According to VSEPR theory, which molecule adopts the molecular geometry pictured below?

14A

Question

According to VSEPR theory, which molecule adopts the molecular geometry pictured below?

14A

BlackTom AI · Accepted Answer

To determine which molecule adopts the pictured geometry, we need to compare the VSEPR shapes produced by different electron arrangements around the central atom.
Option SF4: This molecule has one lone pair on sulfur in addition to the four S–F bonds. The presence of a lone pair distorts the geometry from a perfect tetrahedron to a see-saw shape, not the symmetric tetrahedral arrangement shown.
Option All 3 molecules lead to the molecular geometry shown: This would require that CF4, SF4, and XeF4 all exhibit the same arrangement. However, XeF4 has two lone pairs on xenon, which gives a square planar geometry, not tetrahedral. Therefore this option is incorrect.
Option XeF4: With two lone pairs on xenon, the electron-pair geometry is octahedral-like for the lone pairs, and the molecular shape is square planar, not the tetrahedral geometry depicted. Thus this choice does not match the image.
Option CF4: Carbon in CF4 has four bonding pairs to fluorine and zero lone pairs. According to VSEPR theory, four electron groups with no lone pairs adopt a tetrahedral electron-pair geometry and a tetrahedral molecular geometry, which matches the depicted shape precisely.
In summary, the only option that yields a symmetric tetrahedral arrangement with four identical bonds and no lone pairs is CF4, while the others introduce lone pairs that alter the geometry.

CHEM 1210 AU2025 (15738) Exam 4- Requires Respondus LockDown Browser

According to VSEPR theory, which molecule adopts the molecular geometry pictured below? 14A

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