-weighted average — 40-hour work week). Undiluted ozone has a bluish color. Liquid ozone is bluish black, and solid ozone is violet- black. Oxygen is very reactive and capable of combining with most elements. It is a component of hundreds of thousands of organic compounds. It is essential for respiration of all plants and animals and for practically all combustion. In hospitals it is frequently used to aid respiration of patients. Its atomic weight was used as a standard of comparison for each of the other elements until 1961 when the International Union of Pure and Applied Chemistry adopted carbon 12 as the new basis. Oxygen has thirteen recognized isotopes. Natural oxygen is a mixture of three isotopes. Oxygen 18 occurs naturally, is stable, and is available commercially. Water (H2O with 1.5% 18O) is also available. Commercial oxygen consumption in the U.S. is estimated to be 20 million short tons per year and the demand is expected to increase substantially in the next few years. Oxygen enrichment of steel blast furnaces accounts for the greatest use of the gas. Large quantities are also used in making synthesis gas for ammonia and methanol, ethylene oxide, and for oxy-acetylene welding. Air separation plants produce about 99% of the gas, electrolysis plants about 1%. The gas costs 5￠/ft3 ($1.75/cu. meter) in small quantities.
- UsesIn oxyhydrogen or oxyacetylene flame for welding metals and for lighting (calcium light, etc); submarine work by divers, propellant for rockets. In the production of synthesis gas which can be used in the Fischer-Tropsch process for liquid fuels.
- UsesOxygen has many uses due to its high electronegativity with the ability to oxidize manyother substances. Only fluorine has higher electronegativity and is thus a stronger oxidizer.Besides the essential use to support life, oxygen has many other uses.
It is used in the smelting process to free metals from their ores. It is particularly importantin the oxygen-converter process in the production of steel from iron ore.
Oxygen is used in making several important synthetic gases and in the production ofammonia, methyl alcohol, and so on.
It is the oxidizer for liquid rocket fuels, and as a gas, oxygen is used in a mixture withhelium to support the breathing of astronauts and divers and to aid patients who have difficultybreathing. It is use to treat (oxidize) sewage and industrial organic wastes.
Oxygen has many uses because of its ability to accept electrons from other elements to formionic bonds or to share electrons with other elements to form covalent bonds.
- DefinitionDioxygen: the normal form of molecularoxygen, O2, used to distinguishit from oxygen atoms or fromozone （O3）.
- Definitionoxygen: Symbol O. A colourlessodourless gaseous element belongingto group 16 (formerly VIB) of the periodictable; a.n. 8; r.a.m. 15.9994; d.1.429 g dm–3; m.p. –218.4°C; b.p.–183°C. It is the most abundant elementin the earth’s crust (49.2% byweight) and is present in the atmosphere(28% by volume). Atmosphericoxygen is of vital importance for allorganisms that carry out aerobic respiration.For industrial purposes it isobtained by fractional distillation of liquid air. It is used in metallurgicalprocesses, in high-temperatureflames (e.g. for welding), and inbreathing apparatus. The commonform is diatomic (dioxygen, O2);there is also a reactive allotropeozone (O3). Chemically, oxygen reactswith most other elements formingoxides. The element wasdiscovered by Joseph Priestley in1774.
- DefinitionThe most abundant elementon earth, making up about 47% of the earth’s mass,and essential for respiration.
- General DescriptionOxygen is a colorless, odorless and tasteless gas. Oxygen will support life. Oxygen is noncombustible, but will actively support the burning of combustible materials. Some materials that will not burn in air will burn in Oxygen. Materials that burn in air will burn more vigorously in Oxygen. As a non-liquid gas Oxygen is shipped at pressures of 2000 psig or above. Pure Oxygen is nonflammable. Under prolonged exposure to fire or intense heat the containers may rupture violently and rocket. Oxygen is used in the production of synthesis gas from coal, for resuscitation and as an inhalant.
- Reactivity ProfilePropellant; ignites upon contact with alcohols, alkali metals, amines, ammonia, beryllium alkyls, boranes, dicyanogen, hydrazines, hydrocarbons, hydrogen, nitroalkanes, powdered metals, silanes, or thiols [Bretherick 1979. p.174]. Heat of water will vigorously vaporize liquid Oxygen, pressures may build to dangerous levels if this occurs in a closed container. Liquid Oxygen gives a detonable mixture when combined with powdered aluminum [NFPA 491M. 1991].
- HazardAlthough oxygen itself is not flammable or explosive, as is sometimes believed, its mainhazard is that, in high concentrations, oxygen can cause other materials to burn much morerapidly.
Oxygen is toxic and deadly to breathe when in a pure state at elevated pressures. In addition,such pure oxygen promotes rapid combustion and can produce devastating fires, such asthe fire that killed the Apollo 1 crew on a test launch pad in 1967. It spread rapidly because thepure oxygen was at normal pressure rather than the one-third pressure used during flight.
