The correct order of dipole moments of NH_3,H | vedclass

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Question

(A) The dipole moments are: $H_2O = 1.85 \ D$,$NH_3 = 1.47 \ D$,and $NF_3 = 0.24 \ D$. In $NH_3$,the dipole moments of the three $N-H$ bonds and the l

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$H_2O > NH_3 > NF_3$

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(A) The dipole moments are: $H_2O = 1.85 \ D$,$NH_3 = 1.47 \ D$,and $NF_3 = 0.24 \ D$. In $NH_3$,the dipole moments of the three $N-H$ bonds and the lone pair are in the same direction,resulting in a higher net dipole moment. In $NF_3$,the dipole moments of the three $N-F$ bonds are in the opposite direction to the lone pair,which partially cancels out the net dipole moment. $H_2O$ has a higher dipole moment than $NH_3$ due to the higher electronegativity difference between $O$ and $H$ compared to $N$ and $H$,and the presence of two lone pairs. Thus,the correct order is $H_2O > NH_3 > NF_3$.

The correct order of dipole moments of $NH_3$,$H_2O$ and $NF_3$ is

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