Choose the incorrect order.

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(A) Let us analyze each option:$A$. $IE_2$ order: $Li^+ (1s^2)$,$O^+ (1s^2 2s^2 2p^3)$,$F^+ (1s^2 2s^2 2p^4)$. $Li^+$ has a noble gas configuration,so

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$Li > O > F$ ($IE_2$ order)

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(A) Let us analyze each option:$A$. $IE_2$ order: $Li^+ (1s^2)$,$O^+ (1s^2 2s^2 2p^3)$,$F^+ (1s^2 2s^2 2p^4)$. $Li^+$ has a noble gas configuration,so it has the highest $IE_2$. $F^+$ has higher $Z_{eff}$ than $O^+$,so $IE_2$ order is $Li > F > O$. Thus,option $A$ is incorrect.$B$. $EA$ order: $Mg$ ($3s^2$,stable),$S$ $(3p^4)$,$Cl$ $(3p^5)$. $EA$ increases across a period. $Mg$ has near-zero $EA$. The order $Mg $C$. Size order: $I > Br > F > O > N$. The given order $I > Br > N > O > F$ is incorrect because $N, O, F$ are in the same period and size decreases from $N$ to $F$. Thus,option $C$ is also incorrect.$D$. $Z_{eff}$ order: $Na (Z=11, Z_{eff}=2.2)$,$K (Z=19, Z_{eff}=2.2)$,$Ca (Z=20, Z_{eff}=2.85)$. The order $Na Note: Both $A$ and $C$ are incorrect orders.

Similar Questions

Which of these does not reflect the periodicity of the elements?

Which of the following statements is/are correct?

Which of the following represents the correct order of ionization enthalpy?
$(i) Ba < Sr < Ca$
$(ii) S^{2-} < S < S^{2+}$
$(iii) C < O < N$
$(iv) Mg < Al < Si$

Consider the following orders :-
$(I)$ $Li > Na$ (Reducing nature)
$(II)$ $BF_3 > BCl_3 > BBr_3 > BI_3$ (Rate of hydrolysis)
$(III)$ $B > C > N > O > F$ ($1^{st}$ ionization energy)
$(IV)$ $CCl_4 > SiCl_4$ (Boiling point)
The $CORRECT$ order$(s)$ are :-

$(a)$ $Be$ and $Mg$ are alkaline earth metals.
$(b)$ $K^{+}$ has larger radii than $Ca^{2+}$.
$(c)$ All $d$-block elements are transition elements.
$(d)$ $H^{-}$ ion is larger than $F^{-}$.
Incorrect statement is/are

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