Need help ly, due tomorrow

[needhelpperson]

Need help urgently, due tomorrow...

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 metal oxides are polar and nonmetal oxides are nonpolar, and i can explain it using those definitions. But I have no idea how to explain this using ionization energy. This is due tomorrow. Please help

 

[chem_tr]

I think it is too late now, but if there is similar homeworks in the future, you can use this analogy.

The primary ionization energies (1IE) of metal ions are very low, whereas it is very high in ametals, as you know. When a metal oxide (say, sodium oxide) is reacted with water, the following reaction is likely to occur:

$$Na_2O + H_2O \rightarrow 2~Na^+ + OH^-$$

An ametal oxide (for example, As₂O₃) gives arsenite acid:
$$As_2O_3 + H_2O \rightarrow 2~HAsO_2$$

Here, as sodium has a low 1IE, it can easily form a cation to allow the remaining as an anion. Therefore, Na⁺ needs OH^-.

But arsenic(III) oxide forms an anion due to inefficient 1IE, so a complex [AsO₂]^- will be formed, with accompanying H⁺.

Regards

 

[ravenprp]

!Hello,

I can definitely understand your urgency in needing help with this question. Let me try to explain the connection between the contrasting behavior of metal and nonmetal oxides and ionization energies.

First, let's briefly define ionization energy. Ionization energy is the energy required to remove an electron from a neutral atom or molecule. This process results in the formation of a positively charged ion.

Now, let's look at the behavior of metal and nonmetal oxides. Metal oxides, such as sodium oxide (Na2O) or magnesium oxide (MgO), are formed when a metal reacts with oxygen. These oxides are polar in nature, meaning they have a slight positive and negative charge on opposite ends of the molecule. This polarity is due to the difference in electronegativity between the metal and oxygen atoms. In this case, the metal has a lower electronegativity than oxygen, causing it to have a slight positive charge.

On the other hand, nonmetal oxides, such as carbon dioxide (CO2) or sulfur dioxide (SO2), are formed when a nonmetal reacts with oxygen. These oxides are nonpolar in nature, meaning they have no overall charge. This is because the electronegativity of the nonmetal is similar to that of oxygen, resulting in a symmetrical distribution of electrons in the molecule.

Now, let's consider the ionization energies of these elements. Metals have lower ionization energies compared to nonmetals. This means that it takes less energy to remove an electron from a metal atom compared to a nonmetal atom. This is because metals have fewer electrons in their outermost energy level, making it easier for them to lose an electron and form a positively charged ion. Nonmetals, on the other hand, have higher ionization energies because they have more electrons in their outermost energy level, making it more difficult for them to lose an electron and form a positively charged ion.

Bringing this all together, we can see that the contrasting behavior of metal and nonmetal oxides is connected to their ionization energies. Metal oxides, being polar in nature, have a higher tendency to form positively charged ions due to their lower ionization energies. Nonmetal oxides, being nonpolar in nature, have a lower tendency to form positively charged ions due to their higher ionization energies.

I hope this explanation helps you understand the connection between these concepts. If you have any further questions,