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Hund's rule of maximum multiplicity, often simply referred to as Hund's rule, is a principle of atomic chemistry which states that a greater total spin state usually makes the resulting atom more stable, most commonly manifested in a lower energy state, because it forces the unpaired electrons to reside in different spatial orbitals. A commonly given reason for the increased stability of high multiplicity states is that the different occupied spatial orbitals create a larger average distance between electrons, reducing electron-electron repulsion energy. In reality, it has been shown that the actual reason behind the increased stability is a decrease in the screening of electron-nuclear attractions. Total spin state is calculated as the total number of unpaired electrons + 1, or twice the total spin + 1 written as 2s+1.
Friedrich Hund discovered this rule and others referred to collectively as Hund's rules for atomic energy levels. They are important for spectroscopy and quantum chemistry.
As a result of Hund's rule of Maximum multiplicity, constraints are placed on the way atomic orbitals are filled using the Aufbau principle. Before any two electrons occupy an orbital in a subshell, other orbitals in the same subshell must first each contain one electron. Also, the electrons filling a subshell will have parallel spin before the shell starts filling up with the opposite spin electrons (after the first orbital gains a second electron). As a result, when filling up atomic orbitals, the maximum number of unpaired electrons (and hence maximum total spin state) is assured.
In 2004, it was reported in PhysicsWeb that researchers had synthesized 5-dehydro-m-xylylene (DMX), the first organic molecule known to violate Hund's rule. . The journal article reporting the discovery is in Angewante Chemie (L Slipchenko et al. Angew. Chem. Int. Ed. 2004 43 742)
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References
- 2004, Radical molecule breaks the rules, Physics Web, retrieved December 21, 2005.
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"Hund's rule of Maximum Multiplicity"