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Which of the molecule have strongest P=O bond present the given molecules are POF3, POCl3, POBr3 and PO(CH3)3 ?

All the given molecules have same hybridization (sp3) and same central atom (P) the we can apply Bent's rule of hybridization. And according to Bent’s rule more electronegative atoms attach in those hybrid orbital’s which have less s-character or more electronegative atoms decreases s-character and increases p-character.

In case of POF3  fluorine is more electronegative hence s-character  is increase more and more in P=O bond  as compare to other given molecules so P=O bond is shortest in POF3  than others and also increase with decreasing electronegativity.  Hence P=O bond length order is x1 < x2 < x3 < x4  and Bond strength order is reverse of bond length.

Related Questions:

What is Bent’s rule of hybridization?

Which of the following compound have longest (S=O)bond length , O=SF2, O=SCl2, O=SBr2.

Why Bond length of O-O is greater in H2O2 than O2F2?

How to arrange increasing (C-H) bond length in increasing order and H-C-F bond angle in the given compounds, CH4, CH3F, CH2F2 and CHF3 ?

Dipole moment of PCl3F2 molecule is zero while dipole moment of PCl2F3 molecule is non zero why?

Dipole moment of P(CH3)2(CF3)2 molecule is zero while dipole moment of P(CH3)2(CF)3 molecule is non zero why?

How to compare equatorial bond angle (F-S-F) and S-F bond length of SOF4 and SF4 molecules ?

How to compare P=O bond length of POF3, POCl3, POBr3 and PO(CH3)3 molecules?


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