WO2014181194A2 - Appareil et procédé de production en phase condensée de trisilylamine - Google Patents

Appareil et procédé de production en phase condensée de trisilylamine Download PDF

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WO2014181194A2
WO2014181194A2 PCT/IB2014/001629 IB2014001629W WO2014181194A2 WO 2014181194 A2 WO2014181194 A2 WO 2014181194A2 IB 2014001629 W IB2014001629 W IB 2014001629W WO 2014181194 A2 WO2014181194 A2 WO 2014181194A2
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solvent
monohalosilane
trisilylamine
solution
reaction mixture
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PCT/IB2014/001629
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WO2014181194A3 (fr
Inventor
Cole J. Ritter, Iii
Matthew Damien STEPHENS
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L'air Liquide Societe Anonyme Pour I'etude Et L'exploitation Des Procedes Georges Claude
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Priority claimed from US13/852,614 external-priority patent/US9701540B2/en
Priority claimed from US14/065,088 external-priority patent/US9446958B2/en
Application filed by L'air Liquide Societe Anonyme Pour I'etude Et L'exploitation Des Procedes Georges Claude filed Critical L'air Liquide Societe Anonyme Pour I'etude Et L'exploitation Des Procedes Georges Claude
Publication of WO2014181194A2 publication Critical patent/WO2014181194A2/fr
Publication of WO2014181194A3 publication Critical patent/WO2014181194A3/fr

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    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
    • C01B21/00—Nitrogen; Compounds thereof
    • C01B21/082—Compounds containing nitrogen and non-metals and optionally metals
    • C01B21/087—Compounds containing nitrogen and non-metals and optionally metals containing one or more hydrogen atoms
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01C—AMMONIA; CYANOGEN; COMPOUNDS THEREOF
    • C01C1/00—Ammonia; Compounds thereof
    • C01C1/16—Halides of ammonium
    • C01C1/164—Ammonium chloride

Definitions

  • This invention relates to a batch method for synthesizing silylamines, particularly trisilylamine in a solvent.
  • the invention relates to a process that promotes reaction conditions suitable for a high efficiency synthesis of silylamines.
  • the primary silylamine of interest is trisilylamine. Production of disilylamine in commercial quantities is also within the scope of the present invention.
  • TSA Trisilylamine
  • Wells and Schaeffer J. Am. Chem. Soc, 88:1, 37 (1996) discuss a batch method of preparing trisilylamine by the reaction silyl chloride with ammonia. They report the yield of trisilylamine varied depending on the method of mixing and the purity of the reactants.
  • Wells and Schaeffer allowed the reactants to mix in the gas phase by introducing the ammonia from below into a 1 liter bulb containing silylchloride. After introducing the gaseous ammonia very slowly, the reaction bulb and contents were allowed to remain at room temperature for 15 min. Copious amounts of white solid were precipitated on the walls of the bulb as soon as mixing occurred. The product was removed and the trisilylamine recovered. The process yield was about 77% of the theoretical amount of trisilylamine.
  • US 2010/0310443 is directed to a tubular flow gas phase reactor and a process for the synthesis of silylamines which have been found to produce high volumes, at high yield efficiencies of silylamines.
  • the reactor has a combination of characteristics found in plug flow and laminar flow devices. This combination of properties results in a high volume high efficiency synthesis of silylamines.
  • the primary silylamine of interest is trisilylamine. Production of disilylamines in commercial quantities is also within the scope of the present invention. This process produces high volumes of ammonium halide requiring the reaction tube to be opened and cleaned after each production batch is produced. This is a labor intensive process leading to significant down time.
  • the present invention is directed to a condensed phase batch process for synthesis of TSA comprising: (a) adding a solvent to a reactor vessel; (b) cooling the solvent; (c) condensing monohalosilane into the solvent to form a solution; (d) adding anhydrous ammonia into the solution to form a reaction mixture; (e) separating the silylamines, excess monohalosilane and TSA from the reaction mixture; and (f) purifying the silylamines to obtain TSA;
  • the general benefit of this approach is the formation of TSA in the condensed phase followed by vacuum stripping of the product from the reaction slurry and discharge of the waste salt/solvent slurry from the reactor vessel after which the reactor can be re-charged with solvent and excess, liquefied monohalosilane for another batch synthesis.
