Oxygen dichloride (OCI2) is polar.
As explained by chemicalminds, Cl2O (or OCl2) molecule has 4 electron repulsions around the central atom, which gives the molecule a basic tetrahedral shape. Two are bonding sets and two are non-bonding sets, so the molecule has a bent shape.
OCl2 also contains polar bonds. The bonds are polar as the atoms in the bonds have different electronegativity values. In OCl2, the polar bonds are arranged asymmetrically around the central atom in a bent shape as there are two lone pair of electrons on the central atom. The bond dipoles do not cancel and the molecule is polar.
When atoms of different electronegativities form a bond, the electrons tend to be more controlled by the atom with the higher electronegativity.
The resulting bond is a dipole — it has a slight negative charge on the higher electronegativity side, and a slight positive charge on the other end.
This type of bond is called a polar bond. Examples of polar bonded molecules include hydrochloric acid (HCl) and water (H2O).
Not all molecules with polar bonds are polar molecules. To be a polar molecule, the entire molecule must be a dipole – it must have slightly positive and slightly negative ends.
To learn more about Polar and Non-Polar Bonds, visit College-Cram Chemistry.
Check out these Study Tips for Chemistry Students, shared by University of Pittsburgh at Bradford.