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Chapter 23: Problem 24

Germanium has the same crystal structure as diamond (Figure 11.41). Based on this fact, do you think germanium is likely to exhibit metallic properties? Explain your answer.

Short Answer

Expert verified
Germanium is not likely to exhibit metallic properties because it shares the same crystal structure as diamond, which is a non-metal with covalent bonding. This structure leads to a strong and rigid lattice, but does not form a "sea of electrons" for efficient electrical or thermal conductivity. Additionally, this type of lattice structure is not likely to be malleable or ductile, which are characteristic properties of metals.

Step by step solution

01

Understand the diamond crystal structure

The diamond crystal structure is a type of crystal lattice, which is characterized by a repeating pattern of atoms in a three-dimensional network. In the case of diamond, it has a face-centered cubic structure (also known as FCC). Each carbon atom in diamond is covalently bonded to four other carbon atoms, forming a tetrahedral structure. This leads to a very strong and rigid lattice structure.
02

Compare germanium and diamond's crystal structures

Germanium has the same crystal structure as diamond, meaning that it also has a face-centered cubic lattice structure, and each germanium atom forms four covalent bonds with four other germanium atoms in a tetrahedral arrangement. We can deduce that germanium has a similar strong and rigid lattice structure to diamond due to their shared crystal structure.
03

Consider characteristics of metals

Metals have several characteristic properties, including electrical and thermal conductivity (attributed to the so-called "sea of electrons"), malleability, and ductility. Metals have a large number of valence electrons that can move freely throughout the lattice, forming a conductive pathway for both electricity and heat.
04

Determine if germanium exhibits metallic properties

Germanium and diamond both have a face-centered cubic crystal structure with tetrahedral covalent bonding. While this results in a strong and rigid lattice structure, it does not lead to the formation of a "sea of electrons" that would allow for efficient electrical or thermal conductivity. In addition, a covalently bonded lattice with a strong, rigid structure is not likely to be malleable or ductile. Based on this analysis, it can be concluded that germanium is not likely to exhibit metallic properties due to its diamond-like crystal structure and the lack of characteristics typically associated with metals.

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