Exploring E-e Repulsion: Stability of Half and Full P Sub-Shells Explained

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In summary, the stability of a half-filled p sub-shell is attributed to the absence of electron-electron repulsion, as electrons first fill the orbitals singly before pairing up according to Hund's rule. However, a fully occupied p sub-shell with 6 electrons is also considered stable, despite the potential for e-e repulsion. This is in contrast to a filled s sub-shell with 2 electrons, which is said to undergo e-e repulsion and is therefore considered unstable. This can be seen in the ionization energy values of helium and hydrogen, where helium's I.E is less than twice that of atomic hydrogen due to its inertness. The measure of stability/instability, in this case, is not solely determined by the
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htneT
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I am fully aware that a half filled p sub-shell is stable due to no repulsion as electrons first occupy the orbitals singly before pairing up according to Hunds rule, why is that however a fully occupied p sub-shell with 6 electrons is also considered stable? Where as a filled s sub-shell with 2 electrons is said to undergo e-e repulsion, hence the I.E value of He is less than that of Hydrogen's I.E by a factor of 2 (90% to be exact).

In short: Why is a full p sub-shell with 6 electrons not said to undergo e-e repulsion (considered stable), whereas a full s sub-shell with 2 electrons is said to undergo e-e repulsion (unstable).
 
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The ionization energy of Helium is a little less than twice that of atomic hydrogen, i.e. helium is more inert than atomic hydrogen.
See the table of values here.
 
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Doesn't it have to do with e-e repulsion?
 
  • #4
htneT said:
Doesn't it have to do with e-e repulsion?
Does what have to do with electron-electron repulsion? You said that helium has a lower ionization energy than helium, which is not the case. Similarly you are talking about p sub-shells but only referring to hydrogen and helium, which only have half and fully filled 1s sub-shells respectively.
 
  • #5
Vagn said:
Does what have to do with electron-electron repulsion? You said that helium has a lower ionization energy than helium, which is not the case. Similarly you are talking about p sub-shells but only referring to hydrogen and helium, which only have half and fully filled 1s sub-shells respectively.
My main question is why is a full p sub-shell considered stable, whereas a full s sub-shell considered unstable and its electrons undergo e-e repulsion?
 
  • #6
htneT said:
Where as a filled s sub-shell with 2 electrons is said to undergo e-e repulsion
Each electron in a multi-electron atom will of course experience e-e repulsion regardless of which subshell the electron under consideration occupies.
htneT said:
a full s sub-shell considered unstable
What is the measure of stability/instability you are using, I.E.? Ionization energy is not only determined by the number of electrons present in the atom, but also by the nuclear charge.
 

1. What is E-e repulsion and why is it important in exploring sub-shells?

E-e repulsion refers to the electrostatic repulsion between electrons in an atom. As electrons are negatively charged particles, they repel each other and this plays a crucial role in determining the stability of sub-shells. This is because the repulsion between electrons affects the energy levels and spatial arrangement of sub-shells, ultimately determining the overall stability of an atom.

2. How does the stability of half and full p sub-shells differ?

The stability of a half p sub-shell is lower than that of a full p sub-shell. This is due to the energy levels and spatial arrangement of the electrons in the sub-shell. In a half p sub-shell, the electrons are distributed across two energy levels and their repulsion is not fully neutralized, leading to a less stable configuration. In a full p sub-shell, the electrons are fully paired and their repulsion is completely neutralized, resulting in a more stable configuration.

3. What factors contribute to the stability of half and full p sub-shells?

The stability of half and full p sub-shells is determined by the number of electrons and their spatial arrangement. A full p sub-shell has an even number of electrons, which allows for complete pairing and neutralization of electron repulsion. In contrast, a half p sub-shell has an odd number of electrons, leading to incomplete pairing and higher repulsion. Additionally, the spatial arrangement of electrons in a full p sub-shell is more symmetrical, resulting in a more stable configuration.

4. How does the stability of sub-shells impact an atom's chemical properties?

The stability of sub-shells is closely linked to an atom's chemical properties. A more stable sub-shell configuration allows for stronger bonding between atoms, leading to a more stable molecule. On the other hand, a less stable sub-shell configuration makes an atom more reactive and likely to form chemical bonds in order to achieve a more stable electronic configuration.

5. Can the stability of sub-shells be altered?

The stability of sub-shells is primarily determined by the number of electrons and their spatial arrangement, which are inherent characteristics of an atom. However, external factors such as temperature, pressure, and the presence of other atoms can also affect the stability of sub-shells. For example, certain chemical reactions can alter the electron configuration and overall stability of an atom.

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