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(B) $1$. For $NH_3$ and $NF_3$: The dipole moment of $NH_3$ $(1.46 \ D)$ is greater than $NF_3$ $(0.24 \ D)$ because in $NH_3$,the orbital dipole and

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$CO < CO_2$ ($C-O$ bond length)

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(B) $1$. For $NH_3$ and $NF_3$: The dipole moment of $NH_3$ $(1.46 \ D)$ is greater than $NF_3$ $(0.24 \ D)$ because in $NH_3$,the orbital dipole and bond dipoles are in the same direction,while in $NF_3$,they oppose each other. Thus,$A$ is incorrect.$2$. For $CO$ and $CO_2$: The $C-O$ bond length in $CO$ $(1.128 \ \mathring{A})$ is shorter than in $CO_2$ $(1.16 \ \mathring{A})$ due to the triple bond character in $CO$. Thus,$B$ is correct.$3$. For $NH_2^-$ and $NH_4^+$: $NH_2^-$ is $sp^3$ hybridized with two lone pairs (bond angle $\approx 104.5^\circ$),while $NH_4^+$ is $sp^3$ hybridized with zero lone pairs (bond angle $109.5^\circ$). Thus,$NH_2^- $4$. For $I_3^-$ and $N_3^-$: $I_3^-$ has $3$ lone pairs on the central $I$ atom,while $N_3^-$ has $0$ lone pairs on the central $N$ atom. Thus,$I_3^- > N_3^-$. Option $D$ is incorrect.

Find the correct option regarding the given chemical properties.

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