Close Packed structures Chemistry Notes

Close Packed structures Chemistry Notes

→ The constituent particles in solids are closely packed and minimum vacant space is found between them. This vacant space is called void or interstitial space. If constituent partcles are present in the form of solid spheres then their three-dimensional close packing can be explained as follows:

→ Close-Packing in One Dimension A number of solid spheres of same size are arranged and placed side by side in a row. In this arrangement, each sphere is in contact with two neighbouring spheres, which is its coordination number. Thus, it is clear that the coordination number in one-dimensional close packing is two.

Close Packed structures Chemistry Notes 1

Note: Coordination Number: The number of touching neighbouring spheres of one particle is called its coordination number

Close Packed structures Chemistry Notes

Close Packing in Two Dimensions :

It is of two types :

→ Square Close Packing : In this type of close packing, the second row of particles is so arranged in contact with first row that the spheres of second row are exactly above the spheres of first row and spheres of both rows are arranged horizontally as well as vertically. Here, each sphere remains in contact with four neighboring spheres. So, its coordination number is 4.It is called square close packing or also called AAAA type of arrangement. (figure 1.27)

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→ Hexagonal Close Packing : In this type of close packing, the second row of particles is so placed in contact with first row that the spheres of second row come in depressions of spheres of first row. In this arrangement, free space is less and this type of packing is more efficient than square close packing. Here, each sphere remains in contact with six neighbouring spheres.

→ So the coordination number of two-dimensional hexagonal close packing is 6. This is also called ABAB type of arrangement. Here, some empty spaces or voids are found at surface whose shape is triangular. These triangular voids are of two types i.e., horizontally (in one row) and vertically (in other row). (figure 1.28)

Close Packed structures Chemistry Notes 3

Fig. 1.28. Hexagonal Close Packing in Two-dimensions

Three Dimensional Close packing :

→ Three dimensional structure can be obtained by placing two dimensional layers one over the other. These are of following types

Three dimensional closed packing from two dimensional square closed packed layers :

→ Here, the layers of two dimensional square close packing are so arranged one over the other that spheres come one above the other and spheres of all layers one arranged in straight line horizontally and vertically. Such type of formed lattice is simple cubic lattice and its unit cell is primitive cubic unit cell (Figure 1.29)

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→ Three dimensional closed packing from two dimensional hexagonal close packed layers In this arrangement, three-dimensional close packing is done as follows:

Placing Second Layer Over the First Layer :

→ In this type of arrangement, the spheres of second, layer are arranged in depressions of first layer. Since spheres of both layers are aligned differently, so first layer is called layer A and Second layer is called layer B. Here, tetrahedral voids are formed in this type of arrangement. Octahedral voids are also formed.

  • The number of octahedral voids generated = N
  • Number of tetrahedral voids generated = 2N

Close Packed structures Chemistry Notes

→ Interstitial void : Constituent particles are closely packed in solids and minimum empty space is found between them. This empty space is called void. Voids are of two types (a) Tetrahedral void : It is formed due to combination of centres of four spheres. It is represented in figure 1.30

Close Packed structures Chemistry Notes 4

→ Octahedral Void : Such type of void is formed by six spheres. This type of void is created when the triangular voids of second layers are over the triangular voids of first layers. It is represented in figure 1.31.

Close Packed structures Chemistry Notes 5

→ The arrangement of a tetrahedral and octahedral voids can be represented by the following figure 1.32

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→ Placing Third Layer Over Second Layer There are two possibilities in this arrangement (i) Covering of Tetrahedral voids or Hexagonal Close Packing (hcp) In this position, the spheres of third layer are verically aligned with spheres of first layer and the spheres of fourth layer are vertically aligned with sphere of second layers. So, the pattern of spheres is repeated in uniform manner. It is called ABAB… pattern. Here, the coordination number is 12 and packing efficiency is 74%. This arrangement is found in magnesium and zinc (fig 1.33)

Close Packed structures Chemistry Notes 8

→ Covering of Octahedral voids or cubic close packing (ccp) Structure Here, spheres are so arranged that the spheres of fourth layer are vertically aligned with first layer and spheres of fifth layer are vertically aligned with second layer.

Close Packed structures Chemistry Notes

→ So, the pattern of spheres repeated in uniform manner. This arrangement is called ABCABC pattern. Here, the coordination number is also 12 and packing efficiency is 74%. This arrangement is found in copper, silver, gold etc, (figure 1.34)

Close Packed structures Chemistry Notes 9

Chemistry Notes

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