  • the reactor does not have to be cleaned before the next batch run as the ammonium chloride salt byproduct of the reaction is removed as a slurry in the solvent.
  • Suitable solvents such as anisole (methoxybenzene) provide vapor pressure depression/boiling point elevation of the MCS reagent, which promotes the formation of liquefied MCS and favorable condensed-phase disilylamine (“DSA”) intermediate reaction kinetics.
  • anisole methoxybenzene
  • the solvent acts as a uniform heat transfer medium in which byproduct waste salt is dispersed and localized predominantly in the reaction mixture.
  • silylamines of the present invention are produced in accord with the following reaction sequence:
  • FIG. 1 is a simplified schematic diagram of a condensed phase reactor of the invention utilizing a Schlenk tube.
  • FIG. 2 is a simplified schematic diagram of a condensed phase reactor of the invention utilizing a Parr reactor vessel.
  • FIG. 3 is the graphic representation of temperature and pressure versus time for Experiment 8.
  • FIG. 4 is the graphic representation of temperature and pressure versus time for Experiment 9.
  • FIG. 5 is the graphic representation of temperature and pressure versus time for Experiment 11.
  • FIG. 6 is the graphic representation of temperature and pressure versus time for Experiment 12.
  • FIG. 7 is the graphic representation of temperature and pressure versus time for Experiment 13.
  • FIG. 8 is the graphic representation of solvent polarity (ET N ) and Lewis Basicity (Donor Number "DN”) for specific solvents.
  • the general method of this invention includes the following:
  • Forming silylamines in the reaction mixture include, volume of the solvent, concentration of the monohalosilane, temperature of the solvent reaction mixture, mixing efficiency, and the rate of heat transfer out of the reaction vessel.
  • a preferred rate of addition of ammonia for moderate sized batch reactions would be from about 100 mg to 5 g/minute, for larger and production batches the rate of addition would be a function of batch size and therefore would be proportionately greater; a preferred temperature of the reaction solvent throughout the addition of ammonia is from about 70 °C to just above the freezing point of the solvent and reactant solution.
  • Reaction product silylamines are trisilylamine and disilylamine.
  • Preferred methods of separation include vacuum stripping or distilling the product mixture, which may be preceded by filtration, at reduced pressure once all of the ammonia has been added and collecting the distillates which contain the product(s) in a low temperature cryotrap.
  • the temperature of the reaction mixture may be raised during vacuum stripping. In pilot scale batches the reaction mixture temperature has be raised to about 100 °C during vacuum stripping.
  • the preferred aminosilane is trisilylaming ("TSA"); preferred purification processes are fractionation or distillation.
  • the reactor can then be re-charged for another batch synthesis.
  • a process for preparing silylamine comprising:
  • the solvent has a DN between about 6 to about 24 and an ⁇ ⁇ from about 0.1 to about 0.4.
  • anisole is the solvent and an excess of about 20 to about 50 mole % monohalosilane to ammonia is used and an initial reaction temperature of about 10 °C to about 60 °C.
  • the monohalosilane is MCS.
  • the preferred ammonia addition process is to react the ammonia and MCS in the solution and limit any gas-phase reactions in the headspace above the solution thereby avoiding ammonium chloride build up on the exposed surface of the reactor vessel and down stream of the reaction vessel such as in the cryogenic traps.
  • Ammonium chloride salt found in the downstream storage vessels is referred to as "down stream salt.”
  • the solvent aspect ratio is defined as the relationship of the height of solvent (liquid level) divided by the internal diameter of the reactor and is important relative to the path the ammonia or intermediate disilylamine (DSA) product has to travel to break through the surface of the liquid at the solvent-headspace interface.
  • the lower limit value for the aspect ratio is not critical but is an experienced based guide for setting an anhydrous ammonia gas flow/feed rate in a particular reactor in light of the following parameters; solvent, MCS concentration, temperature and pressure.
  • Preferred operation of the reactor is achieved when the feed rate of the ammonia gas is adjusted such that all of the ammonia is reacted with MCS in solution and none of ammonia gas escapes the solution to enter the headspace above the solvent surface.
