Electrolysis: processes – compositions used therein – and methods – Electrolytic synthesis – Preparing organic compound
Reexamination Certificate
2001-01-12
2002-03-05
Wong, Edna (Department: 1741)
Electrolysis: processes, compositions used therein, and methods
Electrolytic synthesis
Preparing organic compound
Reexamination Certificate
active
06352635
ABSTRACT:
BACKGROUND OF THE INVENTION
This invention concerns the preparation of certain 4-aminopicolinic acids by electrochemical reduction. More particularly, this invention concerns the selective reduction of halogen substituents in the 5-position of halogenated 4-aminopicolinic acids in the presence of halogen substituents in the 3- and 6-positions.
A co-pending U.S. Patent application filed concurrently with this application discloses certain 4-amino-3-halopicolinic acid derivatives and their use as herbicides. It would be desirable to be able to produce these herbicides in as few steps as possible from commercially available raw materials, such as 4-amino-3,5,6-trichloropicolinic acid (picloram).
While chemical reductions of halogenated pyridines are known, see, for example, U.S. Pat. No. 4,087,431 in which hydrazine is employed as a reducing agent, efficiency of material utilization is poor and costs are relatively high. Electrolytic reductions, on the other hand, can be very efficient as well as selective. U.S. Pat. No. 3,694,332 discloses the selective electrolytic reduction of halogenated pyridines and halogenated cyanopyridines in the 4-position. U.S. Pat. No. 4,217,185 discloses the electrolytic reduction of tetrachloropicolinic acid in the 4- and 5-positions. U.S. Pat. 4,242,183 discloses the electrolytic reduction of symmetrical tetrachloropyridine to 2,3,5-trichloropyridine using an activated silver mesh cathode. This patent also claims methods for activating the silver cathode. Russian Patent SU 1807686 A1 discloses the electrolytic reduction of polychlorinated pyridinecarboxylic acids. Such selective electrolytic reductions are limited to halogenated pyridines that contain only carboxylic acid or cyano substituents. It would be desirable to have electrochemical methods that could selectively reduce halogenated pyridines containing other substituents.
SUMMARY OF THE INVENTION
It has now been found according to the present invention that 4-amino-3-halopicolinic acids can be prepared by the electrochemical reduction of the corresponding 4-amino-3,5-dihalopicolinic acids. More particularly, the present invention concerns a process for the preparation of a 4-amino-3-halopicolinic acid of Formula I
wherein
X represents Cl or Br;
Y represents H, F, Cl, Br or C
1
-C
4
alkyl; and
R independently represents H or C
1
-C
4
alkyl
which comprises passing a direct or alternating electric current from an anode to a cathode through a solution of a 4-amino-3,5-dihalopicolinic acid of Formula II
wherein
X, Y and R are as previously defined, and
wherein
both of X are either Cl or Br at a cathode potential of about −0.4 to about −1.7 volts relative to an Ag/AgCl (3.0 M Cl
−
) reference electrode and recovering the product, with the proviso that, when X is Cl, Y is not Br. Surprisingly, the halogen in the 5-position is selectively removed in the presence of the 4-amino group in high yield.
DETAILED DESCRIPTION OF THE INVENTION
The present invention concerns the selective electrochemical reduction of the 5-halo substituent of 4-amino-3,5-dihalopicolinic acids. As used herein, the term “halogen” or “halo” refers to Cl or Br.
The reactions involved in the reduction of the 4-amino-3,5-dihalopicolinic acid may be depicted as follows:
A) Neutralization:
B) Cathode Reaction:
C) Anode Reaction:
2(OH
−
)→½O
2
+H
2
O+2
e
−
D) Overall Reaction:
The carboxylic acid is recovered by acidifying the reaction mixture and recovering the product by conventional techniques.
