Electrochemical synthesis of perfluoroalkylfluorophosphoranes

Details Electrochemical synthesis of perfluoroalkylfluorophosphoranes Electrochemical synthesis of perfluoroalkylfluorophosphoranes

2000-05-26

2001-07-24

Wong, Edna (Department: 1741)

Electrolysis: processes, compositions used therein, and methods

Electrolytic synthesis

Preparing organic compound

Reexamination Certificate

active

06264818

ABSTRACT:

The invention relates to a process for preparing perfluoroalkylfluorophosphoranes of the general formula
(C
n
F
2n+m
)
y
PF
5−y
  (I)
where
n is 1, 2, 3, 4, 5, 6, 7 or 8
m is +1 or −1 and
y is 1, 2 or 3,
where the ligands (C
n
F
2n+m
) may be identical or different, and also to their use as electrolytes and as precursors for conducting salts, and to their employment in lithium batteries.
Perfluoroalkylfluorophosphoranes are of widespread interest as starting materials for synthesizing a variety of organofluorophosphorus compounds (N. V. Pavlenko et. al., Zh. Obshch. Khim. (Russ.) 1989, Vol. 59, 534-537).
Perfluoroalkylfluorophosphoranes may be synthesized in a variety of ways, e.g. starting from elemental phosphorus and perfluoroalkyl iodides (F. W. Bennett et. al., J. Chem. Soc. 1953, 1565-1571). This reaction normally leads initially to the formation of a complex mixture of mono-, bis- and trisperfluoroalkylphosphanes, which can then be converted by chlorination and fluorination processes into the corresponding phosphoranes (M. Görg et. al., J. Fluorine Chem. 1996, Vol. 79, 103-104). A variety of by-products are produced by the side reactions, and these are difficult to remove and dispose of. One of the disadvantages of this synthetic route is the reaction in the presence of Hg, which remains detectable in the downstream products. Products prepared by this process are unsuitable for use in batteries. In addition, only small laboratory-scale batches can be prepared.
A relatively new method (J. J. Kampa et. al., Angew. Chem. 1995, Vol. 107, 1334-1337) for synthesizing trisperfluoroalkyldifluorophosphoranes is to react elemental fluorine with the corresponding alkyl phosphanes. The disadvantages of this method are complicated operation and very expensive starting materials. The fluorinated solvents needed for the process are expensive to prepare, special safety precautions have to be taken when they are used, and they are expensive to dispose of once used.
The most convenient method known hitherto is the electrochemical fluorination of trialkylphosphine oxides described in DE 26 20 086, using Simons' electrochemical fluorination. The disadvantages of the process are that only trisperfluoroalkylphosphoranes can be prepared and that the yields, from 40 to 50%, are low and decrease still further as the chain length of the alkyl radical rises. Another disadvantage is the unavoidable parallel formation of toxic and explosive by-products, e.g. oxygen difluoride.
The methods known hitherto for obtaining perfluoroalkylphosphoranes by electrochemical fluorination require the presence of strongly electro-negative substituents, such as fluorine or chlorine, or of oxygen, to stabilise the electrofluorination starting materials with respect to the operating medium (DE 19641138 and WO 98/15562). This is confirmed in the literature (Journal of Fluorine Chemistry 75, 1995, 157-161).
The object of the present invention is therefore to provide a cost-effective process which is simple to carry out and which gives the perfluoroalkylfluorophosphoranes in improved yields and high purities, so that the products prepared are suitable for employment in battery electrolytes. Another object of the invention is to provide a process which avoids the formation of toxic and explosive by-products.
The object of the invention is achieved by electrochemical fluorination of alkylphosphoranes or of alkylphosphanes of the general formula (II) with identical or different alkyl substituents on the phosphorus. This permits the synthesis of cyclic, linear and branched perfluoroalkylphosphoranes of the general formula (I) from compounds of the general formula (II) in high yields by the following reaction scheme
where
n is 1, 2, 3, 4, 5, 6, 7 or 8,
m is +1 or −1,
X is H, Cl or F,
Y is 1, 2, or 3 and
Z is 3 or 5, with the condition that
X is H, Cl or F, if Z=3 and
X is Cl or F, if Z=5.
From the alkyls class use is made of cyclic, linear or branched methyl, ethyl, propyl, butyl, pentyl, hexyl, heptyl and octyl ligands.
The invention therefore provides a process for preparing perfluoroalkylfluorophosphoranes by an electrochemical synthesis.
The starting substances used according to the invention from the alkylphosphoranes and alkylphosphanes classes form the corresponding phosphonium salts in anhydrous hydrogen fluoride, and these have very good solubility in hydrogen fluoride. Advantageously, solutions with phosphorane or phosphane concentrations from 30 to 60% are not combustible, unlike the pure alkylphosphoranes or alkylphosphanes, and can therefore be used as starting materials which are easy to handle.
It has been found that no explosive substances are formed during the novel electrochemical fluorination of alkylphosphoranes or alkylphosphanes.
The main by-products of the novel electrochemical fluorination are phosphorus pentafluoride and fluoroalkanes, which in turn may be used industrially as ozone-friendly propellant, solvent or synthesis building block.
In contrast to previous assumptions it has been found that it is particularly the unsubstituted trialkylphosphanes having chain lengths of C22 which have particularly high suitability as starting materials for electrochemical perfluorination reactions. Contrary to expectations their stability is very high. Whereas trimethylphosphane is extensively degraded by the electrochemical fluorination, probably due to the cleavage of difluorocarbene, etc., even triethylphosphane is converted with very good yields into triperfluoroethyldifluorophosphorane.
To prepare the compounds according to the invention, use is made of an electrolysis cell which consists of, for example, a cylindrical double-walled vessel, and the material of which, e.g. stainless steel, is stable with respect to the prevailing reaction conditions. The electrolysis cell comprises an electrode package with alternating nickel anodes and cathodes made from HF-resistant materials with in each case an effective surface area of, for example 4.58 dm
2
for nickel anodes and nickel cathodes. The electrolysis cell has a commercially available meter to determine the consumption of current during the reaction. To carry out the process, the cell is cooled to temperatures of from −15° C. to 19° C., or temperatures up to 40° C. may be used with increased pressure. Experiments have shown that good results are achieved at from −10° C. to 10° C. However, the temperature preferably used is 0° C., since this temperature is particularly easily maintained, e.g. by ice-water cooling. The cell has a reflux condenser to condense gaseous reaction products. The gas outflow is cooled to temperatures of from −10° C. to −35° C. Cooling to from −15° C. to −33° C. is preferred. It is particularly preferable to carry out operations at −30° C. by using ethanol as cooling medium.
An appropriate amount of liquid hydrogen fluoride is pre-electrolysed for from 2 to 100 hours, depending on moisture content. 48 hours are generally sufficient. The starting materials are used batchwise in the form of 10 to 70% solutions in HF, since these are not combustible. The experiments have shown that the best results are achieved with 30 to 45% solutions. The liquid reaction products are collected at the base of the cell. Gaseous products are conducted away via the reflux condenser and condensed with the aid of two cooling traps in succession which are cooled to from −50° C. to −100° C. The temperature range used is preferably from −60° C. to −85° C., since in this temperature range most of the gaseous products condense. It is very particularly preferable to work at −78° C. with easy cooling by means of dry ice. The process is carried out at a pressure of from 1 to 3 bar. Working at higher pressure requires peripheral equipment specifically designed for this pressure and resulting in considerable costs. For cost-effectiveness reasons it is preferable to work at a small gauge pressure of from 1 to 0.5 bar. The reacti

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