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Atomic Number:8Atomic Symbol:O
Atomic Weight:15.9994Electron Configuration:2-6
Shells:2,6Filling Orbital:2p4
Melting Point:-218.4oCBoiling Point:-183.0oC
Uses:Combustion, life support, welding, steel making etc.


(Gr. oxys, sharp, acid, and genes, forming; acid former) For many centuries, workers occasionally realized air was composed of more than one component. The behavior of oxygen and nitrogen as components of air led to the advancement of the phlogiston theory of combustion, which captured the minds of chemists for a century.

Oxygen was prepared by several workers, including Bayen and Borch, but they did not know how to collect it, did not study its properties, and did not recognize it as an elementary substance.

Joseph Priestley of England is generally credited with its dicovery, although Carl Wilhelm Scheele of Sweden also discovered it independently.

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 is the third most abundant element found in the sun, and it plays a part in the carbon-nitrogen cycle, the process once thought to give the sun and stars their energy. Oxygen under excited conditions is responsible for the bright red and yellow-green colors of the Aurora.

A gaseous element, oxygen forms 21% of the atmosphere by volume and is 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 under ordinary pressures and temperatures) helps prevent harmful ultraviolet rays of the sun from reaching the earth's surface. Pollutants in the atmosphere may have a detrimental effect on this ozone layer. Ozone is toxic and exposure should not exceed 0.2 mg/m# (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, which is very reactive, is a component of hundreds of thousands of organic compounds and combines with most elements.


Plants and animals rely on oxygen for respiration. Hospitals frequently prescribe oxygen for patients with respiratory ailments.


Oxyen has nine isotopes. Natural oxygen is a mixture of three isotopes.

Natural occurring oxygen 18 is stable and available commercially, as is water (H2O with 15% 18-O). Commercial oxygen consumption in the U.S. is estimated at 20 million short tons per year and the demand is expected to increase substantially.

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, while electrolysis plants produce about 1%.


The gas costs 5 cents / ft3 in small quantities, and about $15/ton in large quantities

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