Home
Class 12
CHEMISTRY
The contibution of the particle present ...

The contibution of the particle present at the edge centre of a particular unit cell is :

A

`1//2`

B

`1//4`

C

1

D

`1//8`

Text Solution

Verified by Experts

The correct Answer is:
B

Each particle at edge centre is surrounded by four unit cells. Thus, the contribution to each unit cell is `1//4`
Promotional Banner

Similar Questions

Explore conceptually related problems

Assertion(A) : Total number of octahedral voids present in unit cell of cubic close packing including the one that is present at the body centre, is four. Reason ( R) : Besides the body centre there is one octahedral void present at the centre of each of the six faces of the unit cell and each of which is shared between two adjacent unit cells.

The coordination number of a particle in a bcc unit cell is-

The volume of a cubic unit cell is xcm^(3) whose 26% remains unoccupied by the constituent particles. If the radius of each particle is 0.3535x^(1//3)cm , then the number of particles per unit cell is-

The unoccupied space in a body centred cubic unit cell is.

A metal has face-centred cubic unit cell. The radius of an atom of the metal is 1.28Å. What is the edge length of the unit cell?

Show that for a body-centred cubic unit cell made up of identical particles, the radius is 0.43 times the edge length of the unit cell.

Corners and face-centres of a cubic unit cell are occupied by atoms. What fractions of a corner particle and a face-centred particle belong to the unit cell?

A cubic unit cell with an edge length of a cm consists of identical particles. The mass of each particle is m g and the density of the unit cell is (4m)/a^(3)g*cm^(-3) . Identify the type of the cubic unit cell.

Chromium crystallises in a body-centred cubic structure. The radius of a chromium atom is 125pm. What is the edge length of a unit cell in chromium crystal?

A compound consists of element A and B. It crystallises in a cubic crystal structure with unit cell having A atoms at the corners of the cell and B atom at the face centres of the cell. If the edge-length of the unit cell is 5Å, and the atomic masses of A and B are 60 and 90 respectively, then calculate the density of the compound.