Calculate the density of metal having volume of unit cell $$64 \times 10^{-24} \mathrm{~cm}^3$$ and molar mass of metal $$192 \mathrm{~g} \mathrm{~mol}^{-1}$$ containing 4 particles in unit cell.

Calculate the number of atoms in 5 gram metal that crystallises to form simple cubic unit cell structure having edge length $$336 \mathrm{~pm}$$. (Density of metal $$=9.4 \mathrm{~g} \mathrm{~cm}^{-3}$$ )

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

An element has $$\mathrm{BCC}$$ structure with edge length of unit cell $$600 \mathrm{~pm}$$. What is the atomic radius of element?