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.

Answered by Prashan B. Chemistry tutor

8970 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

What is meant by the term salt? And how would you confirm if the salt had chloride ions in?


Explain what is meant by Enthalpy


What is the rate-determining step?


What are the differences between covalent and ionic bonding?


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences