The molecular geometry of ${\text{SF}}_4$ is:

To find the molecular geometry of sulfur tetrafluoride (${\text{SF}}_4$), we determine its hybridization and steric number using Valence Shell Electron Pair Repulsion (VSEPR) theory:
* The central sulfur ($\text{SS}$) atom has $6$ valence electrons.
* It forms $4$ single covalent bonds with four fluorine ($\text{F}$) atoms, utilizing $4$ electrons.
* The remaining $2$ electrons form $1$ lone pair.

$$\text{Steric Number}=\text{Number of bond pairs}+\text{Number of lone pairs}=4+1=5$$

A steric number of $5$ corresponds to ${\text{sp}}^3\text{d}$ hybridization, yielding a trigonal bipyramidal electron-pair geometry. To minimize lone pair-bond pair repulsions, the lone pair occupies an equatorial position. This structural arrangement leaves the four fluorine atoms in a distorted tetrahedral shape, commonly referred to as a see-saw geometry.