Question:
In a compound, atoms of element Y form hexagonal close-packed structure. Atoms of element X occupy \(2/3\) of the octahedral voids. What is the formula of the compound?
In a compound, atoms of element Y form hexagonal close-packed structure. Atoms of element X occupy \(2/3\) of the octahedral voids. What is the formula of the compound?
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In a close packed lattice, the number of octahedral voids equals the number of atoms.
Updated On: Nov 12, 2026
- \(\text{X}_{2}\text{Y}_{3}\)
- \(\text{X}_{4}\text{Y}_{3}\)
- \(\text{X}_{3}\text{Y}_{2}\)
- \(\text{X}_{4}\text{Y}_{5}\)
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The Correct Option is A
Solution and Explanation
Step 1: Understanding the Concept
In a close packed structure, N atoms give N octahedral voids and 2N tetrahedral voids.
Step 2: Count the atoms
Let Y atoms be N. Then the octahedral voids are N. X occupies \(\dfrac{2}{3}\) of them, so X atoms \(=\dfrac{2N}{3}\).
Step 3: Calculation
X : Y \(=\dfrac{2N}{3}:N=2:3\). So the formula is \(\text{X}_2\text{Y}_3\).
Final Answer:
The formula of the compound is X2Y3, which is option (A). \[ \boxed{\text{(A) }\text{X}_{2}\text{Y}_{3}} \]
In a close packed structure, N atoms give N octahedral voids and 2N tetrahedral voids.
Step 2: Count the atoms
Let Y atoms be N. Then the octahedral voids are N. X occupies \(\dfrac{2}{3}\) of them, so X atoms \(=\dfrac{2N}{3}\).
Step 3: Calculation
X : Y \(=\dfrac{2N}{3}:N=2:3\). So the formula is \(\text{X}_2\text{Y}_3\).
Final Answer:
The formula of the compound is X2Y3, which is option (A). \[ \boxed{\text{(A) }\text{X}_{2}\text{Y}_{3}} \]
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