Why electrons must occupy degenerate orbitals with parallel spins?

In summary, the conversation discusses the reasons for why electrons occupy degenerate orbitals with parallel spins and the concept of stability due to exchange pairing of electrons. It is mentioned that Hunds rule explains this phenomenon, but there are exceptions to this rule. The argument behind Hunds rule is that parallel spins result in a smaller coulomb repulsion due to the antisymmetric orbital wavefunction. The exchange pairing or exchange interaction is also mentioned as a factor in this process.
  • #1
tasnim rahman
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Why electrons occupy degenerate orbitals with parallel spins? heard something of stability due to exchange pairing of electrons. someone kindly clarify this matter.
 
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  • #2
They needn't. This statement is known as Hunds rule and there are many exceptions known.
The usual argument behind Hunds rule is the following: If the spins are oriented parallel, the orbital part of the wavefunction has to be antisymmetric whence the probability to find two electrons at the same position is 0. This leads to a smaller coulomb repulsion than in a symmetric spatial wavefunction.
 
  • #3
thank you very much. Just to be sure, what is this exchange pairing of electrons or exchange interaction?
 

FAQ: Why electrons must occupy degenerate orbitals with parallel spins?

1. Why do electrons have to occupy degenerate orbitals?

Electrons are subject to the Pauli exclusion principle, which states that no two electrons in an atom can have the same set of quantum numbers. Degenerate orbitals have the same energy level, but different spin states, allowing for multiple electrons to occupy them without violating this principle.

2. What is the significance of parallel spins in degenerate orbitals?

Parallel spins in degenerate orbitals help to minimize the repulsion between electrons, as electrons with opposite spins are attracted to each other. This arrangement also contributes to the stability of the atom.

3. Can electrons in degenerate orbitals have opposite spins?

No, electrons in degenerate orbitals must have parallel spins to follow the Pauli exclusion principle. If they were to have opposite spins, they would have the same set of quantum numbers and would violate this principle.

4. How does the occupation of degenerate orbitals affect an atom's properties?

The occupation of degenerate orbitals can impact an atom's properties, such as its magnetic moment, reactivity, and stability. This is because the arrangement of electrons in degenerate orbitals influences the overall energy and behavior of the atom.

5. Are degenerate orbitals only found in certain elements?

No, degenerate orbitals can be found in any element, as they are a fundamental aspect of electron behavior. However, certain elements and electron configurations are more likely to have degenerate orbitals due to their electronic structure.

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