Multiple Choice
What is the molecular geometry of SO_2?
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12. Molecular Shapes & Valence Bond Theory
Molecular Geometry
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What is the molecular geometry and polarity of xenon tetrafluoride (XeF_4)?
A
Tetrahedral; polar
B
Octahedral; nonpolar
C
Trigonal bipyramidal; polar
D
Square planar; nonpolar
Verified step by step guidance1
Identify the central atom and the number of valence electrons. Xenon (Xe) is the central atom with 8 valence electrons, and each fluorine (F) atom contributes 7 valence electrons, but since they form bonds, focus on Xe's electrons and bonding pairs.
Determine the total number of electron pairs around the central atom. XeF_4 has 4 bonding pairs (from the 4 fluorine atoms) and 2 lone pairs on xenon, making a total of 6 electron pairs.
Use the VSEPR (Valence Shell Electron Pair Repulsion) theory to predict the electron pair geometry. Six electron pairs arrange themselves in an octahedral geometry to minimize repulsion.
Consider the positions of the lone pairs. The two lone pairs occupy positions opposite each other (axial positions) in the octahedral arrangement, which leaves the four fluorine atoms in a square planar arrangement.
Analyze the molecular polarity. Because the molecule is symmetric with lone pairs opposite each other, the dipole moments cancel out, making XeF_4 nonpolar despite having polar Xe-F bonds.
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