Oxygen used for therapeutic purposes in adults can cause convulsions if the concentrationis too high. At one time, high levels of oxygen were given to premature infants to assist theirbreathing. It was soon discovered that a high concentration of O2 caused blindness in some ofthe infants. This practice has been abandoned, or the oxygen levels have since been reduced,and this is no longer a medical problem.
Oxygen involved in metabolic processes are prone to form “free radicals,” which arethought to cause damage to cells and possibly be associated with cancer and aging.
- Health HazardOxygen is nontoxic under the usual conditions of laboratory use. Breathing pure oxygen at one atmosphere may produce cough and chest pains within 8 to 24 h, and concentrations of 60% may produce these symptoms in several days. Liquid oxygen can cause severe "burns" and tissue damage on contact with the skin due to extreme cold.
- Health HazardInhalation of 100% Oxygen can cause nausea, dizziness, irritation of lungs, pulmonary edema, pneumonia, and collapse. Liquid may cause frostbite of eyes and skin.
- Fire HazardBehavior in Fire: Increases intensity of any fire. Mixtures of liquid Oxygen and any fuel are highly explosive.
- Fire HazardOxygen itself is nonflammable, but at concentrations greater than 25% supports and vigorously accelerates the combustion of flammable materials. Some materials (including metals) that are noncombustible in air will burn in the presence of oxygen.
- Flammability and ExplosibilityOxygen itself is nonflammable, but at concentrations greater than 25% supports and vigorously accelerates the combustion of flammable materials. Some materials (including metals) that are noncombustible in air will burn in the presence of oxygen.
- Agricultural UsesOxygen (O) is an odorless, colorless, gaseous element
that belongs to group 16 (formerly group VI) of the
Periodic Table. It is the most abundant element
in the earth's crust (49.2% by weight), is present in the
atmosphere (20% by volume) and is a constituent of
water. It exists in three isotopes 16, 17 and 18. Oxygen is
essential for respiration of most living organisms and for
combustion. It is used in metallurgical processes, in high
temperature flames (welding) and in medical treatment.
The common form of oxygen is di-atomic oxygen (O2) There is also another form - reactive allotrope ozone (O3)C.h emically, oxygen reacts with most other elements forming oxides. For industrial use, it is obtained by fractional distillation of liquid air. This has been replaced by a process which utilizes ambient temperature separation by means of a pressure cycle in which molecular sieves of synthetic zeolite preferentially absorb nitrogen from air, giving 95 % oxygen and 5 % argon.
The most popular industrial use of oxygen is in oxygen enrichment of steel blast furnaces. Large quantities of oxygen are used in the synthesis of nitric acid from ammonia, methanol and ethylene oxide, as also in oxy-acetylene welding.
- Safety ProfileHuman systemic effects by inhalation: cough and other pulmonary changes. Human teratogenic effects by inhalation: developmental abnormalities of the fetal cardovascular system. Mutation data reported. Not toxic as gas. In liquid form it can cause severe "burns" and tissue damage on contact with the slun due to extreme cold. An oxidant. Though itself nonflammable,it is essential to combustion. Even a slight increase in the oxygen content of the air above the normal 21% greatly increases the oxidation or burning rate (and the hazard) of many materials. Exclusion of O2 from the neighborhood of a fire is one of the principal methods of extinguishment. Avoid smoking, flames, electric sparks. Liquid O2 can explode on contact with readdy oxidizable materials, especially at high temperatures. Under the proper condltions of temperature, pressure, and reagent concentration it can react violently with acetaldehyde, acetylene, acetone, secondary alcohols (e.g., 2-propanol, 2-butanol) aluminum, Al(BH4)3, AH3, aluminumtitanium alloys, alkali metals @hum, cesium, potassium, rubidlum, sodlum, potassium), ammonia, ammonia + platinum, asphalt, ccl4, chlorinated hydrocarbons, cyanogen, barium, benzene, 1,4-benzenediol + 1-propanol, benzoic acid, Be(BH4)2, biological materials + ether, BAszBr3, B2H10, diH6, boron tribromide, boron trichloride, bromine + chlorotrifluoroethylene, butane + Ni(CO)4, carbon