Question

All the $P - Cl$ bonds in $PC{l_5}$ are not equivalent. Why? Explain.

Answer 1

In gaseous and liquid states, phosphorus pentachloride hybridization is $s{p^3}d$ , with a trigonal bipyramidal geometry. It has three equatorial $PCl$ bonds and two axial $PCl$ bonds. Phosphorus pentachloride is a crystalline greenish-yellow substance that is dissolved by water into hydrochloric acid and phosphoric acid when heat energy is released.

Complete answer:
One $P - Cl$ bond is above the equatorial plane, while the other is below the plane, forming an angle with the plane. The plane's angle is given as ${90^ \circ }$ .
$3P - Cl$ bonds that lay in one plane and form an angle with each other are known as equatorial bonds. The angle formed between them is ${120^ \circ }$ .
$PC{l_5}$ has a trigonal bipyramidal structure in the gaseous and liquid states. The two axial $P - Cl$ bonds are longer and less stable than the three equatorial $P - Cl$ bonds in this structure. This is due to the axial bonds greater bond pair - bond pair repulsion.
As a result, none of the bonds in $PC{l_5}$ are equivalent.

Additional Information:
-It is used to chlorinate water.
-In the pharmaceutical industry, it is used to make penicillin and cephalosporin.
-It is used to make acid chlorides.
-It is used as a catalyst in the production of acetyl cellulose, as well as condensation and cyclization reactions.

Note:
The chemical phosphorus pentachloride is a reactive substance. Phosphorus Pentachloride can cause weakness, nausea, headaches, dizziness, and vomiting when inhaled directly. It has the potential to harm the liver and kidneys.