In a compound, oxide ions constitute cubic close packing. Cations A occupy 50% of tetrahedral holes while cations B occupy all the octahedral voids. The empirical formula of the compound is ?

$A B_{2} O_{4}$

No worries! We‘ve got your back. Try BYJU‘S free classes today!

$A B O_{2}$

No worries! We‘ve got your back. Try BYJU‘S free classes today!

$A_{2} B O_{4}$

No worries! We‘ve got your back. Try BYJU‘S free classes today!

$A B O$

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Open in App

Solution

The correct option is D
$A B O$

Number of $O^{2 -}$ ions per unit cell $= \frac{1}{8} \times 8 (c o r n e r s) + \frac{1}{2} \times 6 (f a c e s) = 4$
Number of A cations per unit cells $= \frac{50}{100} \times 8 (t e t r a h e d r a l v o i d s) = 4$
Number of B cations per unit cell = 4 (octahedral voids).
Hence, the empirical formula $= A_{4} B_{4} O_{4}$ or $A B O$

Suggest Corrections

Similar questions

In a compound, oxide ions constitute cubic close packing. Cations A occupy 50% of tetrahedral holes while cations B occupy all the octahedral voids. The empirical formula of the compound is ?

Q. In a compound, oxide ions have a cubic close packing arrangement. Cations A are present in half of the tetrahedral voids and cation B occupies the octahedral voids. The simplest formula of the compound is:

Q. In a metallic oxide, oxide ions are arranged in cubic close packing. One sixth of the tetrahedral voids are occupied by cations

P

and one third of octahedral voids are occupied by the cation

Q

. Deduce the formula of the compound.

Q. In the structure of a compound, oxide ions are cubic close packed whereas

\frac{1}{8} t h

of tetrahedral voids are occupied by

A^{2 +}

cation and half of octahedral voids are occupied by

B^{3 +}

cations. The general formula of the compound having structure is:

Q5) in a crystalline solid , anions 'C' are arranged in cubic close packing cations 'A' occupy 50%of tetrahedral voids and cations 'B' occupy 50% of octahedral voids .what is the formula of the solid

Join BYJU'S Learning Program

In a compound, oxide ions constitute cubic close packing. Cations A occupy 50% of tetrahedral holes while cations B occupy all the octahedral voids. The empirical formula of the compound is ?

The correct option is D ABO Number of O2− ions per unit cell =18×8(corners)+12×6 (faces)=4 Number of A cations per unit cells =50100×8(tetrahedral voids)=4 Number of B cations per unit cell = 4 (octahedral voids). Hence, the empirical formula =A4B4O4 or ABO