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Question

In the CsCl structure, r−r+=1.37. The side length of the unit cell in terms of r−, will be:

A
a=2 r
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B
a=r
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C
a=1.414 r
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D
a=4 r
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Solution

The correct option is A a=2 r
In CsCl structure, Cl form simple cubic lattice. Here, the Cl occupies the corners of the cubic unit cell.
Cs+ ion occupies cubical void present in the body centre.

A cube of edge length "a" has a body diagonal of 3×a.

In a BCC structure cations and anions are touching each other along the body diagonal such that
Body diagonal =2(r++r)=3a
Given,
r+=r1.37
Substituting the r+ term in above equation gives,
2(r1.37+r)=1.732 a
2(0.732 r+r)=1.732 a
2r(0.73+1)=1.732 a
2r×1.73=1.732 a
2r=a.
Thus, option (a) is correct.

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