The radius of $K^{+}$ is $133 \ pm$ and that of $Cl^{-}$ is $181 \ pm$. The volume of the unit cell of $KCl$ expressed in $10^{-22} \ cm^{3}$ is

Which of the following expressions is correct in the case of a $CsCl$ unit cell (edge length,$a$)?

$A$ metal has $BCC$ structure with edge length of unit cell $400 \ pm$. The density of the metal is $4 \ g \ cm^{-3}$. What is the molar mass of the metal?

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

The edge length of the unit cell of a metal $(M_w = 24 \ g \ mol^{-1})$ having a cubic structure is $4.53 \ \mathring{A}$. If the density of the metal is $1.74 \ g \ cm^{-3}$, the radius of the metal atom is ............... $pm$ $(N_A = 6 \times 10^{23} \ mol^{-1})$

$CsBr$ has $b.c.c.$ structure with edge length $4.3 \ \mathring{A}$. The shortest inter-ionic distance between $Cs^{+}$ and $Br^{-}$ is ........... $\mathring{A}$.