Which molecule has the largest dipole moment?

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(D) The dipole moment $\mu$ is defined as the product of the magnitude of the charge $(q)$ and the distance of separation $(d)$ between the charges, i

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$HF$

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(D) The dipole moment $\mu$ is defined as the product of the magnitude of the charge $(q)$ and the distance of separation $(d)$ between the charges, i.e., $\mu = q 	imes d$. In the hydrogen halides $(HF, HCl, HBr, HI)$, the electronegativity of the halogen decreases as we move down the group $(F > Cl > Br > I)$. Consequently, the electronegativity difference between hydrogen and the halogen is highest for $HF$, leading to the largest partial charges $(q)$. Although the bond length $(d)$ increases from $HF$ to $HI$, the effect of the large electronegativity difference in $HF$ dominates, making $HF$ the most polar molecule with the largest dipole moment.

List-$I$	List-$II$
$(1)$ ${\rm{HBr}}$	$(A)$ $0.23$
$(2)$ ${{\rm{H}}_2}{\rm{S}}$	$(B)$ $1.04$
$(3)$ ${\rm{N}}{{\rm{F}}_3}$	$(C)$ $1.07$
$(4)$ ${\rm{CC}}{{\rm{l}}_4}$	$(D)$ $0.79$
$(5)$ ${\rm{CHC}}{{\rm{l}}_3}$	$(E)$ $0.00$
	$(F)$ $0.95$

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