Ionization Energy: Explain Metal-Nonmetal Oxide Reactions

[needhelpperson]

When metal oxides react with water, the oxygen generally ends up as the hydroxide ion, separate from the metal. In contrast, when nonmetallic oxides react with water, the oxygen ends up as part of the nonmetals species. What connection is there between this contrasting behaviour of metal and nonmetal oxides and ionization energies?

I know that the metal oxides dissociate because they are their bonds are polar, since ionic. As well the nonmetal oxides are not polar which is why they do not dissociate. But I am wondering how can i use ionization energy to explain this? please help

 

[Nate810]

The difference in the behavior of metal and nonmetal oxides when they react with water is due to the differing electronegativities of the elements involved. Metal oxides contain metals that have relatively low ionization energies, meaning it is easier for them to lose electrons and form positive ions. Nonmetallic oxides contain elements that have higher ionization energies, making it much more difficult for them to lose electrons. The metals in metal oxides are therefore more likely to dissociate and form ions in aqueous solutions, while the nonmetals in nonmetal oxides are more likely to remain intact and form molecules when they react with water.

 

[M98Ranger]

Ionization energy is the energy required to remove an electron from an atom or ion in the gas phase. In the case of metal oxides, the metal atoms have low ionization energies, which means they are easily able to lose electrons and form positive ions. This is why the oxygen in metal oxides ends up as a separate hydroxide ion, as the metal ion is more stable in this form.

On the other hand, nonmetal oxides have high ionization energies, meaning they are less likely to lose electrons and form positive ions. This is why the oxygen in nonmetal oxides remains in the nonmetal species, as it is more stable in this form. The high ionization energy of nonmetals also explains why they do not dissociate in water, as the energy required to remove an electron is not readily available in the aqueous environment.

In summary, the contrasting behavior of metal and nonmetal oxides in reactions with water can be attributed to their different ionization energies. Metals have lower ionization energies and therefore are more likely to form positive ions, while nonmetals have higher ionization energies and are less likely to form positive ions. This helps to explain why metal oxides dissociate and nonmetal oxides do not in these reactions.