Question

Write complete balanced equation for the preparation of the following compounds: (a) \(\mathrm{XeO}_{3}\) (b) \(\mathrm{XeO}_{4}\) (c) \(\mathrm{XeOF}_{2}\)

Short answer

The balanced equations for the creation of the compounds are: a) \(\mathrm{2Xe} + \mathrm{3O}_2 \rightarrow \mathrm{2XeO}_{3}\)b) \(\mathrm{XeO}_{3} + \mathrm{O}_2 \rightarrow \mathrm{XeO}_{4}\)c) \(\mathrm{Xe} + \mathrm{O}_2 + \mathrm{2F}_{2} \rightarrow \mathrm{XeOF}_{2}\)

Step-by-step solution

- Preparing \(\mathrm{XeO}_{3}\)

Xenon trioxide (\(\mathrm{XeO}_{3}\)) can be prepared from xenon and oxygen. The balanced equation describing this reaction is: \[ \mathrm{2Xe} + \mathrm{3O}_2 \rightarrow \mathrm{2XeO}_{3} \]

- Preparing \(\mathrm{XeO}_{4}\)

Xenon tetroxide (\(\mathrm{XeO}_{4}\)) can be prepared from Xenon trioxide (\(\mathrm{XeO}_{3}\)) and Oxygen. The balanced equation for this reaction is: \[ \mathrm{XeO}_{3} + \mathrm{O}_2 \rightarrow \mathrm{XeO}_{4}\]

- Preparing \(\mathrm{XeOF}_{2}\)

Xenon oxydifluoride (\(\mathrm{XeOF}_{2}\)) can be prepared from xenon, oxygen, and fluorine. The balanced equation is: \[ \mathrm{Xe} + \mathrm{O}_2 + \mathrm{2F}_{2} \rightarrow \mathrm{XeOF}_{2}\]

Key concepts

Balanced Chemical Equations

Chemical reactions are processes that transform one set of chemical substances into another. To accurately convey the reactants and products involved, as well as their proportions, scientists use balanced chemical equations. These are written representations of chemical reactions, demonstrating that matter is conserved, conforming to the Law of Conservation of Mass. This law states that in a closed system, matter cannot be created or destroyed.

To write a balanced equation, one must ensure the same number of each type of atom appears on both sides of the reaction arrow. For example, the balanced equation for producing xenon trioxide from xenon and oxygen is \(2\text{Xe} + 3\text{O}_2 \rightarrow 2\text{XeO}_3\). Notice that there are two xenon atoms and six oxygen atoms on both sides of the equation, demonstrating balance. Mastering the skill of balancing equations is crucial for understanding chemical reactions and is a foundational aspect of chemistry study.

Xenon Trioxide (XeO3)

Xenon trioxide, represented chemically as \(\mathrm{XeO}_{3}\), is an intriguing compound notable for its explosive properties and is used in studying the chemistry of noble gases. The preparation of \(\mathrm{XeO}_{3}\) involves a direct reaction between xenon and oxygen. In the laboratory, it can be formed by the hydrolysis of \(\mathrm{XeF}_{6}\), illustrating the versatility of xenon chemistry.

The mencioned balanced equation for the synthesis of xenon trioxide is simple: \(2\text{Xe} + 3\text{O}_2 \rightarrow 2\text{XeO}_3\). What is particularly interesting about this compound is its molecular structure and the ability of xenon, a so-called 'inert' gas, to form such a stable oxide. This discovery was part of a series of findings that expanded the understanding of the chemical reactivity of noble gases.

Xenon Tetroxide (XeO4)

Xenon tetroxide (\(\mathrm{XeO}_{4}\)) is another example of how xenon defies its 'inert' label by forming diverse compounds. This compound is notable for its highly oxidizing nature and instability at room temperature, decomposing explosively upon contact with organic material. The production of \(\mathrm{XeO}_{4}\) involves oxidizing \(\mathrm{XeO}_{3}\) with additional oxygen, as shown in the balanced reaction \(\mathrm{XeO}_{3} + \mathrm{O}_2 \rightarrow \mathrm{XeO}_{4}\).

Its synthesis is not only of academic interest but also contributes to the understanding of the noble gas element group's potential for forming multiple oxidation states. Considering its explosive nature, \(\mathrm{XeO}_{4}\) is often studied under controlled conditions and is not typically encountered outside of specialized research laboratories.

Xenon Oxydifluoride (XeOF2)

Complementing the already fascinating field of xenon chemistry is xenon oxydifluoride (\(\mathrm{XeOF}_{2}\)), a compound that showcases the element's ability to form stable bonds with both oxygen and fluorine. The preparation of \(\mathrm{XeOF}_{2}\) involves reacting xenon with oxygen and fluorine, as described by the balanced chemical equation: \(\mathrm{Xe} + \mathrm{O}_2 + 2\mathrm{F}_{2} \rightarrow \mathrm{XeOF}_{2}\).

Chemists are intrigued by this compound due to its unusual molecular geometry and the fact that it is one of the few known compounds where xenon directly bonds with oxygen. In research applications, \(\mathrm{XeOF}_{2}\) serves as a starting point for synthesizing other xenon compounds and is used in studies exploring the reactivity and bonding of noble gases.