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(B) The octet rule states that atoms tend to gain,lose,or share electrons to achieve a stable configuration of $8$ electrons in their valence shell.Le

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$6$

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(B) The octet rule states that atoms tend to gain,lose,or share electrons to achieve a stable configuration of $8$ electrons in their valence shell.Let us analyze each molecule:$1$. $CO_2$: Carbon has $8$ electrons (complete octet).$2$. $NO_2$: Nitrogen has an odd number of electrons ($7$ electrons,exception).$3$. $H_2SO_4$: Sulfur has an expanded octet ($12$ electrons,exception).$4$. $BF_3$: Boron has an incomplete octet ($6$ electrons,exception).$5$. $CH_4$: Carbon has $8$ electrons (complete octet).$6$. $SiF_4$: Silicon has $8$ electrons (complete octet).$7$. $ClO_2$: Chlorine has an odd number of electrons ($7$ electrons,exception).$8$. $PCl_5$: Phosphorus has an expanded octet ($10$ electrons,exception).$9$. $BeF_2$: Beryllium has an incomplete octet ($4$ electrons,exception).$10$. $C_2H_6$: Carbon has $8$ electrons (complete octet).$11$. $CHCl_3$: Carbon has $8$ electrons (complete octet).$12$. $CBr_4$: Carbon has $8$ electrons (complete octet).The molecules that are exceptions to the octet rule are: $NO_2, H_2SO_4, BF_3, ClO_2, PCl_5, BeF_2$.Total number of exceptions = $6$.

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

Number of molecules from the following which are exceptions to the octet rule is. . . .
$CO_2, NO_2, H_2SO_4, BF_3, CH_4, SiF_4, ClO_2, PCl_5, BeF_2, C_2H_6, CHCl_3, CBr_4$

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Number of molecules from the following which are exceptions to the octet rule is. . . .$CO_2, NO_2, H_2SO_4, BF_3, CH_4, SiF_4, ClO_2, PCl_5, BeF_2, C_2H_6, CHCl_3, CBr_4$