Ammonium chloride crystallises in a body-centred cubic lattice with a unit distance of 387 pm. Calculate (a) the distance between oppositely charged ions in the lattice and (b) and radius of the `NH_(4)^(+)` ion of the radius of `Cl^(-)` ion is 181 pm.

NH_(4)Cl crystallises in a body centred cubic lattice with a unit cell distance of 387 pm. Calculate (a) the distance between the oppositely charged ions in the lattice. (b) the radius of NH_(4)^(+) ion if that of Cl^(-) ion is 181 pm.

NH_(4)Cl crystallises in a body centred cubic lattice with a unit cell distance of 387 pm. Calculate (a) the distance between the oppositely charged ions in the lattice. (b) the radius of NH_(4)^(+) ion if that of Cl^(-) ion is 181 pm.

NH_(4)Cl crystallises in a body centred cubic lattice with a unit cell distance of 387 pm. Calculate (a) the distance between the oppositely charged ions in the lattice. (b) the radius of NH_(4)^(+) ion if that of Cl^(-) ion is 181 pm.

NH_(4)Cl crystallizes in a body centred cubic lattice , with a unit cell distance of 387 pm. Calculate (a) the distance between the oppositely charged ions in the lattice and (b) the radius of the NH_(4)^(+) ion if the radius of the Cl^(-) ion is 181 pm.

AB crystallizes in a body centred cubic lattice with edge length 'a' eqal to 387 pm. The distance between two oppositely charged ions in the lattice is :