Even otherwise, the net resultant dipole moment of the molecule is the vector sum of the individual moments. If the angle of a bond is more, then its contribution to the vector sum will be less as the component value of the bond is p * cos Ф = q d cos Ф. The less the bond angle is, more the sum.

Relationship between Bond Angle and Dipole Moment

Bond angle and dipole moment are both important concepts in chemistry. The bond angle is the angle between two adjacent bonds in a molecule, while the dipole moment is a measure of the separation of positive and negative charges within a molecule.

Effect of Bond Angle on Dipole Moment

The bond angle has a significant effect on the dipole moment of a molecule. This is because the dipole moment is a vector quantity that depends on both the magnitude and direction of the charge separation within the molecule.

As the bond angle decreases, the dipole moment of the molecule increases. This is because a smaller bond angle results in a greater separation of charges within the molecule.

For example, water (H2O) has a bond angle of approximately 104.5 degrees. This results in a dipole moment of 1.85 Debye units, which indicates a significant separation of charges within the molecule.

In contrast, carbon dioxide (CO2) has a bond angle of approximately 180 degrees, resulting in a dipole moment of zero. This is because the charges within the molecule are evenly distributed and cancel each other out.

Summary

In summary, the bond angle has a significant effect on the dipole moment of a molecule. A smaller bond angle leads to a greater separation of charges within the molecule, resulting in a larger dipole moment. Conversely, a larger bond angle results in a smaller dipole moment, as the charges within the molecule are more evenly distributed.