An element with an atomic mass of $96 \, amu$ has a unit cell density of $10.3 \, g/cm^3$ and an edge length of $314 \, pm$. The crystal structure is of the type:

Calculate the volume of $fcc$ unit cell if the radius of a particle in it is $106.05 \ pm$.

In a $CsCl$ crystal,the interionic distance between $Cs^+$ and $Cl^-$ ions is:

Gold has a cubic close-packed structure which can be viewed as spheres occupying $74\%$ of the total volume. What is the edge length of the unit cell if the density of gold is $19.3 \ g/cm^3$? $(Au = 197 \ amu)$

An element has a density of $6.8 \ g \ cm^{-3}$ and crystallizes in a $bcc$ structure with a unit cell edge length of $290 \ pm$. The number of atoms in $200 \ g$ of the element is:

Calculate the edge length of a unit cell if a metal having an atomic radius of $170 \ pm$ forms a simple cubic unit cell.