Cesium chloride crystallizes in cubic unit cell with Cl ⊖ ions at the corners and a Cs ⊕ ion in the centre of the cube. How many CsCl molecules are there in the unit cell?

A BCC unit cell has atoms at each corner of the cube and an atom at the centre of the structure. According to this structure, the atom at the body centre wholly belongs to the unit cell in which it is present. In BCC unit cell every corner has atoms. There is one atom present at the centre of the structure. BCC describes the structure of CsCl . So, a cubic cell has the following number of atoms, 8 × 1 8 + 1 = 2 . In the CsCl crystal, each unit cell has 2 atoms.

E M B I B E

Chemistry Standard 12>Chapter 1 - Solid State>Exercises>Q 3

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What are the consequences of Schottky defect?

Important Questions on Solid State

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Chemistry Standard 12>Chapter 1 - Solid State>Exercises>Q 3

Cesium chloride crystallizes in cubic unit cell with

{Cl}^{⊖}

ions at the corners and a

{Cs}^{\oplus}

ion in the centre of the cube. How many

CsCl

molecules are there in the unit cell?

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Chemistry Standard 12>Chapter 1 - Solid State>Exercises>Q 3

Cu

crystallizes in fcc unit cell with edge length of

495 pm

. What is the radius of

Cu

atom?

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Chemistry Standard 12>Chapter 1 - Solid State>Exercises>Q 3

Obtain the relationship between density of a substance and the edge length of unit cell.

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Chemistry Standard 12>Chapter 1 - Solid State>Exercises>Q 4

The density of iridium is

22.4 g / {cm}^{3}

. The unit cell of iridium is fcc. Calculate the radius of iridium atom. Molar mass of iridium is

192.2 g / mol

.

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Chemistry Standard 12>Chapter 1 - Solid State>Exercises>Q 5

Aluminium crystallizes in cubic close packed structure with $a = 353.6 pm$ . What is the radius of $Al$ atom? How many unit cells are there in $1.00 {cm}^{3}$ of $Al ?$

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Chemistry Standard 12>Chapter 1 - Solid State>Exercises>Q 6

In an ionic crystalline solid atoms of element

Y

form hcp lattice. The atoms of element

X

occupy one third of tetrahedral voids. What is the formula of the compound ?

(X_{2} Y_{3})

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Chemistry Standard 12>Chapter 1 - Solid State>Exercises>Q 7

How are tetrahedral and octahedral voids formed?

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Chemistry Standard 12>Chapter 1 - Solid State>Exercises>Q 8

Third layer of spheres is added to second layer so as to form hcp or ccp structure. What is the difference between the addition of third layer to form these hexagonal close-packed structures?

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