P in ${PCl}_{5}$ has $s p^{3} d -$ hybridisation which of the following statements are correct about ${PCl}_{5}$ structure?

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All $P - Cl$ bond lengths are identical.

Two $P - Cl$ bonds are axial and longer than three $P - Cl$ equatorial bonds.

${PCl}_{5}$ decomposes into ${PCl}_{3}$ and ${Cl}_{2}$ on heating

${PCl}_{5}$ has trigonal bipyramidal geometry with non-polar nature

answer is B, C, D.

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Detailed Solution

In this structure, the three equatorial $ $P - Cl$ $ bonds are longer and more stable than the two axial $ $P - Cl$ $ bonds. This is brought on by the stronger bond pair–bond pair repulsion in the axial bonds.
The nonpolar compound phosphorous pentachloride ( ${PCl}_{5}$ ) is phosphorus. Its geometry is trigonal, symmetric, and bipyramidal, with bond angles of 90° and 120°.
Because none of the bonds in ${PCl}_{5}$ are identical, heating ${PCl}_{5}$ produces ${PCl}_{3}$ and ${Cl}_{2}$ .