Structure of a mixed oxide is cubic close-packed (ccp). The cubic unit cell of mixed oxide is composed of oxide ions. One-fourth of the tetrahedral voids are occupied by divalent metal A and the octahedral voids are occupied by a monovalent metal B. The formula of the oxide is-

Options

A. `A_(2)BO_(2)`
B. `A_(2)B_(3)O_(4)`
C. `AB_(2)O_(2)`
D. `ABO_(2)`

Answer

C

Explanation

The cubic unit cell of mixed oxide is composed of `O^(2-)` ions.
`therefore` The number of `O^(2-)` ions = 4.
`A^(2+)` ions are in `1/4th` of the tetrahedral voids and `B^(+)` ions are in octahedral voids of the ccp lattice.
Therefore, the number of `A^(2+)` ions = `1/4xx8=2` and the number of `B^(+)` ions = 4.
Therefore, the formula of the metal oxide will be `AB_(2)O_(2)`.