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Chapter 22: Problem 32

Why are there so few compounds of the noble gases?

Short Answer

Expert verified
There are so few compounds of noble gases due to their unique electron configuration resulting in high stability, low reactivity, high ionization energies, and low electron affinities. This makes it difficult for noble gases to form compounds with other elements, with rare exceptions occurring under extreme conditions or with highly reactive elements.

Step by step solution

01

Introduction to Noble Gases

Noble gases are elements found in Group 18 of the periodic table. They include helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and radon (Rn).
02

Electron Configuration

Noble gases have a unique electron configuration which makes them highly stable. They have completely filled electron shells. For example, helium has a filled 1s orbital, while neon has filled 2s and 2p orbitals. A filled electron shell is very stable, meaning noble gases have very low reactivity.
03

Low Reactivity

The electron configuration of noble gases makes them nearly inert, meaning they do not readily participate in chemical reactions. This is because their electron shells are already at their maximum capacity, and they have no tendency to gain, lose, or share electrons with other atoms.
04

Ionization Energy and Electron Affinity

Due to the stability of their electron configuration, noble gases have high ionization energies (energy required to remove an electron) and low electron affinities (energy released when an electron is added). This means that it is challenging to remove electrons from or add electrons to noble gases, further explaining their low reactivity.
05

Exceptions and Rare Compounds

There are a few rare examples of compounds involving noble gases, particularly with xenon (Xe) and krypton (Kr). These are formed under extreme conditions, such as high pressure or in the presence of highly reactive elements like fluorine. These compounds are not easily formed and are typically not stable, reinforcing the overall low reactivity of noble gases. In summary, there are so few compounds of noble gases because of their electron configuration resulting in high stability, low reactivity, high ionization energies, and low electron affinities, which make it difficult for them to form compounds with other elements.

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Most popular questions from this chapter

What is the anhydride for each of the following acids: (a) \(\mathrm{H}_{2} \mathrm{SO}_{4}\), (b) \(\mathrm{HClO}_{3}\) (c) \(\mathrm{HNO}_{2}\), (d) \(\mathrm{H}_{2} \mathrm{CO}_{3}\) (e) \(\mathrm{H}_{3} \mathrm{PO}_{4} ?\)

The solubility of \(\mathrm{Cl}_{2}\) in \(100 \mathrm{~g}\) of water at STP is \(310 \mathrm{~cm}^{3}\). Assume that this quantity of \(\mathrm{Cl}_{2}\) is dissolved and equilibrated as follows: $$ \mathrm{Cl}_{2}(a q)+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{Cl}^{-}(a q)+\mathrm{HClO}(a q)+\mathrm{H}^{+}(a q) $$ If the equilibrium constant for this reaction is \(4.7 \times 10^{-4}\), calculate the equilibrium concentration of \(\mathrm{HClO}\) formed.

The atomic and ionic radii of the first three group \(6 \mathrm{~A}\) elements are (a) Explain why the atomic radius increases in moving downward in the group. (b) Explain why the ionic radii are larger than the atomic radii. (c) Which of the three anjons would you expect to be the strongest base in water? Explain.

Complete and balance the following equations: (a) \(\mathrm{CaO}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (b) \(\mathrm{Al}_{2} \mathrm{O}_{3}(s)+\mathrm{H}^{+}(a q) \longrightarrow\) (c) \(\mathrm{Na}_{2} \mathrm{O}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(I) \longrightarrow\) (d) \(\mathrm{N}_{2} \mathrm{O}_{3}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (e) \(\mathrm{KO}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (f) \(\mathrm{NO}(g)+\mathrm{O}_{3}(g) \longrightarrow\)

(a) Give the names and chemical symbols for the three isotopes of hydrogen. (b) List the isotopes in order of decreasing natural abundance.
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