Question

# The radius ratio of Cs+ to Cl− is 0.90. If the radius of Cl− ion is 1.80 ∘A, the false statement regarding the CsCl structure is ?

A

The distance between the centres of Cl ions is greater than 3.60 A

No worries! We‘ve got your back. Try BYJU‘S free classes today!
B

The distance between Cs+ ion and Cl is 3.60 A

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
C

The distance between Cs+ ion and Cl is 3.42 A

No worries! We‘ve got your back. Try BYJU‘S free classes today!
D

The distance between two Cs+ ions is greater than 3.24 A

No worries! We‘ve got your back. Try BYJU‘S free classes today!
Open in App
Solution

## The correct option is B The distance between Cs+ ion and Cl− is 3.60 ∘A rCs+rCl−=0.90 ∘A⇒rCs+=0.90×rCl−=0.90×1.80=1.62 ∘A For precise fitting of the cubic voids, rCs+rCl− must be 0.732 which is smaller than the given value of 0.90. Hence cubic packing of Cl− ions is loose to some extent, i.e., two Cl− ions are not in touch with each other and the distance between two Cl− ions will be greater than 3.60 ∘A. The Cs+ ion at the centre of the body is in touch with 2Cl− ions at the opposite corners of the cube. Hence distance between Cs+ and Cl−=rCS++rCl−=1.62 ∘A+1.80 ∘A=3.42 ∘A

Suggest Corrections
0
Join BYJU'S Learning Program
Select...
Related Videos
Examples of Ionic Compounds
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
Select...