Problem 174 - A Complete Resource Book in Chemistry for JEE Main

Question

\(\mathrm{XeF}_{6}\) on hydrolysis gives: (a) \(\mathrm{XeO}_{2} \mathrm{~F}_{2}\) (b) \(\mathrm{XeOF}_{4}\) (c) \(\mathrm{XeO}_{4}\) (d) \(\mathrm{XeO}_{3}\)

Step-by-Step Solution

Answer

The final product of \(\mathrm{XeF}_{6}\) on hydrolysis is \(\mathrm{XeO}_{3}\).

Step 1: Understand the Reaction

To solve this problem, we need to determine what happens when xenon hexafluoride (\(\mathrm{XeF}_{6}\)) undergoes hydrolysis. Hydrolysis is a chemical process that involves interaction with water, often resulting in the breaking of bonds in the molecule.

Step 2: Determine the Interaction

\(\mathrm{XeF}_{6}\) is known to react with water (\(\mathrm{H}_{2}\mathrm{O}\)) leading initially to the formation of \(\mathrm{XeOF}_{4}\) and hydrofluoric acid (\(\mathrm{HF}\)). This partial hydrolysis can be represented by the equation: \[ \mathrm{XeF}_{6} + \mathrm{H}_{2}\mathrm{O} \rightarrow \mathrm{XeOF}_{4} + 2\mathrm{HF} \]

Step 3: Recognize Further Hydrolysis

If further hydrolysis occurs, \(\mathrm{XeOF}_{4}\) can react with more water to produce \(\mathrm{XeO}_{3}\), alongside additional \(\mathrm{HF}\). So if hydrolysis continues, the equation would be: \[ \mathrm{XeOF}_{4} + 2\mathrm{H}_{2}\mathrm{O} \rightarrow \mathrm{XeO}_{3} + 4\mathrm{HF} \]

Step 4: Identify the Final Product

Considering the complete hydrolysis, where \(\mathrm{XeF}_{6}\) is eventually converted through \(\mathrm{XeOF}_{4}\) to \(\mathrm{XeO}_{3}\), the final predominant product when \(\mathrm{XeF}_{6}\) undergoes complete hydrolysis is \(\mathrm{XeO}_{3}\).

Key Concepts

Chemical Reaction Mechanisms

Chemical reaction mechanisms are like the step-by-step instructions for how a chemical reaction occurs. They show the detailed sequence of events, such as bond-making and bond-breaking, that transform reactants into products. These mechanisms give us insights into the specific changes at the molecular level. This is crucial because it helps chemists understand why reactions happen the way they do.

The reaction of xenon hexafluoride (\(\mathrm{XeF}_{6}\)) with water involves multiple steps. Initially, \(\mathrm{XeF}_{6}\) reacts with water to form \(\mathrm{XeOF}_{4}\), releasing hydrofluoric acid (\(\mathrm{HF}\)). This partial hydrolysis is just one part of the mechanism. By diving into each step, chemists can predict and manipulate the outcome of reactions. This understanding is essential for developing new reactions and products, especially in fields like pharmaceuticals and materials science.

Knowledge of reaction mechanisms also helps in controlling reaction rates, as it shows which bonds are formed and broken, and what conditions are necessary for these transformations. For example, the mechanism for \(\mathrm{XeF}_{6}\) hydrolysis highlights the possible further interactions with water, leading to the formation of \(\mathrm{XeO}_{3}\). This is a great example of how understanding mechanisms can clarify the pathway of complicated chemical processes.

Hydrolysis Process

Hydrolysis is a process where water is used to break chemical bonds, typically resulting in the decomposition of a compound. The term literally means 'water-splitting'. In the context of xenon hexafluoride (\(\mathrm{XeF}_{6}\)), hydrolysis involves using water to break the bonds in \(\mathrm{XeF}_{6}\), transforming it into other compounds.

Initially, this process forms xenon oxyfluoride (\(\mathrm{XeOF}_{4}\)) and hydrofluoric acid (\(\mathrm{HF}\)). This is a partial hydrolysis since \(\mathrm{XeF}_{6}\) has not fully reacted with water. Partial hydrolysis can continue to advance if more water is added or if the reaction conditions encourage it — such as increased temperature or presence of a catalyst. In the case of complete hydrolysis, \(\mathrm{XeOF}_{4}\) reacts further with water to produce the end product, xenon trioxide (\(\mathrm{XeO}_{3}\)), along with more \(\mathrm{HF}\).

The importance of understanding the hydrolysis process lies in its widespread application. It's fundamental in driving reactions in organic and inorganic chemistry, impacting everything from biological systems to industrial manufacturing. In the laboratory setting, hydrolysis is often used to modify and control the chemical structure and properties of compounds.

Xenon Compounds

Xenon compounds are fascinating due to their unexpected reactivity. Xenon is a noble gas, traditionally considered inert. However, it forms stable compounds, such as xenon hexafluoride (\(\mathrm{XeF}_{6}\)), under specific conditions. These reactions challenge the idea that noble gases are entirely unreactive.

\(\mathrm{XeF}_{6}\) is one of the most reactive xenon compounds, thanks to its ability to form bonds with highly electronegative elements like fluorine. Its structure allows it to undergo reactions like hydrolysis, forming interesting products like \(\mathrm{XeOF}_{4}\) and \(\mathrm{XeO}_{3}\). These compounds provide insight into the bonding capabilities and chemical behavior of xenon.

The study of xenon compounds extends into potential applications in chemistry and industry. They offer a unique perspective on chemical bonding theories and help develop new materials. Also, these compounds are used in scientific research to explore the limits of reactivity and potential of other typically non-reactive elements.

Inorganic Chemistry Reactions

Inorganic chemistry reactions encompass transformations involving elements other than carbon, typically highlighting the role of metals, metalloids, and nonmetals. These reactions are fundamental to understanding how elements behave in various conditions and combinations. Xenon's reactions fall under this category, shedding light on its unexpected behavior as a noble gas.

Reactions like the hydrolysis of \(\mathrm{XeF}_{6}\) illustrate the diversity and complexity of inorganic chemistry. These involve interactions that typically include breaking and forming of covalent bonds and sometimes producing ions. These transformations provide insights into how elements combine to form new substances with distinct properties.

Inorganic reactions are not just limited to the lab. They have practical applications in many fields, including material science, environmental science, and even biology. Understanding these reactions enriches our knowledge of the natural world and allows for the innovation of new processes and materials beneficial to society.