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Packing faction or Packing efficiency is the percentage of total space filled by the particles.
Both hcp & ccp though different in form are equally efficient. They occupy the maximum possible space which is about 74% of the available volume. Hence they are called closest packing.
In addition to the above two types of arrangements a third type of arrangement found in metals is body centred cubic (bcc) in which space occupied is about 68%.
Packing Efficiency =
Let us calculate the packing efficiency in different types of structures
Let ‘a’ be the edge length of the unit cell and r be the radius of sphere.
As sphere are touching each other
Therefore a = 2r
No. of spheres per unit cell = 1/8 × 8 = 1
Volume of the sphere = 4/3 πr3
Volume of the cube = a3= (2r)3 = 8r3
∴ Fraction of the space occupied = 1/3πr3 / 8r3 = 0.524
∴ % occupied = 52.4 %
In body centred cubic unit cell
Let DF= b
and we know that
ED=EF= a (edge length)
b2 = a2 + a2 = 2a2
Let, AF = c
We know that
FD = b
& AD = a (edge length)
c2 = a2 + b2 = a2 + 2a2 = 2a2
or c = √3 a
we know that c is body diagonal. As the sphere at the centre touches the sphere at the corner. Therefore body diagonal c = 4r
i.e. √3 a = 4r
or r = (√3/4)a
or a = 4r / √3
∴ Volume of the unit cell = a3 = (4r / √3)3 = 64r3 / 3√3
No. of spheres in bcc = 2
∴ volume of 2 spheres = 2 × 4/3πr3
Let ‘r’ be the radius of sphere and ‘a’ be the edge length of the cube
As there are 4 sphere in fcc unit cell
∴ Volume of four spheres = 4 (4/3 πr3)
In fcc, the corner spheres are in touch with the face centred sphere. Therefore, face diagonal AD is equal to four times the radius of sphere
AC = √AD2 + DC2 = √a2 + a2= √2a
4r = √2a
or a = 4/√2 r
∴ volume of cube = (2/√2 r)3
Refer to the following video for packing efficiency:
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 10-24cm3 and density of the element is 7.20gm/cm3, calculate no. of atoms present in 200gm of the element.
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
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
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
Show by simple calculation that the percentage of space occupied by spheres in hexagonal cubic packing (hcp) is 74%
Let the edge of hexagonal base =a
And the height of hexagon = h
And radius of sphere = r
The centre sphere of the first layer lies exactly over the void of 2nd layer B.
The centre sphere and the spheres of 2nd layer B are in touch
So, In Δ PQR (an equilateral triangle)
PR = 2r, Draw QS tangent at points
∴ In Δ QRS ∠QRS = 30°, SR = r
Cos30° = SR/QR
QR = r / √3/2 = 2r / √3
∴ PQ = √PR2 – QR2 = √4r2 – 4r2 / 3
h1 = √8r2 / 3 = 2 √2/3 r
∴ h = 2h1 = 4 √2/3 r
Now, volume of hexagon = area of base x height
= 6 × √3 / 4 a2 × h => 6 × √3/4 (2r)2 × 4 √2/3 r
[∴ Area of hexagonal can be divided into six equilateral triangle with side 2r)
No. of sphere in hcp = 12 × 1/6 + 1/2 × 2 + 3 = 2+1+3 = 6
∴ Volume of spheres = 6 × 4/3πr3
∴ Percentage of space occupied by sphere = 6 × 4/3 πr3 / 6 × √3/4 × 4r2 × 4√2/3 r × 100 = 74%
From the unit cell dimensions, it is possible to calculate the volume of the unit cell. Knowing the density of the metal. We can calculate the mass of the atoms in the unit cell. The determination of the mass of a single atom gives an accurate determination of Avogadro constant.
Suppose edge of unit cell of a cubic crystal determined by X – Ray diffraction is a, d is density of the solid substance and M is the molar mass, then in case of cubic crystal
Volume of a unit cell = a3
Mass of the unit cell = no. of atoms in the unit cell × mass of each atom = Z × m
Here Z = no. of atoms present in one unit cell
m = mass of a single atom
Mass of an atom present in the unit cell = m/NA
Question 1: Packing efficiency of simple cubic unit cell is ..
Question 2: Which of the following crystal systems has minimum packing efficiency?
d. Simple Cubic
Question 3: Which of the following cubic unit cell has packing efficiency of 64%?
Question 4: For BCC unit cell edge length (a) =
b. 4r / √3
c. 4/√2 r
Question 5: For FCC unit cell, volume of cube =
a. 64 / 2√2 r3
b. 64r3 / 3√3
c. 25r3 / 3√3
d. 64/ 3r3
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