Tetrahedral void and octahedral void.
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Tetrahedral Voids
(Source: Chemistrystackexchange)
Now there are two types of three-dimensional close packing in crystals. One such type is Cubic Close packing. Here the two-dimensional structures are stacked in a specific alignment. The layers alternate with each other. So the second layer will be located in the depression of the first layer.
You will notice that a triangle-shaped void is seen in this type of alignment. The sphere which is in the depression will leave a void between itself and the sphere in the layer above. This void is the Tetrahedral Void.
There is a simple way to calculate the number of Tetrahedral Voids in a lattice. Here if the number of spheres (i.e. unit cells) is said to be “n”, then the number of voids will be twice as many. So the number of tetrahedral voids will be “2n”.
The void is much smaller than the sphere, i.e. it has a smaller volume. And the coordination number of a tetrahedral void is four because of the void forms at the center of four spheres.
Octahedral Voids
If you observe a three-dimensional structure of a crystal lattice you will observe the gaps in between the spheres. These are the voids. As you see that tetrahedral voids are triangular in shape. When two such voids combine, from two different layers they form an octahedral void.
So when the tetrahedral void of the first layer and the tetrahedral void of the second layer align together, they form an octahedral void. Here the void forms at the center of six spheres. So we say the coordination number of an octahedral void is six.
To calculate octahedral void, if th
(Source: Chemistrystackexchange)
Now there are two types of three-dimensional close packing in crystals. One such type is Cubic Close packing. Here the two-dimensional structures are stacked in a specific alignment. The layers alternate with each other. So the second layer will be located in the depression of the first layer.
You will notice that a triangle-shaped void is seen in this type of alignment. The sphere which is in the depression will leave a void between itself and the sphere in the layer above. This void is the Tetrahedral Void.
There is a simple way to calculate the number of Tetrahedral Voids in a lattice. Here if the number of spheres (i.e. unit cells) is said to be “n”, then the number of voids will be twice as many. So the number of tetrahedral voids will be “2n”.
The void is much smaller than the sphere, i.e. it has a smaller volume. And the coordination number of a tetrahedral void is four because of the void forms at the center of four spheres.
Octahedral Voids
If you observe a three-dimensional structure of a crystal lattice you will observe the gaps in between the spheres. These are the voids. As you see that tetrahedral voids are triangular in shape. When two such voids combine, from two different layers they form an octahedral void.
So when the tetrahedral void of the first layer and the tetrahedral void of the second layer align together, they form an octahedral void. Here the void forms at the center of six spheres. So we say the coordination number of an octahedral void is six.
To calculate octahedral void, if th
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