  • Better gas dispersion methods, better mixing and a higher solvent aspect ratio are process methods that will support a higher ammonia gas flow rate thereby speeding processing time.
  • the preferred initial temperature of the process is about -55 °C to about 60 °C.
  • the lower limit of the operating temperature of the reaction process is the melting point of MCS in the solvent and the upper temperature limit is determined by engineering conditions such as to avoid product decomposition and reduced efficiency of the process.
  • the upper temperature limit is determined by engineering conditions such as to avoid product decomposition and reduced efficiency of the process.
  • anisole depending on how much MCS is added, there is a considerable melting point depression below the anisole melting point of -37.3 °C.
  • the melting point of a given concentration of MCS in a particular solvent is easily determined by one skilled in the art without undue experimentation.
  • the solvent of the present invention acts as a heat transport medium and as a medium for dispersing ammonium chloride formed during the formation of TSA.
  • the solvent must have all of the following characteristics:
  • the ratio of the vapor pressure of solvent to the vapor pressure of TSA at a given temperature is about 1 :5, preferably about 1 : 10 or less to facilitate vacuum stripping of the reaction products from the solvent.
  • a ratio of vapor pressure of 1 : 10 will be considered less than a vapor pressure ratio of 1 :5.
  • a vapor pressure ratio of 100: 1 will be considered greater than a ration of 10: 1.
  • the solvent is anisole and at a temperature of about 20 to about 40 °C the ratio of vapor pressure for anisole to TSA is 3.5:315 which equals about 1 :90.
  • the vapor pressure ratio is an important indicator of the separation efficiency for removing TSA and DSA from the solvent by vacuum stripping or distillation.
  • a solvent with a low vapor pressure with respect to the vapor pressure of DSA and TSA will facilitate vacuum stripping of the DSA and TSA from the reaction solvent and collecting the DSA and TSA products.
  • a solvent with a high vapor pressure with respect to DSA and TSA will also facilitate removal of the solvent from the DSA and TSA leaving a concentrated DSA and TSA product in a storage vessel that will not collect the lower boiling higher vapor pressure solvent.
  • the DSA and TSA products collected may then be further purified by standard techniques such as those disclosed herein and in the literature.
  • Suitable solvents are solvents that are aprotic, non-acidic (Lewis acidic) and solvents that do not form strong hydrogen bonds (N-H a source of hydrogen bonding). Suitable solvents have a Donor Number ("DN") between from about 6 to about 28 and preferably between from about 6 to about 24 and a solvent polarity ("ET N ”) between from about 0.1 to about 0.4.
  • DN Donor Number
  • ET N solvent polarity
  • DN is a quantitative measure of Lewis basicity.
  • a donor number is defined as the negative enthalpy value for the 1 : 1 adduct formation between a Lewis base and the standard Lewis acid SbCl 5 (antimony
  • the units are kilocalories per mole.
  • the donor number is a measure of the ability of a solvent to solvate cations and Lewis acids. The method was developed by V. Gutmann in 1976, "Solvent effects on the reactivities of organometallic compounds". Coord. Chem. Rev. 18 (2): 225. Likewise Lewis acids are characterized by acceptor numbers. In summary, the Gutmann Acceptor (AN) and Donor Number (DN) are measures of the strength of solvents as Lewis acids or bases. The Acceptor Number is based on the 31 P-NMR chemical shift of triethylphosphine oxide in the solvent. The Donor Number is based on the heat of reaction between the 'solvent' and SbCl 5 in CH 2 C1CH 2 C1 .
  • Preferred solvents are selected from the group consisting of aliphatic
  • solvents were selected that had at least about a 1 : 10 vapor pressure ratio (solven TSA) relative to TSA in which TSA could easily be vacuum-stripped with little solvent transport.
  • TSA has a vapor pressure of 315 torr at 25 °C
  • anisole has a vapor pressure of 3.5 at the same temperature.
  • a preferred solvent is anisole.
