The CsCl structure is a simple cubic array of chloride ions with a cesium ion at the center of each cubic array (see Exercise 71 ). Given that the density of cesium chloride is 3.97 g / cm^3, and assuming that the chloride and cesium ions touch along the body diagonal of the cubic unit cell, calculate the distance between the centers of adjacent Cs^ and Cl^- ions in the solid. Compare this value with the expected distance based on the sizes of the ions. The ionic radius of Cs^ is 169 pm, and t
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CsCl crystallizes in a cubic structure that has a Cl^-at each corner and a Cs^ at the center of the unit cell. Use the ionic radii listed in Table 10.1 to predict the lattice constant, a, and compare with the value of a calculated from the observed density of CsCl, 3.97  g / cm^3. FIGURE CANT COPY Fig. 10-5 | Numerade
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Answer the following in brief. Cesium chloride crystallizes in cubic unit cell with Cl– ions at the corners and a Cs ion in the centre of the cube. How many CsCl molecules are there in the unit cell? - Chemistry | Shaalaa.com
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