Phosgene, Cl2 C=O, has a smaller dipole moment than formaldehyde, H2 C=O, even though it contain

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Phosgene, Cl2 C=O, has a smaller dipole moment than...

Phosgene, $\mathrm{Cl}_{2} \mathrm{C}=\mathrm{O},$ has a smaller dipole moment than formaldehyde, $\mathrm{H}_{2} \mathrm{C}=\mathrm{O},$ even though it contains electronegative chlorine atoms in place of hydrogen. Explain.

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Key Concepts

Bond Polarity

Bond polarity arises from differences in electronegativity between two bonded atoms, creating a partial positive and a partial negative end. In molecules like formaldehyde and phosgene, the polarity of bonds (such as C=O, C–H, and C–Cl) depends on the electronegativities of the atoms involved and the nature of the bonds.

Molecular Geometry and Vector Addition of Dipole Moments

The overall dipole moment of a molecule is determined by the vector sum of its individual bond dipoles, which depends on the geometry of the molecule. In phosgene, the arrangement of chlorine atoms relative to the carbonyl group causes the bond dipoles to partially cancel out, leading to a smaller net dipole moment compared to formaldehyde, where the molecular geometry results in a larger net dipole.

Dipole Moment

A dipole moment is a measure of the separation of electrical charges within a molecule, resulting from differences in electronegativity between bonded atoms. This concept quantifies how polar a molecule is by taking into account the magnitude of each bond's charge separation and their spatial arrangement.

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