  • a non- limiting list of solvents useful in the present invention would include: anisole (methoxybenzene), high boiling ethers; di-n-butyl ether, di-t-butyl ether, di-sec-butyl ether, di-n-hexyl ether, dioxane (two oxygens, cyclic ether), diglyme. See above and Table 2, high volatility ethers may work as well such as diethyl ether and tetrahydrofuran (“THF"); these latter ethers may be more difficult to separate from TSA due to their proximities in boiling points and vapor pressures.
  • THF diethyl ether and tetrahydrofuran
  • the high-boiling ethers are more preferred, aliphatic hydrocarbons, cyclic and ring-fused hydrocarbons, aromatic hydrocarbons, and fused aromatic compounds that have melting points below 0 °C are preferred. Mixtures of solvents are also within the scope of the invention.
  • a 250 mL Schlenk tube 19, fitted with an internal thermocouple probe (1 ⁇ 2" o.d. stainless steel, T-type) 15, 1 ⁇ 2" o.d. stainless steel ammonia sparge tube 18, and 1 ⁇ 4" o.d. HDPE tubing was charged with 100 mL of anhydrous anisole under nitrogen. The tube was placed in a temperature controlled bath. The end of the sparge tube was raised above the liquid level and the solvent was cooled to -35 °C (freezing point of anisole is - 37 °C). The head space nitrogen was then removed in vacuo from the Schlenk tube, with agitation of the solvent with magnetic stir bar 17, to a final pressure of less than 1 torr.
  • a 7.8L (internal volume) carbon steel cylinder, which contained 900 torr pressure MCS (26.4 g, 397 mmoles) 25 was then added (through tube 27) into the adjacent U-trap (not shown) with the reaction tube closed.
  • the valve adapter (see Figure 1) 29 on the Schlenk tube was then opened and the MCS in the U-trap was allowed to warm to ambient temperature, upon which it condensed into the reaction tube 19.
  • the tube was cooled further to -60 °C and the internal pressure dropped to approximately 63 torr.
  • the inert gas purge was reduced by adjusting the rotameter (14, Cole-Parmer 65-mm correlated flow meter, Aluminum with SS float; PN: EW-32044-06) to a lower setting (approximately 80% flow reduction).
  • the anhydrous ammonia feed was then started by closing 24 and opening 12; the ammonia pressure and flow rate were adjusted by manipulating 11 and 14 (FM setting at 50).
  • the sparge tube was quickly submerged into the MCS/anisole solution 16 and a white precipitate was immediately formed.
  • the yield of TSA based on the amount of ammonia "consumed” in the reaction, is 74.4% (98.8% purity checked by GC-MS analysis) with a total hydride recovery of 90+% (based on silicon content). No evidence of solvent fragmentation contamination was observed in the analysis of purified TSA.
  • a 600 cc Parr 100 reactor was charged with 200 mL of anhydrous anisole 106 under nitrogen. (The reaction apparatus is shown in Figure 2). The reactor was then cooled in an ice bath (not shown) and the nitrogen removed in vacuo. Monochlorosilane (65.7 g, 987 mmol., 200 mole % excess) was charged into the reactor through a dip tube 101. The internal pressure of the reactor was approximately 900 Torr at 0 °C. The dip tube was then purged with nitrogen delivered through flow meter 111 and tube 107 to clear the line and dip tube. Anhydrous ammonia was immediately added to the reactor through the dip tube.
  • the reactor was stirred with a stirring rod 102 throughout the entire reagent loading and reaction time at a rate of 250 rpm.
  • the temperature and pressure was monitored via an internal K-type thermocouple 103 and a 0-60 psig pressure gauge 104.
  • Anhydrous ammonia (7.5 g, 440 mmol.) was added to the reactor at a rate of 140 mg/min. over the course of 54 minutes from the ammonia cylinder (440 cc sslb containing 6.7 g NH 3 , 393 mmoles; internal pressure approximately 100 psig) 110 through flow meter 109 and valve 108.
  • the reaction mixture was stirred at 0 °C for an additional 45 minutes and the volatiles removed under dynamic vacuum.
  • the product gas was collected in a U-trap (not shown) held at -196 °C downstream from a solvent trap (U-trap) cooled to -35 °C. Less than 2 mL of solvent was collected in the solvent trap.
