Xenon forms several oxyfluorides that exhibit expanded valence shells. One such molecule is XeO3F2, whose atoms are bonded to the xenon center in the order O, O, O, F, F. Assume no two peripheral atoms are bonded to each other.
(1) Draw a complete Lewis diagram for XeO3F2, showing all lone pairs on every atom.
(2) Compute the formal charge on xenon and on each oxygen and fluorine atom in your diagram.
(3) Verify that the overall formal-charge tally is consistent with the neutrality of the molecule.
(4) Several alternative Lewis structures can be constructed by assigning double bonds between xenon and one or more oxygen atoms. Using the formal-charge criterion, determine which arrangement of single and double bonds yields the most favorable structure. Provide quantitative justification.