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Chapter 12: Problem 101

Introduction of carbon into a metallic lattice generally results in a harder, less ductile substance with lower electrical and thermal conductivities. Explain why this might be so.

Short Answer

Expert verified
Introducing carbon atoms into a metallic lattice causes the lattice structure to distort as the carbon occupies interstitial sites and contributes additional valence electrons. This results in a harder, less ductile substance due to local stress points impeding the motion of metal atoms. Furthermore, the increased number of valence electrons leads to lower electrical conductivity as electron movement is hindered. Lastly, the thermal conductivity decreases as carbon atoms disrupt the flow of lattice vibrations (phonons). Overall, the presence of carbon in a metallic lattice leads to a stronger, less ductile material with reduced electrical and thermal conductivities.

Step by step solution

01

Understanding Metallic Lattices

A metallic lattice is a 3D arrangement of metal atoms held together by metallic bonds. The positively charged metal ions are surrounded by a sea of delocalized electrons, which are free to move throughout the lattice. This structure is responsible for the characteristic properties of metals, such as malleability, ductility, and high electrical and thermal conductivities.
02

Introducing Carbon Atoms

Carbon atoms can be introduced into the metallic lattice by methods such as alloying or forming interstitial solids. When carbon atoms are added, they occupy the interstitial spaces (voids) between the metal atoms, while contributing additional valence electrons into the electron sea.
03

Hardening and Reduced Ductility

The introduction of carbon atoms causes distortions in the metallic lattice, since the carbon atoms occupy the interstitial sites and create local stress points within the lattice. These stress points impede the motion of metal atoms and make it more difficult for the lattice to be deformed. Consequently, the resulting material becomes harder (stronger) and less ductile (less capable of being drawn into a wire or deformed without breaking).
04

Lower Electrical Conductivity

The additional valence electrons provided by the carbon atoms in the metallic lattices also lead to a reduced electrical conductivity. As the electron sea becomes more crowded with electrons, they are more likely to collide with each other and impede their free movement. Additionally, the distortions in the lattice structure may also hinder the movement of electrons. Consequently, the ease at which electrical current can flow through the lattice is reduced.
05

Lower Thermal Conductivity

Lastly, the reduced thermal conductivity can be attributed to the effect of carbon atoms on the movement of lattice vibrations, known as phonons. The interstitial carbon atoms disrupt the flow of phonons and create more scattering points for lattice vibrations. As a result, the overall ability of the metal to conduct heat efficiently is decreased. In conclusion, the introduction of carbon into a metallic lattice results in a harder, less ductile substance with lower electrical and thermal conductivities due to the distortions in the lattice structure, the increase in the number of valence electrons, and the disruption of lattice vibrations (phonons).

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Most popular questions from this chapter

Teflon is a polymer formed by the polymerization of \(\mathrm{F}_{2} \mathrm{C}=\mathrm{CF}_{2}\) - (a) Draw the structure of a section of this polymer. (b) What type of polymerization reaction is required to form Teflon?

Aluminum metal crystallizes in a face-centered cubic unit cell. (a) How many aluminum atoms are in a unit cell? (b) What is the coordination number of each aluminum atom? (c) Estimate the length of the unit cell edge, \(a\), from the atomic radius of aluminum (1.43 ?). (d) Calculate the density of aluminum metal.

(a) What is a monomer? (b) Which of these molecules can be used as a monomer: benzene, ethene (also called ethylene), methane?

Besides the cubic unit cell, which other unit cell(s) has edge lengths that are all equal to each other? (a) Orthorhombic, (b) hexagonal, (c) rhombohedral, (d) triclinic, (e) both rhombohedral and triclinic.

Which of the following properties are typical characteristics of a covalent- network solid, a metallic solid, or both: (a) ductility, (b) hardness, (c) high melting point?
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