Structure of a mixed oxide is cubic close - packed (ccp). The cubic unit cell of mixed oxide is composed of oxide ions

Explanation:

The correct answer is Option C i.e formula of given oxide is AB₂O_2.

Given, the mixed oxide described has a cubic-close packing structure (ccp).

Effective no of atoms/ions/lattice points (Z) in ccp = 4

No. of octahedral voids = Z

No. of tetrahedral voids = 2Z

Therefore, no. of octahedral and tetrahedral voids in given ccp structure is 4 and 8 respectively.

Given,

A⁺² occupies 1/4th of tetrahedral voids

So, no. of A⁺² ions in given mixed oxide = ¼ x 8= 2

Also given,

B⁺¹ occupy all the octahedral voids

So, no. of B⁺¹ ions in given mixed oxide = 4

Since it is an oxide, so oxidation of O = -2

Since the mixed oxide is electrically neutral,

So if no. of O^2- ions = y

Then, 2x2 + 1x4 - 2y = 0

y = 4

So, ratio of no of respective atoms constituting the given mixed oxide i.e.

A: B:O = 2:4:4

= 1:2:2

Final Answer:

Hence, formula if given mixed oxide is determined to be AB₂O_2.

So, the correct answer is Option C.