Photoinitiators are small molecules that are sensitive to light.
Upon light absorption they undergo photochemical cleavage to
produce reactive species (either free radicals or a Bronsted or
Lewis acid) that will interact with the active components in
formulations. In other words, one could say that photoinitiators
take the energy from light and transform it into chemical energy to
induce chemical reactions. This process where a liquid formulation
is transformed into a cross-linked polymer induced by a
photoinitiator and its reaction with light is called
photopolymerization (also known as radiation curing).
There are 2 classes of photoinitiators: Type I and Type II
- Type I photoinitiators are those that undergo unimolecular bond
cleavage after absorption of light to render the reactive species.
No other species are necessary in order for these photoinitiators
to work.
- Type II photoinitiators undergo a bimolecular reaction. After
absorption of light, the photoinitiator reaches excited state from
which reacts with another molecule (co-initiator or synergist) to
create the reactive species.
- Regardless of the photoinitiator used and for a successful
cure, it is extremely important that the absorption bands of the
photoinitiator will overlap with the emission spectrum of the light
source used for curing. Also, there should be minimum competition
for light absorption from other species in the formulation. A poor
match between absorption bands and light emitted by the source will
result in a poor cure or no cure at all.Some small molecules in the
atmosphere can also act as photoinitiators by decomposing to give
free radicals (in photochemical smog). For instance, nitrogen
dioxide is produced in large quantities by gasoline-burning
internal combustion engines. NO2 in the tropospheregives
smog its brown coloration and catalyzesproduction of toxic
ground-level ozone. Molecular oxygen (O2) also serves as
a photoinitiator in the stratosphere, breaking down into atomic
oxygen and combining with O2 in order to form the ozone
in the ozone layer.