The first and second ionization energies of sulfur are 999. k J·mol Amorphous or "plastic" sulfur is produced by rapid cooling of molten sulfur—for example, by pouring it into cold water.

X-ray crystallography studies show that the amorphous form may have a helical structure with eight atoms per turn.

The element sulfur is used in matches, insecticides, and fungicides.

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Being abundant in native form, sulfur was known in ancient times, being mentioned for its uses in ancient India, ancient Greece, China, and Egypt. Today, almost all elemental sulfur is produced as a byproduct of removing sulfur-containing contaminants from natural gas and petroleum.

The greatest commercial use of the element is the production of sulfuric acid for sulfate and phosphate fertilizers, and other chemical processes.

It is normally present as troilite (Fe S), but there are exceptions, with carbonaceous chondrites containing free sulfur, sulfates and other sulfur compounds.

On Earth, elemental sulfur can be found near hot springs and volcanic regions in many parts of the world, especially along the Pacific Ring of Fire; such volcanic deposits are currently mined in Indonesia, Chile, and Japan.

Sulfur, usually as sulfide, is present in many types of meteorites.

Ordinary chondrites contain on average 2.1% sulfur, and carbonaceous chondrites may contain as much as 6.6%.

Sulfur is a chemical element with symbol S and atomic number 16. Under normal conditions, sulfur atoms form cyclic octatomic molecules with a chemical formula S.

Elemental sulfur is a bright yellow crystalline solid at room temperature.

This process happens within a matter of hours to days, but can be rapidly catalyzed.

Ar, the radioactive isotopes of sulfur have half-lives less than 3 hours.

Hydrogen sulfide gives the characteristic odor to rotting eggs and other biological processes.