Standard axial ratio for metallic HCP lattice is 2√( 2/3). It is the ratio of

Atomic radius to hexagon edge length

Hexagon height length to atomic radius

Atomic radius to hexagon height

Which of the following quantities is larger in HCP as compared to FCC if the constituting atoms are similar?

Number of particles per unit cell

A crystal lattice is made up of a very large number of unit cells where every lattice point is occupied by one constituent particle. The unit cell can be seen as a three dimension structure containing one or more atoms. We always observe some void spaces in the unit cell irrespective of the type of packing. Percentage of spaces filled by the particles in the unit cell is known as the packing fraction of the unit cell. In this section we shall learn about packing efficiency. Packing fraction of different types of packing in unit cells is calculated below:

Table of Content

Packing efficiency in face centered cubic unit cell
Packing efficiency in body centered cubic unit cell
Packing efficiency in simple cubic unit cell
Frequently asked questions- FAQs

Packing efficiency in face centered unit cell and Cubic close packing structure:

Hexagonal close packing (hcp) and cubic close packing (ccp) have same packing efficiency. Let us take a unit cell of edge length “a”. Length of face diagonal, b can be calculated with the help of Pythagoras theorem,

Packing Efficiency of a Unit Cell

\(\begin{array}{l} b^{2} = a^{2} + a^{2}\end{array} \)

The radius of the sphere is r
The face diagonal (b) = r + 2r + r = 4r

\(\begin{array}{l} \therefore (4r)^{2} = a^{2} + a^{2}\end{array} \)

\(\begin{array}{l} \Rightarrow (4r)^{2} = 2a^{2}\end{array} \)

\(\begin{array}{l} \Rightarrow a = \sqrt{\frac{16r^{2}}{2}}\end{array} \)

\(\begin{array}{l} \Rightarrow a = \sqrt{8} r\end{array} \)

Volume of the cube = a³ =

\(\begin{array}{l}(\sqrt{8} r)^{3}\end{array} \)

Volume of the sphere = (4/3) π r³

No. of Sphere present in one FCC unit cell =4

The volume of the sphere = 4 x (4/3) π r³

\(\begin{array}{l} The Packing efficiency =\frac{Total volume of sphere}{volume of cube}\times 100\end{array} \)

\(\begin{array}{l} =\frac{\frac{16}{3}\pi r^{3}}{8\sqrt{8}r^{3}}\times 100\end{array} \)

= 74%

Packing efficiency in body centered cubic unit cell:

In body centered cubic unit cell, one atom is located at body center apart from corners of the cube. Let us take a unit cell of edge length “a”. Length of body diagonal, c can be calculated with help of Pythagoras theorem,

Unit Cell

\(\begin{array}{l} c^2~=~ a^2~ + ~b^2 \end{array} \)

Where b is the length of face diagonal, thus b =

\(\begin{array}{l} \sqrt{2}~a\end{array} \)

\(\begin{array}{l}c^2~=~ 3a^2\end{array} \)

=> c =

\(\begin{array}{l} \sqrt{3} \end{array} \)

From the figure, radius of the sphere, r = 1/4 × length of body diagonal, c

=> r =

\(\begin{array}{l} \frac {c}{4}\end{array} \)

\(\begin{array}{l} \frac{\sqrt{3}}{4}~a\end{array} \)

=> a =

\(\begin{array}{l} \frac {4}{\sqrt{3}} \end{array} \)

In body centered cubic structures, each unit cell has two atoms,

Packing efficiency =

\(\begin{array}{l} \frac{volume~ occupied~ by~ two~ spheres~ in~ unit~ cell}{Total~ volume~ of~ unit ~cell}\end{array} \)

× 100

\(\begin{array}{l} \frac {2~×~\left( \frac 43 \right) \pi r^3~×~100}{( \frac {4}{\sqrt{3}})^3}\end{array} \)

= 68%

Packing Efficiency of Diamond

In the structure of diamond C atom present at all corners , all face centres and 50 % tetrahedral voids.

Bond length i.e distance between 2 nearest C atom = \frac{\sqrt{3}a}{4}

Radius of C atom = rc

\(\begin{array}{l}rc = \frac{\sqrt{3}a}{8}\end{array} \)

Packing efficiency of diamond is 34%

– wherein

Number of C atom per unit cell = 8

a = edge length of unit cell

Packing efficiency in simple cubic unit cell:

In simple cubic unit cell, atoms are located at the corners of cube. Let us take a unit cell of edge length “a”. Radius of atom can be given as,

Unit Cell

r =

\(\begin{array}{l} \frac a2 \end{array} \)

=> a = 2r

In simple cubic structures, each unit cell has only one atom,

Packing efficiency =

\(\begin{array}{l} \frac{volume~ occupied~ by~ one~ atom}{Total~ volume~ of~ unit ~cell}\end{array} \)

× 100

\(\begin{array}{l} \frac {\left( \frac 43 \right) \pi r^3~×~100}{( 2 r)^3} \end{array} \)

= 52.4%

For detailed discussion on calculation of packing efficiency, download BYJU’S – the learning app.

Frequently Asked Questions- FAQs

1. What is packing efficiency?

The percentage of the total space which is occupied by the particles in a certain packing is known as packing efficiency. The constituent particles i.e. atoms, ions or molecules are closely packed in the crystal lattice. They can do so either by cubic close packing(ccp) or by hexagonal close packing(hcp). In both the cases, a number of free spaces or voids are left i.e, the total space is not occupied.

2. What is the packing efficiency in HCP and CCP structure?

The Packing efficiency of Hexagonal close packing (hcp) and cubic close packing (ccp) is 74%.

3. Is CCP and FCC same?

The cubic closed packing is CCP, FCC is cubic structures entered for the face. When we put the atoms in the octahedral void, the packing is of the form of ABCABC, so it is known as CCP, while the unit cell is FCC. These are two different names for the same lattice.

4. What is the packing efficiency in BCC?

The packing efficiency of body centred cubic unit cell (BCC) is 68%.

5. What is the packing efficiency in SCC?

The packing efficiency of simple cubic unit cell (SCC) is 52.4%.