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Chapter 8: Problem 69

As a group, the noble gases are very stable chemically (only \(\mathrm{Kr}\) and Xe are known to form compounds). Use the concepts of shielding and the effective nuclear charge to explain why the noble gases tend to neither give up electrons nor accept additional electrons.

Short Answer

Expert verified
Noble gases are chemically stable due to their high effective nuclear charge and shielding effect, both contributing to a full shell of valence electrons. This full shell creates a high ionization energy barrier, making it hard to lose or gain electrons, thus they rarely form compounds.

Step by step solution

01

Understanding the Concept of Shielding

The shielding effect can be understood as the effect where core electrons (inner shell electrons) prevent outer shell electrons from feeling the full positive charge of the nucleus. In noble gases, the core electrons create a shield around the nucleus that prevents the outer electrons from feeling the full attractive force of the positive charge of the protons in the nucleus.
02

Understanding the Concept of Effective Nuclear Charge

Effective nuclear charge refers to the net positive charge experienced by an electron in a multi-electron atom. It takes into account the number of protons in the nucleus (which attract the electron) and the degree of shielding by other electrons (which repel the electron). In noble gases, due to their full shell of valence electrons, they have a very high effective nuclear charge, hence it's very difficult to remove an electron (high ionization energy) or to add an extra electron (high electron affinity).
03

Connecting Shielding and Effective Nuclear Charge to Noble Gas Stability

In the case of noble gases, as stated above, the full shell of valence electrons results in a high effective nuclear charge, which gives them a noble gas configuration (very stable). The shielding effect protects the core electrons, which makes it hard for noble gases to lose electrons. This is why noble gases are extremely stable and tend not to react with other elements or compounds, neither losing nor accepting additional electrons.

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Most popular questions from this chapter

The air in a manned spacecraft or submarine needs to be purified of exhaled carbon dioxide. Write equations for the reactions between carbon dioxide and (a) lithium oxide \(\left(\mathrm{Li}_{2} \mathrm{O}\right),\) (b) sodium peroxide \(\left(\mathrm{Na}_{2} \mathrm{O}_{2}\right),\) and \((\mathrm{c})\) potassium superoxide \(\left(\mathrm{KO}_{2}\right)\)

You are given four substances: a fuming red liquid, a dark metallic-looking solid, a pale-yellow gas, and a yellow-green gas that attacks glass. You are told that these substances are the first four members of Group 7A, the halogens. Name each one.

Use the third period of the periodic table as an example to illustrate the change in first ionization energies of the elements as we move from left to right. Explain the trend.

Arrange the following atoms in order of decreasing atomic radius: \(\mathrm{Na}, \mathrm{Al}, \mathrm{P}, \mathrm{Cl}, \mathrm{Mg} .\)

Why do noble gases have negative electron affinity values?
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