Interhalogen compounds are formed between two different halogens. They have a general formula of XYn where X and Y are different halogens and n is the number of halogen atoms.

Stability of interhalogen compounds:

The stability of interhalogen compounds depends on the size of the halogen atoms and their electronegativity. The larger the size of the halogen atom, the less stable the compound will be. The higher the electronegativity of the halogen atom, the more stable the compound will be.

Order of stability:

The stability of interhalogen compounds follows the order IF3 > BrF3 > CIF3. This can be explained as follows:

1. IF3 (Iodine trifluoride):

Iodine is the largest halogen atom among the three. It has a low electronegativity and a larger size, which makes it less stable. However, the compound IF3 has a high stability due to the presence of a strong intermolecular force of attraction between the iodine and fluorine atoms.

2. BrF3 (Bromine trifluoride):

Bromine is smaller than iodine and has a higher electronegativity. The compound BrF3 has a lower stability than IF3 due to the weaker intermolecular force of attraction between the bromine and fluorine atoms.

3. CIF3 (Chlorine trifluoride):

Chlorine is the smallest halogen atom among the three and has the highest electronegativity. The compound CIF3 has the lowest stability due to the strong repulsion between the small chlorine atoms.

Therefore, the stability of interhalogen compounds follows the order IF3 > BrF3 > CIF3.