AP EAMCET · Chemistry · Solid State
In a mixed oxide of \(A\) and \(B, A\) occupies all the octahedral voids while \(B\) occupies \((2 / 3)^{\text {rd }}\) the tetrahedral voids. The molecular formula of this oxide is
- A \(\mathrm{A}_3 \mathrm{~B}_4 \mathrm{O}_3\)
- B \(\mathrm{A}_3 \mathrm{~B}_2 \mathrm{O}_3\)
- C \(\mathrm{A}_3 \mathrm{BO}_3\)
- D \(A B_2 \mathrm{O}_3\)
Answer & Solution
Correct Answer
(A) \(\mathrm{A}_3 \mathrm{~B}_4 \mathrm{O}_3\)
Step-by-step Solution
Detailed explanation
According to mixed oxide, number of \(\mathrm{O}^{2-}\) ions \(=4\) So, number of tetrahedral voids \(=8\) and number of octahedral voids \(=4\) \(B\) occupies 2/3rd of tetrahedral void \(=8 \times \frac{2}{3}=16 / 3\) \(A\) occupies all octahedral voids \(=4\) Now,…
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