Ionic Solids and their Structures

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)

If in $\mathrm{NaCl}$ crystal all ions present along one axis passing through centre of two opposite faces are removed then formula of the crystal will be:

What is the maximum possible radius of the anion, If the radius of cation is $200 \mathrm{pm}$ in a solid $\mathrm{AB}$ (Rock-salt type) ?

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 radius of the ${\mathrm{Na}}^{+}$ is $95 \mathrm{pm}$ and that of ${\mathrm{Cl}}^{-}$ ion is $181 \mathrm{pm}.$ Predict the co-ordination number of ${\mathrm{Na}}^{+} :$

In an ionic compound ${\mathrm{A}}^{+}{\mathrm{X}}^{-}$, the radii of ${\mathrm{A}}^{+}$ and ${\mathrm{X}}^{-}$ are $1 \mathrm{pm}$ and $2 \mathrm{pm}$ respectively. The volume of unit cell of crystal $\mathrm{AX}$ is $\dots \dots ..$ and structure is similar to$\dots \dots \dots$

In fluorite unit cell

In zinc blende $\left(\mathrm{ZnS}\right)$, distance between two closest ${\mathrm{Zn}}^{2+}$ ions is $5\stackrel{\circ }{\mathrm{A}}$ then distance between two next closest ${\mathrm{S}}^{2-}$ ions is -

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

The mass of a unit cell of $\mathrm{CsCl}$ corresponds to:

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

$\mathrm{AB}$ crystal has $\mathrm{CsCl}$ type structure. If edge length of unit cell is $100 \mathrm{pm}$ then nearest distance between cation and anion is :-

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 $\left[{\mathrm{N}}_{\mathrm{A}}=6\times {10}^{23}\right]\mathrm{ }$