Question

What are the products formed in the reaction of xenon hexafluoride with silicon dioxide? (a) \(\mathrm{XeO}_{3}+\mathrm{SiF}_{2}\) (d) \(\mathrm{XeF}_{2}+\mathrm{SiF}_{4}\) (b) \(\mathrm{XeOF}_{4}+\mathrm{SiF}_{4}\) (c) \(\mathrm{XeSiO}_{4}+\mathrm{HF}\)

Short answer

The products formed are XeOF$_4$ and SiF$_4$ (option b).

Step-by-step solution

Identify the Reactants

The reaction involves xenon hexafluoride ( XeF$_6$) and silicon dioxide ( SiO$_2$). We need to determine what products result from these reactants.

Understand the Reaction

When xenon hexafluoride reacts with silicon dioxide, a rearrangement and exchange of fluorine and oxygen atoms occur. Normally, such reactions form interhalogen compounds.

Analyze Possible Product Combinations

Considering the typical behavior of xenon compounds, XeF$_6$ often converts to xenon oxide or other less fluorinated forms with additional compounds. Look at the product list to find the feasible combinations based on known chemistry.

Match the Correct Products

Review the given options: **a)** XeO$_3$ + SiF$_2$ **b)** XeOF$_4$ + SiF$_4$ **c)** XeSiO$_4$ + HF **d)** XeF$_2$ + SiF$_4$. Considering the typical conversion of XeF$_6$, the option with four fluorine atoms on the silicon and xenon is viable.

Finalize the Reaction Products

The combination that matches the expected behavior is: **b),** forming xenon oxyfluoride ( XeOF$_4$) and silicon tetrafluoride ( SiF$_4$). This is consistent with the reactivity patterns of these elements.

Key concepts

Xenon Compounds

Xenon, a noble gas, is incredibly stable in its unreacted state. However, under certain conditions, it can form compounds, especially with more electronegative elements like fluorine and oxygen. Xenon compounds are unique because they show that even noble gases can participate in chemical reactions, challenging the previous belief that these gases were entirely inert.

Some key xenon compounds include:

• Xenon Fluorides: These compounds, such as \(\text{XeF}_2\), \(\text{XeF}_4\), and \(\text{XeF}_6\), are formed under controlled conditions. They display interesting chemistry due to their strong fluorine bonds.
• Xenon Oxides: Compounds like \(\text{XeO}_3\) and \(\text{XeOF}_4\) highlight xenon's ability to bond with oxygen, and they further illustrate that special conditions permit noble gases to form stable compounds.

These compounds are particularly valuable in scientific research as they help us understand the potential uses and reactivity of noble gases in different situations.

Silicon Dioxide Reaction

Silicon dioxide, commonly known as silica, is a well-known compound found in sand and quartz. It is composed of one silicon atom bonded to two oxygen atoms. This structure gives it stability and a significant role in chemical reactions involving silicon.

When silicon dioxide participates in a reaction, its robust silicon-oxygen bond changes, allowing it to interact with other reactive species. In particular, when it reacts with xenon hexafluoride (\(\text{XeF}_6\)), a fascinating exchange occurs:

• The silicon in silicon dioxide can replace the oxygen as a binding partner to other elements like fluorine.
• This exchange enables the formation of compounds such as \(\text{SiF}_4\), showcasing silicon's versatility in forming tetrafluoride with additional elements.

The reaction with xenon hexafluoride is especially remarkable as it highlights silicon’s ability to form highly stable products despite the presence of xenon's strong fluorine attraction.

Xenon Hexafluoride Chemistry

Xenon hexafluoride (\(\text{XeF}_6\)) is one of the well-studied fluorides of xenon. It is a powerful fluorinating agent due to its high oxidation state and the strong electronegativity of fluorine atoms.

In chemical reactions, \(\text{XeF}_6\) is reactive enough to fluorinate a range of compounds and alter their structure. When reacted with silicon dioxide:

• \(\text{XeF}_6\) rearranges and bonds with oxygen to form xenon oxyfluoride (\(\text{XeOF}_4\)), a less fluorinated and more stable product.
• Simultaneously, \(\text{SiO}_2\) transforms to silicon tetrafluoride (\(\text{SiF}_4\)), as noted in the original exercise's solution.

This veracity of reaction showcases the unique chemistry involved when a noble gas compound like xenon hexafluoride engages with other compounds, leading to fascinating interactions and resulting in useful products such as xenon oxyfluorides and silicon fluorides.