Final answer:
In CCl₂O, the double bond between carbon and oxygen causes the Cl-C-Cl bond angle to be slightly less than 120 degrees, due to the higher electron density and increased repulsion compared to single bonds.
Step-by-step explanation:
The effect of multiple bond angles can be observed in molecules with double or triple bonds. For instance, in CCl₂O (carbonyl dichloride), which is analogous to CH₂O (formaldehyde) and has a molecular geometry described as trigonal planar, the presence of a double bond between the central carbon atom and the oxygen atom results in the carbon-oxygen double bond taking up more space than a single bond would.
This higher electron density around the double bond can cause the bond angles surrounding the central carbon to be smaller than the ideal 120 degrees typically observed in a perfect trigonal planar geometry.
In a molecule like CCl₂O with a double bond, the Cl-C-Cl bond angle is slightly less than 120 degrees due to the increased repulsion caused by the electron density of the C=O double bond.
The other bond angles in the molecule are similarly affected, resulting in a slightly distorted trigonal planar shape compared to a molecule with only single bonds.