Which of the following molecules has the high | vedclass

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(D) The dipole moment of a molecule depends on its geometry and the electronegativity difference between the bonded atoms.$1$. $BCl_3$ is a trigonal p

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$H_2O$

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(D) The dipole moment of a molecule depends on its geometry and the electronegativity difference between the bonded atoms.$1$. $BCl_3$ is a trigonal planar molecule with a symmetric structure,resulting in a net dipole moment of $0$.$2$. $PCl_5$ is a trigonal bipyramidal molecule with a symmetric structure,resulting in a net dipole moment of $0$.$3$. $NH_3$ has a pyramidal geometry with a lone pair on the nitrogen atom. Its dipole moment is approximately $1.47 \ D$.$4$. $H_2O$ has a bent geometry. The bond dipoles of the two $O-H$ bonds and the lone pairs on the oxygen atom reinforce each other,resulting in a higher net dipole moment of approximately $1.85 \ D$.Therefore,$H_2O$ has the highest dipole moment among the given options.

Which of the following molecules has the highest dipole moment?

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