Hund, Friedrich

Household bleach, 369-370 Household solutions, 81t Hund, Friedrich, 148... 

Hund, Friedrich (1974), The History of Quantum Mechanics, Harper Row New York, NY. 

Hoffmann-Ostenhoff Maria, 423 Hoffmann-Ostenhoff Thomas, 423 Hogervorst Wim, 150 Hohenberg Pierre, 675 Holthausen Max C., 676, 715, 665, 676 Hooke Robert, 349 Howard Brian J., 899 Hubble Edwin Powell, 594 Hue Ivan, 971, 976 Hiickel Erich, 392, 427 Huckel Walter, 427 Hull Erika, 715 Hund Friedrich Hermann, 161, 461 Hurley Andrew... 

Huckel Walter 361 Hult Erika 611 Humbel Stephane 309 Hund Friedrich Hermann 144, 331, 343, 392,393,423, 672, 673,986 Hurley Andrew Crowther 520 Huygens Christiaan 41 Huzinaga Sigeru 358 Hylleraas Egil Andersen 196, 208-210, 502,506,513, 562... 

Similar situations arise frequently. There is a general principle that applies in all such cases Hund s rule (Friedrich Hund, 1896-1997) predicts that, ordinarily,... 

The last rule needed to generate electron configurations for all the atoms in the periodic table came from a German scientist named Friedrich Hund. Hund s rule can be expressed in several ways. The most precise definition is that atoms in a higher total spin state are more stable than those in a lower spin state. Thus, the sixth electron in carbon-12 must have the same spin as the fifth one. The Pauli exclusion principle then requires that it fill an empty p orbital. 

Quotation from Robert Mulliken, "Spectroscopy, Molecular Orbitals, and Chemical Bonding," Nobel Lectures. Chemistry. 19631970 (Amsterdam Elsevier, 1972) 131160, on 137. See Friedrich Hund, "Zur Deutung der Molekulspektren. IV." ZP 40 (1927) 742764, 42 (1927) 93120, 43 (1927) 805826 and Oyvind Burrau, "Berechnung des Energiewertes des Wasserstoff-Molekel-Ions (H2+) im Normalzustand," Danske Videnskabernes Selskab. Mat.-fys. Meddelser 7 (1927) 14. 

Physical basis of Hund s rule (a) J. A. Berson, in The Chemistry of the Quinonoid Compounds, Vol. II, S. Patai and Z. Rappoport, Eds., John Wiley Sons, Inc., New York, 1988. (h) W. Kutzelnigg, Friedrich Hund and Chemistry, Angew. Chem. Inti. Ed. Engl. 1996, 35, 573. 

The second step is called Hund s rule, for the German spectroscopist Friedrich Hund, who first proposed it. This procedure gives the configuration of the atom that corresponds to the lowest total energy, taking into... 

R. S. Mulliken, Life of a Scientist. An Autobiographical Account of the Development of Molecular Orbital Theory, with an Introductory Memoir by Friedrich Hund, ed. B. J. Ransil, Springer-Verlag, Berlin, 1989. 

Friedrich Hund determined a set of rules to determine the ground state of a... 

Knowledge of the physical forces that influence the total energy of a system thus reveals the theoretical underpinnings of nearly aU of experimental chemistry. In fact, much of the early activity in chemical bonding theory was the result of attempts to understand the results of molecular spectroscopy experiments. The developers of what came to be called molecular orbital theory, Robert Mulhken (US) and Friedrich Hund (Germany), established a professional and personal relationship based on their conunon interest in the spectra of diatomic molecules especially in the influence of isotope effects. When compared to other theories of the time, a major advantage of their theoretical approach was the ability to directly apply the results to the elucidation of molecular spectra. ... 

Universitat Gottingen, Friedrich-Hund-Platz 1, 37077 Gottingen, Germany Y. FILINCHUK... 

ASTRID PUNDT UNIVERSITAT GOTTINGEN FRIEDRICH-HUND-PLATZ 1 37077 GOTTINGEN GERMANY Tel t-49 551 39 5002 Fax +49 551 39 5012 apundt ump.swds.de... 

The energy order for the different terms and levels in Fig. 5.9 is in accord with the so-called Hund s rules put forward by the German spectroscopist Friedrich Hund (1896-1998), as follows ... 

Friedrich Hund determined a set of rules to determine the ground state of a multi-electron atom in the 1920s. One particular rule is called Hund s Rule in introductory chemistry courses. Hund s rule states that every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin. 

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