(A) The ionic radius of Cs⁺ is 167 pm. Use Figure 12-49 and information in Examples 12-9 and 12-11 to determine the edge length of the unit cell of CsCl.

(B) Use the length of the unit cell of NaCl obtained in Example 12-11, together with the molar mass of NaCl and the Avogadro constant, to estimate the density of NaCl.

Figure 12-49

Examples 12-9

(A) Potassium crystallizes in the bcc structure. What is the length of the unit cell in this structure? Use the metallic radius of potassium given in Figure 9-11.

(B) Aluminum crystallizes in an fcc structure. Given that the atomic radius of Al is 143.1 pm, what is the volume of a unit cell?

Figure 9-11

Examples 12-11

The ionic radii of Na⁺ and Cl^- in NaCl are 99 and 181 pm, respectively. What is the edge length of the unit cell?

Transcribed Image Text:

= Cr = Cs+