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Chapter 22: Problem 29

Why does xenon form stable compounds with fluorine, whereas argon does not?

Short Answer

Expert verified
Xenon forms stable compounds with fluorine due to its lower ionization energy and significant difference in electronegativity compared to argon. This allows for the formation of a chemical bond between the two elements. In contrast, argon does not form compounds with fluorine because of its higher ionization energy and similar electronegativity value, which makes it difficult for a bond to form between them.

Step by step solution

01

Verify Electronic Configurations

For Xenon (Xe) and Argon (Ar), we need to find their electronic configurations. Xe is in period 5 and group 18, while Ar is in period 3 and group 18. Their electronic configurations are: Xe: \[1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6\] Ar: \[1s^2 2s^2 2p^6 3s^2 3p^6\]
02

Understand Ionization Energy and Electronegativity

The ionization energy of an atom is the energy required to remove an electron from the outermost shell. The electronegativity of an atom is its tendency to attract a bonding pair of electrons. Generally, elements that have lower ionization energy and higher electronegativity tend to form compounds more easily.
03

Compare Ionization Energies and Electronegativity

Xenon has a lower ionization energy than argon. This means that it is easier to remove an electron from xenon than from argon. The electronegativity values for fluorine, xenon, and argon are 3.98, 2.6, and 3.24, respectively. Fluorine being highly electronegative, it can attract electrons from xenon, which has a relatively lower ionization energy. In contrast, argon has a higher ionization energy and its electronegativity value is closer to fluorine. As a result, argon does not readily lose electrons to form a bond with fluorine.
04

Relate Ionization Energy and Electronegativity to the Formation of Chemical Bonds

The difference in ionization energy and electronegativity between xenon and fluorine allows for the transfer of electrons between the two elements, which leads to the formation of the compound. On the other hand, the similar ionization energies and electronegativity values for argon and fluorine prevent the formation of a chemical bond between them.
05

Conclusion

Xenon forms stable compounds with fluorine because it has a lower ionization energy and a significant difference in electronegativity compared to argon. This allows for the formation of a chemical bond between the two elements. Argon does not form compounds with fluorine because of its higher ionization energy and similar electronegativity value, making it difficult for the elements to form a bond.

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Most popular questions from this chapter

Write a balanced equation for each of the following reactions: (a) Hydrogen cyanide is formed commercially by passing a mixture of methane, ammonia, and air over catalyst at \(800^{\circ} \mathrm{C} .\) Water is a by-product of the reaction. (b) Baking soda reacts with acids to produce carbon dioxide gas. (c) When barium carbonate reacts in air with sulfur dioxide, barium sulfate and carbon dioxide form.

Write a balanced net ionic equation for each of the following reactions: (a) Dilute nitric acid reacts with zinc metal with formation of nitrous oxide. (b) Concentrated nitric acid reacts with sulfur with formation of nitrogen dioxide. (c) Concentrated nitric acid oxidizes sulfur dioxide with formation of nitric oxide. (d) Hydrazine is burned in excess fluorine gas, forming \(\mathrm{NF}_{3}\) . (e) Hydrazine reduces \(\mathrm{CrO}_{4}^{2-}\) to \(\mathrm{Cr}(\mathrm{OH})_{4}^{-}\) in base (hydrazine is oxidized to \(\mathrm{N}_{2} )\) .

Complete and balance the following equations:$$ \begin{array}{l}{\text { (a) } \mathrm{ZnCO}_{3}(s) \stackrel{\Delta}{\longrightarrow}} \\ {\text { (b) } \mathrm{BaC}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow} \\ {\text { (c) } \mathrm{C}_{2} \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow}\end{array} $$ $$\begin{array}{l}{\text { (c) ~ } \mathrm{CS}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow} \\ {\text { (e) } \mathrm{Ca}(\mathrm{CN})_{2}(s)+\mathrm{HBr}(a q) \longrightarrow}\end{array}$$

Write the Lewis structure for each of the following species, describe its geometry, and indicate the oxidation state of the nitrogen: (a) HNO \(_{2},(\mathbf{b}) \mathrm{N}_{3},(\mathbf{c}) \mathrm{N}_{2} \mathrm{H}_{5}^{+},(\mathbf{d}) \mathrm{NO}_{3}^{-} .\)

Although the \(\mathrm{ClO}_{4}^{-}\) and \(\mathrm{IO}_{4}^{-}\) ions have been known for a long time, \(\mathrm{BrO}_{4}^{-}\) was not synthesized until \(1965 .\) The ion was synthesized by oxidizing the bromate ion with xenon difluoride, producing xenon, hydrofluoric acid, and the perbromate ion. (a) Write the balanced equation for this reaction. (b) What are the oxidation states of Br in the Br-containing species in this reaction?
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