Solid State Question 66
Question: In a cubic dosed packed structure of mixed oxides, the lattice is made up of oxide ions, one eighth of tetrahedral/voids are occupied by divalent ions $ ({{A}^{2+}}), $ while one half of the octahedral voids are occupied by trivalent ions $ ({{B}^{3+}}) $ . What is the formula of the oxide-
Options:
A) $ A_3B_2O_4 $
B) $ A_2B_2O_4 $
C) $ AB_2O_5 $
D) $ AB_2O_4 $
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Answer:
Correct Answer: D
Solution:
[d] Let number of oxides $ =x $ Number of octahedral void $ =x $ Number of tetrahedral void $ =2x $ Number of $ {{A}^{2+}} $ ion $ =\frac{1}{8}.2x=\frac{x}{4} $ Number of $ {{B}^{3+}} $ ion $ =\frac{x}{2} $ $ \begin{matrix} {{A}^{2+}}: & {{B}^{3+}}: & {{O}^{2-}} \\ \frac{x}{4}: & \frac{x}{2}: & x \\ 1 & 2 & 4 \\ \end{matrix} $ Hence, formula of oxide is $ AB_2O_4 $ .
BETA
