Calculate the edge length of a simple cubic unit cell if the radius of an atom is $167.3 \ pm$. (in $pm$)

Calculate the density of a metal having molar mass $197 \ g \ mol^{-1}$ if it forms $fcc$ structure. $\left[a^3 \times N_{A}=40 \ cm^3 \ mol^{-1}\right]$ (in $g \ cm^{-3}$)

The cubic unit cell of a metal (molar mass $= 63.55 \ g \ mol^{-1}$) has an edge length of $362 \ pm$. Its density is $8.92 \ g \ cm^{-3}$. The type of unit cell is

Solid $AB$ has $NaCl$ type structure. If the radius of $A^{+}$ and $B^{-}$ are $0.5 \ \mathring{A}$ and $1.5 \ \mathring{A}$ respectively and the formula mass of $AB$ is $48 \ g/mol$,what is the density of $AB$ solid? $(N_A = 6 \times 10^{23})$

Copper crystallizes in an $fcc$ lattice with a unit cell edge length of $361 \ pm$. What is the radius of the copper atom in $pm$?

$X$-rays of wavelength $1 \ \mathring{A}$ are diffracted by the planes of particles in a metal. The second-order diffraction occurs at an angle of $60^{\circ}$. Calculate the distance between two parallel planes in $\mathring{A}$.