Chemistry and Chemical Reactivity (9th Edition)

Published by Cengage Learning
ISBN 10: 1133949649
ISBN 13: 978-1-13394-964-0

Chapter 12 The Solid State - Study Questions - Page 467a: 10


176 pm

Work Step by Step

There's one ion each in the unit cell so: Mass: $(132.905+35.45)\ g/mol\div 6.022\times 10^{23}\ atoms/mol=2.796\times10^{-22}\ g/cell$ Volume: $2.796\times10^{-22}\ g/cell\div 3.99\ g/cm^3=7.007\times 10^{-23}\ cm^3/cell$ Side length: $\sqrt[3]{7.007\times 10^{-23}\ cm^3}=4.12\times10^{-8}\ cm=412\ pm$ Cube diagonal: $l.\sqrt3=2.r_{Cs^+}+2.r_{Cl^-}$ $r_{Cs^+}=176\ pm$
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