Question

Although they were formerly called the inert gases, the heavier elements of Group 8 do form relatively stable compounds. For example, at high temperatures in the presence of an appropriate catalyst, xenon gas will combine directly with fluorine gas to produce solid xenon tetrafluoride. Write the unbalanced chemical equation for this process.

Short answer

The unbalanced chemical equation for the reaction between xenon gas and fluorine gas to produce solid xenon tetrafluoride is: \(Xe + F_2 \rightarrow XeF_4\)

Step-by-step solution

Identify the chemical formula of each reactant and product

For this process, we need to know the chemical formulas of the reactants and product: - Xenon gas (Xe): Xenon is a noble gas and exists as a monoatomic molecule. - Fluorine gas (F2): As a diatomic molecule, Fluorine exists as F2. - Xenon tetrafluoride (XeF4): The compound XeF4 is made of one Xenon atom and four Fluorine atoms.

Write the unbalanced chemical equation

Now, we can write the unbalanced chemical equation using the chemical formulas of the reactants and product: Xe + F2 → XeF4 This unbalanced equation represents the reaction between xenon gas and fluorine gas to produce solid xenon tetrafluoride.

Key concepts

Xenon Tetrafluoride

Xenon tetrafluoride, represented by the chemical formula XeF4, is a fascinating compound that serves as an example of the chemical reactivity of noble gases. Contrary to what their group name might imply, not all noble gases are completely 'inert' or unreactive. Xenon, a heavy noble gas, can form stable compounds, such as xenon tetrafluoride, under certain conditions.

This compound is created when xenon gas reacts with fluorine gas under the influence of a catalyst at high temperatures. The structure of xenon tetrafluoride is particularly interesting due to its square planar geometry, which is a result of the arrangement of the four fluorine atoms around the xenon atom, adhering to the principles of VSEPR theory.

Understanding the properties of xenon tetrafluoride can shed light on the molecular geometry and reactivity of noble gases, challenging the earlier perception that they cannot form compounds. Such compounds are not only significant in theoretical chemistry but also have practical applications in areas such as nuclear fuel processing and as strong oxidizing agents.

Chemical Formula

Chemical formulas are a shorthand method of representing the elements in a compound and the ratios in which they combine. For instance, the chemical formula of xenon tetrafluoride, XeF4, tells us that each molecule consists of one atom of xenon and four atoms of fluorine. The subscript '4' after the symbol for fluorine indicates there are four fluorine atoms bonded to the lone xenon atom in the compound.

The process of writing chemical formulas involves understanding the valency and combining capacity of the involved atoms. In the case of xenon tetrafluoride, the xenon atom utilizes eight of its electrons to form a stable octet with four fluorine atoms, which is depicted accurately in its chemical formula. This ability to quickly gauge the composition of compounds from their chemical formula is a foundational skill in chemistry, aiding in balancing chemical equations, understanding molecular structures, and predicting reaction outcomes.

Noble Gases

Noble gases, the elements occupying Group 18 in the periodic table, include helium, neon, argon, krypton, xenon, and the radioactive radon. These gases were originally termed 'inert gases' due to their reluctance to react with other elements. This lack of reactivity is primarily due to their full valence electron shell, which provides great stability and no tendency to gain or lose electrons.

However, this notion has been revised with the discovery of noble gas compounds. Xenon and krypton, due to their larger atomic sizes and lower ionization energies compared to other noble gases, can still participate in chemical reactions under specific conditions. The formation of xenon compounds, such as xenon tetrafluoride, is a remarkable example that showcases that despite a full valence shell, noble gases can react with highly electronegative elements like fluorine, leading to stable and intriguing compounds that have broadened the view on the chemical behavior of these once deemed 'inert' gases.