I have a situation in which I want to hydrolyze a phosphonic acid halide under basic conditions. In my specific case, the halide is a fluorine substituent. Other halides like chlorine and bromine are known to hydrolyze quite quickly under aqueous conditions. Until now fluorine abstraction was not possible, even under strongly basic conditions. An additional substituent on the phosphorous is an oxido moiety which carries a negative charge. I am wondering about two things: Is there the possibility to increase the leaving capacity of fluorine by electron-donating groups in close proximity (bond to the same atom)? When the oxido moiety is replaced by an alkyl group R- or Alkoxygroup RO-, the molecule loses a negative charge, which might stabilize the fluorine and inhibits the hydrolyzation. What are the underlying principles that might explain the problems of hydrolyzation? Or are there other strategies to make hydrolyzation an energetically more favored process?

I have a situation in which I want to hydrolyze a phosphonic acid halide under basic conditions. In my specific case, the halide is a fluorine substituent. Other halides like chlorine and bromine are known to hydrolyze quite quickly under aqueous conditions. Until now fluorine abstraction was not possible, even under strongly basic conditions. An additional substituent on the phosphorous is an oxido moiety which carries a negative charge. I am wondering about two things: Is there the possibility to increase the leaving capacity of fluorine by electron-donating groups in close proximity (bond to the same atom)? When the oxido moiety is replaced by an alkyl group R- or Alkoxygroup RO-, the molecule loses a negative charge, which might stabilize the fluorine and inhibits the hydrolyzation. What are the underlying principles that might explain the problems of hydrolyzation when an oxido moiety is present? Are there other strategies to make hydrolyzation an energetically more favored process?

I have a situation in which I want to hydrolyze a phosphonic acid halide under basic conditions. In my specific case the halide is a fluorine substituent. Other halides like chlorine and bromine are known to hydrolyze quite quickly under aquoues conditions. Until now fluorine abstraction was not possible, even under strongly basic conditions. An additional substituent on the phosphorous is an oxido moiety which carries a negative charge. I am wondering about two things: Is there the possibility to increase the leaving capacity of fluorine by electron-donating groups? When the oxido moiety is replaced by an alkyl group R- or Alkoxygroup RO-, the molecule looses a negative charge, which might stabilize the fluorine and inhibits the hydrolysation. What are the underlying principles that might explain the problems of hydrolyisation? Or are there other strategies to make the hydrolysation an energeticlay more favored process?

I have a situation in which I want to hydrolyze a phosphonic acid halide under basic conditions. In my specific case, the halide is a fluorine substituent. Other halides like chlorine and bromine are known to hydrolyze quite quickly under aqueous conditions. Until now fluorine abstraction was not possible, even under strongly basic conditions. An additional substituent on the phosphorous is an oxido moiety which carries a negative charge. I am wondering about two things: Is there the possibility to increase the leaving capacity of fluorine by electron-donating groups in close proximity (bond to the same atom)? When the oxido moiety is replaced by an alkyl group R- or Alkoxygroup RO-, the molecule loses a negative charge, which might stabilize the fluorine and inhibits the hydrolyzation. What are the underlying principles that might explain the problems of hydrolyzation? Or are there other strategies to make hydrolyzation an energetically more favored process?