A Lewis structure is a two-dimensional representation of a molecule that does not necessarily show what shape that molecule would take in three dimensions.Based on the Lewis structure and your knowledge of VSEPR theory, approximate the smallest bond angle in this molecule.*Picture attached* The image is a Lewis structure of a generic tetrahedral molecule, which consists of a central atom denoted as 'Y' bonded to four outer atoms labeled 'X'. The structure is organized as follows:- The central atom 'Y' has two pairs of electrons (dots) marked above it, indicating lone pairs.- Four single lines radiate from the 'Y', representing single bonds to each 'X' atom. This forms a symmetrical tetrahedral shape.- Each 'X' represents an atom bonded to 'Y', typically part of a more complex molecular structure.This diagram illustrates the basic bonding and spatial arrangement in a tetrahedral molecule, a common molecular geometry in chemistry.

VSEPR theory is Valence Shell Electron Pair Repulsion theory. This theory gives the best possible geometry of the bonding electron and lone pair of electron so that the repulsion in the compound will be minimum. Here in the figure, there is 4 bond pair which means 4 atoms are bonded to central atom and one lone pair of electron is also present. So this is AX4E type compound, where A is the central atom X is the bond pair electron E is the lone pair of electron So the best possible geometry of this type of compound is Sea saw geometry. One of the example of this type of compound is SF4. The electronic geometry should be trigonal bipyramidal which has two type of bond angle 900 and 1200. But due to the presence of lone pair of electron, there is slight deviation in these ideal bond angle. So there is two different angle present in the sea saw geometry. One is lesser than 900 and another is lesser than 1200. The angle of this compound is shown in image-