Answer:
Magnesium oxide has stronger ionic attraction
Explanation:
Ionic attraction force (F) is represented as-
[tex]F=k\frac{\mid q_{+}q_{-}\mid }{(r_{+}+r_{-})^{2}}[/tex]
where k is constant, [tex]q_{+}[/tex] is charge on cation, [tex]q_{-}[/tex] is charge on anion, [tex]r_{+}[/tex] is radius of cation and [tex]r_{-}[/tex] is radius of anion.
Here anion for both oxides is [tex]O^{2-}[/tex]. So, for both of them [tex]r_{-}[/tex] is same.
For lithium oxide [tex](Li_{2}O)[/tex], cation is [tex]Li^{+}[/tex]. So, [tex]q_{+}[/tex] is +1.
For magnesium oxide (MgO), cation is [tex]Mg^{2+}[/tex]. So [tex]q_{+}[/tex] is +2
Hence [tex]\mid q_{+}q_{-}\mid (Li_{2}O)< \mid q_{+}q_{-}\mid (MgO)[/tex].
As, radius of lithium ion is greater than radius of magnesium ion therefore-
[tex](r_{+}+r_{-})(Li_{2}O)> (r_{+}+r_{-})(MgO)[/tex]
So altogether [tex]F(MgO)> F(Li_{2}O)[/tex]
