Structure of Ionic Compounds

A compound AB has rock salt type structure. The formula weight of AB is 6.023 Y amu, and the closest AB distance is $Y^{\frac{1}{3}}$ nm, where Y is an arbitrary number. The density of lattice is

In which of the following crystals, the alternate tetrahedral voids are occupied?

The edge length of ${\mathrm{M}}^{+}{\mathrm{X}}^{-}$ ($\mathrm{fcc}$ structure) is $7.2 \stackrel{\mathrm{o}}{\mathrm{A}}$. Assuming ${\mathrm{M}}^{+}-{\mathrm{X}}^{-}$ contact along the cell edge, calculate the radius of ${\mathrm{X}}^{-}$ ion $\left({\mathrm{r}}_{{\mathrm{M}}^{+}}=1.6 \stackrel{\mathrm{o}}{\mathrm{A}}\right)?$

A student finds a crystal of $\mathrm{NaCl}$ having mass $58.5 \mathrm{mg}.$ He uses some of it to prepare $0.05\mathrm{M},10 \mathrm{mLNaCl}$ solution. How many unit cells are remained in the crystal ? $\left({\mathrm{N}}_{\mathrm{A}}=6\times {10}^{23}\right)$

A crystal is made of particles $\mathrm{A}$ and $\mathrm{B}$. A forms $\mathrm{F}\mathrm{C}\mathrm{C}$ packing and $\mathrm{B}$ occupies all the octahedral voids. If all the particles along the plane as shown in figure are removed, then, the formula of the crystal would be :

The coordination number (CN) of a ${\mathrm{M}}^{2+}$ ion in ${\mathrm{MX}}_2$ is $8$. Hence, CN of${\mathrm{X}}^{-}$ is-

A solid compound $\mathrm{XY}$ has $\mathrm{NaCl}$ structure. If the radius of the cation is $100 \mathrm{pm}$, the radius of the anion $\left({\mathrm{Y}}^{-}\right)$ in pm will be

(Round of the answer up to four significant figures)

In $\mathrm{NaCl}$ solid, if all the ions are removed along one of the axes joining the centres of any two diagonally opposite edges in a unit cell, then the resulting stoichiometry of the solid is

The interionic distance between cation and anion in caesium chloride crystal will be :-

In $\mathrm{NaCl}$ crystal, the number of nearest neighbours of each ${\mathrm{Na}}^{+}$ ions are:-

An ionic solid $\mathrm{PQ}$ crystallises in rock salt structure with density $4.0\mathrm{ }\mathrm{gm}/{\mathrm{cm}}^3.$. If the radius of cation and anion is $83$and $167 \mathrm{pm}$ respectively, then the molar mass of solid is $\left[{\mathrm{N}}_{\mathrm{A}}=6\times {10}^{23}\right]\mathrm{ }$

The radius of ${\mathrm{Ag}}^{+}$ ion is $126 \mathrm{pm}$ and ${\mathrm{I}}^{-}$ ion is $216 \mathrm{pm}$. The co-ordination number of ${\mathrm{Ag}}^{+}$ ion is:-

Which type of structure does $\mathrm{RbCl}$ have if ionic radii of ${\mathrm{Rb}}^{\oplus }$ and ${\mathrm{I}}^{\Theta }$ respectively are $1.46 \stackrel{°}{\mathrm{A}}$ and $2.16 \stackrel{°}{\mathrm{A}}$:-

The tetrahedral voids formed by $\mathrm{ccp}$ arrangement of ions ${\mathrm{Cl}}^{-}$ in rock salt structure are

What will be value of ${\mathrm{r}}_{{\mathrm{Cs}}^{+}}+{\mathrm{r}}_{\mathrm{Cr}}$ in $\mathrm{CsCl}$ crystal having edge length $\text{'}\mathrm{a}\text{'}$?

The positions of ${\mathrm{C}}^{-}$ ions in $\mathrm{NaCl}$ structure are:

In a solid $\text{'}\mathrm{AB}\text{'}$ having the $\mathrm{NaCl}$ structure, $\text{'}\mathrm{A}\text{'}$ atoms occupy the every $\mathrm{CCP}$ and $\mathrm{B}$ atoms are in $\mathrm{OHV}$. If all the face-centred atoms along one of the axes are removed, then the resultant stoichiometry of the solid is-
 

The edge length of face centred cubic unit cell having rock salt structure is $508 \mathrm{pm}$. If the radius of the cation is $110\mathrm{pm},$ the radius of the anion is-