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Chapter 7: Problem 99

The first ionization energy of the oxygen molecule is the energy required for the following process: $$ \mathrm{O}_{2}(g) \longrightarrow \mathrm{O}_{2}^{+}(g)+\mathrm{e}^{-} $$ The energy needed for this process is \(1175 \mathrm{~kJ} / \mathrm{mol}\), very similar to the first ionization energy of Xe. Would you expect \(\mathrm{O}_{2}\) to react with \(\mathrm{F}_{2}\) ? If so, suggest a product or products of this reaction.

Short Answer

Expert verified
Yes, we would expect \(\mathrm{O}_{2}\) to react with \(\mathrm{F}_{2}\) due to their high reactivity, similar ionization energies, and energetically favorable nature of potential products. The likely product of this reaction is oxygen difluoride (OF₂).

Step by step solution

01

Examine the reactivity of oxygen and fluorine

Oxygen (O₂) and fluorine (F₂) are both highly reactive elements. Oxygen tends to easily form covalent bonds with other elements, while fluorine is the most electronegative element and has a strong tendency to attract and gain electrons. This reactivity suggests that they might have the potential to react with each other.
02

Analyze the ionization energy

The ionization energy given for the oxygen molecule is \(1175 \mathrm{~kJ/mol}\), which is quite similar to the ionization energy of xenon (Xe). This means that removing an electron from an oxygen molecule requires approximately the same amount of energy as removing an electron from a xenon atom. Since reactions generally proceed when there is a decrease in energy, it is important to consider whether the reactions between \(O_2\) and \(F_2\) would lead to a net decrease in energy.
03

Examine the potential products

Based on the reactivity of oxygen and fluorine, one possible reaction between \(O_2\) and \(F_2\) would be the formation of a compound where fluorine gains an electron from oxygen, resulting in a compound like OF₂ (oxygen difluoride). \(O_2 + F_2 \longrightarrow 2\: OF\) The energetics of this reaction are favorable because the highly electronegative fluorine atoms have a strong affinity for electrons, and gaining electrons is an energy-releasing process. Thus, the energy released when fluorine gains an electron compensates the ionization energy required to remove an electron from oxygen, and the reaction proceeds spontaneously.
04

Conclusion

Given that oxygen and fluorine are both highly reactive, the similarities in their ionization energies, and the energetically favorable nature of the potential products, we would expect them to react. The likely product of this reaction is oxygen difluoride (OF₂).

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Most popular questions from this chapter

What is the relationship between the ionization energy of an anion with a 1 - charge such as \(\mathrm{F}^{-}\) and the electron affinity of the neutral atom, F?

Some metal oxides, such as \(\mathrm{Sc}_{2} \mathrm{O}_{3},\) do not react with pure water, but they do react when the solution becomes either acidic or basic. Do you expect \(\mathrm{Sc}_{2} \mathrm{O}_{3}\) to react when the solution becomes acidic or when it becomes basic? Write a balanced chemical equation to support your answer.

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Use electron configurations to explain the following observations: (a) The first ionization energy of phosphorus is greater than that of sulfur. (b) The electron affinity of nitrogen is lower (less negative) than those of both carbon and oxygen. (c) The second ionization energy of oxygen is greater than the first ionization energy of fluorine. (d) The third ionization energy of manganese is greater than those of both chromium and iron.

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