The void between two oppositly directed planar triangles of spheres in adjacent layers is called
The void between two oppositly directed planar triangles of spheres in adjacent layers is called
A
Cubic void
B
Tetrahedral void
C
Octahedral void
D
Tetrahedral (or) Octahedral void
Text Solution
AI Generated Solution
The correct Answer is:
To solve the question regarding the void between two oppositely directed planar triangles of spheres in adjacent layers, we can follow these steps:
### Step-by-Step Solution:
1. **Understanding the Structure**:
- Visualize the arrangement of spheres in a crystal lattice. In this case, we are considering two layers of spheres where the spheres in one layer are positioned in a way that they create a triangular arrangement.
2. **Identifying the Voids**:
- When two layers of spheres are stacked, there are spaces or voids created between them. The question specifically mentions "oppositely directed planar triangles," which indicates that the spheres in the two layers are arranged in a staggered manner.
3. **Determining the Type of Void**:
- The void created between two adjacent layers of spheres can be classified based on its geometry. In this case, the void is surrounded by six spheres: three from the upper layer and three from the lower layer.
4. **Recognizing the Octahedral Void**:
- The specific arrangement of six surrounding spheres (three above and three below) corresponds to what is known as an **octahedral void**. This is a common type of void found in close-packed structures.
5. **Final Answer**:
- Therefore, the void between the two oppositely directed planar triangles of spheres in adjacent layers is called an **octahedral void**.
Similar Questions
Explore conceptually related problems
The cemanting layer of pectin between adjacent plant cell is called.
The gap between two neurons is called a
The interval between two ecdyses is called
Two dimensional close packed structure can be generated by stacking the rows of close packed spheres. This can be done in two different ways. (I) The second row may be placed in contact with the first one, such that the spheres of the second row are exactly above those of first row. The spheres of the two rows are aligned vertically as well as horizontally. If we call the first row as 'A' type of row, the second row being exactly same as the first one is also of 'A' type. Similarly, we may place more rows to obtain AAAA.... type arrangement (II) In this type, the second row may be placed above the first one in a staggered manner such that its spheres. fit in depressions of first row. if the arrangement of spheres in the first row is called 'A' type the one in the second row is different and may be called 'B' type. When the third row is placed adjacent to the second in staggered manner, its spheres are aligned with those of first layer. Hence this layer is also 'A' type. The spheres of similarly placed fourth row will be aligned with those of the second row ('B' type). Hence this arrangement is of ABAB.... type The type of voids generated in type (I) & (II) respectively are
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). Mark the false statement :
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). In the spinel structure, oxide ions are cubic close packed whereas 1/8th of tetrahedral voids are occupied by A^(2+) cations and 1/2 of octahedral voids are occupied by B^(3+) cations. The general formula of the compound having spinel structure is
The distance or length of the myofibril between two adjacent z-bands is called
Recommended Questions
- The void between two oppositly directed planar triangles of spheres in...
Text Solution
|
- The cemanting layer of pectin between adjacent plant cell is called...
Text Solution
|
- While placing the second layer over that first layer , if the sphere o...
Text Solution
|
- How many tetrahedral voids and octahedral voids are possible if the nu...
Text Solution
|
- In HCP or CCP constituent particles occupy 74% of the available space....
Text Solution
|
- In HCP or CCP constituent particles occupy 74% of the available space....
Text Solution
|
- In HCP or CCP constituent particles occupy 74% of the available space....
Text Solution
|
- In HCP or CCP constituent particles occupy 74% of the available space....
Text Solution
|
- Explain AAAA and ABABA and ABCABC type of three dimensional packing wi...
Text Solution
|