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(C) Let us determine the number of lone pairs for each molecule:$1$. $H_2O$: Oxygen has $2$ lone pairs.$2$. $N_2$: Each Nitrogen atom has $1$ lone pai

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$4$

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(C) Let us determine the number of lone pairs for each molecule:$1$. $H_2O$: Oxygen has $2$ lone pairs.$2$. $N_2$: Each Nitrogen atom has $1$ lone pair,total $2$ lone pairs.$3$. $CO$: Carbon has $1$ lone pair and Oxygen has $1$ lone pair,total $2$ lone pairs.$4$. $XeF_4$: Xenon has $2$ lone pairs.$5$. $NH_3$: Nitrogen has $1$ lone pair.$6$. $NO$: Nitrogen has $1$ lone pair and Oxygen has $2$ lone pairs (total $3$ lone pairs).$7$. $CO_2$: Carbon has $0$ lone pairs,each Oxygen has $2$ lone pairs (total $4$ lone pairs).$8$. $F_2$: Each Fluorine has $3$ lone pairs (total $6$ lone pairs).Thus,the molecules with exactly $2$ lone pairs are $H_2O, N_2, CO,$ and $XeF_4$.The total count is $4$.

Order	Property
$(A)$ $NO_2 > O_3 > H_2O$	Bond angle
$(B)$ $H_2O > HF > NH_3$	Dipole moment
$(C)$ $I_2 > F_2 > N_2$	Bond length

The number of molecules from the following which contain only two lone pairs of electrons is $........$.
$H_2O, N_2, CO, XeF_4, NH_3, NO, CO_2, F_2$

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The number of molecules from the following which contain only two lone pairs of electrons is $........$.$H_2O, N_2, CO, XeF_4, NH_3, NO, CO_2, F_2$