XeF₂ contains three lone pairs and two Xe–F bonds around the central xenon atom
CHEMISTRY · Single correct · A Level · Chemistry · Bonding · Bonding
Problem
XeF₂ contains three lone pairs and two Xe–F bonds around the central xenon atom. Which statement most accurately describes the overall polarity of XeF₂?
(a) The molecule is polar because fluorine is much more electronegative than xenon, so the two Xe–F bonds create a net dipole along the bond axis.
(b) The molecule is non-polar because it adopts a linear geometry that causes the two Xe–F bond dipoles to cancel.
(c) The molecule is polar because its molecular shape is trigonal bipyramidal, so the bond dipoles do not cancel.
(d) The molecule is polar because the three equatorial lone pairs create a net dipole perpendicular to the Xe–F bond axis.