What is Packing in Solid?
Crystalline solids exhibit a regular and repeating pattern of constituent particles. The diagrammatic representation of three-dimensional arrangements of constituent particles in a crystal, in which each particle is depicted as a point in space is known as crystal lattice. In a crystal lattice, the atoms are very closely packed leaving very little space between them.
Packing in solids in different dimensions is discussed below:
Close packing in crystalline solids in one dimension:
In one dimension close packing, spheres are arranged in a row such that adjacent atoms are in contact with each other. The coordination number is defined as the no. of the nearest neighbour particles. In the case of one dimensional close packing, the coordination number is equal to two.
Close packing in crystalline solids in two dimensions:
In two-dimensional close packing, a row of closed packed spheres are stacked to obtain a two-dimensional pattern. This stacking is done in two ways:
- Square close packing:
Packing in Solids: One and Two Dimensions
The second row can be placed exactly below the first row in a close packing. Thus, if we call the first row as “A” type row, the second row is arranged exactly the same as the first one, is also of “A” type. In such an arrangement each sphere is in contact with four other spheres. Hence, it has a coordination number equal to four. We observe that if the centres of the four immediate neighbouring spheres are joined, a square is formed. This type of packing in crystalline solids is known as square close packing in two dimensions.
- Hexagonal close packing: The second row can be placed below the first row in a staggered manner such that its spheres fit in the depressions of the first row. Thus, if we call the first row as “A” type row, the second row being arranged differently can be named as “B” type. Again the third row appears as “A” type. This type of packing is referred to as “ABAB” type. In such an arrangement each sphere is in contact with six other spheres. Hence, it has a coordination number equal to six. We observe that if the centres of the six immediate neighbouring spheres are joined, a hexagon is formed. This type of packing in solids is known as hexagonal close packing in two dimensions. It has lesser free space and hence higher packing efficiency in comparison to square close packing.
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Frequently Asked Questions – FAQs
What is the reason for the close packing of solid?
Near crystal, packing refers to the effective arrangement of constituent particles in a crystal lattice in a vacuum. We have to assume that all particles (atoms, molecules and ions) are of the same spherical solid form to grasp this set more precisely.
What is the packing efficiency?
The packing quality is the proportion of the atoms directly occupied by the crystal (or unit cell). It must often be less than 100 percent, since spheres (atoms are usually spherical) can not be filled without any empty space between them.
What are point defects?
Point defects are zero dimensional lattice defects, i.e. they do not have lattice structure in any dimension. Typical point defects contain impurity atoms, vacancies and self-interstitials in pure metal.
What is hexagonal packing?
Hexagonal tightly packed (hcp) refers to layers of packed spheres such that spheres overlay each other in alternating layers. A slip framework, which is a close-packed structure, is hexagonal near packed. For elemental metals, the hcp structure is very general, including: beryllium.
What is the closest packing arrangement?
The word “closest packed structures” refers to the crystal structures (lattices) with the most closely packed or space-efficient composition. Imagine an atom as a sphere inside a crystal lattice. The nearest packed systems are considered such configurations. Stable structures of crystals can be represented by the packing of spheres.
For a detailed discussion on packing in crystalline solids in one and two dimensions, download BYJU’S – the learning app.
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