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. The octahedral voids are occupied by a monovalent metal B. The formula of the oxide is
- $ABO_2$
- $A_2B_3O_4$
- $A_2BO_2$
- $AB_2O_2$
The Correct Option is D
Solution and Explanation
$\therefore$ No. of octahedral voids = $n$
No. of tetrahedral voids = $2n$
Divalent metal ions A present = $\frac{2n}{4} =\frac{n}{2}$
Monovalent metal ions $B$ present = $n$
$\therefore$ Ration $A : B : O^{-2} =\frac{n}{2} : n : n =\frac{1}{2} : 1 : 1 = 1 : 2 : 2$
Hence, formula = $AB_2O_2$
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Concepts Used:
Solid State
Solids are substances that are featured by a definite shape, volume, and high density. In the solid-state, the composed particles are arranged in several manners. Solid-state, in simple terms, means "no moving parts." Thus solid-state electronic devices are the ones inclusive of solid components that don’t change their position. Solid is a state of matter where the composed particles are arranged close to each other. The composed particles can be either atoms, molecules, or ions.
Types of Solids:
Based on the nature of the order that is present in the arrangement of their constituent particles solids can be divided into two types;
- Amorphous solids behave the same as super cool liquids due to the arrangement of constituent particles in short-range order. They are isotropic and have a broad melting point (range is about greater than 5°C).
- Crystalline solids have a fixed shape and the constituent particles are arranged in a long-range order.