What shape does XeF4 take?

Molecular shape depends on the number of electron pairs around the central atom. Electrons are negatively charged and so each of the electron pairs will repel each other. Lone pairs tend to repel more than bonding pairs and so try to sit position themselves as far away as possible from each other.Start by working out how many electron pairs there are: Xe has 8 outer electrons F has 1 bonding electron, so the four F contribute 4 electrons Total electrons = 12 Electron pairs = 6 Four of the electron pairs are used in bonding between Xe and F, leaving two sets of lone pairs. The lone pairs will sit opposite each other, leaving the Fs to form a square planar shape.

LS
Answered by Laura S. Chemistry tutor

7406 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

Would you expect a calcium ion to be bigger, smaller or the same size as a calcium atom? Give TWO reasons to explain your answer.


What 2 reagents are required to form NO2+ (state conditions)? Write an equation for this reaction.


How can you convert benzene to N-phenylethanamide in 3 steps?


Calculate the empirical and molecular formula of unknown compound A which gave an m/z of 181 in the mass spectrum for the molecular ion peak. Elemental analysis by combustion shows the compound is C 53%, O 35.4%, H 3.9% and N 7.7%.


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