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+=r−1.37
Substituting the r+ term in above equation gives,
2(r−1.37+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.