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(B) The dipole moments of the given molecules are as follows:$1. \ H_2O$: It has a bent geometry with a high dipole moment of $1.85 \ D$ $(A-IV)$.$2.

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$A-IV, B-I, C-III, D-II$

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(B) The dipole moments of the given molecules are as follows:$1. \ H_2O$: It has a bent geometry with a high dipole moment of $1.85 \ D$ $(A-IV)$.$2. \ BF_3$: It has a trigonal planar geometry,making it a symmetric molecule with a net dipole moment of $0 \ D$ $(B-I)$.$3. \ NH_3$: It has a trigonal pyramidal geometry with a dipole moment of $1.47 \ D$ $(C-III)$.$4. \ NF_3$: It also has a trigonal pyramidal geometry,but due to the high electronegativity of fluorine,the bond dipoles oppose the lone pair dipole,resulting in a lower dipole moment of $0.23 \ D$ $(D-II)$.Therefore,the correct matching is $A-IV, B-I, C-III, D-II$.

Match the following molecules in List-$I$ with their respective dipole moments in List-$II$:
| List-$I$ (Molecules) | List-$II$ (Dipole moment $\mu$,$D$) |
| :--- | :--- |
| $A. \ H_2O$ | $I. \ 0$ |
| $B. \ BF_3$ | $II. \ 0.23$ |
| $C. \ NH_3$ | $III. \ 1.47$ |
| $D. \ NF_3$ | $IV. \ 1.85$ |

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Match the following molecules in List-$I$ with their respective dipole moments in List-$II$:| List-$I$ (Molecules) | List-$II$ (Dipole moment $\mu$,$D$) || :--- | :--- || $A. \ H_2O$ | $I. \ 0$ || $B. \ BF_3$ | $II. \ 0.23$ || $C. \ NH_3$ | $III. \ 1.47$ || $D. \ NF_3$ | $IV. \ 1.85$ |