$A$ diatomic molecule has a dipole moment of $1.2 \ D$. If the bond distance is $1 \ \mathring{A}$,then fractional charge on each atom is.........$\times 10^{-2}$ (Given $1 \ D = 10^{-18} \ esu \ cm$ )

Which one of the following molecules has a zero dipole moment?

$PCl_3Br_2$ exhibits geometric isomerism,and its geometric isomers are shown below. Which of these does not have a dipole moment?

Given below are two statements:
Statement-$I$: Since fluorine is more electronegative than nitrogen,the net dipole moment of $NF_3$ is greater than $NH_3$.
Statement-$II$: In $NH_3$,the orbital dipole due to lone pair and the dipole moment of $N-H$ bonds are in opposite direction,but in $NF_3$ the orbital dipole due to lone pair and dipole moments of $N-F$ bonds are in same direction.
In the light of the above statements,choose the most appropriate from the options given below.

Which of the following has the lowest dipole moment?

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