CHEMISTRY · Multi-part · CBSE · Chemistry · Chemical Bonding and Molecular Structure · Chemical Bonding and Molecular Structure
Problem
Xenon forms the oxyfluoride XeOF4, which is thermally stable under dry conditions.
Analyze the bonding and geometry of XeOF4 as described below.
(a) Determine the total number of valence electrons that must be represented in a complete Lewis diagram for XeOF4.
(b) Draw two plausible Lewis diagrams for XeOF4—one in which xenon forms a single bond to oxygen and one in which xenon forms a double bond to oxygen. Show all lone pairs explicitly in each diagram.
(c) For each diagram you drew in part (b), compute the formal charge on every atom.
(d) Using the formal-charge data and the relative electronegativities of O, Xe, and F, decide which diagram is the better representation of the actual molecule. Justify your choice thoroughly.
(e) Based on the preferred Lewis diagram, predict the molecular geometry around xenon and discuss whether the molecule is expected to be polar or nonpolar. Support your answer with reasoning tied to the spatial arrangement of electron pairs.