The incorrect statement among the following i | vedclass

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(B) $NCl_5$ does not exist because nitrogen lacks vacant $d$-orbitals,whereas $PCl_5$ exists due to the presence of $d$-orbitals in phosphorus.$Pb$ ex

Vedclass · Accepted Answer

$Pb$ prefers to form tetravalent compounds

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(B) $NCl_5$ does not exist because nitrogen lacks vacant $d$-orbitals,whereas $PCl_5$ exists due to the presence of $d$-orbitals in phosphorus.$Pb$ exhibits the inert pair effect,which makes the $+2$ oxidation state more stable than the $+4$ state; therefore,$Pb$ prefers to form divalent compounds rather than tetravalent ones.In the $CO_3^{2-}$ ion,all three $C-O$ bonds are equivalent due to resonance.Both $O_2^{+}$ and $NO$ contain unpaired electrons in their molecular orbitals,making them paramagnetic.Thus,the statement in option $B$ is incorrect.

List-$I$	List-$II$
$(P). \ IF_7$	$(a). \ \text{Planar} \ \& \ \text{Polar}$
$(Q). \ SO_2$	$(b). \ \text{Non-planar} \ \& \ \text{Polar}$
$(R). \ SF_4$	$(c). \ \text{Planar} \ \& \ \text{Non-polar}$
$(S). \ CS_2$	$(d). \ \text{Non-planar} \ \& \ \text{Non-polar}$

The incorrect statement among the following is/are:

Similar Questions

The total number of right angles $\angle ClPCl$ present in $PCl_5$,$PCl_4^+$,and $PCl_6^-$ are . . . . . . , . . . . . . , . . . . . . respectively.

Match List-$I$ with List-$II$:

List-$I$ List-$II$

$(P). \ IF_7$ $(a). \ \text{Planar} \ \& \ \text{Polar}$

$(Q). \ SO_2$ $(b). \ \text{Non-planar} \ \& \ \text{Polar}$

$(R). \ SF_4$ $(c). \ \text{Planar} \ \& \ \text{Non-polar}$

$(S). \ CS_2$ $(d). \ \text{Non-planar} \ \& \ \text{Non-polar}$

What is the formal charge on the $N$ atom in the $NH_4^{+}$ ion?

The decreasing order of bond angles in $BF_3$,$NH_3$,$PF_3$ and $I_3^-$ is

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

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