Question

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 \(\mathrm{Xe}\). Would you expect \(\mathrm{O}_{2}\) to react with \(\mathrm{F}_{2}\) ? If so, suggest a product or products of this reaction.

Short answer

Yes, O2 will react with F2, and the product of the reaction would be oxygen difluoride (OF2).

Step-by-step solution

Comparing Ionization Energies

First, we need to compare the ionization energies of the oxygen molecule and the noble gas (Xe) given in the exercise. The ionization energy for the oxygen molecule is \(1175kJ/mol\), which is very similar to the ionization energy of Xenon (Xe). Noble gases like Xe are known to be relatively inert or non-reactive due to their full electron shells.

Determine Reactivity of Oxygen

Oxygen (O2) is generally a very reactive element due to its electronegativity, which is the tendency of an atom to attract electrons towards itself. Since the ionization energy of O2 is similar to that of Xe, this indicates that O2 might be less reactive than typically thought in this case.

Analyze Reactivity with Fluorine

Fluorine (F2) is the most reactive non-metal and has the highest electronegativity of all elements. It tends to form strong bonds with other elements due to its ability to attract electrons towards itself. The reactivity of fluorine would certainly influence the reaction with oxygen.

Determine Possible Reaction and Products

Taking into account that oxygen might be less reactive than typically thought in this case, and considering fluorine's high reactivity, it is plausible that a reaction between O2 and F2 might occur. When oxygen reacts with fluorine, the expected product will be a fluoride compound. In this case, with O2 and F2, the product formed would be oxygen difluoride (OF2). So, the answer to the question if O2 would react with F2 is yes, and the product of the reaction would be oxygen difluoride (OF2).

Key concepts

Ionization Energy of Oxygen

Ionization energy is a fundamental concept in chemistry that refers to the energy required to remove an electron from an atom or molecule. For oxygen, a molecule with the formula O2, this energy is measured at 1175 kJ/mol, which is quite significant. This reflects the stability and reluctance of the oxygen molecule to give up an electron.

Given that oxygen often forms compounds by sharing electrons rather than losing them, the high ionization energy underscores its preference for covalent bonding. Typically, high ionization energy is associated with noble gases such as Xenon (Xe); however, the fact that oxygen's ionization energy is close to that of Xe gives us an interesting perspective.

The resemblance suggests that under certain conditions, oxygen can exhibit less reactivity similarly to the noble gases, which are known for their inert nature due to their filled electron shells. This nuance in oxygen's chemical behavior plays a crucial role when considering its reactivity with other elements, such as fluorine in the formation of compounds like oxygen difluoride (OF2).

Chemical Reactivity

Chemical reactivity refers to the likelihood of a substance to engage in a chemical reaction. For elements like fluorine (F2), this propensity is incredibly high, largely due to its high electronegativity. This means that fluorine aggressively attracts electrons to form bonds.

Oxygen, on the other hand, is also highly reactive, not because it seeks electrons as greedily as fluorine, but because it readily forms covalent bonds by sharing electrons. This characteristic leads to the widespread presence of oxygen in a variety of compounds. The ionization energy can influence reactivity; a higher ionization energy can indicate a lower reactivity as it suggests a resistance to losing electrons. However, in the case of oxygen, its chemical reactivity must be considered in the context of its preferred bonding scenarios and the substances it interacts with.

For instance, when oxygen interacts with high-electronegativity elements like fluorine, the outcome can be different from the expected trends. Oxygen, although less reactive than fluorine, can still form stable compounds through covalent bonding, which leads us to the discussion of oxygen difluoride formation.

Oxygen Difluoride Formation

The formation of oxygen difluoride (OF2) results from the reaction between oxygen (O2) and fluorine (F2). Despite oxygen's high ionization energy, which hints at a lower reactivity, the exceptional reactivity of fluorine allows it to overcome this barrier, facilitating the formation of OF2. This compound is an example of the chemical reactivity between two highly electronegative elements.

Oxygen difluoride showcases the unique chemical behaviors that occur under specific conditions, such as the presence of highly reactive fluorine. During this reaction, each oxygen atom shares one electron with the fluorine atoms, resulting in a covalent bond.

This understanding aligns with the clarification provided in the exercise solution, reinforcing the concept that while oxygen has a high ionization energy resembling that of noble gases, it can indeed react with fluorine to form oxygen difluoride. This formation exemplifies the complexity of chemical reactivity, where multiple factors such as ionization energy, electron sharing, and electronegativity interplay to determine the products of a reaction.