1. Example 4.1 The Effect of Temperature on Vacancy Concentrations
Calculate the concentration of vacancies in copper at room temperature (25oC). What temperature will be needed to heat treat copper such that the concentration of vacancies produced will be 1000 times more than the equilibrium concentration of vacancies at room temperature? Assume that 20,000 cal are required to produce a mole of vacancies in copper.
Example 4.1 SOLUTION
The lattice parameter of FCC copper is nm. The basis is 1, therefore, the number of copper atoms, or lattice points, per cm3 is:

2. Example 4.1 SOLUTION (Continued)
At room temperature, T = = 298 K:
We could do this by heating the copper to a temperature at which this number of vacancies forms:

3. Example 4.2 Vacancy Concentrations in Iron
Determine the number of vacancies needed for a BCC iron crystal to have a density of 7.87 g/cm3. The lattice parameter of the iron is  10-8 cm.
Example 4.2 SOLUTION
The expected theoretical density of iron can be calculated from the lattice parameter and the atomic mass.

4. Example 4.2 SOLUTION (Continued)
Let’s calculate the number of iron atoms and vacancies that would be present in each unit cell for the required density of 7.87 g/cm3:
Or, there should be 2.00 – = vacancies per unit cell. The number of vacancies per cm3 is:

5. Example 4.3 Sites for Carbon in Iron
In FCC iron, carbon atoms are located at octahedral sites at the center of each edge of the unit cell (1/2, 0, 0) and at the center of the unit cell (1/2, 1/2, 1/2). In BCC iron, carbon atoms enter tetrahedral sites, such as 1/4, 1/2, 0. The lattice parameter is nm for FCC iron and nm for BCC iron. Assume that carbon atoms have a radius of nm. (1) Would we expect a greater distortion of the crystal by an interstitial carbon atom in FCC or BCC iron? (2) What would be the atomic percentage of carbon in each type of iron if all the interstitial sites were filled?

6. (c) 2003 Brooks/Cole Publishing / Thomson Learning
Figure 4.2 (a) The location of the ¼, ½, 0 interstitial site in BCC metals, showing the arrangement of the normal atoms and the interstitial atom (b) ½, 0, 0 site in FCC metals, (for Example 4.3). (c) Edge centers and cube centers are some of the interstitial sites in the FCC structure (Example 4.3).

7. From Figure 4.2(a), we find that:
Example 4.3 SOLUTION
1. We could calculate the size of the interstitial site at the 1/4, 1/2, 0 location with the help of Figure 4.2(a). The radius RBCC of the iron atom is:
From Figure 4.2(a), we find that:
For FCC iron, the interstitial site such as the 1/2, 0, 0 lies along directions. Thus, the radius of the iron atom and the radius of the interstitial site are [Figure 4.2(b)]:

8. Example 4.3 SOLUTION (Continued)
The interstitial site in the BCC iron is smaller than the interstitial site in the FCC iron. Although both are smaller than the carbon atom, carbon distorts the BCC crystal structure more than the FCC crystal. As a result, fewer carbon atoms are expected to enter interstitial positions in BCC iron than in FCC iron.

9. Example 4.3 SOLUTION (Continued)
2. We can find a total of 24 interstitial sites of the type 1/4, 1/2, 0; however, since each site is located at a face of the unit cell, only half of each site belongs uniquely to a single cell. Thus: (24 sites)(1/2) = 12 interstitial sites per unit cell
Atomic percentage of carbon in BCC iron would be:
In FCC iron, the number of octahedral interstitial sites is: (12 edges) (1/4) + 1 center = 4 interstitial sites per unit cell
Atomic percentage of carbon in BCC iron would be: