Why is this PH3 considered to be an unhybridized molecule? [duplicate]








**This question already has answers here**:
 
 




[Hybridization in PH3](/questions/14791/hybridization-in-ph3)

 (2 answers)
 

Closed 5 years ago.



Also, don't hybrid orbitals appear in all molecules? 


[![enter image description here](https://i.stack.imgur.com/Kg7X0.jpg)](https://i.stack.imgur.com/Kg7X0.jpg)


The answer by "ron" says "the molecule can be viewed as being unhybridized":
[How does lone pair of a central atom affect the dipole moment?](https://chemistry.stackexchange.com/questions/13907/how-does-lone-pair-of-a-central-atom-affect-the-dipole-moment)




I'll try to explain this by comparing this with the case of NH3. 
N is a better electron withdrawing group than P. So in the case of NH3 the electron cloud is more closer to N. And therefore the repulsion in the bonds causes the 3 H atoms to be farther away from each other resulting in a bond angle of about 109°. But in the case of PH3 the electron cloud is farther away from the central atom(P) than in the case of NH3. So the bond pair - bond pair repulsion is comparatively lesser, causing the 3 H atoms to move closer together to an angle of almost 90°, resembling the px, py, and pz orbitals, as a consequence it's lone pairs are present in almost pure s - orbital. So it is is said that PH3 can be viewed as unhybridized.


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It is due to greater difference in energy of atomic orbitals of phosphorous such as 3s and 3p.


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