---
title: "A student determines the Lewis diagram and geometry for a molecule of xenon tetrafluoride, \\(\\text{XeF}_4\\). Which of the following correctly identifies the molecular geometry of \\(\\text{XeF}_4\\) and provides the valid justification?"
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date_modified: "2026-08-23T05:01:53+00:00"
---

# A student determines the Lewis diagram and geometry for a molecule of xenon tetrafluoride, \(\text{XeF}_4\). Which of the following correctly identifies the molecular geometry of \(\text{XeF}_4\) and provides the valid justification?

A student determines the Lewis diagram and geometry for a molecule of xenon tetrafluoride, \(\text{XeF}_4\). Which of the following correctly identifies the molecular geometry of \(\text{XeF}_4\) and provides the valid justification?

- **A.** Tetrahedral, because the central \(\text{Xe}\) atom is bonded to four fluorine atoms arranged symmetrically to minimize electron repulsion.
- **B.** See-saw, because the central \(\text{Xe}\) atom has four bonding pairs and one lone pair that distorts the bond angles.
- **C.** Octahedral, because the central \(\text{Xe}\) atom has six total electron domains directed toward the vertices of an octahedron.
- **D.** Square planar, because the central \(\text{Xe}\) atom has six electron domains with two lone pairs positioned \(180^\circ\) apart to minimize electron repulsion.

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