disulfide, carbon disulfide + mercury + anthracene, carbon monoxide, CsH, calcium, calcium hosphide, copper + hydrogen sulfide, Cl0H14, cyclohexane-l,2-done biskhenylhydrazone), cycl0℃tatetraene, dborane, diboron tetrafluoride, dimethoxymethane, dimethylketene, dimethyl sulfide, diphenyl ethylene, disilane, ethers (e.g., diethyl ether, diisopropyl ether, tetrahydro furan, dtoxane, ethyl ether), fibrous fabrics, fluorine + hydrogen, fuels, germanium, glycerol, halocarbons (e.g., l,l,l-trichloroethane, trichloroethylene, chlorotrifluoroethylene, bromotrifluoroethylene), hydrazine, hydrocarbons (e.g., 1,l-dphenylethylene, gasoline, cyclohexane, ethylene, cumene, pxylene, but-3-yne), hydrocarbons + promoters (e.g., methyl nitrate, nitromethane, ethyl nitrate, tetrafluorohydrazine), hydrogen, hydrogen sulfide, lithiated dalkylnitrosoamines, magnesium, metals, metal hydrides (e.g., sodtum hydride, uranium hydride, lithium h ydride, potassium hydride , rubidium hydride, cesium hydride, magnesium hydride), methane, methoxycycl0℃tatetraene, 4-methoxytoluene7 Ni(CO)4 + butane, nonmetal hydrides (e.g., diborane, tetraborane(lO), phosphine, pentaborane(1 l), pentaborane(9) , decaborane(l4), aluminum tetrahydroborate), oil films, organic matter, (OF2 + H20), phosphorus, phosphorus tribromide, phosphorus trifluoride, phosphorus(IⅡ) oxide, polymers [e.g., foam rubber, neoprene, polytetrafluoroethylene (teflon)], polytetrafluoroethylene + stainless steel, polyurethane, polyvinyl chloride, propylene oxide, K2O2, rhenium, trirhenium nonachloride, rubber + ozone, rubberized fabric, selenium, NaH, sodium hydroxide + tetramethyldsiloxane, strontium, tetracarbonylnickel, tetracarbonylnickel + mercury, tetrafluoroethylene, tetrafluorohydrazine, tetrasilane, titanium and alloys, trisilane, CH2Cl2, oil, paraformaldehyde, wood, charcoal. Compressed O2 is shipped in steel cylinders under hgh pressure. If these containers are broken due to shock or exposed to high temperature, an explosion and fire may result.
- Potential ExposureCompressed oxygen is used in various oxidation processes, for feedstock; and enrichment purposes; as a medicinal gas; a chemical intermediate; in oxyacetylene welding; in metallurgy. Liquid oxygen is used as a rocket fuel. Oxygen is naturally present at a concentration of 21% in breathing air.
- ShippingUN1072 Oxygen, compressed & UN1073 Oxygen, refrigerated liquid (cryogenic liquid), Hazard Class: 2.2; Labels: 2.2-Nonflammable compressed gas; 5.1- Oxidizer. Cylinders must be transported in a secure upright position, in a well-ventilated truck. Protect cylinder and labels from physical damage. The owner of the compressed gas cylinder is the only entity allowed by federal law (49CFR) to transport and refill them. It is a violation of transportation regulations to refill compressed gas cylinders without the express written permission of the owner.
- Purification MethodsPurify it by passing the gas over finely divided platinum at 673oK and Cu(II) oxide (see under nitrogen) at 973o, then condensed in a liquid N2-cooled trap. HIGHLY EXPLOSIVE in contact with organic matter.
- IncompatibilitiesA strong oxidizer. Reacts violently with nearly every element, combustibles, organics, and reducing materials.
- Waste DisposalReturn refillable compressed gas cylinders to supplier. Vent to atmosphere.
Oxygen Preparation Products And Raw materials
- Preparation Products3-Hydroxybenzoic acidp-Toluic acidCarbarylCARBONYL SULFIDE1,3-Dihydroxyadamantane3-Methyl-2-butanone1,3-DiphenylguanidineDichloroacetyl chlorideThiobencarbTrimanganese tetraoxideDIETHOFENCARB4,4'-Bis(dimethylamino)benzophenone3,5-diisopropylphenol 1-AdamantanolOsmium tetraoxide1-deoxy-1-(6-phenylazo-3,4-xylidino)-D-ribitol2,2'-(Ethylenedioxy)diethanolMicaceous Iron Oxide4-Ethylbenzoic acid4-Bromobenzoic acidBarium peroxideDeemulsifier SP-169Zirconium hydroxide 1,4-Naphthalenedicarboxylic acid2-Bromobenzoic acidEthephonRUTHENIUM TETROXIDESTRONTIUM CHROMATE3,5-Dimethylbenzoic acidSodium peroxide3-Methylthiopropanolpolyacrylonitrile pyrolysis productD-ARABINONIC ACIDpolypyrrole synthesized by electrolytic polymerizationTrimesic acidmagnesium oxide whisker：magnesia whiskercatalyst of Hopcalite MC-15，DB-75 and DB-834-Pentylbenzoic acid4-Butylbenzoic acid
- Raw materialsPotassium hydroxide NitrogenHydrogen HEAVY CUT RESIDUE OILPentachlorophenolCompressor
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