Grimm–Sommerfeld rule

In today's article we are going to explore different aspects related to Grimm–Sommerfeld rule. From its origin and evolution, to its possible implications and applications today. Throughout this journey, we will analyze different approaches and perspectives that will allow us to better understand the role that Grimm–Sommerfeld rule has played over time and how it continues to impact various areas of society. From historical and cultural aspects, to its relevance in the current panorama, we will delve into a wide range of topics to understand the importance and significance of Grimm–Sommerfeld rule in the contemporary world. Join us on this journey of discovery and inquiry about Grimm–Sommerfeld rule and discover its fascinating universe from a multidisciplinary perspective.

In chemistry, the Grimm–Sommerfeld rule[1] predicts that binary compounds with covalent character that have an average of 4 electrons per atom will have structures where both atoms are tetrahedrally coordinated (e.g. have the wurtzite structure). Examples are silicon carbide, the III-V semiconductors indium phosphide and gallium arsenide, the II-VI semiconductors, cadmium sulfide, cadmium selenide.

Gorynova expanded the scope of the rules to include ternary compounds where the average number of valence electrons per atom was four. Examples of this are the I-IV2-V3 CuGe2P3 compound which has a zincblende structure.[2]

Compounds or phases that obey the Grimm–Sommerfeld rule are termed Grimm–Sommerfeld compounds or phases.[3]

The rule has also been extended to predict bond lengths in Grimm–Sommerfeld compounds. When the sum of the atomic numbers is the same the bond lengths are the same.[4] An example is the series of bond lengths ranging from 244.7 pm to 246 pm. for the Ge–Ge bond in elemental germanium, the Ga–As bond in gallium arsenide, the Zn–Se bond in zinc selenide and the Cu–Br bond in copper(I) bromide.[4]

References

  1. ^ Grimm, H.G.; Sommerfeld, A (1926). "Über den. Zusammenhang des Abschlusses der Elektronengruppen im Atom mit den chemischen Valenzzahlen". Zeitschrift für Physik. 36 (1): 36–59. Bibcode:1926ZPhy...36...36G. doi:10.1007/bf01383924. S2CID 120248399.
  2. ^ Adachi, Sadao (2009). Properties of Semiconductor Alloys: Groups IV, III–V and II–VI Semiconductors. Wiley. ISBN 978-0470743690.
  3. ^ Concise Encyclopedia Chemistry, Mary Eagleson, Walter de Gruyter, 1994 ISBN 3-11-011451-8
  4. ^ a b Ulrich Müller, "Inorganic Structural Chemistry" 2d edition, John Wiley & Sons, Chichester, New York, Brisbane, Toronto, Singapore, 2007


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