User:Pkornbl2/Photoinitiators
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A photoinitiator is any chemical compound that decomposes into free radicals when exposed to light. Photoinitiators are found both in nature (in photochemical smog) and in industry (for example, in plastics production).
In nature, photoinitiators are present througout the atmosphere. Nitrogen dioxide is produced in large quantities by gasoline-burning internal combustion engines. NO2 in the troposphere gives smog its brown coloration and catalyzes production of toxic ground-level ozone. Molecular oxygen (O2) also serves as a photoinitiator in the stratosphere, breaking down into atomic oxygen and later forming the ozone in the ozone layer.
In industry, photoinitiators are primarily used to promote polymerization reactions, notably in the production of polyethylene plastic. There are a handful of medical applications as well; for instance, benzoyl peroxide creams are commonly prescribed as acne medication.
Reactions[edit]
All photoinitiators have bonds that cleave via photolysis. For example, peroxides like hydrogen peroxide are perfect examples, with the O-O bond cleaving to form two hydroxyl radicals.
- H2O2 --> 2OH
Certain diazo compounds (such as azobisisobutyronitrile), can also photolytically cleave, forming two alkyl radicals and nitrogen gas:
- RCH2-N=N-H2CR --> 2RCH2 + N2
These free radicals can now promote other reactions.
Atmospheric Photoinitiators[edit]
Peroxides[edit]
Since molecular oxygen can abstract H atoms from certain radicals, the HOO radical is easily created. This particular radical can further abstract H atoms, creating H2O2, hydrogen peroxide. Hydrogen peroxide can cleave photolytically into 2 hydroxyl radicals, which can serve to oxidize organic compounds in the atmosphere.
- H2O2 --> 2OH
- OH + CH4 --> CH3 + H2O
Nitrogen Dioxide[edit]
Nitrogen dioxide can also be photolytically cleaved by photons of wavelength less than 400 nm[1]producing atomic oxygen and nitric oxide.
- NO2 --> NO + O
Atomic oxygen is a highly reactive species, and can abstract a H atom from anything, including water.
- O + H2O --> 2OH
Nitrogen dioxide can be regenerated through a reaction between certain peroxy-containing radicals and NO.
- ROO + NO --> NO2 + RO
Molecular Oxygen[edit]
In the stratosphere, molecular oxygen (O2) is an important photoinitiator that begins the ozone-production process in the ozone layer. Oxygen can be photolyzed into atomic oxygen by light with wavelength less than 240 nm. [2]
- O2 → 2O
Atomic oxygen can then combine with more molecular oxygen to form ozone.
- O + O2 → O3
However, ozone can also be photolyzed back into O and O2.
- O3 → O + O2
Furthermore, atomic oxygen and ozone can combine into O and O3.
- O + O3 → 2O2
This set of reactions are known as the Chapman Reactions and govern the production of ozone.
Commercial Photoinitiators & Uses[edit]
AIBN[edit]
- Main Article: Azobisisobutyronitrile
Azobisisobutyronitrile is a white powder often used as a photoinitiator for vinyl-based polymers such as polyvinyl chloride, also known as PVC. Because this particular photoinitiator produces nitrogen gas (N2) upon decomposition, it is often used as a blowing agent to change the shape and/or texture of plastics.[3]
Benzoyl Peroxide[edit]
- Main Article: Benzoyl Peroxide
Benzoyl peroxide, much like azobisisobutyronitrile, is a white powder used as a photoinitiator in various commercial and industrial processes, including plastics production. Unlike AIBN, however, benzoyl peroxide produces oxygen gas upon decomposing, giving this compound a host of medical uses as well.[4]
Benzoyl peroxide-based Upon contact with the skin, benzoyl peroxide breaks down, producing oxygen gas, among other things. The oxygen gas is absorbed into the pores of the skin, where it kills off the acne-causing bacteria Propionibacterium acnes.
In addition, the free radicals produced can break down dead skin cells. Clearing out these dead cells prevents pore blockage and, by extension, acne breakouts.[5]
See Also[edit]
References[edit]
- ^ vanLoon, Gary W.; Duffy, Stephen J. (2005). Environmental Chemistry: A Global Perspective. New York, NY: Oxford University Press. pp. 74–79. ISBN 0-19-927499-1.
{{cite book}}: Cite has empty unknown parameter:|coauthors=(help) - ^ vanLoon, Gary W.; Duffy, Stephen J. (2005). Environmental Chemistry: A Global Perspective. New York, NY: Oxford University Press. pp. 48–49. ISBN 0-19-927499-1.
{{cite book}}: Cite has empty unknown parameter:|coauthors=(help) - ^ "Azobisisobutyronitrile - Chemical Dictionary", lookchem.com, accessed October 22, 2009
- ^ "Benzoyl Peroxide", chemicalland21.com, accessed October 29, 2009
- ^ "Benzoyl Peroxide", http://www.about.com, accessed October 29, 2009