F is highly electronegative it attracts electrons of N towards itself and hence the elctrons aren't easily available on N of NF3 molecule making it a weaker ligand or donor. Thats the reasonis why NF3 does not ionises to give Flouride ions is aqueous solution .instead
NF3+H20-->HNO3+ NO+HF

NF3 and Fluoride Ion in Aqueous Medium

Introduction:
NF3, also known as nitrogen trifluoride, is a covalent compound composed of a nitrogen atom bonded to three fluorine atoms. In an aqueous medium, NF3 does not dissociate to form fluoride ions (F-), as it is a weak acid and does not completely ionize. However, a small amount of NF3 can react with water to produce some fluoride ions.

Reaction:
The reaction of NF3 with water can be represented as follows:

NF3 + H2O → NH3 + 3HF

In this reaction, nitrogen trifluoride reacts with water to form ammonia (NH3) and hydrofluoric acid (HF). The hydrofluoric acid then dissociates into fluoride ions (F-) and hydrogen ions (H+).

Explanation:
- When NF3 is dissolved in water, a small fraction of it reacts with water molecules.
- The reaction between NF3 and water results in the formation of ammonia (NH3) and hydrofluoric acid (HF).
- The ammonia molecule is a weak base and can accept a proton (H+) from the water molecule, resulting in the formation of ammonium ions (NH4+).
- The hydrofluoric acid produced in the reaction is a weak acid and partially dissociates in water to produce fluoride ions (F-) and hydrogen ions (H+).
- The fluoride ions (F-) formed in the solution can be considered as a source of fluoride ions, although the concentration might be quite low due to the weak acid nature of NF3.
- The overall reaction shows that NF3 does not dissociate completely to produce fluoride ions in an aqueous medium.

Conclusion:
NF3 does not give a significant amount of fluoride ions in an aqueous medium. While a small fraction of NF3 can react with water to form fluoride ions, the concentration of fluoride ions produced is relatively low due to the weak acid nature of NF3. It is important to note that fluoride ions are commonly obtained from other sources, such as soluble fluorides, which readily dissociate to produce fluoride ions in water.