An ionic compound has unit cells consisting of $A$ ions at the corners of a cube and $B$ ions on the centres of the faces of the cube. The empirical formula of this compound is

The number of octahedral voids in a unit cell of a cubical closest packed structure is

An alloy made up of $A$ and $B$ metals crystallises in a cubic lattice, where $B$ atoms occupy the corners and $A$ atoms occupy the face centers. The formula of the alloy formed is

In an alloy of metals $M$ and $N$,$N$ atoms form a $bcc$ structure,while $M$ atoms occupy the center of each face. If the cube is cut such that all atoms along one body diagonal are removed,the formula of the resulting solid will be ...........

In a compound,$W$ atoms are at the corners of the unit cell,$O$ atoms are at the edges of the unit cell,and $Na$ atoms are at the body center. The molecular formula of the compound is:

In an $AgI$ crystal,$I^{-}$ ions form a close-packed structure. What percentage of the tetrahedral voids is occupied by $Ag^{+}$ ions?