How does the electronic structure of the Noble Gases account for their lack of reactivity?

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How does the electronic structure of the Noble Gases account for their lack of reactivity?

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Md Ariful Islam · Answer 1 · Apr 02, 2024 09:48:30

If you are doing your Chemistry or Physics homework there should be a Table in front of you now (in addition to the table or desk that you write on!).

The RIGHTMOST column on the $"Periodic Table"$, i.e. on your right as you face the Table, is $"Group 18"$, which consists of the so-called $"Noble Gases"$. Because these elements, $"He, Ne, Ar, etc"$ were not known to undergo chemical reaction, they were dubbed the $"Noble Gases"$, i.e. a select, insular group that did not undergo reaction with more common elements.

This lack of reactivity, this inertness, can be traced to the electronic configuration of Group 18, which features a full valence shell. Because of this full valence shell, Noble Gases are $"(i)"$ difficult to oxidize (the nuclear charge tenaciously binds the valence electrons), and $"(ii)"$ difficult to reduce (electrons must enter a higher energy valence shell).

These days, we know that the Noble Gases do in fact form a few compounds with the more promiscuous oxidants, i.e. fluorine, and oxygen, and a Noble Gas chemistry has been developed.

How does the electronic structure of the Noble Gases account for their lack of reactivity?

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