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(A) Assertion $A$ is true: Both $NH_3$ and $NF_3$ have a pyramidal geometry with one lone pair on the $N$ atom. The dipole moment of $NH_3$ $(1.46 \ D

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Both $A$ and $R$ are true and $R$ is the correct explanation of $A$

Vedclass · Answer

(A) Assertion $A$ is true: Both $NH_3$ and $NF_3$ have a pyramidal geometry with one lone pair on the $N$ atom. The dipole moment of $NH_3$ $(1.46 \ D)$ is greater than that of $NF_3$ $(0.24 \ D)$.Reason $R$ is true: In $NH_3$,the direction of the dipole moment of the $N-H$ bonds is towards the nitrogen atom,which is the same as the direction of the lone pair orbital dipole. This leads to reinforcement and a higher resultant dipole moment.In $NF_3$,the $N-F$ bond dipoles are directed away from the nitrogen atom (since $F$ is more electronegative than $N$),which opposes the direction of the lone pair orbital dipole,resulting in a smaller net dipole moment.Thus,$R$ is the correct explanation for $A$.

Similar Questions

Which of the following are arranged in the decreasing order of dipole moment?

Dipole moment of $HCl = 1.03 \ D$ and $HI = 0.38 \ D$. Bond length of $HCl = 1.3 \ \mathring{A}$ and $HI = 1.6 \ \mathring{A}$. The ratio of the fraction of electric charge,$\delta$,existing on each atom in $HCl$ and $HI$ is:

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

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

If compound $MX_4$ has $\mu = 0$,then the most probable geometry will be:

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