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.

List-$I$	List-$II$
$(1)$ ${\rm{HBr}}$	$(A)$ $0.23$
$(2)$ ${{\rm{H}}_2}{\rm{S}}$	$(B)$ $1.04$
$(3)$ ${\rm{N}}{{\rm{F}}_3}$	$(C)$ $1.07$
$(4)$ ${\rm{CC}}{{\rm{l}}_4}$	$(D)$ $0.79$
$(5)$ ${\rm{CHC}}{{\rm{l}}_3}$	$(E)$ $0.00$
	$(F)$ $0.95$

Which of the following molecules has the highest dipole moment?

Similar Questions

Which of the following compounds has the highest dipole moment $(D)$?

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Reason : Polarizability is observed only in those molecules which have a permanent dipole moment.

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