Explain the hybridization involved in PCl5 molecule.

Question

Accepted Answer

>

> [!TLDR]
> $PCl_5$'s central P atom undergoes $sp^3d$ hybridisation, producing 5 equivalent hybrid orbitals arranged in a trigonal bipyramidal geometry, though the resulting axial and equatorial bonds are not equal in length.
>
> **Ground state configuration of P** ($Z=15$): $[Ne]\,3s^2 3p^3$, with 5 valence electrons — 2 in $3s$, 3 in $3p$.
>
> To form 5 bonds to chlorine, phosphorus first promotes one $3s$ electron into an empty $3d$ orbital, giving the excited-state configuration $3s^1 3p^3 3d^1$ — five singly-occupied orbitals ($1\ s$, $3\ p$, $1\ d$).
>
> These five orbitals ($s + p_x+p_y+p_z + d$) mix to form **five equivalent $sp^3d$ hybrid orbitals**, each overlapping with a $3p$ orbital of a chlorine atom to form 5 P–Cl sigma bonds.
>
> **Geometry:** the five $sp^3d$ orbitals point towards the corners of a **trigonal bipyramid**:
> - 3 orbitals lie in a horizontal (equatorial) plane, $120°$ apart from each other.
> - 2 orbitals point perpendicular to this plane, one above and one below (axial), each $90°$ to the equatorial plane and $180°$ to each other.
> …

Hybridization	Orbitals Mixed	Number of Hybrids	Geometry	Bond Angle	Example
$sp$	one $s$ + one $p$	2	Linear	$180^\circ$	$\text{BeCl}_2$
$sp^2$	one $s$ + two $p$	3	Trigonal planar	$120^\circ$	$\text{BF}_3$
$sp^3$	one $s$ + three $p$	4	Tetrahedral	$109.5^\circ$	$\text{CH}_4$

Q.Explain the hybridization involved in PCl5 molecule.

Concept understanding — Orbital Hybridization Theory

Orbital Hybridization Theory – From Intuition to Precision

The Problem That Started It All

The Core Intuition

The Precise Statement

The Three Common Hybridizations

How It Works: The Methane Example

Q.Explain the hybridization involved in PCl5 molecule.

🎓Unlock everything free for 14 days

Unlock everything free for 14 days