Xenon forms a stable molecular compound XeF₄.
(a) Draw a complete Lewis electron-dot diagram for XeF₄.
(b) Determine the total number of regions of electron density around the xenon atom, indicating how many are bonding regions and how many are lone pairs.
(c) Identify the three-dimensional molecular shape (name only) about the xenon atom.
(d) Predict the approximate F–Xe–F bond angle between adjacent fluorine atoms (not trans to each other) and explain how lone pairs influence this value.
(e) Discuss whether XeF₄ is expected to possess a net molecular dipole moment and justify your answer using symmetry considerations.
(a) Lewis electron-dot diagram
(b) Regions of electron density
(c) Molecular shape
(d) Bond-angle prediction with explanation
(e) Dipole moment discussion