Final answer:
The Lewis structure of SF4 (sulfur tetrafluoride) consists of a central sulfur atom bonded to four fluorine atoms with a lone pair of electrons. It exhibits an sp³d hybridization and a 'seesaw' molecular structure, as predicted by the VSEPR theory.
Step-by-step explanation:
Understanding the Lewis Structure of SF4
The Lewis structure of SF4, or sulfur tetrafluoride, shows a central sulfur atom with four single bonds connecting to fluorine atoms and one lone pair of electrons. This configuration indicates five regions of electron density around the sulfur atom, making the hybridization of sulfur in SF4 sp³d. The molecular structure of SF4 is often described in terms of the VSEPR theory, which predicts a 'seesaw' shape due to the arrangement of four bonding pairs and one lone pair.
The valence electron count for sulfur is six, and for each fluorine atom, it is seven. In constructing the Lewis structure, we account for these electrons through bonds and lone pairs. Each fluorine atom has three lone pairs while the sulfur atom has one lone pair after forming single bonds with each of the four fluorine atoms.
Predicting the electron-pair geometry and molecular structure for SF4 involves understanding that it is an AB4E type molecule under the VSEPR theory, with 'A' representing the central atom, 'B' the bonded atoms, and 'E' the lone pairs. The geometrical shape and molecular structure are important in understanding the properties of SF4, especially its utility as a fluorinating agent in the creation of fluorine-containing compounds used for applications such as herbicides.