Observe the following statements:i. The dipol | vedclass

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(A) $i$. In $NH_3$,the direction of the dipole moment of $N-H$ bonds and the lone pair are in the same direction,whereas in $NF_3$,the dipole moment o

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Only $i$ is correct

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(A) $i$. In $NH_3$,the direction of the dipole moment of $N-H$ bonds and the lone pair are in the same direction,whereas in $NF_3$,the dipole moment of $N-F$ bonds and the lone pair are in opposite directions. Thus,the dipole moment of $NH_3$ $(1.46 \ D)$ is higher than $NF_3$ $(0.24 \ D)$. Statement $i$ is correct.$ii$. Chloroform $(CHCl_3)$ has a net dipole moment of $1.04 \ D$ due to the difference in electronegativity between $C-H$ and $C-Cl$ bonds. Statement $ii$ is incorrect.$iii$. According to Fajan's rule,$Cu^+$ (a pseudo-noble gas configuration) has higher polarising power than $Na^+$ (a noble gas configuration). Therefore,$CuCl$ has more covalent character than $NaCl$. Statement $iii$ is incorrect.Therefore,only statement $i$ is correct.

$(I)$	Dipole moment	$NF_3 > NH_3 > BF_3$
$(II)$	Covalent bond length	$C-O > N-O > O-H$
$(III)$	Bond order	$C_2 > B_2 > He_2$

Observe the following statements:
$i$. The dipole moment of $NH_3$ is higher than the dipole moment of $NF_3$.
$ii$. The dipole moment of chloroform $(CHCl_3)$ is zero.
$iii$. Covalent bond character in $NaCl$ is more compared to $CuCl$.

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Observe the following statements:$i$. The dipole moment of $NH_3$ is higher than the dipole moment of $NF_3$.$ii$. The dipole moment of chloroform $(CHCl_3)$ is zero.$iii$. Covalent bond character in $NaCl$ is more compared to $CuCl$.