Explain Why all P-Cl bonds in PCl5 are not equal in length

Due to inter electronic repulsion between cl-cl and differ in angle b|wthem,identify the pcl5 has two axial lines and 3 equatorial line.

The structure of Pcl5 is s p3d. Its three epuitorial bonds are connected with a angle of 120 degree.but one equitorial and one axial are connected with a angle of 90 degree. For this type of structure every equitorial bonds are repulshed with two bond therefore every axial bonds are repulshed with there bond.so the length of axial bonds are higher than equitorial bonds.

In PCl5 , P is undergoing sp3d hybridization geometry of the molecule is trigonal bi pyramidal with bond angle 90° and 120° . Hence due to inter electronic repulsion the bond length increases and P-Cl bond is not stable.

Dear Student,
Please find below the solution to your problem.

PCl5 has the sp3d hybridization geomtery in which two Cl atoms are at vertical position top and bottom that is axially attached.
Rest three atoms are located at equitorial positions which are same in length.
Hence axial Cl atoms bond lengths are longer in length.

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