Question

\(\mathrm{XeF}_{4}\) and \(\mathrm{XeF}_{6}\) are expected to be (a) reducing (b) oxidizing (c) unreactive (d) strongly basic

Short answer

(b) oxidizing

Step-by-step solution

Understanding the Oxidation States

Xenon (Xe) is a noble gas, typically exhibiting oxidation states of 0, +2, +4, +6, and +8. In \(\mathrm{XeF}_4\), xenon is in the +4 oxidation state, and in \(\mathrm{XeF}_6\), xenon is in the +6 oxidation state. Given that xenon atoms can form compounds, they generally act as oxidizing agents by accepting electrons to revert to lower oxidation states.

Analyzing the Chemical Properties

Xenon tetrafluoride (\(\mathrm{XeF}_4\)) and xenon hexafluoride (\(\mathrm{XeF}_6\)) both act as powerful oxidizing agents. Xe is capable of being reduced as it can convert from higher oxidation states (+4 or +6) to lower ones by accepting electrons. Elements with high oxidation states tend to be good oxidizing agents.

Excluding Unlikely Options

These compounds are not basic in nature, as they do not donate hydroxide ions or form hydroxide ions in solution. Neither are they stable or inert enough to be considered unreactive. They are generally not reducing agents, because reducing agents typically lose electrons, whereas xenon's role in these compounds involves gaining electrons.

Conclusion

\(\mathrm{XeF}_4\) and \(\mathrm{XeF}_6\) are best classified as oxidizing agents due to their ability to accept electrons and reduce to lower oxidation states. This is consistent with xenon's role in forming higher oxidation state fluorides that act as oxidizing agents.

Key concepts

Xenon Compounds

Xenon, a member of the noble gases, is an intriguing element that was once thought to be completely inert and unable to form compounds. However, the landscape of chemistry changed dramatically with the discovery of xenon compounds such as xenon tetrafluoride (\(\mathrm{XeF}_4\)) and xenon hexafluoride (\(\mathrm{XeF}_6\)). These compounds are known for their unique chemical properties. Xenon's capability to form compounds is due to its ability to exist in multiple oxidation states, differentiating it from its fellow noble gases.
- **Xenon Tetrafluoride (\(\mathrm{XeF}_4\)):** In this compound, xenon is bonded to four fluorine atoms and exists in the +4 oxidation state. It is a colorless crystalline solid under standard conditions and is also known for being a strong oxidizing agent.- **Xenon Hexafluoride (\(\mathrm{XeF}_6\)):** Here, xenon is bonded to six fluorine atoms, putting it in the +6 oxidation state. This compound is less stable than \(\mathrm{XeF}_4\) and is characterized by its ability to interact strongly with other substances, often oxidizing them.The existence of these compounds highlights that noble gases can indeed form stable, chemical compounds under the right conditions. This discovery expanded our understanding of chemical bonding and reactivity.

Oxidation States

Understanding oxidation states is essential for studying the behavior of elements in chemical reactions. For xenon, a noble gas, oxidation states indicate its capacity to combine with other elements by sharing or transferring electrons.
- **Definition:** The oxidation state, or oxidation number, of an atom is a hypothetical charge that an atom would have if all bonds to atoms of different elements were fully ionic. It helps in understanding the nature and strength of the chemical bonds between atoms.- **Oxidation States of Xenon:** Xenon typically exhibits oxidation states of 0, +2, +4, +6, and +8. In its compounds, the higher the oxidation state, the more likely xenon is serving as an oxidizing agent. For instance, in \(\mathrm{XeF}_4\), xenon is in the +4 state, and in \(\mathrm{XeF}_6\), it is in the +6 state.This inclination to occupy higher oxidation states allows xenon to stabilize itself by gaining electrons, thus acting as an oxidizing agent. Such a process is integral to redox reactions, where the oxidation state of substances is altered as they accept or donate electrons.

Noble Gases Chemistry

Noble gases are known for their lack of reactivity, a characteristic that largely stems from their complete valence electron shells. However, xenon breaks this stereotype by actively participating in chemical reactions, particularly forming compounds with other elements.
- **Traditional View:** Noble gases, such as helium, neon, and argon, are typically characterized by their lack of chemical reactivity due to having full valence electron shells. This stability makes them rarely participate in chemical bonding under standard conditions. - **Xenon's Role:** Unlike other noble gases, xenon can form a variety of compounds due to its ability to access higher energy levels for bonding with more electronegative elements, such as fluorine. The reactivity of xenon has allowed chemists to rethink the rigidity of the noble gas group in the periodic table. It offers insights into how under specific circumstances, even the most inert elements can participate in complex reactions, broadening our comprehension of chemical reactivity and bonding. Xenon's ability to form stable compounds, albeit under specific conditions, points to the diversity and potential of noble gas chemistry.