Mg^{2+} is . . . . . . than Al^{3+}. | vedclass

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Question

(C) According to Lewis acid-base theory,a Lewis acid is an electron pair acceptor. The acidity of a metal cation depends on its charge-to-size ratio (

Vedclass · Accepted Answer

a weaker Lewis acid

Vedclass · Answer

(C) According to Lewis acid-base theory,a Lewis acid is an electron pair acceptor. The acidity of a metal cation depends on its charge-to-size ratio (ionic potential). $Al^{3+}$ has a higher charge $(+3)$ and a smaller ionic radius compared to $Mg^{2+}$ $(+2)$. Therefore,$Al^{3+}$ has a higher charge density and is a stronger Lewis acid than $Mg^{2+}$. Conversely,$Mg^{2+}$ is a weaker Lewis acid than $Al^{3+}$.

$Mg^{2+}$ is . . . . . . than $Al^{3+}$.

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