Calculate the volume of a simple cubic unit cell if the radius of the particle in it is $400 \ pm$.

Iron crystallizes in different structures. At $911 \, ^oC$,it undergoes a transition from $bcc$ to $fcc$ structure. If the distance between the nearest neighbors is the same in both structures at the transition temperature,the ratio of the densities of $bcc$ and $fcc$ structures will be ..........

$CsBr$ has $bcc$ structure with edge length $4.3 \ \mathring{A}$. The shortest interionic distance in between $Cs^{+}$ and $Br^{-}$ (in $\mathring{A}$) is :

What is the volume of one particle in $BCC$ structure if '$a$' is edge length?

Calculate the molar mass of a metal having a density of $9.3 \ g \ cm^{-3}$ that forms a simple cubic unit cell. $[a^3 \cdot N_A = 22.6 \ cm^3 \ mol^{-1}]$

$A$ metal crystallises in a face-centred cubic $(FCC)$ structure with a metallic radius of $\sqrt{2} \ \mathring{A}$. The volume of the unit cell (in $m^{3}$) is: