A cubic unit cell of a metal with molar mass of 63.55 gmol^–1 has an edge length of 362pm. Its density is 8.92 g cm^-3. The type of unit cell is 

$$\begin{gathered} \mathrm{Z}=\frac{\mathrm{Z}\times \mathrm{M}}{{\mathrm{a}}^3\times {\mathrm{N}}_{\mathrm{A}}} \\ \mathrm{Z}=\frac{\mathrm{d}\times {\mathrm{N}}_{\mathrm{A}}\times {\mathrm{a}}^3}{\mathrm{M}} \\ =\frac{8.92\times 6.023\times {10}^{23}\times {\left(362\times {10}^{-10}\right)}^3}{63.55} \\ =4 \end{gathered}$$

Now, the face-centered cubic (fcc) contains 4 atoms per unit cell.
∴The metal crystallises in fcc.