In Class 11 Chemistry (Chemical Bonding), calculating the hybridization of central atoms is a key concept. Let's determine the hybridization and molecular geometry of Phosphorus Pentachloride (PCl₅).
Central Atom: Phosphorus (P).
Hybridization: sp³d.
Lone Pairs: Zero.
Shape: Trigonal Bipyramidal.
Bond Angles: 120° (equatorial) and 90° (axial).
To find the hybridization, we analyze the central atom, Phosphorus (P).
Steric Number = (Number of bonded atoms) + (Number of lone pairs) Steric Number = 5 + 0 = 5.
A steric number of 5 corresponds to sp³d Hybridization. (One s-orbital, three p-orbitals, and one d-orbital mix together).
Because there are no lone pairs to distort the shape, PCl₅ adopts a perfect Trigonal Bipyramidal geometry.
Note: The axial bonds in PCl₅ are slightly longer and weaker than the equatorial bonds due to greater electron repulsion.
The hybridization of the central phosphorus atom in PCl5 is sp3d, because it forms 5 sigma bonds with 5 chlorine atoms and has zero lone pairs.
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