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Chemistry
Chemical Bonding and Molecular Structure
describe the hybridisation in case of pcl5 why ar...

Question:
Describe the hybridisation in case of PCl₅. Why are the axial bonds longer as compared to equatorial bonds?

Answer:

Atomic number of Phosphorous is 15.

The Ground state configuration is

& the excited state configuration is

The 5 electrons present in valence shell form bond pairs with the electrons of five chlorine atoms. Phosphorus atom is sp3d hybridized in the excited state.

PCl₅

The geometry of PCl₅ is trigonal bipyramidal .The P atom lies in the centre of an equatorial triangle & three P-Cl bonds (equatorial bonds) are directed towards its three corners with 120° bond angle. The remaining two P-Cl bonds (axial bonds) lie above & below the plane of the triangle at bond angle 90° .

The axial bonds are longer than equatorial bonds because the axial Cl atoms suffer from more repulsion then the equatorial Cl atoms,as a result the axial Cl atoms tries to reside far away from the equatorial Cl atoms, & hence axial bond are longer than equatorial bonds.

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Question:
Describe the hybridisation in case of PCl₅. Why are the axial bonds longer as compared to equatorial bonds?

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Question: Describe the hybridisation in case of PCl5. Why are the axial bonds longer as compared to equatorial bonds?

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Question:
Describe the hybridisation in case of PCl₅. Why are the axial bonds longer as compared to equatorial bonds?