Calculations for Standard Cubical Unit Lattice

Calcium crystallizes in a face centred cubic unit cell with a $\text{=}\text{0}\text{.560}\text{nm}\text{.}$  The density of the metal if it contains 0.1% schottky defects would be:

Copper crystallises in a face-centred cubic lattice and has a density of  $8.930\mathrm{g}{\mathrm{cm}}^{-3}$ at $393 \mathrm{K}.$ The radius of a copper atom is:
[Atomic mass of$\mathrm{Cu}=63.55\mathrm{u},{\mathrm{N}}_{\mathrm{A}}=6.02\times {10}^{23}{\mathrm{mol}}^{-1}]$

Iron has a body-centered cubic unit cell of cell edge $286.65 \mathrm{pm}$. The density of iron is $7.87 \mathrm{g} {\mathrm{cm}}^{-3}$. The Avogadro number is

(Atomic mass of iron $=56\hspace{0.17em}\mathrm{g}\hspace{0.17em}{\mathrm{mol}}^{-1}$)

X-rays diffraction studies show that copper crystallizes in an FCC unit cell with cell edge of  $3.6885\times {10}^{-8}\mathrm{cm}.$ In a separate experiment, copper is determined to have a density of  $\text{8}{\text{.92g/cm}}^{\text{3}}$, the atomic mass of copper would be:

In face-centred cubic $\left(\mathrm{FCC}\right)$ and body centred cubic $\left(\mathrm{BCC}\right),$ whose unit cell lengths are $3.5$ and $3.0$ $\mathrm{\AA }$ respectively, a metal crystallises into two cubic phases. What is the ratio of densities of $\mathrm{FCC}$ and $\mathrm{BCC}?$

A unit cell of sodium chloride has four formula units with an edge length of the unit cell $0.564 \mathrm{nm}$. What is the density of sodium chloride?

The coordination number of a metal crystallizing in a hexagonal close-packed structure is:

$\mathrm{CsBr}$ has bcc structure with edge length $4.3 \mathrm{\AA }$ . The shortest inter ionic distance in between ${\mathrm{Cs}}^{+}$ and ${\mathrm{Br}}^{-}$ is:

Atoms of metals $\mathrm{x}, \mathrm{y}$ and $\mathrm{z}$ form face-centred cubic (fcc) unit cell of edge length ${\mathrm{L}}_{\mathrm{x}}$, body-centred cubic (bcc) unit cell of edge length ${\mathrm{L}}_{\mathrm{y}}$, and simple cubic unit cell of edge length ${\mathrm{L}}_{\mathrm{z}}$, respectively. If ${\mathrm{r}}_{\mathrm{z}}=\frac{\sqrt{3}}{2}{\mathrm{r}}_{\mathrm{y}};{\mathrm{r}}_{\mathrm{y}}=\frac{8}{\sqrt{3}}{\mathrm{r}}_{\mathrm{x}};{\mathrm{M}}_{\mathrm{z}}=\frac{3}{2}{\mathrm{M}}_{\mathrm{y}}$ and ${\mathrm{M}}_{\mathrm{z}}=3{\mathrm{M}}_{\mathrm{x}}$, then the correct statement(s) is(are)

[Given: ${\mathrm{M}}_{\mathrm{x}},{\mathrm{M}}_{\mathrm{y}}$, and ${\mathrm{M}}_{\mathrm{z}}$ are molar masses of metals $\mathrm{x}, \mathrm{y}$, and $z$, respectively. ${\mathrm{r}}_{\mathrm{x}},{\mathrm{r}}_{\mathrm{y}}$, and ${\mathrm{r}}_{\mathrm{z}}$ are atomic radii of metals $\mathrm{x},\mathrm{y}$, and $\mathrm{z}$, respectively.]

Atom $\mathrm{X}$ occupies the fcc lattice sites as well as alternate tetrahedral voids of the same lattice. The packing efficiency (in $\%$) of the resultant solid is closest to

Copper crystallizes in an FCC unit cell with cell edge of  $3.608\times {10}^{-8}\mathrm{cm}.$ The density of copper is  $\mathrm{8}.92 \mathrm{g}/{\mathrm{cm}}^{\mathrm{3}}$, Calculate the atomic mass of copper.

Ice crystallises in a hexagonal lattice. At the low temperature at which the structure was determined, the lattice constants were $\mathrm{a}=4.53 \mathrm{\AA }$ and $\mathrm{c}=7.41 \mathrm{\AA }$. How many ${\mathrm{H}}_2\mathrm{O}$ molecules are contained in a unit cell? The density of ice is $0.92 \mathrm{g}/\mathrm{cc}$ at $0 °\mathrm{C}.$ A unit cell of ${\mathrm{H}}_2\mathrm{O}$ is shown below:

What is the radius of sodium atom if it crystallizes in $\mathrm{bcc}$ structure with the cell edge of $400 \mathrm{pm}$ ?

A unit cell of sodium chloride has four formula units. The edge of length of the unit cell is $0.564 \mathrm{nm}.$ What is the density of sodium chloride. Atomic Mass of $N\mathrm{a}=23,\mathrm{Cl}=35.5$

$\mathrm{Al}$ (atomic weight $26.98$) crystallizes in the cubic system with $\mathrm{a} = 4.05 \mathrm{\AA }$. Its density is $2.7 \mathrm{g} \mathrm{per} {\mathrm{cm}}^3$. Determine the cell type. Calculate the radius of $\mathrm{Al}$atom.

If the radius of a metal atom is $2.00 \mathrm{A}$ and its crystal structure in cubic close packed ($\mathrm{fcc}$ lattice), what is the volume (in ${\mathrm{cm}}^3$ ) of one unit cell?

Copper crystallises in a structure of face centerd cubic unit cell. The atomic radius of copper is $1.28 \mathrm{A}$. What is axial length on an edge of copper.

Zinc selenide$\left(\mathrm{ZnSe}\right)$ crystallizes in a face-centred cubic unit cell and has a density of $5.267 \mathrm{g}/\mathrm{cc}.$ Calculate the edge length of the unit cell.

Give the answer as the nearest integer.