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
The CsCl structure is a simple cubic array of chloride ions with a cesiu…
Nov 11, 2019
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Crystalline CsCl has density 3.988 g cm-3. The volume occupied by single CsCl pair in the crystal will be ______. | Shaalaa.com
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the madelung constant for cscl consider the structure of cscl a typical sc crystal there is always one type of atom on the corners of a cube the other type of atom exactly in the middle of e 02809
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Given that the density of solid CsCl is 3.97 g cm−3, calculate ... | Filo
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Calculate the theoretical density of a CsCl given that the close packed directions are , the ionic radii of Cs and Cl- are 0.170 and 0.181 nm, respectively, and the atomic weights of Cs and Cl are 133 and 35 g/mol respectively. Answer: 4.2 g/cm3 There's the answer but I'm not sure how to get that answer. I keep getting 4.59 g/cm^3. Please show work so I can see what I'm doing wrong... Thanks!!
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