Sulfur tetrafluoride adopts a see-saw geometry with two axial F atoms with a F–S–F angle of about 18 — Bonding Chemistry Question
Question
Sulfur tetrafluoride adopts a see-saw geometry with two axial F atoms with a F–S–F angle of about 180º and two equatorial F atoms at about 90º from the axial fluorines. Which statement most accurately describes the axial and equatorial S–F bonds?
A.✓ Correct
The axial S–F bonds are longer because the two fluorines must share bonding to the same orbital on sulfur.
B.
The axial S–F bonds are longer because they experience greater repulsion from the other fluorine atoms in the molecule.
C.
The equatorial S–F bonds are longer because the equatorial F–S–F bond angle is the smallest in the molecule.
D.
The equatorial S–F bonds are longer because they experience greater repulsion from the lone pair on sulfur.
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