Identify the correct statement among the foll | vedclass

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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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$CO < CO_2$ (Bond length of $C-O$)

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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,whereas in $NF_3$,they oppose each other. Thus,$NH_3 > NF_3$. Option $A$ is incorrect.$2$. For $CO$ and $CO_2$: The bond order of $CO$ is $3$ $(C \equiv O)$,and the bond order of $CO_2$ is $2$ $(O=C=O)$. Higher bond order implies shorter bond length. Thus,$CO $3$. For $NH_2^-$ and $NH_4^+$: $NH_2^-$ has $sp^3$ hybridization with $2$ lone pairs (bond angle $\approx 104.5^\circ$),while $NH_4^+$ has $sp^3$ hybridization with $0$ 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.

Identify the correct statement among the following options.

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