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Chapter 20: Problem 77

There is evidence that radon reacts with fluorine to form compounds similar to those formed by xenon and fluorine. Predict the formulas of these \(\operatorname{Rn} \mathrm{F}_{x}\) compounds.

Short Answer

Expert verified
Based on the compounds formed between Xenon and Fluorine, we predict that Radon will form similar compounds with Fluorine, specifically \(RnF_2\), \(RnF_4\), and \(RnF_6\), with Radon having oxidation states of +2, +4, and +6, respectively.

Step by step solution

01

Identify the group numbers of Xenon (Xe) and Radon (Rn)

Both Xenon (Xe) and Radon (Rn) belong to Group 18, which is the group of noble gases. Noble gases are known for being chemically inert due to their full valence electron shells. However, Xenon and Radon can form compounds with highly electronegative elements like fluorine because of their large atomic size and relatively low ionization energies.
02

Identify the group number of Fluorine (F)

Fluorine (F) belongs to Group 17, which is the group of halogens. Halogens are one electron short of having a full valence electron shell. As a result, they have a tendency to gain one electron from other elements to complete their octet, making them highly electronegative and reactive.
03

Understand the compounds formed by Xenon (Xe) with Fluorine (F)

Xenon forms several compounds with fluorine such as XeF2, XeF4, and XeF6. These compounds are formed due to the transfer of valence electrons from Xenon to Fluorine. In these compounds, Xenon has an oxidation state of +2, +4, and +6, respectively.
04

Predict the formulas of Radon (Rn) and Fluorine (F) compounds

Since both Xenon and Radon belong to Group 18, it is likely that Radon will also form compounds with fluorine in a similar manner as Xenon. Therefore, we can predict that Radon will form compounds with fluorine such as RnF2, RnF4, and RnF6, with Radon having oxidation states of +2, +4, and +6, respectively.
05

Conclusion

Based on our understanding of the periodic table and the compounds formed between Xenon and Fluorine, we predict that Radon will form compounds similar to those formed by Xenon and Fluorine, specifically RnF2, RnF4, and RnF6. These compounds indicate that Radon has the capacity to form compounds with fluorine rather than being completely chemically inert, as is commonly associated with noble gases.

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Most popular questions from this chapter

The inert-pair effect is sometimes used to explain the tendency of heavier members of Group 3 \(\mathrm{A}\) to exhibit \(+1\) and \(+3\) oxidation states. What does the inert-pair effect reference? (Hint:Consider the valence electron configuration for Group 3 \(\mathrm{A}\) elements.)

Trisodium phosphate (TSP) is an effective grease remover. Like many cleaners, TSP acts as a base in water. Write a balanced equation to account for this basic behavior.

Write the Lewis structure for \(\mathrm{O}_{2} \mathrm{F}_{2}\) . Predict the bond angles and hybridization of the two central oxygen atoms. Assign oxidation states and formal charges to the atoms in $\mathrm{O}_{2} \mathrm{F}_{2} .\( The compound \)\mathrm{O}_{2} \mathrm{F}_{2}$ is a vigorous and potent oxidizing and fluorinating agent. Are oxidation states or formal charges more useful in accounting for these properties of $\mathrm{O}_{2} \mathrm{F}_{2} ?$

Beryllium shows some covalent characteristics in some of its compounds, unlike the other alkaline earth compounds. Give a possible explanation for this phenomenon.

For each of the following, write the Lewis structure(s), predict the molecular structure (including bond angles), and give the expected hybridization of the central atom. a. \(\mathrm{KrF}_{2} \quad\) b. \(\mathrm{KrF}_{4} \quad\) c. $\mathrm{XeO}_{2} \mathrm{F}_{2} \quad\( d. \)\mathrm{XeO}_{2} \mathrm{F}_{4}$
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