Dimethyldichlorosilane

Dimethyldichlorosilane

Names
Preferred IUPAC name Dichlorodi(methyl)silane
Other names Dichlorodimethylsilane, dichlorodimethylsilicon, dimethylsilicon dichloride, dimethylsilane dichloride, DMDCS
Identifiers
CAS Number	75-78-5  Y
3D model (JSmol)	Interactive image
ChemSpider	6158  Y
ECHA InfoCard	100.000.820
EC Number	200-901-0
PubChem CID	6398
RTECS number	VV3150000
UNII	8TSJ92JX69  Y
UN number	1162
CompTox Dashboard (EPA)	DTXSID9026425
InChI InChI=1S/C2H6Cl2Si/c1-5(2,3)4/h1-2H3 Y Key: LIKFHECYJZWXFJ-UHFFFAOYSA-N Y InChI=1/C2H6Cl2Si/c1-5(2,3)4/h1-2H3 Key: LIKFHECYJZWXFJ-UHFFFAOYAT
SMILES C[Si](C)(Cl)Cl
Properties
Chemical formula	C2H6Cl2Si
Molar mass	129.06 g·mol−1
Appearance	Colorless liquid
Density	1.07 g·cm−3 (l)
Melting point	−76 °C (−105 °F; 197 K)
Boiling point	70 °C (158 °F; 343 K)
Solubility in water	Decomposes
Hazards
GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H225, H315, H319, H335
Precautionary statements	P210, P233, P240, P241, P242, P243, P261, P264, P271, P280, P302+P352, P303+P361+P353, P304+P340, P305+P351+P338, P312, P321, P332+P313, P337+P313, P362, P370+P378, P403+P233, P403+P235, P405, P501
Flash point	−9 °C (16 °F; 264 K)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Y  verify  (what is  YN ?) Infobox references

Dimethyldichlorosilane is a tetrahedral organosilicon compound with the formula Si(CH₃)₂Cl₂. At room temperature it is a colorless liquid that readily reacts with water to form both linear and cyclic Si-O chains. Dimethyldichlorosilane is made on an industrial scale as the principal precursor to dimethylsilicone and polysilane compounds.

History

The first organosilicon compounds were reported in 1863 by Charles Friedel and James Crafts who synthesized tetraethylsilane from diethylzinc and silicon tetrachloride. ^[1] However, major progress in organosilicon chemistry did not occur until Frederick Kipping and his students began experimenting with diorganodichlorosilanes (R₂SiCl₂) that were prepared by reacting silicon tetrachloride with Grignard reagents. Unfortunately, this method suffered from many experimental problems. ^[2]

In the 1930s, the demand for silicones increased due to the need for better insulators for electric motors and sealing materials for aircraft engines, and with it the need for a more efficient synthesis of dimethyldichlorosilane. To solve the problem, General Electric, Corning Glass Works, and Dow Chemical Company began a partnership that ultimately became the Dow Corning Company. During 1941–1942, Eugene G. Rochow, a chemist from General Electric, and Richard Müller, working independently in Germany, found an alternate synthesis of dimethyldichlorosilane that allowed it to be produced on an industrial scale. ^[1] This Direct Synthesis, or Direct process, which is used in today’s industry, involves the reaction of elemental silicon with methyl chloride in the presence of a copper catalyst.

Preparation

Main article: Direct process

Rochow's synthesis involved passing methyl chloride through a heated tube packed with ground silicon and copper(I) chloride. ^[2] The current industrial method places finely ground silicon in a fluidized bed reactor at about 300 °C. The catalyst is applied as Cu₂O. Methyl chloride is then passed through the reactor to produce mainly dimethyldichlorosilane.

$${\displaystyle {\ce {2 CH3Cl + Si -> (CH3)2SiCl2}}}$$

The mechanism of the direct synthesis is not known. However, the copper catalyst is essential for the reaction to proceed.

In addition to dimethyldichlorosilane, products of this reaction include CH₃SiCl₃, CH₃SiHCl₂, and (CH₃)₃SiCl, which are separated from each other by fractional distillation. The yields and boiling points of these products are shown in the following chart. ^[3]

Product	Yield (%)	Boiling pt (°C)
(CH3)2SiCl2	80–90	70.0
CH3SiCl3	5–15	65.7
CH3SiHCl2	3–5	40.7
(CH3)3SiCl	3–5	57.3

Main reactions

Dimethyldichlorosilane hydrolyzes to form linear and cyclic silicones, compounds containing Si-O backbones. The length of the resulting polymer is dependent on the concentration of chain ending groups that are added to the reaction mixture. The rate of the reaction is determined by the transfer of reagents across the aqueous-organic phase boundary; therefore, the reaction is most efficient under turbulent conditions. The reaction medium can be varied further to maximize the yield of a specific product.

