Phosphorus trichloride (PCl3) is a chemical compound consisting of one phosphorus (P) atom bonded to three chlorine (Cl) atoms. It is a key representative of phosphorus compounds and finds applications in various chemical processes.
The molecule's structure and bonding can be elucidated by understanding the concept of hybridization in the phosphorus atom. Let’s learn what is the hybridization of PCl3 in detail.
To understand the hybridization scheme for PCl3 (phosphorus trichloride), we need to look at its molecular geometry and the number of sigma bonds and lone pairs around the phosphorus atom. See number of electrons in ground state and excited state in phosphorus in given diagram.
In PCl₃ :
Now, let's count the number of sigma bonds and lone pairs around phosphorus:
As per the valence shell electron pair repulsion theory, the geometry around phosphorus is tetrahedral (three sigma bonds and one lone pair). The hybridization is determined by the number of sigma bonds and lone pairs.
For PCl₃ :
If there are 3 sigma bonds and 1 lone pair, the hybridization is sp³.
Therefore, the phosphorus in PCl₃ undergoes sp³ hybridization. In sp³ hybridization, one s orbital and three p orbitals combine to form four equivalent sp³ hybrid orbitals. These orbitals are then used to overlap with the orbitals of the chlorine atoms, resulting in the formation of three sigma bonds and one lone pair, giving PCl₃ a trigonal pyramidal molecular geometry.
(Session 2025 - 26)