The incorrect relation among the following is

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(B) The first ionization energy $(IE_1)$ of $Mg$ $([Ne] 3s^2)$ is higher than $Al$ $([Ne] 3s^2 3p^1)$ because $Mg$ has a stable fully-filled $s$-orbit

Vedclass · Accepted Answer

$(Mg)_{IE_2} > (Na)_{IE_2}$

Vedclass · Answer

(B) The first ionization energy $(IE_1)$ of $Mg$ $([Ne] 3s^2)$ is higher than $Al$ $([Ne] 3s^2 3p^1)$ because $Mg$ has a stable fully-filled $s$-orbital. Thus,$(Al)_{IE_1} For $IE_2$,$Na$ $([Ne] 3s^1)$ loses its second electron from the stable $2p^6$ configuration,while $Mg$ $([Ne] 3s^2)$ loses its second electron from the $3s^1$ orbital. Thus,$(Na)_{IE_2} > (Mg)_{IE_2}$. Therefore,the relation $(Mg)_{IE_2} > (Na)_{IE_2}$ is incorrect.$(Na)_{IE_1} $(Mg)_{IE_3} > (Al)_{IE_3}$ is correct because $Mg^{2+}$ has a stable noble gas configuration,making the removal of the third electron very difficult compared to $Al^{2+}$.

Similar Questions

Observe the following statements.
Statement $(A)$: In general,the ionisation potential value decreases on moving down in the group.
Statement $(B)$: The $1$st ionisation potential of sodium is greater than that of potassium.
Correct answer is:

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If first ionization enthalpies of element $X$ and $Y$ are $419 \ kJ \ mol^{-1}$ and $590 \ kJ \ mol^{-1}$,respectively and second ionization enthalpies of $X$ and $Y$ are $3069 \ kJ \ mol^{-1}$ and $1145 \ kJ \ mol^{-1}$,respectively. Then the correct statement is :-

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