Strontium forms a face centered cubic unit cell and has a density of [tex]2.64g/cm^{3}[/tex]. The radius of a strontium is [tex]2.136 x 10^{-8}[/tex] cm.
Density provides an easy way to calculate a body's mass from its volume or vice versa; the mass is equal to the volume multiplied by the density (M = Vd), and the volume is equal to the mass divided by the density (V = M/d).
The structure of strontium (Sr) is similar to that of FCC. In FCC, the relationship between edge length and atomic radius is 2-a=4r2a=4r because unit cell atoms are present in the cube's corner and face centres. In this question, we are given an atomic radius and must calculate the edge length.
Here r=215pmr=215pm so a=4×2152–√=608.2pma=4×2152=608.2pm.
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