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Molality

If the densit...

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If the density of crystalline CsCl is 3.988g/cm calculate the volume effectively occupied by a single CsCl Ion pair in the Crystal (CsCl =168.4)

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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}]

C s C l

has density 3.988 g

c m^{- 3} .

The volume occupied by a single

C s C l

ion pair in the crystal will be:

Q. Volume occupied by single

C s C l

ion pair in a crystal is

7.014 \times 10^{- 23} {c m}^{3}

C s - C s

internuclear distance is equal to length of the side of the cube corresponding to volume of one

C s C l

ion pair. The smallest

C s

C s

internuclear distance is nearly :

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. Assertion (A) : In

C s C l

crystal, the coordination number of

C s^{\oplus}

8

C l^{⊖}

C s C l

adopt bcc type of packing.

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