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A pyrophoric substance (from Greek πυροφόρος, pyrophoros, "fire-bearing") is a substance that ignites spontaneously in air at or below 54 °C (129 °F) (for gases) or within 5 minutes after coming into contact with air (for liquids and solids). Examples are iron sulfide and many reactive metals including plutonium and uranium, when powdered or thinly sliced. Pyrophoric materials are often water-reactive as well and will ignite when they contact water or humid air. They can be handled safely in atmospheres of argon or (with a few exceptions) nitrogen. Most pyrophoric fires should be extinguished with a Class D fire extinguisher for burning metals.
The creation of sparks from metals is based on the pyrophoricity of small metal particles, and pyrophoric alloys are made for this purpose. This has certain uses: the sparking mechanisms in lighters and various toys, using ferrocerium; starting fires without matches, using a firesteel; the flintlock mechanism in firearms; and spark-testing ferrous metals.
Small amounts of pyrophoric liquids are often supplied in a glass bottle with a PTFE (Teflon)-lined septum. Larger amounts are supplied in metal tanks similar to gas cylinders, designed so a needle can fit through the valve opening. A syringe, carefully dried and flushed of air with an inert gas, is used to extract the liquid from its container.
Pyrophoric solids require the use of a sealed glove box flushed with inert gas. Glove boxes are expensive and require maintenance. Thus, many pyrophoric solids are sold as solutions, or dispersions in mineral oil or lighter hydrocarbon solvents. Mildly pyrophoric solids (such as lithium tetrahydridoaluminate (lithium aluminium hydride) and sodium hydride) can be handled in the air for brief periods of time, but the containers must be flushed with inert gas before storage.
- White phosphorus, the original "phosphor"
- Alkali metals (lithium, sodium, potassium, rubidium, caesium), including the alloy NaK
- Finely divided metals (iron, aluminium, magnesium, calcium, zirconium, uranium, titanium, bismuth, hafnium, thorium, osmium, neodymium)
- Some metals and alloys in bulk form (cerium, plutonium)
- Alkylated metal alkoxides or nonmetal halides (diethylethoxyaluminium, dichloro(methyl)silane)
- Potassium graphite (KC8)
- Metal hydrides (sodium hydride, lithium aluminium hydride, uranium trihydride)
- Methane tellurol (CH3TeH), an analog of methanol where tellurium replaces oxygen
- Partially or fully alkylated derivatives of metal and nonmetal hydrides (diethylaluminium hydride, trimethylaluminium, triethylaluminium, butyllithium), with a few exceptions (i.e. dimethylmercury and tetraethyllead)
- Copper fuel cell catalysts, e.g., Cu/ZnO/Al2O3
- Grignard reagents (compounds of the form RMgX)
- Used hydrogenation catalysts such as palladium on carbon or Raney nickel (especially hazardous because of the adsorbed hydrogen)
- Iron sulfide: often encountered in oil and gas facilities where corrosion products in steel plant equipment can ignite if exposed to air.
- Lead and carbon powders produced from decomposition of lead citrate
- Uranium is pyrophoric, as shown in the disintegration of depleted uranium penetrator rounds into burning dust upon impact with their targets. In finely divided form it is readily ignitable, and uranium scrap from machining operations is subject to spontaneous ignition.
- Several compounds of plutonium are pyrophoric, and they cause some of the most serious fires occurring in United States Department of Energy facilities.
- Petroleum hydrocarbon (PHC) sludge.
- Metalorganics of main group metals (e.g. aluminium, gallium, indium, zinc and cadmium etc.)
- Phosphine, PH3 is only pyrophoric if impure, with P2H4 present.
- GHS, seventh revised version. https://www.unece.org/fileadmin/DAM/trans/danger/publi/ghs/ghs_rev07/English/ST_SG_AC10_30_Rev7e.pdf
- N. Pradeep Sharma, Dictionary Of Chemistry
- Angelo & Subramanian (2008), Powder metallurgy: science, technology and applications, p. 48,
Powders of aluminium, iron and magnesium are highly pyrophoric in nature
- C.W. Corti et al. / Applied Catalysis A: General 291 (2005) 257
- Pyrophoric lead composition and method of making it
- Charles J (1966). "The Reaction of Pyrophoric Lead with Oxygen". The Journal of Physical Chemistry. 70: 1478–1482. doi:10.1021/j100877a023.
- DOE | Office of Health, Safety and Security | Nuclear Safety and Environment | Uranium, retrieved 3 September 2013; archived on 24 August 2010.
- DOE | Office of Health, Safety and Security | Nuclear Safety and Environment | Plutonium, retrieved 3 September 2013; archived on 28 September 2010.