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.

Label	Order	Property
$i.$	$NH_3 > H_2O > SO_2$	Bond angle
$ii.$	$H_2O > NH_3 > H_2S$	Dipole moment
$iii.$	$N_2 > O_2 > H_2$	Bond enthalpy
$iv.$	$NO^{+} > O_2 > O_2^{2-}$	Bond order

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Observe the following sets:
Label Order Property
$i.$ $NH_3 > H_2O > SO_2$ Bond angle
$ii.$ $H_2O > NH_3 > H_2S$ Dipole moment
$iii.$ $N_2 > O_2 > H_2$ Bond enthalpy
$iv.$ $NO^{+} > O_2 > O_2^{2-}$ Bond order

Which of the above sets are correctly matched?

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