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Chapter 8: Problem 67

As a group, the noble gases are very stable chemically (only Kr and Xe are known to form some compounds). Why?

Short Answer

Expert verified
The noble gases are chemically very stable because they have full valence electron shells, which means they do not need to gain or lose electrons to achieve maximum stability. However, the heavier noble gases Krypton (Kr) and Xenon (Xe) can form some compounds due to their larger atomic sizes and lower ionization energies.

Step by step solution

01

Understanding the Nature of Noble Gases

Noble gases are elements that belong to group 18 of the periodic table, consisting of helium, neon, argon, krypton, xenon, and radon. They are known for their low reactivity, which means they rarely partake in chemical reactions.
02

Examination of Electron Configuration

The stability and reactivity of elements largely depend on their electron configurations. In simpler terms, it means how electrons are arranged in energy levels or orbitals around the nucleus of an atom. Noble gases have specific electron configurations. They have their outermost energy levels, also known as valence shells, completely filled with electrons.
03

Understanding the Stability of Noble Gases

Having a full set of electrons in their outermost energy level makes noble gases very stable. This is because in order to achieve maximum stability, atoms tend to either fill or empty their outermost electron orbitals. As noble gases already have full outer electron shells, they do not need to gain, lose, or share electrons, resulting in them being chemically inert.
04

Exceptions in Noble Gases

Although all noble gases are generally stable and inert, some can indeed form compounds under certain conditions. Krypton (Kr) and Xenon (Xe) are such exceptions. These heavier noble gases can form compounds mainly due to their larger atomic sizes and therefore their lower ionization energies. This makes it somewhat easier for them to accept electrons and form compounds than the other noble gases.

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Most popular questions from this chapter

Name the ions with +3 charges that have these electron configurations: (a) \([\mathrm{Ar}] 3 d^{3},(\mathrm{~b})[\mathrm{Ar}],\) (c) \([\mathrm{Kr}] 4 d^{6}\) (d) \([\mathrm{Xe}] 4 f^{14} 5 d^{6}\)

A student is given samples of three elements, \(X, Y\) and \(Z\), which could be an alkali metal, a member of Group \(4 \mathrm{~A},\) and a member of Group \(5 \mathrm{~A}\). She makes the following observations: Element X has a metallic luster and conducts electricity. It reacts slowly with hydrochloric acid to produce hydrogen gas. Element \(Y\) is a light-yellow solid that does not conduct electricity. Element \(Z\) has a metallic luster and conducts electricity. When exposed to air, it slowly forms a white powder. A solution of the white powder in water is basic. What can you conclude about the elements from these observations?

A neutral atom of a certain element has 17 electrons. Without consulting a periodic table, (a) write the ground-state electron configuration of the element, (b) classify the element, (c) determine whether the atoms of this element are diamagnetic or paramagnetic.

Define valence electrons. For representative elements, the number of yalence electrons of an element is equal to its group number. Show that this is true for the following elements: \(\mathrm{Al}, \mathrm{Sr}, \mathrm{K}, \mathrm{Br}, \mathrm{P}, \mathrm{S}, \mathrm{C}\).

What is Moseley's contribution to the modern periodic table?
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