The dipole moment of H2 O is 1.85 D. The O-H bond moment would be (given the H-O-H bond angle as

step 1 Now the question is the dipole moment of H2O is 1 .85. So we have a data which is mu1 is equal t

The dipole moment of H2 O is 1.85 D. The O-H bond moment...

The dipole moment of $\mathrm{H}_{2} \mathrm{O}$ is $1.85 \mathrm{D}$. The $\mathrm{O}-\mathrm{H}$ bond moment would be (given the $\mathrm{H}-\mathrm{O}-\mathrm{H}$ bond angle as $104.5^{\circ}$ and $\left.\cos 104.5^{\circ}=-0.25\right)$ (a) $1.51 \mathrm{D}$ (b) $2.41 \mathrm{D}$ (c) $1.86 \mathrm{D}$ (d) $1.91 \mathrm{D}$

The dipole moment of $\mathrm{H}_{2} \mathrm{O}$ is $1.85 \mathrm{D}$. The $\mathrm{O}-\mathrm{H}$ bond moment would be (given the $\mathrm{H}-\mathrm{O}-\mathrm{H}$ bond angle as $104.5^{\circ}$ and $\left.\cos 104.5^{\circ}=-0.25\right)$
(a) $1.51 \mathrm{D}$
(b) $2.41 \mathrm{D}$
(c) $1.86 \mathrm{D}$
(d) $1.91 \mathrm{D}$

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Key Concepts

Effect of Molecular Geometry

The spatial arrangement of bonds, such as the bond angles in a molecule, plays a critical role in determining the net dipole moment. By using vector addition (often with the law of cosines), the contributions of individual bond dipoles are combined, and the resulting net dipole moment reflects both the magnitudes and the orientations of these bonds.

Vector Addition of Dipole Moments

When a molecule has more than one bond dipole, the overall molecular dipole moment is the vector sum of the individual bond dipoles. The directions and magnitudes of these vectors, combined with the bond angles, determine how much they reinforce or cancel each other out.

Dipole Moment

A dipole moment measures the separation of positive and negative charges in a molecule. It is a vector quantity that defines not just the magnitude of the charge separation, but also its direction, which is critical when considering how molecular bonds contribute to the overall polarity of a molecule.

Bond Dipole Moment

A bond dipole moment refers to the polarity of an individual chemical bond, arising from a difference in electronegativity between the bonded atoms. Each bond dipole is represented as a vector, and its magnitude depends on both the charge difference and the distance between the charges.

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