Bonds in Semiconductor crystals

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SUMMARY

The bonding structure in semiconductor crystals, specifically silicon (Si) and germanium (Ge), is primarily covalent, with each atom contributing four electrons from its outer shell for bonding. Traditional 2D representations of these crystals oversimplify the bonding picture, failing to accurately depict the three-dimensional diamond lattice structure that characterizes these materials. The concept of orbital hybridization is crucial for understanding the true nature of bonding in these semiconductors, as it allows for the formation of strong covalent bonds in a 3D arrangement.

PREREQUISITES
  • Covalent bonding in semiconductor materials
  • Understanding of silicon (Si) and germanium (Ge) crystal structures
  • Knowledge of orbital hybridization concepts
  • Familiarity with 3D crystal lattice representations
NEXT STEPS
  • Research the diamond crystal structure of silicon and germanium
  • Study the principles of orbital hybridization in covalent bonding
  • Explore advanced semiconductor physics and material properties
  • Examine 3D visualization tools for crystal structures
USEFUL FOR

Students and professionals in materials science, semiconductor physics, and electrical engineering who seek a deeper understanding of bonding mechanisms in semiconductor crystals.

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Hi!
I study semiconductors and I am confused with the bonding picture for semiconductor crystals. For example, it is said that in Si crystal one can find covalent bonds. In the most books this bonds are shown like that: 2D crystal structure where lines between atoms are a covalent bonds, each line stands for one electron (like here http://www.aplusphysics.com/courses/honors/microe/silicon.html). At the same time it is well known that in Si or in Ge there are only 4 electrons on the upper shell: two s electrons and two p electrons, only these ones can form bonds. Therefore it follows that for such 2D pictures of Si or Ge crystals we are just running out of electrons to make covalent bonds for the third dimension (usual crystal has 3D)!
Can you please explain what's going on with the third dimension. If such representations which i mentioned above is not true (or partially true), then what is complete 3Dimentional picture for bonding in semiconductors should look like?
 
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It seems i found the answer: those 2D pictures are huge simplifications. in reality Si and Ge have diamond structures. Plus you have to keep in mind orbital hybridization. Here is the best description of semiconductor structures and bonding:
 
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