A compound is formed by elements A, B and O. | vedclass

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(C) Let the number of oxygen atoms in the $ccp$ lattice be $1$. Since the number of octahedral voids is equal to the number of atoms, the number of oc

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$AB_2O_4$

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(C) Let the number of oxygen atoms in the $ccp$ lattice be $1$. Since the number of octahedral voids is equal to the number of atoms, the number of octahedral voids is $1$. The number of tetrahedral voids is twice the number of atoms, so the number of tetrahedral voids is $2$. Atoms of $A$ occupy $\frac{1}{8}$ of the tetrahedral voids, so the number of $A$ atoms $= \frac{1}{8} 	imes 2 = \frac{1}{4}$. Atoms of $B$ occupy half of the octahedral voids, so the number of $B$ atoms $= \frac{1}{2} 	imes 1 = \frac{1}{2}$. The ratio of $A:B:O$ is $\frac{1}{4} : \frac{1}{2} : 1$. Multiplying the ratio by $4$, we get $1 : 2 : 4$. Thus, the molecular formula of the compound is $AB_2O_4$.

$A$ compound is formed by elements $A$, $B$ and $O$. Atoms of oxygen form $ccp$ lattice. Atoms of $A$ (cation) occupy $\frac{1}{8}^{\text{th}}$ of tetrahedral voids and atoms of $B$ (cation) occupy half of octahedral voids. What is the molecular formula of the compound?

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