$A$ compound is formed by two elements $A$ and $B$. Atoms of the element $B$ (as anion) make $ccp$ lattice and those of element $A$ (as cation) occupy all tetrahedral voids. The formula of the compound is

In a crystalline solid with the formula $AB_2O_4$,the oxide ions are arranged in a cubic close-packed $(CCP)$ lattice,while the cations $A$ are present in tetrahedral voids and cations $B$ are present in octahedral voids. What are the percentages of tetrahedral and octahedral voids occupied by $A$ and $B$ respectively?

Calculate the total volume occupied by all particles in a $fcc$ unit cell if the volume of unit cell is $5.2 \times 10^{-23} \ cm^3$.

An ionic solid is $HCP$ of $B^{2-}$ ions and $A^{x+}$ ions are in one-fourth of tetrahedral voids. The value of $x$ should be

An octahedral void is surrounded by how many spheres?

$A$ solid is made of two elements $X$ and $Z$. The atoms $Z$ are in $CCP$ arrangement while the atoms $X$ occupy all the tetrahedral sites. What is the formula of the compound?