Question

Explain the Structure of PCl5​

Answer 1

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It has a pyramidal shape as shown, in which phosphorus is sp3 hybridised.

2) Structure of PCl5:

It has a trigonal bipyramidal structure, in gaseous and liquid phases.

The three equatorial P–Cl bonds are equivalent, while the two axial bonds are longer than equatorial bonds.

Answer 2

In both gaseous and liquid states, $PCl_{5}$ possesses a trigonal bipyramidal structure.

Hybridization of $PCl_{5}$

• The elements in the third period include s and p orbitals as well as D orbitals.
• Comparable to 3s and 3p orbitals in energy are 3d orbitals.
• Similar to 4s and 4p orbitals, 3d orbitals have the same energy.
• This opens up the possibility of hybridizations including 3s, 3p, and 3d as well as 3d, 4s, and 4p.
• No hybridization between the 3p, 3d, and 4s orbitals is possible since the energies of the 3p and 4s orbitals are different.

How does $PCl_{5}$ come to be?

• Hybridization is possible with the first three orbitals, 1s, 3p, and 1d.
• As a consequence, it is possible to create a set of 5sp3d hybrid orbitals that are aligned to the 5 corners of a trigonal bipyramidal (VSEPR theory).
• It is interesting how different each bond angle is in trigonal bipyramidal geometry.
• In $PCl_{5}$, the chlorine atoms' p orbitals and the 5sp3d phosphorus orbitals match up.
• The p orbitals are solely occupied.
• Five P-Cl sigma bonds are created when they join.

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