Explain how the electron pair repulsion theory can be used to deduce the shape of, and the bond angle in, PF3

Phosphorous has five electrons in its outermost shell of electrons. Fluorine provides three electrons to the phosphorous allowing the formation of a stable central phosphorous atom which now has 8 electrons and 3 fluorine atoms which now also share 8 electrons in its outershell. However as there are only 3 bonding pairs there must be a lone pair of electrons in this molecule. As bond pairs repel each other you would expect a tetrahedral shape to the molecule with a bond angle of 109 however due to the presence of the lone pair, there is more repulsion which distorts the shape slightly and it becomes trigonal pyramidal with a bond angle of 107.

PB
Answered by Prashan B. Chemistry tutor

9896 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

Why does phenol readily undergo electrophilic substitution but benzene does not without the aid of a catalyst?


What makes phenol different from alcohols?


What is an enthalpy change?


25cm^3 of 0.1M NaOH is reacted with 0.01M HCl until the equivalence point is reached. What volume of HCl was required to be added?


We're here to help

contact us iconContact ustelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

MyTutor is part of the IXL family of brands:

© 2025 by IXL Learning