Home
Class 12
CHEMISTRY
Statement-1:The coordination number of a...

Statement-1:The coordination number of a cation present in an O void is 6
Statement-2:O-voids are formed due to overlapping of two trigonal voids of adjacent layers.

A

Statement-1 is true, statement-2 is true, statement-2 is a correct explanation for statement-1

B

Statement-1 is true, statement-2 is true, statement-2 is not correct explanation for statement-1

C

Statement-1 is true, statement-2 is false

D

Statement-1 is false, statement-2 is true

Text Solution

AI Generated Solution

The correct Answer is:
To analyze the given statements, we need to evaluate each one based on our understanding of coordination numbers and voids in crystal structures. ### Step-by-Step Solution: 1. **Understanding Statement 1**: - The statement claims that the coordination number of a cation present in an octahedral void is 6. - In crystal structures, an octahedral void is surrounded by 6 atoms. For example, in a face-centered cubic (FCC) lattice, the octahedral void is located at the center of the cube, surrounded by the atoms located at the corners and face centers. - Therefore, Statement 1 is **True**. 2. **Understanding Statement 2**: - The statement claims that octahedral voids are formed due to the overlapping of two trigonal voids of adjacent layers. - To visualize this, consider a cubic lattice where we have atoms positioned at the corners and face centers. The octahedral void can be conceptualized as being formed by the arrangement of atoms in two triangular formations from adjacent layers. - When we look at the arrangement of atoms in these layers, the octahedral void indeed arises from the overlap of these triangular voids. - Therefore, Statement 2 is also **True**. 3. **Evaluating the Relationship Between the Statements**: - Since both statements are true, we need to determine if Statement 2 correctly explains Statement 1. - Statement 2 explains how octahedral voids are formed, which is relevant to the coordination number mentioned in Statement 1. The coordination number of 6 is a direct consequence of the arrangement described in Statement 2. - Thus, Statement 2 is a correct explanation for Statement 1. 4. **Conclusion**: - Both statements are true, and Statement 2 correctly explains Statement 1. Therefore, the answer is that both statements are true, and Statement 2 is the correct explanation for Statement 1. ### Final Answer: Both Statement 1 and Statement 2 are true, and Statement 2 is the correct explanation for Statement 1. ---
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • THE SOLID STATE

    AAKASH INSTITUTE ENGLISH|Exercise ASSIGNMENT SECTION-F (MATRIX MATCH)|2 Videos

  • THE SOLID STATE

    AAKASH INSTITUTE ENGLISH|Exercise ASSIGNMENT SECTION-G (INTEGER)|6 Videos

  • THE SOLID STATE

    AAKASH INSTITUTE ENGLISH|Exercise ASSIGNMENT SECTION-D (LINKED COMPREHENSION)|9 Videos

  • THE S-BLOCK ELEMENTS

    AAKASH INSTITUTE ENGLISH|Exercise Assignment (Section-J)|10 Videos

  • THERMODYNAMICS

    AAKASH INSTITUTE ENGLISH|Exercise ASSIGNMENT (Section -D) Assertion-Reason Type Questions|15 Videos

Similar Questions

Explore conceptually related problems

The coordination number of cation and anion in fluorite CaF_(2) and anti-fluroite Na_(2)O are respectively:

The coordination number of Cr in Cr_(3)O(CH_(3)COO)_(6)3H_(2)O is ,

Statement 1 : Zygote is the vital link between two generations. Statement 2 : Zygote is formed due to fusion of two haploid gametes.

Statement-1 : In caro's acid the oxidation state of sulphur is +5 Statement-2: In caro's acid, there is one peroxolinkage. (-O-O-)

Statement-1 : The ratio of Zn^2+ and F^(-) per unit cell of ZnS and CaF_2 is 1 :2 Statement-2 : In ZnS, Zn^2+ ions occupy alternate tetrahedral voids and in CaF_2, F^(-) ions occupy all the tetrahedral voids of FCC unit cell.

Which of the following given statement(s) is/are correct for both fluorite and antifluorite structures? (i) coordination number of cation is 8 (ii) Number of formula unit is one unit cell is 4 (iii) 100% tetrahedral voids are occupied (iv) Radius ratio of cation and anion is 0.20

Total number of T-voids and O-voids in HCP and CCP structures are different . (True/False)

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 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

Home
Profile