Which of the following orders is not correct | vedclass

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(B) Let us analyze each option:$1$. First ionisation enthalpy: The order is $N > O > P > S$. Nitrogen $(2p^3)$ has a stable half-filled configuration,

Vedclass · Accepted Answer

$F > Cl > O > S$ - Negative electron gain enthalpy

Vedclass · Answer

(B) Let us analyze each option:$1$. First ionisation enthalpy: The order is $N > O > P > S$. Nitrogen $(2p^3)$ has a stable half-filled configuration,making its $IE_1$ higher than Oxygen $(2p^4)$. Similarly,Phosphorus $(3p^3)$ is higher than Sulfur $(3p^4)$. Across the period,$N > O$ and $P > S$,and down the group $N > P$ and $O > S$. Thus,$N > O > P > S$ is correct.$2$. Negative electron gain enthalpy: The correct order is $Cl > F > S > O$. Chlorine has a higher electron gain enthalpy than Fluorine due to inter-electronic repulsion in the small $2p$ orbital of Fluorine. Similarly,Sulfur is higher than Oxygen. The given order $F > Cl > O > S$ is incorrect.$3$. Size: For the same element in different oxidation states,the size decreases as the positive charge increases. Thus,$Fe^{3+} $4$. Non-metallic character: Non-metallic character increases across a period and decreases down a group. $O$ and $N$ are more non-metallic than $S$ and $P$. Among $O$ and $N$,$O$ is more electronegative/non-metallic. Thus,$O > N > S > P$ is correct.Therefore,the incorrect order is option $B$.

Which of the following orders is not correct about the property shown against it?

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