Calculate the radius of a metal atom if it forms a $bcc$ unit cell having an edge length of $530 \ pm$. (in $pm$)

Calculate the volume of the unit cell if an element having a molar mass of $180 \ g \ mol^{-1}$ forms an $fcc$ unit cell. $\left[\rho \cdot N_{A} = 120 \times 10^{21} \ g \ cm^{-3} \ mol^{-1}\right]$

The cubic unit cell of aluminium (Molar mass $27.0 \ g \ mol^{-1}$) has an edge length of $405 \ pm$. Its density is $2.70 \ g \ cm^{-3}$. The type of unit cell is

The density of chromium metal is $7 \ g \ cm^{-3}$. If the edge length of the unit cell is $300 \ pm$, identify the type of unit cell. (Atomic mass of $Cr = 52$)

For a simple cubic system,find the ratio of the interplanar distances between the $(100)$,$(110)$,and $(111)$ planes.

In an ionic compound with a $bcc$ structure, the distance between the two nearest ions is $173 \, pm$. What is the edge length of the unit cell in $pm$?