Sulfur tetrafluoride 1SF42 reacts slowly with O2 to form sulfur
tetrafluoride monoxide 1OSF42 according to the following
unbalanced reaction:
SF41g2 + O21g2¡OSF41g2
The O atom and the four F atoms in OSF4 are bonded to a
central S atom.
(e) For each of the molecules you drew in part (d), state how many
fluorines are equatorial and how many are axial.

Verified step by step guidance

1. Identify the molecular geometry of SF_4. SF_4 has a seesaw shape due to the presence of one lone pair on the sulfur atom.
2. In a seesaw geometry, there are two types of positions for the fluorine atoms: equatorial and axial.
3. Determine the positions of the fluorine atoms in SF_4. In a seesaw shape, there are typically two equatorial positions and two axial positions.
4. Now, consider the molecular geometry of OSF_4. The presence of an additional oxygen atom bonded to sulfur may alter the geometry slightly, but the basic seesaw shape remains.
5. For OSF_4, identify the positions of the fluorine atoms. Typically, the equatorial positions are occupied first, so expect two equatorial and two axial fluorines.

Key Concepts

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is determined by the number of bonding pairs and lone pairs of electrons around the central atom, which influences the shape of the molecule. For sulfur tetrafluoride (SF4), the geometry is based on the VSEPR (Valence Shell Electron Pair Repulsion) theory, which predicts that the molecule adopts a seesaw shape due to the presence of one lone pair.

Equatorial and Axial Positions

In molecules with a trigonal bipyramidal geometry, such as SF4, the positions of atoms can be classified as equatorial or axial. Equatorial positions are located in the plane of the molecule and are 120 degrees apart, while axial positions are aligned above and below the equatorial plane at 90 degrees to the equatorial atoms. Understanding these positions is crucial for predicting molecular behavior and reactivity.

Bonding and Hybridization

Bonding in molecules involves the overlap of atomic orbitals to form covalent bonds. In SF4, sulfur undergoes sp3d hybridization, which allows it to form four equivalent bonds with fluorine atoms and accommodate one lone pair. This hybridization is essential for understanding the molecule's geometry and the distribution of electron density around the central sulfur atom.