Hund's rules
Rules to determine the ground state of an atom
Hund's rules
In atomic physics and quantum chemistry, Hund's rules refers to a set of rules that German physicist Friedrich Hund formulated around 1925, which are used to determine the term symbol that corresponds to the ground state of a multi-electron atom. The first rule is especially important in chemistry, where it is often referred to simply as Hund's Rule. The three rules are: For a given electron configuration, the term with maximum multiplicity has the lowest energy. The multiplicity is equal to 2 S + 1 {\displaystyle 2S+1\ } , where S {\displaystyle S} is the total spin angular momentum for all electrons. The multiplicity is also equal to the number of unpaired electrons plus one. Therefore, the term with lowest energy is also the term with maximum S {\displaystyle S\,} and maximum number of unpaired electrons with equal...
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