Packing in Solids

The lattice generated in three-dimensional closed packing from two-dimensional square close-packed layers is

The coordination number in one-dimension close packing is 

The lattice generated in three-dimensional closed packing from two-dimensional square close-packed layers is

How many unit cells are present in a cube shaped ideal crystal of $\mathrm{NaCl}$ of mass $1\mathrm{g} ?$

Which one of the following schemes of ordering closed packed sheets of equal sized spheres does not generate closed packed lattice.

Atoms of an element $\mathrm{Z}$ form hexagonal closed packed $\left(\mathrm{hcp}\right)$ lattice and atoms of element $\mathrm{X}$ occupy all the tetrahedral voids. The formula of the compound is

In reference to crystal structure, explain the meaning of the coordination number.

The space occupied by $\mathrm{BCC}$ arrangement is approximately

Total number of layers between a distance of $14\mathrm{R}\sqrt{\frac{2}{3}}$ in $\mathrm{hcp}$ lattice (including first and last) are:

The number of hexagonal faces that are present in a truncated octahedron is

The co-ordination number of a metal crystallising in a hexagonal close-packed structure is:

Co-ordination number of atoms in $\mathrm{HCP}$is:

In a crystalline solid $\mathrm{x}$ atoms occupy hcp and $\frac{1}{4}$th of tetrahedral voids are occupied by $\mathrm{y}$ atoms. Then empirical formula of crystalline solid is:

In any compound, atoms of $\mathrm{A}$ occupies in $\mathrm{HCP}$ packing and atoms of $\mathrm{B}$ is at $\frac{1}{3^{\mathrm{rd}}}$ of tetrahedral voids. Then empirical formula of compound is:-

In any compound, atom $\mathrm{B}$ occupies in $\mathrm{HCP}$ packing and $\mathrm{A}$ is $1/3^{\mathrm{rd}}$ of tetrahedral voids. Then empirical formula of compound is:-

The coordination number of hexagonal closest packed $\left(\mathrm{HCP}\right)$ structure is
 

$\mathrm{HCP}$ crystal in made of $\mathrm{A}$ ions and $\mathrm{B}$ ions are arranged in $2/3^{\text{rd }}$ of octahedral voids. The simplest formula of unit cell is
 

How will you distinguish between the following pairs of terms:

Hexagonal close-packing and cubic close packing.

How will you distinguish between the following pairs of terms? 

Hexagonal close packing and cubic close packing.

In a cubic close packed structure of mixed oxides, the lattice is made up of oxide ions, one eighth of tetrahedral voids are occupied by divalent $\left({\mathrm{X}}^{2+}\right)$ ions, while one-half of the octahedral voids are occupied by trivalent ions $\left({\mathrm{Y}}^3+\right),$ then the formula of the oxide is:-