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(B) $(I)$ Incorrect: In $NH_3$,the orbital dipole due to the lone pair and the net dipole moment of the three $N-H$ bonds are in the same direction,wh

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$II, III$ only

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(B) $(I)$ Incorrect: In $NH_3$,the orbital dipole due to the lone pair and the net dipole moment of the three $N-H$ bonds are in the same direction,whereas in $NF_3$,they are in opposite directions. Thus,$\mu(NH_3) > \mu(NF_3)$. $BF_3$ is symmetrical and has zero dipole moment. The correct order is $NH_3 > NF_3 > BF_3$.$(II)$ Correct: Bond length increases with the increase in the size of the atoms. Atomic radii follow the order $C > N > O > H$,so the bond length order $C-O > N-O > O-H$ is correct.$(III)$ Correct: According to Molecular Orbital Theory,the bond order of $C_2$ is $2$,$B_2$ is $1$,and $He_2$ is $0$. The order $C_2 > B_2 > He_2$ is correct.

List-$I$	List-$II$
$(A)$ $C_{2}H_{4}$	$(I)$ $3\sigma$ bonds, $2\pi$ bonds
$(B)$ $C_{2}H_{2}$	$(II)$ $3\sigma$ bonds, $1$ lone pair
$(C)$ $CH_{4}$	$(III)$ $4\sigma$ bonds
$(D)$ $NH_{3}$	$(IV)$ $5\sigma$ bonds, $1\pi$ bond

Which of the following orders are correct against the property given?
$(I)$ Dipole moment $NF_3 > NH_3 > BF_3$
$(II)$ Covalent bond length $C-O > N-O > O-H$
$(III)$ Bond order $C_2 > B_2 > He_2$

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

Which of the following orders are correct against the property given? $(I)$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$