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Types of Unit Cell

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Select the incorrect statement in a CsCl crystal:(a) Cs forms a simple cubic lattice, Cl forms a simple cubic lattice(b) Cl occupies body centre of Cs(c) Cs occupies body centre of Cl(d) It is impossible for CI to occupy body centre of Cs because the body centre void of Cs issmaller than Cl ion size

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Q. In a cubic crystal of CsCl (density

= 3.97

^{- 3}

), the eight corners are occupied by

C l^{-}

C s^{+}

ions at the body centre. Calculate the distance (in

˚ A

) between the neighbouring

C s^{+}

C l^{-}

Q. If the length of body diagonal for

CsCl

, which crystallises into a cubic structure with

{Cl}^{-}

ions at the corners and

{Cs}^{+}

ions at the centre of unit cell is

7 ˚ A

and the radius of

{Cs}^{+}

1.69 ˚ A

. The radius of

{Cl}^{-}

C s C l

crystals are formed by bcc crystal lattice where

C l^{-}

occupies the corners and

C s^{+}

occupies the centre of the cube.

The density of crystalline

C s C l

4 g / c c

. The effective volume occupied by a single

C s C l

ion pair in the crystal is
[Molar mass of

C s C l = 168 {g mol}^{- 1}]

Q. If the length of the body diagonal for CsCl which crystallises into a cubic structure with

C l^{-}

ions at the corners and

C s^{+}

ions at the centre of the unit cells is

7 o A

and the radius of the

C s^{+}

1.69 o A

. What is the radii for

C l^{-}

C s C l

has cubic structure of ions in which

C s^{+}

ions is present in the body-centre of the cube. If density is

3.99 g c m^{- 3}

.
(a) Calculate the length of the edge of a unit cell.
(b) What is the distance between

C s^{+}

C l^{-}

ions?
(c) What is the radius of

C s^{+}

ion if the radius of

C l^{-}

180 p m

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