Noble Gas Compounds - Online Tutor, Practice Problems & Exam Prep

Xenon, a noble gas, uniquely forms stable compounds among the group 8 elements, primarily reacting with fluorine. This reaction produces various xenon fluoride compounds, denoted as XeF_n, where n can be 1, 2, 3, or up to 6. The resulting compounds include xenon difluoride (XeF₂), xenon tetrafluoride (XeF₄), and xenon hexafluoride (XeF₆), showcasing xenon's ability to bond with multiple fluorine atoms, which is significant in understanding noble gas chemistry.

Noble Gas Compounds

When it comes to noble gas compounds, among all Group 88 elements, only xenon forms stable compounds. We're going to say it reacts directly with fluorine and it forms fluorides.

Now if we take a look here, we have xenon as a gas. It's a noble gas and it reacts with some set number of fluorine gas molecules. Here N can represent 1-2 or three and it produces xenon with some set number of fluorine atoms connected to it.

X here could represent 2-4 or six. So just remember xenon is an old gas that we focus on. It reacts directly with fluorine and it creates different types of xenon fluoride compounds with two fluorines, 4 fluorines or even up to six fluorines.

Noble Gas Compounds Example

In this example it says a double gas fluoride is a colorless crystalline solid at room temperature. Which one of the following is the most likely formula of this compound?

So here it's a fluoride. All these examples are fluorides. It exists as a crystalline solid at room temperature, which indicates it's pretty stable. And we know that out of all the noble gases, it's xenon that helps to make stable compounds, and it makes stable compounds with fluorine.

If we take a look, the only option that possesses xenon in the formula is option D. Here we have xenon tetrafluoride as this stable colorless crystalline solid found at room temperature.

Which of the following xenon compounds are too unstable to exist?

• A. XeF₂
• B. XeI₄
• C. XeF₄
• D. XeF₆

Here’s what students ask on this topic:

What are the stable compounds formed by xenon with fluorine?

Xenon forms stable compounds with fluorine, known as xenon fluorides. The primary xenon fluorides are XeF₂, XeF₄, and XeF₆. These compounds are formed when xenon reacts directly with fluorine gas. The number of fluorine atoms bonded to xenon can vary, resulting in different types of xenon fluoride compounds. XeF₂ has two fluorine atoms, XeF₄ has four fluorine atoms, and XeF₆ has six fluorine atoms bonded to xenon.

Why is xenon unique among noble gases in forming stable compounds?

Xenon is unique among noble gases in forming stable compounds because it has a relatively large atomic size and low ionization energy compared to other noble gases. This allows xenon to participate in chemical reactions, particularly with highly electronegative elements like fluorine. The ability of xenon to form stable compounds is due to its ability to expand its valence shell and accommodate more electrons, leading to the formation of xenon fluorides such as XeF₂, XeF₄, and XeF₆.

How does xenon react with fluorine to form xenon fluorides?

Xenon reacts with fluorine gas through a direct reaction to form xenon fluorides. The reaction can be represented by the general equation:

${\mathrm{Xe}}_{}+n_{}{F}_2\to {\mathrm{XeF}}_{x_{}}$

where n can be 1, 2, or 3, and x can be 2, 4, or 6. For example, when xenon reacts with one molecule of fluorine gas, it forms XeF₂. When it reacts with two molecules of fluorine gas, it forms XeF₄, and with three molecules of fluorine gas, it forms XeF₆.

What are the possible oxidation states of xenon in its compounds with fluorine?

In its compounds with fluorine, xenon can exhibit several oxidation states. The most common oxidation states of xenon in xenon fluorides are +2, +4, and +6. These correspond to the compounds XeF₂ (xenon in +2 oxidation state), XeF₄ (xenon in +4 oxidation state), and XeF₆ (xenon in +6 oxidation state). The ability of xenon to exhibit multiple oxidation states is due to its relatively low ionization energy and the high electronegativity of fluorine, which allows xenon to form stable bonds with varying numbers of fluorine atoms.

What is the significance of xenon fluorides in chemistry?

Xenon fluorides are significant in chemistry because they challenge the traditional view that noble gases are completely inert and do not form compounds. The discovery of xenon fluorides demonstrated that under certain conditions, even noble gases can participate in chemical reactions. This has expanded our understanding of chemical bonding and reactivity. Additionally, xenon fluorides have practical applications in areas such as fluorination reactions, where they serve as powerful fluorinating agents, and in the study of noble gas chemistry, providing insights into the behavior of other noble gases under extreme conditions.