$${\displaystyle {\begin{alignedat}{4}n\ {\ce {(CH3)2SiCl2}}\ +&&n\ {\ce {H2O}}\ \longrightarrow &&{\ce {[Si(CH3)2O]}}_{n}\quad \,+&&2n\ {\ce {HCl}}\\m\ {\ce {(CH3)2SiCl2}}\ +&&\ (m\!+\!1)\ {\ce {H2O}}\ \longrightarrow &&\ \ {\ce {HO[Si(CH3)2O]}}_{m}{\ce {H}}\ +&&\ 2m\ {\ce {HCl}}\end{alignedat}}}$$

Dimethyldichlorosilane reacts with methanol to produce dimethoxydimethylsilanes.

$${\displaystyle {\ce {(CH3)2SiCl2 + 2CH3OH -> (CH3)2Si(OCH3)2 + 2 HCl}}}$$

Although the hydrolysis of dimethoxydimethylsilanes is slower, it is advantageous when the hydrochloric acid byproduct is unwanted: ^[3]

$${\displaystyle n\ {\ce {(CH3)2Si(OCH3)2}}+n\ {\ce {H2O -> [(CH3)2SiO]}}_{n}+2n\ {\ce {CH3OH}}}$$

Because dimethyldichlorosilane is easily hydrolyzed, it cannot be handled in air. One method used to overcome this problem is to convert it to a less reactive bis(dimethylamino)silane.

$${\displaystyle {\ce {(CH3)2SiCl2 + 4 HN(CH3)2 -> (CH3)2Si[N(CH3)2]2 + 2H2N(CH3)2Cl}}}$$

Another benefit to changing dimethyldichlorosilane to its bis(dimethylamino)silane counterpart is that it forms an exactly alternating polymer when combined with a disilanol comonomer. ^[4]

$${\displaystyle n\ {\ce {(CH3)2Si[N(CH3)2]2}}+n\ {\ce {HO(CH2)2SiRSi(CH2)2OH -> [(CH3)2SiO(CH2)2SiRSi(CH2)2O]}}_{n}+2n\ {\ce {HN(CH3)2}}}$$

Sodium–potassium alloy can be used to polymerize dimethyldichlorosilane, producing polysilane chains with a Si-Si backbone. For example, dodecamethylcyclohexasilane can be prepared in this way: ^[5]

$${\displaystyle {\ce {6 (CH3)2SiCl2 + 12 M -> [(CH3)2Si]6 + 12 MCl}}\ {\ce {(M = Na, K)}}}$$

The reaction also produces polydimethylsilane and decamethylpentasilane. Diverse types of dichlorosilane precursors, such as Ph ₂SiCl₂, can be added to adjust the properties of the polymer. ^[3]

In organic synthesis it (together with its close relative diphenyldichlorosilane) is used as a protecting group for gem-diols.^{[ citation needed ]}

Applications

Container with the substance, showing UN number 1162, in Japan.

The main purpose of dimethyldichlorosilane is for use in the synthesis of silicones, an industry that was valued at more than $10 billion per year in 2005. It is also employed in the production of polysilanes, which in turn are precursors to silicon carbide. ^[3] In practical uses, dichlorodimethylsilane can be used as a coating on glass to avoid the adsorption of micro-particles. ^[6]

References

1. Silicon: Organosilicon Chemistry. Encyclopedia of Inorganic Chemistry Online, 2nd ed.; Wiley: New Jersey, 2005. doi : 10.1002/0470862106.ia220
2. Rochow, Eugene G (1950). "Dimethyldichlorosilane". Inorg. Synth. 3: 56–58. doi:10.1002/9780470132340.ch14.
3. Polysiloxanes and Polysilanes. Encyclopedia of Inorganic Chemistry Online, 2nd ed.; Wiley: New Jersey, 2005. doi : 10.1002/0470862106.ia201
4. Ulrich Lauter,† Simon W. Kantor, Klaus Schmidt-Rohr, and William J. MacKnight, Vinyl-Substituted Silphenylene Siloxane Copolymers: Novel High-Temperature Elastomers. Macromolecules. 1999, 32, pp 3426-3431. doi : 10.1021/ma981292f
5. West, Robert; Brough, Lawrence; Wojnowski, Wieslaw (2007). "Dodecamethylcyclohexasilane". Inorganic Syntheses: 265–268. doi:10.1002/9780470132500.ch62. ISBN   9780470132500.
6. Monjushiro, H. et al. "Size sorting of biological micro-particles by Newton-ring nano-gap device" Elsevier December 7, 2005