Question

1. What is the electron (or electron group) geometry of Cl20? trigonal bipyramidal O tetrahedral linear O octahedreal Otrigonal planar

Answer 1

To draw OCl₂, first count how the electrons go. The O-Cl bond is a single covalent bond. Thus we can draw the O atom in the centre, with two Cl atoms connected to it by covalent bonds. The O atom will be referred to as our central atom; since O has six valence electrons and two are utilized in bonding with the Cl, we have four electrons remaining. These electrons form two lone pairs. Thus, you can draw the molecule by drawing O first, then use pencil to lightly draw a cross through it. Two adjacent arms of the cross would be lone pairs and the other two arms would be the bonds with the Cl. Using the VSEPR (valence shell electron pair repulsion) theory, we know that there are 4 regions of electron density and 2 lone pairs. These regions of electron density will orientate themselves in such a way to minimize electrostatic repulsion. Hence, the electron-pair geometry is tetrahedral and the molecular geometry is bent.