Answer: Hund’s (First) Rule
Explanation:
According to the first rule, electrons always enter an empty orbital before they pair up. Electrons are negatively charged and, as a result, they repel each other. Electrons tend to minimize repulsion by occupying their own orbitals, rather than sharing an orbital with another electron. Furthermore, quantum-mechanical calculations have shown that the electrons in singly occupied orbitals are less effectively screened or shielded from the nucleus. Electron shielding is further discussed in the next section.
Electrons will not pair in a set of equal energy orbitals if an empty orbital is available in the statement of Hund's Rule.
According to the first rule or Hund's Rule:
Hence, the statement Electrons will not pair in a set of equal energy orbitals if an empty orbital is available in the statement of Hund's Rule.
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