Exploring the Stable State of Noble Gases

In summary, the octet configuration of an atom is extremely stable because it leads to a balance of electron configuration and thus conserves angular momentum.
  • #1
jancarlo
5
0
Hi, I am a student currently engaged in AP Physics B and AP Physics C, and I am curious as to why it is that most of the Noble Gases exhibit and exist in such a stable state. In AP Chem last year I learned that having a configuration in which the valence shell of an atom has eight electrons leads to a very electrically neutral and stable atom. I like to apply the knowledge I learn in physics to other fields, so I was just interested as to WHY the octet configuration is extremely stable. I asked my physics teacher, and he said it had something to do with conservation of angular momentum, so if anyone can elaborate on this I would appreciate it.

PS
I have looked this up in various textbooks but I have not gained the information I wish to obtain.
 
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  • #2
A full octet of electrons is sort of an equilibrium point for atoms. Everything is even, there's a lot less disharmony in their configuration. All atoms on the Periodic table want to take the quickest path to a full octet they can. So, for the Alkali Metals, the quickest path for them is to lose an electron, giving them a positive charge and a full octet (or full s-orbital, in the case of Lithium). Similarly, the Alkali Earth Metals want to lose two electrons. On the other side of the chart, the Halogen family wants to pick up an electron, giving them a negative charge and a full octet.

The Noble Gases are the most stable because they have a full octet *and* a net charge of 0.

So they're basically willing to take on a charge if it means they can have a full octet, because of how it brings them to that sort of equilibrium.

Of course, the transition metals get more complicated because of their d-orbitals and f-orbitals, but that's the basis of it.
 
  • #3
I understand the notion that atoms typically want to have an octet- metals like to lose electrons and non-metals, like fluorine for example, like to gain electrons to form such an octet. My question is WHAT makes an octet so favorable- in other words- why is there less "disharmony" in such a configuration, and why is it an equilibrium point for atoms? Why eight and not ten, or twelve, etc.?
 
  • #4
That has to do with the electron orbitals. The smallest are s-orbitals, with each holding two electrons. The next up is the p-orbital, holding six electrons. If I recall correctly, all of the elements on the left and right sides of the periodic table have s or p orbitals as their 'outermost' orbital (there are also d and f orbitals, which are bigger, and are what trans-metals have as their outermost orbitals). Thus, filling their last set of s and p orbitals gives them an octet, which makes them happy.

This gets complicated quickly as you move into the concepts of quantum numbers and electron configuration if you haven't heard about the s, p, d, and f orbital set ups before.
 
  • #5
I totally understand what you are telling me, with regards to the 4 quantum numbers and anything relating to it. What I am really looking for is a explanation from a physics standpoint. Like I mentioned earlier, what does angular momentum and its conservation have to do with such stable equilibrium?
 
  • #6
Helium does not have an 'octet'. Of the remaining noble gases, only Neon and Argon have octets in their valence shell. Krypton and Xenon have 18 electrons in their valence shell, Radon has 32... not exactly 'octets' unless you define octets to mean that the outermost (valence) shell contains completely full s and p orbitals.
 
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  • #7
Thanks for the clarification, but YES what I meant was the "octet" of electrons that are part of valence shell. So, what is so great about having these configurations? I am sure there has to be a reason why "eight" is the lucky number.
 
  • #8
So your question is why does an 's' orbital contain 2 electrons and a 'p' orbital contain 6?
 
  • #9
Not really. What I am aiming toward is more of the mechanics behind the configuration of this system. How is it synergistically balanced? Is the underlying concept conservation of angular momentum, or something else?
 
  • #10
I also want to know the answer to this. I think you're asking what are the mechanics of the atom, so that it "wants" to have 8 electrons in its outer shell. Can someone please give a good answer to this? I want to know and I feel like (no offense) no one who answered understood the question.
 

Related to Exploring the Stable State of Noble Gases

1. What are noble gases?

Noble gases are a group of chemical elements that are characterized by their full outer electron shell, making them very stable and unreactive. The noble gases include helium, neon, argon, krypton, xenon, and radon.

2. Why are noble gases considered stable?

Noble gases are considered stable because they have a full outer electron shell. This means that they have achieved the maximum number of valence electrons and do not need to gain or lose electrons to form chemical bonds. This makes them very unreactive and stable.

3. How are noble gases used in everyday life?

Noble gases have a variety of practical uses in everyday life. For example, helium is used in balloons and airships due to its low density. Neon is used in neon lights, argon is used in light bulbs to prevent oxidation, and krypton and xenon are used in energy-efficient lighting. Noble gases are also used in various medical and industrial applications.

4. How do scientists explore the stable state of noble gases?

Scientists explore the stable state of noble gases through various experiments and studies. This includes examining their electronic structure, properties, and reactions with other elements. They also use advanced techniques such as spectroscopy and computational methods to better understand the behavior of noble gases.

5. Can noble gases form compounds?

While noble gases are generally considered unreactive, they can form compounds under certain conditions. These compounds are known as "noble gas compounds" and have been observed with elements such as fluorine, oxygen, and xenon. However, these compounds are usually unstable and quickly decompose, making them difficult to study.

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