Which of the following statements is correct?

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(D) $1$. Bond angle: In $NH_3$,the electronegativity of $N$ is higher than $H$,so bond pairs are closer to $N$. In $NF_3$,$F$ is more electronegative

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(D) $1$. Bond angle: In $NH_3$,the electronegativity of $N$ is higher than $H$,so bond pairs are closer to $N$. In $NF_3$,$F$ is more electronegative than $N$,so bond pairs are closer to $F$. Thus,$NH_3$ has a larger bond angle $(107^\circ)$ compared to $NF_3$ $(102^\circ)$. So,$NH_3 > NF_3$ is correct.$2$. Reactivity towards Lewis acid: $NH_3$ is a stronger Lewis base than $NF_3$ because the highly electronegative $F$ atoms in $NF_3$ withdraw electron density from the $N$ atom,reducing the availability of the lone pair. Thus,$NH_3 > NF_3$ is correct.$3$. Dipole moment: In $NH_3$,the orbital dipole due to the lone pair and the resultant dipole of $N-H$ bonds are in the same direction. In $NF_3$,the orbital dipole and the resultant dipole of $N-F$ bonds are in opposite directions. Thus,$NH_3$ $(1.46 \ D)$ has a higher dipole moment than $NF_3$ $(0.24 \ D)$. So,$NH_3 > NF_3$ is correct.

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