  • the product mixture was transferred to a 440 cc stainless steel lecture bottle and the contents were purified via fractional condensation using two U-traps cooled to -78 and -196 °C.
  • the contents of the -78 °trap contained 9.84 g TSA (92 mmoL, 83% yield) and the -196 °C trap contained excess MCS and trace silane.
  • Examples 3 to 7 were prepared by the procedure of Example 2 under the conditions described in Table 1. The yield of each example is reported in Table 1.
  • the yield and mole percent hydrides recovered results may contain residual solvent contamination.
  • the "% salt downstream” indicates a weight percentage of ammonium chloride that is collected in the cryo-trap from the maximum amount calculated (theoretical amount) for each experiment.
  • the reactants are contacted in a manner that optimizes reaction conditions thereby avoiding excessive reaction conditions such as heat build up from the exothermic reaction which can result in product decomposition and the formation of synthesis byproducts, notably silane and silazane polymers.
  • the process causes the ammonium halide by product of the reaction to stay in the reactor while the gaseous products such as disilylamine and trisilylamine are vacuum stripped from the solvent mixture and flow out of the reactor and are collected in a cold trap vessel substantially free of ammonium halide and solvent which can cause decomposition of the hydride products.
  • the ammonium halide byproduct of the synthesis is crystalline under reaction conditions, therefore it remains in the solvent in the reactor while the gaseous products continue to travel up the reactor and out of the reactor.
  • the boiling point of trisilylamine is 52 °C at one atmosphere.
  • the reactor is run at reduced pressure or at pressures up to about 2000 Torr.
  • the reactor is kept at pressure of about equal to or lower than the vapor pressure of the monohalosilane at any given reaction temperature.
  • the reactor pressure will drop as the monohalosilane is depleted.
  • a preferred operating pressure would be about two atmospheres or less.
  • Maximum operating pressure is about 80 psig.
  • the solvent has a DN between about 6 to about 24 and an ⁇ from about 0.1 to about 0.4.
  • the temperature of the solvent may optionally be adjusted prior to condensing monochlorosilane into the solvent to form a solution.
  • the temperature of the solvent may be adjusted to be between from about 70 °C to about - 78 °C, preferably from about 60 °C to about - 20 °C, and most preferably from about 50 °C to about -20 °C.
  • Monohalosilanes useful in the present invention include monofluorosilane, monochlorosilane, monobromosilane and monoiodosilane. Monochlorosilane is preferred.
  • TSA was synthesized in a 4L Autoclave stirred-tank reactor with anisole as the solvent media. A total of six runs were conducted with varying target reaction temperatures, excess MCS amounts and the solvent to NH 3 ratio. Based on the results of the runs the following reaction conditions are recommended:
  • Reaction Temperature equals about 20 °C to about 60 °C
  • Excess MCS amount equals about 25 % to about 40 % excess to theoretical MCS amount on a mole to mole basis.
  • Solvent to NH 3 mass ratio equals about 25: lto about 30: 1. Solvent to NH 3 mass ratio will be expressed as a whole number throughout this specification.
  • FIG. 3 The temperature and pressure profile in the reactor as a function of time is shown in FIG. 3.
  • the top broken line in FIG. 3 represents temperature (°C) and the bottom solid line represents pressure (psig)
  • the temperature and pressure profile as a function of time is shown in FIG. 4.
  • the top line in FIG. 4 represents temperature (°C) and the bottom line represents pressure (psig).
  • the TSA yield was 85.4%.
  • Target reaction temperature 25 °C / room temperature
  • Excess MCS 39 %
  • Solvent to NH 3 ratio 25
  • the pressure and temperature profile during the run is given in FIG. 5.
  • the top line in FIG. 5 represents temperature (°C) and the bottom line represents pressure (psig).
  • the TSA yield was 94.3%.
  • the above results indicate that as the MCS in the Iqiuid phase is consumed, the reaction shifts to the vapor phase with the formation of TSA increasing with time, with a corresponding decrease of MCS.
  • the increase of SiH 4 amount can either be (i) SiH 4 in the MCS feed or (ii) decomposition of TSA in anisole due to the presence of salts.
  • Target reaction Temp 25 °C or room temperature
  • the pressure and temperature profile during the run is as follows in FIG. 6.
