A solid `AB` has `CsCl`-type structure. The edge length of the unit cell is `404` pm. Calculate the distance of closest approach between `A^(o+)` and `B^(Θ)` ions.

a. MgO has the structure of NaCl and TICI has the structure of CsCl . What are the coordiantion number of the ions in MgO and TICI ? If the closed-packed cations in an XY -type solid have a raidus of 73.2 pm, what would be the maximum and minimum sizes of the anions filling voids? c. Fe_(2)O_(3) (haematite) forms ccp arrangement of O^(2-) ions with Fe_(3+) ions occupying initerstitial positions. Predict whether fe^(3+) ions are in the OV or TV . Given r_(Fe^(3+)) = 0.7 Å and r_(O^(2-)) = 1.4 Å d. A solid XY has CsCl -type structure. The edge length of the unit cell is 400 pm Calculate the distance of closest approach between X^(o+) and Y^(ɵ) ions.

A solid AB has ZnS-type structure. The edge lenth of unit cell is 400 pm abd the radius of 'B^-' ion is 0.130 nm. Then the radius of 'A^+' ion is

If 'a' is the edge length of the unit cell of a fcc crystal, then what is the distance of closest approach between the two atoms in the crystal ?

A solid AB has NaCl type structure with edge length 580.54 pm.The radius of A^(+) is 100 pm. The radius of B^(-) is

KF has NaCl structure. The edge length of its unit cell has been found to be 537.6 pm. The distance between K^(+) and F^(-) in KF is :