(A) Step $1$: Calculate the number of atoms of $A$ per unit cell. Since $A$ atoms are at the $8$ corners, each contributes $1/8$ to the unit cell. Num

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(A) Step $1$: Calculate the number of atoms of $A$ per unit cell. Since $A$ atoms are at the $8$ corners, each contributes $1/8$ to the unit cell. Number of $A = 8 \times (1/8) = 1$.Step $2$: Calculate the number of atoms of $B$ per unit cell. Since $B$ atom is at the body center, it contributes $1$ to the unit cell. Number of $B = 1$.Step $3$: Determine the ratio of $A$ to $B$. The ratio is $1:1$.Step $4$: The formula of the compound is $AB$.

Class 12 Chemistry Solid State Crystal structure and Coordination number

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$A$ compound formed by elements $A$ and $B$ crystallizes in a cubic structure where $A$ atoms are at the corners of the cube and $B$ atoms are at the center of the cube. What is the formula of the compound?

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A
$AB$
B
$A_2B$
C
$AB_2$
D
$A_2B_2$

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Crystal structure and Coordination number

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In an ionic crystal,$\frac{r^{+}}{r^{-}} = 0.524$,the coordination number of the cation is:

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Determine the number of atoms per unit cell in a body-centered cubic $(BCC)$ unit cell.

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In an $fcc$ crystal lattice,atoms $A$ are present at the corners and atoms $B$ are present at the face centers. If one atom $A$ is missing from a corner,what is the molecular formula of the compound?

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An element crystallises in a face-centred cubic (fcc) unit cell with cell edge $a$. The distance between the centres of two nearest octahedral voids in the crystal lattice is

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$A$ compound formed by elements $A$ and $B$ crystallizes in a cubic structure where $A$ atoms are at the corners of the cube and $B$ atoms are at the center of the cube. What is the formula of the compound?

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