  • the top line in FIG. 6 represents temperature (°C) and the bottom line represents pressure (psig).
  • the TSA Yield was 81.9. %
  • the reactor pressure was steady at about 5 psig for most of the run but after about 120 minutes the pressure increased rapidly. Samples of vapor phase in the reactor were taken at different times during the run.
  • An analysis of the MCS feed showed that it contained about 1% silane and so based on the amount of MCS added it can be estimated that 1.08 gms of SiH 4 was added in the feed.
  • An overall mass balance of silane showed that about 50% of the silane in the feed MCS is in the vapor phase and so the remaining should be solubilized in anisole.
  • An independet set of tests conducted with MCS and anisole showed that about 66% of the S1H 4 in the MCS feed can be accounted for in the vapor phase.
  • Target reaction Temp 25 °C or room temperature
  • Excess MCS 27 %
  • Slovent/NH 3 Mass ratio 26
  • NH 3 addition rate 0.5 grams/min
  • the pressure and temperature profile during the run is as follows in FIG. 6.
  • the top line in FIG. 7 represents temperature (°C) and the bottom line represents pressure (psig).
  • the TSA Yield was 50.9%.
  • TSA in was analyzed by a gas chromatographic procedure. The analysis conditions are indicated below.
  • Abboud and Notario provide extensive tables listing the properties of a number of solvents.
  • Abboud Table la assigns numbers, Abboud Number, to a listing of compounds.
  • Abboud Table 2a provides the ET N for the compounds and Abboud Table 2d provides the DN for the compounds.
  • Table 2 below compiles a non-limiting list of solvents, inventive and non- inventive.
  • Inventive compounds will have an ET N between about 0.1 and about 0.4 and a DN between about 6 and about 28.
  • Figure 8 graphically represents the inventive ranges of ET N and DN and the relationship of several inventive and non-inventive solvents.
  • a non-limiting list of solvents suitable for the present invention includes: acetonitrile, butanenitrile, diethyl ether, di-n-propyl ether, di- isopropyl ether, dibenzyl ether, anisole, ethyl phenyl ether, bis(2-chloroethyl) ether, diglyme, furan, tetrohydrofuran (THF), 2-methyl THF, tetrahydropyrane and 1 ,4-dioxane.
  • E T (30) and E T N [0125] are possibly the most widely used empirical solvent 'polarity' scales.
  • the E T (30) value for a specified solvent is defined as the molar transition energy (in kcal/mol) for the long wavelength electronic transition of dye la, 2,6-diphenyl-4-(2,4,6-triphenylpyridinio)-phenolate as a solution in this solvent at 25.0 °C and at a pressure of 0.1 MPa.
  • ⁇ (30) is obtained from the experimentally determined vacuum wavelength of the absorption maximum of this transition (lmax) through eqn (11):
  • Equation (12) allows the indirect estimation of the ⁇ (30) values for low polarity solvents.
  • E T N is a dimensionless 'normalized' scale, defined through eqn 13:
  • TMS tetramethylsilane
  • the DN scale has been very widely used, particularly in the field of coordination chemistry.

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Abstract

La présente invention concerne un procédé par lots, en phase condensée, pour la synthèse de trisilylamine (TSA). Selon l'invention, un procédé de synthèse amélioré consiste à incorporer un solvant pour aider à favoriser une réaction en phase condensée entre de l'ammoniac gazeux (ou liquide) et du monochlorosilane (MCS) liquéfié, avec de bons rendements. Ce procédé favorise l'élimination de sous-produits résiduaires, avec un temps d'arrêt de réacteur faible à nul, une réduction sensible de la contamination par des matières solides en aval, et l'obtention d'un produit de pureté élevée provenant d'une distillation de première passe.
PCT/IB2014/001629 2013-03-28 2014-03-25 Appareil et procédé de production en phase condensée de trisilylamine WO2014181194A2 (fr)

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US13/852,614 US9701540B2 (en) 2011-10-07 2013-03-28 Apparatus and method for the condensed phase production of trisilylamine
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US14/065,088 US9446958B2 (en) 2011-10-07 2013-10-28 Apparatus and method for the condensed phase production of trisilylamine
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