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Which defect causes decreases in the den...

Which defect causes decreases in the density of crystal?

A

Frenkel

B

Schottky

C

Interstitial

D

F-centre

Text Solution

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The correct Answer is:
B
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Ionic lattic has two major points defects ,(1) Schottky (2) Frenkel defects . Schottkly defects occurs due to the cations - anion pair's missing from the lattice sites . Frenkel defects occurs levels its lattic site and fits into an intersitial space. The neturaity of the crystal is benig maintained and we considerd all losses from interstitical positions. which defect decrease density of the crystal ?

AAKASH INSTITUTE-THE SOLID STATE -ASSIGNMENT SECTION-A (OBJECTIVE)
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  2. The cubic unit cell of a metal (molar mass= 63.55 "mol"^(-1)) has an e...

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  3. CsBr crystallises in a body- centred cubic lattice. The unit cell leng...

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  4. In the crystals of which of the following ionic compounds would you ex...

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  5. Lithium metal crystallizes in a body centred cubic crystals. If the le...

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  6. Coordinating number of Na^(+) in NaCl is

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  7. Body -centred cubic lattice has a corrdination number of

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  8. When molten zinc is cooled to solid state, it assumes hcp structure. T...

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  9. The unit cell of a binary compound of A and B has ccp structure with A...

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  10. Which of the following unit cell is not possible for monoclinic crysta...

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  11. Which defect causes decreases in the density of crystal?

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  12. Schottky defect occurs mainly in electrovalent compounds where

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  13. Which one of the following is the correct statement ?

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  14. The appearance of colour in solid alkali metal halides is generally du...

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  15. Doping silicon with boron produces a -

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  16. What type of crystal defect is indicated in the diagram given below : ...

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  17. The pyknometric density of sodium chloride crystal is 2.165xx10^(3)kg ...

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  18. The non-stoichiometric compound Fe0.94O is formed when some Fe^(+2) io...

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  19. To get n-type doped semiconductor, impurity to be added to silicon sho...

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  20. A binary solid (A^(+)B^(+)) has a rock sell structure .If the edge len...

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