Calculate the density of CsCl. Use 169pm as the radius of Cs+.
rCs+= 169pm
length= 2*169= 338pm= 3.38*10^-8
v= l^3= (3.38*10^-8)^3 = 3.86*10^-23
m= 2* 168.36 g/mol / 6.022*10^23 = 5.59*10^-24g
d= m/v
d= 5.59*10^-24g/ 3.86*10^-23
d= 14.48 g/cm^3
BUT the correct answer is 4.24 g/cm^3. I can't figure out my mistake I've done it several times
4 answers
How did you get that answer then?
You used the cation radius when calculating volume rather than the anion radius.
Side of cube(unit cell) is root(3)×a=4r.
You are using 2r
Thats wrong.
You are using 2r
Thats wrong.
Actually you have to use 4r=/3.a for volume then you get 1095.8 kg/m3 for one atom. and one unit cell has 4 cation (cs+) and 1 anion (cl-) and you have multiply 4x1x1095.8 = 4380 kg/m3.
0 answers