In a solid crystal of a mixed oxide, the oxide ions constitute ccp lattice. Element 'A' occupy half of the octahedral voids while the element 'B' occupy 12.5% of tetrahedral voids. The formula of the

Question

In a solid crystal of a mixed oxide, the oxide ions constitute ccp lattice. Element 'A' occupy half of the octahedral voids while the element 'B' occupy 12.5% of tetrahedral voids. The formula of the oxide is…….?

Prashant Kotian · Accepted Answer

Correct answer: C. Oxide ions constitute ccp means fcc unit cells, i.e. Number of oxide ions per unit cell = 4 Number of ‘A’ per unit cell 4 2 2   (As ‘A’ occupy half of the octahedral voids) Number of ‘B’, per unit cell

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