Match the type of unit cell given in Column I with the features given in Column II.
Column I | Column II | |||
A | Primitive cubic unit cell | 1. | Each of the three perpendicular edges compulsorily have the different edge length i.e., a ≠ b ≠ c | |
B | Body centred cubic unit cell | 2. | Number of atoms per unit cell is one. | |
C | Face centred cubic unit cell | 3. | Each of the three perpendicular edges compulsorily have the same edge length i.e., a=b=c | |
D | End centred orthorhombic | 4. | In addition to the contribution from the corner unit cell atoms the number of atoms present in a unit cell is one | |
5. | In addition to the contribution from the corner atoms the number of atoms present in a unit cell is three |
Codes:
Options: | A | B | C | D |
1. | 2,5 | 3,1 | 4,2 | 1,3 |
2. | 1 | 2 | 3 | 5 |
3. | 2,3 | 3,4 | 3,5 | 1,4 |
4. | 4 | 5 | 3 | 2 |
Total number of atoms per unil cell = 1/8x 8=1
Here, 1/8 is due to contribution of each atom present at corner.
B. For body centred cubic unit cell, a=b=c
This lattice contain atoms at corner as well as body centre. Contribution duo to atoms at corner = 1/8 x 8 = 1contribution due to atoms at body centre = 8
C. For face centred unit cell, a=b=c
Total constituent Ions per unit cell present at corners = 18x 8 = 1
Total constituent ions per unit cell present at face centre = 12 x 6 = 3
D. For end centered orthorhombic unit cell, a≠b≠c
Total contribution of atoms present at corner =18×8=1
Total contribution of atoms present at end centre =12×2=1
Hence, other than corner it contain total one atom per unit cell.
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