Abstract:
Preparation of titanium tetraperchlorate, vanadium perchlorate, and chromylerchlorate by the reactions of chlorine perchlorate with the respective anhydrous metal chlorides at a temperature from about -45° C to about 20° C. These perchlorates are useful in compounding gas generating compositions.

Description:
BACKGROUND OF THE INVENTION 
     1. Field of the Invention 
     The invention pertains to the preparation of inorganic oxidizing salts and in particular to the preparation of anhydrous metal perchlorates. 
     2. Prior Art 
     Syntheses of anhydrous metal perchlorates have been restricted mainly to metals from Groups I and II. A few preparations have been reported for transition metal perchlorates as well as NO 2   +   and NH 4   +   complex perchlorates. 
     One method is known for the preparation of anhydrous titanium tetraperchlorate. This method proceeds by the reaction of anhydrous perchloric acid with anhydrous titanium tetrachloride. However the product is not pure as is evidenced by the data presented pertaining to the melting point, analysis, stability, yield, and polycrystalline form. A major disadvantage of the impurities in the product is the necessity of refrigeration. Other disadvantages of this synthesis are the scarcity, expense, and danger of anhydrous perchloric acid. 
     The known method for the preparation of chromyl perchlorate is through the reaction of chromyl chloride and dichlorine hexoxide. Although the reaction product is pure, the synthesis has the disadvantages which result from the scarcity, expense, and danger of anhydrous dichlorine hexoxide. 
     SUMMARY OF THE INVENTION 
     It is, therefore, an object of this invention to form anhydrous metal perchlorates safely, quickly, and inexpensively. 
     Another object of this invention is to form anhydrous metal perchlorates in a high degree of purity. 
     These and other objects are achieved by a method which proceeds by the following reactions: 
     
         CrO.sub.2 Cl.sub.2 + 2Cl.sub.2 O.sub.4 -- 2Cl.sub.2 + CrO.sub.2 (ClO.sub.4).sub.2 
    
     
         tiCl.sub.4 + 4Cl.sub.2 O.sub.4 -- 4Cl.sub.2 + Ti(ClO.sub.4).sub.4 
    
     
         vocl.sub.3 + 3Cl.sub.2 O.sub.4 -- VO(ClO.sub.4).sub.3 + 3Cl.sub.2 
    
     and which occur at a temperature from -45° C to 20° C. 
     DETAILED DESCRIPTION OF THE INVENTION 
     Due to the strong oxidizing strength of the perchlorate group the method of the invention must proceed in vessels constructed from stainless steel, platinum, teflon, monel or similar non-oxidizable materials or coated therewith. The reaction is carried out at ambient pressure and at a temperature from about -45° C to about 20° C but preferably from -25° C to 0° C. Stirring is optional because the bubbling of the by-product chlorine through the reaction solution provides sufficient agitation. Completion of the reaction is determined preferably by monitoring the chlorine gas by-product. Generally the reaction is complete within 4 to 6 hours and the perchlorate product may then be collected. 
     Preferably, chlorine perchlorate is prepared by the method disclosed in U.S. Pat. No. 3,694,172 by Schack et al. 
     The reactants are added in stoichiometric amounts. Thus for the synthesis of chromyl perchlorate the reactants are added in a CrO 2  Cl 2  -to-Cl 2  O 4  mole ratio of 1:2. For the synthesis of vanadium perchlorate, the reactants are added in a VOCl 3  -to-Cl 2  O 4  mole ratio of 1:3. It is preferred that an extra 5 to 10 mole percent of Cl 2  O 4  is added in order to decrease the reaction time. Since water produces impurities in the perchlorate product, the reactants and the system should be anhydrous. 
     The reactants may be added in any order or in any rate. However the reactions are exothermic; so, measures must be taken to ensure that reaction temperature does not exceed about 20° C. According to a preferred embodiment of this invention the reactants are added to the reaction vessel in the solid state, thereby minimizing the vapors of the reactants. 
     This embodiment is utilized in Example I given hereinafter. It is understood that the examples are given by way of illustration and are not intended to limit the disclosure or the claims to follow in any way. 
    
    
     EXAMPLE I 
     Titanium tetrachloride (1.22 mmol) and ClOClO 3  (6.01 mmol) were combined at -196° in a 75 ml stainless steel cylinder and then gradually warmed to -25°. After several days, recooling to -196° showed no noncondensable gases were present. The contents of the reactor were separated by fractional condensation in a series of U-traps cooled to -78°, - 112°, and -196°. Nothing was trapped at -78° while the -112° fraction consisted solely of unreacted Cl 2  O 4  (1.17 mmol), and the -196° fraction was Cl 2  (4.88 mmol). The pale yellow solid residue left in the reactor weighed 0.525 g. The weight calculated for 1.22 mmol of Ti(ClO 4 ) 4  was 0.544 g and therefore the yield of Ti(ClO 4 ) was 97 percent. Vacuum sublimation of the Ti(ClO 4 ) 4  was carried out in a Pyrex apparatus at 50°-60° using a -78° cold finger. The sublimed material was nearly colorless and had a m.p. with dec. of 101°-2°. Almost no residue remained unsublimed. Anal. Calcd. for Ti(ClO 4 ) 4  : Ti, 10.75; ClO 4 , 89.25. Found: Ti, 10.8; ClO 4 , 87.9. A sample of Ti(ClO 4 ) 4  (0.242 mmol) was heated in a stainless steel cylinder for 4 hours at 115° followed by 1.5 hr. at 190°. This produced O 2  (1.705 mmol), Cl 2  (0.481 mmol), and a white solid residue of TiO 2  (0.241 mmol). All temperatures are in degrees Centigrade. 
     EXAMPLE II 
     Chromyl chloride (1.41 mmol) and ClOClO 3  (3.16 mmol) were reacted at -45° for several days in a stainless steel cylinder. After separation and identification, the volatile products found were CrO 2  F 2  (0.18 mmol), Cl 2  (2.59 mmol), and Cl 2  O 4  (0.66 mmol). The CrO 2  (ClO 4 ) 2  (1.23 mmol) remained in the cylinder. The CrO 2  F 2  probably arose through reaction of CrO 2  Cl 2  with the ClF 3  passivated metal surfaces in the reactor and/or vacuum line during transfers. Anal., Calcd. for CrO 2  (ClO 4 ) 2  : ClO 4 , 70.3. Found: ClO 4 , 69.6. A sample of CrO 2  (ClO 4 ) 2  (0.65 mmol) was pyrolyzed for 15 hrs at 110° producing Cl 2  (0.66 mmol), O 2  (2.21 mmol) and CrO 3  (0.65 mmol), m.p. 195°-7°, lit. 196°. All temperatures are in degrees Centigrade. 
     As can be seen from the examples, the method of this invention produces a highly pure anhydrous metal perchlorate without the use of the scarce and dangerous anhydrous perchloric acid or dichlorine hexoxide. The anhydrous titanium perchlorate has been stored at room temperature for over three months without degradation. 
     Obviously many modifications and variations of the present invention are possible in light of the above teachings. It is therefore to be understood that within the scope of the appended claims the invention may be practiced otherwise than as specifically described.