A siloxane is a functional group in organosilicon chemistry with the Si–O–Si linkage. The parent siloxanes include the oligomeric and polymeric hydrides with the formulae H(OSiH2)nOH and (OSiH2)n. Siloxanes also include branched compounds, the defining feature of which is that each pair of silicon centres is separated by one oxygen atom. The siloxane functional group forms the backbone of silicones, the premier example of which is polydimethylsiloxane. The functional group (RO)3Si is called siloxy.
Siloxanes generally adopt structures expected for linked tetrahedral ("sp3-like") centers. The Si–O bond is 1.64 Å (vs Si–C distance of 1.92 Å) and the Si–O–Si angle is rather open at 142.5°. By way of contrast, the C–O distance in a typical dialkyl ether is much shorter at 1.414(2) Å with a more acute C–O–C angle of 111°. It can be appreciated that the siloxanes would have low barriers for rotation about the Si–O bonds as a consequence of low steric hindrance. This geometric consideration is the basis of the useful properties of some siloxane-containing materials, such as their low glass transition temperatures.
Synthesis of siloxanes
The main route to siloxane functional group is by condensation of two silanols:
- 2 R3Si–OH → R3Si–O–SiR3 + H2O
Usually the silanols are generated in situ by hydrolysis of silyl chlorides. With a disilanol, R2Si(OH)2 (derived from double hydrolysis of a silyldichloride), the condensation can afford linear products terminated with silanol groups:
- n R2Si(OH)2 → H(R2SiO)nOH + n−1 H2O
Alternatively the disilanol can afford cyclic products
- n R2Si(OH)2 → (R2SiO)n + n H2O
Starting from trisilanols, cages are possible, such as the species with the formula (RSi)nO3n/2 with cubic (n = 8) and hexagonal prismatic (n = 12). (RSi)8O12 structures. The cubic cages are cubane-type clusters, with silicon centers at the corners of a cube oxygen centres spanning each of the twelve edges.
Oxidation of organosilicon compounds, including siloxanes, gives silicon dioxide. This conversion is illustrated by the combustion of hexamethylcyclotrisiloxane:
- ((CH3)2SiO)3 + 12 O2 → 3 SiO2 + 6 CO2 + 9 H2O
- ((CH3)3Si)2O + 2 NaOH → 2 (CH3)3SiONa + H2O
This reaction proceeds by production of silanols. Similar reactions are used industrially to convert cyclic siloxanes to linear polymers.
Cyclomethicones are a group of methyl siloxanes, a class of liquid silicones (cyclic polydimethylsiloxane polymers) that possess the characteristics of low viscosity and high volatility as well as being skin emollients and in certain circumstances useful cleaning solvents. Unlike dimethicones, which are linear siloxanes that do not evaporate, cyclomethicones are cyclic: both groups consist of a polymer featuring a monomer backbone of one silicon and two oxygen atoms bonded together, but instead of having a very long "linear" backbone surrounded by a series of methyl groups (which produces a clear, non-reactive, non-volatile liquid ranging from water-thin to taffy-thick), cyclomethicones have short backbones that make closed or nearly-closed rings or "cycles" with their methyl groups, giving them many of the same properties of dimethicones but making them much more volatile. They are used in many cosmetic products where eventual complete evaporation of the siloxane carrier fluid is desired. In this way they are useful for products like deodorants and antiperspirants which need to coat the skin but not remain tacky afterward. Most cyclomethicone is manufactured by Dow Corning.
The word siloxane is derived from the words silicon, oxygen, and alkane. In some cases, siloxane materials are composed of several different types of siloxide groups; these are labeled according to the number of Si-O bonds. M-units: (CH3)3SiO0.5, D-units: (CH3)2SiO, T-units: (CH3)SiO1.5
|Cyclic siloxanes (cyclomethicones)||CAS||Linear siloxanes||CAS|
|L2, MM: hexamethyldisiloxane||107-46-0|
|D3: hexamethylcyclotrisiloxane||541-05-9||L3, MDM: octamethyltrisiloxane||107-51-7|
|D4: octamethylcyclotetrasiloxane||556-67-2||L4, MD2M: decamethyltetrasiloxane||141-62-8|
|D5: decamethylcyclopentasiloxane||541-02-6||L5, MD3M: dodecamethylpentasiloxane||141-63-9|
|D6: dodecamethylcyclohexasiloxane||540-97-6||L6, MD4M: tetradecamethylhexasiloxane||107-52-8|
Safety and environmental considerations
|This section requires expansion. (April 2015)|
Because silicones are heavily used in biomedical and cosmetic applications, their toxicology has been intensively examined. "The inertness of silicones toward warmblooded animals has been demonstrated in a number of tests." With an LD50 in rats of>50 g/kg, they are virtually nontoxic.
Cyclomethicones are ubiquitous because they are widely used in biomedical and cosmetic applications and can be found at high levels in American cities and can be toxic to aquatic animals in concentrations often found in the environment. The cyclomethicones D4 and D5 are bioaccumulative in some aquatic organisms, according to one report. However, Norwegian researcher Nicholas Warner cautioned that findings about bioaccumulation have been largely based on laboratory-studies, while field-studies of bioaccumulation are still contradicting each other. "Even if the concentrations of siloxanes we have found in fish are high compared to concentrations of classical contaminants like PCBs, several other studies in the Oslo fjord in Norway, Lake Pepin in the US and Lake Erie in Canada have shown concentrations of siloxanes to decrease as you proceed higher up in the food chain. This raises several questions about which factors influence the bioaccumulation potential of siloxanes."
In the European Union, D4 and D5 have been deemed hazardous as per the REACH directive. Canada regulates D4 under a pollution prevention plan. A scientific review in Canada in 2011 concluded that "Siloxane D5 does not pose a danger to the environment."
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