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In a close packed array of N spheres, th...

In a close packed array of N spheres, the number of tetrahedral holes are

A

4 N

B

`N//2`

C

2N

D

N

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To determine the number of tetrahedral holes in a close-packed array of N spheres, we can follow these steps: ### Step-by-Step Solution: 1. **Understanding Close-Packed Structures**: - In a close-packed structure, spheres are arranged in a way that maximizes the packing efficiency. The two common types of close-packed structures are Face-Centered Cubic (FCC) and Hexagonal Close-Packed (HCP). 2. **Identifying Tetrahedral and Octahedral Holes**: - In any close-packed arrangement, there are two types of voids: tetrahedral and octahedral. - The number of octahedral voids is equal to the number of spheres (N). - The number of tetrahedral voids is related to the number of octahedral voids. 3. **Relationship Between Tetrahedral and Octahedral Holes**: - For every octahedral void, there are two tetrahedral voids. Therefore, the number of tetrahedral holes can be calculated as: \[ \text{Number of Tetrahedral Holes} = 2 \times \text{Number of Octahedral Holes} \] 4. **Calculating the Number of Tetrahedral Holes**: - Since the number of octahedral holes is equal to N (the number of spheres), we can substitute this into the equation: \[ \text{Number of Tetrahedral Holes} = 2 \times N \] 5. **Conclusion**: - Thus, the number of tetrahedral holes in a close-packed array of N spheres is: \[ \text{Number of Tetrahedral Holes} = 2N \] ### Final Answer: The number of tetrahedral holes in a close-packed array of N spheres is \( 2N \). ---
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Correct the following statement by changing the underlined part of the sentence. In a close packed lattice, the number of ul("tetrahedral sites formed will be equal to that of the number of spheres") .

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In HCP or CCP constituent particles occupy 74% of the available space. The remaining space (26%) in between the spheres remains unoccupied and is called interstitial voids or holes. Considering the close packing arrangement, each sphere in the second layer rests on the hollow space of the first layer, touching each other. The void created is called tetrahedral void. If R is the radius of the spheres in the close packed arrangement then, R (radius of tetrahedral void) = 0.225 R In a close packing arrangement, the interstitial void formed by the combination of two triangular voids of the first and second layer is called octahedral coid. Thus, double triangular void is surrounded by six spheres. The centre of these spheres on joining, forms octahedron. If R is the radius of the sphere. in a close packed arrangement then, R (radius of octahedral void = 0.414 R). If the anions (A) form hexagonal close packing and cations (C ) occupy only 2/3rd octahedral voids in it, then the general formula of the compound is

In HCP or CCP constituent particles occupy 74% of the available space. The remaining space (26%) in between the spheres remains unoccupied and is called interstitial voids or holes. Considering the close packing arrangement, each sphere in the second layer rests on the hollow space of the first layer, touching each other. The void created is called tetrahedral void. If R is the radius of the spheres in the close packed arrangement then, R (radius of tetrahedral void) = 0.225 R In a close packing arrangement, the interstitial void formed by the combination of two triangular voids of the first and second layer is called octahedral coid. Thus, double triangular void is surrounded by six spheres. The centre of these spheres on joining, forms octahedron. If R is the radius of the sphere. in a close packed arrangement then, R (radius of octahedral void = 0.414 R). In the figure given below, the site marked as S is a

In HCP or CCP constituent particles occupy 74% of the available space. The remaining space (26%) in between the spheres remains unoccupied and is called interstitial voids or holes. Considering the close packing arrangement, each sphere in the second layer rests on the hollow space of the first layer, touching each other. The void created is called tetrahedral void. If R is the radius of the spheres in the close packed arrangement then, R (radius of tetrahedral void) = 0.225 R In a close packing arrangement, the interstitial void formed by the combination of two triangular voids of the first and second layer is called octahedral coid. Thus, double triangular void is surrounded by six spheres. The centre of these spheres on joining, forms octahedron. If R is the radius of the sphere. in a close packed arrangement then, R (radius of octahedral void = 0.414 R). In Schottky defect

In HCP or CCP constituent particles occupy 74% of the available space. The remaining space (26%) in between the spheres remains unoccupied and is called interstitial voids or holes. Considering the close packing arrangement, each sphere in the second layer rests on the hollow space of the first layer, touching each other. The void created is called tetrahedral void. If R is the radius of the spheres in the close packed arrangement then, R (radius of tetrahedral void) = 0.225 R In a close packing arrangement, the interstitial void formed by the combination of two triangular voids of the first and second layer is called octahedral coid. Thus, double triangular void is surrounded by six spheres. The centre of these spheres on joining, forms octahedron. If R is the radius of the sphere. in a close packed arrangement then, R (radius of octahedral void = 0.414 R). Mark the false statement :

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