Primitive Unit Cell (Simple Cubic) and Centred Unit Cells Class 12 Notes | EduRev

: Primitive Unit Cell (Simple Cubic) and Centred Unit Cells Class 12 Notes | EduRev

Bravais Lattices

Bravais (1848) showed from geometrical considerations that there are only seven shapes in which unit cells can exist. 

These are

  • Cubic
  • Orthorhombic
  • Rhombohedral
  • Hexagonal
  • Tetragonal
  • Monoclinic  
  • Triclinic 

Moreover, he also showed that there are basically four types of unit cells depending on the manner in which they are arranged in a given shape. These are:

  • Primitive
  • Body-Centered
  • Face Centered 
  • End Centered

He also went on to postulate that out of the possible twenty-eight unit cells (i.e. seven shapes, four types in each shape = 28 possible unit cells), only fourteen actually would exist. These he postulated based only on symmetry considerations. These fourteen unit cells that actually exist are called Bravais Lattices.

Seven Crystal Systems

The seven crystal systems are given below.

Cubic
Primitive Unit Cell (Simple Cubic) and Centred Unit Cells Class 12 Notes | EduRev

  • Bravais Lattices
    Primitive, face Centered, Body Centered = 3
  • Parameters of Unit Cell
    (i) Intercepts: a=b=c
    (ii) Crystal angle: α = β = γ = 90o
    Example: Pb, Hg, Ag, Au, Diamond, NaCl, ZnS

 Orthorhombic
Primitive Unit Cell (Simple Cubic) and Centred Unit Cells Class 12 Notes | EduRev

  • Bravais Lattices:
    Primitive, Face Centered, Body-Centered, End Centered = 4
  • Parameters of Unit Cell:
    (i) Intercepts: a ≠ b≠ c
    (ii) Crystal angle: α = β = γ = 90o
    Example: KNO2, K2SO4

 Tetragonal
Primitive Unit Cell (Simple Cubic) and Centred Unit Cells Class 12 Notes | EduRev

  • Bravais Lattices:
    Primitive, Body-Centered =2
  • Parameters of Unit Cell:
    (i) Intercepts: a = b≠ c
    (ii) Crystal angle: α = β = γ = 90o
    Example: TiO2, SnO2

 Monoclinic
Primitive Unit Cell (Simple Cubic) and Centred Unit Cells Class 12 Notes | EduRev

  • Bravais Lattices
    Primitive, End Centered =2
  • Parameters of Unit Cell
    (i) Intercepts: a ≠ b≠ c
    (ii) Crystal angle: α =  γ = 90o   
    Example: CaSO4.2H2O

 Triclinic
Primitive Unit Cell (Simple Cubic) and Centred Unit Cells Class 12 Notes | EduRev

  • Bravais Lattices
    Primitive = 1
  • Parameters of Unit Cell
    (i) Intercepts: a ≠ b≠ c
    (ii) Crystal angle:  α  ≠ β ≠ γ
    Example: K2Cr2O7, CaSO5H2O

 Hexagonal
Primitive Unit Cell (Simple Cubic) and Centred Unit Cells Class 12 Notes | EduRev

  • Bravais Lattices
    Primitive = 1
  • Parameters of Unit Cell
    (i) Intercepts: a = b≠ c
    (ii) Crystal angle: α = β = 90o γ =120o
    Example: Mg, SiO2, Zn, Cd

 Rhombohedral
Primitive Unit Cell (Simple Cubic) and Centred Unit Cells Class 12 Notes | EduRev

  • Bravais Lattices:
    Primitive = 1
  • Parameters of Unit Cell
    (i) Intercepts: a = b= c
    (ii) Crystal angle: α = γ = 90o, β≠ 90o
    Example:  As, Sb, Bi, CaCO3

The table given below can be used to summarize types of lattice formation.
Primitive Unit Cell (Simple Cubic) and Centred Unit Cells Class 12 Notes | EduRev


Q.1: Lithium borohydride crystallizes in an orthorhombic system with 4 molecules per unit cell. The unit cell dimensions are a = 6.8 Å,  b = 4.4 Å and C = 7.2 Å. If the molar mass is 21.76 g. Calculate the density of the crystal. 
Solution: 
Since, Density,  Primitive Unit Cell (Simple Cubic) and Centred Unit Cells Class 12 Notes | EduRevHere z = 4, Av. No = 6.023 x 1023 &
Volume = V = a x b x c
= 6.8 x 108 x 4.4 x 108 x 7.2 x 108 cm
= 2.154 x 1022 cm3

Primitive Unit Cell (Simple Cubic) and Centred Unit Cells Class 12 Notes | EduRev
= 0.6708 gm/cm3


Q.2. An element crystallizes into a structure which may be described by a cubic type of unit cell having one atom in each corner of the cube and two atoms on one of its face diagonals. If the volume of this unit cell is 24 x 10-24 cm3 and density of the element is 7.20 gm/cm3, calculate no. of atoms present in 200 gm of the element.
Ans: Number of atoms contributed in one unit cell = one atom from the eight corners + one atom from the two face diagonals = 1+1 = 2 atoms
Mass of one unit cell = volume × its density
= 24 × 10–24 cm3 × 7.2 gm cm3 
= 172.8 × 10–24 gm
∴ 172.8 10–24 gm is the mass of one – unit cell i.e., 2 atoms
∴ 200 gm is the mass = 2 × 200 / 172.8 × 10–24 atoms = 2.3148 × 1024 atoms


Q.3. Calculate the void fraction for the structure formed by A and B atoms such that A form hexagonal closed packed structure and B occupies 2/3 of octahedral voids. Assuming that B atoms exactly fitting into octahedral voids in the HCP formed by A.
Ans: Total volume of A atom = 6 × 4 / 3 πrA3 
Total volume of B atoms = 4 × 4/3 πrA3 
=4 × 4/3 π(0.414rA)3 
Since rB/rA as B is in octahedral void of A
Volume of HCP = 24√2rA3 
Packing fraction = 6 × 4/3 πrA3 + 4 × 4/3 π (0.414rA)3 / 24√2rA3 = 0.7756
Void fraction = 1-0.7756 = 0.2244


Q.4: An element with molar mass 2.7×10-2kg mol-1 forms a cubic unit cell with edge length 405 pm. If its density is 2.7×103kg-3, what is the nature of the cubic unit cell? 
Ans: d = 2.7×103kg-3
M = 2.7×10 -kg mol-1
a= 405 pm = 405 X 10-12
NA= 6.023 X 1023
Using the formula

Primitive Unit Cell (Simple Cubic) and Centred Unit Cells Class 12 Notes | EduRev

Z=4
Unit cell is fcc unit cell.
Volume of 54 g of the element = 0.054/(2.7 x 103) = 2 X 10-6
Number of unit cell in this volume = volume of 554 g of element/volume of each unit cell = 2 x 10-6/(405 x 10-12)3 = 3.012 x 1022

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