The desired electrolytic reduction is carried out by techniques that are generally known in the art. In general, the starting 4-amino-3,5-dihalopicolinic acid is dissolved in a solvent to form an electrolyte which is added to the electrolytic cell while enough current is passed through the electrolyte until the desired degree of reduction is obtained.
It should be appreciated by those skilled in the art that the reduction potential of bromine is about 0.5 volt higher (less negative) than the comparable chlorine potential. The bromine will always be reduced off first. Thus, when X is Cl, Y cannot be Br.
The design of the electrolysis cell is not critical. The electrolysis can be conducted batch-wise, or in a continuous or semi-continuous fashion. The cell may be a stirred tank containing the electrodes or a flow cell of any conventional design. In some cases, it may be desirable to employ a separator to divide the cell into separate anodic and cathodic compartments. Examples of useful separator materials are various anion and cation exchange membranes, porous Teflon, asbestos, and glass. While the use of three electrodes in which the potential of the cathode is controlled relative to a reference electrode is preferred, the electrolysis can alternatively be performed using only two electrodes, an anode and a cathode, and controlling either the cell current, the cell voltage, or both. For convenience, a 3-electrode undivided cell in which the electrolyte serves as both the catholyte and the anolyte is preferred.
The anode can be any chemically inert material including, for example, platinum, graphite, carbon, metal oxides such as silver oxide on silver, or alloys such as Hastelloy C, with graphite, carbon and Hastelloy C being preferred. Similarly the cathode can be constructed from a number of materials, including mercury, lead, iron, tin, zinc or silver, with silver being preferred. Electrodes may be in the form of plates, rods, wires, screens, gauze, wool, sheets or pools, with expanded mesh screens being preferred. The anode or cathode may also consist of a coating applied to another material, an example of which is a noble metal oxide such as ruthenium oxide coated onto titanium.
The most preferred cathodes are activated silver cathodes prepared as described in U.S. Pat. Nos. 4,217,185 and 4,242,183. Such activated cathodes can be prepared by depositing a layer of silver microcrystals on a conductive substrate to form a composite electrode or by anodization of a silver electrode itself. For example, to illustrate the latter, an unactivated silver electrode can be dipped or immersed in an aqueous caustic catholyte solution and anodized, thus converting some of the silver at the surface of the electrode to colloidal silver oxide and roughening the surface at the same time. The polarity of the electrode is then reversed and the oxide electrolytically converted into particles of microcrystalline silver adhered to the surface of the electrode. The activation procedure involves increasing the potential from an initial value of zero volts to a final value of at least +0.3 volts and preferably about +0.7 volts. Reduction of the oxide deposit requires negative polarization of the cathode. The cathode potential is gradually reduced from the value of about +0.3 to about +0.7 volts attained during the oxidation step, to a value of about −0.5 volts or less. It is not necessary to add any silver to the catholyte or aqueous base in this method.
Water is the most preferred solvent for the electrolysis but, in some circumstances, it is possible to use an organic solvent either alone or as a co-solvent. The solvent or the co-solvent system should dissolve all or most of the starting material and the electrolyte, or at least enough to allow the reduction to proceed at a reasonable rate. In addition, the solvent or the co-solvent system should be inert to the electrolysis conditions, i.e., it does not detrimentally alter or react with the cathode or the catholyte materials to an intolerable extent. Other than water, preferred solvents/co-solvents are miscible with water and include lower molecular weight alcohols, ethers such as tetrahydrofuran, dioxane and polyglycol ethers, and lower amides such as dimethyl formamide or dimethyl acetamide.
Alkali metal hydroxides are preferred as the supporting electrolyte but many other substances such as quaternary ammonium or metallic hydroxides, chlorides, carbonates, etc. may be used. NaOH is the most preferred supporting electrolyte.
Bott Craig Joseph
Gullo Michael Frederick
Hull, Jr. John Wesley
Krumel Karl Leopold
Scortichini Carey Lee
Dow AgroSciences LLC
Mixan Craig E.
Wong Edna
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