Which of the following does not obey the octe | vedclass

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Question

(D) 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. $

Vedclass · Accepted Answer

$CO$ and $PCl_5$

Vedclass · Answer

(D) 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. $CO$ (Carbon monoxide) has a total of $10$ valence electrons ($4$ from $C$ and $6$ from $O$). In the structure $:C \equiv O:$,the carbon atom has only $6$ electrons in its valence shell,which is an incomplete octet. $PCl_5$ (Phosphorus pentachloride) has $5$ valence electrons from $P$ and $5$ from $5$ $Cl$ atoms,resulting in $10$ electrons around the central $P$ atom,which is an expanded octet. Therefore,both $CO$ and $PCl_5$ do not obey the octet rule.

Column-$I$	Column-$II$
$(P)$ $\underline PCl_5 \to PCl_3 + Cl_2$	$(i)$ Change in hybridisation
$(Q)$ $\underline SO_3 \to \underline SO_2 + \frac{1}{2}O_2$	$(ii)$ Change in bond angle
$(R)$ $\underline NH_3 + H^{+} \to \underline NH_4^+$	$(iii)$ Change in shape
$(S)$ $H_2\underline O + H^{+} \to H_3\underline O^{+}$	$(iv)$ Change in oxidation state

Which of the following does not obey the octet rule?

Similar Questions

What is formal charge? Explain by example.

Each of the following compounds contains $p\pi -d\pi$ bonds except:

The formal charges of $N_{(1)}$,$N_{(2)}$ and $O$ atoms in the structure shown below are respectively:
$:N_{(1)}=N_{(2)}=\ddot{O}:$

Which one of the following is a correct set?

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