Ncert Exercises & Solutions

Describe hybridisation in the case of PCl₅ and SF₆. The axial bonds are longer as compared to equatorial bonds in PCl₅ wherea in SF₆ both axial bonds and equatorial bonds have the same bond length. Explain.

Formation of PCl₅

In PCl₅, phosphorus is sp³d hybridised to produce a set of five sp³d hybrid orbitals which are directed towards the five corners of a trigonal bipyramidal. These five sp³d hydrid orbitals overlap with singly occupied p-orbitals to Cl-atoms to form five P-Cl sigma bonds.

Three P-Cl bonds lie in one plane make an angle of

120 °

with each other. These bonds are called equatorial bonds. The remaining two P-Cl bonds one lying above and other lying below the plane make and angle of

90 °

with the equatorial plane.

These bonds are called axial bonds. Axial bonds are slightly longer than equatorial bonds because axial bond pairs suffer more repulsive interaction from the equatorial bond pairs.

Formation of SF₆

In SF₆, sulphur is sp³d² hybridised to produce a set of six sp³d² hybrid orbitals which are directed towards the six corners of a regular octahedron. These six sp³d² hybrid orbitals overlap with simgly occupied orbitals of fluorine atoms to form six S-F sigma bonds.

Thus, SF₆ molecule has a regular octahedral geometry and all S-F bonds have same bond length.

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