In $\text{ClF}_3$, the central chlorine atom is $sp^3d$ hybridised and possesses 3 bond pairs and 2 lone pairs of electrons. According to the VSEPR theory, it adopts a T-shaped geometry derived from a trigonal bipyramidal structure. The two lone pairs occupy the equatorial positions to minimise repulsions. As a result, the two axial $\text{Cl-F}$ bonds suffer greater repulsion from the lone pairs and are longer than the single equatorial $\text{Cl-F}$ bond. Therefore, all bonds in $\text{ClF}_3$ are not equal. Conversely, in $\text{BF}_3$ (trigonal planar), $\text{AlF}_3$, and $\text{NF}_3$ (trigonal pyramidal), all bonds are equivalent in length.