Draw the Lewis structure for COCl2, including lone pairs

The COCl2 molecule has 3 areas of electron repulsion around the central C atom, so the shape is trigonal planar.

Both C–Cl bonds are polar, due to the difference in electronegativity of C and Cl.

The Lewis structure of the COCl2 molecule shows that there is a double bond between the O and the central C atom. A double bond represents a slightly larger electron domain which disrupts the ideal 120° Cl-C-Cl bond angle, making it smaller. Because three electron domains surround the central atom, we might expect a trigonal-planar geometry with 120° bond angles. The double bond, however, seems to act much like a nonbonding pair of electrons, reducing the Cl-C-Cl bond angle to 111.4°:

The C=O bond is also polar, due to the difference in electronegativity of C and O. Even though the shape is trigonal planar, the molecule is asymmetrical, as the electronegativity difference of the three bonds is not the same. Therefore the effects of these polar bonds are not cancelled and the molecule is polar overall.

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