The molecular geometry of dichlorine monoxide is bent as a result of the lone electron pairs located on the oxygen atom. Molecular geometry is physical representation of the relation between elements in a compound.
Molecular geometry is characterized by the Valence Shell Electron-Pair Repulsion Model. This three-dimensional model is based on the repulsive forces between electron pairs. It starts with the principle that the octet rule must be satisfied for each element. This means that each element must have eight valence electrons in the outer shell. Since many elements do not have eight valence electrons in their outer shell, electron sharing results. The electrons that are not shared are illustrated by dots.
There are a total of 13 molecular geometries. These geometries are differentiated from one another by several factors, including the number of bonding groups and lone pair electrons on the central atom. An additional factor is the electron pair geometry, which can be one of five types. This is important for dichlorine monoxide since there are two molecular geometries that are classified as bent. Because the central oxygen atom has two lone electron pairs, it is classified as tetrahedral bent rather than trigonal planar bent. This geometric formation is characterized by bonding angles that are less than 109.5 degrees.