An ionic compound $X^{+}Y^{-}$ has a $bcc$ structure. The distance between two nearest ions is $1.73 \, \mathring{A}$. What would be the edge length of the unit cell in $pm$?

The density of $NaCl$ is $2.165 \, g \, cm^{-3}$. The distance between $Na^+$ and $Cl^-$ ions in the $NaCl$ crystal is $281 \, pm$. Based on this information,the value of Avogadro's number is ...

What is the relation between edge length $a$ and the total volume occupied by atoms in a $BCC$ unit cell?

Calculate the molar mass of an element having a density of $8.6 \ g \ cm^{-3}$ if it forms a $bcc$ structure $[a^3 \times N_{A} = 22.0 \ cm^3 \ mol^{-1}]$.

When silver crystallizes, it forms face-centered cubic $(FCC)$ unit cells. If the volume of the unit cell is $6.84 \times 10^{-23} \text{ cm}^3$, calculate the density of silver. (Molar mass of silver is $108 \text{ g/mol}$, $N_A = 6.022 \times 10^{23} \text{ mol}^{-1}$) (in $\text{ g cm}^{-3}$)

How can you determine the atomic mass of an unknown metal if you know its density and the dimension of its unit cell? Explain.